If the largest value of`m_(1) `for an electron is `+ 3` in what type of subshell the electron may be present ?

Explanation

To solve the question, we need to determine the type of subshell in which an electron may be present, given that the largest value of the magnetic quantum number \( m_l \) is +3.

### Step-by-Step Solution:

1. **Understanding the Magnetic Quantum Number**:
- The magnetic quantum number \( m_l \) can take on integer values ranging from \(-l\) to \(+l\), where \( l \) is the azimuthal (or angular momentum) quantum number.

2. **Identifying the Value of \( l \)**:
- Given that the largest value of \( m_l \) is +3, we can deduce that:
\[ m_l = +3 \implies l \geq 3 \]
- The possible values of \( l \) are:
- \( l = 0 \) (s subshell)
- \( l = 1 \) (p subshell)
- \( l = 2 \) (d subshell)
- \( l = 3 \) (f subshell)
- \( l = 4 \) (g subshell), and so on.

3. **Determining the Subshell**:
- Since \( m_l \) can take values from \(-l\) to \(+l\), if \( l = 3 \), the values of \( m_l \) would be:
\[ m_l = -3, -2, -1, 0, +1, +2, +3 \]
- This gives a total of \( 2l + 1 = 2(3) + 1 = 7 \) possible values for \( m_l \), confirming that the maximum value of \( m_l \) is indeed +3.

4. **Conclusion**:
- The azimuthal quantum number \( l = 3 \) corresponds to the f subshell. Therefore, the electron with the largest \( m_l \) value of +3 must be present in the **f subshell**.

### Final Answer:
The electron may be present in the **f subshell**.