What is the oxidation state of chromium in [Cr(NH3)6]Cl3?

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Q: What is the oxidation state of chromium in [Cr(NH3)6]Cl3?

Solution: The complex is neutral, and the three chloride ions contribute -3 charge. Therefore, the oxidation state of Cr must be +3.

Steps: 7

Step 1: Identify the complex ion. The complex is [Cr(NH3)6]Cl3, which means it has a chromium ion surrounded by six ammonia (NH3) ligands.
Step 2: Determine the charge of the ligands. Ammonia (NH3) is a neutral ligand, so it does not contribute any charge.
Step 3: Identify the overall charge of the complex. The entire complex [Cr(NH3)6] must be neutral because it is balanced by the three chloride ions (Cl-).
Step 4: Calculate the total charge contributed by the chloride ions. Each chloride ion has a charge of -1, and there are three chloride ions, so they contribute a total of -3 charge.
Step 5: Set up the equation for the oxidation state of chromium. Let the oxidation state of chromium be x. Since the complex is neutral, we have: x (from Cr) + (-3) (from Cl) = 0.
Step 6: Solve the equation. Rearranging gives us x = +3.
Step 7: Conclude that the oxidation state of chromium in [Cr(NH3)6]Cl3 is +3.