Electron affinity (data page): Difference between revisions
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|[[Deuterium]]||data-sort-value="0.75467"|0.754 67(4)||data-sort-value="72.814"|72.814(4)||<ref name=BeyerD/> |
|[[Deuterium]]||data-sort-value="0.75467"|0.754 67(4)||data-sort-value="72.814"|72.814(4)||<ref name=BeyerD/> |
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|2||He||[[Helium]]||data-sort-value="-0.5"|−0.5(2) ||data-sort-value="-48"|−48(20) || |
|2||He||[[Helium]]||data-sort-value="-0.5"|−0.5(2) ||data-sort-value="-48"|−48(20) ||est.<ref name=Bratsch /> |
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|3||Li||[[Lithium]]||data-sort-value="0.61804922"|0.618 049(22)||data-sort-value="59.632"|59.632 6(21)||<ref name=HaefflerLi /> |
|3||Li||[[Lithium]]||data-sort-value="0.61804922"|0.618 049(22)||data-sort-value="59.632"|59.632 6(21)||<ref name=HaefflerLi /> |
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|54||Xe||[[Xenon]]||data-sort-value="-0.8"|−0.8(2)||data-sort-value="-77"|−77(20)||est.<ref name=Bratsch /> |
|54||Xe||[[Xenon]]||data-sort-value="-0.8"|−0.8(2)||data-sort-value="-77"|−77(20)||est.<ref name=Bratsch /> |
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|55||Cs||[[Caesium]]||data-sort-value="0.4715983"|0.4715983(38)||data-sort-value="45.5023"|45.5023(4)||<ref>{{cite journal | last=Navarro Navarrete | first=José E. | last2=Nichols | first2=Miranda | last3=Ringvall-Moberg | first3=Annie | last4=Welander | first4=Jakob | last5=Lu | first5=Di | last6=Leimbach | first6=David | last7=Kristiansson | first7=Moa K. | last8=Eklund | first8=Gustav | last9=Raveesh | first9=Meena | last10=Chulkov | first10=Ruslan | last11=Zhaunerchyk | first11=Vitali | last12=Hanstorp | first12=Dag | title=High-resolution measurement of the electron affinity of cesium | journal=Physical Review A | volume=109 | issue=2 | date=2024-02-21 | issn=2469-9926 | doi=10.1103/PhysRevA.109.022812| doi-access=free }}</ref> |
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|56||Ba||[[Barium]]||data-sort-value="0.14462"|0.144 62(6)||data-sort-value="13.954"|13.954(6)||<ref name=PetruninBa /> |
|56||Ba||[[Barium]]||data-sort-value="0.14462"|0.144 62(6)||data-sort-value="13.954"|13.954(6)||<ref name=PetruninBa /> |
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== Molecules == |
== Molecules == |
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The electron affinities ''E''<sub>ea</sub> of some |
The electron affinities ''E''<sub>ea</sub> of some molecules are given in the table below, from the lightest to the heaviest. Many more have been listed by {{harvp|Rienstra-Kiracofe|Tschumper|Schaefer|Nandi|2002}}. The electron affinities of the [[radical (chemistry)|radicals]] OH and SH are the most precisely known of all molecular electron affinities. |
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|I<sub>2</sub>||[[Iodine|Diiodine]]||2.524(5)||243.5(5)||{{harvp|Zanni|Taylor|Greenblatt|Soep|1997}} |
|I<sub>2</sub>||[[Iodine|Diiodine]]||2.524(5)||243.5(5)||{{harvp|Zanni|Taylor|Greenblatt|Soep|1997}} |
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|IBr||[[Iodine |
|IBr||[[Iodine monobromide]]||2.512(3)||242.4(4)||{{harvp|Sheps|Miller|Lineberger|2009}} |
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|LiCl||[[Lithium chloride]]||0.593(10)||57.2(10)||{{harvp|Miller|Leopold|Murray|Lineberger|1986}} |
|LiCl||[[Lithium chloride]]||0.593(10)||57.2(10)||{{harvp|Miller|Leopold|Murray|Lineberger|1986}} |
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|FeO||[[Iron(II) oxide]]||1.4950(5)||144.25(6)||{{harvp|Kim|Weichman|Neumark|2015}} |
|FeO||[[Iron(II) oxide]]||1.4950(5)||144.25(6)||{{harvp|Kim|Weichman|Neumark|2015}} |
