Bond Order and Magnetism Analysis for CS2 Molecule

What is the bond order for the molecule CS2 and would it be paramagnetic or diamagnetic?

Choose the correct option:

A. Diamagnetic

B. Paramagnetic

Answer:

The molecule CS2 is diamagnetic due to all electrons being paired in molecular orbitals. Bond order is greater than zero indicating stability, but an exact number would require a molecular orbital diagram.

Predicting the bond order for the molecule CS2 and whether it would be paramagnetic or diamagnetic involves understanding molecular orbital (MO) theory. Due to the configuration of electrons in carbon (C) and sulfur (S), the electrons are paired in the MO diagram for CS2. This results from the combination of atomic orbitals from carbon and sulfur to form molecular orbitals in which all the electrons are paired. Thus, having no unpaired electrons suggests that CS2 would be diamagnetic. As for the bond order, a qualitative MO diagram would need to be considered for CS2, but the bond order can be expected to be greater than zero as it is a stable molecule observed in the gas phase at high temperatures.

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