document_title: Charlotte's Web

question_text: what is the girl's name from charlotte's web

question_tokens: what is the girl 's name from charlotte 's web

text: Charlotte's Web

text: Plot summary

text: After her father spares the life of a piglet from slaughtering it as runt of the litter, a little girl named Fern Arable nurtures the piglet lovingly, naming him Wilbur. On greater maturity, Wilbur is sold to Fern's uncle, Homer Zuckerman, in whose barnyard he is left yearning for companionship but is snubbed by other barn animals, until befriended by a barn spider named Charlotte, living on a web overlooking Wilbur's enclosure. Upon Wilbur's discovery that he is intended for slaughter, she promises to hatch a plan guaranteed to spare his life. Accordingly, she secretly weaves praise of him into her web, attracting publicity among Zuckerman's neighbors who attribute the praise to divine intervention. As time passes, more inscriptions appear on Charlotte's webs, increasing his renown. Therefore, Wilbur is entered in the county fair, accompanied by Charlotte and the rat Templeton, whom she employs in gathering inspiration for her messages. There, Charlotte spins an egg sac containing her unborn offspring, and Wilbur, despite winning no prizes, is later celebrated by the fair's staff and visitors (thus made too prestigious alive to justify killing him). Exhausted apparently by laying eggs, Charlotte remains at the fair and dies shortly after Wilbur's departure. Having returned to Zuckerman's farm, Wilbur guards Charlotte's egg sac and is saddened further when the new spiders depart shortly after hatching. The three smallest remain, however, and take up residence in the doorway where Charlotte used to live. Pleased at finding new friends, Wilbur names one of them Nellie, while the remaining two name themselves Joy and Aranea. The book then concludes by mentioning that more generations of spiders kept him company in subsequent years.

text: Characters

text:
Wilbur is a rambunctious pig, the runt of his litter. He is often strongly emotional.
Charlotte A. Cavatica, or simply Charlotte, is a spider who befriends Wilbur. In some passages, she is the heroine of the story.[2]
John Arable: Wilbur's first owner.
Fern Arable, John's daughter, who adopts Wilbur in his infancy, and later visits him. She is the only human in the story capable of understanding nonhuman conversation.
Templeton is a rat who helps Charlotte and Wilbur only when offered food. He serves as a somewhat caustic, self-serving comic relief to the plot.
Avery Arable is the elder brother of Fern. Like Templeton, he is a source of comic relief.
Homer Zuckerman is Fern’s uncle who keeps Wilbur in his barn. He has a wife, Edith, and an assistant named Lurvy.
Other animals in Zuckerman’s barn, with whom Wilbur converses, are a disdainful lamb, a talkative goose, and an intelligent "old sheep".
Henry Fussy is a boy of Fern’s age, of whom Fern becomes fond.
Dr. Dorian is the family physician/psychologist consulted by Fern's mother and something of a wise old man character.
Uncle is a large pig whom Charlotte disdains for coarse manners and Wilbur’s rival at the fair.
Charlotte's children are the 514 children of Charlotte. Although they were born at the barn, all but three of them go their own ways by ballooning.

text: History

text: White's editor Ursula Nordstrom said that one day, in 1952, E. B. White handed her a new manuscript, the only version of Charlotte's Web then in existence, which she read soon after and enjoyed.[3] Charlotte's Web was published three years after White began writing it.[4]

text: Since White published Death of a Pig in 1948,[5] an account of his own failure to save a sick pig (bought for butchering), Charlotte's Web can be seen as White's attempt "to save his pig in retrospect".[6] White's overall motivation for the book has not been revealed and he has written: "I haven't told why I wrote the book, but I haven't told you why I sneeze, either. A book is a sneeze".[7]

text: When White met the spider who originally inspired Charlotte, he called her Charlotte Epeira (after Epeira sclopetaria, the Grey Cross spider, now known as Larinioides sclopetarius), before discovering that the more modern name for that genus was Aranea.[8] In the novel, Charlotte gives her full name as "Charlotte A. Cavatica", revealing her as a barn spider, an orb-weaver with the scientific name Araneus cavaticus.

text: The arachnid anatomical terms (mentioned in the beginning of chapter nine) and other information that White used, came mostly from American Spiders by Willis J. Gertsch and The Spider Book by John Henry Comstock, both of which combine a sense of poetry with scientific fact.[9] White incorporated details from Comstock's accounts of baby spiders, most notably the "flight" of the young spiders on silken parachutes.[9] White sent Gertsch’s book to illustrator Garth Williams.[10] Williams’ initial drawings depicted a spider with a woman’s face, and White suggested that he simply draw a realistic spider instead.[11]

text: White originally opened the novel with an introduction of Wilbur and the barnyard (which later became the third chapter) but decided to begin the novel by introducing Fern and her family on the first page.[10] White’s publishers were at one point concerned with the book’s ending and tried to get White to change it.[12]

text: Charlotte's Web has become White's most famous book; but White treasured his privacy and that of the farmyard and barn that helped inspire the novel, which have been kept off limits to the public according to his wishes.[13]

text: Reception

text: Charlotte's Web was generally well-reviewed when it was released. In The New York Times, Eudora Welty wrote, "As a piece of work it is just about perfect, and just about magical in the way it is done."[14] Aside from its paperback sales, Charlotte's Web is 78th on the all-time bestselling hardback book list. According to publicity for the 2006 film adaptation (see below), the book has sold more than 45 million copies and been translated into 23 languages. It was a Newbery Honor book for 1953, losing to Secret of the Andes by Ann Nolan Clark for the medal. In 1970, White won the Laura Ingalls Wilder Medal, a major prize in the field of children's literature, for Charlotte's Web, along with his first children's book, Stuart Little, published in 1945. Seth Lerer, in his book Children’s Literature, finds that Charlotte represents female authorship and creativity, and compares her to other female characters in children’s literature such as Jo March in Little Women and Mary Lennox in The Secret Garden.[15] Nancy Larrick brings to attention the "startling note of realism" in the opening line, "Where's Papa going with that Ax?"[16]

text: Illustrator Henry Cole expressed his deep childhood appreciation of the characters and story, and calls Garth Williams' illustrations full of “sensitivity, warmth, humor, and intelligence.”[17] Illustrator Diana Cain Bluthenthal states that Williams' illustrations inspired and influenced her.[18]

