document_title: Compounds of fluorine

question_text: if there are 5 fluorines and 1 phosphorous atom. what is the formal name

question_tokens: if there are 5 fluorines and 1 phosphorous atom . what is the formal name

text: Compounds of fluorine

text: Difluorine[edit]

text: While an individual fluorine atom has one unpaired electron, molecular fluorine (F2) has all the electrons paired. This makes it diamagnetic (slightly repelled by magnets) with the magnetic susceptibility of −1.2×10−4 (SI), which is close to theoretical predictions.[5] In contrast, the diatomic molecules of the neighboring element oxygen, with two unpaired electrons per molecule, are paramagnetic (attracted to magnets).[6]

text:
Halogen bond energies (kJ/mol)[7]

X
XX
HX
BX3
AlX3
CX4

F
159
574
645
582
456

Cl
243
428
444
427
327

Br
193
363
368
360
272

I
151
294
272
285
239

text: The fluorine–fluorine bond of the difluorine molecule is relatively weak when compared to the bonds of heavier dihalogen molecules. The bond energy is significantly weaker than those of Cl2 or Br2 molecules and similar to the easily cleaved oxygen–oxygen bonds of peroxides or nitrogen–nitrogen bonds of hydrazines.[8] The covalent radius of fluorine of about 71 picometers found in F2 molecules is significantly larger than that in other compounds because of this weak bonding between the two fluorine atoms.[9] This is a result of the relatively large electron and internuclear repulsions, combined with a relatively small overlap of bonding orbitals arising due to the small size of the atoms.[10]

text: The F2 molecule is commonly described as having exactly one bond (in other words, a bond order of 1) provided by one p electron per atom, as are other halogen X2 molecules. However, the heavier halogens' p electron orbitals partly mix with those of d orbitals, which results in an increased effective bond order; for example, chlorine has a bond order of 1.12.[11] Fluorine's electrons cannot exhibit this d character since there are no such d orbitals close in energy to fluorine's valence orbitals.[11] This also helps explain why bonding in F2 is weaker than in Cl2.[10]

text: Reactivity[edit]

text: Reactions with elemental fluorine are often sudden or explosive. Many substances that are generally regarded as unreactive, such as powdered steel, glass fragments, and asbestos fibers, are readily consumed by cold fluorine gas. Wood and even water burn with flames when subjected to a jet of fluorine, without the need for a spark.[12][13]

text:
External video

 Cold gas impinging on several substances causes bright flames: video by the University of Nottingham.Extra footage.
Fluorine reacting with caesium, video by the Royal Institution.
(Both videos filmed at a fluorine laboratory of the University of Leicester.)

text: Reactions of elemental fluorine with metals require different conditions that depend on the metal. Often, the metal (such as aluminium, iron, or copper) must be powdered because many metals passivate by forming protective layers of the metal fluoride that resist further fluoridation.[7] The alkali metals react with fluorine with a bang (small explosion), while the alkaline earth metals react not quite as aggressively. The noble metals ruthenium, rhodium, palladium, platinum, and gold react least readily, requiring pure fluorine gas at 300–450 °C (575–850 °F).[14]

text: Fluorine reacts explosively with hydrogen in a manner similar to that of alkali metals.[15] The halogens react readily with fluorine gas[16] as does the heavy noble gas radon.[17] The lighter noble gases xenon and krypton can be made to react with fluorine under special conditions, while argon will undergo chemical transformations only with hydrogen fluoride.[18] Nitrogen, with its very stable triple bonds, requires electric discharge and high temperatures to combine with fluorine directly.[19] Fluorine reacts with ammonia to form nitrogen and hydrogen fluoride .

text: Chemical characteristics, effects of presence in a molecule[edit]

text: Fluorine's chemistry is dominated by its strong tendency to gain an electron. It is the most electronegative element and elemental fluorine is a strong oxidant. The removal of an electron from a fluorine atom requires so much energy that no known reagents are known to oxidize fluorine to any positive oxidation state.[20]

text:
Therefore, fluorine's only common oxidation state is −1. It differs from this value in elemental fluorine, where the atoms are bonded to each other and thus at oxidation state 0, and a few polyatomic ions: the very unstable anions F−
2 and F−
3 with intermediate oxidation states exist at very low temperatures, decomposing at around 40 K.[21] Also, the F+
4 cation and a few related species have been predicted to be stable.[22]

text: Fluorine forms compounds with all elements except neon and helium. In particular, it forms binary compounds, named fluorides, with all said elements except argon. All of the elements up to einsteinium, element 99, have been checked except for astatine and francium,[23] and fluorine is also known to form compounds with mendelevium, element 101,[24] rutherfordium, element 104,[25] and seaborgium, element 106.[26]

text: As a result of its small size and high negative charge density, the fluoride anion is the "hardest" base (i.e., of low polarizability). Because of this, fluorides in real salt crystals often have higher effective charges than oxides of the same metal, even though oxygen's formal charge is twice as great as fluorine's.[citation needed]

text:
As a part of a molecule, it is a part with great inductive effect. In the latter case, it significantly increases the acidity of a molecule: the anion formed after giving the proton off becomes stable as a result. Consider acetic acid and its mono-, di-, and trifluoroacetic derivatives and their pKa values (4.74, 2.66, 1.24, and 0.23[note 2]);[27] in other words, the trifluoro derative is 33,800 times stronger an acid than acetic.[28] Fluorine is a principal component of the strongest known charge-neutral acid, H
2FSbF
6.[29] There is evidence for an even stronger acid, H
2FAuF
6, but it has not proved isolable.[30]

text: In a molecule that is composed of a central atoms and fluorines attached to it, the intermolecular bonding is not very strong. Moreover, the dense negative balls that fluorines are repel each other. Therefore, the intermolecular bonding strength falls further down, a result of which is the low melting point of high fluorides.[citation needed]

text: Hydrogen fluoride[edit]

text:
HF and H2O similarities

Boiling points of the hydrogen halides (blue) and hydrogen chalcogenides (red): HF and H2O break trends.
Freezing point of HF/ H2O mixtures: arrows indicate compounds in the solid state.

text: Fluorine combines with hydrogen to make a compound (HF) called hydrogen fluoride or, especially in the context of water solutions, hydrofluoric acid. The H-F bond type is one of the few capable of hydrogen bonding (creating extra clustering associations with similar molecules). This influences various peculiar aspects of hydrogen fluoride's properties. In some ways the substance behaves more like water, also very prone to hydrogen bonding, than one of the other hydrogen halides, such as HCl.[31][32][33]

text: Hydrogen bonding amongst HF molecules gives rise to high viscosity in the liquid phase and lower than expected pressure in the gas phase. Hydrogen fluoride does not boil until 20 °C in contrast to the heavier hydrogen halides which boil between −85 °C and −35 °C (−120–30 °F). HF is fully miscible with water (will dissolve in any proportion), while the other hydrogen halides have large solubility gaps with water. Hydrogen fluoride and water also form several compounds in the solid state, most notably a 1:1 compound that does not melt until −40 °C (−40 °F), which is 44 degrees Celsius (79 degrees Fahrenheit) above the melting point of pure HF.[34]

text:
Unlike other hydrohalic acids, such as hydrochloric acid, hydrogen fluoride is only a weak acid in water solution, with acid dissociation constant(pKa) equal to 3.19.[35] HF's weakness as an aqueous acid is paradoxical considering how polar the HF bond is, much more so than the bond in HCl, HBr, or HI. The explanation for the behavior is complicated, having to do with various cluster-forming tendencies of HF, water, and fluoride ion, as well as thermodynamic issues.[note 3] At great concentrations, a property called homoconjugation is revealed. HF begins to accept fluoride ions, forming the polyatomic ions (such as bifluoride, HF−
2) and protons, thus greatly increasing the acidity of the compound.[37] Hydrofluoric acid is also the strongest of the hydrohalic acids in acetic acid and similar solvents.[38] Its hidden acidity potential is also revealed by the fact it protonates acids like hydrochloric, sulfuric, or nitric.[39] Despite its weakness, hydrofluoric acid is very corrosive, even attacking glass (hydrated only).[37]

text: Dry hydrogen fluoride dissolves low-valent metal fluorides readily. Several molecular fluorides also dissolve in HF. Many proteins and carbohydrates can be dissolved in dry HF and can be recovered from it. Most non-fluoride inorganic chemicals react with HF rather than dissolving.[40]

text: Metal fluorides[edit]

text: Metal fluorides have similarities with other metal halides but are more ionic. In many respects, metal fluorides differ from other metal halides (chlorides, bromides, iodides), very similar to each other. Instead, fluorides are more similar to oxides, often having similar bonding and crystal structures.[41]

text: The metal fluorides show broad trends based on the charge of the metal. Metals in an oxidation state of +3 or lower tend to form ionic, refractory, fluorides. Metals charged +5 or higher tend to form covalently bonded fluorides, polymers or discrete molecules, and are more volatile. (The tetrafluorides are a transition zone.) The bonding variations mean that metal fluorides can be solids,[42] liquids,[43] or gases[44] at room temperature.

text: The solubility of fluorides varies greatly but tends to decrease as the charge on the metal ion increases. Dissolved fluorides produce basic solutions. (F− is a weak base because HF is a weak acid.)[45]

text:
The fluorides of transition metal elements 25–29

Manganese difluoride
Iron trifluoride
Cobalt difluoride
Nickel difluoride
Copper difluoride

text: Low oxidation state metal fluorides[edit]

text: The alkali metals form monofluorides. All are soluble and have the sodium chloride (rock salt) structure,[46] which is also adopted by some alkaline earth oxides such as CaO.[47] Because the fluoride anion is highly basic, many alkali metal fluorides form bifluorides with the formula MHF2. Among other monofluorides, only silver(I)[48] and thallium(I)[49] fluorides are well-characterized. Both are very soluble, unlike the other halides of those metals.

text: Unlike the monofluorides, the difluorides may be either soluble or insoluble. Several transition metal difluorides, such as those of copper(II) and nickel(II), are soluble.[48] The alkaline earth metals form difluorides that are insoluble.[48] In contrast, the alkaline earth chlorides are readily soluble.[48]

text: Many of the difluorides adopt the fluorite structure, named after calcium fluoride (and also adopted by several metal dioxides such as CeO2, UO2, ThO2, etc.), which surrounds each metal cation with 8 fluorides. Some difluorides adopt the rutile structure, named after a form of titanium dioxide and adopted by several other metal dioxides also. The structure is tetragonal and puts metal atoms in octahedral coordination.

text: Beryllium difluoride is different from the other difluorides. In general, beryllium has a tendency to bond covalently, much more so than the other alkaline earths and its fluoride is partially covalent (although still more ionic than its other halides). BeF2 has many similarities to SiO2 (quartz) a mostly covalently bonded network solid. BeF2 has tetrahedrally coordinated metal and forms glasses (is difficult to crystallize). When crystalline, beryllium fluoride has the same room temperature crystal structure as quartz and shares many higher temperatures structures also.

