hssci ii chemistry

Higher Secondary School Certificate Examination Syllabus

CHEMISTRY

CLASSES XI-XII

Published by Aga Khan University-Examination Board

Bungalow # 233/E.1, Daudpota and Raja Ghazanfar Ali Khan Roads,

Behind Hotel Mehran, Off Sharae Faisal, Karachi, Pakistan.

September 2008

Higher Secondary School Certificate Examination Syllabus

CHEMISTRY

CLASSES XI-XII

S. No. Contents Page No.

Preface 5

1. Topics and Specific Learning Objectives of the Examination Syllabus

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2. Scheme of Assessment 61

3. Teaching-Learning Approaches 64

4. Areas for Development of Learning Support Materials 64

5. Recommended Texts, Reference Books 64

6. Definition of Cognitive Levels and Command Words in the Specific Learning Objectives and in Examination Papers

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Annex A: HSSC Scheme of Studies 68

Annex B: List of Practical Activities 73

For queries and feedback Address: AKU-Examination Board

Bungalow No. 233/E.I. Lines Daudpota and Raja Ghazanfar Ali Khan Roads, Behind Hotel Mehran, Karachi-Pakistan.

Phone: (92-21) 5224702-09 Fax: (92-21) 5224711 E-mail: [email protected] Website: www.aku.edu/akueb/

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PREFACE In pursuance of National Education Policy (1998-2010), the Curriculum Wing of the Federal Ministry of Education has begun a process of curriculum reform to improve the quality of education through curriculum revision and textbook development (Preface, National Curriculum documents 2000 and 2002). AKU-EB was founded in August 2003 with the same aim of improving the quality of education nationwide. As befits an examination board it seeks to reinforce the National Curriculum revision through the development of appropriate examinations for the Secondary School Certificate (SSC) and Higher Secondary School Certificate (HSSC) based on the latest National Curriculum and subject syllabus guidance. AKU-EB has a mandate by Ordinance CXIV of 2002 to offer such examination services to English and Urdu medium candidates for SSC and HSSC from private schools anywhere in Pakistan or abroad, and from government schools with the relevant permissions. It has been accorded this mandate to introduce a choice of examination and associated educational approach for schools, thus fulfilling a key objective of the National Curriculum of Pakistan: “Autonomy will be given to the Examination Boards and Research and Development cells will be established in each Board to improve the system” (ibid. para. 6.5.3 (ii)). AKU-EB is committed to creating continuity of educational experience and the best possible opportunities for its students. In consequence it offered HSSC for the first time in September, 2007 to coincide with the arrival of its first SSC students in college or senior secondary school. Needless to say this is not an exclusive offer. Private candidates and students joining AKU-EB affiliated schools and colleges for HSSC Part 1 are eligible to register as AKU-EB candidates even though they have not hitherto been associated with AKU-EB. This examination syllabus exemplifies AKU-EB’s commitment to national educational goals. o It is in large part a reproduction, with some elaboration, of the Class XI and XII

National Syllabus of the subject. o It makes the National Syllabus freely available to the general public. o The syllabus recommends a range of suitable textbooks already in print for student

purchase and additional texts for the school library. o It identifies areas where teachers should work together to generate classroom activities

and materials for their students as a step towards the introduction of multiple textbooks, another of the Ministry of Education’s policy provisions for the improvement of secondary education (ibid. para. 6.3.4).

This examination syllabus brings together all those cognitive outcomes of the National Curriculum statement which can be reliably and validly assessed. While the focus is on the cognitive domain, particular emphasis is given to the application of knowledge and understanding, a fundamental activity in fostering “civilized behaviour, attitudes befitting useful and peaceful citizens and the skills for and commitment to lifelong learning which is

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the cornerstone of national economic development” (Preface to National Curriculum documents 2000 and 2002). To achieve this end AKU-EB has brought together university academicians, teacher trainers, writers of learning materials and above all, experienced teachers, in regular workshops and panel meetings. AKU-EB provides copies of the examination syllabus to subject teachers in affiliated schools to help them in planning their teaching. It is the syllabus, not the prescribed textbook which is the basis of AKU-EB examinations. In addition, the AKU-EB examination syllabus can be used to identify the training needs of subject teachers and to develop learning support materials for students. Involving classroom teachers in these activities is an important part of the AKU-EB strategy for improving the quality of learning in schools. The Curriculum Wing of the Federal Ministry of Education has recently released new subject specifications and schemes of study to take effect in September, 2008. These documents are a major step forward towards a standards-related curriculum and have been welcomed by AKU-EB. Our current HSSC syllabuses have been revised to ensure conformity with the new National Curriculum 2006. We stand committed to all students who have embarked upon the HSSC courses in facilitating their learning outcomes. Our examination syllabus document ensures all possible support.

Dr. Thomas Christie Director, Aga Khan University Examination Board September 2008

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1. Topics and Specific Learning Outcomes of the Examination Syllabus

Part –I (Class XI)

Cognitive Level1 Topics Specific Learning Objectives

K U A 1. Stoichiometry

1.1. Mole and Avogadro’s

Number 1.2. Mole Calculation 1.3. Percentage Composition 1.4. Excess and Limiting

reagent

Candidates should be able to: 1.1.1 define moles concept with the help of Avagadro’s Number; 1.1.2 define moles and Avagadro’s Number; 1.1.3 calculate the number of moles of substance; 1.1.4 interpret balance chemical equation in terms of interacting moles,

representative particle, masses and volume of gases at STP (22.4 L); 1.2.1 calculate mole ratio from balance equation for use as conversion factors in

stoichiometric problems; 1.3.1 calculate % (percentage) by mass of elements in compounds; 1.4.1 identify limiting reagent in reactions; 1.4.2 calculate maximum amount of product produced and amount of any

excess reagent, knowing the limiting reagent in reaction; 1.4.3 calculate the gram molecular mass of a gas from density measurement of

gases at STP;

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1 K = Knowledge, U = Understanding, A= Application (for explanation see section 8: Definition of command words used in Specific Learning Objectives and in Examination Questions).

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1.5 Chemistry as a Quantitative Science

1.6. Theoretical and Actual

yield

1.5.1 list down the significance of chemistry as quantitative science in daily life;

1.6.1 Differentiate between actual yield, % age yield and theoretical yield; 1.6.2 Calculate the percentage yield of a product in a given reaction.

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2. Atomic Structure 2.1 Discharge tube experiment 2.2 Application of Bohr’s

model 2.3 Plank’s quantum theory. 2.4 X-Rays and Atomic

Number

Candidates should be able to: 2.1.1 construction, working of discharge tube and its consequences; 2.2.1 concept of Bohr’s model to calculate the radius and energy n the orbits; 2.2.2 explain spectrual line of Hydrogenatom; 2.2.3 explain the significance sepectred line with reference to laseu and from

daily life; 2.2.4 calculate the radius and energy of nth orbital w.r.t Bohr’s model (w.r.t

hydrogen atom); 2.3.1 using Plank’s theory interpreter relation between energy frequency and

wave length; 2.4.1 describe the Mosley’s experiment with reference to X-rays; 2.4.2 explain the production, properties, types and uses of X-rays; 2.4.3 explain use of x-rays, production and properties.

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2.5 Quantum number and orbitals / Hersen berg

2.5.1 describe the concepts of orbitals on the basis of uncertainty principal; 2.5.2 compare orbit and orbital; 2.5.3 apply the concept of quantum number for the position of electron/for distribution of electron;

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K U A 2.6 Dual nature of electron 2.6.1 explain the dual nature of electron with reference to De-borgliy equation;

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2.7 Electronic configuration 2.7.1 state the following rules of Electronic configuration (sufban, Hurd’s, and Pauli’s exclusion);

2.7.2 write correct electronic configuration based on above rules.

