CAPE Chemistry Syllabus UNIT 1 page 1 of 9Atomic Structure & Periodic Table (Module 1)a) discuss process of theoretical change with respect to Dalton’s atomic theoryb) know the structure of an atom with respect to (wrt) properties of the sub-atomic particles, their relative charges and masses, location and behaviour in electric and magnetic fieldsc) define proton number, mass number, isotopes, relative atomic massd) state and explain concept of radioactivity e) describe the different types of nuclear decayf) write nuclear equations illustrating the different types of decayg) understand the n/p ratio, the island of stability and its significance to the stability of the nucleush) be able to predict which type of decay a radioactive isotope would undergo to fall within the island of stabilityi) state at least three uses of radioactive isotopesj) calculate relative atomic masses of elements given isotopic masses and abundancesk) describe how an emission spectrum of an element is obtainedl) show how emission spectra provides evidence for the existence of discrete energy levels (refer to the Bohr model, using the hydrogen spectrum as an example)m) state and explain the origins of the Lyman, Balmer and Paschen series in the hydrogen spectrumn) be able to perform calculations using energy, wavelength and frequency e.g. ΔE OR dE = hvo) define the terms orbital, sub-shell and shellp) state and describe the shapes of s and p orbitals and the relative energies of s, p and d orbitals (pay special attention to 3d and 4s relative energies)q) state and apply the rules of filling s, p and d orbitals with electrons r) state the electronic configurations of atoms and common ions of elements with atomic number from 1 – 30s) define the term first ionisation energy and illustrate it with an equation t) state and explain the factors that influence first ionisation energy (atomic radii, nuclear charge, shielding)u) state and explain the general trend in the first ionisation energy in periods 2 and 3 as well as the anomalies v) show how first ionisation energy gives evidence for sub-shells (use period 3)w) be able to determine the group # of an element based on ionisation energies

CAPE Chemistry Syllabus UNIT 1 page 2 of 9 Forces of Attraction (Module 1)a) state the various forces of attraction between particles:- ionic bonds, covalent bonds, metallic bonds, dative bonds, hydrogen bonds, Van der Waals forcesb) state the relationship between the forces of attraction and states of matterc) relate physical properties( variation in m.p /b.p, solubilities) to differences in strength of forces of attractiond) explain the formation of i) ionic bonds ii) covalent bonds (sigma and pi bonds) iii) metallic bonds, also include relationship between electronegativity and polarity of bondse) describe the formation of dative bonds e.g. NH3 + H+, BF3 and NH3

f) explain how hydrogen bonds, Van der Waals forces (temporary dipole-induced dipole and permanent dipole-dipole) are formedg) state and explain VSEPR theoryh) use VESPR theory to predict shapes of, and bond angles in simple molecules and ions BeCl2 (linear), BF3 (trigonal planar), NH4

+, CH4 (tetrahedral), NH3, CH3

+, H3O+ (pyramidal), H2O (bent / non-linear)i) explain concept of hybridisation and resonancej) explain shapes and bond angles of methane, ethane, ethane and benzenek) predict shapes and bond angles of molecules similar to ethane and ethane e.g. substituted derivatesl) describe qualitatively the lattice structure of crystalline solids and their relation to physical properties e.g. simple molecular (I2), hydrogen bonded (ice), giant molecular (SiO2), ionic (NaCl), metallic (Cu) and giant atomic (diamond, graphite)

The Mole Concepta) define mole, Avogadro’s Law and molar massb) perform calculations involving Avogadro’s Law and molar massc) construct balanced ionic equations from full equationsd) state molar volumes of gases at stp and rtpe) define molar concentration and mass concentrationf) perform calculations involving molar conc., mass conc., and volumes of gasesg) calculate empirical and molecular formulae given appropriate datah) perform calculations involving titrimetric analyses

CAPE Chemistry Syllabus UNIT 1 page 3 of 9Redox Reactions (Module 1)a) define the term redox b) define the terms oxidation and reductionc) determine the oxidation state of free elements or elements within compounds using oxidation state rulesd) determine whether a reaction is redox or non-redoxe) determine whether a substance is a reducing agent or oxidising agent based on changes of oxidation statesf) write a full ionic equation from two half equations

Kinetic Theory (Module 1)a) state basic assumptions of the kinetic theory with reference to an ideal gasb) explain the differences between real and ideal gasesc) describe the conditions necessary for a gas to approach ideal behaviourd) state why gases deviate from ideal gas behaviour at high pressures and low temperaturese) illustrate ideal gas behaviour using graphical representationsf) state Charles’ Law and Boyle’s Law and ideal gas equation and perform calculationsg) represent Charles’ Law and Boyle’s Law graphicallyh) explain i) the liquid state ii) melting iii) vaporisation

