Question

nf₃
draw the molecule by placing atoms on the grid and connecting them with bonds. include all lone pairs of electrons.

Explanation:

Step1: Determine the central atom

Nitrogen (\(N\)) is the central atom as it has a lower electronegativity than fluorine (\(F\)).

Step2: Calculate the total number of valence electrons

Nitrogen has \(5\) valence electrons and each fluorine has \(7\) valence electrons. For \(NF_3\), the total number of valence electrons is \(5+(3\times7)=26\).

Step3: Form single bonds

Form three single bonds (\(N - F\)) which use \(3\times2 = 6\) electrons.

Step4: Distribute the remaining electrons

We have \(26 - 6=20\) electrons left. Each fluorine atom gets \(6\) non - bonding electrons (three lone pairs) and nitrogen gets \(2\) non - bonding electrons (one lone pair).

Answer:

The Lewis structure of \(NF_3\) has a central nitrogen atom bonded to three fluorine atoms. Each \(N - F\) bond is a single bond. Nitrogen has one lone pair of electrons and each fluorine has three lone pairs of electrons.