Difference between revisions of "Lithium"

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|EA-ref = <ref>{{citation | last1 = Hotop | first1 = H. | last2 = Lineberger | first2 = W. C. | title = Binding energies in atomic negative ions. II | journal = J. Phys. Chem. Ref. Data | year = 1985 | volume = 14 | issue = 3 | pages = 731–50 | doi = 10.1063/1.555735}}.</ref><ref>{{citation | last1 = Dellwo | first1 = J. | last2 = Liu | first2 = Y. | last3 = Pegg | first3 = D. J. | last4 = Alton | first4 = G. D. | title = Near-Threshold Photodetachment of the Li<sup>−</sup> Ion | journal = Phys. Rev. A | year = 1992 | volume = 45 | issue = 3 | pages = 1544–47 | doi = 10.1103/PhysRevA.45.1544}}.</ref><ref>{{citation | last1 = Haeffler | first1 = G. | last2 = Hanstorp | first2 = G. | last3 = Kiyan | first3 = I. | last4 = Klinkmüller | first4 = A. E. | last5 = Ljungblad | first5 = U. | last6 = Pegg | first6 = D. J. | title = Electron affinity of Li: A state-selective measurement | journal = Phys. Rev. A | year = 1996 | volume = 53 | issue = 6 | pages = 4127–31 | doi = 10.1103/PhysRevA.53.4127}}.</ref>
 
|EA-ref = <ref>{{citation | last1 = Hotop | first1 = H. | last2 = Lineberger | first2 = W. C. | title = Binding energies in atomic negative ions. II | journal = J. Phys. Chem. Ref. Data | year = 1985 | volume = 14 | issue = 3 | pages = 731–50 | doi = 10.1063/1.555735}}.</ref><ref>{{citation | last1 = Dellwo | first1 = J. | last2 = Liu | first2 = Y. | last3 = Pegg | first3 = D. J. | last4 = Alton | first4 = G. D. | title = Near-Threshold Photodetachment of the Li<sup>−</sup> Ion | journal = Phys. Rev. A | year = 1992 | volume = 45 | issue = 3 | pages = 1544–47 | doi = 10.1103/PhysRevA.45.1544}}.</ref><ref>{{citation | last1 = Haeffler | first1 = G. | last2 = Hanstorp | first2 = G. | last3 = Kiyan | first3 = I. | last4 = Klinkmüller | first4 = A. E. | last5 = Ljungblad | first5 = U. | last6 = Pegg | first6 = D. J. | title = Electron affinity of Li: A state-selective measurement | journal = Phys. Rev. A | year = 1996 | volume = 53 | issue = 6 | pages = 4127–31 | doi = 10.1103/PhysRevA.53.4127}}.</ref>
 
|EA1 = 0.618 050(74) eV<br/>59.6328(72)  kJ mol<sup>−1</sup>
 
|EA1 = 0.618 050(74) eV<br/>59.6328(72)  kJ mol<sup>−1</sup>
−
|thermo-ref = <ref name="NIST"/><ref>{{CODATA thermo}}.</ref>
+
|thermo-ref = <ref name="NIST"/><ref name="G&E"/><ref>{{CODATA thermo}}.</ref>
 
|entropy = 29.12(20) J K<sup>−1</sup> mol<sup>−1</sup>
 
|entropy = 29.12(20) J K<sup>−1</sup> mol<sup>−1</sup>
 
|enthalpy-atomization = 159.3(10) kJ mol<sup>−1</sup>
 
|enthalpy-atomization = 159.3(10) kJ mol<sup>−1</sup>
−
|entropy-atomization = 138.782(10) J K<sup>−1</sup> mol<sup>−1</sup>
+
|entropy-atomization = 109.66(20) J K<sup>−1</sup> mol<sup>−1</sup>
 
|enthalpy-fusion = 2.38 kJ mol<sup>−1</sup>
 
|enthalpy-fusion = 2.38 kJ mol<sup>−1</sup>
−
|radius-ref = &#32;<ref>{{Cordero et al. (2008)}}.</ref><ref>{{Shannon (1976)}}.</ref><ref>{{Bondi (1964)}}.</ref>
+
|enthalpy-vaporization = 148 kJ mol<sup>−1</sup>
 +
|radius-ref = <ref name="G&E"/><ref>{{Cordero et al. (2008)}}.</ref><ref>{{Shannon (1976)}}.</ref><ref>{{Bondi (1964)}}.</ref>
 +
|metallic-radius = 152 pm
 
|covalent-radius = 128 pm
 
|covalent-radius = 128 pm
 
|vdw-radius = 182 pm
 
|vdw-radius = 182 pm
Line 47: Line 49:
  
