To determine the types of orbitals found in the principal energy level \( n = 2 \), we need to consider the rules governing atomic orbitals.
1. Principal Quantum Number \( n \): The principal quantum number, \( n \), defines the energy level of the electron. For \( n = 2 \), this denotes the second energy level.
2. Orbital Types: The types of orbitals available in a given energy level are influenced by the azimuthal quantum number \( l \). The values of \( l \) range from \( 0 \) to \( n-1 \).
For \( n = 2 \):
- When \( l = 0 \), this corresponds to an \( s \)-orbital.
- When \( l = 1 \), this corresponds to a \( p \)-orbital.
Therefore, at the principal energy level \( n = 2 \), we have:
- \( s \)-orbitals (\( l = 0 \))
- \( p \)-orbitals (\( l = 1 \))
There are no \( d \)-orbitals (which would correspond to \( l = 2 \)) or \( f \)-orbitals (which would correspond to \( l = 3 \)) present at this energy level because these values are not within the range of \( l \) for \( n = 2 \).
Given the choices:
- A. \( s \)
- B. \( s, f \)
- C. \( s, d \)
- D. \( s, p \)
- E. \( s, p, d \)
The correct types of orbitals present in the principal energy level \( n = 2 \) are:
D. [tex]\( s, p \)[/tex]
