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2 Ammonia, NH_(3) is a simple molecular compound. (a) Hydrogen bonding occurs between molecules of ammonia. Figure 2 shows two molecules of ammonia. H H-N: H-stackrel (N)(H)-H Figure 2 Draw one hydrogen bond between the two molecules shown in Figure 2. You should include the partial charges on the molecules. (b) Ammonia can be reacted with acids to form salts. The salts formed can be used as fertilisers. (i) Ammonia reacts with sulfuric acid to form the salt ammonium sulfate. Identify the correct formula for ammonium sulfate. (2) (1)

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2 Ammonia, NH_(3) is a simple molecular compound. (a) Hydrogen bonding occurs between molecules of ammonia. Figure 2 shows two molecules of ammonia. H H-N: H-stackrel (N)(H)-H Figure 2 Draw one hydrogen bond between the two molecules shown in Figure 2. You should include the partial charges on the molecules. (b) Ammonia can be reacted with acids to form salts. The salts formed can be used as fertilisers. (i) Ammonia reacts with sulfuric acid to form the salt ammonium sulfate. Identify the correct formula for ammonium sulfate. (2) (1)

2 Ammonia, NH_(3) is a simple molecular compound. (a) Hydrogen bonding occurs between molecules of ammonia. Figure 2 shows two molecules of ammonia. H H-N: H-stackrel (N)(H)-H Figure 2 Draw one hydrogen bond between the two molecules shown in Figure 2. You should include the partial charges on the molecules. (b) Ammonia can be reacted with acids to form salts. The salts formed can be used as fertilisers. (i) Ammonia reacts with sulfuric acid to form the salt ammonium sulfate. Identify the correct formula for ammonium sulfate. (2) (1)

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JenaMaster · Tutor for 5 years

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- Drawn hydrogen bond: Can be illustrated as a dotted line between the \( \delta^- \) of the nitrogen atom in one \( \mathrm{NH}_3 \) molecule and \( \delta^+ \) on the hydrogen atom of another \( \mathrm{NH}_3 \) molecule including the partial charges as described.<br />- Correct formula for ammonium sulfate: C \( \left(\mathrm{NH}_{4}\right)_{2} \mathrm{SO}_{4} \)

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## Drawing Hydrogen Bond:<br />To illustrate a hydrogen bond between two molecules of ammonia, it's essential to show the interaction between the hydrogen atom in one ammonia molecule, which has a partial positive charge (\(\delta^+\)), and the nitrogen atom of another ammonia molecule, which has a partial negative charge (\(\delta^-\)). This dipole-dipole interaction results in a hydrogen bond, represented typically as a dashed line.<br />## Writing the partial charges:<br />Given ammonia's molecular structure, each hydrogen atom (connected to nitrogen, more electronegative) carries a partial positive charge. Conversely, the nitrogen atom, being more electronegative, carries a partial negative charge.<br /><br />## Identifying Ammonium Sulfate:<br />When ammonia \( \left( \mathrm{NH}_3 \right) \) reacts with sulfuric acid \( \left( \mathrm{H}_2\mathrm{SO}_4 \right) \), it accepts a hydrogen ion (\( \mathrm{H}^+ \)) from the sulfuric acid, forming the ammonium ion \( \left( \mathrm{NH}_4^+ \right) \). The sulfate ion \( \left( \mathrm{SO}_4^{2-} \right) \) remains unchanged. To balance out the charges, two ammonium ions are required for every sulfate ion, leading to the formula \( \left( \mathrm{NH}_4 \right)_2 \mathrm{SO}_4 \).<br /><br />### For the chemical reaction:<br />\[ \mathrm{2NH}_3 + \mathrm{H}_2\mathrm{SO}_4 \rightarrow \left( \mathrm{NH}_4 \right)_2\mathrm{SO}_4 \]
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