Question

determine the maximum number of electrons that can be found in each of the following subshells. part 1 of 4 5s subshell: part 2 of 4 6d subshell: part 3 of 4 7p subshell: part 4 of 4 4f subshell:

Explanation:

Step1: Recall the formula for the number of electrons in a subshell

The formula for the maximum number of electrons in a subshell is \(2(2l + 1)\), where \(l\) is the azimuthal quantum number. For \(s\) - subshell \(l = 0\), for \(p\) - subshell \(l=1\), for \(d\) - subshell \(l = 2\), for \(f\) - subshell \(l=3\)

Step2: Calculate for \(5s\) subshell

For \(s\) - subshell \(l = 0\). Using the formula \(2(2l + 1)\), we substitute \(l = 0\):

$$2(2\times0 + 1)=2\times1 = 2$$

Step3: Calculate for \(6d\) subshell

For \(d\) - subshell \(l = 2\). Substitute \(l = 2\) into the formula \(2(2l + 1)\):

$$2(2\times2+ 1)=2\times(4 + 1)=2\times5=10$$

Step4: Calculate for \(7p\) subshell

For \(p\) - subshell \(l = 1\). Substitute \(l = 1\) into the formula \(2(2l + 1)\):

$$2(2\times1+ 1)=2\times(2 + 1)=2\times3 = 6$$

Step5: Calculate for \(4f\) subshell

For \(f\) - subshell \(l = 3\). Substitute \(l = 3\) into the formula \(2(2l + 1)\):

$$2(2\times3+ 1)=2\times(6 + 1)=2\times7=14$$

Answer:

Part 1 of 4: \(2\)
Part 2 of 4: \(10\)
Part 3 of 4: \(6\)
Part 4 of 4: \(14\)