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\begin{tabular}{l|l|l}
\hline
chlorite & [tex]$ClO_2^{-}$[/tex] & peroxide \\
\hline
hypochlorite & [tex]$ClO^{-}$[/tex] & phosphate \\
\hline
\end{tabular}

Type the correct answer in each box.

What is the oxidation state of each element in the compound [tex]$CaSO_4$[/tex]? Include + or - in your answers as appropriate.

- The oxidation state of calcium is [tex]$\square$[/tex].
- The oxidation state of sulfur is [tex]$\square$[/tex].
- The oxidation state of oxygen is [tex]$\square$[/tex].



Answer :

GinnyAnswer
Alright, let's determine the oxidation states of each element in the compound [tex]\( \text{CaSO}_4 \)[/tex].

1. Oxidation state of Calcium (Ca):
Calcium is in Group 2 of the periodic table, and elements in this group typically have an oxidation state of +2.

The oxidation state of calcium is [tex]\( \boxed{+2} \)[/tex].

2. Oxidation state of Oxygen (O):
Oxygen typically has an oxidation state of -2 in most of its compounds.

The oxidation state of oxygen is [tex]\( \boxed{-2} \)[/tex].

3. Oxidation state of Sulfur (S):
The compound [tex]\( \text{CaSO}_4 \)[/tex] must be overall neutral. Therefore, the sum of the oxidation states of all the atoms in the compound must equal 0.

Given that:
- The oxidation state of calcium (Ca) is +2.
- The oxidation state of oxygen (O) is -2 and there are 4 oxygen atoms in the formula unit (4 atoms × -2 = -8).

Let [tex]\( x \)[/tex] be the oxidation state of sulfur (S). The charge balance equation is:
[tex]\[ +2 (Ca) + x (S) + 4(-2) (O) = 0 \][/tex]
Simplifying this equation:
[tex]\[ +2 + x - 8 = 0 \][/tex]
[tex]\[ x - 6 = 0 \][/tex]
[tex]\[ x = +6 \][/tex]

The oxidation state of sulfur is [tex]\( \boxed{+6} \)[/tex].

To summarize, the oxidation states in [tex]\( \text{CaSO}_4 \)[/tex] are:
- Calcium: [tex]\( \boxed{+2} \)[/tex]
- Sulfur: [tex]\( \boxed{+6} \)[/tex]
- Oxygen: [tex]\( \boxed{-2} \)[/tex]

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