Multiple Choice
Which of the following best describes the Lewis dot structure for a neutral molecule of I2?
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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 XeF_4 (xenon tetrafluoride)?
A
Xe at the center with two F atoms bonded to it, and three lone pairs on Xe.
B
Xe at the center with four F atoms bonded to it, and no lone pairs on Xe.
C
Xe at the center with four F atoms bonded to it, and one lone pair on Xe.
D
Xe at the center with four F atoms bonded to it, and two lone pairs on Xe.
Verified step by step guidance1
Step 1: Determine the total number of valence electrons for XeF_4. Xenon (Xe) is in group 18 and has 8 valence electrons, and each fluorine (F) atom has 7 valence electrons. Since there are 4 fluorine atoms, calculate the total valence electrons as: \$8 + 4 \times 7$.
Step 2: Draw the skeletal structure with xenon (Xe) at the center and four fluorine (F) atoms bonded to it. Each Xe-F bond represents 2 electrons.
Step 3: Subtract the electrons used in bonding from the total valence electrons to find the remaining electrons. These remaining electrons will be placed as lone pairs on the atoms, starting with fluorine atoms to complete their octets.
Step 4: After completing the octets of the fluorine atoms, place any remaining electrons as lone pairs on the central xenon atom. Remember that xenon can have an expanded octet because it is in period 5.
Step 5: Count the lone pairs on xenon after placing all electrons. For XeF_4, xenon will have two lone pairs, which along with the four bonding pairs, gives the correct Lewis structure.
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