Question

what are the angles a and b in the actual molecule of which this is a lewis structure? note for advanced students: give the ideal angles, and dont worry about small differences from the ideal that might be caused by the fact that different electron groups may have slightly different sizes.

Explanation:

Step1: Analyze the left - hand carbon

The left - hand carbon with the angle \(a\) is \(sp^{2}\) hybridized. In an \(sp^{2}\) hybridized carbon, the ideal bond - angle is based on trigonal planar geometry.
The ideal bond - angle for \(sp^{2}\) hybridized carbon is \(120^{\circ}\). So \(a = 120\).

Step2: Analyze the right - hand carbon

The right - hand carbon with the angle \(b\) is \(sp^{3}\) hybridized. In an \(sp^{3}\) hybridized carbon, the ideal bond - angle is based on tetrahedral geometry.
The ideal bond - angle for \(sp^{3}\) hybridized carbon is \(109.5^{\circ}\). So \(b=109.5\).

Answer:

\(a = 120\)
\(b = 109.5\)