The energy of an electron of 2 py orbital is (a) Greater...

The energy of an electron of $2 p_{y}$ orbital is
(a) Greater than $2 p_{x}$ orbital
(b) Less than $2 p_{s}$ orbital
(c) Equal to $2 \mathrm{~s}$ orbital
(d) Same as that of $2 p_{x}$ and $2 p_{z}$ orbital

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Key Concepts

Electron Orbitals and Quantum Numbers

Electron orbitals are defined by a set of quantum numbers including the principal quantum number, which indicates the energy level, and the angular momentum quantum number, which gives the orbital shape. For example, 2p orbitals are characterized by the principal quantum number n=2 and the angular momentum quantum number l=1, with further specification by the magnetic quantum number which distinguishes the different spatial orientations of the orbitals.

Orbital Degeneracy

Orbital degeneracy is the occurrence when multiple electron orbitals possess the same energy level. In the case of 2p orbitals, despite having different orientations (such as 2p_x, 2p_y, and 2p_z), they have the same energy in an atom that does not experience external perturbations, thereby illustrating the degeneracy of these orbitals.

Energy Levels and Orbital Ordering

The arrangement of electron energy levels in atoms follows specific patterns where electrons fill lower energy orbitals before occupying higher ones. While different subshells (s, p, d, etc.) have characteristic energy tendencies influenced by electron shielding and penetration effects, within a particular subshell like the p orbitals the energy is the same across different orientations due to degeneracy.

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