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|CN||[[Cyano radical]]||3.862(4)|| ||<ref>{{cite journal | last=Bradforth | first=Stephen E. | last2=Kim | first2=Eun Ha | last3=Arnold | first3=Don W. | last4=Neumark | first4=Daniel M. | title=Photoelectron spectroscopy of CN−, NCO−, and NCS− | journal=The Journal of Chemical Physics | publisher=AIP Publishing | volume=98 | issue=2 | date=1993-01-15 | issn=0021-9606 | doi=10.1063/1.464244 | pages=800–810}}</ref> |
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| colspan=5 align=center |''Triatomics'' |
| colspan=5 align=center |''Triatomics'' |
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!Z!![[Chemical element|Element]]!!Name!!Electron affinity ([[electronvolt|eV]])!!Electron affinity ( |
!Z!![[Chemical element|Element]]!!Name!!Electron affinity ([[electronvolt|eV]])!!Electron affinity (kJ/mol)!![[#References|References]] |
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|7||N<sup>−</sup>||Nitrogen||data-sort-value="-6.98"| |
|7||N<sup>−</sup>||Nitrogen||data-sort-value="-6.98"|-6.98||data-sort-value="-0.0000048"|-673||<ref name="Rayner-Canham"> |
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Rayner-Canham Appendix 5: Data summarised from J. E. Huheey et al., Inorganic Chemistry, 4th ed. (New York: |
Rayner-Canham Appendix 5: Data summarised from, and see also, J. E. Huheey et al., Inorganic Chemistry, 4th ed. (New York: |
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HarperCollins, 1993) [https://bcs.whfreeman.com/WebPub/Chemistry/raynercanham6e/Appendices/Rayner-Canham%205e%20Appendix%205%20-%20Electron%20Affi%20nities%20of%20Selected%20Nonmetals.pdf]</ref> |
HarperCollins, 1993) [https://bcs.whfreeman.com/WebPub/Chemistry/raynercanham6e/Appendices/Rayner-Canham%205e%20Appendix%205%20-%20Electron%20Affi%20nities%20of%20Selected%20Nonmetals.pdf]</ref> |
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|7||N<sup>2−</sup>||Nitrogen||data-sort-value="-11.09"| |
|7||N<sup>2−</sup>||Nitrogen||data-sort-value="-11.09"|-11.09||data-sort-value="-0.0000076"|-1070||<ref name=Rayner-Canham/> |
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|8||O<sup>−</sup>||Oxygen||data-sort-value="7.71"| |
|8||O<sup>−</sup>||Oxygen||data-sort-value="-7.71"|-7.71||data-sort-value="-0.0000053"|-744||<ref name=Rayner-Canham/> |
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|15||P<sup>−</sup>||Phosphorus||data-sort-value="-4.85"| |
|15||P<sup>−</sup>||Phosphorus||data-sort-value="-4.85"|-4.85||data-sort-value="-0.0000033"|-468||<ref name=Rayner-Canham/> |
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|15||P<sup>2−</sup>||Phosphorus||data-sort-value="-9.18"| |
|15||P<sup>2−</sup>||Phosphorus||data-sort-value="-9.18"|-9.18||data-sort-value="-0.0000063"|-886||<ref name=Rayner-Canham/> |
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|16||S<sup>−</sup>||Sulfur||data-sort-value="-4.73"|-4.73||data-sort-value="-0.0000032"|-456||<ref name=Rayner-Canham/> |
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|33||As<sup>−</sup>||Arsenic||data-sort-value="-4.51"|-4.51||data-sort-value="-0.0000031"|-435||<ref name=Rayner-Canham/> |
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|33||As<sup>2−</sup>||Arsenic||data-sort-value="-8.31"|-8.31||data-sort-value="-0.0000057"|-802||<ref name=Rayner-Canham/> |
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* {{citation|first1=M.J.|last1=Travers|first2=D.C.|last2=Cowles|first3=G.B.|last3=Ellison|title=Reinvestigation of the electron affinities of O<sub>2</sub> and NO|journal=Chem. Phys. Lett.|volume=164|issue=5|page=449|year=1989|doi=10.1016/0009-2614(89)85237-6|bibcode=1989CPL...164..449T}} |
