LEARNING OBJECTIVE

LEARNING OBJECTIVE TUTORIAL DK014

1.0  MATTER

1.1 Definition and Classification

1.1(a) Define matter

1.1(b) Classify matter into pure substances (elements and compounds) and mixtures (homogeneous and heterogeneous)

1.2 States Of Matter

1.2(a)Explain the general properties of solid, liquid and gas in terms of arrangement of particles , shape, density and compressibility.

Experiment 1: Determination of the density of water

1.3 Elements

1.3(a)Define element

1.3(b) Introduce the period and group of elements in the periodic table. (Limited to group 1, 2 and 13 to 18)

1.4 Physical And Chemical Changes

1.4(a) i)Describe the physical and chemical changes of matter. Physical change : Change in physical state but not in composition.

1.4(a)ii)Chemical change : formation of new substance through chemical reaction.

2.0  ATOMS, MOLECULES AND IONS

2.1 Proton Number, Nucleon Number And Isotope.

2.1(a) Describe proton, electron and neutron as sub-atomic particles.)

2.1(b) Define proton number (Z), nucleon number (A) and isotope.

2.1(c) Write isotope notation

2.1(d) State the limitation of Bohr's atomic model.

2.2 Atomic And Molecular Masses

2.2 (a) define relative atomic mass (A.) and relative molecular mass (M.) based on the C-12 scale.

2.3 Nomenclature Of Inorganic Compound

2.3 (a) Define cations and anions.

2.3 (b) Name cations, anions and salts according to IUPAC nomenclature. Include polyatomic ion,

e.g. P043-, S042+ , NH4+ etc. Exclude complex ions.

3.0  MOLE CONCEPT

3.1 Avogadro Number And Molar Mass

3.1(a) Define mole in terms of mass of carbon-12 and Avogadro 's constant (NA).

3.1(b) Relate Avogadro's number with molar mass and molar volume of gas at s.t.p.

3.2 Empirical And Molecular Formula

a) Define the term empirical and molecular formulae

b) Determine empirical and molecular formulae from mass composition or combustion

3.3 Concentration

3.3(a) Define molarity

3.3(b) Perform calculations on molarity.

4.0  CHEMICAL EQUATION AND STOICHIOMETRY

4.1 Chemical Equation

4.1(a) Determine the oxidation number of an element in a chemical formula.

4.1(b) i) write and balance chemical equation by inspection method.

4.1(b) ii) write and balance redox equation by ion-electron method

4.2 Stoichiometry

4.2(a)Stoichiometric mass calculation: calculate the amount of reactant and product from a balanced chemical equation.

4.2(a)i) Calculation involve: Reacting masses and moles

4.2(a)ii) Calculation involve: Volume of gases at s.t.p.(e.g. combustion of hydrocarbon

4.2(a)iii) Calculation involve: Volume and concentration of solutions

Experiment 2: Standard solution and determination of the concentration of acid solution

Experiment 3: Quantitative analysis of baking soda

4.2(b)i) Define limiting reactant

4.2(b)ii) theoretical and actual yield

4.2(b)iii) percentage yield.

4.2(c) Perform calculation involving limiting reactant and percentage yield.

5.0  ELECTRONIC CONFIGURATION

5.1 Quantum Numbers Of Electrons

5.1(a) Define the term orbital.

5.1(b) state and describe all the four quantum numbers of an electron in an orbital:

5.1(b)i) principal quantum number (n)

5.1(b)ii) angular momentum quantum number (l)

5.1(b)iii) magnetic quantum number (m)

5.1(b)iv) iv. electron spin quantum number (s)

( Other terms for l are azimuthal or subsidiary quantum number)

5.1(c) Sketch and describe the shapes of s, p and d orbitals with correct orientation.

5.2 Electronic Configuration Of Atom

5.2(a) State aufbau principle, Hund's rule and Pauli's Exclusion Principle .

5.2(b) Apply the rules in (a) to fill electrons into atomic orbitals.

5.2(c) Write the electronic configuration of atoms and monatomic ions using spdf notation .