 
===References===
 
===References===
−
{{reflist|2}}
+
{{reflist}}
  
 
==External links==
 
==External links==

Latest revision as of 10:07, 27 December 2010

helium ← lithium → beryllium
H
↑
Li
↓
Na
Atomic properties
Atomic number 3
Standard atomic weight 6.941(2)[note 1]
Electron configuration 1s2 2s1
Physical properties[1][2]
Melting point 179 °C (452 K)
Boiling point 1317 °C (1590 K)
Density 0.534 g cm−3 (20 °C)
Chemical properties[3]
Electronegativity 0.98 (Pauling)
Solubility in water reacts violently
Ionization energies[4]
1st 5.391 718 96(64) eV
517.658 593(60) kJ mol−1
2nd 75.638 eV
7298.0 kJ mol−1
3rd 122.451 eV
11 814.7 kJ mol−1
Total 203.481 eV
19 632.9 kJ mol−1
Electron affinity[5][6][7]
0.618 050(74) eV
59.6328(72) kJ mol−1
Atomic radii[2][8][9][10]
Covalent radius 128 pm
Metallic radius 152 pm
Ionic radius 73.0 pm (Li+, Td)
Van der Waals radius 182 pm
Thermodynamic properties[1][2][11]
Standard entropy 29.12(20) J K−1 mol−1
Enthalpy change of atomization 159.3(10) kJ mol−1
Entropy change of atomization 109.66(20) J K−1 mol−1
Enthalpy change of fusion 2.38 kJ mol−1
Enthalpy change of vaporization 148 kJ mol−1
Hazards[12]
GHS pictograms Water-react. 1Skin Corr. 1B
GHS signal word DANGER
GHS hazard statements H260, H314 [note 2]
Miscellaneous
CAS number 7439-93-2
EC number 231-102-5
Where appropriate, and unless otherwise stated, data are given for 100 kPa (1 bar) and 298.15 K (25 °C).
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Lithium (symbol: Li) is a chemical element, the lightest of the alkali metals.

Notes and references

Notes

  1. ↑ Commercially available lithium materials have atomic weights that range between 6.939 and 6.996; if a more accurate value is required, it must be determined for the specific material.
  2. ↑ Within the European Union, the following additional hazard statement (EUH014) must also be displayed on labelling: Reacts violently with water.

References

  1. ↑ 1.0 1.1 Lithium. In NIST Chemistry WebBook; National Institute for Standards and Technology, <http://webbook.nist.gov/cgi/inchi/InChI%3D1S/Li>. (accessed 20 June 2010).
  2. ↑ 2.0 2.1 2.2 Greenwood, Norman N.; Earnshaw, A. Chemistry of the Elements; Pergamon: Oxford, 1984; pp 75–116. ISBN 0-08-022057-6.
  3. ↑ Allred, A. L. Electronegativity values from thermochemical data. J. Inorg. Nucl. Chem. 1961, 17 (3–4), 215–21. DOI: 10.1016/0022-1902(61)80142-5.
  4. ↑ Moore, Charlotte E. Ionization potentials and ionization limits derived from the analyses of optical spectra. Natl. Stand. Ref. Data Ser., (U.S. Natl. Bur. Stand.) 1970, 34, 1–22, <http://www.nist.gov/data/nsrds/NSRDS-NBS34.pdf>.
  5. ↑ Hotop, H.; Lineberger, W. C. Binding energies in atomic negative ions. II. J. Phys. Chem. Ref. Data 1985, 14 (3), 731–50. DOI: 10.1063/1.555735.
  6. ↑ Dellwo, J.; Liu, Y.; Pegg, D. J.; Alton, G. D. Near-Threshold Photodetachment of the Li− Ion. Phys. Rev. A 1992, 45 (3), 1544–47. DOI: 10.1103/PhysRevA.45.1544.
  7. ↑ Haeffler, G.; Hanstorp, G.; Kiyan, I.; Klinkmüller, A. E.; Ljungblad, U.; Pegg, D. J. Electron affinity of Li: A state-selective measurement. Phys. Rev. A 1996, 53 (6), 4127–31. DOI: 10.1103/PhysRevA.53.4127.
  8. ↑ Cordero, Beatriz; Gómez, Verónica; Platero-Prats, Ana E.; Revés, Marc; Echeverría, Jorge; Cremades, Eduard; Barragán, Flavia; Alvarez, Santiago Covalent radii revisited. Dalton Trans. 2008 (5), 2832–38. DOI: 10.1039/b801115j.
  9. ↑ Shannon, R. D. Revised effective ionic radii and systematic studies of interatomic distances in halids and chalcogenides. Acta Crystallogr. A 1976, 32 (5), 751–67. DOI: 10.1107/S0567739476001551.
  10. ↑ Bondi, A. van der Waals Volumes and Radii. J. Phys. Chem. 1964, 68 (3), 441–51. DOI: 10.1021/j100785a001.
  11. ↑ Cox, J. D.; Wagman, D. D.; Medvedev, V. A. CODATA Key Values for Thermodynamics; Hemisphere: New York, 1989. ISBN 0891167587, <http://www.codata.org/resources/databases/key1.html>.
  12. ↑ Index no. 003-001-00-4 of Annex VI, Part 3, to Regulation (EC) No 1272/2008 of the European Parliament and of the Council of 16 December 2008 on classification, labelling and packaging of substances and mixtures, amending and repealing Directives 67/548/EEC and 1999/45/EC, and amending Regulation (EC) No 1907/2006. OJEU L353, 31.12.2008, pp 1–1355 at p 340.

External links

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