For the reaction KCIO → KCl + 0, 2 assign oxidation numbers to each element on each side of the equation. K in KCIO: K in KCl: Cl in KC1O: Cl in KCl: O in KCIO: O in O2:
For the reaction KCIO → KCl + 0, 2 assign oxidation numbers to each element on each side of the equation. K in KCIO: K in KCl: Cl in KC1O: Cl in KCl: O in KCIO: O in O2:
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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![### Assigning Oxidation Numbers
**For the reaction:**
\[ \text{KClO} \longrightarrow \text{KCl} + \frac{1}{2} \text{O}_2 \]
Assign oxidation numbers to each element on each side of the equation.
#### Elements and Their Oxidation Numbers:
1. **Potassium (K) in KClO:**
\[ \text{K in KClO:} \ \ \ \ \ \ \ \ \ \ \ \]
2. **Potassium (K) in KCl:**
\[ \text{K in KCl:} \ \ \ \ \ \ \ \ \ \ \ \]
3. **Chlorine (Cl) in KClO:**
\[ \text{Cl in KClO:} \ \ \ \ \ \ \ \ \ \ \ \]
4. **Chlorine (Cl) in KCl:**
\[ \text{Cl in KCl:} \ \ \ \ \ \ \ \ \ \ \ \]
5. **Oxygen (O) in KClO:**
\[ \text{O in KClO:} \ \ \ \ \ \ \ \ \ \ \ \]
6. **Oxygen (O) in \( \text{O}_2 \):**
\[ \text{O in } \text{O}_2: \ \ \ \ \ \ \ \ \ \ \ \]
##### Explanation of the Reaction
The provided reaction involves the decomposition of potassium hypochlorite (KClO) into potassium chloride and oxygen gas. To better understand this reaction, each element's oxidation state must be determined before and after the reaction. This is crucial for identifying any redox (reduction-oxidation) processes occurring within the reaction.
#### How to Determine Oxidation Numbers:
1. For a molecule or compound:
- The sum of the oxidation numbers must equal the overall charge of the molecule or compound.
2. Common oxidation states include:
- Group 1 elements (e.g., K) always have an oxidation state of +1.
- Group 17 elements (e.g., Cl) typically have an oxidation state of -1.
- Oxygen generally has an oxidation state of -2 in most compounds.
#### Example:
For \( \text](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Ff00f8b75-2bac-4335-a200-62a4fa07a89d%2F3467d5d3-c0e9-4615-a391-05e14150c77e%2Fz7eaj4_processed.png&w=3840&q=75)
Transcribed Image Text:### Assigning Oxidation Numbers
**For the reaction:**
\[ \text{KClO} \longrightarrow \text{KCl} + \frac{1}{2} \text{O}_2 \]
Assign oxidation numbers to each element on each side of the equation.
#### Elements and Their Oxidation Numbers:
1. **Potassium (K) in KClO:**
\[ \text{K in KClO:} \ \ \ \ \ \ \ \ \ \ \ \]
2. **Potassium (K) in KCl:**
\[ \text{K in KCl:} \ \ \ \ \ \ \ \ \ \ \ \]
3. **Chlorine (Cl) in KClO:**
\[ \text{Cl in KClO:} \ \ \ \ \ \ \ \ \ \ \ \]
4. **Chlorine (Cl) in KCl:**
\[ \text{Cl in KCl:} \ \ \ \ \ \ \ \ \ \ \ \]
5. **Oxygen (O) in KClO:**
\[ \text{O in KClO:} \ \ \ \ \ \ \ \ \ \ \ \]
6. **Oxygen (O) in \( \text{O}_2 \):**
\[ \text{O in } \text{O}_2: \ \ \ \ \ \ \ \ \ \ \ \]
##### Explanation of the Reaction
The provided reaction involves the decomposition of potassium hypochlorite (KClO) into potassium chloride and oxygen gas. To better understand this reaction, each element's oxidation state must be determined before and after the reaction. This is crucial for identifying any redox (reduction-oxidation) processes occurring within the reaction.
#### How to Determine Oxidation Numbers:
1. For a molecule or compound:
- The sum of the oxidation numbers must equal the overall charge of the molecule or compound.
2. Common oxidation states include:
- Group 1 elements (e.g., K) always have an oxidation state of +1.
- Group 17 elements (e.g., Cl) typically have an oxidation state of -1.
- Oxygen generally has an oxidation state of -2 in most compounds.
#### Example:
For \( \text
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