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3. Theories of Covalent bonding and Shape of Molecules

3.1. Shape of Molecular Resonance 3.2 Theories of Covalent

bonding 3.2 VBT and hybridization

Candidates should be able to: 3.1.1 discuss the postulate of VSEPR; 3.1.2 use VSEPR theory to describe the shape of simple covalent molecular; 3.1.3 explain the phenomenon of resonance with reference to Sp2 hybrid

orbital; 3.2.1 compare V.B.T and M.O.T; 3.2.2 predict the shapes of molecules with the help of M.O.T; 3.2.3 explain hybridization (Sp, Sp2, Sp3, dsp3);

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3.3. Bond Characteristics 3.4. Effect of bonding on

physical and chemical properties

3.3.1 define bond energy; 3.3.2 relate bond energy with bond strength; 3.3.3 define bond length; 3.3.4 explain ionic character of covalent bond; 3.3.5 predict the nature of bonding on the basis of electro negativity; 3.3.6 explain dipole moment; 3.3.7 predict geometry dipole moment of different molecules on the basis of

moleculer theory; 3.4.1 explain the solubility of ionic and covalent compounds on the nature of

bonding; 3.4.2 explain chemical properties of ionic and covalent compound; 3.4.3 compare directional and non-directional nature of ionic and covalent

bonds.

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4. States of Matter: Gases Candidates should be able to: K U A

4.1. Kinetic Molecular Theory of gases

4.2. Absolute Temperature

scale on the basis of Charles’s law

4.3. Avogadro’s law 4.4. Ideal Gas equation

4.1.1 list down the postulate of Kinetic Molecular Theory (K.M.T) of Gases; 4.1.2 state and explain the Gas laws; 4.1.3 describe the gas laws with reference to Kinetic Molecular Theory

(K.M.T); 4.2.1 explain absolute zero on the basis of Charles’s laws; 4.2.2 convert the temperature into different scales; 4.3.1 state and explain the significance of Avog. Law; 4.4.1 derive ideal gas equation; 4.4.2 apply ideal gas equation for calculation of gas co-efficient; 4.4.3 explain the significance of ideal gas equation; 4.4.4 explain the significance of different units of ideal gas constant;

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4.5. Deviation from ideal behaviour.

4.6. Van der Waal’s Equation 4.7. Liquefaction of gases 4.8. Fourth State of water

plasma

4.5.1 explain why gases deviate from their ideal behaviour; 4.5.2 explain the significance of ideal gas equation(using example of pressure

cooker and scuba diver); 4.6.1 drive v an der Waal’s equation; 4.6.2 explain pressure and volume correction for non ideal gases; 4.7.1 explain the liquefaction of gases; 4.8.1 define and explain (properties) of plasma.

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5. States of Matter II liquids Candidates should be able to: K U A

5.1. Kinetic molecular interpretation of liquid

5.2. Intermolecular forces 5.3. Energetic of phase charge 5.4. Liquid Crystals

5.1.1 using kinetic molecular theory explain the term diffusion, compression

expansion motion of molecular, kinetic energy in liquids; 5.2.1 explain Vander Waal’s forces and its types; 5.2.2 explain parameter affecting intermolecular forces; 5.2.3 compare the volatility of different liquids at same temperature based on

inter molecular forces; 5.3.1 define molar heat of fusion heat of vaporization, molar heat of

sublimation; 5.3.2 relate energy change and intermolecular forces; 5.3.3 describe dynamic equilibrium between different physical states of matter; 5.4.1 explain the formation of liquid crystal; 5.4.2 differentiate liquid crystals from pure liquids and crystalline solid; 5.4.3 explain anomalous behaviour of water according to hydrogen bonding; 5.4.4 state the uses of liquid crystals (wrist watches and calculator).

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6. States of Mater III Solids Candidates should be able to: K U A

6.1. Kinetic molecular

interpretation of solids 6.2. Types of solids 6.3. Properties of solids 6.4. Crystal Lattice 6.5. Types of Crystalline Solid

6.1.1 describe simple properties of solid e.g. diffusion, compression, expansion,

motion of molecular spaces between inter molecular forces and kinematics energy with reference to Kinetic molecular theory;

6.2.1 differentiate between crystalline and amorphous solid; 6.2.2 differentiate between isomorphism and polymorphism; 6.2.3 relate polymorphism and allotropy; 6.2.4 define transition temperature; 6.3.1 describe different properties of crystalline solid e.g., symmetry, melting

point, anisotropy, cleavage plane, crystal growth, geometrical shape, habit of crystals;

6.4.1 define unit cell; 6.4.2 explain energy changes in the formation of sodium chloride crystals

lattice; 6.4.3 predict the energy changes for the formation pf MgCl2 and CaCl2 by the

given I.P and E.A value; 6.5.1 differentiate between different types of crystalline solid (ionic, molecular,

metallic, covalent); 6.5.2 list example of crystalline amorphous solid along with their uses in daily

life.

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7. Chemical Equilibrium Candidates should be able to: K U A

7.1. Reversible reaction and

Dynamic Equilibrium 7.2. Factor affecting the

Equilibrium 7.3. Industrial application of

Le-Chateller’s Principle 7.4. Solubility product and

Precipitation reactions 7.5. Common Ion Effect

7.1.1 define reversible reaction; 7.1.2 define equilibrium reaction; 7.1.3 write equilibrium expression for different given reaction; 7.2.1 define Le-Chatelier principle; 7.2.2 explain the conditions favourable for equilibrium (concentration,

temperature, pressure, catalyst) to focus the high yield of industrial products;

7.2.3 recognize the equilibrium state from the given value of Kc; 7.2.4 relate the equilibrium constant with ratio between concentration product

and reactant; 7.3.1 apply Le-Chatler’s principle on different example; 7.3.2 discuss the effect of temperature, pressure and concentration on the

equilibrium state of given reversible reactions; 7.4.1 define the solubility product; 7.4.2 differentiate between solubility and solubility product; 7.4.3 explain why some substances are more soluble and some are less soluble; 7.5.1 define the common ion effect; 7.5.2 discuss common ion effect and its application.

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8. Acid, Base and Salts Candidates should be able to: K U A

8.1. Acids, Bases and

Amphoteric Substances 8.2. Lowery - Bronsted Definitions of Acids and

Bases 8.3. Conjugate Acid and Base 8.4. Strengths of Acids and

Bases 8.5. Lewis concept of acid and

base

8.1.1 define acid, bases and amphoteric compounds; 8.1.2 explain the significance of acid base reaction in daily life (Food

preservation, allergic reactions, importance of iodine in salt, gastric acidity, curdling of milk);

8.1.3 perform acid base titration to calculate molarity and strength of given sample solutions.;

8.2.1 define acids and base on the bases Lowery – Bronsted theory; 8.3.1 define conjugate acid and conjugate base; 8.3.2 compare the strength of conjugate acids and bases; 8.4.1 explain the ionization constant of water (Kw); 8.4.2 compare the strength of acid and base on the bases of pH and pOH; 8.4.3 derive the dissociation constants of acid, base and water (Ka, Kb and

Kw); 8.4.4 calculate the +OH3 concentration by using the given Ka and molar

concentration of weak acid; 8.5.1 define Lewis acids and Lewis bases along with examples; 8.5.2 identify Lewis acid and base from given compounds (e.g. NH3, AlCl3,

BF3);

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K U A

8.6. Buffer Solution 8.7. Hydrolysis / Hydration

8.6.1 define the buffer solution; 8.6.2 state the importance of buffer in daily life; 8.6.3 describe the preparation of different types of buffer; 8.6.4 explain the buffer action to maintain pH of solution (with the help of

equations); 8.6.5 explain levelling effect; 8.7.1 define hydrolysis; 8.7.2 explain the types of salt on the basis of hydrolysis; 8.7.3 differentiate between hydrolysis and hydration; 8.7.4 calculate concentration of ions of slightly soluble salts.

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9. Chemical Kinetics 9.1. Chemical Kinetics 9.2. Rate of Reaction and

Activation Energy

Candidates should be able to: 9.1.1 define chemical kinetics; 9.2.1 explain the relation of speed of reaction with the time; 9.2.2 define the terms like rate of reaction, rate equation, order of reactions, rate

constant and rate determining step; 9.2.3 write the rate law for the given reaction; 9.2.4 relate activation energy and activated complex with the rate of reaction; 9.2.5 calculate the initial rate using concentration data of given reaction; 9.2.6 draw an energy diagram that represents the activation energy and show

the effect of catalyst; 9.2.7 deduce the order of reaction using the method of initial rate;

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K U A

9.3. Collision theory and transition state

9.4. Catalysis

9.3.1 explain the effects of concentration, temperature and surface area on reaction rate by using collision theory;

9.4.1 explain how homogeneous and heterogeneous catalyst work; 9.4.2 explain effect of catalyst on the rate of reaction; 9.4.3 explain the significance of enzymes in daily life (Biological catalyst,

removing stains from fabrics).

