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\begin{tabular}{|l|l|l|l|}
\hline
& & & \\
\hline
hypochlorite & [tex]$ClO ^{-}$[/tex] & phosphate & [tex]$PO _4{ }^{3-}$[/tex] \\
\hline
chlorate & [tex]$ClO _3^{-}$[/tex] & hydrogen phosphate & [tex]$HPO _4{ }^{2-}$[/tex] \\
\hline
perchlorate & [tex]$ClO _4^{-}$[/tex] & dihydrogen phosphate & [tex]$H _2 PO _4{ }^{-}$[/tex] \\
\hline
hydronium & [tex]$H _3 O ^{+}$[/tex] & sulfate & [tex]$SO _4{ }^{2-}$[/tex] \\
\hline
permanganate & [tex]$MnO _4^{-}$[/tex] & \begin{tabular}{l}
hydrogen sulfate \\
(bisulfate)
\end{tabular} & [tex]$HSO _4{ }^{-}$[/tex] \\
\hline
nitrate & [tex]$NO _3^{-}$[/tex] & sulfite & [tex]$SO _3{ }^{2-}$[/tex] \\
\hline
\end{tabular}

Type the correct answer in each box.

Chromium(III) sulfate is a transition metal compound containing the metal chromium and the polyatomic ion sulfate. The oxidation state of chromium in this compound is [tex]$\square$[/tex], and the chemical formula of the compound is [tex]$\square$[/tex].

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To determine the oxidation state of chromium and the chemical formula of chromium(III) sulfate, follow these steps:

1. Understanding the given information:
- Chromium(III) indicates that the oxidation state of chromium is +3.
- Sulfate is a polyatomic ion with the formula [tex]\( \text{SO}_4^{2-} \)[/tex].

2. Oxidation State of Chromium:
- The term "Chromium(III)" tells us that the oxidation state of chromium is +3. This is because the Roman numeral III suggests an oxidation state of +3.

3. Neutral Compound Formation:
- In order to form a neutral compound, the total positive charge must balance the total negative charge.
- Chromium has an oxidation state of +3, so each chromium ion contributes a +3 charge.
- Sulfate ([tex]\( \text{SO}_4^{2-} \)[/tex]) has a charge of -2.

4. Balancing the Charges:
- To balance the charges between chromium and sulfate:
- Two chromium ions (each +3) give a total charge of [tex]\( 2 \times (+3) = +6 \)[/tex].
- Three sulfate ions (each -2) give a total charge of [tex]\( 3 \times (-2) = -6 \)[/tex].

5. Writing the Chemical Formula:
- The formula needs to represent a neutral compound. Since the charges are balanced with two chromium ions and three sulfate ions, the chemical formula will be [tex]\( \text{Cr}_2(\text{SO}_4)_3 \)[/tex].

Therefore, the oxidation state of chromium in this compound is [tex]\( \boxed{3} \)[/tex], and the chemical formula of the compound is [tex]\( \boxed{\text{Cr}_2(\text{SO}_4)_3} \)[/tex].
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