The principal quantum number n is not associated with electron spin; it describes the energy level.

The spin quantum number (m_s) does not affect the energy level of the electron.

The principal quantum number n, azimuthal quantum number l, and magnetic quantum number m_l do not describe the spin of an electron. The spin quantum number s does.

For a 3p electron, n=3 and l=1. The magnetic quantum number m_l can be -1, 0, or +1.

For a 4d orbital, n=4 and l=2. The m_l value can be -2, -1, 0, +1, +2.

For l=0, m_l can only be 0. Therefore, n=1, l=0, m_l=1 is not allowed.

For l=1, m_l can only be -1, 0, or +1. Therefore, m_l=2 is not possible.

Electrons have a negligible mass compared to protons and neutrons.

Electrons fill orbitals in order of increasing energy, and the 4s orbital is filled before the 3d orbital.

In the quantum mechanical model, electrons are described by wave functions, which give the probability of finding an electron in a certain region.

Isotopes have the same number of protons but different numbers of neutrons.

Both statements A and B are true regarding electron configurations.

The azimuthal quantum number (l) can have a value of 0, which corresponds to an s orbital.

The magnetic quantum number (m_l) describes the orientation of an orbital in space.

The azimuthal quantum number (l) determines the shape of the orbital.

The principal quantum number n determines the energy level of an electron in an atom.

The magnetic quantum number (m_l) determines the orientation of an orbital in space.

The magnetic quantum number (m_l) determines the orientation of an orbital.

The azimuthal quantum number (l) determines the shape of the orbital.

The magnetic quantum number (m_l) describes the orientation of an orbital in space.

The principal quantum number (n) cannot be negative; it must be a positive integer.