Multiple Choice
After drawing the Lewis structure of H2CS (thioformaldehyde), what are the electron domain geometry and molecular geometry around the central carbon atom?
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11. Bonding & Molecular Structure
Lewis Dot Structures: Neutral Compounds
Multiple Choice
Which of the following is the correct Lewis dot structure for OF2 (oxygen difluoride)?
A
O atom in the center with double bonds to each F atom; O has one lone pair, each F has two lone pairs.
B
F atom in the center with single bonds to two O atoms; F has three lone pairs, each O has two lone pairs.
C
O atom in the center with two single bonds to F atoms; O has two lone pairs, each F has three lone pairs.
D
O atom in the center with single bonds to F atoms; O has three lone pairs, each F has two lone pairs.
Verified step by step guidance1
Step 1: Determine the total number of valence electrons for OF2. Oxygen (O) has 6 valence electrons, and each fluorine (F) has 7 valence electrons. Since there are two fluorine atoms, total valence electrons = 6 + 2 \(\times\) 7 = 20 electrons.
Step 2: Identify the central atom. Oxygen is less electronegative than fluorine, so oxygen will be the central atom with the two fluorine atoms bonded to it.
Step 3: Draw single bonds between the central oxygen atom and each fluorine atom. Each single bond represents 2 electrons, so 2 bonds use 4 electrons out of the total 20.
Step 4: Distribute the remaining electrons as lone pairs to satisfy the octet rule. Start by completing the octets of the fluorine atoms first, then place any leftover electrons on the oxygen atom.
Step 5: Count the lone pairs on each atom after distribution. Oxygen should have two lone pairs (4 electrons), and each fluorine should have three lone pairs (6 electrons) to complete their octets.
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