Multiple Choice
In the Lewis dot structure of the neutral compound NF_3, how many lone pairs of electrons are present on the nitrogen atom?
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11. Bonding & Molecular Structure
Lewis Dot Structures: Neutral Compounds
Multiple Choice
Which of the following Lewis dot structures represents a valid neutral compound?
A
A structure for CH\(_4\) with the carbon atom having three lone pairs and single bonds to each hydrogen atom.
B
A structure for CO\(_2\) with each oxygen atom having two lone pairs and double bonds to the central carbon atom.
C
A structure for NH\(_3\) with the nitrogen atom having no lone pairs and each hydrogen atom sharing two pairs of electrons with nitrogen.
D
A structure for H\(_2\)O with the oxygen atom having only one lone pair and single bonds to each hydrogen atom.
Verified step by step guidance1
Step 1: Understand the octet rule and the typical bonding patterns for each atom involved. Carbon usually forms 4 bonds to complete its octet, nitrogen typically forms 3 bonds and has one lone pair, oxygen usually forms 2 bonds and has 2 lone pairs, and hydrogen forms 1 bond with no lone pairs.
Step 2: Analyze the CH\(_4\) structure described: carbon with three lone pairs and single bonds to hydrogens. Since carbon has 4 valence electrons, having three lone pairs (6 electrons) plus bonds to hydrogens would exceed the octet rule, making this structure invalid.
Step 3: Examine the CO\(_2\) structure with carbon double bonded to each oxygen and each oxygen having two lone pairs. This arrangement satisfies the octet rule for carbon (4 bonds total) and oxygen (2 bonds plus 2 lone pairs), making it a valid neutral compound.
Step 4: Consider the NH\(_3\) structure with nitrogen having no lone pairs and each hydrogen sharing two pairs of electrons with nitrogen. Nitrogen typically has one lone pair; having no lone pairs and hydrogens sharing two pairs each would violate typical bonding and electron count rules, so this is invalid.
Step 5: Look at the H\(_2\)O structure with oxygen having only one lone pair and single bonds to hydrogens. Oxygen normally has two lone pairs; having only one lone pair would mean oxygen has fewer than 8 electrons, violating the octet rule, so this structure is invalid.
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