Question

What is degeneracy as opposed to a degenerate state? How can we know what orbitals are higher in energy?

Answer 1

Hint: Degenerate orbitals are electron orbitals with the same energy levels. Lower energy levels are filled before higher energy levels, according to the Aufbau principle. Degenerate orbitals are filled uniformly before electrons are filled into higher energy levels, according to Hund's rule.

Complete answer:
A degenerate state is defined as a state in which the energy is the same as other states.
Atomic orbitals that share the same principal quantum number $n$ and angular momentum quantum number $l$, but not ${m_l}$ are necessarily degenerate. They are called degenerate states.
Degeneracy is the total number of different states of the same energy. The degree of degeneracy is another name for it. The degree degeneracy of $p$ orbitals is $3$ . The degree degeneracy of $d$ orbitals is $5$ .The degree degeneracy of $f$ orbitals is $7$.
Because it does not have to face nuclear force, the orbital that is far from the nucleus has the maximum energy, while the orbital that is close to the nucleus has the lowest. The energy of electrons in $3p$ will be the highest. Electrons in $3p$ will be the most energetic.

Note:
Degenerate orbitals are those that have the same energy. Subshell orbitals are no longer degenerate when chemical bonds are formed. The electrons in the same orbital do not degenerate when a magnetic field is applied.