Multiple Choice
Which of the following statements correctly describes the molecular orbital configuration of He₂²⁺?
12. Molecular Shapes & Valence Bond Theory
Molecular Orbital Theory
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Using molecular orbital theory, determine whether F2, F2−, or F22− would have the strongest bond.
A
F2
B
F2−
C
F22−
D
all have the same strength
E
cannot determine
Verified step by step guidance1
Identify the total number of electrons in each species: F2 has 14 electrons, F2⁻ has 15 electrons, and F2²⁻ has 16 electrons.
Construct the molecular orbital (MO) diagram for each species. For diatomic molecules like F2, the order of molecular orbitals is: σ(2s), σ*(2s), σ(2p), π(2p), π*(2p), σ*(2p).
Fill the molecular orbitals with the appropriate number of electrons for each species, following the Aufbau principle, Pauli exclusion principle, and Hund's rule.
Calculate the bond order for each species using the formula: Bond Order = (Number of bonding electrons - Number of antibonding electrons) / 2.
Compare the bond orders: The species with the highest bond order will have the strongest bond. Analyze the bond orders calculated for F2, F2⁻, and F2²⁻ to determine which has the strongest bond.
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