Question

in the ( n = 3 ) principal shell, there are __ subshells that are labeled as __
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2; ( s ) and ( p )
3; ( s ), ( p ), and ( d )
4; ( s ), ( p ), ( d ), and ( f )
3; ( s ), ( p ), and ( f )
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part b
which of the following is the correct electron configuration for oxygen? (oxygen has 8 electrons.)
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( 1 s ^ { 2 } 2 s ^ { 3 } 3 s ^ { 2 } 2 p ^ { 2 } )
( 1 s ^ { 1 } 2 s ^ { 4 } )

Explanation:

For the first question, the number of sub - shells in a principal shell with principal quantum number \(n\) is equal to \(n\). When \(n = 3\), the possible values of the azimuthal quantum number \(l\) are \(l=0,1,2\) which correspond to \(s\), \(p\), and \(d\) sub - shells respectively.
For the second question (assuming the correct options are \(1s^{2}2s^{2}2p^{4}\) which is not shown here, but based on electron - filling rules: electrons fill lower - energy orbitals first. The order of filling is \(1s<2s < 2p\). The \(1s\) orbital can hold 2 electrons, the \(2s\) orbital can hold 2 electrons, and the \(2p\) orbital (for oxygen with 8 electrons: \(2 + 2+4\))

Answer:

For the first question: 3; \(s\), \(p\), and \(d\)
For the second question (assuming the correct electron - configuration is \(1s^{2}2s^{2}2p^{4}\)): \(1s^{2}2s^{2}2p^{4}\)