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* {{citation|last1=Zanni|first1=M.T.|last2=Taylor|first2=T.R.|last3=Greenblatt|first3=B.J.|last4=Soep|first4=B.|last5 =Neumark|first5=D.M.|title=Characterization of the I{{su|b=2|p=−}} anion ground state using conventional and femtosecond photoelectron spectroscopy|journal=J. Chem. Phys.|volume=107|issue=19|page=7613|year=1997|doi=10.1063/1.475110|bibcode=1997JChPh.107.7613Z}} |
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<ref name=AnderssonK>{{cite journal | last1 = Andersson | first1 = K.T. | last2 = Sandstrom | first2 = J. | last3 = Kiyan | first3 = I.Y. | last4 = Hanstorp | first4 = D. | last5 = Pegg | first5 = D.J. | year = 2000 | title = Measurement of the electron affinity of potassium | journal = Phys. Rev. A | volume = 62 | issue = 2| page = 022503 | doi = 10.1103/PhysRevA.62.022503 | bibcode = 2000PhRvA..62b2503A }}</ref> |
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<ref name=BilodeauIrPt>{{cite journal | last1 = Bilodeau | first1 = R.C. | last2 = Scheer | first2 = M. | last3 = Haugen | first3 = H.K. | last4 = Brooks | first4 = R.L. | year = 1999 | title = Near-threshold Laser Spectroscopy of Iridium and Platinum Negative Ions: Electron Affinities and the Threshold Law | journal = Phys. Rev. A | volume = 61 | issue = 1 | page = 012505 | doi = 10.1103/PhysRevA.61.012505 | bibcode = 1999PhRvA..61a2505B }}</ref> |
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<ref name=Carette>{{cite journal| last1 = Carette | first1 = T.| last2 = Drag | first2 = C. | last3 = Scharf | first3 = O. | last4 = Blondel | first4 = C. | last5 = Delsart | first5 = C. | last6 = Fischer | first6 = C. | year = 2000| title = F. & Godefroid M. (2010). Isotope shift in the sulfur electron affinity: Observation and theory | journal = Phys. Rev. A | volume = 81 | page = 042522 | doi = 10.1103/PhysRevA.81.042522 | arxiv = 1002.1297 | s2cid = 54056163}}</ref> |
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<ref name=TangU>Tang R., Lu Y., Liu H. & Ning C. (2021). "Electron affinity of uranium and bound states of opposite parity in its anion". ''Phys. Rev.'' A '''103''', L050801 {{doi|10.1103/PhysRevA.103.L050801}}</ref> |
<ref name=TangU>Tang R., Lu Y., Liu H. & Ning C. (2021). "Electron affinity of uranium and bound states of opposite parity in its anion". ''Phys. Rev.'' A '''103''', L050801 {{doi|10.1103/PhysRevA.103.L050801}}</ref> |
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<ref name=VandevrayeSe>{{cite journal | last1 = Vandevraye | first1 = M. | last2 = Drag | first2 = C. | last3 = Blondel | first3 = C. | year = 2012 | title = Electron affinity of selenium measured by photodetachment microscopy | journal = Phys. Rev. A | volume = 85 | issue = 1| page = 015401 | doi = 10.1103/PhysRevA.85.015401 | bibcode = 2012PhRvA..85a5401V }}</ref> |
<ref name=VandevrayeSe>{{cite journal | last1 = Vandevraye | first1 = M. | last2 = Drag | first2 = C. | last3 = Blondel | first3 = C. | year = 2012 | title = Electron affinity of selenium measured by photodetachment microscopy | journal = Phys. Rev. A | volume = 85 | issue = 1| page = 015401 | doi = 10.1103/PhysRevA.85.015401 | bibcode = 2012PhRvA..85a5401V }}</ref> |
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<ref name=ChenRe>{{cite journal | last1 = Chen | first1 = X.L. | last2 = Ning | first2 = C.G. | year = 2017 | title = Observation of Rhenium Anion and Electron Affinity of Re. | journal = J. Phys. Chem. Lett. | volume = 8 | issue = 12| pages = 2735–2738 | doi = 10.1021/acs.jpclett.7b01079 | pmid = 28581753 }}</ref> |
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Latest revision as of 18:48, 21 November 2024
This page deals with the electron affinity as a property of isolated atoms or molecules (i.e. in the gas phase). Solid state electron affinities are not listed here.
