Question

Chemistry question? Identify two ions that have the following ground-state electron configurations.

1. [Ar]

2. [Ar] 3`d^5`

3. [Kr] 5`s^2`4 `d^10`

Answer 1

1. `S^(2-), Cl^(-)`

2. `Fe^(+), V^(2-)`

3. `Ag^(-), In^(+)`

Explanation:

The third configuration needs a `4s^2` orbital before a 3d orbital, so I assumed that in my answer while keeping the same amount of electrons in the d shell.

For all of these ions, you're simply adding and subtracting electrons from atoms in order to achieve the same number of electrons as the configuration for each question. Since argon has 18 electrons, you need to list ions with 18 electrons. For example, sulfur has 16 in its natural state, so we need to add 2 (the 2- charge) in order to achieve the same electron configuration as Argon.

For the second question, we simply add 7 electrons to Argon (`4s^2 3d^5`) to get a total of 25. Then we follow the same process above.

For the third question, we do the same thing as the second question except with Krypton's electrons instead.