Question

Using Lewis structure drawings, determine which molecule below will have the shortest bond length

between atoms:
A). N₂
B). O₂
C). Cl₂
D). Br₂
E). S₂

Answer 1

The molecule with the shortest bond length among the given options is N₂, which has a triple bond with the highest bond order, leading to a shorter bond than double or single bonds.

Step-by-step explanation:

To determine which molecule will have the shortest bond length, we must consider the Lewis structures and the type of covalent bonds formed between atoms. Bond length is affected by bond order; the greater the bond order, the shorter the bond length.

For each molecule:

• N₂: Forms a triple bond with a bond order of 3.
• O₂: Forms a double bond with a bond order of 2.
• Cl₂: Forms a single bond with a bond order of 1.
• Br₂: Forms a single bond with a bond order of 1.
• S₂: Typically forms a single bond with a bond order of 1.

Therefore, molecule A, N₂, with a triple bond, will have the shortest bond length compared to the other molecules that either have double bonds or single bonds.