Elements
[edit]Electron affinity can be defined in two equivalent ways. First, as the energy that is released by adding an electron to an isolated gaseous atom. The second (reverse) definition is that electron affinity is the energy required to remove an electron from a singly charged gaseous negative ion. The latter can be regarded as the ionization energy of the –1 ion or the zeroth ionization energy.[1] Either convention can be used.[2]
Negative electron affinities can be used in those cases where electron capture requires energy, i.e. when capture can occur only if the impinging electron has a kinetic energy large enough to excite a resonance of the atom-plus-electron system. Conversely electron removal from the anion formed in this way releases energy, which is carried out by the freed electron as kinetic energy. Negative ions formed in these cases are always unstable. They may have lifetimes of the order of microseconds to milliseconds, and invariably autodetach after some time.
| Z | Element | Name | Electron affinity (eV) | Electron affinity (kJ/mol) | References |
|---|---|---|---|---|---|
| 1 | 1H | Hydrogen | 0.754 195(19) | 72.769(2) | [3] |
| 1 | 2H | Deuterium | 0.754 67(4) | 72.814(4) | [4] |
| 2 | He | Helium | −0.5(2) | −48(20) | est.[5] |
| 3 | Li | Lithium | 0.618 049(22) | 59.632 6(21) | [6] |
| 4 | Be | Beryllium | −0.5(2) | −48(20) | est.[5] |
| 5 | B | Boron | 0.279 723(25) | 26.989(3) | [7] |
| 6 | 12C | Carbon | 1.262 122 6(11) | 121.776 3(1) | [8] |
| 6 | 13C | Carbon | 1.262 113 6(12) | 121.775 5(2) | [8] |
| 7 | N | Nitrogen | −0.07 | −6.8 | [5] |
| 8 | 16O | Oxygen | 1.461 112 97(9) | 140.975 970(9) | [9] |
| 8 | 17O | Oxygen | 1.461 108(4) | 140.975 5(3) | [10] |
| 8 | 18O | Oxygen | 1.461 105(3) | 140.975 2(3) | [10] |
| 9 | F | Fluorine | 3.401 189 8(24) | 328.164 9(3) | [11][12] |
| 10 | Ne | Neon | −1.2(2) | −116(19) | est.[5] |
| 11 | Na | Sodium | 0.547 926(25) | 52.867(3) | [13] |
| 12 | Mg | Magnesium | −0.4(2) | −40(19) | est.[5] |
| 13 | Al | Aluminium | 0.432 83(5) | 41.762(5) | [14] |
| 14 | Si | Silicon | 1.389 521 2(8) | 134.068 4(1) | [15] |
| 15 | P | Phosphorus | 0.746 609(11) | 72.037(1) | [16] |
| 16 | 32S | Sulfur | 2.077 104 2(6) | 200.410 1(1) | [15] |
| 16 | 34S | Sulfur | 2.077 104 5(12) | 200.410 1(2) | [17] |
| 17 | Cl | Chlorine | 3.612 725(28) | 348.575(3) | [18] |
| 18 | Ar | Argon | −1.0(2) | −96(20) | est.[5] |
| 19 | K | Potassium | 0.501 459(13) | 48.383(2) | [19] |
| 20 | Ca | Calcium | 0.024 55(10) | 2.37(1) | [20] |
| 21 | Sc | Scandium | 0.179 380(23) | 17.307 6(22) | [21] |
| 22 | Ti | Titanium | 0.075 54(5) | 7.289(5) | [22] |
| 23 | V | Vanadium | 0.527 66(20) | 50.911(20) | [23] |
| 24 | Cr | Chromium | 0.675 928(27) | 65.217 2(26) | [21] |
| 25 | Mn | Manganese | −0.5(2) | −50(19) | est.[5] |
| 26 | Fe | Iron | 0.153 236(35) | 14.785(4) | [24] |
| 27 | Co | Cobalt | 0.662 255(47) | 63.897 9(45) | [25] |
| 28 | Ni | Nickel | 1.157 16(12) | 111.65(2) | [26] |
