His represents a balanced oxidation reduction reaction 2co2g...

This represents a balanced oxidation-reduction reaction: 2CO(g) + O2(g) --> 2CO2(g) Match the statement on the left with the correct choice from the right. Choices can be used more than once or not at all. Each O in O2 has an oxidation number of Each C in CO has an oxidation number of In this reaction, carbon has been Each C in CO2 has an oxidation number of 1. 0 2. -1 3. -2 4. -4 5. +1 6. +2 7. +4 8. Reduced 9. Oxidized

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00:02 Hi there.

00:03 In this question, we have an oxidation reduction reaction, so i want to start off by defining what oxidation is and what reduction is.

00:17 Oxidation is a loss of one or more electrons.

00:26 Since electrons are negatively charged, the oxidation of the substance will increase.

00:34 So the oxidation number will become more positive, or in other words, it will increase because it has lost negativity.

00:51 If something loses negativity becomes more positive.

00:54 All right, reduction is going to be the reverse then.

00:58 It is going to be a gain of electrons.

01:02 One or more electrons.

01:06 It will result in the oxidation number decreasing because if you gain negative particles, the oxidation number will go down.

01:21 All right, so let's get started by assigning some oxidation numbers here.

01:26 Going to start off with just the oxygen, because we know that any uncombined element has an oxidation number of zero.

01:34 So each oxygen in 02 has an oxidation number of zero.

01:38 Then we know that oxygen in a compound has an oxidation number of negative 2 unless it's in a peroxide.

01:47 Well, neither of these oxygens are part of a peroxide here, so their oxidation numbers are negative 2.

01:53 Then we know that in a compound, the sum of the oxidation numbers is always zero.

01:59 That means in co, carbon must be positive 2 because positive 2 plus negative 2 is 0.

02:05 And in co2, there are 2 oxygen that are negative 2 each.

02:10 That gives us negative 4.

02:11 So the only carbon in this molecule must have an oxidation number of positive 4.

02:17 So from this, we can see that carbon goes from positive 2 oxidation number to positive 4.

02:28 It increased...

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