CHEMISTRY
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TABLE OF CONTENTS z
Latest ICSE Reduced Syllabus issued by CISCE for Academic Year 2021 –22
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1.
Periodic Properties and Variations of Properties Topic 1. Modern Periodic Table and Periodicity Topic 2. Periodic Properties and Their Variations Self Assessment Test-Unit-I Chemical Bonding Topic 1. Electrovalent and FRYDOHQWERQGLQJ Topic 2. &RRUGLQDWH%RQGLQJ Self Assessment Test-Unit-II Acids, Bases and Salts Topic 1. Acids and Bases Topic 2. Salts Self Assessment Test-Unit-III Analytical Chemistry Self Assessment Test-Unit-IV Mole Concept and Stoichiometry
z 2. z 3.
z 4. z 5.
1 - 23
z
Self Assessment Test-Unit-V
127 - 127
6.
Electrolysis
128 - 151
Topic 1.
Electrolytes and Non-electrolytes
24 - 24 25 - 44
Topic 2.
78 80 96 98
-
Applications of Electrolysis
z
Self Assessment Test-Unit-VI
152 - 152
7.
Metallurgy
153 - 180
45 - 45 46 - 77
*Topic 1. Gay Lussac’s Law and $YRJDGUR·V/DZ Topic 2. Relative Atomic Mass, Relative Molecular Mass and Mole Concept Topic 3. 3HUFHQWDJH&RPSRVLWLRQ Empirical and Molecular Formula *Topic 4.
8 - 11
Topic 1.
Metals and Non-Metals
*Topic 2.
Extraction of Metals and Alloys
z
Self Assessment Test-Unit-VII
181 - 181
8.
Study of compounds
182 - 236
79 95 97 126
Topic 1. +\GURJHQ&KORULGH*DV Topic 2.
Hydrochloric acid
Topic 3.
Ammonia
Topic 4.
Nitric Acid
Topic 5.
Sulphuric Acid
z
Self Assessment Test-Unit-VIII
237 - 238
9.
Organic Chemistry
239 - 279
Topic 1. 2UJDQLF&RPSRXQGV Topic 2.
Hydrocarbons - Alkanes, Alkenes and Alkynes
Calculations Based on
*Topic 3.
Chemical Equations z
Alcohols and carboxylic acids
Self Assessment Test-Unit-IX
280 - 280
*Note- As per the Latest Reduced Syllabus released by CISCE in July 2021, for Academic year 2021-2022, the chapters marked in grey have been omitted. Therefore, questions from these will not be asked in the final examination to be held in 2022.
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LET THE ADVENTURE BEGIN! India is currently one of the youngest economies in the world. Hence, it’s imperative for our education system to churn out more learners than ever before. It is this ‘learner’s mindset’ which will set
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SYLLABUS CHEMISTRY CLASS 10 Latest Reduced Syllabus issued by CISCE for Academic Year 2021-2022 There will be one paper of two hours duration of 80 marks and Internal Assessment of practical work carrying 20 marks.
(b) Covalent Bonding: z Electron dot structure of non-polar covalent molecules on the basis of duplet and octet of electrons (example: hydrogen, chlorine, oxygen, nitrogen, carbon tetrachloride and methane.
The paper will be divided into two sections, Section I (40 marks) and Section II (40 marks). Section I (compulsory) will contain short answer questions on the entire syllabus.
z Polar Covalent compounds – based on difference in 4 electronegativity:
Section II will contain six questions. Candidates will be required to answer any four of these six questions.
Examples – HCl and H2O including structures.
Note: All chemical process/reactions should be studied with reference to the reactants, products, conditions, observation, the (balanced) equations and diagrams. 1.
z Characteristic properties of Covalent compounds – state of existence, melting and boiling points, conductivity (heat and electricity), ionisation in solution.
Periodic Properties and variations of Properties (i)
Periodic properties and their variations in groups and periods. Definitions and trends of the following periodic properties in groups and periods should be studied:
z
atomic size
z
metallic character
z
non-metallic character
z
ionisation potential
z
electron affinity
z
electronegativity
z
(c)
Electrovalent
and
Covalent
Coordinate Bonding:
z Definition
The meaning of lone pair; the formation of hydronium ion and ammonium ion must be explained with help of electron dot diagrams. 3.
