Question

what are the values of m when l = 2 and how many orbitals are there? -2, -1, 0, 1, 2 and there are 5 orbitals -1, 0, 1 and there are 3 orbitals -2, -1, 0, 1, 2 and there are 2 orbitals -1, 0, 1 and there are 2 orbitals

Explanation:

Step1: Recall the formula for \(m_l\)

The magnetic quantum number \(m_l\) has values from \(-l\) to \(+l\) including \(0\). Given \(l = 2\), then \(m_l=-2,-1,0,1,2\).

Step2: Calculate the number of orbitals

The number of orbitals for a given \(l\) is \(2l + 1\). Substituting \(l = 2\), we get \(2\times2+1=5\).

Answer:

-2, -1, 0, 1, 2 and there are 5 orbitals