Question

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 \boxed{ }, and the chemical formula of the compound is \boxed{ } \boxed{ } (\boxed{ } \boxed{ }) \boxed{ }

Explanation:

Step1: Determine Chromium's Oxidation State

The Roman numeral (III) in Chromium(III) sulfate indicates the oxidation state of chromium. So chromium has an oxidation state of +3.

Step2: Recall Sulfate Ion Formula and Charge

The sulfate ion is $\ce{SO_4^{2-}}$, with a charge of -2.

Step3: Determine Chemical Formula

To form a neutral compound, we balance the charges. Let the formula be $\ce{Cr_x(SO_4)_y}$. The charge from Cr is $x\times(+3)$ and from sulfate is $y\times(-2)$. For neutrality, $3x = 2y$. The smallest integers satisfying this are $x = 2$ and $y = 3$. So the formula is $\ce{Cr_2(SO_4)_3}$.

Answer:

The oxidation state of chromium is $\boldsymbol{+3}$, and the chemical formula is $\boldsymbol{\ce{Cr_2(SO_4)_3}}$ (filling the boxes as: first box: 3; then the formula boxes: Cr, 2, (, SO₄, ), 3).