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10. Solution and Colloids 10.1. General properties of

solutions

Candidates should be able to: 10.1.1 list the characteristics of colloids and suspension that distinguish these

from solution; 10.1.2 differentiate hydrophilic and hydrophobic molecules; 10.1.3 predict the nature of solution in liquid phase in the given examples (w.r.t

miscible, immiscible, partially miscible solution); 10.1.4 identify the solutions, colloids and suspensions in given examples; 10.1.5 interpret the solubility graph on the basis of temperature for different

solutions; 10.1.6 draw the solubility curves from given experimental data;

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10.2. Concentration Units 10.3. Roult’s Law

10.2.1 calculate the different concentration units (morality, mole fraction, ppm, ppb, ppt) from the given data;

10.3.1 state Roult’s law (all three definitions); 10.3.2 identify volatile and non volatile components of solution by plotting

graph; 10.3.3 draw a graph using Roult’s law from the given data;

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K U A

10.4. Colligative properties

10.4.1 define colligative properties of liquids with examples; 10.4.2 explain lowering of vapour pressure, elevation of boiling point and

depression of freezing point; 10.4.3 calculate molar mass of a substance using ebullioscopic and cryoscopic

methods; 10.4.4 differentiate osmotic pressure and reverse osmosis;

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10.5 Colloids 10.5.1 write down the properties of colloids; 10.5.2 explain the types of colloids.

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11. Thermochemistry 11.1. Thermodynamic 11.2. First law of

thermodynamic

Candidates should be able to: 11.1.1 define thermodynamics; 11.1.2 define the terms, system, surrounding, state function, heat, heat capacity,

internal energy, work, and enthalpy; 11.2.1 state and explain the first law of thermodynamic with the help of daily life

examples; 11.2.2 relate change in internal energy of system with thermal energy at constant

temperature and pressure; 11.2.3 calculate internal energy work done by applying the 1st law of

thermodynamic to and heat of a system;

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K U A 11.3. Hess’s Law 11.4. Born-Haber cycle 11.5. Heat Capacity

11.3.1 state and explain Hess’s law of heat summation; 11.3.2 construct simple energy cycle by using Hess’s law from the given

reactions; 11.3.3 calculate standard heat of formation and heat of reaction by using Hess’s

law; 11.3.4 calculate the heat of reaction using experimental data (Cm∆t=q); 11.3.5 explain working of a calorimeter; 11.4.1 explain Born-Haber cycle; 11.5.1 explain the following terms; heat capacity, specific heat capacity and

molar heat capacity.

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12. Electrochemistry Candidates should be able to: K U A

12.1. Oxidation - Reduction

concept 12.2. Electrode Potential and

Electrochemical Series 12.3. Types of electrochemical

cells 12.4 Faraday’s law

12.1.1 define terms like reduction, oxidation, oxidation number, reducing agent,

oxidizing agent; 12.1.2 determine oxidation number of an atom in pure substance or in a

compound; 12.1.3 identify reducing and oxidizing agent by using oxidation –number change

method; 12.1.4 balance the equation using oxidation number change method; 12.1.5 identify oxidation and reduction half reaction; 12.1.6 balance the equation using half reaction method; 12.1.7 explain the uses of redox reactions in daily life (protection of metal

surfaces from corrosion and other harmful agents, solar cell as a source of energy);

12.2.1 define cathode, anode, electrode potential, Standard Hydrogen Electrode

and electrochemical series; 12.3.1 define cell potential; 12.3.2 determine the potential of electrochemical cell from the given data; 12.3.3 describe reaction occurring within a lead storage batteries; 12.3.4 explain production of electrical energy in a fuel cell; 12.3.5 define in standard electrode potential; 12.4.1 state and explain the Faraday’s law (1st and 2nd); 12.4.2 calculate the quantity of charge passed in an electrochemical cell during

electrolysis; 12.4.3 calculate the mass or volume of substance liberated during electrolysis.

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Part–II (Class XII)

13. S-and P-Block elements Candidates should be able to: K U A 13.1. Period (Na to Ar) 13.2. Group 1

13.1.1 identify the demarcation of the periodic table into s, p, d and f-block; 13.1.2 identify group, period and block of given elements by using electronic

configuration; 13.1.3 list down the elements in period 3; 13.1.4 explain the periodicity of physical properties (like atomic radius,

Ionization energy, electro negativity, electrical conductivity, melting and boiling points);

13.1.5 describe the anomalous behaviour in periodic trend of different elements in 3rd periods;

13.1.6 describe the reaction of period 3 elements with water, oxygen and chlorine;

13.1.7 describe the reaction of oxides and chloride of period 3 elements with water;

13.1.8 describe the physical properties of period 3 element (such as solubility and behaviours of oxides);

13.2.1 describe oxidation state and trend of physical properties in group 1 (such

as Ionization energy, electro-negativity, atomic radius, melting and boiling point);

13.2.2 describe the chemical reaction of group 1 elements with OH2 , Oxygen and chlorine;

13.2.3 explain effect of heat on nitrates, carbonates and hydrogen carbonates of group 1 elements;

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13.3. Group 2 13.4. Group 4 13.5. Group 7

13.3.1 describe oxidation state and trend of physical properties in group 2 elements (such as Ionization energy, electro-negativity, atomic radius, melting and boiling point);

13.3.2 describe the chemical reaction of group 2 elements with water, oxygen and nitrogen;

13.3.3 discuss the trend on solubility of hydroxides, sulphates and carbonates of group 2 elements;

13.3.4 discus the trends in thermal stability of the nitrates and carbonates of group 2 elements;

13.3.5 differentiate Beryllium from other members of its group; 13.4.1 describe oxidation state and trend of physical properties of group 4

elements (Ionization energy, electro-negativity, atomic radius, metallic character, melting and boiling property);

13.4.2 explain the variation of oxidation state in group 4 element; 13.4.3 describe the reaction of water with chlorides of carbon, silicon and lead; 13.4.4 compare the structure and stability of chlorides of carbon, silicon and

lead; 13.4.5 describe the structure of CO2 and SiO2; 13.4.6 discuss the acid base behaviour of oxide of group 4 elements; 13.5.1 discuss the oxidation state and trend of physical property of group 7

elements (atomic radius, electro negativity, electron-affinity, meting and boiling point, bond energy);

13.5.2 discuss the bond enthalpies and acidity in hydrogen halide; 13.5.3 compare the strength of halide ion as a reducing agent; 13.5.4 explain the significance of following elements in daily life (Iodine in

Goitre, Fluoride toxicity and deficiency, use of steel, tin, aluminium and glass in beverage and food industry).

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K U A 14. d and f block Element

(Transition)

Candidates should be able to:

14.1. General feature of transition element

14.2. Electronic Structure 14.3. Chemistry of some specific

transition element 14.4. Co-ordination Compound

14.1.1 describe the general features of transition element. (colour, variable oxidation states, use as catalyst);

14.2.1 describe the electronic structure of elements and ions of d-block element; 14.2.2 explain anomalous behaviour of chromium and copper with respect to

electronic configuration; 14.2.3 write down electronic configuration of given elements and ions of d –

block elements; 14.3.1 describe the important reactions (redox reaction) and uses of Vanadium,

Chromium, Copper, Manganese and Iron (as catalyst); 14.4.1 explain shapes, origin, colour and nomenclature of Co-ordination

compounds; 14.4.2 relate the co-ordination number of ion through the crystal structure of a

compound of which they are apart; 14.4.3 describe properties of alloys with reference to its composite metal atom; 14.4.4 describe the reaction of K2Cr2O7 with oxalic acid and Mohr Salts; 14.4.5 describe the reaction of KMnO4 with FeSO4, oxalic acid and Mohr Salts; 14.4.6 calculate concentration of Fe(II) ions with in a solution by titration with KMnO4; 14.4.7 explain the reaction of Hexaaquacopper(II)ion with iodide and determine

the concentration of copper ion in the solution.

