Question

1. what are the n and l values for the following orbitals?

a. 2p b. 4d c. 5f

Explanation:

Step1: Recall the rules for \(n\) and \(l\)

The principal quantum number \(n\) is the number in front of the orbital letter. The angular - momentum quantum number \(l\) has values \(l = 0,1,2,\cdots,n - 1\) and is related to the orbital type (\(s:l = 0\), \(p:l=1\), \(d:l = 2\), \(f:l=3\)).

Step2: Determine \(n\) and \(l\) for \(2p\)

For the \(2p\) orbital, the principal quantum number \(n = 2\) (the number in front of \(p\)). Since it is a \(p\) orbital, \(l = 1\).

Step3: Determine \(n\) and \(l\) for \(4d\)

For the \(4d\) orbital, the principal quantum number \(n = 4\) (the number in front of \(d\)). Since it is a \(d\) orbital, \(l = 2\).

Step4: Determine \(n\) and \(l\) for \(5f\)

For the \(5f\) orbital, the principal quantum number \(n = 5\) (the number in front of \(f\)). Since it is an \(f\) orbital, \(l = 3\).

Answer:

a. \(n = 2\), \(l = 1\)
b. \(n = 4\), \(l = 2\)
c. \(n = 5\), \(l = 3\)