text: There is an unabridged audio book read by White himself which reappeared decades after it had originally been recorded.[19] Newsweek writes that White reads the story "without artifice and with a mellow charm," and that "White also has a plangency that will make you weep, so don't listen (at least, not to the sad parts) while driving."[19] Joe Berk, president of Pathway Sound, had recorded Charlotte's Web with White in White’s neighbor's house in Maine (which Berk describes as an especially memorable experience) and released the book in LP.[20] Bantam released Charlotte’s Web alongside Stuart Little on CD in 1991, digitally remastered, having acquired the two of them for rather a large amount.[20]

text: In 2005, a school teacher in California conceived of a project for her class in which they would send out hundreds of drawings of spiders (each representing Charlotte’s child Aranea going out into the world so that she can return and tell Wilbur of what she has seen) with accompanying letters; they ended up visiting a large number of parks, monuments, and museums, and were hosted by and/or prompted responses from celebrities and politicians such as John Travolta and then-First Lady Laura Bush.[21]

text: In 2003 Charlotte's Web was listed at number 170 on the BBC's The Big Read poll of the UK's 200 "best-loved novels."[22] A 2004 study found that Charlotte's Web was a common read-aloud book for third-graders in schools in San Diego County, California.[23] Based on a 2007 online poll, the National Education Association named the book one of its "Teachers' Top 100 Books for Children."[24] It was one of the "Top 100 Chapter Books" of all time in a 2012 poll by School Library Journal.[25]

text: Its awards and nominations include:

text:
Newbery Honor Book (1953)[26]
Horn Book Fanfare (1953)[27]
Laura Ingalls Wilder Medal (1970) (awarded to White for his children's books: Charlotte's Web and Stuart Little)
Massachusetts Children's Book Award (1984)[28]

text: Adaptations

text: Film

text: The book was adapted into an animated feature of the same name in 1973 by Hanna-Barbera Productions and Sagittarius Productions with a score by the Sherman Brothers. In 2003, a direct-to-video sequel of that film, Charlotte's Web 2: Wilbur's Great Adventure, was released by Paramount Pictures. In 2006, Paramount Pictures, with Walden Media, Kerner Entertainment Company, and Nickelodeon Movies, produced a live-action/animated adaptation starring Dakota Fanning as Fern and the voice of Julia Roberts as Charlotte, released on December 15, 2006.

text: Stage

text: A musical production was created with music and lyrics by Charles Strouse.

text: Video game

text: A video game of the 2006 film was developed by Backbone Entertainment and published by THQ and Sega, and released on December 12, 2006, for the Game Boy Advance, Nintendo DS, PlayStation 2 and PC.


document_title: Wind the Bobbin Up

question_text: where does the song wind the bobbin up come from

root

text: Wind the Bobbin Up

text: Lyrics[edit]

text: Among modern lyrics is:

tag: p

text: Origins[edit]

text: Iona and Peter Opie traced this rhyme back to Netherlands in the 1890s. When they were collecting games in the 1960s and 1970s the version they encountered was:

text: The game[edit]

text: In the 1970s the game involved two players winding fists around each other. At "Pull, Pull" they pushed their fists away from each other and when "Tug, Tug" was reached they pulled their elbows back.[2] It has now become a much more sedate action game, often with small children carrying out the actions in the lyrics.[1]

text: Notes[edit]

text:
^ Jump up to: a b B. Melling, Creative Activities for the Early Years: Thematic Art and Music Activities (Brilliant Publications, 2005), p. 64.
^ Jump up to: a b I. Opie and P. Opie, The Singing Game (Oxford: Oxford University Press, 1985), pp. 379-82.

tag: ol

text: Singing gamesYear of song unknownEnglish nursery rhymes1890s songsSongwriter unknown

tag: ul


document_title: Properties of metals, metalloids and nonmetals

question_text: are metals mostly solid liquid or gas at room temperature

text: Properties[edit]

text: Metals[edit]

text: Metals appear lustrous (beneath any patina); form mixtures (alloys) when combined with other metals; tend to lose or share electrons when they react with other substances; and each forms at least one predominantly basic oxide.

text: Most metals are silvery looking, high density, relatively soft and easily deformed solids with good electrical and thermal conductivity, closely packed structures, low ionisation energies and electronegativities, and are found naturally in combined states.

text: Some metals appear coloured (Cu, Cs, Au), have low densities (e.g. Be, Al) or very high melting points, are liquids at or near room temperature, are brittle (e.g. Os, Bi), not easily machined (e.g. Ti, Re), or are noble (hard to oxidise) or have nonmetallic structures (Mn and Ga are structurally analogous to, respectively, white P and I).

text: Metals comprise the large majority of the elements, and can be subdivided into several different categories. From left to right in the periodic table, these categories include the highly reactive alkali metals; the less reactive alkaline earth metals, lanthanides and radioactive actinides; the archetypal transition metals, and the physically and chemically weak post-transition metals. Specialized subcategories such as the refractory metals and the noble metals also exist.

text: Metalloids[edit]

text: Metalloids are metallic looking brittle solids; tend to share electrons when they react with other substances; have weakly acidic or amphoteric oxides; and are usually found naturally in combined states.

text: Most are semiconductors, and moderate thermal conductors, and have structures that are more open than those of most metals.

text: Some metalloids (As, Sb) conduct electricity like metals.

text: The metalloids, as the smallest major category of elements, are not subdivided further.

text: Nonmetals[edit]

text: Nonmetals have open structures (unless solidified from gaseous or liquid forms); tend to gain or share electrons when they react with other substances; and do not form distinctly basic oxides.

text: Most are gases at room temperature; have relatively low densities; are poor electrical and thermal conductors; have relatively high ionisation energies and electronegativities; form acidic oxides; and are found naturally in uncombined states in large amounts.

text: Some nonmetals (C, black P, S and Se) are brittle solids at room temperature (although each of these also have malleable, pliable or ductile allotropes).

text: From left to right in the periodic table, the nonmetals can be subdivided into the polyatomic nonmetals which, being nearest to the metalloids, show some incipient metallic character; the diatomic nonmetals, which are essentially nonmetallic; and the monatomic noble gases, which are almost completely inert.

text: Comparison of properties[edit]

text: Overview[edit]

text:
Number of metalloid properties that resemble metals or nonmetals

v
t
e

(or that are reasonably distinct)

     Resemble metals
  Relatively distinctive
  Resemble nonmetals

Properties compared:
(36)
 7 (19%)
25
(68%)
5 (13%)

