Be sure to answer all parts. Use MO diagrams to place C2−, C2, C2+ in order of the following properties: (a) increasing bond energy C2− < C2 < C2+ C2− < C2+ < C2 C2 < C2− < C2+ C2 < C2+ < C2− C2+ < C2 < C2− C2+ < C2− < C2 (b) increasing bond length C2− < C2 < C2+ C2− < C2+ < C2 C2 < C2− < C2+ C2 < C2+ < C2− C2+ < C2 < C2− C2+ < C2− < C2

Bond Order = ½ [# bonded e--# antibonded e-]

C2= ½ [6-2] = 2

C2+= ½ [5-2] = 1.5

C2- = ½ [7-2] = 2.5

Bond Length: C2+> C2> C2-

Bond Energy: C2-> C2> C2+

Explanation:

Bond order is a measurement of the number of electrons involved in bonds between two atoms in a molecule.

How to calculate bond order

1. Draw the Lewis structure.

2. Count the total number of bonds.

3. Count the number of bond groups between individual atoms.

4. Divide the number of bonds between atoms by the total number of bond groups in the molecule.

Bond energy (E) is defined as the amount of energy required to break apart a mole of molecules into its component atoms. It is a measure of the strength of a chemical bond.

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