Consider a molecule with the formula AX2. Supposing the A-X bond is polar, how would you expect the dipole moment of the AX2 molecule to change as the X-A-X bond angle decreases from 180° to 100°?

Verified step by step guidance

1. Step 1: Understand the concept of dipole moment. The dipole moment is a measure of the separation of positive and negative charges in a molecule. It is a vector quantity, meaning it has both magnitude and direction.
2. Step 2: Consider the geometry of the AX2 molecule. When the X-A-X bond angle is 180°, the molecule is linear, and if the A-X bonds are equally polar, their dipole moments cancel each other out, resulting in a net dipole moment of zero.
3. Step 3: Analyze the effect of decreasing the bond angle. As the X-A-X bond angle decreases from 180° to 100°, the molecule becomes bent. This change in geometry affects the vector addition of the individual bond dipoles.
4. Step 4: Predict the change in dipole moment. With a bent geometry, the dipole moments of the A-X bonds no longer cancel completely. The net dipole moment becomes non-zero and increases as the bond angle decreases.
5. Step 5: Conclude the relationship. The dipole moment of the AX2 molecule increases as the X-A-X bond angle decreases from 180° to 100°, due to the change from a linear to a bent molecular shape, which prevents complete cancellation of the bond dipoles.