Multiple Choice
Which of the following correctly represents the Lewis dot structure for a neutral molecule of HCl?
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11. Bonding & Molecular Structure
Lewis Dot Structures: Neutral Compounds
Multiple Choice
Which of the following best describes the correct Lewis dot structure for neutral HNO?
A
H is bonded to N, which is single-bonded to O; N has two lone pairs, O has three lone pairs.
B
H is bonded to N, which is double-bonded to O; N has one lone pair, O has two lone pairs.
C
H is bonded to O, which is single-bonded to N; N has three lone pairs, O has two lone pairs.
D
H is bonded to O, which is double-bonded to N; N has two lone pairs, O has one lone pair.
Verified step by step guidance1
Step 1: Determine the total number of valence electrons for the molecule HNO. Hydrogen (H) has 1 valence electron, Nitrogen (N) has 5, and Oxygen (O) has 6. Add these together to find the total valence electrons available for bonding and lone pairs.
Step 2: Decide on a reasonable skeletal structure. Since hydrogen can only form one bond, it will be bonded to either nitrogen or oxygen. Consider typical bonding patterns: hydrogen usually bonds to more electronegative atoms like oxygen, but nitrogen can also bond to hydrogen. Explore both possibilities.
Step 3: Draw bonds between atoms and assign electrons to satisfy the octet rule (or duet for hydrogen). Start by placing single bonds between atoms, then add lone pairs to complete the octets of nitrogen and oxygen. Remember hydrogen only needs 2 electrons total.
Step 4: Check the formal charges on each atom to find the most stable Lewis structure. Calculate formal charge using the formula: \(\text{Formal Charge} = \text{Valence Electrons} - (\text{Nonbonding Electrons} + \frac{1}{2} \times \text{Bonding Electrons})\). The best Lewis structure has formal charges closest to zero on all atoms.
Step 5: Compare the possible Lewis structures based on bonding, lone pairs, and formal charges. The correct structure will have hydrogen bonded to nitrogen, nitrogen double bonded to oxygen, nitrogen with one lone pair, and oxygen with two lone pairs, as this arrangement satisfies the octet rule and minimizes formal charges.
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