640:, where a more negative lattice energy corresponds to a stronger force of attraction between the ions. Generally, greater differences in electronegativity correspond to stronger ionic bonds. For example, the compound sodium chloride (NaCl) has a lattice energy of -786 kJ/mol with an electronegativity difference of 2.23 between sodium and chlorine. Meanwhile, the compound sodium iodide (NaI) has a lower lattice energy of -704 kJ/mol with a similarly lower electronegativity difference of 1.73 between sodium and iodine.
347:
241:
355:
Although the two bonds are the equivalent in the original symmetric molecule, the bond-dissociation energy of an oxygen–hydrogen bond varies slightly depending on whether or not there is another hydrogen atom bonded to the oxygen atom. Thus, the bond energy of a molecule of water is 461.5 kJ/mol
610:
491:
615:
This ratio is notably lower than 1, indicating that there is a large amount of overlap between the valence electron clouds of the two rhenium atoms. From this data, we can conclude that this is a very strong bond. Experimentally, the Re-Re bond in was found to be a
314:, divided by four. The exact value for a certain pair of bonded elements varies somewhat depending on the specific molecule, so tabulated bond energies are generally averages from a number of selected typical chemical species containing that type of bond.
94:
250:
for a given bond is equal to the energy of the individual components that make up the bond when they are free and unbonded minus the energy of the components when they are bonded together. These energies are given by the
512:
396:
236:{\displaystyle {\begin{array}{lcl}\mathrm {D^{\circ }(R-} X)\ =\Delta H_{f}^{\circ }\mathrm {(R)} +\Delta H_{f}^{\circ }(X)-\Delta H_{f}^{\circ }(\mathrm {R} X)\end{array}}}
330:
of a single type of bond in a given molecule. The bond-dissociation energies of several different bonds of the same type can vary even within a single molecule.
496:
This ratio is slightly larger than 1, indicating that the bond itself is slightly longer than the expected minimum overlap between the two boron atoms'
838:
60:
The bond dissociation energy (enthalpy) is also referred to as bond disruption energy, bond energy, bond strength, or binding energy (abbreviation:
1010:
Cotton, F. A.; Curtis, N. F.; Harris, C. B.; Johnson, B. F. G.; Lippard, S. J.; Mague, J. T.; Robinson, W. R.; Wood, J. S. (1964-09-18).
605:{\displaystyle {\frac {224\ {\text{pm}}}{135\ {\text{pm}}+135\ {\text{pm}}}}={\frac {224\ {\text{pm}}}{270\ {\text{pm}}}}\approx \ 0.83}
636:
of the two atoms bonding together has a major effect on their bond energy. The extent of this effect is described by the compound's
486:{\displaystyle {\frac {175\ {\text{pm}}}{85\ {\text{pm}}+85\ {\text{pm}}}}={\frac {175\ {\text{pm}}}{170\ {\text{pm}}}}\approx 1.03}
265:
The enthalpy of formation of a large number of atoms, free radicals, ions, clusters and compounds is available from the websites of
1132:
1107:
889:
810:
1154:
1082:
1058:
778:
868:
507:
is 135 pm, with a Re–Re bond length of 224 pm in the compound . Taking the same steps as above gives a ratio of
933:
359:
When the bond is broken, the bonding electron pair will split equally to the products. This process is called
803:
CRC Handbook of
Chemistry and Physics, 97th Edition (CRC Handbook of Chemistry & Physics) 97th Edition
57:(usually at a temperature of 298.15 K) for all bonds of the same type within the same chemical species.
391:
is 175 pm. Dividing the length of this bond by the sum of each boron atom's radius gives a ratio of
905:
649:
327:
54:
1159:
375:
of the atoms that form the bond to the length of bond itself. For example, the atomic radius of
768:
252:
1011:
692:
Treptow, Richard S. (1995). "Bond
Energies and Enthalpies: An Often Neglected Difference".
