Final answer:
The incorrect statement is that 'The melting point of Methane is higher than that of Ammonia.' The opposite is true; ammonia has a higher melting point than methane due to its stronger hydrogen bonding.
Step-by-step explanation:
The statement that is not correct is 'e) The melting point of Methane is higher than that of Ammonia.' Methane (CH4) has a lower melting point than ammonia (NH3).
Methane's tetrahedral molecular geometry is characterized by H-C-H bond angles of 109.5°, which is larger than the 90° it would be if the molecule was planar. Water's H-O-H bond angle is about 104.5° because of the lone pairs of electrons that occupy more space and exert greater repulsion, slightly reducing the angle from the perfect tetrahedral angle.
Hydrogen bonds contribute to the significantly higher boiling points of molecules like water (H2O), where hydrogen is bonded to highly electronegative atoms such as O, N, or F. This is why the boiling point of H2O is higher than that of H2S, and also why the melting point of H2O is higher than that of more weakly bonded molecules like methane (CH4) and ammonia (NH3).