What is the oxidation state of chromium in the complex [Cr(NH3)4Cl2]+?
Practice Questions
Q1
What is the oxidation state of chromium in the complex [Cr(NH3)4Cl2]+?
+2
+3
+4
+6
Questions & Step-by-Step Solutions
What is the oxidation state of chromium in the complex [Cr(NH3)4Cl2]+?
Step 1: Identify the overall charge of the complex ion. The complex [Cr(NH3)4Cl2]+ has a charge of +1.
Step 2: Identify the charges of the ligands. Ammonia (NH3) is a neutral ligand, so it has a charge of 0. Each chloride ion (Cl) has a charge of -1.
Step 3: Calculate the total charge contributed by the ligands. There are 4 NH3 ligands (4 x 0 = 0) and 2 Cl ligands (2 x -1 = -2). So, the total charge from the ligands is 0 - 2 = -2.
Step 4: Set up the equation for the oxidation state of chromium (Cr). Let the oxidation state of Cr be x. The equation is: x + total charge from ligands = overall charge of the complex. This gives us: x - 2 = +1.
Step 5: Solve for x. Rearranging the equation gives us: x = +1 + 2, which simplifies to x = +3.
Step 6: Conclude that the oxidation state of chromium in the complex [Cr(NH3)4Cl2]+ is +3.