Limit the proton number (Z) to 23 (exclude the anomalous cases of chromium and copper)

6.0  PERIODIC TABLE

6.1 Classification  Of Element

6.1(a) Specify periods, groups and blocks (s,p,d f)

6.1(b) Deduce the position elements in the periodic table from the elentronic configuration

6.2 Trends in some key periodic atomic properties

6.2(a) Explain the variation in atomic and ionic radii across periods 2 and 3. Include effective nuclear charge. exclude the comparison of radii of isoelectronic ions

6.2(b) Define electronegativity and first ionisation energy.

6.2(c) Explain the variation in electronegativity and ionisation energy of elements across period 2 and 3.

Exclude the irregulation of the first ionisation energy between Be and Band  Nand  0.

6.2(d) Compare and explain the size of cation and anion with the corresponding atom.

7.0 Chemical Bonding

7.1 Valence Electron And Lewis Structure

7.1(a) Write the Lewis dot symbol of an atom.

Relate valence electron with Lewis dot symbol

7.1    (b) State the octet rule. Describe how atoms obtain the octet configuration.

7.1  (c) Describe the formation of the following bonds using Lewis symbol.

7.1    (c) i. Ionic or electrovalent bond

7.1  (c) ii. Covalent bond

7.1  (c) iii. Dative or coordinate bond

(Include the explanation in terms of difference in electronegativity. Use only elements of period 2 except Be and H)

7.1(d) Draw Lewis structure of covalent species with single, double and triple bonds.

7.1(e) Determine the formal charge and the most plausible Lewis structure.

7.1(f) Explain the exception to the octet rule : incomplete octet, expanded octet and odd number electrons.

7.2 Molecular Shape

7.2(a) Explain Valence Shell Electron Pair Repulsion Theory (VSEPR)

7.2(b)Draw the basic molecular shapes: liner,trigonal planar, tetrahedral, trigonal bipyramidal and octahedral

7.2(c)Predict and explain the shape of molecule and bond angle in a given species.

7.3 Intermolecular forces

7.3 (a) Explain polarity and dipole moment in linear molecules

7.3 (b) Introduce intermolecular forces

7.3 (b) (i) Van der waals forces

·         Dipole-dipole interactions or permanent dipole

·         London forces or dispersion forces

7.3 (b) (ii) Hydrogen bond

8.0  Chemical Equilibrium

8.1  Dynamic Equilibrium

8.1(a)  Explain a reversible reaction.

8.1(b) State the characteristics of a dynamic equilibrium system and law of mass action or law of chemical equilibrium

8.1(c) Explain the significant figures of a graph of concentration against time for a reversible reaction

8.2 Equilibrium Constant,Kc And Kp

8.2(a)  Define homogeneous and heterogeneous equilibria

8.2(b)  Deduce and write expressions for equilibrium constant in terms of concentration, Kc and partial pressure, Kp for homogeneous and heterogeneous system

Refer to single step reversible only

8.2(c) Calculate Kc, Kp or quantities of species present at equilibrium. (Calculations are limited to problems with quadratic equation only)

9.0  Reaction Kinetic

9.1  Rate of reaction

9.1(a)  Define reaction rate

9.1(b)  Determine the reaction rate based on

9.1 (b) (i) Experimental data given

9.1 (b)(ii) The graph of concentration against time

differential rate equation of a reaction

9.1(c) Write the rate expression in the form of:

9.1 (c) (i) differential rate equation

9.1 (c) (ii) rate law.

(Rate Law= rate equation)

9.1(d) Define order of reaction

9.1(e) Determine reaction rate based on:

9.1 (e) (i) differential rate equation

9.1 (e) (ii) Rate Law

9.1 (f)Determine the order of reaction by initial rate method

9.2 Factor that  affect the following factors on the reaction rate

9.2 (a) Factor that  affect the following factors on the reaction rate:

9.2 (a)  (i) concentration or pressure

9.2 (a) (ii) temperature

9.2 (a) (iii) particle size