What is the oxidation state of chromium in K2Cr2O7? This is a common question in chemistry, especially when studying inorganic compounds. Potassium dichromate, K2Cr2O7, is a well-known compound with a variety of applications, including as an oxidizing agent in chemical reactions. Understanding the oxidation state of chromium in this compound is crucial for comprehending its chemical behavior and reactivity.
In K2Cr2O7, the oxidation state of potassium (K) is +1, as it is a Group 1 element. Oxygen (O) typically has an oxidation state of -2, as it is a Group 16 element. The overall charge of the K2Cr2O7 molecule is 0, meaning that the sum of the oxidation states of all the atoms must add up to zero. With this information, we can calculate the oxidation state of chromium (Cr) in the compound.
Let’s assume the oxidation state of Cr is x. Since there are two chromium atoms in K2Cr2O7, the total oxidation state for Cr is 2x. The oxidation state for oxygen is -2, and there are seven oxygen atoms in the compound, so the total oxidation state for oxygen is -14. The oxidation state for potassium is +1, and there are two potassium atoms, so the total oxidation state for potassium is +2. The equation becomes:
2x + 2(1) + 7(-2) = 0
Simplifying the equation, we get:
2x – 12 = 0
Adding 12 to both sides, we find:
2x = 12
Dividing both sides by 2, we get:
x = 6
Therefore, the oxidation state of chromium in K2Cr2O7 is +6.
Understanding the oxidation state of chromium in K2Cr2O7 is important because it helps us predict the compound’s reactivity and its role in various chemical reactions. For example, the high oxidation state of chromium (+6) in K2Cr2O7 makes it a strong oxidizing agent, which is why it is used in the production of dyes, in leather tanning, and as an antiseptic.
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