Question detail
A compound has a calculated lattice enthalpy of -800 kJ/mol, while the experimental value is -650 kJ/mol. What does this difference suggest about the compound's bonding character?
Try the question, check the answer, then read the explanation to understand the curriculum point.
At a glance
Question
Type
exam_style
Style
Topic
Thermodynamics (A-level only)
Question
A compound has a calculated lattice enthalpy of -800 kJ/mol, while the experimental value is -650 kJ/mol. What does this difference suggest about the compound's bonding character?
Answer
The difference between the calculated and experimental lattice enthalpy suggests that the compound has some covalent character. The experimental value being less negative than the calculated value indicates that the ionic interactions are not as strong as expected, implying that there are additional covalent interactions present.
Explanation
This answer shows the student's ability to analyze numerical data related to lattice enthalpy and draw conclusions about bonding character. It tests their understanding of how discrepancies between theoretical and experimental values can indicate the nature of bonding in a compound.
Common mistake
Misunderstanding Lattice Enthalpy
Students often confuse lattice enthalpy with covalent character, thinking that higher lattice enthalpy always indicates stronger covalent bonding.
To fix this, students should focus on understanding that lattice enthalpy reflects the strength of ionic bonds, while covalent character arises from the degree of electron sharing between atoms.
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