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How many protons, neutrons, and electrons are in this ion?

[tex]\[
\begin{array}{l}
^{33}_{16} \text{S}^{2-}
\end{array}
\][/tex]

A. \( 16 p^{+}, 17 n^{\circ}, 16 e^{-} \)

B. \( 33 p^{+}, 16 n^{\circ}, 35 e^{-} \)

C. \( 16 p^{+}, 17 n^{\circ}, 18 e^{-} \)

D. [tex]\( 16 p^{+}, 33 n^{\circ}, 16 e^{-} \)[/tex]



Answer :

GinnyAnswer
To determine the number of protons, neutrons, and electrons in the ion \( S^{2-} \) with an atomic number of 16 and a mass number of 33, follow these steps:

1. Identify the atomic number and mass number:
- The atomic number (\( Z \)) of sulfur (S) is 16. This means sulfur has 16 protons.
- The mass number (\( A \)) given in the notation \( \frac{33}{16} S \) is 33.

2. Determine the number of neutrons:
- The number of neutrons (\( n \)) is calculated by subtracting the atomic number from the mass number:
[tex]\[ n = A - Z = 33 - 16 = 17 \][/tex]
- Thus, there are 17 neutrons.

3. Determine the number of electrons for the neutral atom:
- In a neutral atom, the number of electrons is equal to the number of protons. Therefore, a neutral sulfur atom (\( S \)) has 16 electrons.

4. Adjust for the ion charge:
- The given ion is \( S^{2-} \), which indicates it has a 2- charge. This means the ion has gained 2 additional electrons compared to the neutral atom.
- Therefore, the number of electrons in \( S^{2-} \) is:
[tex]\[ \text{Electrons} = 16 + 2 = 18 \][/tex]

Given this information, the \( S^{2-} \) ion has:
- 16 protons
- 17 neutrons
- 18 electrons

Thus, the correct answer is:
[tex]\[ \boxed{16 p^{+}, 17 n^{\circ}, 18 e^{-}} \][/tex]

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