Maximum covalency of nitrogen is :

Options

A. 3
B. 5
C. 4
D. 6

Answer

To determine the maximum covalency of nitrogen, we need to analyze its electronic configuration and bonding capabilities. Here’s a step-by-step solution:

### Step 1: Understand the Electronic Configuration of Nitrogen
- Nitrogen (N) has an atomic number of 7.
- Its electronic configuration is 1s² 2s² 2p³.
- This means nitrogen has a total of 5 valence electrons (2 from 2s and 3 from 2p).

**Hint:** Remember that the number of valence electrons determines how many bonds an atom can typically form.

### Step 2: Determine the Maximum Number of Bonds
- In general, covalency refers to the number of covalent bonds an atom can form.
- Nitrogen can form bonds by sharing its valence electrons with other atoms.
- It can form single bonds, double bonds, and in some cases, triple bonds.

**Hint:** Think about how nitrogen can share its electrons with other atoms to form different types of bonds.

### Step 3: Analyze Bonding in Nitrogen Compounds
- In compounds like ammonia (NH₃), nitrogen forms three single bonds with hydrogen.
- In nitrate (NO₃⁻), nitrogen forms one double bond with oxygen and two single bonds with two other oxygen atoms, totaling four bonds.

**Hint:** Consider common nitrogen compounds to see how many bonds nitrogen forms in each case.

### Step 4: Consider the Limitations of Nitrogen
- Nitrogen does not have d-orbitals available for bonding since it is a second-period element.
- Therefore, it cannot expand its octet beyond 8 electrons, which limits its maximum covalency.

**Hint:** Recall that only elements in the third period and beyond can utilize d-orbitals to expand their octet.

### Step 5: Conclusion
- Based on the analysis, nitrogen can form a maximum of four covalent bonds.
- Thus, the maximum covalency of nitrogen is **4**.

**Final Answer:** The maximum covalency of nitrogen is **4**.