8:
825:
Luo, Yu-Ran and Jin-Pei Cheng "Bond
Dissociation Energies". In Lide, David R. (ed) 2017,
311:
664:
1012:"Mononuclear and Polynuclear Chemistry of Rhenium (III): Its Pronounced Homophilicity"
867:
Madhusha (2017), Difference
Between Bond Energy and Bond Dissociation Energy, Pediaa,
1128:
1103:
1078:
1054:
1031:
992:
953:
885:
806:
784:
774:
746:
659:
633:
99:
848:
346:
1023:
984:
945:
852:
843:
736:
728:
701:
629:
497:
1027:
341:
O is the average energy required to break each of the two O–H bonds in sequence:
1051:
Bonding and
Structure: Structural Principles in Inorganic and Organic Chemistry
669:
654:
637:
620:. This method of determination is most useful for covalently bonded compounds.
617:
334:
1148:
1035:
996:
957:
847:, 2nd ed. (the "Gold Book") (1997). Online corrected version: (2006–) "
788:
770:
Advanced
Organic Chemistry: Reactions, Mechanisms, and Structure, 3rd edition
750:
372:
360:
72:). It is defined as the standard enthalpy change of the following fission: R—
32:
906:"Illustrated Glossary of Organic Chemistry - Homolytic cleavage (homolysis)"
856:
741:
500:
clouds. Thus, we can conclude that this bond is a rather weak single bond.
310:) of breaking one molecule of methane into a carbon atom and four hydrogen
363:(homolytic cleavage; homolysis) and results in the formation of radicals.
829:, 97th edition (2016–2017). Boca Raton: Taylor & Francis Group. 9-73.
764:
988:
949:
732:
705:
971:
Atoji, Masao; Wheatley, Peter J.; Lipscomb, William N. (1957-07-01).
380:
20:
972:
337:
is composed of two O–H bonds bonded as H–O–H. The bond energy for H
293:
41:
53:. IUPAC defines bond energy as the average value of the gas-phase
973:"Crystal and Molecular Structure of Diboron Tetrachloride, B2Cl4"
504:
297:
880:
Lehninger, Albert L.; Nelson, David L.; Cox, Michael M. (2005).
719:
Christian, Jerry D. (1973-03-01). "Strength of
Chemical Bonds".
1123:
Huheey, James E.; Keiter, Ellen A.; Keiter, Richard L. (2009).
289:
274:
317:
376:
278:
1125:
Inorganic chemistry: principles of structure and reactivity
869:
Difference
Between Bond Energy and Bond Dissociation Energy
270:
266:
1009:
371:
The strength of a bond can be estimated by comparing the
366:
1102:(Fifth ed.). New York: W. H. Freeman and Company.
623:
88:), is usually derived by the thermochemical equation,
970:
515:
399:
97:
1122:
879:
604:
485:
235:
1146:
763:
345:
1053:. New York: Ellis Horwood. pp. 40–42.
800:
318:Bond energy versus bond-dissociation energy
740:
718:
503:In another example, the atomic radius of
1077:(65th ed.). CRC Press. 1984-06-27.
884:(4th ed.). New York: W.H. Freeman.
805:(97th ed.). CRC Press; 97 edition.
1100:Shriver and Atkins' Inorganic Chemistry
691:
383:, while the length of the B–B bond in B
31:) is one measure of the strength of a
1147:
1097:
1048:
931:
927:
925:
367:Predicting the bond strength by radius
827:CRC Handbook of Chemistry and Physics
687:
685:
882:Lehninger principles of biochemistry
1127:(4th ed.). Cambridge: Harper.
1075:Handbook of Chemistry & Physics
922:
624:Factors affecting ionic bond energy
262:º of the components in each state.
13:
844:Compendium of Chemical Terminology
682:
219:
197:
167:
157:
135:
116:
104:
14:
1171:
246:This equation tells us that the
1116:
1091:
1067:
1042:
1003:
977:The Journal of Chemical Physics
964:
938:The Journal of Chemical Physics
898:
873:
861:
849:Bond energy (mean bond energy)
832:
819:
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757:
712:
226:
215:
191:
185:
160:
154:
126:
113:
1:
1028:10.1126/science.145.3638.1305
801:Haynes, William (2016–2017).
