Given below are two statements: Statement I: Since fluorine is more electronegative than nitrogen, the net dipole…

🧠 Both statements involve the relationship between electronegativity and dipole moment direction in $\mathrm{NH_3}$ and $\mathrm{NF_3}$.

🗺️ Statement I — "$\mathrm{NF_3}$ has greater dipole moment than $\mathrm{NH_3}$":

• Actual values: $\mathrm{NH_3}$ μ ≈ 1.47 D; $\mathrm{NF_3}$ μ ≈ 0.24 D
• $\mathrm{NH_3}$ has the greater dipole moment, not $\mathrm{NF_3}$
• Statement I is FALSE ✗

Statement II — "In $\mathrm{NH_3}$, LP dipole and N–H bond dipoles are in opposite direction; in $\mathrm{NF_3}$ they are in the same direction":

• In $\mathrm{NH_3}$: bond dipoles (N–H) point toward N; lone pair dipole also points away from N in the same direction → they add (same direction)
• In $\mathrm{NF_3}$: bond dipoles (N–F) point away from N; lone pair dipole points toward N → they oppose (opposite direction)
• Statement II has it backwards → Statement II is FALSE ✗

⚡ The correct picture: In $\mathrm{NH_3}$, LP and bond dipoles reinforce → large μ. In $\mathrm{NF_3}$, LP and bond dipoles oppose → small μ. Statement II inverts this.

$\boxed{\text{Answer: Both Statement I and Statement II are false}}$