Maximum number of electrons in an orbital having n = 4 and l = 2 are :

Explanation

To find the maximum number of electrons in an orbital with quantum numbers n = 4 and l = 2, we can follow these steps:

### Step 1: Identify the Quantum Numbers
- The principal quantum number (n) is given as 4.
- The azimuthal quantum number (l) is given as 2.

### Step 2: Determine the Subshell
- The value of l corresponds to a specific subshell:
- l = 0 corresponds to s subshell
- l = 1 corresponds to p subshell
- l = 2 corresponds to d subshell
- Since l = 2, we are dealing with the d subshell.

### Step 3: Use the Formula to Calculate Maximum Electrons
- The maximum number of electrons that can occupy a subshell is given by the formula:
\[ \text{Maximum Electrons} = 2(2l + 1) \]
- Substitute the value of l into the formula:
\[ \text{Maximum Electrons} = 2(2 \times 2 + 1) \]

### Step 4: Perform the Calculation
- Calculate \(2l + 1\):
\[ 2l + 1 = 2 \times 2 + 1 = 4 + 1 = 5 \]
- Now substitute this back into the formula:
\[ \text{Maximum Electrons} = 2 \times 5 = 10 \]

### Conclusion
- The maximum number of electrons that can be accommodated in an orbital with n = 4 and l = 2 is **10**.

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