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15. Organic Compounds Candidates should be able to: K U A

15.1. Sources: Fossils, fuel, coal,

petroleum and natural gas. 15.2. Coal as a source of organic

compound 15.3. Classification of organic

compound 15.4. Detection of element in

organic compound 15.5. Functional Group

15.1.1 explain diversity and magnitude of organic compounds and their general

properties; 15.2.1 explain the destructive distillation of coal; 15.3.1 classify the organic compound on structural basis; 15.3.2 explain the use of coal as a source of both aliphatic and aromatic

compounds; 15.4.1 give the methods to detect the elements present in organic compound. (C,

H, N, S, Halogen); 15.5.1 define the Functional Group.

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16. Hydrocarbons 16.1. Nomenclature and Shapes

of molecule 16.2. Free radical substitution

reaction 16.3. Oxidation of organic

compounds

Candidates should be able to: 16.1.1 describe the nomenclature and shapes of molecule (alkane, alkene, cyclo-

alkane, alkynes, benzenes and substituted benzene); 16.2.1 describe the mechanism of free radical substitution with reference to

methane and ethane; 16.3.1 identify and complete the redox reaction of organic compound;

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K U A

16.4. Alkenes 16.5. Alkynes 16.6. Benzene and Substituted

Benzene

16.4.1 explain the term sigma and pi carbon-carbon bonds with reference to ethene molecule;

16.4.2 describe the reactivity of alkene exemplified by ethane; 16.4.3 explain the terms with suitable example: (isomerism, stereo isomerism

and structural isomerism); 16.4.4 give the preparation: ethene from dehydration of alcohol and dehydro

halogenations of alkyl halide; 16.4.5 describe the reactions of ethene (hydrogenation, Hydration,

Hydrohalogenation, halogenation, halohydration, epooxidation, Ozonolysis, polymerization);

16.5.1 compare the reactivity of alkynes with alkanes, alkenes and arenes

(Aromatic compounds); 16.5.2 describe the preparation of alkynes using elimination reaction; 16.5.3 explain the acidity of alkynes (w.r.t its reaction with metal); 16.5.4 explain the chemistry of alkynes by hydrogenation, hydrohalogenation,

hydration, bromination, ozonolysis); 16.6.1 compare the reactivity of benzene with alkene and alkane; 16.6.2 describe the mechanism of electrophilic substitution reaction of benzene; 16.6.3 discuss the chemistry of benzene and methyl benzene by nitration,

sulphonation, halogenation, Friedal craft alkylation and acylation.

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17. Alkyl halides and Amines Candidates should be able to: K U A

17.1. Alkyl halides 17.2. Nucleophilic substitution

reaction 17.3. Elimination Reaction 17.4. Organo-metallic

Compounds (Grignard reagent)

17.1.1 name alkyl halides using IUPAC system for naming; 17.1.2 discuss physical properties and reactivity of different alkyl halides on the

basis of bond energy; 17.1.3 draw the structure of different alky halides by the given formula; 17.1.4 describe the preparations of alkyl halide by the reaction of alcohol with

HX, SOCl2, PX3 and by radical halogenations of alkane; 17.2.1 describe the mechanism of SN reaction; 17.2.2 compare SN1 and SN2 reaction; 17.2.3 write down the mechanism of SN reaction for the given alkyl halide; 17.2.4 identify Nucleophile (base), substrate and leaving group from the given

reaction; 17.2.5 discuss carbo-cation and its stability; 17.3.1 describe the mechanism of different types of elimination reaction; 17.3.2 compare E1 and E2 reaction; 17.3.3 write down the mechanism of elimination reaction in the given alkyl

halide; 17.3.4 compare substitution reaction and elimination reaction; 17.4.1 describe the preparation and reactivity of grignard reagent; 17.4.2 describe chemical reaction of grignard reagent with aldehyde, ketones, esters and CO2;

*

* * * * * * * * * * *

* * *

44

NOTES

45

K U A

17.5. Amines

17.5.1 name amines applying IUPAC system; 17.5.2 discuss physical properties of amines (M.P, B.P and solubility); 17.5.3 draw the structure of Amines (Primary, secondary and tertiary) from the

given formula; 17.5.4 explain basicity of amines (basic character); 17.5.5 describe preparation of amines by alkylation of NH3, by alkyl halide and

reduction of nitrile, nitro and amide functional groups; 17.5.5 describe chemical reaction of amines (alkylation with RX, reaction with

aldehyde and ketones); 17.5.6 describe preparation of amides and diazonium salts; 17.5.7 describe isomerism in alkyl halides and amines; 17.5.8 describe the test to detect nitrogen in the given organic compound.

* * * * * * *

* *

18. Alcohol, Phenols and ethers 18.1. Alcohols

Candidates should be able to: 18.1.1 name different alcohols using IUPAC system; 18.1.2 describe the physical properties and structure of alcohol; 18.1.3 discuss the preparation of alcohol by reduction of aldehyde, ketone,

carboxylic acid and esters; 18.1.4 discuss the acidic character of alcohol (as exemplified by ethanol); 18.1.5 describe the chemistry of alcohol by preparation of ether, esters, oxidative

cleavage of 1-2-diols; 18.1.6 define thiols (RSH); 18.1.7 describe the use of alcohol (disinfectant and antiseptic);

* *

* * * *

*

46

NOTES

47

K U A

18.2. Phenols 18.3 Ether

18.2.1 apply IUPAC system for naming phenols; 18.2.2 discuss physical properties, structure and acidic behaviour of phenol; 18.2.3 prepare phenols from the given compound in the form of equation

(benzene sulphonic acid, chlorobenzene, acidic oxidation of cumene and hydrolysis of diozomium salts;

18.2.4 discuss the chemistry of phenol (electrophilic aromatic substitution, reaction with Na metal and oxidation);

18.2.5 differentiate between alcohols and phenol; 18.2.6 explain isomerism in alcohol and phenol; 18.3.1 apply IUPAC system for naming ether from the given formula; 18.3.2 describe the physical and chemical properties of ether; 18.3.3 give chemical equation for the preparation of ether (Williamson Synthesis, reaction of alcohol and excess H2SO4); 18.3.4 explain the use of ether in medicine (for anaesthesia).

*

* * * * * *

* * *

48

NOTES

49

K U A 19. Carbonyl Compound I:

Aldelyde and ketones Candidates should be able to:

19.1. Nomenclature / Structure 19.2. Physical Properties 19.3. Preparation of Aldehyde

and Ketone 19.4. Reaction of Aldehyde and

Ketone. 19.5. Isomerism 19.6 Use

19.1.1 write the IUPAC nomenclature of aldelydes and ketones; 19.1.2 draw the structure of given aldehydes and ketones; 19.2.1 explain the physical properties of aldehydes and ketones; 19.3.1 write chemical equations for the preparation of aldehydes and ketones (by

ozonolysis of alkene, hydration of alkyne, oxidation of alcohol, Friedal Craft acylation of aromatics;

19.4.1 discuss the role of ά – hydrogen for comparing the reactivity of aldehyde

and ketones; 19.4.2 describe acid / base catalysed nucleophilic addition reaction of aldehyde

and ketones; 19.4.3 discuss the chemistry of aldeyde and ketons by their reduction to

hydrocarbon, alcohols, by using carbon nucleophiles, nitrogen nucleophiles and oxygen neucleophiles;

19.4.4 describe the oxidation reactions of aldelyde and ketones; 19.5.1 draw all possible isomers of given aldehydes and ketones; 19.5.2 describe glucose and fructose as example of aldeydes and ketones; 19.6.1 list down the use of formaldehyde vapours in adhesives, varnishes, paints,

foam insulations, permanent press clothing;

*

* * * * * *

* * * *

50

NOTES

51

K U A 20. Carbonyl Compound 2:

Carboxylic acid and functional derivatives

Candidates should be able to:

20.1. Nomenclature 20.2. Structure and Physical

Properties 20.3. Acidity

20.1.1 apply IUPAC system for naming carboxylic acid and their derivatives; 20.2.1 describe the structure and physical properties (solubility M.P and B.P) of

carboxylic acid; 20.2.2 draw the structure of given compounds of carboxylic acids and their

derivatives; 20.3.1 discuss the acidic behaviour of carboxylic acid (on the basis of alpha

carbon) and derivatives of carboxylic acid;

* *

* *

20.4. Preparation of Carboxylic acid.

20.5. Reactivity 20.6. Reaction of Carboxylic

acid.