Physical
(21)
 5 (24%)
14
(67%)
2 (10%)

 •  Presentation & structure
(10)
 2
6

2 (20%)

 •  Electron-related
(6)
 1
5

 •  Thermodynamics
(5)
 2
3

Chemical
(16)
 2 (13%)
11
(69%)
3 (19%)

 •  Elemental chemistry
(6)
 3
3 (50%)

 •  Combined form chemistry
(6)
 2
4

 •  Environmental chemistry
(4)
4

tag: table

text: The characteristic properties of metals and nonmetals are quite distinct, as shown in the table below. Metalloids, straddling the metal-nonmetal border, are mostly distinct from either, but in a few properties resemble one or the other, as shown in the shading of the metalloid column below and summarized in the small table at the top of this section.

text: Authors differ in where they divide metals from nonmetals and in whether they recognize an intermediate metalloid category. Some authors count metalloids as nonmetals with weakly nonmetallic properties.[n 1] Others count some of the metalloids as post-transition metals.[n 2]

text: Detailed[edit]

text:
Physical and chemical properties[n 3]

v
t
e

Metals[8]
Metalloids
Nonmetals[8]

Presentation and structure

Colour

nearly all are shiny and grey-white
Cu, Cs, Au: shiny and golden[9]

shiny and grey-white[10]

most are colourless or dull red, yellow, green, or intermediate shades[11]
C, P, Se, I: shiny and grey-white

Reflectivity

intermediate to typically high[12][13]

intermediate[14][15]

zero or low (mostly)[16] to intermediate[17]

Form

almost all solid
Rb, Cs, Fr, Ga, Hg: liquid at/near stp[18][19][n 4]

all solid[10]

most are gases[21]
C, P, S, Se, I: solid; Br: liquid

Density

generally high, with some exceptions such as the alkali metals[22]

lower than nearby metals but higher than nearby nonmetals[23]

often low

Deformability (as a solid)

most are ductile and malleable
some are brittle (Cr, Mn, Ga, Ru, W, Os, Bi)[24][n 5]

brittle[27]

brittle, when solid
some (C, P, S, Se) have non-brittle forms[n 6]

Poisson's ratio[n 7]

low to high[n 8]

low to intermediate[n 9]

low to intermediate[n 10]

Crystalline structure at freezing point[47]

most are hexagonal or cubic
Ga, U, Np: orthorhombic; In, Sn, Pa: tetragonal; Sm, Hg, Bi: rhombohedral; Pu: monoclinic

B, As, Sb: rhombohedral
Si, Ge: cubic
Te: hexagonal

H, He, C, N, Se: hexagonal
O, F, Ne, P, Ar, Kr, Xe, Rn: cubic
S, Cl, Br, I: orthorhombic

Packing & coordination number

close-packed crystal structures[48]
high coordination numbers

relatively open crystal structures[49]
medium coordination numbers[50]

open structures[51]
low coordination numbers

Atomic radius
(calculated)[52]

intermediate to very large
112–298 pm, average 187

small to intermediate: B, Si, Ge, As, Sb, Te
87–123 pm, average 115.5 pm

very small to intermediate
31–120 pm, average 76.4 pm

Allotropes[53][n 11]

around half form allotropes
one (Sn) has a metalloid-like allotrope (grey Sn, which forms below 13.2 °C[54])

all or nearly all form allotropes
some (e.g. red B, yellow As) are more nonmetallic in nature

some form allotropes
some (e.g. graphitic C, black P, grey Se) are more metalloidal or metallic in nature

Electron-related

Periodic table block

s, p, d, f[55]

p[56]

s, p[56]

Outer s and p electrons

few in number (1–3)
except 0 (Pd); 4 (Sn, Pb, Fl); 5 (Bi); 6 (Po)

medium number (3–7)

high number (4–8)
except 1 (H); 2 (He)

Electron bands: (valence, conduction)

nearly all have substantial band overlap
Bi: has slight band overlap (semimetal)

most have narrow band gap (semiconductors)
As, Sb are semimetals

most have wide band gap (insulators)
C (graphite): a semimetal
P (black), Se, I: semiconductors

Electron behaviour

"free" electrons (facilitating electrical and thermal conductivity)

valence electrons less freely delocalized; considerable covalent bonding present[57]
have Goldhammer-Herzfeld criterion[n 12] ratios straddling unity[61][62]

no, few, or directionally confined "free" electrons (generally hampering electrical and thermal conductivity)

Electrical conductivity

good to high[n 13]

intermediate[64] to good[n 14]

poor to good[n 15]

... as a liquid[70]

falls gradually as temperature rises[n 16]

most behave like metals[61][72]

increases as temperature rises

Thermodynamics

Thermal conductivity

medium to high[73]

mostly intermediate;[27][74] Si is high

almost negligible[75] to very high[76]

Temperature coefficient of resistance[n 17]

nearly all positive (Pu is negative)[77]

negative (B, Si, Ge, Te)[78] or positive (As, Sb)[79]

nearly all negative (C, as graphite, is positive in the direction of its planes)[80][81]

Melting point

very high and solid at room temperature (except mercury)

very high and solid at room temperature

mostly low and gas at room temperature

Melting behaviour

volume generally expands[82]

some contract, unlike (most)[83] metals[84]

volume generally expands[82]

Enthalpy of fusion

low to high

intermediate to very high

very low to low (except C: very high)

Elemental chemistry

Overall behaviour

metallic

nonmetallic[85]

nonmetallic

Ion formation

tend to form cations

some tendency to form anions in water[6]
solution chemistry dominated by formation and reactions of oxyanions[86][87]

tend to form anions

Bonds

seldom form covalent compounds

form salts as well as covalent compounds[88]

form many covalent compounds

Oxidation number

nearly always positive

positive or negative[89]

positive or negative

Ionization energy

relatively low

intermediate[90][91]

high

Electronegativity

usually low

close to 2,[92] i.e., 1.9–2.2[93][n 18]

high

Combined form chemistry

With metals

form alloys

can form alloys[88][96][97]

form ionic or interstitial compounds

With carbon

carbides and organometallic compounds

same as metals

carbon-nonmetal (e.g. CO2, CS2)[n 19] or organic (e.g. CH4, C6H12O6) compounds

With hydrogen (hydrides)

ionic, with alkali, alkaline earth metals
metallic, with transition metals
covalent, with post-transition metals

covalent, volatile hydrides[98]

covalent, gaseous or liquid hydrides

With oxygen (oxides)

nearly all solid (Mn2O7 is a liquid)
very few glass formers[99]
lower oxides: ionic and basic
higher oxides: more covalent, acidic

solid
glass formers (B, Si, Ge, As, Sb, Te)[100]
polymeric in structure;[101] tend to be amphoteric or weakly acidic[10][102]

solid, liquid or gaseous
few glass formers (P, S, Se)[103]
covalent, acidic

With sulfur (sulfates)

do form[n 20][n 21]

most form[n 22]

some form[n 23]

