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3 cards from this section. Quick, good the night before a test.
Define bond enthalpy.
Think about energy and bond breaking.
What is the first step in estimating enthalpy changes using bond enthalpy?
Visual representation helps identify bonds.
What is bond enthalpy?
Think about the energy changes when bonds are created or broken.
True or False: Bond enthalpies are constants for all molecules.
Consider how different contexts change energy requirements.
Given the reaction: N₂(g) + 3H₂(g) → 2NH₃(g), estimate ΔH using bond enthalpies: N≡N = 945 kJ/mol, H-H = 436 kJ/mol, N-H = 391 kJ/mol. Show all calculations.
Remember to keep track of what bonds are being broken and formed!
Comparing C-O versus C-C bonds: Why do you think double bonds have higher enthalpies? Provide examples from diatomic and polyatomic molecules.
Think about how additional bonds change stability in molecules.
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