20.4.1 give chemical equation for the preparation of carboxylic acid by Grignard Reagent, hydrolysis of nitriles, oxidation of primary alcohol, aldehydes and alkyl benzene;

20.5.1 describe the reactivity of carboxylic acid; 20.5.2 compare the reactivity in different derivatives of carboxylic acid; 20.6.1 give the equations for the preparation of following (acyl halides, acid

anhydrides, esters, amides); 20.6.2 write the inter-conversion reactions of carboxylic acids derivatives

(mentioned above); 20.6.3 describe reaction of carboxylic acid derivatives (mentioned above);

* * * *

* *

52

NOTES

53

K U A 20.7 Isomers 20.8 Use

20.7.1 describe isomerism in carboxylic acids (chain and functional); 20.7.2 draw all possible isomers of carboxylic acid (given formula); 20.8.1 list carboxylic acids present in fruits, vegetables and other natural products; 20.8.1 list the use of carboxylic acid (as preservatives in food and food products,

leather industry).

* *

* *

21. Biochemistry 21.1. Carbohydrates, Protein and

lipids 21.2. Enzymes 21.3 Nucleic acid 21.4 Mineral of biological

significance

Candidates should be able to: 21.1.1 explain the basis of classification of carbohydrates and protein; 21.1.2 describe structure-function relationship of carbohydrates, protein and

lipids. 21.1.3 explain role of carbohydrate in health and disease; 21.1.4 explain the nutritional important of protein and lipids; 21.1.5 explain different types of lipids (simple, conjugate, steroids); 21.1.6 explain the effect of lowering of pH (by using lemon juice) on the process

of precipitation of milk protein; 21.2.1 describe the role of enzymes as biological catalyst (in conversion of food); 21.2.2 explain the factors effecting the enzymes activity; 21.2.3 explain the role of enzymes as inhibitors; 21.3.1 identify the structural components of DNA and RNA 21.3.2 state the role of DNA in terms of genetic informations. 21.3.4 explain the role of RNA in terms of protein synthesis. 21.4.1 describe the role of Fe, Ca, P and Zn in nutrition. 21.4.2 explain the role of biochemical compounds (insulin, cholesterol) to

regulate human health.

* *

* * * * * * * * * * * *

54

NOTES

55

22. Industrial Chemistry Candidates should be able to: K U A

22.1. Introduction 22.2. Safety measurement 22.3. Dyes and Pesticides 22.4. Petro-chemicals 22.5 Synthetic Polymers (PVC

and nylon) 22.6 Synthetic Adhesive

22.1.1 discuss the importance of chemical industries in the economy of Pakistan; 22.1.2 list the raw materials available in Pakistan for various chemical industries

pharmaceutical, textile, petrochemicals); 22.2.1 discuss the safety measurement for industrial process according to ISO

certification for the given industry (as mentioned above); 22.2.2 identify risks associated with the manufacturing of chemicals (as

mentioned above); 22.3.1 discuss the importance of dyes and pesticides; 22.4.1 describe the fractional distillation and refining of petroleum; 22.4.2 describe the basic building block process in petrochemical technology

(polymerization with its examples); 22.4.3 identify in the given equation the petrochemicals and chemicals derived

from them (monomer and polymer); 22.4.4 list some major petrochemicals; 22.5.1 describe the chemical process of addition and condensation

polymerization; 22.5.2 describe the formation and Uses of PVC and nylon; 22.5.3 describe preparation and application of various cosmetics like shampoos,

sun blocks and fairness creams; 22.6.1 describe types and application of synthetic adhesive.

* *

* * * * * * * * * * *

56

NOTES

57

23. Environmental Chemistry Candidates should be able to: K U A

23.1. Chemistry of Troposphere

and Stratosphere 23.2. Water pollution water

treatment. 23.3 Green Chemistry

23.1.1 write down the various chemical reactions occurring in the atmosphere

(w.r.t depletion of ozone); 23.1.2 discuss the release of oxide of C, S, N and VOCs which are associated

with combustion of hydrocarbon based fuel; 23.1.3 outline problems associated with release of pollutants ( e.g. acid rain and

hazardous inorganic and organic compound like PAN (Peroxy Acetylic Nitrate);

23.1.4 describe causes and impacts of urban smog; 23.1.5 describe the role of CFCs in destroying ozone in the stratosphere; 23.1.6 list possible alternatives for the use of CFCs; 23.1.7 explain green house effect and global warming as resulting in climate

change; 23.2.1 explain the various techniques / methods of water analysis (using pH

meter, TDS meter, titration method); 23.2.2 explain the methods of treatment for water purification (filtration, sewage

treatment, Zeolite process, Reverse Osmosis); 23.3.1 describe green chemistry and its significance; 23.3.2 write some micro wave reactions (green chemistry) with their industrial

applications.

* * *

* * * * * * * *

58

NOTES

59

24. Analytical Chemistry Candidates should be able to: K U A

24.1. Classical and modern

methods of analysis

24.1.1 compare the classical and modern methods of analysis (w.r.t structural

analysis of compounds); 24.1.2 discuss the procedure of combustion analysis of hydrocarbon; 24.1.3 define spectroscopy and discuss its application in analytical chemistry; 24.1.4 explain the different regions of electromagnetic spectrum (according to

wavelength); 24.1.5 explain the basic principle of IR Spectroscopy; 24.1.6 identify benzene, acetone, carboxylic acid and ethanol from given IR

spectra; 24.1.7 predict whether a given molecule will absorb in the UV / visible region; 24.1.8 outline in simple terms the principles of proton NMR spectroscopy; 24.1.9 explain instrumentation and working of mass spectroscopy. (MS); 24.1.10 outline the use of MS in determination of relative isotopic masses; 24.1.11 explain atomic emission and atomic absorption spectrum; 24.1.12 discuss the use of MS in determination of drug abuse in forensic sciences.

* * * *

* * * * * * * *

60

NOTES

61

2. Scheme of Assessment

Class XI

Table 1: Number of Specific learning objectives by Cognitive level

SLOs Topic No.

Topics No. of Sub Topics K U A

Total

1 Stiochiometry 6 3 1 8 12 2 Atomic Structure 6 1 3 0 4 3 Theories of Covalent Bonding and

Shapes of Molecules 4 4 10 2 16

4 States of Matter I (Gases) 8 8 7 2 17 5 States of Matter II (Liquids) 4 3 7 1 11 6 States of Matter III (Solid) 5 3 6 2 11 7 Chemical Equilibrium 5 6 6 2 14 8 Acids, Bases and Salts 7 10 8 5 23 9 Chemical Kinetics 4 2 7 3 12 10 Solution and Colloids 5 4 4 8 16 11 Thermochemistry 2 4 6 1 11 12 Electrochemistry 4 4 4 8 16 Total 60 52 69 42 163 Percentage 32 42 26 100

Table 2: Allocation of Marks for the Objective Test,

Constructed Response Paper and Extended Response Questions

Marks Topic No.

Topics No. of Sub Topics Objective CRQs ERQs

Total

1 Stiochiometry 6 2 5 - 7 2 Atomic Structure 6 3 3 5 11 3 Theories of Covalent

Bonding and Shapes of Molecules

4 3 6 - 9

4 States of Matter I (Gases) 8 5 States of Matter II

(Liquids) 4

6 States of Matter III (Solid) 5

6 5 - 11

7 Chemical Equilibrium 5 2 4 - 6 8 Acids, Bases and Salts 7 4 5 5 14 9 Chemical Kinetics 4 2 4 - 6 10 Solution and Colloids 5 3 3 - 6 11 Thermo-chemistry 2 12 Electrochemistry 4 5 5 5 15

Total 60 30 40 15 85 Practical 15 Total 100

62

Class XII Table 3: Number of Specific learning objectives by Cognitive level

SLOs Topic No. Topics No. of Sub

Topics K U A Total

13 S-and P-Block elements 5 1 16 0 17

14 D and of block Element (Transition) 4 0 8 4 12

15 Organic Compound 5 3 3 0 6 16 Hydrocarbons 6 0 11 5 16 17 Alkyl halides and Amines 5 1 11 5 17 18 Alcohol, Phenol and Ether 3 3 10 4 17

19 Carbonyl compound 1. Aldehydes and Ketones 6 1 6 3 10

20 Carboyl Compound 2. Carboxyl acid and functional derivative

8 3 6 6 15

21 Biochemistry 4 2 13 0 15 22 Industrial chemistry 6 2 11 0 13 23 Environmental chemistry 3 3 8 0 11 24 Analytical chemistry 1 4 8 0 12 Total 56 23 111 27 161 Percentage 14 69 17 100

