Question

an electron in an atom is in the n=2 and l=1 quantum level. part 1 of 2 what are all of the possible values of l at n=2? l= □ □,□,... part 2 of 2 what are all of the possible values of ( m_l ) that it can have? ( m_l = ) □ □,□,...

Explanation:

Part 1 of 2

Step1: Recall quantum number rules

The azimuthal quantum number \( l \) can take integer values from \( 0 \) to \( n - 1 \), where \( n \) is the principal quantum number. Here, \( n = 2 \).

Step2: Calculate possible \( l \) values

For \( n = 2 \), \( l \) can be \( 0 \) (since \( 0\leq l < 2 \)) and \( 1 \) (since \( 1 < 2 \)). So the possible values of \( l \) are \( 0, 1 \).

Step1: Recall \( m_l \) rules

The magnetic quantum number \( m_l \) can take integer values from \( -l \) to \( +l \), including \( 0 \). Here, \( l = 1 \) (from the problem statement where the electron is in \( l = 1 \) for \( n = 2 \)).

Step2: Calculate possible \( m_l \) values

For \( l = 1 \), \( m_l \) can be \( -1 \), \( 0 \), and \( +1 \) (since \( -1\leq m_l\leq 1 \)).

Answer:

\( 0, 1 \)

Part 2 of 2