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 = 3s ℓ = 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

Explanation:

Step1: Determine the principal quantum number \(n\)

The principal quantum number \(n\) is related to the shell. For the \(3s\) subshell, \(n = 3\) as the number in front of the subshell label (\(s\)) represents the principal quantum number.

Step2: Determine the angular momentum quantum number \(\ell\)

The angular momentum quantum number \(\ell\) is related to the sub - shell type. For an \(s\) sub - shell, \(\ell=0\). The rule is: \(s\) sub - shell corresponds to \(\ell = 0\), \(p\) sub - shell to \(\ell=1\), \(d\) sub - shell to \(\ell = 2\), and \(f\) sub - shell to \(\ell=3\).

Step3: Determine the magnetic quantum number \(m_{\ell}\)

The magnetic quantum number \(m_{\ell}\) has values ranging from \(-\ell\) to \(+\ell\). Since \(\ell = 0\) for the \(s\) sub - shell, \(m_{\ell}=0\)

Answer:

For \(3s\):

• \(n = 3\)
• \(\ell=0\)
• \(m_{\ell}=0\)