Q4E

Question

Use valence bond theory to explain the bonding in\({{\rm{F}}_2},{\rm{HF}}\), and\({\rm{ClBr}}\). Sketch the overlap of the atomic orbitals involved in the bonds.

Step-by-Step Solution

Verified

Answer

The sketch is given below:

1Step 1: Definition of Concept

Bonds are formed by the overlapped valence orbitals on different atoms, according to the Valence Bond Theory. The orbitals that overlap must be occupied one at a time.

It is generally used to describe bonding in organic molecules like \({{\rm{H}}_{\rm{2}}}{\rm{,\;}}{{\rm{F}}_{\rm{2}}}{\rm{,HCl,ClBr}}\)etc.

2Step 2: Sketch the overlap of the atomic orbitals involved in the bonds

\({{\rm{F}}_{\rm{2}}}\): The single \({\rm{F - F}}\) sigma bond form from the sidewise overlap of the 2 p orbital in \({\rm{F}}\)atom with the 2 p orbital of the other \({\rm{F}}\) atom.

\({\rm{HF}}\): The single H-F sigma bond form from the sidewise overlap of the 1 s orbital of H atom with the 2 p orbital of the other F atom.

ClBr: The single Cl-Br sigma bond is formed by the sidewise overlap of the Cl atom's 3 p orbital with the other Br atom's 4 p orbital.

Therefore, the sketch is given below:

Q3 E

Q5 E

Other exercises in this chapter

Q1E

Explain how \({\rm{\sigma }}\) and \({\rm{\pi }}\) bonds are similar and how they are different.

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Q3 E

Explain why bonds occur at specific average bond distances instead of the atoms approaching each other infinitely close.

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Q5 E

Use valence bond theory to explain the bonding in\({{\rm{O}}_{\rm{2}}}\). Sketch the overlap of the atomic orbitals involved in the bonds in \({{\rm{O}}_{\rm{2}

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Q6 E

How many \({\rm{\sigma }}\)and \({\rm{\pi }}\)bonds are present in the molecule HCN?

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