| 29 | Cu | Copper | 1.235 78(4) | 119.235(4) | [27] |
| 30 | Zn | Zinc | −0.6(2) | −58(20) | est.[5] |
| 31 | Ga | Gallium | 0.301 166(15) | 29.058 1(15) | [28] |
| 32 | Ge | Germanium | 1.232 676 4(13) | 118.935 2(2) | [29] |
| 33 | As | Arsenic | 0.804 8(2) | 77.65(2) | [30] |
| 34 | Se | Selenium | 2.020 604 7(12) | 194.958 7(2) | [31] |
| 35 | Br | Bromine | 3.363 588(3) | 324.536 9(3) | [11] |
| 36 | Kr | Krypton | −1.0(2) | −96(20) | est.[5] |
| 37 | Rb | Rubidium | 0.485 916(21) | 46.884(3) | [32] |
| 38 | Sr | Strontium | 0.052 06(6) | 5.023(6) | [33] |
| 39 | Y | Yttrium | 0.311 29(22) | 30.035(21) | [21] |
| 40 | Zr | Zirconium | 0.433 28(9) | 41.806(9) | [34] |
| 41 | Nb | Niobium | 0.917 40(7) | 88.516(7) | [35] |
| 42 | Mo | Molybdenum | 0.747 23(8) | 72.097(8) | [21] |
| 43 | Tc | Technetium | 0.55(20) | 53(20) | est.[36] |
| 44 | Ru | Ruthenium | 1.046 27(2) | 100.950(3) | [21] |
| 45 | Rh | Rhodium | 1.142 89(20) | 110.27(2) | [26] |
| 46 | Pd | Palladium | 0.562 14(12) | 54.24(2) | [26] |
| 47 | Ag | Silver | 1.304 47(3) | 125.862(3) | [27] |
| 48 | Cd | Cadmium | −0.7(2) | −68(20) | est.[5] |
| 49 | In | Indium | 0.383 92(6) | 37.043(6) | [37] |
| 50 | Sn | Tin | 1.112 070(2) | 107.298 4(3) | [38] |
| 51 | Sb | Antimony | 1.047 401(19) | 101.059(2) | [39] |
| 52 | Te | Tellurium | 1.970 875(7) | 190.161(1) | [40] |
| 53 | 127I | Iodine | 3.059 046 5(37) | 295.153 1(4) | [41] |
| 53 | 128I | Iodine | 3.059 052(38) | 295.154(4) | [42] |
| 54 | Xe | Xenon | −0.8(2) | −77(20) | est.[5] |
| 55 | Cs | Caesium | 0.4715983(38) | 45.5023(4) | [43] |
| 56 | Ba | Barium | 0.144 62(6) | 13.954(6) | [44] |
| 57 | La | Lanthanum | 0.557 546(20) | 53.795(2) | [45] |
| 58 | Ce | Cerium | 0.600 160(27) | 57.906 7(26) | [46] |
| 59 | Pr | Praseodymium | 0.109 23(46) | 10.539(45) | [47] |
| 60 | Nd | Neodymium | 0.097 49(33) | 9.406(32) | [47] |
| 61 | Pm | Promethium | 0.129 | 12.45 | [48] |
| 62 | Sm | Samarium | 0.162 | 15.63 | [48] |
| 63 | Eu | Europium | 0.116(13) | 11.2(13) | [49] |
| 64 | Gd | Gadolinium | 0.212(30) | 20.5(29) | [21] |
| 65 | Tb | Terbium | 0.131 31(80) | 12.670(77) | [47] |
| 66 | Dy | Dysprosium | 0.015(3) | 1.45(30) | [50] |
| 67 | Ho | Holmium | 0.338 | 32.61 | [48] |
| 68 | Er | Erbium | 0.312 | 30.10 | [48] |
| 69 | Tm | Thulium | 1.029(22) | 99(3) | [51] |
| 70 | Yb | Ytterbium | −0.02 | −1.93 | est.[36] |
| 71 | Lu | Lutetium | 0.238 8(7) | 23.04(7) | [52] |
| 72 | Hf | Hafnium | 0.178 0(7) | 17.18(7) | [53] |
| 73 | Ta | Tantalum | 0.328 859(23) | 31.730 1(22) | [21] |
| 74 | W | Tungsten | 0.816 26(8) | 78.76(1) | [54] |
| 75 | Re | Rhenium | 0.060 396(64) | 5.827 3(62) | [55] |
| 76 | Os | Osmium | 1.077 661(24) | 103.978 5(24) | [21] |
| 77 | Ir | Iridium | 1.564 057(12) | 150.908 6(12) | [56] |
| 78 | Pt | Platinum | 2.125 10(5) | 205.041(5) | [57] |
| 79 | Au | Gold | 2.308 610(25) | 222.747(3) | [58] |
| 80 | Hg | Mercury | −0.5(2) | −48(20) | est.[5] |
| 81 | Tl | Thallium | 0.320 053(19) | 30.880 4(19) | [59] |