With halogens (halides, esp. chlorides) (see also[124])

typically ionic, involatile
generally insoluble in organic solvents
mostly water-soluble (not hydrolysed)
more covalent, volatile, and susceptible to hydrolysis[n 24] and organic solvents with higher halogens and weaker metals[125][126]

covalent, volatile[127]
usually dissolve in organic solvents[128]
partly or completely hydrolysed[129]
some reversibly hydrolysed[129]

covalent, volatile
usually dissolve in organic solvents
generally completely or extensively hydrolyzed
not always susceptible to hydrolysis if parent nonmetal at maximum covalency for period e.g. CF4, SF6 (then nil reaction)[130]

Environmental chemistry

Molar composition of Earth's ecosphere[n 25]

about 14%, mostly Al, Na, Ng, Ca, Fe, K

about 17%, mostly Si

about 69%, mostly O, H

Primary form on Earth

most occur in combined states, as carbonates, silicates, phosphates, oxides, sulfides, or halides
some (e.g. Au, Cu, Ag, Pt) occur in free or uncombined states[134]

all occur in combined states, as borates, silicates, sulfides, or tellurides

elemental C, N, O, S, noble gases are plentiful
H,[n 26] F[n 27], Se occur primarily in compounds
P, Cl, Br, I occur only in compounds, as phosphates, oxides, selenides or halides

Required by mammals

large amounts needed: Na, Mg, K, Ca
trace amounts needed of some others

trace amounts needed: B, Si, As

large amounts needed: H, C, N, O, P, S, Cl
trace amounts needed: Se, Br, I, possibly F
only noble gases not needed

Composition of the human body, by weight

about 1.5% Ca
traces of most others through 92U

trace amounts of B, Si, Ge, As, Sb, Te

about 97% O, C, H, N, P
others detectable except noble gases

text: Anomalous properties[edit]

text:
There were exceptions…in the periodic table, anomalies too—some of them profound. Why, for example, was manganese such a bad conductor of electricity, when the elements on either side of it were reasonably good conductors? Why was strong magnetism confined to the iron metals? And yet these exceptions, I was somehow convinced, reflected special additional mechanisms at work…
“
”

Oliver Sacks
Uncle Tungsten (2001, p. 204)

tag: div

text: Within each category, elements can be found with one or two properties very different from the expected norm, or that are otherwise notable.

text: Metals[edit]

text: Sodium, potassium, rubidium, caesium, barium, platinum, gold

text: The common notions that "alkali metal ions (group 1A) always have a +1 charge"[136] and that "transition elements do not form anions"[137] are textbook errors. The synthesis of a crystalline salt of the sodium anion Na− was reported in 1974. Since then further compounds ("alkalides") containing anions of all other alkali metals except Li and Fr, as well as that of Ba, have been prepared. In 1943, Sommer reported the preparation of the yellow transparent compound CsAu. This was subsequently shown to consist of caesium cations (Cs+) and auride anions (Au−) although it was some years before this conclusion was accepted. Several other aurides (KAu, RbAu) have since been synthesized, as well as the red transparent compound Cs2Pt which was found to contain Cs+ and Pt2− ions.[138]

text: Manganese

text: Well-behaved metals have crystal structures featuring unit cells with up to four atoms. Manganese has a complex crystal structure with a 58-atom unit cell, effectively four different atomic radii, and four different coordination numbers (10, 11, 12 and 16). It has been described as resembling "a quaternary intermetallic compound with four Mn atom types bonding as if they were different elements."[139] The half-filled 3d shell of manganese appears to be the cause of the complexity. This confers a large magnetic moment on each atom. Below 727 °C, a unit cell of 58 spatially diverse atoms represents the energetically lowest way of achieving a zero net magnetic moment.[140] The crystal structure of manganese makes it a hard and brittle metal, with low electrical and thermal conductivity. At higher temperatures "greater lattice vibrations nullify magnetic effects"[139] and manganese adopts less complex structures.[141]

text: Iron, cobalt, nickel, gadolinium, terbium, dysprosium, holmium, erbium, thulium

text: The only elements strongly attracted to magnets are iron, cobalt, and nickel at room temperature, gadolinium just below, and terbium, dysprosium, holmium, erbium, and thulium at ultra cold temperatures (below −54 °C, −185 °C, −254 °C, −254 °C, and −241 °C respectively).[142]

text: Iridium

text: The only element encountered with an oxidation state of +9 is iridium, in the [IrO4]+ cation. Other than this, the highest known oxidation state is +8, in Ru, Xe, Os, Ir, and Hs.[143]

text: Gold

text: The malleability of gold is extraordinary: a fist sized lump can be hammered and separated into one million paper back sized sheets, each 10 nm thick,[citation needed] 1600 times thinner than regular kitchen aluminium foil (0.016 mm thick).[citation needed]

text: Mercury

text:
Bricks and bowling balls will float on the surface of mercury thanks to it having a density 13.5 times that of water. Equally, a solid mercury bowling ball would weigh around 50 pounds and, if it could be kept cold enough, would float on the surface of liquid gold.[citation needed]
The only metal having an ionisation energy higher than some nonmetals (sulfur and selenium) is mercury.[citation needed]
Mercury and its compounds have a reputation for toxicity but on a scale of 1 to 10, dimethylmercury ((CH3)2Hg) (abbr. DMM), a volatile colourless liquid, has been described as a 15. It is so dangerous that scientists have been encouraged to use less toxic mercury compounds wherever possible. In 1997, Karen Wetterhahn, a professor of chemistry specialising in toxic metal exposure, died of mercury poisoning ten months after a few drops of DMM landed on her "protective" latex gloves. Although Wetterhahn had been following the then published procedures for handling this compound, it passed through her gloves and skin within seconds. It is now known that DMM is exceptionally permeable to (ordinary) gloves, skin and tissues. And its toxicity is such that less than one-tenth of a ml applied to the skin will be seriously toxic.[144]

text: Lead

text: The expression, to "go down like a lead balloon" is anchored in the common view of lead as a dense, heavy metal—being nearly as dense as mercury. However, it is possible to construct a balloon made of lead foil, filled with a helium and air mixture, which will float and be buoyant enough to carry a small load.[citation needed]

text: Bismuth

text: Bismuth has the longest half life of any naturally occurring element; its only primordial isotope, bismuth-209, was found in 2003 to be slightly radioactive, decaying via alpha decay with a half life more than a billion times the estimated age of the universe. Prior to this discovery, bismuth-209 was thought to be the heaviest naturally occurring stable isotope;[145] this distinction now belongs to lead-208.