text: Beryllium difluoride is very soluble in water,[48] unlike the other alkaline earths. (Although they are strongly ionic, they do not dissolve because of the especially strong lattice energy of the fluorite structure.) However, BeF2 has much lower electrical conductivity when in solution or when molten than would be expected if it were fully ionic.[50][51][52][53]

text:
Order and disorder in difluorides

The fluorite structure, adopted by many difluorides
Disordered structure of beryllium fluoride glass (sketch, two dimensions)

text: Many metals form trifluorides, such as iron, bismuth, the rare-earth elements, and the metals in the aluminium and scandium columns of the periodic table. The trifluorides of many rare earths, as well as bismuth, have the YF3 structure. Trifluorides of plutonium, samarium (at high temperature), and lanthanum adopt the LaF3 structure. Iron and gallium trifluorides have the FeF3 structure, which is similar to rhenium trioxide. Only ScF3 is cubic (ReO3) at ambient temperature; this material also has the unusual property of negative thermal expansion, meaning it shrinks on heating, over a quite broad temperature range.

text: Gold trifluoride adopts a structure of linked –AuF4– squares that align in a helix (spiral chain).[54] In contrast to gold's distinctly ionic trifluoride, its trichloride and tribromide are volatile dimeric molecules.[55] Aluminium trifluoride is a high melting point solid which is a monomer in the gas phase, while its other trihalides are low-melting, volatile molecules or linear polymeric chains that form dimers as gases phase.[56] No trifluoride is soluble in water, but several are soluble in other solvents.[57]

text: The tetrafluorides show a mixture of ionic and covalent bonding. Zirconium, hafnium, plus many of the actinides form tetrafluorides with an ionic structure that puts the metal cation in an 8-coordinate square antiprism.[58][59] Melting points are around 1000 °C.[60]

text: Titanium and tin tetrafluorides are polymeric, with melting points below 400 °C. (In contrast, their tetrachlorides are molecular and liquids at room temperature.) Vanadium tetrafluoride has a similar structure to tin's[61] and disproportionates at 100–120 °C to the trifluoride and the pentafluoride.

text: The tetrafluorides of iridium, platinum, palladium, and rhodium all share the same structure which was not known until 1975. They have octahedrally coordinated metal atoms with four of the fluorines shared and two unshared. The melting points, where known, are below 300 °C.

text: Manganese tetrafluoride is an unstable solid that decomposes even at room temperature.[62] Only one of the two allotropes, α-MnF4, is understood. In this compound, manganese forms –MnF6– octahedra which share bridging fluorines to make –Mn4F20– rings which are then further connected three dimensionally.[63]

text:
Some tetrafluoride structures

ZrF4, common tetrafluoride structure
The polymeric structure of SnF4
The –Mn4F20– ring of MnF4

text: High oxidation state metal fluorides[edit]

text: Metal penta- and higher fluorides are all covalently bonded and volatile. This behavior contrasts with the corresponding oxides. Oxygen is a weaker oxidant and inherently more likely to form covalent bonds, but it only forms molecules with six metals (manganese heptoxide, technetium heptoxide, ruthenium tetroxide, osmium tetroxide, plutonium tetroxide,[64] and iridium tetroxide[65]). Fluorine forms molecules with fourteen metals because its small size and single charge as an ion allows surrounding metal atoms with more fluorines than oxygen can.

text: Vanadium, niobium, and tantalum lie in a periodic table column that typically reaches +5 as the highest oxidation state. They form pentafluorides as their highest fluoride. Vanadium pentafluoride is the only non-volatile high-charged metal fluoride, with vanadium being centers of –VF6– octahedrons. The niobium and tantalum pentafluorides, have the same tetrahedrons in their structures, with the difference being the formation of the tetra- (rather than poly-) meric molecules.[66]

text: Bismuth's highest fluoride is a volatile penta species that is a powerful fluorinating agent. In the solid state, it is polymeric, consisting of linear chains of octahedra, sharing axial fluorides. In combination with alkali metals, pentavalent bismuth can form hexafluorobismuthate, [BiF6]−, upon reaction with a fluoride donor, either strong (such as NaF[67][68]) or not (such as XeF4[69]).

text: Many metals that form hexafluorides also can form pentafluorides. For instance, uranium, which has a well-known hexafluoride, also forms two different pentafluoride structures. The room-temperature (alpha) form has the same linear chain structure as bismuth pentafluoride. As a molecular (gas) species, UF5 has a square pyramidal structure.

text:
The structure of bismuth (or alpha-uranium) pentafluoride

Structure of a (XF5)n chain; X=Bi, U.
Packing of chains

text: The metals that make well-characterized hexafluorides include nine metals in the center of the periodic table (molybdenum, technetium, ruthenium, rhodium, tungsten, rhenium, osmium, iridium, and platinum) along with elements 92–94: uranium, neptunium, and plutonium. At room temperature, tungsten hexafluoride is a gas. Molybdenum hexafluoride and rhenium hexafluoride are liquids. The rest are volatile solids.

text: Metal hexafluorides are oxidants because of their tendency to release fluorines: for example, platinum hexafluoride was the first compound to oxidize molecular oxygen[70] and xenon.[71] Polonium also forms a hexafluoride, but it is understudied.[72]

text: Rhenium is the only metal known to bond with seven fluorides, which is the record for number of charged ligands for a charge-neutral metal compound.[73]Rhenium heptafluoride adopts a pentagonal bipyramid molecular geometry. Calculations shows that the currently unknown but perhaps possible iridium heptafluoride[74] (report of synthesis is being prepared[65]), technetium heptafluoride,[75] and osmium heptafluoride[76] will also have this structure.

text: Osmium octafluoride was first reported in 1913, but in 1958 that compound was shown to be actually osmium hexafluoride.[77] A 1993 theoretical study predicted very weak bonds in osmium octafluoride and said that it would be difficult to ever detect experimentally. The study predicted that, if made, OsF8 would have Os–F bonds of two different lengths.[78]

text: Nonmetal fluorides[edit]

text: The nonmetal binary fluorides are volatile compounds. They show a great difference between period 2 and other fluorides. For instance, period 2 elements elements fluorides never exceed the octet in their atoms. (Boron is an exception due to its specific position in the periodic table.) Lower-period elements, however, may form hypervalent molecules, such as phosphorus pentafluoride or sulfur hexafluoride.[79] The reactivity of such species varies greatly—sulfur hexafluoride is inert, while chlorine trifluoride is extremely reactive—but there are some trends based on periodic table locations.

text: Boron trifluoride is a planar molecule. It has only six electrons around the central boron atom (and thus an incomplete octet), but it readily accepts a Lewis base, forming adducts with lone-pair-containing molecules or ions such as ammonia or another fluoride ion which can donate two more electrons to complete the octet.[80] Boron monofluoride is an unstable molecule with an unusual (higher than single) bond to fluorine. The bond order has been described as 1.4 (intermediate between a single and double bond). It is isoelectronic with N2.[81]

text: Silicon tetrafluoride, similar to carbon tetrafluoride and germanium tetrafluoride, adopts a molecular tetrahedral structure.[82] SiF4 is stable against heating or electric spark, but reacts with water (even moist air), metals, and alkalies, thus demonstrating weak acidic character.[83] Reactions with organomagnesium compounds, alcohols, amines, and ammonia yield adduction compounds.[83] Fluorosilicic acid, a derivative of SiF4, is a strong acid in aqueous solution (the anhydrous form does not exist).[84]

text:
Pnictogens (nitrogen's periodic table column) show very similar trends in reactivity and acidity of the highest fluorides (pentafluorides) and most common ones (trifluorides), with the said property increasing down the group: NF3 is stable against hydrolysis,[85] PF3 hydrolyzes very slowly in moist air,[86] while AsF3 completely hydrolyzes.[85] SbF3 hydrolyzes only partially because of the increasing ionic character of the bond to fluorine. The compounds are weak Lewis bases, with NF3 again being an exception.[85] The pentafluorides of phosphorus[86] and arsenic[87] are much more reactive than their trifluorides; antimony pentafluoride is such a strong acid that it holds the title of the strongest Lewis acid.[87] Nitrogen is not known to form a pentafluoride, although the tetrafluoroammonium cation (NF+
4) features nitrogen in the formal oxidation state of +5.[88] Nitrogen monofluoride is a metastable species that has been observed in laser studies. It is isoelectronic with O2 and like BF, unusually, has a higher bond order than single-bonded fluorine.[2][89]

text:
The chalcogens (oxygen's periodic table column) are somewhat similar: The tetrafluorides are thermally unstable and hydrolyze, and are also ready to use their lone pair to form adducts to other (acidic) fluorides. Sulfur and selenium tetrafluorides are molecular while TeF4 is a polymer.[90] The hexafluorides are the result of direct fluorination of the elements (compare: other hexahalides of these elements do not even exist). They increase in reactivity with atomic number: SF6 is extremely inert, SeF6 is less noble (for example, reacts with ammonia at 200 °C (400 °F)), and TeF6 easily hydrolyzes to give an oxoacid.[90] Oxygen's highest fluoride is oxygen difluoride,[90] but fluorine can theoretically (as of 2012) oxidize it to a uniquely high oxidation state of +4 in the fluorocation: OF+
3.[91] In addition, several chalcogen fluorides occur which have more than chalcogen (O2F2,[92] S2F10,[93] etc.).

text:
The well-characterized heavier halogens (chlorine, bromine, and iodine) all form mono-, tri-, and pentafluorides: XF, XF3, and XF5. Of the neutral +7 species, only iodine heptafluoride is known.[94] While chlorine and bromine heptafluorides are not known, the corresponding cations ClF+
6 and BrF+
6, extremely strong oxidizers, are.[95] Astatine is not well-studied, and although there is a report of a non-volatile astatine monofluoride,[96] its existence is debated.[97] Many of the halogen fluorides are powerful fluorinators. Chlorine trifluoride is particularly noteworthy—readily fluorinating asbestos and refractory oxides—and may be even more reactive than chlorine pentafluoride. Used industrially, ClF3 requires special precautions similar to those for fluorine gas because of its corrosiveness and hazards to humans.[98][99]

text: Superacids[edit]

text:
Several important inorganic acids contain fluorine. They are generally very strong because of the high electronegativity of fluorine. One such acid, fluoroantimonic acid (HSbF6), is the strongest charge-neutral acid known.[29] The dispersion of the charge on the anion affects the acidity of the solvated proton (in form of H
2F+): The compound has an extremely low pKa of −28 and is 10 quadrillion (1016) times stronger than pure sulfuric acid.[29] Fluoroantimonic acid is so strong that it protonates otherwise inert compounds like hydrocarbons. Hungarian-American chemist George Olah received the 1994 Nobel Prize in chemistry for investigating such reactions.[100]

text: Noble gas compounds[edit]

text: The noble gases are generally non-reactive because they have fully filled electronic shells, which are extremely stable. Until the 1960s, no chemical bond with a noble gas was known. In 1962, Neil Bartlett used fluorine-containing platinum hexafluoride to react with xenon. He called the compound he prepared xenon hexafluoroplatinate, but since then the product has been revealed to be mixture of different chemicals. Bartlett probably synthesized a mixture of monofluoroxenyl(II) pentafluoroplatinate, [XeF]+[PtF5]−, monofluoroxenyl(II) undecafluorodiplatinate, [XeF]+[Pt2F11]−, and trifluorodixenyl(II) hexafluoroplatinate, [Xe2F3]+[PtF6]−.[101] Bartlett's fluorination of xenon has been called one of the ten most beautiful experiments in the history of chemistry.[102] Later in 1962, xenon was reported to react directly with fluorine to form the di- and tetrafluorides. Since then, chemists have made extensive efforts to form other noble gas fluorides.

