962 Chemistry [PPU] Semester 2 Topics-Syllabus
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Transcript of 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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7.4 The solubility of
solids in liquids
2 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
8.1 Half-cell and redox
equations
26
2
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) 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
3 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.
Eº cell
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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
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) describe the electroplating of coated plastics.
9 Periodic Table: Periodicity
9.1 Physical properties of
elements of Period 2
and Period 3
10
5
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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(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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10.2 Anomalous behaviour
of beryllium
2
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 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.
11.4 Silicon, silicone and
silicates
1 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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(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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13 Transition Elements
13.1 Physical properties of
first row transition
elements
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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(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
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
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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