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 \( n \), the possible values of the azimuthal quantum number \( l \) are \( l = 0,1,\cdots,n - 1 \). When \( n=2 \), \( l = 0\) and \( l = 1\).

Step2: Calculate 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: Sum up the number of orbitals

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

Answer:

4