Question

The oxidation state of chromium in ($K_2Cr_2O_7$) is:

• A. +4
• B. +5
• C. +6
• D. +7

Hint:

Chromium in the $+6$ state is a very strong oxidizing agent. This is why $K_2Cr_2O_7$ is commonly used in laboratories for titration and organic oxidation reactions.

Answer 1

The Correct Option is C

Step 1: Understanding the Concept:
The oxidation state is the hypothetical charge an atom would have if all bonds to atoms of different elements were 100% ionic. The sum of oxidation states in a neutral compound must be zero.

Step 2: Identifying Known Oxidation States:
In $K_2Cr_2O_7$:
• Potassium ($K$) is an alkali metal, so its state is $+1$.
• Oxygen ($O$) is usually $-2$.
• Let the oxidation state of Chromium ($Cr$) be $x$.

Step 3: Calculation:
Set up the equation for the neutral molecule: \[ 2(+1) + 2(x) + 7(-2) = 0 \] \[ 2 + 2x - 14 = 0 \] \[ 2x - 12 = 0 \] \[ 2x = 12 \implies x = +6 \]

Step 4: Final Answer:
The oxidation state of Chromium in Potassium Dichromate is +6.