Question

give the chemical symbol for the element with the ground - state electron configuration ne3s²3p². symbol: si determine the quantum numbers n and ℓ and select all possible values for m_ℓ for each subshell of the element. 3s n = 3 3s ℓ = 0 the possible values of m_ℓ for the 3s subshell are 0 - 3, - 2, - 1,0,+1,+2,+3 - 1,0,+1 - 2, - 1,0,+1,+2 3p n = 3p ℓ = the possible values of m_ℓ for the 3p subshell are 0 - 2, - 1,0,+1,+2 - 1,0,+1 - 3, - 2, - 1,0,+1,+2,+3

Explanation:

Step1: Determine \(n\) for \(3p\)

The principal quantum number \(n\) is related to the shell. For \(3p\), the shell number is \(3\), so \(n = 3\).

Step2: Determine \(\ell\) for \(3p\)

The angular - momentum quantum number \(\ell\) has values based on the sub - shell. For \(s\)-subshell \(\ell=0\), for \(p\)-subshell \(\ell = 1\), for \(d\)-subshell \(\ell=2\), and for \(f\)-subshell \(\ell = 3\). Since it is \(p\)-subshell, \(\ell=1\).

Step3: Determine \(m_{\ell}\) for \(3p\)

The magnetic quantum number \(m_{\ell}\) has values from \(-\ell\) to \(+\ell\). Given \(\ell = 1\), then \(m_{\ell}=-1,0, + 1\)

Answer:

For \(3p\):

• \(n = 3\)
• \(\ell=1\)
• The possible values of \(m_{\ell}\) for the \(3p\) subshell are \(-1,0,+1\)