What is the single oxidation number of carbon in C6H14?
Options:
a) +7/3
b) +14
c) -14
d) -7/3
e) 0
The sum of the oxidation numbers in a neutral molecule is always zero. In C6H14, the hydrogen atoms have an oxidation number of +1 each, so the total oxidation number from hydrogen is +14. Since the sum of the oxidation numbers must be zero, the oxidation number of carbon must be -14. Therefore, the correct option is c) -14.
i thought it was d)
I apologize for the mistake. You are correct. The oxidation number of carbon in C6H14 is -7/3, not -14. Each hydrogen atom has an oxidation number of +1, and since the molecule is neutral, the sum of the oxidation numbers must be zero. Therefore, 6 * (-7/3) + 14 * (+1) = 0. The correct option is d) -7/3.
What is the change in oxidation number of an atom of iodine in the half-reaction I ^- (aq) → I2 (s)?
a) an decrease of 1
b) a increase of 1
c) an decrease of 2
d) a increase of 2
e) an decrease of 3
In the given half-reaction, the oxidation state of iodine changes from -1 in I^- (aq) to 0 in I2 (s).
Therefore, the change in oxidation number of iodine is an increase of 1.
The correct option is b) a increase of 1.
To determine the oxidation number of carbon in a compound, we need to consider the rules for assigning oxidation numbers.
Oxidation numbers are hypothetical charges assigned to atoms in a compound. In hydrocarbons like C6H14 (hexane), we assume that hydrogen has an oxidation number of +1, and the overall charge of the molecule is 0.
In this case, there are 14 hydrogen atoms with an oxidation number of +1 each, totaling +14. Since the overall charge of the molecule is 0, the total oxidation numbers of all the atoms must also add up to 0.
Therefore, we can set up the equation: Oxidation number of carbon + 14 = 0.
Simplifying, we find that the oxidation number of carbon is -14.
So, the correct option is c) -14.