Question

1. use the periodic table to choose the best answers to find the electron configuration for silicon. which two sublevels does silicon have? p s f d 7. use the periodic table to choose the best answer to find the electron configuration for silicon. what is the electron configuration for silicon? 1s²2s²2p⁸3s²3p² 1s²2s²2p⁶3s²3p² 1s²2s²2p⁶3s²3p⁴4s² 1s²2s²2p⁶

Explanation:

• Question 6: Silicon (\(Si\)) has atomic number \(14\). The electron configuration of \(Si\) is \(1s^{2}2s^{2}2p^{6}3s^{2}3p^{2}\). The sublevels present are \(s\) (in \(1s\), \(2s\), \(3s\)) and \(p\) (in \(2p\), \(3p\)). The \(f\) - sublevel starts to fill from lanthanides (\(n = 4\) for \(4f\)) and \(d\) - sublevel starts to fill from transition metals (\(n=3\) for \(3d\), but \(3d\) is filled after \(4s\) and \(Si\) does not have electrons in \(d\) or \(f\) sublevels).
• Question 7:
• The maximum number of electrons in a \(p\) - sublevel is \(6\). The option \(1s^{2}2s^{2}2p^{8}3s^{2}3p^{2}\) is incorrect because \(2p\) cannot hold \(8\) electrons.
• For \(Si\) (\(Z = 14\)), we fill electrons in the order \(1s<2s < 2p<3s<3p\). \(1s^{2}2s^{2}2p^{6}3s^{2}3p^{2}\) has \(2 + 2+6 + 2+2=14\) electrons.
• The option \(1s^{2}2s^{2}2p^{6}3s^{2}3p^{4}4s^{2}\) has \(2 + 2+6 + 2+4 + 2=18\) electrons (which is for \(Ar\)).
• The option \(1s^{2}2s^{2}2p^{6}\) has \(2+2 + 6=10\) electrons (which is for \(Ne\)).

Answer:

• Question 6: \(p\), \(s\)
• Question 7: \(1s^{2}2s^{2}2p^{6}3s^{2}3p^{2}\)