Question

which of the following electron configurations is impossible? o 1p² o 2p² o 1s² o 2s² question 17 0.4 pts the highest energy level in a silver atom is o 5 o 4 o 3 o 6

Explanation:

Step1: Recall electron - shell rules

Electrons fill orbitals in a specific order. The first energy level ($n = 1$) has only an $s$ orbital ($1s$), and there is no $p$ orbital in the first energy level. The second energy level ($n=2$) has both $s$ ($2s$) and $p$ ($2p$) orbitals, the third energy level ($n = 3$) has $s$, $p$, and $d$ orbitals etc.

Step2: Analyze each option

• For $1p^{2}$: Since the first energy level ($n = 1$) has only the $1s$ orbital and no $p$ orbital, this electron - configuration is impossible.
• For $2p^{2}$: The second energy level can have a $2p$ orbital, and it can hold 2 electrons in the $2p$ sub - shell, so this is possible.
• For $1s^{2}$: The first energy level has a $1s$ orbital which can hold 2 electrons, so this is possible.
• For $2s^{2}$: The second energy level has a $2s$ orbital which can hold 2 electrons, so this is possible.

Step3: Recall silver's electron - configuration

The electron - configuration of silver ($Ag$, atomic number = 47) is $[Kr]4d^{10}5s^{1}$. The highest energy level occupied by electrons in a silver atom is $5$.

Answer:

1. The impossible electron - configuration is: $1p^{2}$
2. The highest energy level in a silver atom is: 5