Energetics (Module 1)a) state conditions needed for a reaction to occur b) state that in all chemical reactions bonds are broken and bonds are formedc) understand that energy changes occur with the breakage and formation of bondsd) understand which changes require or release energye) define the terms endothermic and exothermicf) list at least 3 examples of endothermic and exothermic reactionsg) illustrate endothermic and exothermic reactions using energy profile diagramsh) define the term bond energyi) show the relationship between bond energy, strength of covalent bonds and reactivity of covalent molecules (use lack of reactivity of nitrogen as an example)j) state and explain factors that affect bond energyk) define the terms:- enthalpy of formation, enthalpy of combustion, enthalpy of reaction, enthalpy of hydration, enthalpy of solution,

CAPE Chemistry Syllabus UNIT 1 page 4 of 9enthalpy of neutralisation, enthalpy of atomisation, ionisation energy, electron affinity and lattice energyl) states processes involved in formation of an ionic compoundm) understand that certain processes cannot be determined experimentally and must be calculated using Hess’s Lawn) define Hess’s Lawo) understand that the Born-Haber cycle is an application of Hess’s Law for ionic compoundsp) state steps involved in a Born-Haber cycleq) use Hess’s Law to determine unknown processes in the formation of an ionic compound given appropriate datar) state and explain the effect of ionic charge and radius on the magnitude of lattice energy

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Rates of reactions (Module 2)a) states conditions needed for a reaction to occurb) state and explain factors that affect rates of reactions (include simple experiments that could study the effects of any factor)c) explain necessity of knowledge of reaction rates e.g. keeping food in fridge to last longer, manufacture of chemicals in shortest possible timed) define and describe the terms in relation to reaction rates:- rate constant, order of reaction, half-life, rate determining step, activation energy, collision theory, catalysis e) state and explain different types of catalysis (homogeneous and heterogeneous)f) illustrate zero, first and second order reactions graphicallyg) determine the order of a reaction using supplied data h) construct rate equations for zero, first and second order reactions using data supplied from experimentsi) use order of reactions to deduce possible reaction mechanismsj) interpret concentration vs time and concentration vs rate for zero and first order reactionsk) calculate initial rates and rate constants using rate datal) perform calculations using half-life datam) state and explain the effect of temperature and catalysts on the rate of a reaction (use Boltzman distribution curve and collision frequency)

Principles of Chemical Equilibrium (Module 2)a) explain the term equilibrium in a chemical reaction

CAPE Chemistry Syllabus UNIT 1 page 5 of 9b) state differences between static and dynamic equilibriumc) state 4 characteristics of dynamic equilibrium d) define terms K, Kc and Kp (write equilibrium constant expressions)e) perform calculations involving Kc and Kp

f) state Le Chatelier’s principle and apply it to explain effect of changes in temperature, concentration and pressure on a system in equilibriumg) state and explain how changes in concentration, pressure, temperature or a catalyst would affect the value of the equilibrium constant (use Haber and Contact processes as example)

Acid/Base Equilibrium (Module 2)a) define the terms strong and weak for acids and bases using Bronsted-Lowry theoryb) define the terms Ka, Kb, pH, pKa, pKb, Kw, pKw

c) perform calculations involving Ka, Kb, pH, pKa, pKb, Kw, pKw

d) sketch pH changes during various types of acid-base titrationse) describe and explain pH changes of an indicator (use methyl orange and phenolphthalein as examples)f) state basis of choice of indicator for use in a titration g) show and explain the effectiveness of different indicators in titrations

Buffers and pH (Module 2)a) define the term buffer solutionb) explain how buffer solutions control pHc) calculate the pH of buffer solutions from appropriate datad) describe simple experiments on how to determine the pH of buffer solutionse) state the buffer systems in blood (hydrogen carbonate, phosphate and amino acids) and the importance of presence of buffer systems in biological systemsf) state how exercise can change the pH of bloodg) state and explain how the buffer systems in blood control pH during various levels of exerciseh) explain importance of buffer systems in industrial processes e.g. enzyme catalysed reactions and food processing industry

Solubility Product (Module 2)

CAPE Chemistry Syllabus UNIT 1 page 6 of 9a) define the term solubility product (write the Ksp expression for any given sparingly soluble salt)b) state and explain principles underlying solubility productc) state the relationship between Le Chatelier’s Principle and the common ion effectd) describe how common ion effect can be illustrated via experimentatione) perform calculations involving solubility productf) describe how to determine the solubility product of a substanceg) relate solubility product principle to qualitative analysis and kidney stone formation

Redox Equilibrium (Module 2)a) define the terms standard electrode potential and standard cell potentialb) describe, sketch and label a diagram of the standard hydrogen electrodec) describe methods used to measure the standard electrode potentials of:- metals or non-metals in contact with their ions in aqueous solution and ions of the same element in different oxidation states (include labelled diagrams of electrochemical cells)d) be able to calculate standard cell potentials from standard electrode potentials of two half cellse) use standard electrode potentials of cells to determine:- the direction of electron flow and the feasibility of a reaction (include cell diagram or notation of the type Zn (s)| Zn2+ (aq) || Cu2+ (aq) | Cu (s)f) predict how the value of an electrode potential varies with concentration (apply Le Chatelier’s Principle)g) apply the principles of redox processes to energy storage devices (include references to batteries and fuel cells)