text: Uranium

text: The only element with a naturally occurring isotope capable of undergoing nuclear fission is uranium.[146] The capacity of uranium-235 to undergo fission was first suggested (and ignored) in 1934, and subsequently discovered in 1938.[n 28]

text: Plutonium

text: It is a commonly held belief that metals reduce their electrical conductivity when heated. Plutonium increases its electrical conductivity when heated in the temperature range of around –175 to +125 °C.[citation needed]

text: Metalloids[edit]

text: Boron

text: Boron is the only element with a partially disordered structure in its most thermodynamically stable crystalline form.[149]

text: Boron, antimony

text: These elements are record holders within the field of superacid chemistry. For seven decades, fluorosulfonic acid HSO3F and trifluoromethanesulfonic acid CF3SO3H were the strongest known acids that could be isolated as single compounds. Both are about a thousand times more acidic than pure sulfuric acid. In 2004, a boron compound broke this record by a thousand fold with the synthesis of carborane acid H(CHB11Cl11). Another metalloid, antimony, features in the strongest known acid, a mixture 10 billion times stronger than carborane acid. This is fluoroantimonic acid H2F[SbF6], a mixture of antimony pentafluoride SbF5 and hydrofluoric acid HF.[citation needed]

text: Silicon

text:
The thermal conductivity of silicon is better than that of most metals.[citation needed]
A sponge-like porous form of silicon (p-Si) is typically prepared by the electrochemical etching of silicon wafers in a hydrofluoric acid solution.[150] Flakes of p-Si sometimes appear red;[151] it has a band gap of 1.97–2.1 eV.[152] The many tiny pores in porous silicon give it an enormous internal surface area, up to 1,000 m2/cm3.[153] When exposed to an oxidant,[154] especially a liquid oxidant,[153] the high surface-area to volume ratio of p-Si creates a very efficient burn, accompanied by nano-explosions,[150] and sometimes by ball-lightning-like plasmoids with, for example, a diameter of 0.1–0.8 m, a velocity of up to 0.5 m/s and a lifetime of up to 1s.[155] The first ever spectrographic analysis of a ball lightning event (in 2012) revealed the presence of silicon, iron and calcium, these elements also being present in the soil.[156]

text: Arsenic

text: Metals are said to be fusible, resulting in some confusion in old chemistry as to whether arsenic was a true metal, or a nonmetal, or something in between. It sublimes rather than melts at standard atmospheric pressure, like the nonmetals carbon and red phosphorus.[citation needed]

text: Antimony

text: A high-energy explosive form of antimony was first obtained in 1858. It is prepared by the electrolysis of any of the heavier antimony trihalides (SbCl3, SbBr3, SbI3) in a hydrochloric acid solution at low temperature. It comprises amorphous antimony with some occluded antimony trihalide (7–20% in the case of the trichloride). When scratched, struck, powdered or heated quickly to 200 °C, it "flares up, emits sparks and is converted explosively into the lower-energy, crystalline grey antimony."[157]

text: Nonmetals[edit]

text: Hydrogen

text:
Water (H2O), a well known oxide of hydrogen, is a spectacular anomaly.[158] Extrapolating from the heavier hydrogen chalcogenides, namely hydrogen sulfide H2S, hydrogen selenide H2Se, and hydrogen telluride H2Te, water should be "a foul-smelling, poisonous, inflammable gas…condensing to a nasty liquid [at] around –100° C". Instead, due to hydrogen bonding, water is "stable, potable, odorless, benign, and…indispensable to life".[159]
Less well known of the oxides of hydrogen is the trioxide, H2O3. Berthelot proposed the existence of this oxide in 1880 but his suggestion was soon forgotten as there was no way of testing it using the technology of the time.[160] Hydrogen trioxide was prepared in 1994 by replacing the oxygen used in the industrial process for making hydrogen peroxide, with ozone. The yield is about 40 per cent, at –78 °C; above around –40 °C it decomposes into water and oxygen.[161] Derivatives of hydrogen trioxide, such as F3C–O–O–O–CF3 ("bis(trifluoromethyl) trioxide") are known; these are metastable at room temperature.[162] Mendeleev went a step further, in 1895, and proposed the existence of hydrogen tetroxide HO–O–O–OH as a transient intermediate in the decomposition of hydrogen peroxide;[160] this was prepared and characterised in 1974, using a matrix isolation technique.[citation needed] Alkali metal ozonide salts of the unknown hydrogen ozonide (HO3) are also known; these have the formula MO3.[162]

text: Helium

text:
At temperatures below 0.3 and 0.8 K respectively, helium-3 and helium-4 each have a negative enthalpy of fusion. This means that, at the appropriate constant pressures, these substances freeze with the addition of heat.[citation needed]
Until 1999 helium was thought to be too small to form a cage clathrate—a compound in which a guest atom or molecule is encapsulated in a cage formed by a host molecule—at atmospheric pressure. In that year the synthesis of microgram quantities of He@C20H20 represented the first such helium clathrate and (what was described as) the world's smallest helium balloon.[163]

text: Carbon

text:
Graphite is the most electrically conductive nonmetal, better than some metals.[citation needed]
Diamond is the best natural conductor of heat; it even feels cold to the touch. Its thermal conductivity (2,200 W/m•K) is five times greater than the most conductive metal (Ag at 429); 300 times higher than the least conductive metal (Pu at 6.74); and nearly 4,000 times that of water (0.58) and 100,000 times that of air (0.0224). This high thermal conductivity is used by jewelers and gemologists to separate diamonds from imitations.[citation needed]
Graphene aerogel, produced in 2012 by freeze-drying a solution of carbon nanotubes and graphite oxide sheets and chemically removing oxygen, is seven times lighter than air, and ten per cent lighter than helium. It is the lightest solid known (0.16 mg/cm3), conductive and elastic.[164]

