Textbook Question
Assume that the MOs of diatomics from the third row of the periodic table, such as P2, are analogous to those from the second row.
a. Which valence atomic orbitals of P are used to construct the MOs of P2?
12. Molecular Shapes & Valence Bond Theory
MO Theory: Homonuclear Diatomic Molecules
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Using a MO diagram, write the electron configuration for the P2 molecule
A
(σ2s)2(σ*2s)2(π2p)4(σ2p)2
B
(σ2s)2(σ*2s)2(π2p)2(σ2p)2(π*2p)2
C
(σ3s)2(σ*3s)2(π3p)4(σ3p)2
D
(σ3s)2(σ*3s)2(π3p)2(σ3p)2(π*3p)2
Verified step by step guidance1
Identify the atomic orbitals involved in the formation of the P2 molecule. Phosphorus (P) has an atomic number of 15, so its valence electrons are in the 3s and 3p orbitals.
Construct the molecular orbital (MO) diagram for P2. The MO diagram will include the following orbitals: σ3s, σ*3s, π3p, σ3p, and π*3p.
Fill the molecular orbitals with the total number of valence electrons from both phosphorus atoms. Each phosphorus atom contributes 5 valence electrons, so P2 has a total of 10 valence electrons.
Distribute the 10 valence electrons in the molecular orbitals according to the Aufbau principle, starting from the lowest energy orbital (σ3s) and moving to higher energy orbitals (σ*3s, π3p, σ3p, π*3p).
Write the electron configuration for the P2 molecule based on the filled molecular orbitals. Ensure that the configuration reflects the correct number of electrons in each orbital, considering the given options.
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