| 82 | Pb | Lead | 0.356 721(2) | 34.418 3(3) | [60] |
| 83 | Bi | Bismuth | 0.942 362(13) | 90.924(2) | [61] |
| 84 | Po | Polonium | 1.40(7) | 136(7) | calc.[62] |
| 85 | At | Astatine | 2.415 78(7) | 233.087(8) | [63] |
| 86 | Rn | Radon | −0.7(2) | −68(20) | est.[5] |
| 87 | Fr | Francium | 0.486 | 46.89 | est.[64][36] |
| 88 | Ra | Radium | 0.10 | 9.648 5 | est.[65][36] |
| 89 | Ac | Actinium | 0.35 | 33.77 | est.[36] |
| 90 | Th | Thorium | 0.607 69(6) | 58.633(6) | [66] |
| 91 | Pa | Protactinium | 0.55 | 53.03 | est.[67] |
| 92 | U | Uranium | 0.314 97(9) | 30.390(9) | [68] |
| 93 | Np | Neptunium | 0.48 | 45.85 | est.[67] |
| 94 | Pu | Plutonium | −0.50 | −48.33 | est.[67] |
| 95 | Am | Americium | 0.10 | 9.93 | est.[67] |
| 96 | Cm | Curium | 0.28 | 27.17 | est.[67] |
| 97 | Bk | Berkelium | −1.72 | −165.24 | est.[67] |
| 98 | Cf | Californium | −1.01 | −97.31 | est.[67] |
| 99 | Es | Einsteinium | −0.30 | −28.60 | est.[67] |
| 100 | Fm | Fermium | 0.35 | 33.96 | est.[67] |
| 101 | Md | Mendelevium | 0.98 | 93.91 | est.[67] |
| 102 | No | Nobelium | −2.33 | −223.22 | est.[67] |
| 103 | Lr | Lawrencium | −0.31 | −30.04 | est.[67] |
| 111 | Rg | Roentgenium | 1.565 | 151.0 | calc.[69] |
| 113 | Nh | Nihonium | 0.69 | 66.6 | calc.[70] |
| 115 | Mc | Moscovium | 0.366 | 35.3 | calc.[70] |
| 116 | Lv | Livermorium | 0.776 | 74.9 | calc.[70] |
| 117 | Ts | Tennessine | 1.719 | 165.9 | calc.[70] |
| 118 | Og | Oganesson | 0.080(6) | 7.72(58) | calc.[71] |
| 119 | Uue | Ununennium | 0.662 | 63.87 | calc.[64] |
| 120 | Ubn | Unbinilium | 0.021 | 2.03 | calc.[72] |
| 121 | Ubu | Unbiunium | 0.57 | 55 | calc.[36] |
Molecules
[edit]The electron affinities Eea of some molecules are given in the table below, from the lightest to the heaviest. Many more have been listed by Rienstra-Kiracofe et al. (2002). The electron affinities of the radicals OH and SH are the most precisely known of all molecular electron affinities.
Second and third electron affinity
[edit]| Z | Element | Name | Electron affinity (eV) | Electron affinity (kJ/mol) | References |
|---|---|---|---|---|---|
| 7 | N− | Nitrogen | -6.98 | -673 | [74] |
| 7 | N2− | Nitrogen | -11.09 | -1070 | [74] |
| 8 | O− | Oxygen | -7.71 | -744 | [74] |
| 15 | P− | Phosphorus | -4.85 | -468 | [74] |
| 15 | P2− | Phosphorus | -9.18 | -886 | [74] |
| 16 | S− | Sulfur | -4.73 | -456 | [74] |
| 33 | As− | Arsenic | -4.51 | -435 | [74] |
| 33 | As2− | Arsenic | -8.31 | -802 | [74] |
| 34 | Se− | Selenium | -4.25 | -410 | [74] |
Bibliography
[edit]- Janousek, Bruce K.; Brauman, John I. (1979), "Electron affinities", in Bowers, M. T. (ed.), Gas Phase Ion Chemistry, vol. 2, New York: Academic Press, p. 53.
- Rienstra-Kiracofe, J.C.; Tschumper, G.S.; Schaefer, H.F.; Nandi, S.; Ellison, G.B. (2002), "Atomic and molecular electron affinities: Photoelectron experiments and theoretical computations", Chem. Rev., vol. 102, no. 1, pp. 231–282, doi:10.1021/cr990044u, PMID 11782134.
