TABLE 1-2 Average Bond Energies of Common Single Bonds H N F CI Br I Si kJ kcal kJ kcal kJ kcal J kcal kJ kcal kJ kcal kJ kcal kJ kcal kJ kcal mol mol mol mol mol mol mol mol mol mol mol mol mol mol mol mol mol mol 436 104 418 100 389 93 460 110 569 136 431 103 368 88 297 71 301 72 418 100 339 81 289 69 351 84 439 105 331 79 280 67 238 57 289 69 N 389 93 289 69 159 38 180 43 272 65 201 48 243 58 169 40 355 85 460 110 351 84 180 43 138 33 209 50 209 50 222 53 238 57 430 103 F 569 136 439 105 272 65 209 50 159 38 251 60 251 60 280 67 586 140 CI 431 103 331 79 201 48 209 50 251 60 243 58 222 53 209 50 402 96 Br 368 88 280 67 243 58 222 53 251 60 222 53 192 46 180 43 289 69 I 297 71 238 57 169 40 238 57 280 67 209 50 180 43 151 36 209 50 Si 301 72 289 69 355 85 430 103 586 140 402 96 289 69 209 50 223 53 2 2
Types of Chemical Bonds
The attractive force which has the ability of holding various constituent elements like atoms, ions, molecules, etc. together in different chemical species is termed as a chemical bond. Chemical compounds are dependent on the strength of chemical bonds between its constituents. Stronger the chemical bond, more will be the stability in the chemical compounds. Hence, it can be said that bonding defines the stability of chemical compounds.
Polarizability In Organic Chemistry
Polarizability refers to the ability of an atom/molecule to distort the electron cloud of neighboring species towards itself and the process of distortion of electron cloud is known as polarization.
Coordinate Covalent Bonds
A coordinate covalent bond is also known as a dative bond, which is a type of covalent bond. It is formed between two atoms, where the two electrons required to form the bond come from the same atom resulting in a semi-polar bond. The study of coordinate covalent bond or dative bond is important to know about the special type of bonding that leads to different properties. Since covalent compounds are non-polar whereas coordinate bonds results always in polar compounds due to charge separation.
According to Table 1-2, which of the following compounds has the strongest single bond? The weakest? HCl; CH4; H2O; HF; Cl2
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