What do you think about (C-H) bonds of `CH_4` molecule?
I)They are equivalent.
II) They have equal bond energy.
Choose the correct option.

Options

A. Only I
B. Only II
C. I and II
D. None of these

Answer

To analyze the (C-H) bonds in the `CH_4` molecule, we can follow these steps:

### Step 1: Understand the Structure of `CH_4`
The `CH_4` molecule, also known as methane, has a tetrahedral geometry. This is due to the arrangement of the four hydrogen atoms around the central carbon atom. The bond angles are approximately 109.5 degrees.

**Hint:** Consider the VSEPR theory to determine the molecular geometry.

### Step 2: Identify the Nature of the Bonds
In `CH_4`, the carbon atom forms four single covalent bonds with four hydrogen atoms. Each bond involves the sharing of one electron from carbon and one from hydrogen.

**Hint:** Recall that covalent bonds are formed by the sharing of electrons between atoms.

### Step 3: Determine the Equivalence of the Bonds
Since the `CH_4` molecule has a symmetrical tetrahedral structure and no lone pairs on the carbon atom, all four C-H bonds are equivalent. This means that they have the same length and strength.

**Hint:** Think about how symmetry affects bond characteristics in a molecule.

### Step 4: Assess Bond Energies
Because the C-H bonds are equivalent, they also have equal bond energies. This means that the energy required to break each C-H bond is the same.

**Hint:** Consider how bond strength is related to bond energy and the equivalence of bonds.

### Step 5: Evaluate the Given Statements
Now we can evaluate the two statements provided:
I) They are equivalent. - This is true.
II) They have equal bond energy. - This is also true.

**Hint:** Check if both statements align with your understanding of molecular structure and bonding.

### Conclusion
Both statements are correct, so the correct option is that both statements I and II are true.

**Final Answer:** The correct option is III (Both I and II are correct).