Let's analyze the given electron configuration and deduce the necessary information step by step.
1. Identify the Chemical Symbol for the Ion:
The electron configuration given is [tex]\( [Kr] \, 5s^2 \, 4d^{10} \, 5p^1 \)[/tex].
To find the chemical symbol, we first recognize that the notation [tex]\( [Kr] \)[/tex] represents the noble gas krypton (Kr), which has 36 electrons. Following this, the additional electrons are distributed as [tex]\( 5s^2 \)[/tex] (2 electrons), [tex]\( 4d^{10} \)[/tex] (10 electrons), and [tex]\( 5p^1 \)[/tex] (1 electron).
Adding these up, we get:
[tex]\[
36 \text{ (electrons from Kr)} + 2 \text{ (from } 5s^2\text{)} + 10 \text{ (from } 4d^{10}\text{)} + 1 \text{ (from } 5p^1\text{)} = 49 \text{ electrons}
\][/tex]
The element with 49 electrons (in its neutral state) is indium (In). Therefore, the chemical symbol for the ion is In.
2. Count the Number of Electrons in the Ion:
The ion has a charge of +2, indicating it has lost 2 electrons compared to its neutral state (49 electrons). Therefore, the number of electrons in the ion is:
[tex]\[
49 \text{ (total electrons in neutral indium)} - 2 \text{ (electrons lost due to +2 charge)} = 47 \text{ electrons}
\][/tex]
3. Determine the Number of [tex]\(5p\)[/tex] Electrons in the Ion:
The [tex]\(5p^1\)[/tex] configuration indicates that, in its neutral state, there is 1 electron in the 5p orbital. Since the ion has a +2 charge but the given configuration remains [tex]\(5p^1\)[/tex], it means the number of [tex]\(5p\)[/tex] electrons remains unchanged even after ionization.
Thus, the number of [tex]\(5p\)[/tex] electrons in the ion is 1.
In summary, the detailed answers to the questions are:
1. Chemical Symbol for the Ion: In
2. Number of Electrons in the Ion: 47
3. Number of [tex]\(5p\)[/tex] Electrons in the Ion: 1