text: Having started the noble gases–fluorine compounds class, xenon is also the noble gas to have the most well-known such compounds. Its binary compounds include xenon difluoride, xenon tetrafluoride, and xenon hexafluoride, as well as their derivatives.[103] Xenon forms several oxyfluorides, such as xenon oxydifluoride, XeOF2, by reaction of xenon tetrafluoride with water.[104] Its upper neighbor, krypton, is the only other one to form a well-established compound: krypton difluoride. Krypton tetrafluoride was reported in 1963,[105] but was subsequently shown to be a mistaken identification; the compound seems to be very hard to synthesize now (although even the hexafluoride may exist).[106]

text: In strong accordance with the periodic trends, radon is notably more reactive to oxidizers, including fluorine. It has been shown to readily react with fluorine to form a solid compound, which is generally thought to be radon difluoride. The exact composition is uncertain as the compound is prone to decomposition. Calculations indicate that radon difluoride may be ionic, unlike all other binary noble gas fluorides.[96]

text: The lighter noble gases (helium through argon) do not form stable binary fluorides. Argon forms no binary fluoride, but reacts in extreme conditions with hydrogen fluoride to form argon fluorohydride; it is the only "stable"[note 4] argon compound. Helium and neon do not form any stable chemical compounds at all. Helium forms helium fluorohydride; it has been shown to be unstable in gas phase, but there are specific conditions for which it may be stable.[107] Neon, the least reactive element,[note 5] is not now expected to form a stable compound capable of synthesis.

text:
Oganesson, the last currently known group 18 element, is predicted to form oganesson difluoride, OgF
2, and oganesson tetrafluoride, OgF
4, which is likely to have the tetrahedral molecular geometry.[110] However, only a few atoms of oganesson have been synthesized,[111] and its chemical properties have not been examined.

text: Highest oxidation states: fluorine versus oxygen[edit]

text:
Ruthenium's highest fluoride and oxide

Ruthenium hexafluoride: Six fluorines fit around the ruthenium but only make a +6 oxidation state.
Ruthenium tetroxide: Four oxygens fit around the ruthenium, making a +8 oxidation state.

text: Elements frequently have their highest oxidation state in the form of a binary fluoride. Several elements show their highest oxidation state only in a few compounds, one of which is the fluoride; and some elements' highest known oxidation state is seen exclusively in a fluoride.

text:
For groups 1–5, 10, 13–16, the highest oxidation states of oxides and fluorides are always equal. Differences are only seen in chromium, groups 7–9, copper, mercury, and the noble gases. Fluorination allows some elements to achieve relatively low[note 6] highest oxidation states that are otherwise hard to achieve. For example, no binary oxide is known for krypton, but krypton difluoride is well-studied.[112] At the same time, for some other elements, certain very high oxidation states are known only for the oxygen-based species, not the fluorine-based ones. For the previously mentioned volatile oxides, there are no corresponding hepta- or octafluorides. (For example, ruthenium octafluoride is unlikely to be ever synthesized,[113] while ruthenium tetroxide has even found an industrial use.[114]) The main problem that prevents fluorine from forming the highest states in covalent hepta- and octafluorides is that it is hard to attach such a large number of ligands around a single atom; the number of ligands is halved in analogous oxides.[115][note 7] However, octafluoride anions, such as the octafluoroiodate (IF−
8), octafluorozirconate (ZrF4−
8), and octafluoroxenate (XeF2−
8) anions are well-known.

text:
The highest oxidation states may be uncommon to everyday life, or even industrial usage. For example, the synthesis of mercury tetrafluoride, the first compound to achieve an oxidation state above +2 for a group 12 element, breaking the filled 5d-shell, again showing the significance of the relativistic effects on the heavy elements, and fueling the debate over whether mercury, cadmium, and zinc are transition metals,[116] occurred at cryogenic temperatures and the compound decomposes at the temperatures of solid nitrogen.[117] More unstable still, the only cobalt(V) species, the CoF+
4 cation, has only been observed in gas phase (with no interactions with other atoms, thus no shown stability in any chemical environment).[113] The reason why such unstable species exist is complicated, yet can be summarized as follows on the example of the hypothesized NF
5 molecule: According to the modern calculations, five fluorine atoms and one nitrogen atoms can theoretically arrange themselves in different ways, such as NF
3 and F
2, NF•
4 and F
•, NF
5, etc. The NF
3+F
2 system is of the smallest energy (most stable). However, if a NF
5 molecule was synthesized, it would have to go through a high-energy transitional state, from which it could decay into two molecules. But since the transitional state is higher in energy than the hexatomic molecule, the energy difference would need to be added to reach the transitional state and thus allow the decay. This energy is called reaction activation barrier. (The second decay mode has an analogical position.) Thus if little energy was added (low temperatures), then the compound could exist; however, the synthesis is a serious problem (not yet solved).[118]

text: Organofluorine compounds[edit]

text: The carbon–fluorine chemical bond of the organofluorine compounds is the strongest bond in organic chemistry.[119] Along with the low polarizability of the molecules, these are the most important factors contributing to the great stability of the organofluorines.[120]

text: The carbon–fluorine bond of the smaller molecules is formed in three principal ways: Fluorine replaces a halogen or hydrogen, or adds across a multiple bond. The direct reaction of hydrocarbons with fluorine gas can be dangerously reactive, so the temperature may need to be lowered even to −150 °C (−240 °F).[121] "Solid fluorine carriers", compounds that can release fluorine upon heating, notably cobalt trifluoride,[122] may be used instead, or hydrogen fluoride. After the reaction, the molecular size is not changed significantly, as the elements have very similar van der Waals radii.[120] Direct fluorination becomes even less important when it comes to organohalogens or unsaturated compounds reactions, or when a prefluorocarbon is desired (then HF-based electrolysis is typically used).[123] In contrast, the fluoropolymers are formed by polymerizing free radicals; other techniques used for hydrocarbon polymers do not work in that way with fluorine.[124]

text: The range of organofluorine compounds is diverse, reflecting the inherent complexity of organic chemistry. A vast number of small molecules exist with varying amounts of fluorine substitution, as well as many polymers—research into particular areas is driven by the commercial value of applications.[125]

text:
Some important fluorocarbons

Fluoromethane (methyl
fluoride), used in
semiconductor processing
1,1,1,2-Tetrafluoroethane
(R-134a), a HFC
Dichlorodifluoromethane
(R-12 refrigerant), a CFC
Trifluoromethanesulfonic
acid (triflic acid),
a superacid
Perfluorooctanesulfonic
acid, a fluorosurfactant
(the anion is depicted)
A section of
polytetrafluoroethylene
(Teflon) polymer

text: Small molecules[edit]

text: Monofluoroalkanes (alkanes with one hydrogen replaced with fluorine) may be chemically and thermally unstable, yet are soluble in many solvents; but as more fluorines are in instead of hydrogens, the stability increases, while melting and boiling points, and solubility decrease. While the densities and viscosities are increased, the dielectric constants, surface tensions, and refractive indices fall.[126]

text: Partially fluorinated alkanes are the hydrofluorocarbons (HFCs). Substituting other halogens in combination with fluorine gives rise to chlorofluorocarbons (CFCs) or bromofluorocarbons (BFCs) and the like (if some hydrogen is retained, HCFCs and the like). Properties depend on the number and identity of the halogen atoms. In general, the boiling points are even more elevated by combination of halogen atoms because the varying size and charge of different halogens allows more intermolecular attractions.[127] As with fluorocarbons, chlorofluorocarbons and bromofluorocarbons are not flammable: they do not have carbon–hydrogen bonds to react and released halides quench flames.[127]

text: When all hydrogens are replaced with fluorine to achieve perfluoroalkanes, a great difference is revealed. Such compounds are extremely stable, and only sodium in liquid ammonia attacks them at standard conditions. They are also very insoluble, with few organic solvents capable of dissolving them.[126]

text: However, if a perfluorocarbon contains double or triple bonds (perfluoroalkenes or -alkynes), a very reactive towards ligand accepting result, even less stable than corresponding hydrocarbons.[128] Difluoroacetylene, which decomposes even under liquid nitrogen temperatures,[129] is a notable example. If such a molecule is asymmetric, then the more fluorinated carbon is attacked, as it holds positive charge caused by the C–F bonds and is shielded weakly[128] (similarly to that how unsaturated hydrocarbons attacked by HF add hydrogen to the more hydrogen-rich atom per Markovnikov's rule[130]).

text: Perfluorinated compounds, as opposed to perfluorocarbons, is the term used for molecules that would be perfluorocarbons—only carbon and fluorine atoms—except for having an extra functional group (even though another definition exists[131]). They share most of perfluorocarbon properties (inertness, stability, non-wettingness and insolubility in water and oils, slipperiness, etc.),[132] but may differ because of the functional group properties, although the perfluorocarbon tail differ the group-specific properties as compared to those of hydrocarbon-tailed compounds.

