Question

Draw lewis structures for NOBr, NO-, HCN, NBr3

1. which of the molecules are linear
2. which of the molecules have no lone pairs
3. which of the molecules have sp3 hybridization
4. which molecules have an atom with nonzero formal charge

Answer 1

HCN is the only linear molecule with no lone pairs and sp hybridization. NOBr, NO-, and NBr3 are molecules that have atoms with nonzero formal charges, with NBr3 having sp3 hybridization.

Step-by-step explanation:

When drawing Lewis structures for NOBr, NO-, HCN, and NBr3, consider the total number of valence electrons for each molecule to ensure that each atom achieves a full octet where possible, or in the case of boron and hydrogen, a satisfied valence shell. Here is a breakdown responding to the student's query:

1. HCN is a linear molecule with no lone pairs on either the hydrogen or nitrogen. Nitrogen is sp hybridized in HCN, forming a triple bond with carbon and a single bond with hydrogen.
2. NOBr is a nonlinear molecule and has lone pairs on both the nitrogen and bromine atoms. Nitrogen has one lone pair, and bromine has three. This molecule displays a range of formal charges, due to the bonding arrangement.
3. The anion NO- has one lone pair on the nitrogen atom and is bent due to the lone pair-bonding pair repulsion. Nitrogen here has a nonzero formal charge.
4. NBr3 is a trigonal pyramidal molecule with sp3 hybridization and a lone pair on the nitrogen atom. Here, nitrogen will have a nonzero formal charge.

To quickly summarize:

1. The only linear molecule is HCN.
2. The molecule with no lone pairs is HCN.
3. The molecule with sp3 hybridization is NBr3.
4. Molecules with an atom with nonzero formal charge are NOBr, NO-, and NBr3.