type in the maximum number of electrons that can be present in each shell or subshell below.\n$n = 5$…

Explanation:

Step1: Recall electron - shell formula

The maximum number of electrons in a shell with principal quantum number $n$ is given by $2n^{2}$.

Step2: Calculate for $n = 5$ shell

Using the formula $2n^{2}$, when $n = 5$, we have $2\times5^{2}=2\times25 = 50$.

Step3: Calculate for $n = 2$ shell

Using the formula $2n^{2}$, when $n = 2$, we have $2\times2^{2}=2\times4 = 8$.

Step4: Recall sub - shell electron capacity

For a sub - shell with angular momentum quantum number $l$, the number of orbitals is $2l + 1$, and each orbital can hold 2 electrons. So the number of electrons in a sub - shell is $2(2l + 1)$.

Step5: Calculate for $n = 2,l = 0$ subshell

Since $l = 0$, the number of orbitals is $2\times0+1 = 1$. The number of electrons is $2\times1=2$.

Step6: Calculate for $n = 2,l = 1$ subshell

Since $l = 1$, the number of orbitals is $2\times1 + 1=3$. The number of electrons is $2\times3 = 6$.

Step7: Identify $l$ value for $d$ subshell

For a $d$ subshell, $l = 2$. The number of orbitals is $2\times2+1 = 5$. The number of electrons is $2\times5=10$.

Step8: Identify $l$ value for $s$ subshell

For an $s$ subshell, $l = 0$. The number of orbitals is $2\times0 + 1=1$. The number of electrons is $2\times1=2$.

Step9: Identify $l$ value for $f$ subshell

For an $f$ subshell, $l = 3$. The number of orbitals is $2\times3+1 = 7$. The number of electrons is $2\times7 = 14$.

Answer:

$n = 5$ shell: 50 $n = 2$ shell: 8 $n = 2,l = 0$ subshell: 2 $n = 2,l = 1$ subshell: 6 $3d$ subshell: 10 $2s$ subshell: 2 $5f$ subshell: 14