721:Journal of Chemical Education
694:Journal of Chemical Education
675:
35:. It is sometimes called the
1098:Atkins; et al. (2009).
932:Slater, J. C. (1964-11-15).
7:
643:
16:Strength of a chemical bond
10:
1176:
934:"Atomic Radii in Crystals"
328:bond-dissociation energies
306:is the enthalpy change (∆
1155:Chemical bond properties
650:Bond-dissociation energy
326:) is the average of all
55:bond-dissociation energy
857:10.1351/goldbook.B00701
361:homolytic bond cleavage
281:. Most authors use the
1049:Alcock, N. W. (1990).
606:
487:
350:
237:
607:
488:
349:
253:enthalpy of formation
238:
47:average bond enthalpy
513:
397:
285:values at 298.15 K.
95:
1022:(3638): 1305–1307.
773:, New York: Wiley,
379:is estimated at 85
214:
184:
152:
665:Isodesmic reaction
602:
483:
356:(110.3 kcal/mol).
351:
233:
231:
200:
170:
138:
84:, denoted by Dº(R—
1134:978-0-06-042995-9
1109:978-1-4292-1820-7
989:10.1063/1.1743668
950:10.1063/1.1725697
944:(10): 3199–3204.
910:www.chem.ucla.edu
891:978-0-7167-4339-2
733:10.1021/ed050p176
706:10.1021/ed072p497
660:Ionization energy
634:electronegativity
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1160:Binding energy
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1002:
983:(1): 196–199.
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42:bond enthalpy
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33:chemical bond
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913:. Retrieved
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765:March, Jerry
759:
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373:atomic radii
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85:
81:
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40:
36:
28:
24:
18:
25:bond energy
1149:Categories
915:2019-11-27
727:(3): 176.
700:(6): 497.
676:References
1036:0036-8075
997:0021-9606
958:0021-9606
789:642506595
751:0021-9584
594:≈
478:≈
211:∘
198:Δ
195:−
181:∘
168:Δ
149:∘
136:Δ
120:−
109:∘
37:mean bond
21:chemistry
767:(1985),
644:See also
312:radicals
294:hydrogen
1016:Science
505:rhenium
298:methane
1131:
1106:
1081:
1057:
1034:
995:
956:
888:
809:
787:
777:
749:
632:, the
597:
583:
570:
550:
536:
523:
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454:
434:
420:
407:
290:carbon
277:, and
275:CODATA
130:
80:. The
76:→ R +
839:IUPAC
377:boron
304:(C–H)
279:IUPAC
68:, or
49:, or
1129:ISBN
1104:ISBN
1079:ISBN
1055:ISBN
1032:ISSN
993:ISSN
954:ISSN
886:ISBN
807:ISBN
785:OCLC
775:ISBN
747:ISSN
600:0.83
481:1.03
271:NASA
267:NIST
1024:doi
1020:145
985:doi
946:doi
853:doi
851:".
737:hdl
729:doi
702:doi
628:In
580:270
567:224
547:135
533:135
520:224
464:170
451:175
404:175
283:BDE
248:BDE
82:BDE
62:BDE
19:In
1151::
1030:.
1018:.
1014:.
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471:pm
458:pm
438:pm
431:85
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417:85
411:pm
387:Cl
381:pm
324:BE
301:BE
273:,
269:,
66:BE
64:,
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1137:.
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704::
561:=
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445:=
428:+
389:4
385:2
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292:–
259:f
257:H
255:Δ
227:)
224:X
220:R
216:(
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202:H
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189:X
186:(
176:f
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158:R
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114:(
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86:X
78:X
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27:(
Text is available under the Creative Commons Attribution-ShareAlike License. Additional terms may apply.