- Updated values can be found in the NIST chemistry webbook for around three dozen elements and close to 400 compounds.
Specific molecules
[edit]- Adams, C.L.; Schneider, H.; Ervin, K.M.; Weber, J.M. (2009), "Low-energy photoelectron imaging spectroscopy of nitromethane anions: Electron affinity, vibrational features, anisotropies, and the dipole-bound state", J. Chem. Phys., 130 (7): 074307, Bibcode:2009JChPh.130g4307A, doi:10.1063/1.3076892, PMID 19239294
- Borshchevskii, A.Ya.; Boltalina, O.V.; Sorokin, I.D.; Sidorov, L.N. (1988), "Thermochemical quantities for gas-phase iron, uranium, and molybdenum fluorides, and their negative ions", J. Chem. Thermodyn., 20 (5): 523, doi:10.1016/0021-9614(88)90080-8
- Chaibi, W.; Delsart, C.; Drag, C.; Blondel, C. (2006), "High precision measurement of the 32SH electron affinity by laser detachment microscopy", J. Mol. Spectrosc., 239 (1): 11, Bibcode:2006JMoSp.239...11C, doi:10.1016/j.jms.2006.05.012
- Chowdhury, S.; Kebarle, P. (1986), "Electron affinities of di- and tetracyanoethylene and cyanobenzenes based on measurements of gas-phase electron-transfer equilibria", J. Am. Chem. Soc., 108 (18): 5453, doi:10.1021/ja00278a014
- Ervin, K.M.; Ho, J.; Lineberger, W.C. (1988), "Ultraviolet photoelectron spectrum of nitrite anion", J. Phys. Chem., 92 (19): 5405, doi:10.1021/j100330a017
- Ervin, K.M.; Lineberger, W.C. (1991), "Photoelectron spectra of C−
2 and C2H−", J. Phys. Chem., 95 (3): 1167, doi:10.1021/j100156a026 - George, P.M.; Beauchamp, J.L. (1979), "The electron and fluoride affinities of tungsten hexafluoride by ion cyclotron resonance spectroscopy", Chem. Phys., 36 (3): 345, Bibcode:1979CP.....36..345G, doi:10.1016/0301-0104(79)85018-1
- Goldfarb, F.; Drag, C.; Chaibi, W.; Kröger, S.; Blondel, C.; Delsart, C. (2005), "Photodetachment microscopy of the P, Q, and R branches of the OH−(v=0) to OH(v=0) detachment threshold", J. Chem. Phys., 122 (1): 014308, Bibcode:2005JChPh.122a4308G, doi:10.1063/1.1824904, PMID 15638660
- Huang, Dao-Ling; Dau, Phuong Diem; Liu, Hong-Tao; Wang, Lai-Sheng (2014), "High-resolution photoelectron imaging of cold C−
60 anions and accurate determination of the electron affinity of C60", J. Chem. Phys., 140 (22): 224315, Bibcode:2014JChPh.140v4315H, doi:10.1063/1.4881421, PMID 24929396, S2CID 1061364 - Kim, J.B.; Weichman, M.L.; Neumark, D.M. (2015), "Low-lying states of FeO and FeO− by slow photoelectron spectroscopy", Mol. Phys., 113 (15–16): 2105, Bibcode:2015MolPh.113.2105K, doi:10.1080/00268976.2015.1005706, S2CID 13868986
- Mathur, B.P.; Rothe, E.W.; Tang, S.Y.; Reck, G.P. (1976), "Negative ions from phosphorus halides due to cesium charge exchange", J. Chem. Phys., 65 (2): 565, Bibcode:1976JChPh..65..565M, doi:10.1063/1.433109
- Mead, R.D.; Lykke, K.R.; Lineberger, W.C.; Marks, J.; Brauman, J.I. (1984), "Spectroscopy and dynamics of the dipole-bound state of acetaldehyde enolate", J. Chem. Phys., 81 (11): 4883, Bibcode:1984JChPh..81.4883M, doi:10.1063/1.447515
- Miller, T.M.; Leopold, D.G.; Murray, K.K.; Lineberger, W.C. (1986), "Electron affinities of the alkali halides and the structure of their negative ions", J. Chem. Phys., 85 (5): 2368, Bibcode:1986JChPh..85.2368M, doi:10.1063/1.451091
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