text: The perfluoroalkanesulfonic acids are also very notable for their acidity. The sulfonic acid derivative, trifluoromethanesulfonic acid, is comparable in strength to perchloric acid.[133] These compounds lower surface energy; for this reason, they, especially perfluorooctanesulfonic acid (PFOS, formerly the active component in brand "Scotchgard") have found industrial use as surfactants (see above).[133]

text: If a perfluorinated compound has a fluorinated tail, but also a few non-fluorinated carbons (typically two) near the functional group, it is called a fluorotelomer (such molecules are commercially treated as perfluorinated), but such molecules are more of industrial value than chemical. The chain end may similarly be attached to different functiuonal groups (via the hydrogenized terminal carbon), such as hydroxyl resulting in fluorotelomer alcohols, sulfonate resulting in fluorotelomer sulfonates, etc.[132]

text: Polymers[edit]

text: Fluoropolymers are similar in many regards with smaller molecules; adding fluorine to a polymer affects the properties in the same manner as in small molecules (increasing chemical stability, melting point, reducing flammability, solubility, etc.). Each fluoropolymer has own characteristic properties, though.[124]

text: The simplest fluoroplastic is polytetrafluoroethylene (PTFE, DuPont brand Teflon), which is a simple linear chain polymer with the repeating structural unit:–CF2–. PTFE has a backbone of carbons single bonded in a long chain, with all side bonds to fluorines. It contains no hydrogens and can be thought of as the perfluoro analog of polyethylene (structural unit: –CH2–). PTFE has high chemical and thermal stability, as expected for a perfluorocarbon, much stronger than polyethylene. Its resistance to van der Waals forces makes PTFE the only known surface to which a gecko cannot stick.[134] The compound, however, lacks an ability to transform upon melting, which is not a problem for various PTFE deratives, namely FEP (fluorinated ethylene propylene, with some fluorines replaced with the–CF3 group) or PFA (perfluoroalkoxy, some fluorines replaced with –OCF3). They share most properties with PTFE, but there are still differences, namely maximum usage temperature (highest for the non-flexible PTFE).[135]

text: There are other fluoroplastics other than perfluorinated. Polyvinylidene fluoride (PVDF, structural unit: –CF2CH2–), is an analog of PTFE with half the fluorines. PVF (polyvinyl fluoride, structural unit: –CH2CHF–) contains one one-fourth the fluorines of PTFE. Despite this, it still has many properties of more fluorinated compounds.[136] PCTFE (polychlorotrifluoroethylene, structural unit: –CF2CFCl–) is another important compound. It differs from PTFE by having a quarter of fluorine replaced with chlorines, yet this difference brings even greater hardness, creep resistance, and moisture persistence.[136]

text: Mild fluorination of polyethylene gives does not make all of the plastic lose its hydrogens for fluorine; only a thin layer (0.01 mm at maximum) is then affected. This is somewhat similar to metal passivation: the bulk properties are not affected, but the surface properties are, most notably, a greater vapor barrier. Therefore, they are a cheaper alternative to the perfluoro plastics if only surface is important.[137]

text: Nafion is a structurally complicated polymer. It has a PTFE-like backbone, but also contains side chains of perfluoro ether that end in sulfonic acid(–SO2OH) groups. It also possesses great chemical stability, while exact properties vary with morphology. However, because of the difficult chemical structure, it is also relatively easily converted to an ionomer (shows conductivity) by adding cations like Na+ or by converting into the sulfonic acid rather than the given sulfonyl fluoride. The conductivity is due to that the main carbon chain separates from the side chains, thus forming polar and non-polar regions. This form is also very hydroscopic.[138]

text: Fluoroelastomers, like other elastomers (artificial rubbers), consist of disordered polymer chains connected in three dimensions. The main challenges in making fluorelastomers are cross-linking (reacting the unreactive polymers), as well as removing the HF formed during curing. There are three main families of fluoroelasters. VDF/HFP is a copolymer system of vinylidene fluoride and (at least 20%) hexafluoropropylene. TFE/propylene is another copylymer system with better chemical resistance to some solvents. TFE/PMVE (perfluoromethylvinyl ether) is a copolymer system which creates a perfluorinated fluoroelastomer.[139]

text: Notes[edit]

text:
Jump up ^ In this article, metalloids are not treated separately from metals and nonmetals, but among elements they are closer to. For example, germanium is treated as a metal, and silicon as a nonmetal. Antimony is included for comparison among nonmetals, even though it is closer to metals chemically than to nonmetals. The noble gases are treated separately from nonmetals; hydrogen is discussed in the Hydrogen fluoride section and carbon in the Organic compounds section. P-block period 7 elements have not been studied and thus are not included. This is illustrated by the adjacent image: the dark gray elements are metals, the green ones are nonmetals, the light blue ones are the noble gases, the purple one is hydrogen, the yellow one is carbon, and the light gray elements have unknown properties.
Jump up ^ Lower numbers mean greater acidity; note the scale is logarithmical.
Jump up ^ See citation for more detailed explanation.[36]
Jump up ^ In the context of the noble gas compounds, "stable" means not decaying chemically over time under certain (any count) conditions; other ("meta-stable") compounds are not treated in this overview article.
Jump up ^ Even though helium and neon have no known stable compounds, calculations show that helium may be called slightly less unreactive than neon (it may, unlike neon, form some neutral-charged compounds that will not decay over time in specific conditions, and a stable cation of helium (HeH+), the strongest acid of all species,[108] yet existent) has been known since 1925, while no neon cations are. Additionally, clathrates are known for every noble gas but neon.[109]
Jump up ^ There is no general line where oxidation states are "relatively low" or "relatively high", they rely on specific elements (and defined only for elements that have highest oxides and fluorides are in different oxidation states); in general, +7 and +8 are high, while +4 and below are low. States +5 and +6 rely on element properties, like atomic radius; for a small nitrogen atom, +5 is "high" here, but for larger palladium and platinum +6 is still "low".
Jump up ^ Note that aside from the molecular one, other forms of the highest fluorides are not considered to be possible. Such compounds are extremely unlikely to be completely ionic because of large sixth, seventh, and eighth oxidation energies of all elements, which make the reactions that may produce such compounds highly unfavorable (even though the possible osmium octafluoride may be mostly ionic[78]).


document_title: Dallas Stars

question_text: who scored the first goal in dallas stars history

question_tokens: who scored the first goal in dallas stars history

root

text: Dallas Stars

text: Franchise history[edit]

text: Minnesota North Stars (1967–1993)[edit]

text: The Minnesota North Stars began play in 1967 as part of the NHL's six-team expansion. Home games were played at the newly constructed Metropolitan Sports Center ("Met Center") in Bloomington, Minnesota. Initially successful both on the ice and at the gate, the North Stars fell victim to financial problems after several poor seasons in the mid-1970s.

tag: p

text: In 1978, the North Stars were purchased by the owners of the Cleveland Barons (formerly the California Golden Seals), the Gund brothers, George III and Gordon. With both teams on the verge of folding, the NHL permitted the two failing franchises to merge. The merged team continued as the Minnesota North Stars, but assumed the Barons' place in the Adams Division in order to balance out the divisions, while the Seals/Barons franchise records were retired. The merger brought with it a number of talented players, and the North Stars were revived—they reached the Stanley Cup Finals in 1981, where they lost in five games to the New York Islanders. However, by the early 1990s, declining attendance and the inability to secure a new downtown revenue-generating arena led ownership to request permission to move the team to the San Francisco Bay Area in 1990. The NHL rejected the request and instead agreed to award an expansion franchise, the San Jose Sharks, to the Gund brothers. The North Stars were sold to a group of investors that were originally looking to place a team in San Jose, although one of the group's members, Norman Green, would eventually gain control of the team.[3] In the following season, the Minnesota North Stars made it to the Stanley Cup Finals, only to lose to the Pittsburgh Penguins.

text: After the 1991 season, the North Stars suffered through poor attendance and profitability. The team's fortunes were further impeded by the terms of the settlement with the Gund brothers, in which they were permitted to take a number of North Stars players to San Jose. New owner Norman Green explored the possibility of moving the team to Anaheim, however the NHL decided instead to place the expansion Mighty Ducks there in 1992. In their final two seasons in Minnesota, the team adopted a new logo which omitted the "North" from "North Stars", leading many fans to anticipate the team heading south.[4]

text: Relocation to Dallas (1993–1998)[edit]

text: In 1993, amid further attendance woes and bitter personal controversy, Green obtained permission to move the team to Dallas, and the decision was announced on March 10, 1993.[5] Green was convinced by former Dallas Cowboys quarterback Roger Staubach that Dallas would be a suitable market for an NHL team.[4] The NHL, to quell the controversy, promised the fans of Minnesota a return in the future with a new franchise; that promise was fulfilled in 2000 when Minnesota was awarded the Minnesota Wild as an expansion franchise. The Stars would move into Reunion Arena, built in 1980, the downtown arena already occupied by the Dallas Mavericks.

text: The Stars played their first game in Dallas on October 5, 1993, a 6–4 win against the Detroit Red Wings.[6] In that game, Neal Broten scored the first Stars goal in Dallas. Dallas was an experiment for the NHL. At that time, the Stars would be one of the three southern-most teams in the NHL, along with the newly created Tampa Bay Lightning and Florida Panthers as the NHL's first real ventures into southern non-traditional hockey markets. Though the Stars were relatively still unknown, word of the team spread rapidly, and the immediate success of the team on the ice, as well as Mike Modano's career best season (50 goals, 93 points) helped spur the team's popularity in Dallas. The Stars set franchise bests in wins (42) and points (97) in their first season in Texas, qualifying for the 1994 playoffs. The Stars further shocked the hockey world by sweeping the St. Louis Blues in the first round, but lost to the eventual Western Conference Champion Vancouver Canucks in the second round. The Stars' success in their first season, along with American superstar Mike Modano's spectacular on ice performances would be an integral part of the Stars' eventual franchise success in the immediate years to come. The almost immediate success of the Stars was also helped by a long history of second tier hockey in the area. The minor league Central Hockey League had two teams in the area, the Fort Worth Texans and the Dallas Blackhawks for three decades before the Stars arrival.

text: Green, who had run into financial problems stemming from his business ventures outside of hockey, was forced to sell the team to businessman Tom Hicks in December 1995.[4]

text: Building for a championship[edit]

text: The 1994–95 season was shortened by an owners' lockout. The Stars traded captain Mark Tinordi along with Rick Mrozik to the Washington Capitals before the season began for Kevin Hatcher. Long time North Stars hold-over Neal Broten was named his replacement, although he was traded too after only 17 games to the New Jersey Devils. Broten was replaced by Kevin's younger brother Derian Hatcher as team captain, a role he would serve in for the next decade. The Stars played only 48 games that season posting a record of 17–23–8. Despite the shortened season and the losing record, the Stars again made the playoffs, losing in five games to the Red Wings in the first round.[7]

text: 1995–96 would be the first complete season under new owner Tom Hicks. In the offseason, the Stars traded for former Montreal Canadiens' captain and three-time Frank J. Selke Trophy winner Guy Carbonneau, who was then with the St. Louis Blues. With the Stars struggling to begin the season, general manager and head coach Bob Gainey traded for center Joe Nieuwendyk from the Calgary Flames for Corey Millen and Jarome Iginla, then a Stars prospect. The Stars recorded only 11 wins in the first half of the season, and Bob Gainey relinquished his coaching duties in January to be the full-time general manager for the team. The Stars soon hired Michigan K-Wings head coach Ken Hitchcock to replace him; it would be his first NHL head coaching position. The Stars then traded for Benoit Hogue from the Toronto Maple Leafs late in the season, but ultimately finished in sixth place in the Central Division, missing the playoffs for the first time since moving to Texas.[8]

text: In the 1996 off-season, the Stars continued to revamp their roster, adding defensemen Darryl Sydor from the Los Angeles Kings followed by Sergei Zubov from the Pittsburgh Penguins for Kevin Hatcher. Zubov would serve as the Stars' top defenseman and powerplay quarterback until leaving the NHL in 2009. On the ice, Ken Hitchcock's first season proved to be a good one. The Stars bested their 1994 totals, posting 48 wins and reaching the 100-point mark for the first time in franchise history. The Stars won the Central Division, their first division title since 1983–84 (when they were still the Minnesota North Stars) and were seeded second in the playoffs.[9] Despite the regular season success, the youthful Stars were upset in the first round by the Edmonton Oilers in seven games. Defenseman Grant Ledyard tripped in overtime of Game 7, allowing Todd Marchant to score the game- and series-winning goal on a breakaway against goaltender Andy Moog.