Table 4: Allocation of Marks for the Objective Test,

Constructed Response Paper and Extended Response Questions Marks Topic

No. Topics No. of Sub Topics Objective CRQs ERQs Total

13 S and P Block elements 5 4 9 13

14 d and f block Element (Transition) 4 3 4 5 12

15 Organic Compound 5 4 3 7 16 Hydrocarbons 6 2 4 6

17 Alkyl halides and Amines 5 3 4 7

18 Alcohol, Phenol and Ether 3

19 Carbonyl compound 1. Aldehydes and Ketones

6 4 4 8

20 Carboyl Compound 2. Carboxyl acid and functional derivative

8 2 2 4

21 Biochemistry 4 3 4 5 12 22 Industrial chemistry 6 23 Environmental chemistry 3 24 Analytical chemistry 1

5 6 5 16

Total 56 30 40 15 85 Practical 15 Total 100

63

2.1 Tables 1 and 3 summarize the number and nature of SLOs in each topic in class XI and XII. This will serve as a guide in the construction of the examination paper. It also indicates that more emphasis has been given to the Understanding (42%), Application and higher order skills (26%) to discourage rote memorization. There is a gradual increase in higher order skills in class XII. Tables 1 and 3, however, do not translate directly into marks.

2.2 Tables 2 and 4 show the distribution of marks. There will be 30 objective test items

each carrying one mark. The constructed response questions will carry 40 marks and the extended response questions will carry 15 marks. It is AKU-EB policy that every topic should be examined.

2.3 There will be two examinations, one at the end of Class XI and another at the end of

Class XII. 2.4 The question paper will be in two parts: Part I and Part II. Both parts will be

administered within 3 hours. Part I will be a separately timed Objective Test of 45 minutes, administered before the Constructed Response Paper (Part II). There will be no choice in the Objective Test.

2.5 There will be no choice in constructed response questions but extended response

questions will have a choice within alternate topics. 2.6 All constructed response questions will be in a booklet which will also serve as an

answer script. 2.7 Practicals to assess performance skills will carry 15 marks in class XI and 15 marks in

class X. The practicals will be conducted after the theory papers. 2.8 The practicals identified in the SLOs by a “P” should be carried out throughout the

academic year. It is essential for each school to equip its laboratories with chemicals, instruments, apparatus, specimens etc. according to the requirements of the practicals marked in the syllabus as “P”. Each school will be responsible to make sure that each student is provided the opportunity to do the practicals.

List of practicals is attached as annex B.

64

3. Teaching Learning Approaches

1. Concept of Celebration Day Celebration of Mole day on 23 October of every year at 6.02 P.M. Charts, models, debates and other activities related to the theme can be organised.

2. Group based assignments specially on numerical problems. 3. Experiments and demonstration on atomic structure/ gas laws/solution and

solubility colligative properties/ radox reactions and batteries 4. Models of bonding/ shape of molecules, 5. ICT integration

• simulation of bond formation • gas law • Graph plot ….. chemical kinetics

6. Field trips • Steel mill • Cement factory • Textile industry

7. Project on environment / pollution / chemical 8. Experiments: functional group-reaction and spectroscopy

4. Areas for Development of Learning Support Materials

• Electrochemistry • d and f block Element (Transition) • Industrial Chemistry

5. Recommended Texts and Reference Books Textbook

1. Anwar, J. and Ahmed, I, (2003). Chemistry 11 and 12. Lahore: Sheikh Ali and Sons.

Reference Books

1. Bukhari, S and Taj, R. A (2003). Chemistry for 11 and 12. Lahore: Chaudhary Ghulam Rasul and Sons.

2. Muhammad, A. and Qureshi, S, (2003), Chemistry 11 and 12 (2nd edition). Lahore: Punjab Textbook Board.

3. Mathews, Philip. (1996). Advance Chemistry.UK: Cambridge Press 4. Julian L. Robert, J. Leland Hollenberg, James M. Postma. (1975). Chemistry in

the laboratory. USA: W H Freeman 5. Sheikh, M. (2006). Practical Textbook. Lahore: Punjab Textbook Board.

65

6. Definition of Cognitive Levels and Command Words in the Specific Learning Objectives and in Examination Papers 6.1. Definitions of Cognitive Levels (Knowledge, Understanding and Application)

Knowledge: This requires knowing and remembering facts and figures, vocabulary and contexts, and the ability to recall key ideas, concepts, trends, sequences, categories, etc. It can be taught and evaluated through questions based on: who, when, where, what, list, define, describe, identify, label, tabulate, quote, name, state, etc. Understanding: This requires understanding information, grasping meaning, interpreting facts, comparing, contrasting, grouping, inferring causes/reasons, seeing patterns, organizing parts, making links, summarizing, solving, identifying motives, finding evidence, etc. It can be taught and evaluated through questions based on: why, how, show, demonstrate, paraphrase, interpret, summarize, explain, prove, identify the main idea/theme, predict, compare, differentiate, discuss, chart the course/direction, report, solve, etc. Application: This requires using information or concepts in new situations, solving problems, organizing information and ideas, using old ideas to create new ones, generalizing from given facts, analyzing relationships, relating knowledge from several areas, drawing conclusions, evaluating worth, etc. It can be taught and evaluated through questions based on: differentiate, analyse, show relationship, propose an alternative, prioritize, give reasons for, categorize, illustrate, corroborate, compare and contrast, create, design, formulate, integrate, rearrange, reconstruct/recreate, reorganize, predict consequences etc.

6.2 Definition of Command Words:

Knowledge Define Only a formal statement or equivalent paraphrase is required. No examples need to be given

Find: A general terms that may variously be interpreted as calculate, measure, determine etc.

List/Enlist: Requires a number of points, generally each of one word, with no

elaboration. Where a given number of points are specified, this should not be exceeded.

Outline: Implies brevity, i.e. restricting the answer to giving essentials.

Identify: Describe with specific examples of how a given term or concept is

applied in daily life

Calculate: Is used when a numerical answer is required. In general, working should be shown, especially where two or more steps are involved

66

State: Implies concise answer with little or no supporting argument, for example a numerical answer that can be obtained by inspection. Recall: To bring back to mind and write down, as it is given in the text that you have already memorized.

Write: To construct full sentence of continuous prose, not abbreviated text.

Understanding Show: Demonstrate with evidence. Demonstrate: Implies that the candidate is expected to show how is one thing related

to another, usually it is a reference to theory but sometimes it is by physical manipulation or experiment.

Describe: To state in words (Using diagrams where appropriate) the main points

of the topic. It is often used with reference wither to particular phenomena or to particular experiments. In the former instance, the term usually implies that the answer should include reference to (visual) observations associated with the phenomena.

Determine: Often implies that the quantity concerned cannot be measured directly

but is obtained by calculation, substituting measured or known values of other quantities into standard formula, for e.g. relative molecular mass.

Discuss: To give a critical account of the point involved in the topic. Draw/construct: Implies a simple freehand sketch or diagram. Care should be taken

with proportions and the clear labeling of parts. Explain: May imply reasoning or some reference to theory, depending on the

context. Application

Classify: State the basis for categorization of a set of related entities and assign

example to categories. Compare: List the main characteristics of two entities clearly identifying

similarities (and differences) Differentiate: To identify those characteristics which are always or sometimes

distinguish between two categories. Recognize: Involves looking at a given example and stating what it most probably

is.

67

Measure: To determine extent, quantity, amount or degree of something as determine by measurement or calculation.

Narrate: To write down the facts and explanation as given or provided in the

text.

Predict or Implies that the candidates is not expected to produce the required answer

Deduce: By recall but by making a logical connection between other pieces of information. Such information may be wholly given in the question or may depend on answer extracted in an early part of the question.

Purify: Implies a practical activity in which the candidates is expected to apply

an approved methodology with appropriate safety precautious. Relate: Describe how things depend upon, follow from or are part of another.

Explore: to examine thoroughly and systematically to be able to make a

statement about a phenomenon or concept.

