kimiaUNY said:My answer is NH3, because H is smaller than CH3. so lone pair electron of N can easily push the H and make the bond smaller. Is this right?
NH3, or ammonia, has a trigonal pyramidal molecular structure with a bond angle of approximately 107 degrees. N(CH3)3, or trimethylamine, has a trigonal pyramidal molecular structure with a bond angle of approximately 110 degrees.
NH3 has a smaller bond angle of approximately 107 degrees, while N(CH3)3 has a slightly larger bond angle of approximately 110 degrees.
The difference in bond angles between NH3 and N(CH3)3 is due to the presence of three methyl groups in N(CH3)3, which causes repulsion between the electron pairs and results in a slightly larger bond angle.
Yes, bond angles can also be affected by the presence of lone pairs of electrons, as well as the electronegativity and size of the atoms involved in the bonding.
The bond angle can affect the polarity, reactivity, and shape of a molecule, which can in turn affect its physical and chemical properties. For example, NH3 is highly polar and is known for its strong odor, while N(CH3)3 is less polar and has a weaker odor.