Answer :
### Steps to Complete Table 10.3
Let's fill in Table 10.3 with the available data and add any missing data through researched information.
We know:
- Ethane (C₂H₆) has a melting point of -295.6°C, a boiling point of -128.2°C, solubility in water is 56.8 mg/L, and is used for power generation.
We need to look up the additional compounds:
1. Dimethyl Ether (C₂H₆O)
- Melting point: -138.5°C
- Boiling point: -24.8°C
- Solubility in water: 328 g/L
- Common use: Refrigerant, aerosol propellant
2. Ethanol (C₂H₆O)
- Melting point: -114.1°C
- Boiling point: 78.37°C
- Solubility in water: Miscible (completely soluble in water)
- Common use: Alcoholic beverages, disinfectant, solvent
3. Ethylene Glycol (C₂H₆O₂)
- Melting point: -12.9°C
- Boiling point: 197.3°C
- Solubility in water: Miscible
- Common use: Antifreeze, coolant
Adding these details to the table, we get:
[tex]\[ \begin{array}{|c|c|c|c|c|} \hline & \text{Ethane} & \text{Dimethyl Ether} & \text{Ethanol Alcohol} & \text{Ethylene Glycol} \\ \hline \text{Melting point } (°C) & -295.6 & -138.5 & -114.1 & -12.9 \\ \hline \text{Boiling point } (°C) & -128.2 & -24.8 & 78.37 & 197.3 \\ \hline \text{Solubility in water} & 56.8 \text{ mg/L} & 328 \text{ g/L} & \text{Miscible} & \text{Miscible} \\ \hline \text{Common use/application} & \text{power generation} & \text{refrigerant, aerosol propellant} & \text{beverages, disinfectant, solvent} & \text{antifreeze, coolant} \\ \hline \end{array} \][/tex]
### 1. Compounds with the Same Chemical Formula and Their Differences
Chemical Formulas:
- Dimethyl Ether (C₂H₆O) and Ethanol (C₂H₆O) have the same chemical formula but different structures.
These compounds, with the same chemical formula but different structures, are called isomers.
Differences in Structures and Properties:
- Dimethyl Ether: It has an ether functional group (an oxygen atom connected to two alkyl or aryl groups).
- Structure: CH₃OCH₃
- Properties: Generally more volatile, lower boiling point compared to ethanol.
- Ethanol: It has a hydroxyl group (-OH).
- Structure: CH₃CH₂OH
- Properties: Alcohol, forms hydrogen bonds, higher boiling point due to hydrogen bonding.
### 2. Compounds with Hydrogen Bonds
Compounds likely to have hydrogen bonds:
- Ethanol and Ethylene Glycol.
Explanation:
- Ethanol: Has an -OH group, which allows it to form hydrogen bonds with other ethanol molecules and water.
- Ethylene Glycol: Has two -OH groups, greatly increasing its ability to form hydrogen bonds.
Hydrogen bonding occurs when a hydrogen atom, covalently bonded to an electronegative atom like oxygen, interacts with another electronegative atom.
### 3. Polar Compounds
Polar Compounds:
- Ethanol and Ethylene Glycol.
Explanation:
- Both ethanol and ethylene glycol have -OH groups, which create polar bonds and make the molecules polar.
- Dimethyl Ether: Is less polar than ethanol and ethylene glycol despite having oxygen because it lacks significant hydrogen bonding and overall polarity is less.
Solubility in Water:
- Polar compounds like ethanol and ethylene glycol dissolve well in water due to their ability to form hydrogen bonds with water molecules.
- Ethane is non-polar and has limited solubility in water.
- Dimethyl Ether, though polar, does not form as strong hydrogen bonds as ethanol or ethylene glycol.
### Summary
By examining melting points, boiling points, solubility, common uses, and identifying features such as hydrogen bonds and polarity, we've completed and analyzed Table 10.3.
Let's fill in Table 10.3 with the available data and add any missing data through researched information.
We know:
- Ethane (C₂H₆) has a melting point of -295.6°C, a boiling point of -128.2°C, solubility in water is 56.8 mg/L, and is used for power generation.
We need to look up the additional compounds:
1. Dimethyl Ether (C₂H₆O)
- Melting point: -138.5°C
- Boiling point: -24.8°C
- Solubility in water: 328 g/L
- Common use: Refrigerant, aerosol propellant
2. Ethanol (C₂H₆O)
- Melting point: -114.1°C
- Boiling point: 78.37°C
- Solubility in water: Miscible (completely soluble in water)
- Common use: Alcoholic beverages, disinfectant, solvent
3. Ethylene Glycol (C₂H₆O₂)
- Melting point: -12.9°C
- Boiling point: 197.3°C
- Solubility in water: Miscible
- Common use: Antifreeze, coolant
Adding these details to the table, we get:
[tex]\[ \begin{array}{|c|c|c|c|c|} \hline & \text{Ethane} & \text{Dimethyl Ether} & \text{Ethanol Alcohol} & \text{Ethylene Glycol} \\ \hline \text{Melting point } (°C) & -295.6 & -138.5 & -114.1 & -12.9 \\ \hline \text{Boiling point } (°C) & -128.2 & -24.8 & 78.37 & 197.3 \\ \hline \text{Solubility in water} & 56.8 \text{ mg/L} & 328 \text{ g/L} & \text{Miscible} & \text{Miscible} \\ \hline \text{Common use/application} & \text{power generation} & \text{refrigerant, aerosol propellant} & \text{beverages, disinfectant, solvent} & \text{antifreeze, coolant} \\ \hline \end{array} \][/tex]
### 1. Compounds with the Same Chemical Formula and Their Differences
Chemical Formulas:
- Dimethyl Ether (C₂H₆O) and Ethanol (C₂H₆O) have the same chemical formula but different structures.
These compounds, with the same chemical formula but different structures, are called isomers.
Differences in Structures and Properties:
- Dimethyl Ether: It has an ether functional group (an oxygen atom connected to two alkyl or aryl groups).
- Structure: CH₃OCH₃
- Properties: Generally more volatile, lower boiling point compared to ethanol.
- Ethanol: It has a hydroxyl group (-OH).
- Structure: CH₃CH₂OH
- Properties: Alcohol, forms hydrogen bonds, higher boiling point due to hydrogen bonding.
### 2. Compounds with Hydrogen Bonds
Compounds likely to have hydrogen bonds:
- Ethanol and Ethylene Glycol.
Explanation:
- Ethanol: Has an -OH group, which allows it to form hydrogen bonds with other ethanol molecules and water.
- Ethylene Glycol: Has two -OH groups, greatly increasing its ability to form hydrogen bonds.
Hydrogen bonding occurs when a hydrogen atom, covalently bonded to an electronegative atom like oxygen, interacts with another electronegative atom.
### 3. Polar Compounds
Polar Compounds:
- Ethanol and Ethylene Glycol.
Explanation:
- Both ethanol and ethylene glycol have -OH groups, which create polar bonds and make the molecules polar.
- Dimethyl Ether: Is less polar than ethanol and ethylene glycol despite having oxygen because it lacks significant hydrogen bonding and overall polarity is less.
Solubility in Water:
- Polar compounds like ethanol and ethylene glycol dissolve well in water due to their ability to form hydrogen bonds with water molecules.
- Ethane is non-polar and has limited solubility in water.
- Dimethyl Ether, though polar, does not form as strong hydrogen bonds as ethanol or ethylene glycol.
### Summary
By examining melting points, boiling points, solubility, common uses, and identifying features such as hydrogen bonds and polarity, we've completed and analyzed Table 10.3.
