If an electron has spin quantum number of $+ \frac{1}{2}$ and a magnetic quantum number of – 1, it cannot be represented in an

s-orbital

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p-orbital

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d-orbtial

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f-orbital

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Solution

The correct option is A s-orbital
s orbital has one subshell which means it has only one magnetic quantum number possible. $l = 0$
m = – 1 is not possible for s-orbital

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\frac{1}{2}

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If an electron has spin quantum number of + 1/2 and a magnetic quantum number of -1, it cannot be represented in an

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+ 1 / 2

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