962 Chemistry [PPU] Semester 2 Topics-Syllabus

[PPU] Semester 2 Topics-Syllabus

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SECOND TERM Topic 7

Teaching Period

Chemical Energetics

18

7.1

6

Enthalpy changes of reaction, H

Learning Outcome

Candidates should be able to: (a) explain that most chemical reactions are accompanied by enthalpy changes (exothermic or endothermic); (b) define enthalpy change of reaction, H, and state the standard conditions; (c) define enthalpy change of formation, combustion, hydration, solution, neutralisation, atomisation, bond energy, ionisation energy and electron affinity; (d) calculate the heat energy change from experimental measurements using the relationship: heat change, q mc T or q = mc ; (e) calculate enthalpy changes from experimental results.

7.2

Hess‟ law

6

Candidates should be able to: (a) state Hess‟ law, and its use to find enthalpy changes that cannot be determined directly, e.g. an enthalpy change of formation from enthalpy changes of combustion; (b) construct energy level diagrams relating the enthalpy to reaction path and activation energy; (c) calculate enthalpy changes from energy cycles.

7.3

Born-Haber cycle

4

Candidates should be able to: (a) define lattice energy for simple ionic crystals in terms of the change from gaseous ions to solid lattice; (b) explain qualitatively the effects of ionic charge and ionic radius on the numerical magnitude of lattice energy values; (c) construct Born-Haber cycle for the formation of simple ionic crystals.

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Topic 7.4

The solubility of solids in liquids

Teaching Period 2

Learning Outcome Candidates should be able to: (a) construct energy cycles for the formation of aqueous solutions of ionic compounds; (b) explain qualitatively the influence on solubility of the relationship between enthalpy change of solution, lattice energy of solid and enthalpy change of hydration or other solvent-solute interaction.

8

Electrochemistry

26

8.1

2

Half-cell and redox equations

Candidates should be able to: (a) explain the redox processes and cell diagram (cell notation) of the Daniell cell; (b) construct redox equations.

8.2 Standard electrode potential

9

Candidates should be able to: (a) describe the standard hydrogen electrode; (b) use the standard hydrogen electrode to determine standard electrode potential (standard reduction potential), Eº; (c) calculate the standard cell potential using the Eo values, and write the redox equations; (d) predict the stability of aqueous ions from Eº values; (e) predict the power of oxidising and reducing agents from Eº values; (f)

8.3

Non-standard cell potentials

3

predict the feasibility of a reaction from Eºcell value and from the combination of various electrode potentials: spontaneous and nonspontaneous electrode reactions.

Candidates should be able to: (a) calculate the non-standard cell potential, Ecell, of a cell using the Nernst equation.

8.4

Fuel cells

2

Candidates should be able to: (a) describe the importance of the development of more efficient batteries for electric cars in terms of smaller size, lower mass and higher voltage, as exemplified by hydrogen-oxygen fuel cell.

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8.5

Topic

Teaching Period

Electrolysis

6

Learning Outcome Candidates should be able to: (a) compare the principles of electrolytic cell to electrochemical cell; (b) predict the products formed during electrolysis; (c) state the Faraday‟s first and second laws of electrolysis; (d) state the relationship between the Faraday constant, the Avogadro constant and the electronic charge; (e) calculate the quantity of electricity used, the mass of material and/or gas volume liberated during electrolysis.

8.6

Applications of electrochemistry

4

Candidates should be able to: (a) explain the principles of electrochemistry in the process and prevention of corrosion (rusting of iron); (b) describe the extraction of aluminium by electrolysis, and state the advantages of recycling aluminium; (c) describe the process of anodisation of aluminium to resist corrosion; (d) describe the diaphragm cell in the manufacture of chlorine from brine; (e) describe the treatment of industrial effluent by electrolysis to remove Ni2+, Cr3+ and Cd2+; (f)

9

Periodic Table: Periodicity

10

9.1

5

Physical properties of elements of Period 2 and Period 3

describe the electroplating of coated plastics.

Candidates should be able to: (a) interpret and explain the trend and gradation of atomic radius, melting point, boiling point, enthalpy change of vaporisation and electrical conductivity in terms of structure and bonding; (b) explain the factors influencing ionisation energies; (c) explain the trend in ionisation energies across Period 2 and Period 3 and down a group;

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Topic

Teaching Period

Learning Outcome (d) predict the electronic configuration and position of unknown elements in the Periodic Table from successive values of ionisation energies.

9.2

Reactions of Period 3 elements with oxygen and water

2

Candidates should be able to: (a) describe the reactions of Period 3 elements with oxygen and water; (b) interpret the ability of elements to act as oxidising and reducing agents.

9.3

Acidic and basic properties of oxides and hydrolysis of oxides

3

Candidates should be able to: (a) explain the acidic and basic properties of the oxides of Period 3 elements; (b) describe the reactions of the oxides of Period 3 elements with water; (c) describe the classification of the oxides of Period 3 elements as basic, amphoteric or acidic based on their reactions with water, acid and alkali; (d) describe the use of sulphur dioxide in food preservation.

10 Group 2 10.1 Selected Group 2 elements and their compounds

10 7

Candidates should be able to: (a) describe the trends in physical properties of Group 2 elements: Mg, Ca, Sr, Ba; (b) describe the reactions of Group 2 elements with oxygen and water; (c) describe the behaviour of the oxides of Group 2 elements with water; (d) explain qualitatively the thermal decomposition of the nitrates, carbonates and hydroxides of Group 2 elements in terms of the charge density and polarisability of large anions; (e) explain qualitatively the variation in solubility of sulphate of Group 2 elements in terms of the relative magnitudes of the enthalpy change of hydration for the relevant ions and the corresponding lattice energy.

