Molecular Orbital Theory MCQs
Molecular Orbital Theory, proposed by R.S. Mulliken and F. Hund, describes the state of bonded electrons within a molecular orbital, represented as a linear combination of atomic orbitals (LCAO). These molecular orbitals are polycentric, meaning the electrons are influenced by multiple nuclei. A bonding molecular orbital is more stable than an antibonding molecular orbital. The stability of a molecule can be quantified by its bond order: a bond order of 1, 2, and 3 corresponds to single, double, and triple bonds respectively, while a bond order of zero or negative indicates an unstable molecule.
Find the diamagnetic species
(a) H2
(b) H2–
(c) He2+
(d) H2+
O-O bond length is minimum in
(a) O2–
(b) O2
(c) O2+
(d) O22-
Which among the following has the shortest C-C bond length?
(a) Ethene
(b) Ethane
(c) Benzene
(d) Ethyne
Which of the following pairs has the same bond order?
(a) O2+, NO+
(b) N2, O2
(c) O22-, B2
(d) NO, CO
When O2 changes to O2–, the electron goes to which of the orbitals?
(a) 𝜋 orbital
(b) 𝜎 orbital
(c) 𝜋* orbital
(d) 𝜎* orbital
The oxygen molecule is paramagnetic. It can be explained by
(a) Resonance
(b) Hybridisation
(c) Valence bond theory
(d) Molecular orbital theory
Find the molecule having the highest bond order
(a) O2+
(b) O2–
(c) O22-
(d) O2
Each P of P4O10 is attached to how many oxygen atoms?
(a) 3
(b) 2.5
(c) 2
(d) 4
Find the paramagnetic species
(a) CN–
(b) NO+
(c) CO
(d) O2–
Which of the following is not paramagnetic?
(a) CO
(b) N2+
(c) NO
(d) O2–
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