text: In the 1997 off-season, the Stars signed star goaltender Ed Belfour as a free agent after a well publicized falling-out with the San Jose Sharks, who had traded a number of players to the Chicago Blackhawks to obtain him in January in the previous season.[10] Andy Moog was allowed to leave via free agency, but later returned to the Stars as an assistant coach. The 1997–98 season was another banner year for the Stars. The Stars again set franchise records in wins (49) and points (109). Dallas acquired Mike Keane at the deadline from the New York Rangers. The Stars won the franchise's first Presidents' Trophy as the NHL's best regular season team, as well as the Central Division title for the second season in a row. Belfour set franchise season records for goals against average (1.88), wins (37) and just missed out on the Jennings Trophy by one goal to Martin Brodeur of the New Jersey Devils. The Stars were the first overall seed for the 1998 Stanley Cup playoffs and defeated the eighth-seeded San Jose Sharks in six games in the first round. Notorious enforcer Bryan Marchment injured Joe Nieuwendyk's right knee, forcing him to miss the rest of the playoffs with torn ligaments. In the second round, they again met the Edmonton Oilers, this time defeating them in five games. Without Nieuwendyk, however, the Stars lacked the firepower to overcome the defending Stanley Cup champion Detroit Red Wings in the Western Conference Finals, and lost in six games. The Red Wings went on to win their second consecutive Stanley Cup.

text: Dominance, a Stanley Cup, and playoff disappointment (1998–2004)[edit]

text: In the 1998 off-season, after falling just short in the Western Conference Finals, the Stars added what they believed was the final piece toward winning a championship: star goalscoring winger Brett Hull. Hull had already had a magnificent career with the St. Louis Blues, with three consecutive 70-goal seasons and a Hart Memorial Trophy, but a fallout with Blues management led Hull to leave St. Louis via free agency.[11] Additionally, this was the first season for the Stars in the Pacific Division after the 1998 NHL division re-alignment.

text: The Stars 1998–99 season was excellent. The Stars won 51 games, surpassing the 50-win mark for the first time in franchise history. They also recorded 114 points, which still stands today as a franchise record. They won the Pacific Division by 24 points, their third consecutive division title; a second consecutive Presidents' Trophy; the Jennings Trophy as the league's top defensive team; and were awarded the top seed in the 1999 Stanley Cup playoffs. Winger Jere Lehtinen was also awarded the Frank J. Selke Trophy.[12]

text: In the first round of the playoffs, Dallas faced their playoff arch-rivals, the Edmonton Oilers. The Stars swept the Oilers in four tough games, winning Game 4 in the third overtime on a goal by Joe Nieuwendyk. They then faced the St. Louis Blues in the second round. After taking a 2–0 series lead, the Blues stormed back to tie the series. The Stars then won the next two games to beat the Blues in six games. The series again ended on an overtime goal, this time from Mike Modano. In the Conference Finals, they faced the Colorado Avalanche for the first time in Stars history. This would be the first of four playoff meetings between the Stars and Avalanche in the next seven years. After both the Stars and the Avalanche split the first four games at a 2–2 series tie, the Avalanche won Game 5 by a score of 7–5, taking a 3–2 series lead, The Stars rallied winning game six on the road, and game seven at home, both by 4–1 scores.[13]

text: This was the Stars' first Stanley Cup Finals appearance as the Dallas Stars, although they made the finals twice as the Minnesota North Stars. They faced the Eastern Conference champion Buffalo Sabres, who had defeated the Toronto Maple Leafs 4–1 in the Eastern Conference Finals. After splitting the first four games, the Stars vaunted defense would hold the Sabres to only one goal in the next two, winning Game 5 2–0 and Game 6 2–1 on an overtime goal by Brett Hull. Hull's goal at 14:51 of the third overtime was remembered as one of the most controversial goals ever scored. That season, the NHL still had the infamous "crease rule" in effect, which stated that if any player of the attacking team who did not have possession of the puck was in the crease before the puck, then any resulting goal was disallowed. Hull had initially gained possession of the puck outside the crease and had made a shot that was blocked by Buffalo goaltender Dominik Hasek. One of Hull's skates entered the crease as he corralled the rebound, and Hull's second shot scored the Cup-winning goal, followed by a lengthy official review. The goal was eventually allowed, as having simply blocked Hull's shot rather than catching it, Hasek never took possession of the puck away from Hull. Officials therefore determined that rather than calling it a loose puck, Hull would be considered to have had continuous possession of the puck from before his first shot outside the crease. The complexity of the crease rule, and the attendant difficulties in understanding its application by fans and players alike, combined with the controversy arising out of the disputed Cup-winning goal, resulted in the crease rule being repealed the following season. Hull's goal marked the 13th time a Stanley Cup-winning goal was scored in overtime, and only the fourth to be scored in multiple overtimes. This was the only time between 1995 and 2003 that a team other than the New Jersey Devils, Colorado Avalanche or Detroit Red Wings won the Stanley Cup.

text: The team added veterans Kirk Muller, Dave Manson and Sylvain Cote in an effort to defend their Stanley Cup championship in 1999–2000. On December 31, 1999, Brett Hull scored his 600 and 601st career goals in a 5–4 win over the Mighty Ducks of Anaheim. The Stars ultimately won the Pacific Division for the second year in a row, and were seeded second in the Western Conference. Dallas then defeated the Edmonton Oilers and San Jose Sharks in the first and second rounds, both 4–1 series victories. The Stars, for the second season in a row, defeated the Colorado Avalanche in the Western Conference Finals in seven games to reach their second consecutive Stanley Cup Finals, where they met the New Jersey Devils. Because the Devils finished the regular season with one more point than Dallas, the Stars had to play their first playoff series without home ice advantage since 1995.[14] The Stars lost all three games in Reunion Arena in the Finals, and lost the series in Game 6 on a double-overtime goal by New Jersey forward Jason Arnott.

text: Unsuccessful playoff runs[edit]

text: Hoping to win back the Stanley Cup, the Stars again captured the Pacific Division, posting a solid 48–24–8–2 record in the 2000–01 season. In the playoffs, the Stars met the Edmonton Oilers in the first round, battling back-and-forth through the first four games, with each game decided by one goal, including three going into overtime. Game 5 would also go to overtime, as the Stars took a 3–2 series lead on a goal by Kirk Muller. In Game 6 in Edmonton, however, the Stars did not need overtime, advancing to the second round with a 3–1 win. Facing the St. Louis Blues, the Stars would run out of gas, being swept in four straight games. The Game 2 loss would be the last NHL game played in Reunion Arena.

text: Moving into the brand new American Airlines Center for the 2001–02 season, the Stars got off to a slow start to the season, as goaltender Ed Belfour struggled through one of his worst seasons. Coach Ken Hitchcock was eventually fired, being replaced by Rick Wilson. Despite the coaching change, the Stars continued to play poor hockey. With the prospect of missing the playoffs, the Stars traded 1999 Conn Smythe winner Joe Nieuwendyk and Jamie Langenbrunner to the New Jersey Devils in exchange for Randy McKay and Jason Arnott, who scored the game-winning goal in the 2000 Finals against Dallas. The Stars would eventually go on to post a respectable record of 35–28–13–5. However, it would not be enough for the playoffs, as they fell four points short of the final eighth spot in the Western Conference. Following the season, coach Rick Wilson would return to assistant coaching duties, as the Stars brought in Dave Tippett as his replacement.

text: As in the 2002 off-season, Ed Belfour left via free agency to the Toronto Maple Leafs. To begin the 2002–03 campaign, the Stars awarded the starting goaltending position to Marty Turco, who went on to have one of the best seasons in NHL history, posting the lowest goals against average (GAA) since 1940, at 1.76. However, missing 18 games late in the season likely cost him a shot at the Vezina Trophy, awarded to the league's top goaltender. Regardless, the Stars posted the best record in the Western Conference at 46–17–15–4, and along the way, two-way star Jere Lehtinen won his third Frank J. Selke Trophy. In the playoffs, the Stars once again met the Edmonton Oilers, and once again the Oilers would prove a contentious opponent, winning two of the first three games. However, the Stars would prove the better team again by winning the next three games to take the series in six games. The Stars' second round series against the Mighty Ducks of Anaheim got off to an unbelievable start, as the game went deep into overtime tied 3–3. However, Mighty Ducks goaltender Jean-Sebastien Giguere stopped 60 shots as the Ducks scored early in the fifth overtime. Game 2 would be more of the same, as the Ducks stunned the Stars in overtime. Desperately needing a win, the Stars bounced back to take Game 3 in Anaheim. However, the Ducks would take a 3–1 series lead by breaking a scoreless tie late in the third period of Game 4. In Game 5, the Stars finally solved Giguere by scoring four goals to keep their playoff hopes alive. However, the Stars dreams of a return trip to the Stanley Cup Finals would end in heartbreaking fashionm as the Ducks broke a 3–3 tie with 1:06 left in Game 6 on a goal by defenseman Sandis Ozolinsh.

text: Coming off their disappointing playoff loss, the Stars would get off to a shaky start to the 2003–04 season, as they played mediocre hockey through the first three months of the season, posting a sub-.500 record. As the calendar turned to 2004, however, the Stars began to find their game, as they posted a 9–4–3 record in January. As the season wore on, the Stars would get stronger, climbing up the playoff ladder and eventually reaching second place in the Pacific Division, where they finished with a solid 41–26–13–2 record; Marty Turco had another outstanding season, recording a 1.98 GAA. However, the Stars could not carry their momentum into the playoffs, as they were beaten by the Colorado Avalanche in five games in the first round.

