Final answer:
The oxidation state of chromium in the tetrahedral complex with a charge of -1 is +3, and the coordination number is 4, the oxidation state of the chromium is +3.
Step-by-step explanation:
To determine the oxidation state and coordination number of the chromium atom in a tetrahedral complex with Cl- that has an overall charge of -1, we must look at the charges of the ligands and the overall charge of the complex. Chloride ions (Cl-) have a charge of -1 each. Assuming the formula for this complex is [CrCl4]-, we have four chloride ions contributing a total of -4 in charge. Since the overall charge of the complex is -1, we can set up an equation to find the oxidation state of chromium (Cr).
Let x be the oxidation state of Cr, then x + 4(-1) = -1. Solving for x, we get x = +3. Therefore, the oxidation state of chromium in this complex is +3. The coordination number, which is the number of ligand atoms directly bonded to the central metal atom, is 4, since we have four chloride ligands bound to the chromium.
The coordination number for this chromium complex is 4, and the oxidation state of the chromium is +3.