962 Chemistry [PPU] Semester 2 Topics-Syllabus

[PPU] Semester 2 Topics-Syllabus

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962CHEMISTRY

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SECOND TERM

Topic Teaching

Period Learning Outcome

7 Chemical Energetics

7.1 Enthalpy changes of

reaction, H

18

6

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 Teaching


7.4 The solubility of

solids in liquids


(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

8.1 Half-cell and redox

equations

26

2


(a) explain the redox processes and cell diagram

(cell notation) of the Daniell cell;

(b) construct redox equations.

8.2 Standard electrode

potential


(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) predict the feasibility of a reaction from

value and from the combination of various

electrode potentials: spontaneous and non-

spontaneous electrode reactions.

8.3 Non-standard cell

potentials


(a) calculate the non-standard cell potential, Ecell,

of a cell using the Nernst equation.

8.4 Fuel cells


(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.

Eº cell


Topic Teaching


8.5 Electrolysis 6 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


(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) describe the electroplating of coated plastics.

9 Periodic Table: Periodicity

9.1 Physical properties of

elements of Period 2

and Period 3

10

5


(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;


Topic Teaching


(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


(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


(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


(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.


Topic Teaching


10.2 Anomalous behaviour

of beryllium

2


(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


(a) state the uses of Group 2 compounds in

agriculture, industry and medicine.

11 Group 14


Group 14 elements

10

2


(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


(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


(a) explain the relative stability of +2 and +4

oxidation states of the elements in their oxides,

chlorides and aqueous cations.

11.4 Silicon, silicone and

silicates


(a) describe the structures of silicone and silicates

(pyroxenes and amphiboles), sheets (mica) and

framework structure (quartz) (general formulae

are not required);


Topic Teaching


(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


selected Group 17

elements

8

1


(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


(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


(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


(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.


Topic Teaching


13 Transition Elements


first row transition

elements

14

2


(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


(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

;


Topic Teaching


(i) explain the use of first row transition elements

in heterogeneous catalysis, as exemplifed by

Ni and Pt in the hydrogenation of alkenes.

13.3 Nomenclature and

bonding of complexes

3


(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


(a) describe the use of chromium (in stainless

steel), cobalt, manganese, titanium (in alloys)

and TiO2 (in paints).


962 Chemistry [PPU] Semester 2 Topics-Syllabus

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