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Properties of substance:

iron

Group of substances:

inorganic

Physical appearance:

cubic metal

Empirical formula (Hill's system for organic substances):

Fe

Structural formula as text:

Fe

Molar/atomic mass: 55.85

Melting point (°C):

1539

Boiling point (°C):

2870

Solubility (g/100 g of solvent):

diethyl ether: insoluble [Ref.]
ethanol: insoluble [Ref.]
lithium molten: 0.002 (700°C) [Ref.]
magnesium fused: 0.05 (700°C) [Ref.]
magnesium fused: 0.265 (1000°C) [Ref.]
mercury: 0.0000015 (25°C) [Ref.]
mercury: 0.0000019 (100°C) [Ref.]
mercury: 0.0000054 (300°C) [Ref.]
potassium fused: 0.0045 (700°C) [Ref.]
sodium fused: 0.00135 (500°C) [Ref.]
sodium fused: 0.0005 (700°C) [Ref.]
tin liquid: 0.0047 (270°C) [Ref.]
tin liquid: 0.0073 (329°C) [Ref.]
tin liquid: 0.07 (483°C) [Ref.]
tin liquid: 1.26 (773°C) [Ref.]
tin liquid: 12.49 (1125°C) [Ref.]
water: insoluble [Ref.]

Numerical data:

Hardness on the Mohs’ scale: 4-5

Density:

7.874 (20°C, g/cm3)
6.9 (1589°C, d4)

Reactions of synthesis:

  1. [Ref.1aster, Ref.2, Ref.3aster, Ref.4aster, Ref.5aster]
    Fe2O3 + 3H2 → 2Fe + 3H2O
  2. [Ref.1]
    Fe2O3 + 3C → 2Fe + 3CO

Reactions:

  1. [Ref.1, Ref.2]
    Fe + H2O → FeO + H2
  2. [Ref.1]
    Fe + Cl2 → FeCl2
    2FeCl2 + Cl2 → 2FeCl3
  3. [Ref.1]
    4Fe + 6H2O + 3O2 → 4Fe(OH)3
  4. [Ref.1]
    Fe + I2 + 4H2O → FeI2 * 4H2O
  5. [Ref.1]
    Fe + 2HSCN + 3H2O → Fe(SCN)2 * 3H2O + H2
  6. [Ref.1]
    Fe + 2HClO4 + 6H2O → Fe(ClO4)2 * 6H2O + H2
  7. [Ref.1, Ref.2]
    Fe + H2SO4 + 7H2O → FeSO4 * 7H2O + H2
  8. [Ref.1, Ref.2, Ref.3, Ref.4]
    Fe + 4HNO3 + 7H2O → Fe(NO3)3 * 9H2O + NO
  9. [Ref.1]
    Fe + 5CO → Fe(CO)5
  10. [Ref.1]
    Fe + CuSO4 → Cu + FeSO4

Half-life:

4526Fe = 2.2 ms (2p (57%), β+ (< 43%))
4626Fe = 13.0 ms (β+ (100%), β+n (78.7%))
4726Fe = 21.9 ms (β+ (100%), β+n (88.4%))
4826Fe = 45.3 ms (β+ (100%), β+n (15.9%))
4926Fe = 64.7 ms (β+ (100%), β+n (56.7%))
5026Fe = 155 ms (β+ (100%))
5126Fe = 305 ms (β+ (100%))
5226Fe = 8.275 h (β+ (100%))
52m26Fe = 45.9 s (β+ (about 100%), internal transition (0.021%))
5326Fe = 8.51 min (β+ (100%))
53m26Fe = 2.54 min (internal transition (100%))
5426Fe = stable ( (isotopic abundance 5,845%))
54m26Fe = 364 ns (internal transition (100%))
5526Fe = 2.744 y (electron capture (100%))
5626Fe = stable ( (isotopic abundance 91,754%))
5726Fe = stable ( (isotopic abundance 2,119%))
5826Fe = stable ( (isotopic abundance 0,282%))
5926Fe = 44.495 d (β- (100%))
6026Fe = 2 620 000 y (β- (100%))
6126Fe = 5.98 min (β- (100%))
61m26Fe = 241.2 ns (internal transition (100%))
6226Fe = 68 s (β- (100%))
6326Fe = 6.1 s (β- (100%))
6426Fe = 2.0 s (β- (100%))
6526Fe = 810 ms (β- (100%))
65m26Fe = 420 ns (internal transition (100%))
65n26Fe = 1.12 s ()
6626Fe = 351 ms (β- (100%))
6726Fe = 394 ms (β- (100%))
67m26Fe = 64 μs (internal transition (100%))
67n26Fe = 75 μs ()
6826Fe = 188 ms (β- (100%))
6926Fe = 110 ms (β- (100%))
7026Fe = 77 ms (β- (100%))
7126Fe = 28 ms (β- (100%), β-n)

Vapour pressure (Torr):

0.000000001 (799°C)
0.00000001 (858°C)
0.0000001 (924°C)
0.000001 (998°C)
0.00001 (1083°C)
0.0001 (1180°C)
0.001 (1293°C)
0.01 (1425°C)
0.1 (1586°C)
1 (1790°C)
10 (2045°C)
100 (2376°C)

Electrode potential:

Fe2+ + 2e- → Fe, E = -0.44 V (water, 25°C)

Standard molar enthalpy (heat) of formation ΔfH0 (298.15 K, kJ/mol):

0 (s)

Standard molar Gibbs energy of formation ΔfG0 (298.15 K, kJ/mol):

0 (s)

Standard molar entropy S0 (298.15 K, J/(mol·K)):

27.15 (s)

Molar heat capacity at constant pressure Cp (298.15 K, J/(mol·K)):

25 (s)

Molar enthalpy (heat) of fusion ΔfusH (kJ/mol):

13.8

Enthalpy (heat) of vaporization ΔvapH (kJ/mol):

350

LD50 (mg/kg):

98600 (rats, oral)

References:

  1. Авцын А.П., Жаворонков А.А., Риш М.А., Строчкова Л.С. Микроэлементозы человека. - М.: Медицина, 1991. - pp. 92-116 [Russian]
  2. Гринвуд Н., Эрншо А. Химия элементов. - Т.2. - М.: БИНОМ. Лаборатория знаний, 2008. - pp. 400-409 [Russian]
  3. Гурвич Я.А. Справочник молодого аппаратчика-химика. - М.: Химия, 1991. - pp. 50 [Russian]
  4. Иванова М.А., Кононова М.А. Химический демонстрационный эксперимент. - М.: Высшая школа, 1969. - pp. 30 [Russian]
  5. Некрасов Б.В. Основы общей химии. - Т.2. - М.: Химия, 1973. - pp. 325-334, 342 [Russian]
  6. Рабинович В.А., Хавин З.Я. Краткий химический справочник. - Л.: Химия, 1977. - pp. 62 [Russian]
  7. Реми Г. Курс неорганической химии. - Т.2. - М., 1966. - pp. 280-288 [Russian]
  8. Справочник по растворимости. - Т.1, Кн.1. - М.-Л.: ИАН СССР, 1961. - pp. 637 [Russian]
  9. Химическая энциклопедия. - Т. 2. - М.: Советская энциклопедия, 1990. - pp. 139-141 [Russian]

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    © Collected Ruslan Anatolievich Kiper, burewestnik@mail.ru