Question
The table shows the chemical formulas and melting points for four compounds.
Formulas
CH
Melting Point (°C)
-182
0
714
747
H₂O
MgCl₂
NaBr
What types of bonds formed in each of these compounds, and how does the melting point data support this conclusion?
A. CH, and H₂O must have tonic bonds because they have high melting points, whereas MgCl, and NaBr must have covalent bonds because they have low melting points.
OB. CH, and H₂O must have ionic bonds because they have low melting points, whereas MgCl, and NaBr must have covalent bonds because they have high melting points
OC.CH, and H₂O must have covalent bonds because they have low melting points, whereas MgCl, and NaBr must have ionic bonds because they have high melting points.
OD CH, and H,O must have covalent bonds because they have high melting points, whereas MgCl, and NaBr must have ionic bonds because they have low melting points
Formulas
CH
Melting Point (°C)
-182
0
714
747
H₂O
MgCl₂
NaBr
What types of bonds formed in each of these compounds, and how does the melting point data support this conclusion?
A. CH, and H₂O must have tonic bonds because they have high melting points, whereas MgCl, and NaBr must have covalent bonds because they have low melting points.
OB. CH, and H₂O must have ionic bonds because they have low melting points, whereas MgCl, and NaBr must have covalent bonds because they have high melting points
OC.CH, and H₂O must have covalent bonds because they have low melting points, whereas MgCl, and NaBr must have ionic bonds because they have high melting points.
OD CH, and H,O must have covalent bonds because they have high melting points, whereas MgCl, and NaBr must have ionic bonds because they have low melting points
Answers
GPT-4o mini
To analyze the types of bonds and how they relate to the melting points, let's first briefly categorize the bonding types based on the compounds listed:
1. **CH (likely representing methane, CH₄)**: Methane consists of covalent bonds between carbon and hydrogen atoms.
2. **H₂O (water)**: Water also has covalent bonds between hydrogen and oxygen atoms.
3. **MgCl₂ (magnesium chloride)**: This compound has ionic bonds between magnesium and chloride ions.
4. **NaBr (sodium bromide)**: Sodium bromide is another compound with ionic bonds formed between sodium and bromide ions.
Now, let's evaluate the melting points given in the table:
- **CH (melting point -182°C)**: The low melting point suggests weak intermolecular forces (such as van der Waals), consistent with covalent compounds.
- **H₂O (melting point 0°C)**: Although water has hydrogen bonding (a strong intermolecular force for a molecule), it is still relatively low compared to ionic compounds.
- **MgCl₂ (melting point 714°C)** and **NaBr (melting point 747°C)**: Both have high melting points, typical of ionic compounds due to the strong electrostatic interactions between the ions.
Based on this analysis:
- **Covalent bonds (in CH and H₂O)** correlate with lower melting points.
- **Ionic bonds (in MgCl₂ and NaBr)** correlate with higher melting points.
This aligns with **Option C**: "CH₄ and H₂O must have covalent bonds because they have low melting points, whereas MgCl₂ and NaBr must have ionic bonds because they have high melting points."
So the correct answer is: **OC. CH₄ and H₂O must have covalent bonds because they have low melting points, whereas MgCl₂ and NaBr must have ionic bonds because they have high melting points.**
1. **CH (likely representing methane, CH₄)**: Methane consists of covalent bonds between carbon and hydrogen atoms.
2. **H₂O (water)**: Water also has covalent bonds between hydrogen and oxygen atoms.
3. **MgCl₂ (magnesium chloride)**: This compound has ionic bonds between magnesium and chloride ions.
4. **NaBr (sodium bromide)**: Sodium bromide is another compound with ionic bonds formed between sodium and bromide ions.
Now, let's evaluate the melting points given in the table:
- **CH (melting point -182°C)**: The low melting point suggests weak intermolecular forces (such as van der Waals), consistent with covalent compounds.
- **H₂O (melting point 0°C)**: Although water has hydrogen bonding (a strong intermolecular force for a molecule), it is still relatively low compared to ionic compounds.
- **MgCl₂ (melting point 714°C)** and **NaBr (melting point 747°C)**: Both have high melting points, typical of ionic compounds due to the strong electrostatic interactions between the ions.
Based on this analysis:
- **Covalent bonds (in CH and H₂O)** correlate with lower melting points.
- **Ionic bonds (in MgCl₂ and NaBr)** correlate with higher melting points.
This aligns with **Option C**: "CH₄ and H₂O must have covalent bonds because they have low melting points, whereas MgCl₂ and NaBr must have ionic bonds because they have high melting points."
So the correct answer is: **OC. CH₄ and H₂O must have covalent bonds because they have low melting points, whereas MgCl₂ and NaBr must have ionic bonds because they have high melting points.**