Question

1. a molecule has 2 double bonds on the central atom and no lone pairs. predict the electron geometry. predict the molecule geometry. what do you think the bond angles would be?

Explanation:

Step1: Determine electron geometry

According to VSEPR (Valence - Shell Electron - Pair Repulsion) theory, when the central atom has 2 bonding regions (double bonds count as one region for electron - geometry determination) and 0 lone pairs, the electron geometry is based on the number of electron - pair regions around the central atom. The formula for electron - geometry is determined by \(n=\text{number of bonding regions}+\text{number of lone pairs}\). Here \(n = 2+0=2\). The electron geometry for \(n = 2\) is linear.

Step2: Determine molecular geometry

Since there are no lone pairs on the central atom, the molecular geometry is the same as the electron geometry. When there are 2 double bonds (bonding regions) and 0 lone pairs, the molecular geometry is also linear.

Step3: Determine bond angles

For a linear electron and molecular geometry (either from \(sp\) hybridization or VSEPR theory predictions), the bond angles between the two regions (double bonds in this case) is \(180^{\circ}\).

Answer:

• Electron geometry: Linear
• Molecular geometry: Linear
• Bond angles: \(180^{\circ}\)