Maximum Number of Electrons in p-orbital with n=6;m=0

The electronic configuration of an atom is the distribution of electrons in its atomic orbitals. The p-orbital is one of the three types of orbitals - s, p, and d - that are present in the valence shell of an atom. The maximum number of electrons that can be present in a p-orbital with n=6 and m=0 is determined by the quantum numbers n, l, and m.

Quantum Numbers

The quantum numbers are used to describe the electronic configuration of an atom. There are four quantum numbers: n, l, m, and s.

- Principal Quantum Number (n) - It determines the size and energy of the orbital.
- Azimuthal Quantum Number (l) - It determines the shape of the orbital.
- Magnetic Quantum Number (m) - It determines the orientation of the orbital.
- Spin Quantum Number (s) - It determines the spin of the electron.

The p-orbital has l=1, which means it has three sub-orbitals: px, py, and pz. Each sub-orbital can hold a maximum of two electrons. The magnetic quantum number (m) can have values of -1, 0, or 1, which means there are three p-orbitals. The value of m=0 corresponds to the pz orbital.

Maximum Number of Electrons in p-orbital

The maximum number of electrons that can be present in a p-orbital is determined by the Pauli Exclusion Principle, which states that no two electrons in an atom can have the same set of four quantum numbers. Therefore, the maximum number of electrons that can be present in a p-orbital with n=6 and m=0 is 2.

Conclusion

The maximum number of electrons that can be present in a p-orbital with n=6 and m=0 is 2. This is because the pz sub-orbital has only one possible orientation, which means it can hold a maximum of two electrons with opposite spins.