In 3-4 sentences, identify how the geometric structure of NF3 is different than that of NF4+. Explain how the geometry affects the ability of the molecules to experience a dipole affect.

Question

anonymous · Answer

@aaronq @Abhisar

aaronq · Answer

$NF_3$ has an analous geometry to $NH_3$, and $NF_4^+$ has an analogous geometry to $CH_4$, you piece it together

anonymous · Answer

so NF3 is a trigonal pyramidal and NF4+ is a tetrahedral?

anonymous · Answer

@aaronq what is a dipole affect?

aaronq · Answer

that's correct. now in terms of dipole moments, which one has a net dipole moment and which one doesnt?

anonymous · Answer

Would NF4+ have the net dipole moment because it has a positive charge?

aaronq · Answer

nah. remember it's structure is analogous to $CH_4$ or even $CCl_4$ for that matter, do either of those have a net dipole moment?

anonymous · Answer

oh. Well is it NF3 because of the lone electron pair?

aaronq · Answer

yup thats it

anonymous · Answer

so would it be correct to say: "NF3 has a geometric shape of a trigonal pyramid. Because of its lone electron pair at the top, it has a net dipole moment. NF4+ has a geometric shape of a tetrahedral. NF4+ does not have a net dipole moment because it has a positive charge."  OR "NF3 has a geometric shape of a trigonal pyramid. Because of its lone electron pair at the top, it has a net dipole moment. NF4+ has a geometric shape of a tetrahedral. NF4+ does not have a net dipole moment because it has all of its orbitals filled."

aaronq · Answer

$NF_4^+$ does not have net dipole moment because the individual dipole moments of each N-F bond cancel each other out in 3D space.

it has nothing to do with the positive charge, really

anonymous · Answer

oh okay! thank you for the help!