Key term
CCEA AS-Level Chemistry 1110
Formulae, Equations and Amounts of Substance
Atomic Structure
Topic overviewProtons, neutrons and electronsAtomic number, mass number and the composition of ionsIsotopes and relative isotopic massRelative atomic, molecular and formula massMass spectra and relative atomic mass calculationsMass spectra of diatomic elementsElectronic configuration and the building up principleOrbitals, electron spin and orbital shapesThe s-, p-, d- and f-blocks of the Periodic TableIonisation energies and their equationsTrends in ionisation energy as evidence for shells and subshells
Bonding
Topic overviewIonic bonding and electron transferDot and cross diagrams for ionic compoundsCovalent bonding and the shared pairLone pairs and co-ordinate bondingDot and cross diagrams for covalent molecules and ionsThe octet rule and its limitationsElectronegativity and bond polarityMetallic bonding
Intermolecular Forces and Structure
Shapes of Molecules and Ions
Redox
The Halogens
Acid-Base Titrations
Qualitative Tests
Formulae and Amounts of a Substance
Nomenclature and Isomerism in Organic Chemistry
Alkanes
Topic overviewAlkanes as saturated hydrocarbonsBoiling points of alkanes and van der Waals' forcesBoiling points of branched isomersComplete and incomplete combustion of alkanesPollutants from alkane fuels and the atmosphereCatalytic convertersRadicals, homolytic fission and heterolytic fissionFree radical substitution of alkanes
Alkenes
Topic overviewUnsaturated hydrocarbons and the bromine water testSigma and pi bonds in the carbon–carbon double bondElectron density at C=C, reactivity and catalytic hydrogenationAddition of chlorine and bromine to alkenesAddition of hydrogen chloride and hydrogen bromideElectrophiles, heterolytic fission and the addition mechanismCarbocation stability and Markovnikov additionAddition polymerisation of alkenes
Halogenoalkanes
Topic overviewClassification and boiling points of halogenoalkanesLaboratory preparation of a halogenoalkane from an alcoholNucleophiles and hydrolysis with aqueous alkaliReactions with ammonia and with potassium cyanideRelative rates of hydrolysis and carbon–halogen bond enthalpyElimination using ethanolic potassium hydroxideCFCs and the ozone layer
Alcohols
Infrared Spectroscopy
Energetics
Topic overviewExothermic and endothermic changesStandard conditions and the standard enthalpy changeEnthalpy level diagramsStandard enthalpies of combustion and formationStandard enthalpy of neutralisationMeasuring enthalpy changes by experimentEnthalpy calculations using q = mcΔTHess's Law and enthalpy cyclesIndirect enthalpy calculations using Hess's LawAverage bond enthalpies and their limitations
Kinetics
Equilibrium
Group II Elements and Their Compounds
Topic overviews-block character and electronic configurationTrends in atomic radius and first ionisation energyReactions of the elements with oxygen, water and dilute acidsThe oxides and their reactions with water and dilute acidsThermal stability of the carbonates and hydroxidesUses of magnesium oxide, calcium carbonate and limeSolubility trends and solubility curves
Energetics
- 10 subtopics
- 30 things to know
- Unit AS 2
What Energetics covers
Energetics is examined in Unit AS 2, Further Physical and Inorganic Chemistry and an Introduction to Organic Chemistry, and drawn on again in Unit AS 3, Basic Practical Chemistry. It covers exothermic and endothermic changes, standard conditions and the standard enthalpy change, enthalpy level diagrams, standard enthalpies of combustion and formation, standard enthalpy of neutralisation, measuring enthalpy changes by experiment, enthalpy calculations using q = mcΔT, Hess's Law and enthalpy cycles, indirect enthalpy calculations using Hess's Law and average bond enthalpies and their limitations.
Where it is assessed
Unit AS 2
Further Physical and Inorganic Chemistry and an Introduction to Organic Chemistry, and again in Unit AS 3, Basic Practical Chemistry.
Check the CCEA specification ↗The 10 subtopics
Each one has its own page. CCEA AS Chemistry students sit this topic in the first year.
- Exothermic and endothermic changesTerm exothermic reaction, term endothermic reaction and two reactions that are strongly exothermic.Open →
- Standard conditions and the standard enthalpy changeStandard conditions of pressure and temperature used in thermochemistry, term standard enthalpy change and units in which a standard enthalpy change is quoted.Open →
- Enthalpy level diagramsAppearance of an enthalpy level diagram for an exothermic reaction and appearance of an enthalpy level diagram for an endothermic reaction.Open →
- Standard enthalpies of combustion and formationStandard enthalpy of combustion and standard enthalpy of formation.Open →
- Standard enthalpy of neutralisationStandard enthalpy of neutralisation and how the enthalpy of neutralisation is measured in the laboratory.Open →
- Measuring enthalpy changes by experimentTwo assumptions made when a calorimetry result is calculated and specific heat capacity of water used in these calculations.Open →
- Enthalpy calculations using q = mcΔTRecall questions on the meaning of each symbol in q = mcΔT, specific heat capacity, which mass is used in solution, why a temperature change is the same in kelvin and Celsius, converting q to a molar enthalpy change, the sign convention, worked combustion, displacement and dissolving calculations, and why the limiting reagent is used.Open →
- Hess's Law and enthalpy cyclesPrinciple of conservation of energy and hess's Law.Open →
- Indirect enthalpy calculations using Hess's LawRecall questions on using standard enthalpies of formation and of combustion in a Hess cycle, worked calculations on methane, calcium carbonate, ethene, the thermite reaction, iron ore and sulfur dioxide, working backwards to an unknown enthalpy of formation, and checking the sign of the answer.Open →
- Average bond enthalpies and their limitationsRecall questions on the definition of average bond enthalpy and why it is positive, calculating an enthalpy change from bonds broken and made, worked examples on hydrogen chloride, ammonia, methane and ethene, working back to a single bond enthalpy, and why the method is less reliable than Hess's Law.Open →
What you need to know
Answer each one before you reveal it.
