Which of the following statements is false when referring to the oxidation state of carbon?

• A. In C\(_2\)H\(_6\), each carbon atom has an oxidation state of +3.
• B. In CO, the oxidation state of carbon is +2.
• C. In CO\(_2\), the oxidation state of carbon is +4.
• D. In CH\(_4\), the oxidation state of carbon is -4.

Answer: (A)

Verified step by step guidance

1. Recall that the oxidation state (oxidation number) of an element in a compound is a hypothetical charge assigned based on electronegativity differences and bonding, following specific rules.
2. Use the rule that hydrogen generally has an oxidation state of +1 when bonded to nonmetals, and oxygen generally has an oxidation state of -2 in most compounds.
3. Calculate the oxidation state of carbon in each compound by setting up an equation where the sum of oxidation states equals the overall charge of the molecule (which is zero for neutral molecules). For example, in C\(_2\)H\(_6\), let the oxidation state of carbon be x, then 2x + 6(+1) = 0.
4. Solve the equation for each compound to find the oxidation state of carbon: - For C\(_2\)H\(_6\): 2x + 6 = 0, solve for x. - For CO: x + (-2) = 0, solve for x. - For CO\(_2\): x + 2(-2) = 0, solve for x. - For CH\(_4\): x + 4(+1) = 0, solve for x.
5. Compare the calculated oxidation states with the given statements to identify which one is false.