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Chapter 3: Problem 93

How do you convert a neutral sulfur atom to an anion carrying a charge of \(2-?\)

Short Answer

Expert verified
To convert a neutral sulfur atom to an anion carrying a 2- charge, add 2 electrons to the atom. A neutral sulfur atom has 16 electrons, so after adding 2 electrons, the anion will have 18 electrons and be represented as \(S^{2-}\).

Step by step solution

01

Determine the number of electrons in a neutral sulfur atom

A neutral sulfur atom has an equal number of protons and electrons. To determine the number of electrons, we first need to know the atomic number of sulfur, which can be found in the periodic table. The atomic number of sulfur is 16, which means it has 16 protons and 16 electrons.
02

Determine the number of electrons required for a 2- charge

An anion with a 2- charge means that the atom has 2 extra electrons. In order to create a sulfur anion with a 2- charge, we need to add 2 electrons to the neutral sulfur atom.
03

Calculate the total number of electrons in the sulfur anion

We know that a neutral sulfur atom has 16 electrons, and we need to add 2 electrons to achieve a 2- charge. Therefore, the total number of electrons in the sulfur anion will be: \(16 + 2 = 18\)
04

Express the sulfur anion with its charge

The sulfur anion has a total of 18 electrons and carries a 2- charge. We can represent this anion and its charge as: \(S^{2-}\). In conclusion, to convert a neutral sulfur atom to an anion carrying a 2- charge, we need to add 2 electrons, resulting in a sulfur anion with 18 electrons, represented as \(S^{2-}\).

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Most popular questions from this chapter

Fill in the following table: $$ \begin{array}{lcccc} & { }_{8}^{15} \mathrm{O}^{+} & ? & ? & ? \\ \hline \text { Mass number } & ? & 27 & ? & 58 \\ \text { Atomic number } & ? & ? & 15 & ? \\ \text { Number of protons } & ? & 13 & ? & ? \\ \text { Number of neutrons } & ? & ? & 16 & 30 \\ \text { Number of electrons } & ? & ? & ? & 27 \\ \text { Charge on ion } & ? & +3 & -3 & +1 \\ \hline \end{array} $$

The element nitrogen has only two naturally occurring isotopes: \({ }^{14} \mathrm{~N}\) with a mass of \(14.00308\) amu and an abundance of \(99.635 \%\) and \({ }^{15} \mathrm{~N}\) with a mass of \(15.00011\) amu and an abundance of \(0.3650 \%\). Calculate the atomic mass of nitrogen.

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