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\begin{tabular}{|l|l|l|l|}
\hline
\multicolumn{1}{|c|}{Chemical Name} & \multicolumn{1}{|c|}{Chemical Formula} & \multicolumn{1}{|c|}{Chemical Name} & \multicolumn{1}{|c|}{Chemical Formula} \\
\hline
acetate & [tex]$C_2H_3O_2^{-}$[/tex] & nitrite & [tex]$NO_2^{-}$[/tex] \\
\hline
carbonate & [tex]$CO_3^{2-}$[/tex] & ammonium & [tex]$NH_4^{+}$[/tex] \\
\hline
hypocarbonite & [tex]$CO^{2-}$[/tex] & cyanide & [tex]$CN^{-}$[/tex] \\
\hline
\begin{tabular}{l}
hydrogen carbonate \\
(bicarbonate)
\end{tabular} & [tex]$HCO_3^{-}$[/tex] & hydroxide & [tex]$OH^{-}$[/tex] \\
\hline
chlorite & [tex]$ClO_2^{-}$[/tex] & peroxide & [tex]$O_2^{2-}$[/tex] \\
\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]$H_2PO_4^{-}$[/tex] \\
\hline
hydronium & [tex]$H_3O^{+}$[/tex] & sulfate & [tex]$SO_4^{2-}$[/tex] \\
\hline
\end{tabular}

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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].

Sagot :

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To determine the oxidation state of chromium in chromium(III) sulfate and its chemical formula, let's analyze the details step-by-step:

1. Identify the Polyatomic Ion and Its Charge:
- The sulfate ion ([tex]\( \text{SO}_4^{2-} \)[/tex]) has a charge of -2.

2. Given Data about Chromium:
- Chromium(III) indicates that each chromium ion has a charge of [tex]\(+3\)[/tex].

3. Balancing the Charges:
- We need to balance the overall charge of the compound to be neutral.
- Since we have three sulfate ions (each with a charge of -2), the total negative charge is [tex]\( 3 \times (-2) = -6 \)[/tex].

4. Calculate the Number of Chromium Ions:
- To balance the total charge of -6 from the sulfate ions, we need a total positive charge of +6 from chromium ions.
- Given that each chromium ion has a charge of [tex]\(+3\)[/tex], we need [tex]\( \frac{+6}{+3} = 2 \)[/tex] chromium ions.

5. Chemical Formula:
- Thus, with 2 chromium ions ([tex]\( \text{Cr}^{3+} \)[/tex]) and 3 sulfate ions ([tex]\( \text{SO}_4^{2-} \)[/tex]), the chemical formula is [tex]\( \text{Cr}_2(\text{SO}_4)_3 \)[/tex].

6. Oxidation State of Chromium:
- Each chromium ion in this compound has an oxidation state of [tex]\( +3 \)[/tex].

Thus, the oxidation state of chromium in chromium(III) sulfate 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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