Multiple Choice
Which of the following statements correctly describes the Lewis dot structure of the AsF5 molecule?
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11. Bonding & Molecular Structure
Lewis Dot Structures: Ions
Multiple Choice
Which of the following correctly represents the Lewis dot structure for the hypochlorite ion, ClO⁻?
A
Cl with two lone pairs, double bonded to O with two lone pairs, and a negative charge on Cl
B
Cl with three lone pairs, single bonded to O with three lone pairs, and a negative charge on O
C
Cl with two lone pairs, single bonded to O with three lone pairs, and a negative charge on Cl
D
Cl with three lone pairs, single bonded to O with two lone pairs, and a negative charge on Cl
Verified step by step guidance1
Step 1: Determine the total number of valence electrons for the hypochlorite ion (ClO⁻). Chlorine (Cl) has 7 valence electrons, oxygen (O) has 6 valence electrons, and the negative charge adds 1 extra electron. So, total valence electrons = 7 + 6 + 1 = 14 electrons.
Step 2: Draw a skeletal structure connecting Cl and O with a single bond initially, since hypochlorite is known to have a single bond between Cl and O.
Step 3: Distribute the remaining valence electrons as lone pairs to satisfy the octet rule for both atoms. Start by placing lone pairs on oxygen to complete its octet, then place remaining electrons on chlorine.
Step 4: Assign the negative charge to the atom that has the extra electron(s) after completing octets. Typically, the negative charge is placed on the more electronegative atom, which is oxygen in this case.
Step 5: Verify the Lewis structure by checking that the total number of electrons equals 14, both atoms have complete octets, and the formal charges are minimized, with the negative charge correctly placed on oxygen.
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