Strong Chemical Bonds
| Typical bond lengths in pm and bond energies in kJ/mol. |
||
| Bond | Length (pm) |
Energy (kJ/mol) |
|---|---|---|
| H — Hydrogen | ||
| H–H | 74 | 436 |
| H–O | 96 | 366 |
| H–F | 92 | 568 |
| H–Cl | 127 | 432 |
| C — Carbon | ||
| C–H | 109 | 413 |
| C–C | 154 | 348 |
| C–C= | 151 | |
| =C–C≡ | 147 | |
| =C–C= | 148 | |
| C=C | 134 | 614 |
| C≡C | 120 | 839 |
| C–N | 147 | 308 |
| C–O | 143 | 360 |
| C–F | 134 | 488 |
| C–Cl | 177 | 330 |
| N — Nitrogen | ||
| N–H | 101 | 391 |
| N–N | 145 | 170 |
| N≡N | 110 | 945 |
| O — Oxygen | ||
| O–O | 148 | 145 |
| O=O | 121 | 498 |
| F, Cl, Br, I — Halogens | ||
| F–F | 142 | 158 |
| Cl–Cl | 199 | 243 |
| Br–H | 141 | 366 |
| Br–Br | 228 | 193 |
| I–H | 161 | 298 |
| I–I | 267 | 151 |
Strong chemical bonds are the intramolecular forces which hold atoms together in molecules. A strong chemical bond is formed from the transfer or sharing of electrons between atomic centers and relies on the electrostatic attraction between the protons in nuclei and the electrons in the orbitals. Although these bonds typically involve the transfer of integer numbers of electrons (this is the bond order, which represents one transferred electron or two shared electrons), some systems can have intermediate numbers of bonds. An example of this is the organic molecule benzene, where the bond order is 1.5 for each carbon atom, meaning that it has 1.5 bonds (shares three electrons) with each one of its two neighbors.
The types of strong bond differ due to the difference in electronegativity of the constituent elements. A large difference in electronegativity leads to more polar (ionic) character in the bond.
Read more about this topic: Chemical Bond
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