This chemistry question involves key chemical concepts and calculations. The detailed solution below walks through each step, from identifying the reaction type to computing the final answer.
ScanSolve AI Answer
Hey Dany, good to see you again. The overall charge of a complex ion is the net charge of the entire complex. It is the sum of the oxidation state of the central metal ion and the charges of all the ligands attached to it. For the complex ion [CrCl_2(H_2O)_4]^+, the overall charge is given as +1. This means that when you add up the charge of the chromium ion, the charges of the two chloride ligands, and the charges of the four water ligands, the total must equal +1. We used this in Step 2 to find the oxidation state of Chromium: Let x be the oxidation state of Cr. Each Cl^- ligand has a charge of -1. Each H_2O ligand has a charge of 0. The sum of these charges equals the overall charge of the complex: x + 2(-1) + 4(0) = +1 x - 2 = +1 x = +3 So, the central chromium ion has an oxidation state of +3. What's next? Send 'em! 📸