The study of modern periodic table up to period 4 and Group 2 [IIA] (students to be exposed to the complete modern periodic table but no questions will be asked on elements beyond period 4 –Calcium) Periodicity and other related properties to be explained on the basis of nuclear charge and shells (not orbitals).
(Special reference to the alkali metals, alkaline earth metals, halogen groups and inert gases). 2.
of
z The lone pair effect of the oxygen atom of the water molecule and the nitrogen atom of the ammonia molecule to explain the formation of H3O+ and OH- ions in water and NH+ion.
(ii) Periodicity on the basis of atomic number for elements. z
Comparison compounds.
Chemical Bonding Electrovalent, covalent and co-ordinate bonding, structures of various compounds, Electron dot structure. (a) Electrovalent bonding:
zElectron dot structure of Electrovalent compounds NaCl, MgCl2, CaO. zCharacteristic properties of electrovalent compounds
– state of existence, melting and boiling points, conductivity (heat and electricity), dissociation in solution and in molten state to be linked with electrolysis.
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Study of Acids, Bases and Salts (i) Simple definitions in terms of the molecules, their classification and characteristic properties. (ii) Ions present in mineral acids, alkalis and salts and their solutions; use of common acid - base indicators and universal indicator, pH paper to test for acidity and alkalinity. zExamples
with equation for the ionisation/ dissociation of ions of acids, bases and salts.
zAcids
form hydronium ions (only positive ions) and alkalis form hydroxyl ions (only negative ions) with water and their effect on indicators.
zDefinitions
- Salts are formed by partial or complete replacement of the hydrogen ion of an acid by a metal or Ionic definition of salt (To be explained with suitable examples).
zIntroduction to pH scale to test for acidity, neutrality
and alkalinity by using pH paper or Universal indicator. zTypes
of salts: normal salts, acid salt, basic salt, definition and examples.
SYLLABUS 4.
e.g. Na, Mg, Fe, Cu, to form ions) illustrated by the electrolysis of:
Analytical Chemistry (i) Action of Ammonium Hydroxide and Sodium Hydroxide on solution of salts: colour of salt and its solution; formation and colour of hydroxide precipitated from salt solutions of Ca, Fe, Cu, Zn and Pb; special action of ammonium hydroxide on solutions of copper salt and sodium hydroxide on ammonium salts.
zMolten lead bromide zacidified water with platinum electrodes zAqueous copper (II) sulphate with active and inert electrodes; electron transfer at the electrodes. The above electrolytic processes can be studied in terms of electrolyte used, electrodes used, ionization reaction, anode reaction, cathode reaction, use of selective discharge theory, wherever applicable.
On solution of salts: z Colour of salt and its solution. z Action on addition of Sodium Hydroxide to solution of Ca, Fe, Cu, Zn, and Pb salts drop by drop in excess. Formation and colour of hydroxide precipitated to be highlighted with the help of equations. z Action on addition of Ammonium Hydroxide to solution of Ca, Fe, Cu, Zn, and Pb salts drop by drop in excess. Formation and colour of hydroxide precipitated to be highlighted with the help of equations. z Special action of Ammonium Hydroxide on solutions of copper salts and sodium hydroxide on ammonium salts. (ii) Action of caustic alkalis (NaOH, KOH) on aluminium their oxides and hydroxides. Self explanatory. 5.
(v) Applications of electrolysis: zElectroplating with nickel and silver, choice of electrolyte for electroplating. zElectro refining of copper; Reasons and conditions for electroplating; names of the electrolytes and the electrodes used should be given. Equations for the reactions at the electrodes should be given for electroplating, refining of copper. 7.
(i) Occurrence of metals in nature: zMineral and ore - Meaning only. zCommon ores of iron, aluminium and zinc.
Mole Concept and Stoichiometry
(ii) Extraction of Aluminium.
(i) Vapour Density and its relation to relative molecular mass:
(a) Chemical method for purifying bauxite by using NaOH – Baeyer’s Process.
zMolecular
mass = 2×vapour density (formal proof not required)
(b) Electrolytic extraction – Hall Heroult’s process: Structure of electrolytic cell - the various components as part of the electrolyte, electrodes and electrode reactions.
zDeduction
of simple (empirical) and molecular formula from:
(a) the percentage composition of a compound.
