The term 'degenerate' is used to describe atomic orbitals which:

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Consider the concept being tested: degeneracy of atomic orbitals.
Option a: "are equal in energy". This is the core idea of degeneracy in atomic orbitals—orbitals that share the same energy level are degenerate. When two or more orbitals have the same energy, electrons can occupy them without a difference in energy, hence degeneracy.
Option b: "have the same value for n". Having the same principal quantum number n does not guarantee degeneracy. Orbitals with the same n can have different energies depending on the subshell (l) and magnetic quantum number (m_l); for example, 2s and 2p orbitals do not share identical energies in many atoms. Therefore this statement is incorrect as a general rule.
Option c: "do not contain electrons". Degeneracy relates to energy levels and orbital shapes, not to whether an orbital is occupied. An orbital can be degenerate and still contain electrons or be empty, so this option is not an accurate definition of degeneracy.
Option d: "contain two electrons". The statement implies a fixed electron count per degenerate orbital, which is false. Degeneracy concerns energy equality among orbitals, not how many electrons they hold. Orbitals can be singly occupied, doubly occupied, or empty regardless of degeneracy.
In summary, the only option that correctly captures the intended meaning of degeneracy in atomic orbitals is that degenerate orbitals are those that are equal in energy, while the other options misstate or confuse the concept with occupancy, quantum numbers, or energy relationships.

CHM1051 MUM S2 2025 CHM1051 Practice Exam 2

The term 'degenerate' is used to describe atomic orbitals which:

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