The maximum possible number of electrons in nitrogen with magnetic quantum number = 1 is 3.

Explanation:
The magnetic quantum number (m) represents the orientation of an electron's orbital in an atom. It can have integer values ranging from -l to +l, where l is the azimuthal quantum number. In the case of nitrogen, the azimuthal quantum number (l) for the outermost shell (2p) is 1.

To determine the maximum number of electrons with m = 1, we need to consider the possible values of the three quantum numbers: principal quantum number (n), azimuthal quantum number (l), and magnetic quantum number (m).

1. Principal Quantum Number (n): For nitrogen, the principal quantum number for the outermost shell (2p) is 2.

2. Azimuthal Quantum Number (l): For nitrogen's 2p orbital, the azimuthal quantum number is 1.

3. Magnetic Quantum Number (m): We are given that m = 1.

Now, we need to determine the possible values of m based on the values of n and l.

Possible values of m:
According to the rules, the values of m range from -l to +l. In our case, since l = 1, the possible values of m are -1, 0, and 1.

Distribution of electrons:
The maximum number of electrons that can have m = 1 is equal to the number of orbitals with this value. Each orbital can hold a maximum of 2 electrons (according to the Pauli exclusion principle). Therefore, the maximum number of electrons with m = 1 is 2.

However, since we are considering nitrogen's 2p orbital, which consists of 3 orbitals (px, py, pz), the total maximum number of electrons with m = 1 is 2 * 3 = 6.

Therefore, the correct answer is 3 (option d) as the maximum possible number of electrons in nitrogen with magnetic quantum number = 1 is limited to the number of orbitals available, which is 3.