Description of the changes occurring, purpose of the substances used and the main reactions with their equations.
(b) the masses of combining elements. 6.
Metallurgy
Electrolysis (i) Electrolytes and non-electrolytes.
(iii) Alloys – Definition, alloys of Aluminium (only constituent elements), properties and uses.
Definitions and examples. (ii) Substances containing molecules only, ions only, both molecules and ions.
8.
zSubstances
containing molecules only ions only, both molecules and ions.
zExamples;
relating their composition with their behaviour as strong and weak electrolytes as well as non-electrolytes.
(iii) Definition and explanation of electrolysis, electrolyte, electrode, anode, cathode, anion, cation, oxidation and reduction (on the basis of loss and gain of electrons). (iv) An elementary study of the migration of ions, with reference to the factors influencing selective discharge of ions (reference should be made to the activity series as indicating the tendency of metals,
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Study of Compounds A. Hydrogen Chloride Hydrogen chloride: preparation of hydrogen chloride from sodium chloride; refer to the density and solubility of hydrogen chloride (fountain experiment); reaction with ammonia; acidic properties of its solution. zPreparation
of hydrogen chloride from sodium chloride; the laboratory method of preparation can be learnt in terms of reactants, product, condition, equation, diagram or setting of the apparatus, procedure, observation, precaution, collection of the gas and identification (Tests).
zSimple
experiment to show the density of the gas (Hydrogen Chloride) –heavier than air.
SYLLABUS zSolubility
Large scale preparation. Nitric acid as an oxidizing agent.
of hydrogen chloride (fountain experiment); setting of the apparatus, procedure, observation, inference.
z
Laboratory preparation of nitric acid from potassium nitrate or sodium nitrate; the laboratory method to be studied in terms of reactants, products, conditions, equations, setting up of apparatus, diagram, precautions, collection and identification. (Tests)
z
Manufacture of Nitric acid by Ostwald’s process (Only equations with conditions where applicable).
z
As an oxidising agent: its reaction with copper, carbon, sulphur.
zMethod
of preparation of hydrochloric acid by dissolving the gas in water- the special arrangement and the mechanism by which the back suction is avoided should be learnt.
zReaction
with ammonia
zAcidic
properties of its solution - reaction with metals, their oxides, hydroxides and carbonates to give their chlorides; decomposition of carbonates, hydrogen carbonates, sulphides, sulphites.
D. Sulphuric Acid
zPrecipitation
reactions with silver nitrate solution and lead nitrate solution.
B.
Large scale preparation, its behaviour as an acid when dilute, as an oxidizing agent when concentrated oxidation of carbon and sulphur; as a dehydrating agent - dehydration of sugar and copper (II) sulphate crystals; its non-volatile nature.
Ammonia Ammonia: its laboratory preparation from ammonium chloride and collection; ammonium salts. Manufacture by Haber’s Process; density and solubility of ammonia (fountain experiment); aqueous solution of ammonia; its reactions with hydrogen chloride and with hot copper (II) oxide; lead monoxide (PbO) and chlorine; the burning of ammonia in oxygen; uses of ammonia. zLaboratory
preparation from ammonium chloride and collection; (the preparation to be studied in terms of, setting of the apparatus and diagram, procedure, observation, collection and identification (Tests).
Ammonia from ammonium salts using alkalies. The reactions to be studied in terms of reactants, products, conditions and equations.
z Manufacture by Contact Process Equations with conditions where applicable). z Its behaviour as an acid when dilute -reaction with metal, metal oxide, metal hydroxide, metal carbonate, metal bicarbonate, metal sulphite, metal sulphide. z Concentrated sulphuric acid as an oxidizing agent - the oxidation of carbon and sulphur. z Concentrated sulphuric acid as a dehydrating agent(a) the dehydration of sugar (b) Copper (II) sulphate crystals. z Non-volatile nature of sulphuric acid - reaction with sodium or potassium chloride and sodium or potassium nitrate.
z Manufacture by Haber’s Process.
z Identification and Tests for both dilute and concentrated sulphuric acid.
z Density and solubility of ammonia (fountain experiment).
