Question

question 11 (0.25 points) listen which of the following is a correct set of quantum numbers for an electron in a 2s orbital? a) $n = 2, l = 1, m_l = 0$ b) $n = 2, l = 0, m_l = +1$ c) $n = 2, l = 1, m_l = 1$ d) $n = 2, l = 0, m_l = -1$ e) $n = 2, l = 0, m_l = 0$

Explanation:

1. For a 2s orbital:

• The principal quantum number $n$ matches the shell number, so $n=2$.
• For an s orbital, the azimuthal quantum number $l=0$.
• When $l=0$, the magnetic quantum number $m_l$ can only be 0 (since $m_l$ ranges from $-l$ to $+l$).

1. Match these values to the given options.

Answer:

e) $n = 2, l = 0, m_l = 0$