Question
Exam
Review
The table displays the chemical formulas and melting points of four compounds.
Formulas Melting Point (°C)
CH4
-182
0
H2O
714
MgCl2
747
9
NaBr
What types of bonds are present in each of these compounds, and how is this conclusion supported by the melting point data?
(1 point)
CH4 and H2O are deduced to have ionic bonds due to their low melting points, whereas MgCl2 and NaBr are inferred to possess covalent bonds as they exhibit high melting points.
CH4 and H2O are presumed to possess covalent bonds due to their high melting points, while MgCl2 and NaBr are inferred to have ionic bonds based on their low melting points.
CH4 and H2O are indicated to have covalent bonds owing to their low melting points, while MgCl2 and NaBr are suggested to have ionic bonds as indicated by their high melting points.
CH4 and H2O are inferred to possess ionic bonds due to their elevated melting points, while MgCl2 and NaBr are presumed to have covalent bonds as evidenced by their lower melting points.
Review
The table displays the chemical formulas and melting points of four compounds.
Formulas Melting Point (°C)
CH4
-182
0
H2O
714
MgCl2
747
9
NaBr
What types of bonds are present in each of these compounds, and how is this conclusion supported by the melting point data?
(1 point)
CH4 and H2O are deduced to have ionic bonds due to their low melting points, whereas MgCl2 and NaBr are inferred to possess covalent bonds as they exhibit high melting points.
CH4 and H2O are presumed to possess covalent bonds due to their high melting points, while MgCl2 and NaBr are inferred to have ionic bonds based on their low melting points.
CH4 and H2O are indicated to have covalent bonds owing to their low melting points, while MgCl2 and NaBr are suggested to have ionic bonds as indicated by their high melting points.
CH4 and H2O are inferred to possess ionic bonds due to their elevated melting points, while MgCl2 and NaBr are presumed to have covalent bonds as evidenced by their lower melting points.
Answers
Answered by
GPT-4o mini
The correct interpretation of the bonding types in the compounds based on their melting points is as follows:
- **CH4** (methane) and **H2O** (water) are examples of compounds that exhibit **covalent bonds**. This is supported by their relatively low melting points (−182 °C for CH4 and 0 °C for H2O), indicating that the intermolecular forces (like hydrogen bonding in H2O and Van der Waals forces in CH4) are weaker compared to ionic interactions.
- **MgCl2** (magnesium chloride) and **NaBr** (sodium bromide) are examples of compounds that exhibit **ionic bonds**. Their higher melting points (714 °C for MgCl2 and 747 °C for NaBr) suggest that the ionic bonds are strong, requiring more energy to break apart compared to the covalent bonds in CH4 and H2O.
Thus, the analysis concludes as follows:
**CH4 and H2O are indicated to have covalent bonds owing to their low melting points, while MgCl2 and NaBr are suggested to have ionic bonds as indicated by their high melting points.**
This reasoning matches the last option from your list.
- **CH4** (methane) and **H2O** (water) are examples of compounds that exhibit **covalent bonds**. This is supported by their relatively low melting points (−182 °C for CH4 and 0 °C for H2O), indicating that the intermolecular forces (like hydrogen bonding in H2O and Van der Waals forces in CH4) are weaker compared to ionic interactions.
- **MgCl2** (magnesium chloride) and **NaBr** (sodium bromide) are examples of compounds that exhibit **ionic bonds**. Their higher melting points (714 °C for MgCl2 and 747 °C for NaBr) suggest that the ionic bonds are strong, requiring more energy to break apart compared to the covalent bonds in CH4 and H2O.
Thus, the analysis concludes as follows:
**CH4 and H2O are indicated to have covalent bonds owing to their low melting points, while MgCl2 and NaBr are suggested to have ionic bonds as indicated by their high melting points.**
This reasoning matches the last option from your list.