Question

question 13 (1 point)
how many orbitals exist in the n = 2 energy level?
1
4
8
10
12

Explanation:

Step1: Determine the possible values of \( l \)

For a given principal quantum number \( n \), the angular momentum quantum number \( l \) can take values from \( 0 \) to \( n - 1 \). When \( n=2 \), \( l = 0,1 \).

Step2: Determine the number of orbitals for each \( l \)

• When \( l = 0 \) (s - orbital), the magnetic quantum number \( m_l=0 \). So, there is \( 1 \) orbital (\( 2s \)).
• When \( l = 1 \) (p - orbitals), \( m_l=- 1,0,1 \). So, there are \( 3 \) orbitals (\( 2p_x,2p_y,2p_z \)).

Step3: Calculate the total number of orbitals

The total number of orbitals in \( n = 2 \) energy level is \( 1+3=4 \).

Answer:

4