How Many Orbitals In N=4

In chemistry and physics, the number of orbitals in an atom is determined by its principal quantum number, or "n-value". This number is assigned to each electron in an atom, and its value determines the shape of the orbital the electron inhabits.

The principal quantum number (n) of an atom dictates both the number of subshells, or energy levels, and the number of orbitals within each subshell. The number of orbitals in a subshell equals twice the n-value, as each n-value contains two orbitals of equal energy. For example, the 2s subshell of an atom with a n-value of 2 contains two orbitals (2 x 2 = 4).

In the case of a nitrogen atom, the value of n is 4, so there are eight (8) orbitals in its subshells. It has one 4s orbital, three 4p orbitals, and four 4d orbitals. The 4s orbital contains two electrons, while each of the other orbitals contains a maximum of six electrons.

This total of 8 orbitals in a n=4 atom can further be broken down into angular momentum states, each of which is split into two equal upright and two equal inverted orbitals. In the case of the n=4 atom, the angular momentum states available are 4s, 4p, 4d, and 4f. The 4s orbital is made up of one s s-orbital and three p-orbitals, each of which is split into two orientations; so you have one 4s, three 4p, five 4d, and seven 4f orbitals.

In summary, there are eight orbitals in an atom when the principal quantum number, or "n-value" is 4. These orbitals can further be broken down into angular momentum states, each of which is split into two orientations.