solve step by step:The oxidation number for carbon in

CO2(g) is

(Record in the first column)

C2H2(g) is

+/-

(Record in the second column)

H2CO3(aq) is

+/-

(Record in the third column)

CH2O(g) is

+/-

+/-

(Record in the fourth column)

To determine the oxidation number of carbon in various compounds, we follow a set of rules for assigning oxidation states:

1. The oxidation number of a free element is always 0.
2. The oxidation number of a monatomic ion equals the charge of the ion.
3. Oxygen almost always has an oxidation number of -2 in compounds.
4. Hydrogen has an oxidation number of +1 when bonded to non-metals and -1 when bonded to metals.
5. The sum of the oxidation numbers in a neutral compound is 0.
6. The sum of the oxidation numbers in a polyatomic ion is equal to the charge of the ion.

Using these rules, let's solve for the oxidation number of carbon in each given compound step-by-step:

### CO₂ (Carbon Dioxide)
\[ \text{CO}_2 \]

- Oxygen has an oxidation number of -2.
- Let \( x \) be the oxidation number of carbon.

For the molecule CO₂, the equation is:
\[ x + 2(-2) = 0 \]
\[ x - 4 = 0 \]
\[ x = +4 \]

So, the oxidation number for carbon in CO₂ is +4.

### C₂H₂ (Acetylene)
\[ \text{C}_2\text{H}_2 \]

- Hydrogen has an oxidation number of +1.
- Let \( x \) be the oxidation number of carbon.

For the molecule C₂H₂, the equation is:
\[ 2x + 2(+1) = 0 \]
\[ 2x + 2 = 0 \]
\[ 2x = -2 \]
\[ x = -1 \]

So, the oxidation number for carbon in C₂H₂ is -1.

### H₂CO₃ (Carbonic Acid)
\[ \text{H}_2\text{CO}_3 \]

- Hydrogen has an oxidation number of +1.
- Oxygen has an oxidation number of -2.
- Let \( x \) be the oxidation number of carbon.

For the molecule H₂CO₃, the equation is:
\[ 2(+1) + x + 3(-2) = 0 \]
\[ 2 + x - 6 = 0 \]
\[ x - 4 = 0 \]
\[ x = +4 \]

So, the oxidation number for carbon in H₂CO₃ is +4.

### CH₂O (Formaldehyde)
\[ \text{CH}_2\text{O} \]

- Hydrogen has an oxidation number of +1.
- Oxygen has an oxidation number of -2.
- Let \( x \) be the oxidation number of carbon.

For the molecule CH₂O, the equation is:
\[ x + 2(+1) + (-2) = 0 \]
\[ x + 2 - 2 = 0 \]
\[ x = 0 \]

So, the oxidation number for carbon in CH₂O is 0.

### Summary
- CO₂: Carbon oxidation number is +4.
- C₂H₂: Carbon oxidation number is -1.
- H₂CO₃: Carbon oxidation number is +4.
- CH₂O: Carbon oxidation number is 0.

If you have any questions or need further details, feel free to ask!

### Questions to Ask
1. What are the rules for assigning oxidation numbers?
2. How do you determine the oxidation number of carbon in organic compounds?
3. Can the oxidation number of an element in a compound ever be a fraction?
4. How do oxidation numbers relate to redox reactions?
5. What is the significance of the oxidation number in a chemical reaction?

### Tip
Always ensure the sum of oxidation numbers in a neutral compound is zero and in a polyatomic ion equals the charge of the ion.

Learn how to determine the oxidation numbers of carbon in CO2, C2H2, H2CO3, and CH2O with detailed step-by-step solutions. Understand the rules for assigning oxidation states in chemical compounds. Suitable for high school and above.

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