 # Calculate the total number of electrons that can occupy a) zakinutuzi 2021-12-19 Answered
Calculate the total number of electrons that can occupy
a) one s orbital,
b) three p orbitals,
c) five d orbitals,
d) seven f orbitals.
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PART A:
The s subshell corresponds to the angular momentum quantum number $l=0$. For a given angular momentum quantum number l, there are a maximum total of $2\left(2l+1\right)$ electrons. Therefore, an subshell has a maximum total of $2\left[2\left(0\right)+1\right]=2$ electrons.
PART B:
The p subshell corresponds to the angular momentum quantum number $l=1$. For a given angular momentum quantum number l, there are a maximum total of $2\left(2l+1\right)$ electrons. Therefore, a p subshell has a maximum total of $2\left[2\left(1\right)+1\right]=6$ electrons.
PART C:
The d subshell corresponds to the angular momentum quantum number $l=2$. For a given angular momentum, quantum number l, there are a maximum total of $2\left(2l+1\right)$ electrons. Therefore, a d subshell has a maximum total of $2\left[2\left(2\right)+1\right]=10$ electrons.
PART D:
The f subshell corresponds to the angular momentum quantum number $l=3$. For a given angular momentum quantum number £, there are a maximum total of $2\left(2l+1\right)$ electrons. Therefore, an f subshell has a maximum, total of $2\left[2\left(3\right)+1\right]=14$ electrons.
###### Not exactly what you’re looking for? vicki331g8
So, electrons in the orbitals of a sub shell is given as follows, number of electrons $=2\left(2l+1\right)$
(a). for s orbital $l=0$,
Number of electrons $=2\left(2×0+1\right)$
=2 electrons
(b), Three p orbitals, $l=1$
number of electrons $=2\left(2×1+1\right)=6$ electrons
(c) five d orbitals, $l=2$
Number of electrons $=2\left(2×2+1\right)=10$ electrons
(d). seven f orbitals, $l=3$
Number of electrons $=2\left(2×3+1\right)=14$ electrons