text: Phosphorus

text: The least stable and most reactive form of phosphorus is the white allotrope. It is a hazardous, highly flammable and toxic substance, spontaneously igniting in air and producing phosphoric acid residue. It is therefore normally stored under water. White phosphorus is also the most common, industrially important, and easily reproducible allotrope, and for these reasons is regarded as the standard state of phosphorus. The most stable form is the black allotrope, which is a metallic looking, brittle and relatively non-reactive semiconductor (unlike the white allotrope, which has a white or yellowish appearance, is pliable, highly reactive and a semiconductor). When assessing periodicity in the physical properties of the elements it needs to be borne in mind that the quoted properties of phosphorus tend to be those of its least stable form rather than, as is the case with all other elements, the most stable form.[citation needed]

text: Iodine

text: The mildest of the halogens, iodine is the active ingredient in tincture of iodine, a disinfectant. This can be found in household medicine cabinets or emergency survival kits. Tincture of iodine will rapidly dissolve gold,[165] a task ordinarily requiring the use of aqua regia (a highly corrosive mixture of nitric and hydrochloric acids).[citation needed]

text: Notes[edit]

text:
Jump up ^ For example:

Brinkley[2] writes that boron has weakly nonmetallic properties.
Glinka[3] describes silicon as a weak nonmetal.
Eby et al.[4] discuss the weak chemical behaviour of the elements close to the metal-nonmetal borderline.
Booth and Bloom[5] say "A period represents a stepwise change from elements strongly metallic to weakly metallic to weakly nonmetallic to strongly nonmetallic, and then, at the end, to an abrupt cessation of almost all chemical properties ...".
Cox[6] notes "nonmetallic elements close to the metallic borderline (Si, Ge, As, Sb, Se, Te) show less tendency to anionic behaviour and are sometimes called metalloids."

Jump up ^ See, for example, Huheey, Keiter & Keiter[7] who classify Ge and Sb as post-transition metals.
Jump up ^ At standard pressure and temperature, for the elements in their most thermodynamically stable forms, unless otherwise noted
Jump up ^ Copernicium is reported to be the only metal known to be a gas at room temperature.[20]
Jump up ^ Whether polonium is ductile or brittle is unclear. It is predicted to be ductile based on its calculated elastic constants.[25] It has a simple cubic crystalline structure. Such a structure has few slip systems and "leads to very low ductility and hence low fracture resistance".[26]
Jump up ^ Carbon as exfoliated (expanded) graphite,[28] and as metre-long carbon nanotube wire;[29] phosphorus as white phosphorus (soft as wax, pliable and can be cut with a knife, at room temperature);[30] sulfur as plastic sulfur;[31] and selenium as selenium wires.[32]
Jump up ^ For polycrystalline forms of the elements unless otherwise noted. Determining Poisson's ratio accurately is a difficult proposition and there could be considerable uncertainty in some reported values.[33]
Jump up ^ Beryllium has the lowest known value (0.0476) amongst elemental metals; indium and thallium each have the highest known value (0.46). Around one third show a value ≥ 0.33.[34]
Jump up ^ Boron 0.13;[35] silicon 0.22;[36] germanium 0.278;[37] amorphous arsenic 0.27;[38] antimony 0.25;[39] tellurium ~0.2.[40]
Jump up ^ Graphitic carbon 0.25;[41] [diamond 0.0718];[42] black phosphorus 0.30;[43] sulfur 0.287;[44] amorphous selenium 0.32;[45] amorphous iodine ~0.[46]
Jump up ^ At atmospheric pressure, for elements with known structures
Jump up ^ The Goldhammer-Herzfeld criterion is a ratio that compares the force holding an individual atom's valence electrons in place with the forces, acting on the same electrons, arising from interactions between the atoms in the solid or liquid element. When the interatomic forces are greater than or equal to the atomic force, valence electron itinerancy is indicated. Metallic behaviour is then predicted.[58] Otherwise nonmetallic behaviour is anticipated. The Goldhammer-Herzfeld criterion is based on classical arguments.[59] It nevertheless offers a relatively simple first order rationalization for the occurrence of metallic character amongst the elements.[60]
Jump up ^ Metals have electrical conductivity values of from 6.9 × 103 S•cm−1 for manganese to 6.3 × 105 for silver.[63]
Jump up ^ Metalloids have electrical conductivity values of from 1.5 × 10−6 S•cm−1 for boron to 3.9 × 104 for arsenic.[65] If selenium is included as a metalloid the applicable conductivity range would start from ~10−9 to 10−12 S•cm−1.[66][67][68]
Jump up ^ Nonmetals have electrical conductivity values of from ~10−18 S•cm−1 for the elemental gases to 3 × 104 in graphite.[69]
Jump up ^ Mott and Davis[71] note however that 'liquid europium has a negative temperature coefficient of resistance' i.e. that conductivity increases with rising temperature
Jump up ^ At or near room temperature
Jump up ^ Chedd[94] defines metalloids as having electronegativity values of 1.8 to 2.2 (Allred-Rochow scale). He included boron, silicon, germanium, arsenic, antimony, tellurium, polonium and astatine in this category. In reviewing Chedd's work, Adler[95] described this choice as arbitrary, given other elements have electronegativities in this range, including copper, silver, phosphorus, mercury and bismuth. He went on to suggest defining a metalloid simply as, 'a semiconductor or semimetal' and 'to have included the interesting materials bismuth and selenium in the book'.
Jump up ^ Phosphorus is known to form a carbide in thin films.
Jump up ^ See, for example, the sulfates of the transition metals,[104] the lanthanides[105] and the actinides.[106]
Jump up ^ Sulfates of osmium have not been characterized with any great degree of certainty.[107]
Jump up ^ Common metalloids: Boron is reported to be capable of forming an oxysulfate (BO)2SO4,[108] a bisulfate B(HSO4)3[109] and a sulfate B2(SO4)3.[110] The existence of a sulfate has been disputed.[111] In light of the existence of silicon phosphate, a silicon sulfate might also exist.[112] Germanium forms an unstable sulfate Ge(SO4)2 (d 200 °C).[113] Arsenic forms oxide sulfates As2O(SO4)2 (= As2O3.2SO3)[114] and As2(SO4)3 (= As2O3.3SO3).[115] Antimony forms a sulfate Sb2(SO4)3 and an oxysulfate (SbO)2SO4.[116] Tellurium forms an oxide sulfate Te2O3(SO)4.[117] Less common: Polonium forms a sulfate Po(SO4)2.[118] It has been suggested that the astatine cation forms a weak complex with sulfate ions in acidic solutions.[119]
Jump up ^ Hydrogen forms hydrogen sulfate H2SO4. Carbon forms (a blue) graphite hydrogen sulfate C+
24HSO–
4 • 2.4H2SO4.[120] Nitrogen forms nitrosyl hydrogen sulfate (NO)HSO4 and nitronium (or nitryl) hydrogen sulfate (NO2)HSO4.[121] There are indications of a basic sulfate of selenium SeO2.SO3 or SeO(SO4).[122] Iodine forms a polymeric yellow sulfate (IO)2SO4.[123]
Jump up ^ layer-lattice types often reversibly so
Jump up ^ Based on a table of the elemental composition of the biosphere, and lithosphere (crust, atmosphere, and seawater) in Georgievskii,[131] and the masses of the crust and hydrosphere give in Lide and Frederikse.[132] The mass of the biosphere is negligible, having a mass of about one billionth that of the lithosphere.[citation needed] "The oceans constitute about 98 percent of the hydrosphere, and thus the average composition of the hydrosphere is, for all practical purposes, that of seawater."[133]
Jump up ^ Hydrogen gas is produced by some bacteria and algae and is a natural component of flatus. It can be found in the Earth's atmosphere at a concentration of 1 part per million by volume.
Jump up ^ Fluorine can be found in its elemental form, as an occlusion in the mineral antozonite[135]
Jump up ^ In 1934, a team led by Enrico Fermi postulated that transuranic elements may have been produced as a result of bombarding uranium with neutrons, a finding which was widely accepted for a few years. In the same year Ida Noddack, a German scientist and subsequently a three-time Nobel prize nominee, criticised this assumption, writing "It is conceivable that the nucleus breaks up into several large fragments, which would of course be isotopes of known elements but would not be neighbors of the irradiated element."[147][emphasis added] In this, Noddak defied the understanding of the time without offering experimental proof or theoretical basis, but nevertheless presaged what would be known a few years later as nuclear fission. Her paper was generally ignored as, in 1925, she and two colleagues claimed to have discovered element 43, then proposed to be called masurium (later discovered in 1936 by Perrier and Segrè, and named technetium). Had Ida Noddack's paper been accepted it is likely that Germany would have had an atomic bomb and, 'the history of the world would have been [very] different.'[148]


