The covalency of 'N' in `NH_(4)^(+)` ion is equal to number of

Options

A. covalent bonds
B. co-ordinate bonds
C. covalent bonds and co-ordinate bonds
D. valence electrons

Answer

To find the covalency of nitrogen in the \( NH_4^+ \) ion, we need to analyze the bonding and the number of bonds formed by nitrogen in this ion.

### Step-by-Step Solution:

1. **Identify the Valence Electrons of Nitrogen:**
- Nitrogen (N) is in Group 15 of the periodic table and has 5 valence electrons.

2. **Determine the Total Valence Electrons in \( NH_4^+ \):**
- In \( NH_4^+ \), nitrogen is bonded to 4 hydrogen atoms. Each hydrogen atom contributes 1 electron.
- Therefore, the total number of valence electrons contributed by hydrogen is \( 4 \times 1 = 4 \).
- Since the ion has a positive charge (+1), we subtract 1 electron from the total count.
- Total valence electrons = \( 5 \) (from N) + \( 4 \) (from H) - \( 1 \) (due to +1 charge) = \( 8 \) electrons.

3. **Draw the Lewis Structure of \( NH_4^+ \):**
- In the Lewis structure, nitrogen is at the center with four hydrogen atoms surrounding it.
- Nitrogen will form 4 bonds with the hydrogen atoms, utilizing all of its valence electrons.

4. **Identify the Types of Bonds:**
- Each bond between nitrogen and hydrogen is a sigma bond (covalent bond).
- In this case, there are no lone pairs on nitrogen in \( NH_4^+ \).

5. **Count the Number of Bonds:**
- Nitrogen forms 4 sigma bonds with the 4 hydrogen atoms.
- Therefore, the covalency of nitrogen in \( NH_4^+ \) is equal to the number of bonds it forms, which is 4.

### Final Answer:
The covalency of nitrogen in \( NH_4^+ \) ion is equal to 4.

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