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(A) The maximum number of electrons in an orbital subshell is given by the formula $2(2l + 1)$.For a $d$ orbital,the azimuthal quantum number $l = 2$.

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$10$ and $14$

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(A) The maximum number of electrons in an orbital subshell is given by the formula $2(2l + 1)$.For a $d$ orbital,the azimuthal quantum number $l = 2$. Therefore,the maximum number of electrons is $2(2 	imes 2 + 1) = 2(5) = 10$.For an $f$ orbital,the azimuthal quantum number $l = 3$. Therefore,the maximum number of electrons is $2(2 	imes 3 + 1) = 2(7) = 14$.Thus,the maximum number of electrons in $d$ and $f$ orbitals are $10$ and $14$,respectively.

What is the maximum number of electrons that can be accommodated in $d$ and $f$ orbitals,respectively?

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