68

Annex A HSSC Scheme of Studies2 AKU-EB as a national board offers SSC and HSSC qualifications for both English medium and Urdu medium schools. The revised HSSC Scheme of Studies issued by the Curriculum Wing is designed for two years. Each HSSC subject will be taught across both the classes XI and XII. At the HSSC level the marks allocated to subjects are mostly based on the revised National Scheme of Studies of 2006. The first HSSC-I part wise (Class XI) examination based on 2006 national curriculum will be held in 2009 and HSSC-II (Class XII) in 2010. HSSC I-II (Classes XI-XII) subjects on offer for the examinations in 2009 and 2010 HSSC Part-I (Class XI) Science Group (Pre-Medical)

Marks Subjects Theory Practical Total English Compulsory-I 100 - 100 Urdu Compulsory-I OR Pakistan Culture-I a 100 - 100 Physics-I 85 15 100 Chemistry-I 85 15 100 Biology-I 85 15 100 Total: 455 45 500

HSSC Part-II (Class XII) Science Group (Pre-Medical)

Marks Subjects Theory Practical Total English Compulsory-II 100 - 100 Urdu Compulsory-II OR Pakistan Culture-II a 100 - 100 Islamiyat OR Ethics b 50 - 50 Pakistan Studies b 50 - 50 Physics-II 85 15 100 Chemistry-II 85 15 100 Biology-II 85 15 100 Total: 555 45 600

a Foreign students may opt Pakistan Culture in lieu of Urdu Compulsory, subject to

the board’s approval. b For non-Muslim candidates in lieu of Islamiyat. Note: Pakistan Studies, Islamiyat / Ethics will be taught in both Classes XI and XII, but the examination will be conducted at the end of Class XII.

2 Government of Pakistan September 2007 and May 2003. Scheme of Studies for SSC and HSSC (Classes IX-XII), Islamabad: Ministry of Education, Curriculum Wing.

69

HSSC Part-I (Class XI) Science Group (Pre-Engineering)

Marks Subjects Theory Practical Total English Compulsory-I 100 - 100 Urdu Compulsory-I OR Pakistan Culture-I a 100 - 100 Physics-I 85 15 100 Chemistry-I 85 15 100 Mathematics-I 100 - 100 Total: 470 30 500

HSSC Part-II (Class XII) Science Group (Pre-Engineering)

Marks Subjects Theory Practical Total English Compulsory-II 100 - 100 Urdu Compulsory-II OR Pakistan Culture-II a 100 - 100 Islamiyat OR Ethics b 50 - 50 Pakistan Studies b 50 - 50 Physics-II 85 15 100 Chemistry-II 85 15 100 Mathematics –II 100 - 100 Total: 570 30 600



70

HSSC Part-I (Class XI) Science Group (Science General) Marks Subjects Theory Practical Total

English Compulsory-I 100 - 100 Urdu Compulsory-I OR Pakistan Culture-I a 100 - 100 Any one subject combinations of the following: Physics-I OR 85 15 Mathematics-I 100 - Statistics-I 85 15

300/

Economics-I OR 100 - Mathematics-I 100 - Statistics-I 85 15

300/

Economics-I OR 100 - Mathematics-I 100 - Computer Science-I 75 25

300/

Physics-I OR 85 15 Mathematics-I 100 - Computer Science-I 75 25

300/

Mathematics-I 100 - Statistics-I 85 15 Computer Science-I 75 25

300

Total: 500 HSSC Part-II (Class XII) Science Group (Science General)

Marks Subjects Theory Practical Total English Compulsory-II 100 - 100 Urdu Compulsory-II OR Pakistan Culture-II a 100 - 100 Islamiyat OR Ethics b 50 - 50 Pakistan Studies b 50 - 50 Any one subject combinations of the following: Physics-II OR 85 15 Mathematics-II 100 - Statistics-II 85 15

300/

Economics-II OR 100 - Mathematics-II 100 - Statistics-II 85 15

300/

Economics-II OR 100 - Mathematics-II 100 - Computer Science-II 75 25

300/

Physics-II OR 85 15 Mathematics-II 100 - Computer Science-II 75 25

300/

Mathematics-II 100 - Statistics-II 85 15 Computer Science-II 75 25

300

Total: 600 a Foreign students may opt Pakistan Culture in lieu of Urdu Compulsory, subject to


71

HSSC Part-I (Class XI) Commerce Group

Marks Subjects Theory Practical Total English Compulsory-I 100 - 100 Urdu Compulsory-I OR Pakistan Culture-I a 100 - 100 Principles of Accounting 100 - 100 Principles of Economics 75 - 75 Principles of Commerce 75 - 75 Business Mathematics 50 - 50 Total: 500 - 500

HSSC Part-II (Class XII) Commerce Group

Marks Subjects Theory Practical Total English Compulsory-II 100 - 100 Urdu Compulsory-II OR Pakistan Culture-II a 100 - 100 Islamiyat OR Ethics b 50 - 50 Pakistan Studies 50 - 50 Principles of Accounting 100 - 100 Commercial Geography 75 75

60/ 15

Computer Studies OR Banking 75 -

75

Business Statistics 50 - 50 Total: 600 600



72

HSSC Part-I (Class XI) Humanities Group

Subjects Marks English Compulsory-I 100 Urdu Compulsory-I OR Pakistan Culture-I a 100 Any three of the following Elective Subjects 1. Civics Elective-I 2. Computer Science-I (75+25 practical) 3. Economics-I 4. Education-I 5. History of Muslim India-I 6. Islamic Studies-I 7. Mathematics-I 8. Statistics-I (85+15 practical) 9. Psychology-I (85+15 practical) 10. Sociology-I 11. English Literature-I 12. Urdu Literature-I

300 (100 each)

Total: 500 HSSC Part-II (Class XII) Humanities Group

Subjects Marks English Compulsory-II 100 Urdu Compulsory-II OR Pakistan Culture-II a 100 Islamiyat OR Ethics b 50 Pakistan Studies b 50 Any three of the following Elective Subjects 1. Civics Elective-II 2. Computer Science-II (75+25 practical) 3. Economics-II 4. Education-II 5. History of Muslim India-II 6. Islamic Studies-II 7. Mathematics-II 8. Statistics-II (85+15 practical) 9. Psychology-II (85+15 practical) 10. Sociology-II 11. English Literature-II 12. Urdu Literature-II

300 (100 each)

Total: 600

a Foreign students may opt Pakistan Culture in lieu of Urdu Compulsory, subject to the board’s approval.

b For non-Muslim candidates in lieu of Islamiyat. Note: Pakistan Studies, Islamiyat / Ethics will be taught in both Classes XI and XII, but the examination will be conducted at the end of Class XII.

73

Annex B

List of Practical Activities Class XI

EXP# OBJECTIVE EQUIPMENT CHEMICALS DURATION

CHAPTER 1: INTRODUCTION TO STOICHIOMETRY

1 Estimate the Amount of Ba 2+ in the Given Solution of Bacl 2 Gravimetrically

Analytical balance, oven funnel, wash bottle, Whatman filter paper # 42, glass rod, beakers, desiccators, pipette, burner, matches, safety goggles.

Distilled water, potassium chromate solution, barium chloride solution

40x2

CHAPTER 4: STATES OF MATTER I: GASES

2 Demonstrate that Gases spread by diffusion to Areas of lower Concentration.

Glass tube 40cm long and 1 cm in internal diameter, ring stand, clamp, clamp holder, cotton balls, forceps, dropper, rubber stoppers, safety goggles.

Concentrated NH 3 solution, concentrated HCl

40x2

74

CHAPTER 5: STATES OF MATTER II: LIQUIDS

3

Separate the Given Mixture of lnks by Paper Chromatography.