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Topic 10.2 Anomalous behaviour of beryllium

Teaching Period 2

Learning Outcome Candidates should be able to: (a) explain the anomalous behaviour of beryllium as exemplified by the formation of covalent compounds; (b) describe the diagonal relationships between beryllium and aluminium; (c) explain the similarity of aqueous beryllium salts to aqueous aluminium salts in terms of their acidic property.

10.3 Uses of Group 2 compounds

1

Candidates should be able to: (a) state the uses of Group 2 compounds in agriculture, industry and medicine.

11 Group 14 11.1 Physical properties of Group 14 elements

10 2

Candidates should be able to: (a) explain the trends in physical properties (melting points and electrical conductivity) of Group 14 elements: C, Si, Ge, Sn, Pb.

11.2 Tetrachlorides and oxides of Group 14 elements

4

Candidates should be able to: (a) explain the bonding and molecular shapes of the tetrachlorides of group 14 elements; (b) explain the volatility, thermal stability and hydrolysis of tetrachlorides in terms of structure and bonding; (c) explain the bonding, acid-base nature and the thermal stability of the oxides of oxidation states +2 and +4.

11.3 Relative stability of +2 and +4 oxidation states of Group 14 elements

2

11.4 Silicon, silicone and silicates

1

Candidates should be able to: (a) explain the relative stability of +2 and +4 oxidation states of the elements in their oxides, chlorides and aqueous cations. Candidates should be able to: (a) describe the structures of silicone and silicates (pyroxenes and amphiboles), sheets (mica) and framework structure (quartz) (general formulae are not required);

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Topic

Teaching Period

Learning Outcome (b) explain the uses of silicon as a semiconductor and silicone as a fluid, elastomer and resin; (c) describe the uses of silicates as basic materials for cement, glass, ceramics and zeolites.

11.5 Tin alloys

1

Candidates should be able to: (a) describe the uses of tin in solder and pewter.

12 Group 17 12.1 Physical properties of selected Group 17 elements

8 1

Candidates should be able to: (a) state that the colour intensity of Group 17 elements: Cl2, Br2, I2, increase down the group; (b) explain how the volatility of Group 17 elements decreases down the group.

12.2 Reactions of selected Group 17 elements

4

Candidates should be able to: (a) deduce and explain the relative reactivities of Group 17 elements as oxidising agents from Eº values; (b) explain the order of reactivity of F2, Cl2, Br2, I2 with hydrogen, and compare the relative thermal stabilities of the hydrides; (c) explain the reactions of chlorine with cold and hot aqueous sodium hydroxide.

12.3 Reactions of selected halide ions

2

Candidates should be able to: (a) explain and write equations for reactions of Group 17 ions with aqueous silver ions followed by aqueous ammonia; (b) explain and write equations for reactions of Group 17 ions with concentrated sulphuric acid.

12.4 Industrial applications of halogens and their compounds

1

Candidates should be able to: (a) describe the industrial uses of the halogens and their compounds as antiseptic, bleaching agent and in black-and-white photography; (b) explain the use of chlorine in water treatment.

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Topic 13 Transition Elements 13.1 Physical properties of first row transition elements

Teaching Period

Learning Outcome

14 2

Candidates should be able to: (a) define a transition element in terms of incomplete d orbitals in at least one of its ions; (b) describe the similarities in physical properties such as atomic radius, ionic radius and first ionisation energy; (c) explain the variation in successive ionisation energies; (d) contrast qualitatively the melting point, density, atomic radius, ionic radius, first ionisation energy and conductivity of the first row transition elements with those of calcium as a typical s-block element.

13.2 Chemical properties of first row transition elements

8

Candidates should be able to: (a) explain variable oxidation states in terms of the energies of 3d and 4s orbitals; (b) explain the colours of transition metal ions in terms of a partially filled 3d orbitals; (c) state the principal oxidation numbers of these elements in their common cations, oxides and oxo ions; (d) explain qualitatively the relative stabilities of these oxidation states; (e) explain the uses of standard reduction potentials in predicting the relative stabilities of aqueous ions; (f)

explain the terms complex ion and ligand;

(g) explain the formation of complex ions and the colour changes by exchange of ligands. (Examples of ligands: water, ammonia, cyanide ions, thiocyanate ions, ethanedioate ions, ethylenediaminetetraethanoate, halide ions; examples of complex ions: [Fe(CN)6]4 , [Fe(CN)6]3 , [Fe(H2O)5(SCN)]2+); (h) explain the use of first row transition elements in homogeneous catalysis, as exemplifed by Fe2+ or Fe3+ in the reaction between I and S2O82 ;

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Topic

Teaching Period

Learning Outcome (i)

13.3 Nomenclature and bonding of complexes

3

explain the use of first row transition elements in heterogeneous catalysis, as exemplifed by Ni and Pt in the hydrogenation of alkenes.

Candidates should be able to: (a) name complexes using International Union of Pure and Applied Chemistry (IUPAC) nomenclature; (b) discuss coordinate bond formation between ligands and the central metal atom/ion, and state the types of ligands, i.e. monodentate, bidentate and hexadentate.

13.4 Uses of first row transition elements and their compounds

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1

Candidates should be able to: (a) describe the use of chromium (in stainless steel), cobalt, manganese, titanium (in alloys) and TiO2 (in paints).

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