Question

below is the lewis structure of the acetylene $(c_{2}h_{2})$ molecule.

$h:c:::c:h$

count the number of bonding pairs and the number of lone pairs around the left carbon atom in this molecule.

bonding pairs:

lone pairs: 0

Explanation:

Step1: Analyze the bonds of the left carbon atom

In the Lewis structure \(H:C:::C:H\), the left - hand \(C\) atom has a single bond with \(H\) (which is 1 bonding pair) and a triple bond with the other \(C\) atom. A triple bond consists of 3 bonding pairs.

Step2: Calculate the total number of bonding pairs

The total number of bonding pairs around the left - hand \(C\) atom is \(1 + 3=4\)

Answer:

bonding pairs: \(4\)