In each of the following substances NaH, H2 and H2S , hydrogen is assigned an oxidation number of +1. Is this correct? Explain your reasoning. Answer in complete sentences.

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In each of the following substances NaH, H2 and H2S , hydrogen is assigned an oxidation number of +1. Is this correct? Explain your reasoning.

Answer in complete sentences.

 
### Determining Oxidation Numbers of Hydrogen

#### Question
In each of the following substances \( \text{NaH} \), \( \text{H}_2 \), and \( \text{H}_2\text{S} \), hydrogen is assigned an oxidation number of +1. Is this correct? Explain your reasoning.

Answer in complete sentences.

#### Answer Box
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In determining the oxidation number of hydrogen in various compounds, it is important to follow a few key rules about how oxidation numbers are assigned:

1. **Rules for Oxidation Numbers:**
   - For an atom in its elemental form (e.g., \( \text{H}_2 \)), the oxidation number is always 0.
   - For monatomic ions, the oxidation number is equal to the charge of the ion.
   - Hydrogen generally has an oxidation number of +1 when bonded to non-metals and -1 when bonded to metals.

2. **Oxidation Number in \( \text{NaH} \):**
   - Sodium (Na) is a metal and typically forms a +1 oxidation state.
   - Therefore, in \( \text{NaH} \), hydrogen would carry a -1 oxidation state to balance the +1 charge of sodium.
   - Hence, assigning hydrogen an oxidation number of +1 in \( \text{NaH} \) is incorrect.

3. **Oxidation Number in \( \text{H}_2 \):**
   - \( \text{H}_2 \) is hydrogen in its elemental form.
   - Hence, the oxidation number of hydrogen in \( \text{H}_2 \) is 0.
   - Assigning an oxidation number of +1 to hydrogen in \( \text{H}_2 \) is incorrect.

4. **Oxidation Number in \( \text{H}_2\text{S} \):**
   - In \( \text{H}_2\text{S} \), sulfur is a non-metal.
   - Hydrogen is bonded to a non-metal and typically has an oxidation number of +1 in such compounds.
   - Therefore, assigning an oxidation number of +1 to hydrogen in \( \text{H}_2\text{S} \) is correct.

In conclusion, hydrogen is correctly assigned an oxidation number of +1 in \( \text{H}_2\text{S} \). However
Transcribed Image Text:### Determining Oxidation Numbers of Hydrogen #### Question In each of the following substances \( \text{NaH} \), \( \text{H}_2 \), and \( \text{H}_2\text{S} \), hydrogen is assigned an oxidation number of +1. Is this correct? Explain your reasoning. Answer in complete sentences. #### Answer Box [Text Editor Interface] In determining the oxidation number of hydrogen in various compounds, it is important to follow a few key rules about how oxidation numbers are assigned: 1. **Rules for Oxidation Numbers:** - For an atom in its elemental form (e.g., \( \text{H}_2 \)), the oxidation number is always 0. - For monatomic ions, the oxidation number is equal to the charge of the ion. - Hydrogen generally has an oxidation number of +1 when bonded to non-metals and -1 when bonded to metals. 2. **Oxidation Number in \( \text{NaH} \):** - Sodium (Na) is a metal and typically forms a +1 oxidation state. - Therefore, in \( \text{NaH} \), hydrogen would carry a -1 oxidation state to balance the +1 charge of sodium. - Hence, assigning hydrogen an oxidation number of +1 in \( \text{NaH} \) is incorrect. 3. **Oxidation Number in \( \text{H}_2 \):** - \( \text{H}_2 \) is hydrogen in its elemental form. - Hence, the oxidation number of hydrogen in \( \text{H}_2 \) is 0. - Assigning an oxidation number of +1 to hydrogen in \( \text{H}_2 \) is incorrect. 4. **Oxidation Number in \( \text{H}_2\text{S} \):** - In \( \text{H}_2\text{S} \), sulfur is a non-metal. - Hydrogen is bonded to a non-metal and typically has an oxidation number of +1 in such compounds. - Therefore, assigning an oxidation number of +1 to hydrogen in \( \text{H}_2\text{S} \) is correct. In conclusion, hydrogen is correctly assigned an oxidation number of +1 in \( \text{H}_2\text{S} \). However
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