Use Lewis structures and molecular geometry sketches as necessary to support your discussion. Both molecules have four pairs of electrons around the central atom, and so both have a tetrahedral electron configuration, which leads to both having bond angles that are close to 109.5 . However, ammonia has 3 bonding pairs and one lone pair, while water has 2 bonding pairs and two lone pairs. Assign formal charges to all atoms. Identify all s and p bonds and indicate what atomic or hybrid orbitals combine to form the molecular orbitals.
All formal charges are zero.
Use this to predict which molecule has the larger bond energy. Briefly state your reasoning in each case, referring to your answers in question 2 as necessary. If yes, please do so and explain. If no, explain why not. Relationship cannot be predicted.