For d orbitals, the azimuthal quantum number l = 2.

For l=2 (d orbital), m_l can take values from -l to +l, which are -2, -1, 0, 1, 2.

For a p orbital, l=1, so m_l can take values -1, 0, +1.

The spin quantum number (m_s) can take values of -1/2 and +1/2.

For a p orbital (l=1), m_l can take values -1, 0, +1.

For l=2 (d orbital), m_l can take values from -2 to +2, which are -2, -1, 0, 1, 2.

For l=1, m_l can take values -1, 0, 1, which gives 3 possible values.

The quantum numbers correspond to the 2s orbital, where l=0 indicates an s orbital.

The spin quantum number can be either +1/2 or -1/2, so both values are possible.

For l=1, the electron occupies a p orbital.

For l=1, the orbital is a p orbital.

For l=1, m_l can take values -1, 0, +1.

For l=0, m_l can only be 0.

For l=2, m_l can take values -2, -1, 0, 1, 2. Therefore, all of the options are valid.

For l=2, the orbital type is d.

The azimuthal quantum number l = 1 corresponds to p orbitals, which have a dumbbell shape.

The maximum number of electrons in a subshell is given by 2(2l + 1). For l = 2, it is 2(2*2 + 1) = 10.

For n=4, l can take values 0, 1, 2, or 3.

For n=4, l can take values from 0 to n-1, which are 0, 1, 2, and 3.

The 3s orbital has the highest principal quantum number (n=3), indicating it has the highest energy.

The maximum number of electrons in a shell is given by 2n^2. For n=5, it is 2(5^2) = 50.

The maximum number of electrons in a shell is given by 2n^2. For n=4, it is 2(4^2) = 32.

The maximum number of electrons in a shell is given by 2n^2. For n=3, it is 2(3^2) = 18.

The maximum number of electrons in a subshell is given by the formula 2(2l + 1). For l = 2, it is 2(2*2 + 1) = 10.

The maximum number of electrons in a shell is given by 2n^2. For n=2, this is 2(2^2) = 8.

The maximum number of electrons in a shell is given by 2n^2. For n=5, it is 2(5^2) = 50.

A single orbital can hold a maximum of 2 electrons, with opposite spins.

The maximum number of electrons in a subshell is given by the formula 2(2l + 1). For l=2, this gives 2(2*2 + 1) = 10.

The maximum number of electrons in a subshell is given by the formula 2(2l + 1). For l = 2, this gives 2(2*2 + 1) = 10.

For l=1, the number of orbitals is given by 2l + 1 = 3.