document_title: The Greatest Story Ever Told

question_text: who played the role of jesus in the greatest story ever told

text: The Greatest Story Ever Told

text: Cast[edit]

text: The major roles in the movie were following:

text:
Max von Sydow as Jesus
Dorothy McGuire as the Virgin Mary
Charlton Heston as John the Baptist
Claude Rains as Herod the Great
José Ferrer as Herod Antipas
Telly Savalas as Pontius Pilate
Martin Landau as Caiaphas
David McCallum as Judas Iscariot
Donald Pleasence as "The Dark Hermit" (a personification of Satan)
Michael Anderson, Jr. as James the Just
Roddy McDowall as Matthew
Joanna Dunham as Mary Magdalene
Joseph Schildkraut as Nicodemus
Ed Wynn as "Old Aram"

text: Smaller roles (some only a few seconds) were played by Michael Ansara, Ina Balin, Carroll Baker, Robert Blake, Pat Boone, Victor Buono, John Considine, Richard Conte, John Crawford, Jamie Farr, David Hedison, Van Heflin, Russell Johnson, Angela Lansbury, Mark Lenard, Robert Loggia, John Lupton, Janet Margolin, Sal Mineo, Nehemiah Persoff, Sidney Poitier, Gary Raymond, Marian Seldes, David Sheiner, Abraham Sofaer, Paul Stewart, John Wayne, Shelley Winters, and Peter Mann.

text: As of March 2018[update], Max von Sydow, David McCallum, Angela Lansbury, Sidney Poitier, Gary Raymond, John Considine, David Hedison, Pat Boone, Jamie Farr, Robert Blake, David Sheiner, and Michael Anderson Jr. are the only surviving main cast members.

text: Pre-production[edit]

text: The Greatest Story Ever Told originated as a U.S. radio series in 1947, half-hour episodes inspired by the Gospels. The series was adapted into a 1949 novel by Fulton Oursler, a senior editor at Reader's Digest.[2] Darryl F. Zanuck, the head of 20th Century Fox, acquired the film rights to the Oursler novel shortly after publication,[3] but never brought it to pre-production.[4]

text: In 1958, when George Stevens was producing and directing The Diary of Anne Frank at 20th Century Fox, he became aware that the studio owned the rights to the Oursler property. Stevens created a company, "The Greatest Story Productions", to film the novel.[4]

text: The screenplay took two years to write. Stevens collaborated with Ivan Moffat and then with James Lee Barrett. It was the only time Stevens received screenplay credit for a film he directed.[4] Ray Bradbury and Reginald Rose were considered but neither participated. The poet Carl Sandburg was solicited, though it is not certain if any of his contributions were included. Sandburg, however, did receive screen credit for "creative association."[4][5]

text: Financial excesses began to grow during pre-production. Stevens commissioned French artist André Girard to prepare 352 oil paintings of Biblical scenes to use as storyboards. Stevens also traveled to the Vatican to see Pope John XXIII for advice.[2]

text: In August 1961, 20th Century Fox withdrew from the project, noting that $2.3 million had been spent without any footage being shot. Stevens was given two years to find another studio or 20th Century Fox would reclaim its rights. Stevens moved the film to United Artists.[2]

text: Meanwhile, MGM proceeded with their own 1961 Technicolor epic about the life of Christ, King of Kings, starring Jeffrey Hunter as Jesus, which was filmed in Spain, and when released was nearly an hour shorter than The Greatest Story Ever Told.

