Multiple Choice
Which of the following statements correctly describes the Lewis dot structure of NF_3 (nitrogen trifluoride)?
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11. Bonding & Molecular Structure
Lewis Dot Structures: Neutral Compounds
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Which of the following best describes the Lewis dot structure for a neutral molecule of HBr?
A
H is bonded to Br, and neither atom has any lone pairs.
B
H is bonded to Br, and Br has two lone pairs of electrons.
C
H is bonded to Br, and Br has four lone pairs of electrons.
D
H is bonded to Br, and Br has three lone pairs of electrons.
Verified step by step guidance1
Recall that a Lewis dot structure represents the valence electrons of atoms in a molecule, showing bonds as shared pairs and lone pairs as non-bonded electrons around atoms.
Determine the total number of valence electrons for the molecule HBr. Hydrogen (H) has 1 valence electron, and bromine (Br), being in group 17, has 7 valence electrons, so total valence electrons = 1 + 7 = 8.
Draw a single bond between H and Br to represent the shared pair of electrons forming the bond. This bond accounts for 2 electrons.
Distribute the remaining valence electrons as lone pairs on the bromine atom. Since 2 electrons are used in the bond, 6 electrons remain, which correspond to 3 lone pairs on Br.
Verify that hydrogen has 2 electrons around it (satisfying its duet rule) and bromine has 8 electrons total (2 in the bond + 6 in lone pairs), satisfying the octet rule for Br.
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