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Study the image seen here very closely you'll be able to see how the atoms recombine based on the colors of the elemental symbols. Look at the labeled oxidation states for each atom. Use what you know about how these must balance to complete the image with the single missing oxidation number.(1 point)

co2+h2o-- ch2o+02

1 answer

To determine the missing oxidation number in the chemical reaction you provided, let's first clarify the reaction itself:

\[ \text{CO}_2 + \text{H}_2\text{O} \rightarrow \text{CH}_2\text{O} + \text{O}_2 \]

  1. Identify the oxidation states:

    • In carbon dioxide (\( \text{CO}_2 \)):
      • Carbon (C) has an oxidation state of +4.
      • Oxygen (O) has an oxidation state of -2.
    • In water (\( \text{H}_2\text{O} \)):
      • Hydrogen (H) has an oxidation state of +1.
      • Oxygen (O) has an oxidation state of -2.
    • In formaldehyde (\( \text{CH}_2\text{O} \)):
      • Carbon (C) has an oxidation state of +2.
      • Hydrogen (H) has an oxidation state of +1.
      • Oxygen (O) has an oxidation state of -2.
    • In molecular oxygen (\( \text{O}_2 \)):
      • Oxygen (O) has an oxidation state of 0 (as it is in its elemental form).

  2. Balance the oxidation states:

    • On the left side, the total oxidation state is the sum of contributions from \( \text{CO}_2 \) (+4 from C and -4 from two O) and \( \text{H}_2\text{O} \) (+2 from two H and -2 from O), giving +4 - 4 + 2 - 2 = 0.
    • On the right side, we have \( \text{CH}_2\text{O} \) (+2 from C + 2 from two H - 2 from O = 2) and \( \text{O}_2 \) (oxidation state 0), leading to +2 + 0 = +2.

  3. Calculate the missing oxidation number:

    • To balance the half-reaction, we can observe that there is a gain of oxidation state from +4 on the left (in \( \text{CO}_2 \)) to +2 on the right (in \( \text{CH}_2\text{O} \)), and a release of O in the formation of \( \text{O}_2 \).
    • Given that all oxidation states must balance out, the missing oxidation state should also account for the change in oxidation states between carbon in \( \text{CO}_2\) moving to \( \text{CH}_2\text{O} \) and the formation of \( \text{O}_2 \).

In conclusion, the missing oxidation number in the reaction provided can be considered to balance according to the changes in the oxidation states throughout the reaction. If it is specifically asking for a singular oxidation state, it is likely referring to either the final oxidation state of a carbon when moving from +4 to +2, or something related to how many electrons were transferred.

Thus, numerically interpreting the situation, the final answer reflecting the balancing act in terms of common states would be 2.