Bond energies can be obtained by using the following relation: `DeltaH (reaction) = sum`Bond energy of bonds, broken in the reactants `-sum` Bond energy fo bonds, formed in the products
Bond enegry depends on three factors:
a. Greater is the bond length, lesser is the bond enegry.
b. Bond energy increases with the bond multiplicity.
c. Bond enegry increases with electronegativity difference between the bonding atoms.
In `CH_(4)` molecule, which of the following statement is correct about the `C -H` bond enegry?

Options

A. All `C-H` bonds of methane have same enegry.
B. Average of all `C -H` bond energies is considered.
C. Fourth `C -H` bond required highest enegry to break.
D. None of the above

Explanation

To determine the correct statement about the C-H bond energy in the CH₄ molecule, we can follow these steps:

### Step 1: Understand the structure of CH₄
- The CH₄ molecule (methane) has a tetrahedral structure. This means that the carbon atom is at the center, and the four hydrogen atoms are at the corners of a tetrahedron.

### Step 2: Analyze the bonds in CH₄
- In CH₄, there are four C-H bonds. Each bond is formed between a carbon atom and a hydrogen atom.

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