Energetics topic check · H1 Chemistry 8873
Check what you know about H1 Chemistry Energetics, practise what needs work, then check your progress and come back for a later review.
Learning objectives
- explain that most chemical reactions are accompanied by energy changes, principally in the form of heat usually associated with the breaking and forming of chemical bonds; the reaction can be exothermic (∆H negative) or endothermic (∆H positive)
- construct and interpret an energy profile diagram, in terms of the enthalpy change of the reaction and of the activation energy (see also Section 7)
- explain and use the terms: — enthalpy change of reaction and standard conditions, with particular reference to: formation; combustion; neutralisation
- explain and use the terms: — bond energy (∆H positive, i.e. bond breaking) (see also Section 2)
- explain and use the terms: — lattice energy (∆H negative, i.e. gaseous ions to solid lattice)
- calculate enthalpy changes from appropriate experimental results, including the use of the relationship: heat change = mc∆T
- explain, in qualitative terms, the effect of ionic charge and of ionic radius on the numerical magnitude of a lattice energy
- apply Hess’ Law to carry out calculations involving given simple energy cycles and relevant energy terms (restricted to enthalpy changes of formation, combustion and neutralisation), with particular reference to: — determining enthalpy changes that cannot be found by direct experiment, e.g. an enthalpy change of formation from enthalpy changes of combustion
- apply Hess’ Law to carry out calculations involving given simple energy cycles and relevant energy terms (restricted to enthalpy changes of formation, combustion and neutralisation), with particular reference to: — average bond energies [construction of energy cycles is not required]
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Check what I know
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