Multiple Choice
Which of the following statements correctly describes the Lewis dot structure of the SnCl2 molecule?
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11. Bonding & Molecular Structure
Lewis Dot Structures: Ions
Multiple Choice
Which of the following statements correctly describes the Lewis dot structure for the ion NHCl2\(^-\)?
A
Nitrogen is the central atom, bonded to one hydrogen and two chlorine atoms, with no lone pairs and a positive formal charge.
B
Nitrogen is the central atom, bonded to one hydrogen and two chlorine atoms, with one lone pair on nitrogen and a negative formal charge.
C
Nitrogen is the central atom, bonded to two hydrogens and one chlorine atom, with no lone pairs on nitrogen.
D
Chlorine is the central atom, bonded to two hydrogens and one nitrogen atom, with a positive formal charge.
Verified step by step guidance1
Identify the central atom in the ion NHCl2\(^-\) by considering electronegativity and bonding preferences. Nitrogen is less electronegative than chlorine and typically forms multiple bonds, so nitrogen is the central atom.
Determine the total number of valence electrons available for the Lewis structure. Sum the valence electrons from nitrogen (5), hydrogen (1), chlorine atoms (7 each), and add one extra electron for the negative charge.
Draw single bonds between the central nitrogen atom and the surrounding atoms: one hydrogen and two chlorine atoms. Each bond represents two electrons.
Distribute the remaining valence electrons as lone pairs to satisfy the octet rule for each atom, starting with the more electronegative atoms (chlorine) and then placing any leftover electrons on nitrogen.
Calculate the formal charge on each atom using the formula \(\text{Formal charge} = \text{Valence electrons} - \text{Nonbonding electrons} - \frac{1}{2} \times \text{Bonding electrons}\) to confirm that nitrogen carries a negative formal charge and has one lone pair, consistent with the correct Lewis structure.
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