text: Post-lockout era (2005–2008)[edit]

text: Coming out of the owners' lockout that cancelled the entire 2004–05 season, the Stars remained one of the strongest teams in the Western Conference for the start of 2005–06, as they won four of their first five games on the way to a solid October. November would be even better for Dallas, as they won 10 of 13 games and took over first place in the Pacific Division, a position they would hold most of the season, as they went on to finish with a terrific record of 53–23–6. One reason for the Stars success was their strong play in shootouts, as forward Jussi Jokinen was nearly automatic, making 10-of-13 shot attempts. Also performing strong in shootouts was Sergei Zubov, who used a slow-but-steady backhand to go 7-for-12, as the Stars ultimately won 12 of 13 games that were settled by a shootout. As the number two seed in the Western Conference, the Stars faced the seventh-seeded Colorado Avalanche. The Stars were favorited to win the Western Conference, and some even predicted them to win the Stanley Cup. However, the Stars would stumble right from the start, losing Game 1 by a score of 5–2 as the Avalanche scored five unanswered goals after the Stars jumped out to a promising 2–0 lead. Game 2 would see the Stars suffer another setback at home, as the Stars lost in overtime 5–4 on a goal by Joe Sakic. On the road in Game 3, the Stars led 3–2 in the final minute before the Avalanche forced overtime on a goal by Andrew Brunette, while Alex Tanguay won the game just 69 seconds into overtime to put the Stars in a 3–0 hole. The Stars would avoid the sweep with 4–1 win in Game 4, but overtime would doom them again in Game 5, as Andrew Brunette scored the series winner at 6:05, ending the Stars' playoffs hopes after just five games.

text: Dallas hosts the All-Star Game (2006–2007 season)[edit]

text: Following the previous season's disappointing first round playoff upset at the hands of the seventh-seeded Avalanche, the Stars made a number of changes during the 2006 off-season. Former Stars goalkeeper Andy Moog was promoted to assistant general manager for player development (he kept his job as goaltending coach) and former player Ulf Dahlen was hired as an assistant coach. The Stars allowed center Jason Arnott, defenseman Willie Mitchell and goaltender Johan Hedberg to leave as free agents. Forward Niko Kapanen was traded to the Atlanta Thrashers and the remaining two years on fan-favorite right-winger Bill Guerin's contract were bought out. The Stars also received Patrik Stefan and Jaroslav Modry in the Atlanta trade, and signed Eric Lindros, Jeff Halpern, Matthew Barnaby and Darryl Sydor as free agents. Young goaltender Mike Smith was promoted to the NHL to serve as Marty Turco's backup. During the season, key future pieces – center Mike Ribeiro and defenseman Mattias Norstrom – were added through separate trades. Young players Joel Lundqvist, Krys Barch, Nicklas Grossmann and Chris Conner all saw significant ice time while other players were out of the lineup with injuries.

text: On September 29, 2006, Brenden Morrow was announced as new team captain, taking the role over from Mike Modano, who had served as the incumbent since 2003.[15] Jere Lehtinen remained the last Minnesota North Star still with the franchise, although he never wore a Minnesota North Stars jersey; he was drafted by the club while it was still in Minnesota. On March 13, 2007, Mike Modano scored his 500th career NHL goal, making him only the 39th player and second American to ever reach the milestone. On March 17, Modano scored his 502nd and 503rd NHL goals, breaking the record for an American-born player, previously held by Joe Mullen.

text: On January 24, 2007, the 55th National Hockey League All-Star Game was held at the American Airlines Center. Defenseman Philippe Boucher and goaltender Marty Turco would represent the Stars as part of the Western Conference All-Star roster. The Stars qualified for the playoffs as the sixth seed in the Western Conference and squared off against the Vancouver Canucks in the first round. Marty Turco delivered three shutout wins in Games 2, 5 and 6, but the Stars' offense failed to capitalize and they lost the series in seven games, the third season in a row that they lost in the first round.

text: Return to playoff prominence (2007–2008 season)[edit]

text: In the 2007 NHL Entry Draft, the Stars drafted the relatively unknown Jamie Benn 129th overall. After starting a lackluster 7–7–3 in the 2007–08 season, General Manager Doug Armstrong was fired by the team.[16] He was replaced by an unusual "co-general manager" arrangement of former assistant GM Les Jackson and former Stars player Brett Hull. On November 8, 2007, Mike Modano became the top American born point scorer of all-time, finishing off a shorthanded breakaway opportunity on San Jose Sharks goaltender Evgeni Nabokov.[17]

text: On February 26, 2008, just hours before the trade deadline, the Stars traded for All-Star center Brad Richards from the Tampa Bay Lightning for backup netminder Mike Smith and forwards Jussi Jokinen and Jeff Halpern.[18] The Stars rallied to a final record of 45–30–7 and qualified for the playoffs as the fifth seed, matching up with the defending Stanley Cup champion, the Anaheim Ducks, in the first round.[19] After a rough end to the season, only winning two games in March of that year, the Stars shocked everyone by winning the first two games of the series in Anaheim, and then would go on to finish off the Ducks in six games, their first playoff series win since 2003. In the second round, the Stars matched up with the Pacific Division champion San Jose Sharks. Once again, the Stars surprised everyone by winning the first two games of the series on the road. In Game 2, Brad Richards tied an NHL record by recording four points in the third period.[20] The Stars would then take a 3–0 lead after a Mattias Norstome overtime goal in Game 3. Captain Brenden Morrow finished the Sharks off in Game 6 with a powerplay goal nearly halfway into the fourth overtime.[21] The win sent the Stars to their first Conference Finals since 2000, where they met the powerhouse Detroit Red Wings. After falling behind 3–0, the Stars made a series of it, however, winning two games before ultimately finally being ousted by the Red Wings in six games.[22]

text: Fast starts to slow finishes (2008–2011)[edit]

text: The 2008–09 season saw the early loss for the season of captain Brenden Morrow to an ACL tear. Off-season free agent acquisition Sean Avery caused a media uproar over comments he made to a Canadian reporter about ex-girlfriend Elisha Cuthbert and her relationship with Calgary Flames' defenseman Dion Phaneuf before a game in Calgary. The incident forced the team to suspend Avery for the season; he was later waived by the Stars. That incident, plus injuries to key players Brad Richards and Sergei Zubov, caused the Stars to tailspin to a 12th-place finish and the first missed playoffs for Dallas since 2002.

text: In the wake of the season, the Stars hired a new general manager, former player and alternate captain Joe Nieuwendyk. Hull and Jackson remained with the Stars, but were reassigned to new roles within the organization. Less than a week after he was hired, Nieuwendyk fired six-season head coach Dave Tippett on June 10, 2009, and hired Marc Crawford the next day as his replacement. Other off-season moves included the addition of Charlie Huddy as assistant coach in charge of defense and the promotions of Stu Barnes and Andy Moog to assistant coaches.

text: The Stars' 2009–10 season was similar to the previous one. Inconsistent play and defensive struggles plagued the team throughout the season, as they failed to adjust to Marc Crawford's new offensively-minded system, and owner Tom Hicks' financial troubles prevented the team from spending more than $45 million on payroll, over $11 million beneath the league salary cap.[23] The Stars failed to win more than three games in a row all season, finished in last in the Pacific Division and repeated their 12th place conference finish from the year before with a record of 37–31–14 for 88 points.[24] This was the first time that they would miss the playoffs two seasons in a row since the Stars moved to Texas. In the off-season, longtime goaltender Marty Turco was let go in favor of Kari Lehtonen to become the team's number one goaltender for the future.[25] In the last game of the season at the Minnesota Wild, Mike Modano was named the game's first star and skated around the rink after the game wearing his North Stars uniform, receiving a rousing ovation.[26]

text: In the 2010 off-season, the Stars released Marty Turco and Mike Modano, the face of the franchise for the past two decades. Modano subsequently signed with the Detroit Red Wings while Turco joined the Chicago Blackhawks. Winger Jere Lehtinen, who played his entire career with the Stars, announced his retirement in December 2010. The team also made key acquisitions, such as winger Adam Burish (who was on the 2010 Stanley Cup champion Chicago Blackhawks) and goaltender Andrew Raycroft. They also gave Jonathan Cheechoo a try-out, but he was cut and later signed with division rivals San Jose Sharks.

text: To begin the 2010 season, the Stars won their first three games, going on a three-game win streak for the first time since the 2007–08 season by beating the New Jersey Devils in overtime, New York Islanders in a shootout and against Mike Modano and the Red Wings. During the third game against the Red Wings, the Stars crowd gave Modano a standing ovation as he was shown on the Jumbotron.

text: After a hot start to the season, the Stars dominated the first half of the season, staying on the Pacific Division lead and staying in the top three spots of the conference. It seemed like the old Stars were back, as through the first half of the season, they went 30–15–6. But after the All-Star Game, the Stars went into a slump, going on numerous losing streaks and blowing games. Through this though, the Stars still remained in the playoff picture. On the day of the trade deadline, the Stars traded James Neal and Matt Niskanen to the Pittsburgh Penguins for defenseman Alex Goligoski. After an awful second half, the Stars still had a chance to make the playoffs by winning all their games in April. They won all of them except for last, as they lost to the Minnesota Wild 5–3, costing them a playoff spot.

text: After missing the playoffs for the third consecutive season, Dallas fired coach Marc Crawford on April 12, 2011.[27] In the spring of 2011, according to Darren Dreger of TSN, the team has been "financially managed" by the NHL for over a year. On June 16, 2011, Dallas hired Glen Gulutzan to be head coach, making him the sixth coach since the franchise's move from Minnesota.[28] On September 13, 2011, lenders voted to agree to have the Stars file for bankruptcy and sold at auction.[29] On September 21, 2011, Mike Modano announced his retirement from the NHL. By October 22, 2011, competing bids to buy the club were due. Vancouver businessman and Kamloops Blazers owner Tom Gaglardi's bid was the only one submitted, clearing the way for him to enter the final stages of taking over ownership of the team. Gaglardi's purchase was approved by the NHL Board of Governors on November 18, 2011.[29]

text: A bankruptcy court judge approved the bid for an enterprise value of $240 million. First lien creditors got about 75 cents on the dollar. The Stars lost $38 million during their the last fiscal year and $92 million over the last three seasons.[30]

text: Tom Gaglardi era (2011–present)[edit]

text: As the new owner, Gaglardi's first move was bringing back former Stars President Jim Lites to once again take the reins as team president and CEO. To begin the 2011–12 season, the Stars once again jumped out to a fast start, going 22–15–1 through the first 38 games of the season. When the second half of the season began, however, the Stars slumped through the months of January and February, before getting hot again in late February. Throughout March, the Stars regained the lead of the Pacific Division. Beginning on March 26, 2012, the Stars embarked on a western road trip that saw them visit the Calgary Flames, Edmonton Oilers, Vancouver Canucks and San Jose Sharks. Going into the road trip, the Stars were in control of their own destiny, having to gain four points on the road trip to win their first Pacific Division title since the 2005–06 season. After the Stars lost 5–4 in Calgary to the Flames, the Stars beat the Oilers two nights later, 3–1. This would be their last win of the season, as the Stars were rolled over by the Canucks and Sharks. Even though they had lost the division crown, the Stars still had a chance to clinch a playoff spot. The Stars, however, were eliminated from playoff contention on April 5 in a 2–0 loss to the playoff-bound Nashville Predators. The team failed to qualify for the post-season for the fourth consecutive year, setting a franchise record for futility.[31][32]