Whatman filter paper # 1, glass cylinder with a glass support,

water – alcohol mixture, mixture of inks

40 x2

4 Separate the Following lons from a given Mixture of their Salts (Ni 2+ , Co 2+ , Cu 2+ ) by paper Chromatography

Whatman filter paper # 1, glass clinder with a glass support, rubber bung, lead pencil

1% solution of the chlorides of Ni, Co, Cu 2+ , spraying solution (0.1% rubeanic acid in ethyl alcohol), solvent mixture (acetone, distilled water and concentrated HCI mixed in ratio 43:3:4)

40x 2

5 Separate Lead and Cadmium in a mixture solution by paper Chromatography

rubber bung, lead pencil

Sample reagent (mixture of solutions of PbCl 2 and CdCl 2 ) , solvent mixture (n-butanol + 3M HNO 3 ), spraying agent (H 2 S gas)

40 x 2

6 Prove that the Loss of Thermal Energy When a Liquid Evaporates Will Lower the Temperature of the Liquid.

beaker, thermometer, safety goggles

acetone

40 x2

CHAPTER 6: STATES OF MATER III: SOLIDS

7 Crystallize Benzoic Acid from water

China dish, burner, tripod stand, wire gauze, matches, beakers, funnel, filter paper, stirrer, safety goggles

Distilled water and benzoic acid

40 x2

75

CHAPTER 7:CHEMICAL EQUILIBRIUM

8 Purify a Given Sample of Sodium Chloride by Passing HCI Gas. (Application of common ion effect)

beaker 500ml, funnel, round-bottom flask, glass tubing, wire gauze, thistle funnel, burner, stirrer, graduated flask and physical balance

Distilled water, common salt, concentrated H 2 SO 4

40 x 2

CHAPTER 8:ACIDS, BASES AND SALTS

9

Determine the Exact Morality of the Given Solution of H 2 SO 4 and the Volume of this acid required to prepare 500 ml of 0.02 M Acid by Volumetric Method

Burette, pipette, funnel, conical flask, beakers, iron stand

Phenolphthalein, 0.1M NaOH, 0.2M H 2 SO 4 distilled water

40 x2

10 Determine the Percentage of NaOH in the Given Solution by Volumetric Method


Phenolphthalein, 0.1M NaOH, 0.1M HCI, distilled water, solution containing 8gms of a mixture of NaCI and NaOH

40 x2

11 The given solution contains 6gms of Na 2 CO 3 dissolved per dm 3 . Determine the Percentage Purity of the Sample Solution by Volume Method.


Methyl orange, 0.1M Na 2 CO 3 , 0.1M HCI, Distilled water, solution of 6 gms of Na 2 CO 3 in 1 liter.

40 x2

12 Determine the Value of X by Volumetric Method in the Given Sample of 6.3g of (COOH) 2 . XH 2 O Dissolved per dm 3


Phenolphthalein , 0.1M NaOH, 0.1 (COOH) 2 . 2H 2 O, Distilled water

40 x2

13 Determine the Solubility of Oxalic Acid at Room Temperature Volumetrically


Phenolphthalein, 0.1M NaOH, 0.1 (COOH) 2.2H 2 O, Distilled water.

40 x2

76

CHAPTER 11:THERMOCHEMISTRY

14 Determine the Heat of Neutralization of NaOH and HCI

Calorimeter with stirrer, thermometer, balance

1M NaOH, 1M HCI, distilled water

40 x2

CHAPTER 12: ELECTROCHEMISTRY

15 Standardize the Given Solution of KMnO 4 and Calculate the Volume of KMnO 4 Required for Preparing 1 dm 3 of 0.01M KMnO 4 Solution Volumetrically

Burette, pipette, funnel, conical flask, beakers, iron stand, test tube

0.1M FeSO 4 solution 0.02MKMnO 4 solution dilute H 2 SO 4 , distilled water.

40 x 2

16 Determine the Amount of Iron in the Given Sample Volumetrically


0.05M FeSO 4 solution 0.01M KMnO 4 solution dilute H 2 SO 4 , distilled water.

40 x2

17 Determine the Percentage Composition Volumetrically of a Solution Mixture of K 2 C 2 O 4 and K 2 SO


Solution mixture of K 2 C 2 O 4 and K 2 SO 4 0.01M KMnO 4 solution, dilute H 2 SO 4 , distilled water

40 x2

18 Determine the Solubility of Mohr’s Salt at Room Temperature Volumetrically.


0.05M Mohr’s salts solution, 0.01M KMnO 4 solution, dilute H 2 SO 4 distilled water

40 x2

77

Class XII

EXP# OBJECTIVE EQUIPMENT CHEMICALS DURATION MIN

CHAPTER 13:S-AND P- BLOCK ELEMENTS

1 Prepare Potassium Xanthate

Beakers, funnel, filter paper, measuring cylinder, safety goggles

Potassium hydroxide, alcohol, carbon disulphide, ether (for washing of crystals), distilled water, copper sulphate solution

40x 2

2 .Detect the Following Cations: NH 4+ , Mg +2 ,

Al +3 , Cu +2 , Zn +2 , Ba +2 , Pb +2 , Detect the following Anions: CO 3

−2 , NO 3 , NO 2 , SO 4

2 , SO 32 , Cl − , Br − , I − , CrO 4

−2 Perform Tests for the following Gases: NH 3 , CO 2 , CI 2 , H 2 , O 2 , SO 2

Test tubes, test tube holder, test tube rack, delivery tube, measuring clinder, match box, wooden splint, Bunsen burner, safety goggles, glass rod, filter paper, litmus paper

Sodium hydroxide, ammonium hydroxide, dilute acids, barium, lead, silver salt solutions, Al foil, lime water and other necessary chemical solutions for the identification of these ions and gases

40x2

CHAPTER 14: D-F- BLOCK ELEMENTS

3 Prepare Nickel Dimethyl Glyoxime

Test tubes, test tube holder, test tube rack, measuring clinder, Bunsen burner, safety goggles, filter paper, funnel

Dimethyl glyoxime solution, nickel salt solution, distilled water and NH 4 OH

40x2

CHAPTER 16: HYDROCARBONS

4 Prepare Ethylene from Ethylene Bromide

Test tubes, test tube holder, test tubes rack, delivery tube, measuring cylinder, Bunsen burner safety goggles

Pieces of zinc metal, alcohol, ethylene bromide

40 x2

78

CHAPTER 17: ALKYL HALIDES AND AMINES

5 Prepare Azo dye from Amine

Test tubes, test tube rack, test tube holder, measuring cylinder, balance, filter paper, funnel.

Amine, phenol, hydrochloric acid, ice, sodium nitrite, alcohol, distilled water

40 x2

6 1. Identify the Amine Functional Group.

Test tubes, test tube rack, test tube holder, measuring cylinder, balance, filter paper, funnel

Hinsberg test: benzenesulfony chloride, sodium hydroxide, HCl

40 2

CHAPTER 18: ALCOHOLS, PHENOLS AND ETHERS

7 Prepare Iodoform. Test tubes, test tube holder, test tube rack, Bunsen burner, safety goggles

Alcohol, sodium hydroxide, water, solution of iodine in potassium iodide

40 x2

8 Identify the Phenol Function Group.

Test tubes, test tube holder, test tube rack, measuring cylinder, safety goggles.

Litmus solution, Ferric Chloride solution

40 2

CHAPTER 19: CARBONYL COMPOUNDS I: ALDEHYDES AND KETONES

9 Prepare Glucosazone.

Beakers, test tubes, measuring cylinder balance, Bunsen burner, match box, funnel filter paper

Glucose solution, 2,4 – dinitrophenyl hydrazine solution, distilled water

40 x 2

10 identify the aldehyde and Ketone functional Group.

Beakers, test tubes, measuring cylinders, Bunsen burner, match box, funnel, filter papers

Fehling’s solution, Tollen’s reagent, Benedict solution

40 x2

79

CHAPTER 20: CARBONYL COMPOUNDS II CARBOXYLIC ACIDS AND FUNCTIONAL DERIVATIVES.

11 Prepare Benzannilide from Benzoic Acid. Beaker, test tubes, measuring cylinders, Bunsen burner, match box, funnel, filter paper.

Benzoic acid, phosphorous pentachloride, ice, alcohol, distilled water

40 x2

12 Identify the Carboxylic Acid Functional Group.

Test tubes, beakers, balance, measuring cylinders, funnel, filter paper

Dilute sodium hydroxide saturated potassium bicarbonate

40 x2

CHAPTER 21: BIOCHEMISTRY

13 Detect glucose as reducing sugar in urine sample of diabetic patients

Test tubes, beaker conical flask, pipette

Benedict Reagent Fehling’s Solution.

40 x2

14 Detect Protein Urea denaturation

Test tubes, beaker conical flask, pipette

Urea, egg white

40 x2

15 Observe the digestion of starch with salivary amylase

Test tubes, beakers, conical flask pipette, slides.

Freshly prepared starch solution, iodine solution

40 x 2

16 Determine the lodine number of an oil Test tubes, beakers, conical flask, pipette, beakers

iodine solution, oil

40 x 2

hssci ii chemistry

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