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Period Sodium to Argon (Module 3)

CAPE Chemistry Syllabus UNIT 1 page 7 of 9a) explain the variation in physical properties of the elements in terms of structure and bonding (include reference to melting point, electrical conductivity, atomic radii, electronegativity and densityb) describe the reactions of the elements with oxygen, chlorine and water (no treatment of peroxides and superoxides required)c) explain the variation in oxidation number of the oxides and chloridesd) describe the reactions of the oxides chlorides in watere) explain the trend in the acid/base behaviour of the oxides and hydroxidesf) predict the types of chemical bonding present in the chlorides and oxides (refer to differences in electronegativities and ionic radii of the elements)

Group II elements (Module 3)a) explain the variations in properties of the elements in terms of structure and bonding (include reference to atomic and ionic radii and ionisation energies)b) describe the reactions of the elements with oxygen, water and dilute acidsc) explain the variation in the solubility of the sulphates (refer to lattice and hydration energies)d) explain the variation in the thermal decomposition of the carbonates and nitratese) discuss the uses of some of the compounds of magnesium and calcium ( limited to the use of magnesium oxide, calcium oxide, calcium hydroxide and calcium carbonate)

Group IV elements (Module 3)a) explain the variation in physical properties of the elements in terms of structure and bonding ( refer to variations in metallic character and electrical conductivity)b) describe the bonding of the tetrachloridesc) explain the reactions of the tetrachlorides with waterd) discuss the trends in:- (i) bonding (ii) acid/base character (iii) thermal stability of the oxides of oxidation states II and IV (make reference to Eө values of the elements)e) discuss the uses of ceramics based on silicon(IV) oxide

Group VII elements (Module 3)

CAPE Chemistry Syllabus UNIT 1 page 8 of 9a) explain the variations in physical properties of the elements in terms of structure and bonding (refer to volatility, density, state, only a description of the colour is required)b) explain the relative reactivities of the elements as oxidising agents (include reactions with sodium thiosulphate and refer to Eө values, also use solutions of the elements with bleach, bromine water and iodine solution)c) describe the reactions of the elements with hydrogend) explain the relative stabilities of the hydrides (include reference to bond energies)e) describe the reactions of the halide ions with:- (i) aqueous solution of AgNO3 followed by aqueous ammonia (ii) conc. sulphuric acidf) describe the reactions of chlorine with cold and with hot aqueous solution of sodium hydroxide (mention changes in oxidation number)

First Row Transition Metals Module 3)a) describe the characteristics of transition elements ( include variation in oxidation number, complex formation, coloured compounds, catalytic activity, magnetic properties)b) determine the electronic configuration of the first row of transition elements and of their ions (include mention of changes in oxidation number)c) explain the relatively small changes in atomic radii, ionic radii and ionisation energies of the elements across the periodd) explain the formation of coloured ions by transition elements (refer to d orbital separation of energy in octahedral complexes)e) describe the variation in oxidation states of vanadium (include the use of an acidified solution of ammonium vanadate(V) and granulated zinc)f) discuss qualitatively the properties of a transition element when compared to those of calcium as a typical s-block element (refer to melting point, density, atomic radius, ionic radius, first ionisation energy and conductivity)g) predict the shapes of complexes of transition elements (refer to octahedral, tetrahedral and square planar)h) discuss the use of Fe2+ (aq)/Fe3+ (aq), MnO4

- (aq)/ Mn2+ (aq), Cr2O72-

(aq)/ Cr3+ (aq) as redox systemsi) explain the principle of ligand exchange (refer to stability constants and the CO/O2 haemoglobin and NH3 (aq)/Cu2+ (aq) systems)j) describe the process of ligand exchange with reference to Co2+ (aq) and Cu2+ (aq)Identification of Cations and Anions (Module 3)

CAPE Chemistry Syllabus UNIT 1 page 9 of 9a) identify the cations K+, Na+, Ca2+, Ba2+, Cu2+ by their flame tests (refer to atomic emission spectra in Module 1b) identify aqueous cations Mg2+, Al3+, Ca2+, Cr3+, Mn2+, Fe2+, Fe3+, Cu2+, Zn2+, Ba2+, Pb2+, NH4

+ (include reactions with OH- (aq), CO32- (aq) and

NH3 (aq) and confirmatory tests)c) explain the principles upon which the reactions are based (refer to basic oxides, amphoteric oxides and complexation)d) write ionic equations for the reactions of the cationse) identify anions CO3

2-, NO3-, SO4

2-, SO32-, Cl-, Br-, I-, CrO4

2- (include the reactions with HCl, conc. H2SO4, Pb2+ (aq), Ag+ (aq) followed by NH3 (aq), Ca(OH)2 (aq), Ba2+ (aq) followed by dilute acid. For NO3

- use copper turnings and conc H2SO4 or add aluminium powder or zinc powder in the alkaline solution and confirmatory tests for gases where applicablef) write ionic equations with state symbols for the reactions of then anions

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