text: Casting[edit]

text: For The Greatest Story Ever Told, Stevens cast Swedish actor Max von Sydow as Jesus. Von Sydow had never appeared in an English-language film and was best known for his performances in Ingmar Bergman's dramatic films.[6] Stevens wanted an actor unknown to international audiences, free of secular and unseemly associations in the mind of the public.[7]

text: The Greatest Story Ever Told featured an ensemble of well-known actors, many of them in brief, even cameo, appearances. Some critics would later complain that the large cast distracted from the solemnity, notably in the appearance of John Wayne as the Roman centurion who comments on the Crucifixion, in his well-known voice, by stating: "Truly this man was the Son of God."[8][9]

text: Production[edit]

text: Stevens shot The Greatest Story Ever Told in the U.S. southwest, in Arizona, California, Nevada and Utah. Pyramid Lake in Nevada represented the Sea of Galilee, Lake Moab in Utah[10] was used to film the Sermon on the Mount, and California's Death Valley was the setting of Jesus' 40-day journey into the wilderness.[2][11] Parts of the film were also shot at Lake Powell, Canyonlands and Dead Horse Point in Utah.[12]

text: Stevens explained his decision to use the U.S. rather than in the Middle East or Europe in 1962. "I wanted to get an effect of grandeur as a background to Christ, and none of the Holy Land areas shape up with the excitement of the American southwest," he said. "I know that Colorado is not the Jordan, nor is Southern Utah Palestine. But our intention is to romanticize the area, and it can be done better here."[2]

text: Forty-seven sets were constructed, on location and in Hollywood studios, to accommodate Stevens' vision.[13] The Jerusalem city set was built near the northwest corner of RKO Forty Acres by early 1963, and was demolished soon after filming was completed that summer.[14]

text: To fill location scenes with extras, Stevens turned to local sources – R.O.T.C. cadets from an Arizona high school played Roman soldiers (after 550 Navajo Indians from a nearby reservation allegedly did not give a convincing performance; other sources claim they weren't on set long enough and left early to take part in a tribal election[15])[16] and Arizona Department of Welfare provided disabled state aid recipients to play the afflicted who sought Jesus' healing.[2]

text: Principal photography was scheduled to run three months but ran nine months or more[17] due to numerous delays and setbacks (most of which were due to Stevens' insistence on shooting dozens of retakes in every scene).[18] Joseph Schildkraut died before completing his performance as Nicodemus, requiring scenes to be rewritten around his absence. Cinematographer William C. Mellor had a fatal heart attack during production; Loyal Griggs, who won an Academy Award for his cinematography on Stevens’ 1953 Western classic Shane, was brought in to replace him. Joanna Dunham became pregnant, which required costume redesigns and carefully chosen camera angles.[2]

text: Much of the production was shot during the winter of 1962-1963, when Arizona had heavy snow. Actor David Sheiner, who played James the Elder, quipped in an interview about the snowdrifts: "I thought we were shooting Nanook of the North."[19] Stevens was also under pressure to hurry the John the Baptist sequence, which was shot at the Glen Canyon area – it was scheduled to become Lake Powell with the completion of the Glen Canyon Dam, and the production held up the project.[2]

text: Stevens brought in two veteran filmmakers. Jean Negulesco filmed sequences in the Jerusalem streets and the Nativity scenes, while David Lean shot the prologue featuring Herod the Great.[4] Lean cast Claude Rains as Herod.[20]

text: By the time shooting was completed in August 1963, Stevens had amassed six million feet of Ultra Panavision 70 film (about 1829 km or 1136 miles, roughly the radius of the Moon). The budget ran to $20 million (equivalent to $142 million in 2010) plus additional editing and promotion charges,[21] making it the most expensive film shot in the U.S.[4][22]

text: The film was advertised on its first run as being shown in Cinerama. While it was shown on an ultra-curved screen, it was with one projector. True Cinerama required three projectors running simultaneously. A dozen other films were presented this way in the 1960s.

text: Release and reception[edit]

text: The Greatest Story Ever Told premiered 15 February 1965, 18 months after filming wrapped, at the Warner Cinerama Theatre in New York City. Critical reaction toward the movie was divided once it premiered. In its favor, Variety called the film "a big, powerful moving picture demonstrating vast cinematic resource." The Hollywood Reporter stated: "George Stevens has created a novel, reverent and important film with his view of this crucial event in the history of mankind."[4]

text: However, Bosley Crowther in The New York Times wrote: "The most distracting nonsense is the pop-up of familiar faces in so-called cameo roles, jarring the illusion." Shana Alexander in Life Magazine stated: "The pace was so stupefying that I felt not uplifted – but sandbagged!"[4] And John Simon – later notorious as the frequently scathing theater and film critic of New York Magazine – wrote: "God is unlucky in The Greatest Story Ever Told. His only begotten son turns out to be a bore."[23] Bruce Williamson, in Playboy Magazine, likewise called the movie "a big windy bore."[24]

text: Brendan Gill wrote in The New Yorker:

text: Stevens told a New York Times interviewer: "I have tremendous satisfaction that the job has been done – to its completion – the way I wanted it done; the way I know it should have been done. It belongs to the audiences now…and I prefer to let them judge."[4] Reviews to the film continue to be mixed, as it currently holds a 37% rating on Rotten Tomatoes based on 19 reviews.[25]

text: The original running time was 4 hr 20 min (260 min).[23] The time was revised three times, to 3 hr 58 min (238 min); to 3 hr 17 min (197 min) for the United Kingdom, and finally 2 hr 17 min (137 min) for general U.S. release.[2] Commercially, the film was not successful (by 1983 it had grossed less than $8 million, perhaps 17 percent of the amount required to break even),[21] and its inability to connect with audiences discouraged production of biblical epics for years.[26]

text: For the 2001 DVD release, a 3 hr 19 min (199 min) version was presented along with a documentary called He Walks With Beauty, which detailed the film’s tumultuous production history. Its Blu-ray release appeared in 2011.[13]

text: Despite the mixed critical reception and low box office receipts, The Greatest Story Ever Told was nominated for five Academy Awards:[27]

text:
Awards

Award
Date of ceremony
Category
Recipient
Outcome

Academy Awards[28]
April 18, 1966
Best Cinematography, Color
William C. Mellor (posthumous nomination) and Loyal Griggs
Nominated

Best Art Direction – Set Decoration, Color
Art Direction: Richard Day, William J. Creber, and David S. Hall (posthumous nomination)
Set Decoration: Ray Moyer, Fred M. MacLean, and Norman Rockett

Best Costume Design, Color
Marjorie Best and Vittorio Nino Novarese

Best Effects, Special Visual Effects
J. McMillan Johnson

Best Music, Score – Substantially Original
Alfred Newman

text: The film is recognized by American Film Institute in these lists:

text:
2005: AFI's 100 Years of Film Scores – Nominated[29]
2006: AFI's 100 Years...100 Cheers – Nominated[30]
2008: AFI's 10 Top 10:

Nominated Epic Film[31]