Question

Assign oxidation states to all of the atoms in each of the following: a. \(\mathrm{CrCl}_{3}\) b. \(\mathrm{K}_{2} \mathrm{CrO}_{4}\) c. \(\mathrm{K}_{2} \mathrm{Cr}_{2} \mathrm{O}_{7}\) d. \(\operatorname{Cr}\left(\mathrm{C}_{2} \mathrm{H}_{3} \mathrm{O}_{2}\right)_{2}\)

Short answer

In short, the oxidation states are as follows: a. CrCl3: Cr (+3), Cl (-1) b. K2CrO4: K (+1), Cr (+6), O (-2) c. K2Cr2O7: K (+1), Cr (+6), O (-2) d. Cr(C2H3O2)2: Cr (+2), C (+1), H (+1), O (-2)

Step-by-step solution

a. Assigning oxidation states for CrCl3

We know that the oxidation state of chlorine (Cl) in its compounds is -1 and the total charge on the compound is 0. Let x be the oxidation state of chromium (Cr). x + 3(-1) = 0 x = +3 Therefore, the oxidation states are: Cr (+3), and Cl (-1).

b. Assigning oxidation states for K2CrO4

We know the oxidation state of potassium (K) is +1, and oxygen (O) is -2. The total charge on the compound is 0. Let x be the oxidation state of chromium (Cr). 2(+1) + x + 4(-2) = 0 x = +6 Therefore, the oxidation states are: K (+1), Cr (+6), and O (-2).

c. Assigning oxidation states for K2Cr2O7

We know the oxidation state of potassium (K) is +1, and oxygen (O) is -2. The total charge on the compound is 0. Let x be the oxidation state of each chromium (Cr). 2(+1) + 2(x) + 7(-2) = 0 x = +6 Therefore, the oxidation states are: K (+1), Cr (+6), and O (-2).

d. Assigning oxidation states for Cr(C2H3O2)2

First, we need to assign oxidation states of each atom in the acetate ion (C2H3O2). We know that the oxidation state of hydrogen (H) is +1 and oxygen (O) is -2. Let x be the oxidation state of carbon (C). 2(x) + 3(+1) + 2(-2) = -1 (charge on acetate ion) x = +1 Now, let y be the oxidation state of chromium (Cr). y + 2(-1) (charge of two acetate ions) = 0 y = +2 Therefore, the oxidation states are: Cr (+2), C (+1), H (+1), and O (-2).