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Which of the following atoms and ions is (are) isoelectronic with [tex][tex]$S^{2-}$[/tex][/tex]? Choose all that apply.

A. [tex]Si^{4+}[/tex]
B. [tex]Cl^{1-}[/tex]
C. [tex]Ar[/tex]
D. [tex]P^{3-}[/tex]
E. [tex]K^{+}[/tex]
F. [tex]Ca^{2+}[/tex]

Sagot :

GinnyAnswer
To determine which of the given atoms and ions are isoelectronic with [tex]\( S^{2+} \)[/tex], we need to understand that two species are isoelectronic if they have the same number of electrons.

- A neutral Sulfur (S) atom has an atomic number of 16, meaning it has 16 electrons.
- When sulfur loses 2 electrons to form [tex]\( S^{2+} \)[/tex], it will have [tex]\( 16 - 2 = 14 \)[/tex] electrons.

We now check the number of electrons for each of the given species:

(A) [tex]\( Si^{4+} \)[/tex]:
- A neutral Silicon (Si) atom has an atomic number of 14, so it has 14 electrons.
- When silicon loses 4 electrons to form [tex]\( Si^{4+} \)[/tex], it will have [tex]\( 14 - 4 = 10 \)[/tex] electrons.
- This is not isoelectronic with [tex]\( S^{2+} \)[/tex] (14 electrons).

(B) [tex]\( Cl^{3+} \)[/tex]:
- A neutral Chlorine (Cl) atom has an atomic number of 17, so it has 17 electrons.
- When chlorine loses 3 electrons to form [tex]\( Cl^{3+} \)[/tex], it will have [tex]\( 17 - 3 = 14 \)[/tex] electrons.
- This is isoelectronic with [tex]\( S^{2+} \)[/tex] (14 electrons).

(C) [tex]\( Ar \)[/tex]:
- A neutral Argon (Ar) atom has an atomic number of 18, so it has 18 electrons.
- This is not isoelectronic with [tex]\( S^{2+} \)[/tex] (14 electrons).

(D) [tex]\( As^{3+} \)[/tex]:
- A neutral Arsenic (As) atom has an atomic number of 33, so it has 33 electrons.
- When arsenic loses 3 electrons to form [tex]\( As^{3+} \)[/tex], it will have [tex]\( 33 - 3 = 30 \)[/tex] electrons.
- This is not isoelectronic with [tex]\( S^{2+} \)[/tex] (14 electrons).

(E) [tex]\( Si \)[/tex]:
- A neutral Silicon (Si) atom has an atomic number of 14, so it has 14 electrons.
- This is isoelectronic with [tex]\( S^{2+} \)[/tex] (14 electrons).

(F) [tex]\( Al^{3+} \)[/tex]:
- A neutral Aluminum (Al) atom has an atomic number of 13, so it has 13 electrons.
- When aluminum loses 3 electrons to form [tex]\( Al^{3+} \)[/tex], it will have [tex]\( 13 - 3 = 10 \)[/tex] electrons.
- This is not isoelectronic with [tex]\( S^{2+} \)[/tex] (14 electrons).

Therefore, the atoms and ions that are isoelectronic with [tex]\( S^{2+} \)[/tex] are:

- (B) [tex]\( Cl^{3+} \)[/tex]
- (E) [tex]\( Si \)[/tex]

Thus, the correct answer is:
(B) [tex]\( Cl^{3+} \)[/tex], (E) [tex]\( Si \)[/tex]
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