text: On July 1, 2012, the team signed free agent veterans Ray Whitney, Aaron Rome and future Hockey Hall of Famer Jaromir Jagr. The next day, the Stars traded fan-favorite Steve Ott and Adam Pardy to the Buffalo Sabres for center Derek Roy. When 2012–13 NHL lockout ended, the Stars began an up-and-down season, although staying in the race for one of the eight playoff spots in the shortened season, which had only 48 games. In mid-season, forward Michael Ryder was traded to his former team, the Montreal Canadiens, for Erik Cole. This shocked many Stars fans, as Ryder was a fan-favorite to Stars fans and had been producing good stats for the Stars throughout the shortened season. Before the trade deadline in early April, the Stars began to falter, and the team's captain, Brenden Morrow, was traded to the Pittsburgh Penguins; Roy was traded to the Vancouver Canucks; Jagr to the Boston Bruins; and Tomas Vincour to the Colorado Avalanche to close out the trade deadline, all in exchange for draft picks and prospects.[33] After all of the trades at the NHL trade deadline, many counted the Stars out, as it seemed they were beginning to rebuild and throw in the towel during the season. However, the Stars' remaining young players pulled together to win six of their next eight games, thus propelling the Stars back into the 2013 playoff race. The Stars soon became the new Cinderella team and were getting better as their new-found success went on. However, the Stars dropped their final five games, losing all of them and gaining only one point in their final five games, which eliminated them from playoff contention. The Stars had now missed the playoffs for five-straight seasons, continuing to set the all-time record in the franchise (dating back to the Minnesota days) for most consecutive seasons without a playoff appearance.

text: The day after their final regular season game of the 2012–13 season (a 3–0 loss to the Detroit Red Wings), the Stars fired General Manager Joe Nieuwendyk. The next day, the Stars introduced their 11th all-time general manager, Jim Nill, the former assistant general manager of the Red Wings. On May 14, 2013, the coaching staff was also fired,[34] and on May 31, 2013, Scott White was re-introduced as the director of hockey operations.[35] Nill made his first big trade as general manager when he acquired Tyler Seguin, Rich Peverley and Ryan Button from the Boston Bruins for Loui Eriksson, Reilly Smith, Matt Fraser and Joe Morrow. Under new head coach Lindy Ruff, the Stars made it to the 2014 playoffs with a successful run on a 40–31–11 record, finishing fourth in the new-look Central Division for the 2013–14 season. They lost in the first round of the playoffs to the Anaheim Ducks in six games with a 4–2 Game 6 loss.

text: Nill made another big trade as general manager when he acquired Jason Spezza and Ludwig Karlsson from the Ottawa Senators in exchange for Alex Chiasson, Nick Paul, Alex Guptill and a second-round pick in 2015. He also signed Senators player Ales Hemsky as a free agent on a three-year, $12 million contract on July 1, 2014. Despite these moves, the Stars finished with the second-lowest goaltender save percentage in the NHL during the 2014–15 season, which resulted in them failing to qualify for the 2015 playoffs due to their sixth-place finish in the Central Division. The lone bright spot of the 2014–15 season was Jamie Benn winning the Art Ross Trophy. On April 11, 2015, Benn scored 4 points in the Stars' last regular season game to finish with 87 points on the season and win the Art Ross Trophy. His final point, a secondary assist with 8.5 seconds left in the game, allowed him to overtake John Tavares for the award.[36]

text: In the 2015–16 season, the Stars won their first Central Division title since 1998 and posted the best regular season record in the Western Conference. In the first round of the playoffs, they defeated the Minnesota Wild in six games. In the second round, they faced the St. Louis Blues, for the first time since 2001, and lost the series in seven games. The Stars finished with a 34–37–11 record in the 2016–17 season, missing the playoffs for the seventh time in the past nine seasons. As a result, the team announced that head coach Lindy Ruff's contract would not be renewed.

text: Team information[edit]

text: Logo and jersey design[edit]

text: When they debuted in Dallas for the 1993–94 season, they kept the same uniform design from their later Minnesota days, except for the addition of the Texas logo patch on the shoulders. Away uniforms were black and home uniforms were white. With minor trim changes, a darker shade of green, and the word 'Dallas' added in the 1994–95 season, they kept this design until their 1999 Stanley Cup-winning campaign. The black pants have the word 'Dallas' in gold run through the sides with green stripes.

text: In the 1997–98 season, the Stars introduced an alternate uniform that partly resembled those worn during the All-Star Game at the time. The uniform was mostly green on top and black at the bottom, in a star-shaped design. For the 1999–2000 season, it became the primary away uniform, and was paired with a new home uniform featuring the same basic design, with white on top and green at the bottom. They kept this design until the 2006–07 season, during which the NHL switched color designations on home and away jerseys in the 2003–04 season. The striping was also eliminated on the black pants.

text: The Stars introduced an alternate jersey for the 2003–04 season that proved both embarrassing and unpopular to critics and fans. The uniform, which was black with a green bottom and red trim, featured a modern representation of the constellation Taurus topped by a trailing green star with red trail marks. However, fans and critics derided the uniform crest for its resemblance to a uterus, nicknaming it the "Mooterus". The uniform was used until the 2005–06 season.

text: With the switch to the Reebok Edge uniform system, the jerseys underwent a complete redesign. The home black jersey, introduced for the 2007–08 season, features the player's number on the chest and an arched 'Dallas' in white with gold trim, with the primary logo on the shoulders. The primary away jerseys, which were used from 2007–10 and was used as an alternate for its final season, had the Stars logo crest in front and the uniform number on the top right, with the Texas alternate logo on the shoulders. An alternate white jersey based on the home black jersey was introduced for the 2008–09 season; they became the regular away uniforms for the 2010–11 season. The lettering is in green with gold and black trim. Both uniforms were used until the 2012–13 season.

text: A new logo and uniforms were introduced for the 2013–14 season. Silver replaced gold as the tertiary color, while green (in a bright new shade called "Victory Green", similar to the old North Stars' shade of green) was reintroduced as a primary uniform color. The new logo features the letter D centering a star, symbolizing Dallas' nickname as "The Big D". The home uniforms are in green with black and white striping, while the away uniforms are in white with a green shoulder yoke, and black and green striping. The inner collar features the team name on the home uniforms, and the city name on the away uniforms. The secondary logo, with the primary inside a roundel with the team name, is featured in the shoulders.

text: Arena[edit]

text: When the Stars first moved from Minnesota, the Stars moved into Reunion Arena, which was being shared with the NBA's Dallas Mavericks. For hockey, Reunion Arena held 17,001 for NHL games. Throughout the hockey history of Reunion Arena, the arena was known for having one of the worst ice surfaces in the NHL, especially in its final days hosting the Stars. The Stars played at Reunion for eight years, from 1993–2001. Before the 2001–02 NHL season, Both the Stars and the Mavericks moved into the American Airlines Center, which is in the Victory Park neighborhood of Dallas, just north of Reunion Arena. The American Airlines center holds 18,584 for Stars and NHL games. On January 24, 2007, the AAC hosted the 55th National Hockey League All-Star Game. The AAC and the Dallas Stars have won several local and NHL awards for "Best Fan Experience".[37]

text: Traditions[edit]

text: Since the 2005–06 season, the national anthems are performed by Celena Rae, a Fort Worth native and former semi-finalist on American Idol. During The Star-Spangled Banner, the fans yell the word "stars" in the lines "whose broad stripes and bright stars" and "O say does that star spangled banner yet wave."[38] At games, as part of the entertainment, a Kahlenberg KDT-123 fog horn sounds after every Stars goal.[39]

text: When the Stars take the ice at the beginning of each game, the song "Puck Off" (also referred to as the "Dallas Stars Fight Song") by Pantera, is played in the arena. Members of the Dallas–Fort Worth–Arlington metropolitan area band had become friends with members of the Stars in the 1990s, especially following the team's Stanley Cup win in 1999.[40] "Puck Off" later also became the team's goal celebration song. During the song, fans chant the only lyrics in the song, "Dallas! Stars! Dallas! Stars!" while pumping their fists in the air. After each Stars win, the Stevie Ray Vaughan (a Dallas native) and Double Trouble song "The House is Rockin'" is played. A song of unknown origin called "The Darkness Music" is played after nearly every away goal.[41] In recent years, fans have usually yelled, "Who cares!?" after away team goals are announced by the public address announcer.[42]

text: The Stars have hosted a home game on New Year's Eve every year since 1997. For a period of time, the game coincided with the Big D NYE celebration (now on hiatus) on the south side of the arena in AT&T Plaza.[43]

text: Broadcast[edit]

text: All Dallas Stars games are broadcast on radio on KTCK under a five-year deal announced in January 2009.[44] KTCK replaced WBAP, which had broadcast games since the beginning of the 1994 season after KLIF has broadcast the first season in Dallas in 1993. Television coverage occurs primarily on Fox Sports Southwest (FSN), with KTXA (Channel 21) or FSSW+ broadcasting games when FSSW has a conflict.

text: The Stars, along with the Buffalo Sabres, are one of only two NHL teams to simulcast the entirety of their games on TV and radio, which the team has done since their 1993 arrival in Dallas. The original broadcast team from 1993 to 1996 was Mike Fornes (play-by-play) and Ralph Strangis (color). Fornes left the broadcast team after the 1995–96 season; Strangis moved to the play-by-play role and color commentator Daryl "Razor" Reaugh was added. Although both the DFW-area's large media market and the team's fan base could theoretically support separate television and radio broadcast teams, the Stars have continued simulcasting due to the popularity of "Ralph and Razor" (as they are known) among local listeners and viewers. Like other NHL teams, the Stars now have a live radio broadcast transmitted inside American Airlines Center on 97.5 FM. This is done because AM radio signals often cannot penetrate concrete and steel building exteriors.

text: Strangis retired from the booth after the 2014–15 season and was replaced by Dave Strader. In June 2016, Strader was diagnosed with cholangiocarcinoma, a fairly rare and aggressive form of cancer of the bile duct. To begin the 2016–17 season, Reaugh assumed play-by-play duties while Strader underwent treatment. Studio analyst and former Stars defenseman, Craig Ludwig, took over as color commentator. During a break in Strader's treatment, he returned to the broadcast booth on February 18, 2017, a 4-3 overtime home win against the Tampa Bay Lightning. After the game, the Stars saluted Strader at center ice. Tragically, on October 1, 2017, Strader passed away, succumbing to the cancer at the age of 62. The 2017–18 season saw Reaugh and Ludwig promoted permanently.