Your recallNot started
Key term
Describe how the enthalpy change for the displacement of copper by zinc is measured.
Key term
Describe the method used to measure the enthalpy of combustion of a liquid fuel.
Key term
Describe how a graph is used to correct a calorimetry result for heat loss.
Numbers
State the equation used to calculate the heat change in a calorimetry experiment and say what each symbol means.
Key term
Describe how standard enthalpies of formation are used to find the enthalpy change of a reaction.
Key term
Define the term exothermic reaction.
Key term
State the standard conditions of pressure and temperature used in thermochemistry.
Key term
What quantity is plotted on the vertical axis of an enthalpy level diagram?
Key term
Why is the standard enthalpy of formation of an element in its standard state zero?
Key term
State the principle of conservation of energy.
Key term
Why is a bond enthalpy always a positive quantity?
Key term
Define the term endothermic reaction.
Key term
What temperature in degrees Celsius corresponds to 298 K?
Key term
Describe the appearance of an enthalpy level diagram for an endothermic reaction.
Key term
Write the equation whose enthalpy change is the standard enthalpy of combustion of ethanol.
Key term
Why is the enthalpy of neutralisation defined per mole of water rather than per mole of acid?
Key term
Define the term specific heat capacity.
Key term
Explain how Hess's Law follows from the principle of conservation of energy.
Key term
Describe how standard enthalpies of combustion are used to find the enthalpy change of a reaction.
Key term
Why is the word average used in average bond enthalpy?
Key term
State the sign of the enthalpy change for an exothermic reaction and for an endothermic reaction.
Key term
State the units in which a standard enthalpy change is quoted.
Key term
Why does the horizontal axis of an enthalpy level diagram carry no scale?
Key term
Write the equation whose enthalpy change is the standard enthalpy of formation of methane.
Key term
State the approximate value of the enthalpy of neutralisation for a strong acid and a strong alkali.
Key term
Why does a temperature change have the same numerical value in kelvin and in degrees Celsius?
Key term
Why is Hess's Law so useful in thermochemistry?
Numbers
Using ΔfHӨ values of −824 kJ mol⁻¹ for Fe₂O₃(s) and −1676 kJ mol⁻¹ for Al₂O₃(s), calculate ΔH for Fe₂O₃(s) + 2Al(s) → Al₂O₃(s) + 2Fe(s).
Numbers
The enthalpy change for CH₄(g) → C(g) + 4H(g) is +1652 kJ mol⁻¹. Calculate the average C–H bond enthalpy in methane.
Take Energetics further
The same content, four other ways.
Questions from this topic
Each one with the model answer underneath.
- 1
Define the term exothermic reaction.
Model answer
An exothermic reaction is one that releases heat energy to the surroundings, so the temperature of the surroundings rises.
- 2
Define the term endothermic reaction.
Model answer
An endothermic reaction is one that absorbs heat energy from the surroundings, so the temperature of the surroundings falls.
- 3
State the sign of the enthalpy change for an exothermic reaction and for an endothermic reaction.
Model answer
An exothermic reaction has a negative enthalpy change and an endothermic reaction has a positive enthalpy change.
- 4
Why are chemical reactions almost always accompanied by a heat change?
Model answer
The energy stored in the bonds of the products is different from that stored in the bonds of the reactants, and the difference has to be given out to or taken from the surroundings.
- 5
Is breaking a covalent bond exothermic or endothermic, and why?
Model answer
Breaking a bond is endothermic, because energy must be supplied to overcome the electrostatic attraction holding the bonded atoms together.
- 6
Is making a covalent bond exothermic or endothermic, and why?
Model answer
Making a bond is exothermic, because energy is released as the new attraction between the nuclei and the shared electrons is established.
What is inside Levo
Six ways to work the same material.
Energetics revision questions
- Is Energetics examined at AS in CCEA Chemistry?
- Yes. It sits in Unit AS 2, which you take in the first year, so it is on the AS paper as well as counting towards the full A level.
- What does Energetics cover in CCEA AS-Level Chemistry?
- 10 subtopics: exothermic and endothermic changes, standard conditions and the standard enthalpy change, enthalpy level diagrams, standard enthalpies of combustion and formation, standard enthalpy of neutralisation, measuring enthalpy changes by experiment, enthalpy calculations using q = mcδt, hess's law and enthalpy cycles, indirect enthalpy calculations using hess's law and average bond enthalpies and their limitations. Each one has its own page with questions and model answers.
- How is Energetics organised?
- By the CCEA 1110 specification, subtopic by subtopic, so it matches the order you are taught it in.
Every question in Energetics, on a schedule.
Attempt a question from memory, write the correct version, then attempt it again. Levo records the jump between your first attempt and your last, and brings each question back on the day you are due to forget it.
Or £46 a year, about £3.83 a month. Cancel anytime.