text: Affiliated teams[edit]

text: Texas Stars[edit]

text: The Texas Stars are the affiliate of the Dallas Stars, who after becoming unaffiliated with the Iowa Stars of the AHL, did not have an AHL affiliate for the 2008–09 season. The Texas Stars began play in the AHL in the 2009–10 season. They are located in Cedar Park, Texas (Northwest of Austin).

text: Idaho Steelheads[edit]

text: The Idaho Steelheads are the Stars' ECHL affiliate. Based in Boise, the Steelheads have played home games in CenturyLink Arena Boise since 2003.

text: Season-by-season record[edit]

text: This is a partial list of the last five seasons completed by the Stars. For the full season-by-season history, see List of Dallas Stars seasons

text: Note: GP = Games played, W = Wins, L = Losses, OTL = Overtime losses, Pts = Points, GF = Goals for, GA = Goals against

text:
Season
GP
W
L
OTL
Pts
GF
GA
Finish
Playoffs

2012–13
48
22
22
4
48
130
142
5th, Pacific
Did not qualify

2013–14
82
40
31
11
91
235
228
5th, Central
Lost in First Round, 2–4 (Ducks)

2014–15
82
41
31
10
92
261
260
6th, Central
Did not qualify

2015–16
82
50
23
9
109
267
230
1st, Central
Lost in Second Round, 3–4 (Blues)

2016–17
82
34
37
11
79
223
262
6th, Central
Did not qualify

tag: table

text: Players[edit]

text: Current roster[edit]

text:
view
talk
edit

tag: ul

text: Updated February 25, 2018[45][46]

text:
#
Nat
Player
Pos
S/G
Age
Acquired
Birthplace

7001140000000000000♠14
Canada !
Benn, JamieJamie Benn (C)
4.2 !C/LW
L
28
2007
Victoria, British Columbia

7001300000000000000♠30
United States !
Bishop, BenBen Bishop
1.0 !G
L
31
2017
Denver, Colorado

7001400000000000000♠40
Canada !
Elie, RemiRemi Elie
6.0 !LW
L
22
2013
Green Valley, Ontario

7001120000000000000♠12
Czech Republic !
Faksa, RadekRadek Faksa
4.0 !C
L
24
2012
Vítkov, Czech Republic

7000200000000000000♠2
Canada !
Hamhuis, DanDan Hamhuis
2.0 !D
L
35
2016
Smithers, British Columbia

7001100000000000000♠10
Czech Republic !
Hanzal, MartinMartin Hanzal
4.0 !C
L
31
2017
Pisek, Czechoslovakia

7000600000000000000♠6
Finland !
Honka, JuliusJulius Honka
2.0 !D
R
22
2014
Jyväskylä, Finland

7001130000000000000♠13
Sweden !
Janmark, MattiasMattias Janmark
4.0 !C
L
25
2015
Danderyd, Sweden

7001280000000000000♠28
United States !
Johns, StephenStephen Johns
2.0 !D
R
25
2015
Ellwood City, Pennsylvania

7000300000000000000♠3
Sweden !
Klingberg, JohnJohn Klingberg (A)
2.0 !D
R
25
2010
Lerum, Sweden

7001320000000000000♠32
Finland !
Lehtonen, KariKari Lehtonen
1.0 !G
L
34
2010
Helsinki, Finland

7001230000000000000♠23
Finland !
Lindell, EsaEsa Lindell
2.0 !D
L
23
2012
Helsinki, Finland

7001330000000000000♠33
Canada !
Methot, MarcMarc Methot
2.0 !D
L
32
2017
Ottawa, Ontario

7001290000000000000♠29
United States !
Pateryn, GregGreg Pateryn
2.0 !D
R
27
2017
Sterling Heights, Michigan

7001180000000000000♠18
United States !
Pitlick, TylerTyler Pitlick
7.0 !RW
R
26
2017
Minneapolis, Minnesota

7001470000000000000♠47
Russia !
Radulov, AlexanderAlexander Radulov (A)
7.0 !RW
L
31
2017
Nizhny Tagil, Soviet Union

7001250000000000000♠25
Canada !
Ritchie, BrettBrett Ritchie
7.0 !RW
R
24
2011
Orangeville, Ontario

7001210000000000000♠21
France !
Roussel, AntoineAntoine Roussel
6.0 !LW
L
28
2012
Roubaix, France

7001910000000000000♠91
Canada !
Seguin, TylerTyler Seguin (A)
7.2 !RW/C
R
26
2013
Brampton, Ontario

7001170000000000000♠17
Canada !
Shore, DevinDevin Shore
4.0 !C
L
23
2012
Ajax, Ontario

7001460000000000000♠46
Canada !
Smith, GemelGemel Smith
4.0 !C
L
23
2012
Toronto, Ontario

7001900000000000000♠90
Canada !
Spezza, JasonJason Spezza (A)
4.0 !C
R
34
2014
Mississauga, Ontario

text: Retired numbers[edit]

text:
Dallas Stars retired numbers

No.
Player
Position
Career
Date of retirement

7
Neal Broten 1
C
1981–1995, 1997
February 7, 1998

8
Bill Goldsworthy 2
RW
1967–1977
February 15, 1992

9
Mike Modano 1
C
1989–2010
March 8, 2014

19
Bill Masterton 2
C
1967–1968
January 17, 1987

26
Jere Lehtinen
RW
1995–2010
November 24, 2017[47]

text: Notes:

text:
1 Broten and Modano both began their careers with the North Stars and continued to play with the team when the franchise moved to Dallas.
2 Goldsworthy and Masterton played exclusively for the Minnesota North Stars; Dallas continues to honor their retired numbers.
The NHL retired Wayne Gretzky's No. 99 for all its member teams at the 2000 NHL All-Star Game.[48]

text: Team captains[edit]

text: Note: This list does not include former captains of the Minnesota North Stars and Oakland Seals

text:
Mark Tinordi, 1993–1995
Neal Broten, 1995
Derian Hatcher, 1995–2003
Mike Modano, 2003–2006
Brenden Morrow, 2006–2013
Jamie Benn, 2013–present

text: Hall of Famers[edit]

text: Please see the Hall of Fame section for the Minnesota North Stars for a list of franchise Hockey Hall of Fame members.

text:
Brett Hull, RW, 1998–2001, inducted 2009
Joe Nieuwendyk, C, 1995–2002, inducted 2011
Ed Belfour, G, 1997–2002, inducted 2011
Mike Modano, C, 1989–2010, inducted 2014
Eric Lindros, C, 2006–2007, inducted 2016
Sergei Makarov, RW, 1996, inducted 2016[49]

text: First-round draft picks[edit]

text: Note: This list does not include selections of the Minnesota North Stars.

text:
1993: Todd Harvey (9th overall)
1994: Jason Botterill (20th overall)
1995: Jarome Iginla (11th overall)
1996: Ric Jackman (5th overall)
1997: Brenden Morrow (25th overall)
1998: None
1999: None
2000: Steve Ott (25th overall)
2001: Jason Bacashihua (26th overall)
2002: Martin Vagner (26th overall)
2003: None
2004: Mark Fistric (28th overall)
2005: Matt Niskanen (28th overall)
2006: Ivan Vishnevskiy (27th overall)
2007: None
2008: None
2009: Scott Glennie (8th overall)
2010: Jack Campbell (11th overall)
2011: Jamie Oleksiak (14th overall)
2012: Radek Faksa (13th overall)
2013: Valeri Nichushkin (10th overall)
2013: Jason Dickinson (29th overall)
2014: Julius Honka (14th overall)
2015: Denis Guryanov (12th overall)
2016: Riley Tufte (25th overall)
2017: Miro Heiskanen (3rd overall) and Jake Oettinger (26th overall)

text: Franchise scoring leaders[edit]

text: These are the top-ten point-scorers in franchise (Minnesota & Dallas) history.[50] Figures are updated after each completed NHL regular season.

text: *  – current Stars player

text: Note: Pos = Position; GP = Games Played; G = Goals; A = Assists; Pts = Points; P/G = Points per game

text:
Points

Player
Pos
GP
G
A
Pts
P/G

Mike Modano
C
1,459
557
802
1,359
.93

Neal Broten
C
867
274
593
867
1.00

Brian Bellows
LW
753
342
380
722
.96

Dino Ciccarelli
RW
602
332
319
651
1.08

Bobby Smith
C
572
185
369
554
.97

Sergei Zubov
D
839
111
442
553
.66

Dave Gagner
C
609
247
287
534
.88

Brenden Morrow
LW
835
243
285
528
.63

Jamie Benn*
LW
585
218
299
517
.88

Jere Lehtinen
RW
875
243
271
514
.59

Goals

Player
Pos
G

Mike Modano
C
557

Brian Bellows
LW
342

Dino Ciccarelli
RW
332

Neal Broten
C
274

Bill Goldsworthy
RW
267

Dave Gagner
C
247

Jere Lehtinen
RW
243

Brenden Morrow
LW
243

Steve Payne
LW
228

Jamie Benn*
LW
218

Assists

Player
Pos
A

Mike Modano
C
802

Neal Broten
C
593

Sergei Zubov
D
442

Brian Bellows
LW
380

Bobby Smith
C
369

Dino Ciccarelli
RW
319

Tim Young
C
316

Craig Hartsburg
D
315

Jamie Benn*
LW
299

Dave Gagner
C
287

text: NHL awards and trophies[edit]

text: Stanley Cup

text: Presidents' Trophy

text: 1997–98, 1998–99

text: Clarence S. Campbell Bowl

text: 1998–99, 1999–2000

text: Art Ross Trophy

text: Jamie Benn: 2014–15

text: Conn Smythe Trophy

text: Joe Nieuwendyk: 1998–99

text: Frank J. Selke Trophy

text: Jere Lehtinen: 1997–98, 1998–99, 2002–03

text: Lester Patrick Trophy

text: Neal Broten: 1997–98

text: Roger Crozier Saving Grace Award

text:
Ed Belfour: 1999–2000
Marty Turco: 2000–01, 2002–03

text: William M. Jennings Trophy

text: Ed Belfour and Roman Turek: 1998–99

text: Franchise individual records[edit]

text:
Most goals in a season: Dino Ciccarelli; Brian Bellows, 55 (1981–82; 1989–90)
Most assists in a season: Neal Broten, 76 (1985–86)
Most points in a season: Bobby Smith, 114 (1981–82)
Most penalty minutes in a season: Basil McRae, 378 (1987–88)
Most points in a season, defenseman: Craig Hartsburg, 77 (1981–82)
Most points in a season, rookie: Neal Broten, 98 (1981–82)
Most goals in a season, rookie: Neal Broten, 38 (1981–82)*
Most wins in a season: Marty Turco, 41 (2005–06)
Most shutouts in a season: Marty Turco, 9 (2003–04)