9.
(i) Introduction to Organic compounds.
z The burning of ammonia in oxygen. z The catalytic oxidation of ammonia (with conditions and reaction) z Its reactions with hydrogen chloride and with hot copper (II) oxide, lead monoxide (PbO) and chlorine (both chlorine in excess and ammonia in excess).
Organic Chemistry zUnique nature of Carbon atom – tetra valency, catenation.
zFormation of single, double and triple bonds, straight chain, branched chain, cyclic compounds (only benzene).
All these reactions may be studied in terms of reactants, products, conditions, equations and observations. z Aqueous solution of ammonia - reaction with sulphuric acid, nitric acid, hydrochloric acid and solutions of iron(III) chloride, iron(II) sulphate, lead nitrate, zinc nitrate and copper sulphate. C. Nitric Acid Nitric Acid: one laboratory method of preparation of nitric acid from potassium nitrate or sodium nitrate.
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(ii) Structure and Isomerism. zStructure
of compounds with single, double and triple bonds.
zStructural
formulae of hydrocarbons. Structural formula must be given for: alkanes, alkenes, alkynes up to 5 carbon atoms.
zIsomerism
– structural (chain, position)
(iii) Homologous series – characteristics with examples. Alkane, alkene, alkyne series and their gradation in properties and the relationship with the molecular mass or molecular formula.
SYLLABUS Candidates are expected to have completed the following minimum practical work:
(iv) Simple nomenclature. Simple nomenclature of the hydrocarbons with simple functional groups – (double bond, triple bond, alcoholic, aldehydic, carboxylic group) longest chain rule and smallest number for functional groups rule – trivial and IUPAC names (compounds with only one functional group).
1.
Action of heat on the following substances: (a) Copper carbonate, zinc carbonate (b) zinc nitrate, copper nitrate, lead nitrate (c) Hydrated copper sulphate Make observations, identify the products and make deductions where possible (equations not required).
(v) Hydrocarbons : alkanes, alkenes, alkynes. zAlkanes
- general formula; methane (greenhouse gas). Complete combustion of methane and ethane, reaction of methane and ethane with chlorine through substitution.
2.
Make a solution of the unknown substance: add sodium hydroxide solution or ammonium hydroxide solution, make observations and give your deduction. Warming the mixture may be needed. Choose from substances containing Ca2+, Cu2+, Fe2+, Fe3+, Pb2+, Zn2+, NH4+.
3.
Supply a solution of a dilute acid and alkali. Determine which is acidic and which is basic, giving two tests for each.
4.
Add concentrated hydrochloric acid to each of the given substances, warm, make observations, identify any product and make deductions: (a) copper oxide (b) manganese dioxide.
zAlkenes
– (unsaturated hydrocarbons with a double bond); ethene as an example.
zAlkynes
- (unsaturated hydrocarbons with a triple bond); ethyne as an example of alkyne.
Only main properties, particularly addition products with hydrogen and halogen namely Cl2, Br2 and I2 pertaining to alkenes and alkynes. INTERNAL ASSESSMENT OF PRACTICAL WORK Candidates will be asked to observe the effect of reagents and/or of heat on substances supplied to them. The exercises will be simple and may include the recognition and identification of certain gases and ions listed below. The examiners will not, however, be restricted in their choice to substances containing the listed ions.
EVALUATION The assignments/project work are to be evaluated by the subject teacher and by an External Examiner. (The External Examiner may be a teacher nominated by the Head of the school, who could be from the faculty, but not teaching the subject in the section/class. For example, a teacher of Chemistry of Class VIII may be deputed to be an External Examiner for Class X Chemistry projects.)
Gases: Hydrogen, Oxygen, Carbon dioxide, Chlorine, Hydrogen chloride, Sulphur dioxide, Hydrogen sulphide, Ammonia, Water vapour, Nitrogen dioxide.
The Internal Examiner and the External Examiner will assess the assignments independently.
Ions: Calcium, Copper, Iron, Lead, Zinc and Ammonium, Carbonate, Chloride, Nitrate, Sulphide, Sulphite and Sulphate.
Award of marks
Knowledge of a formal scheme of analysis is not required. Semi-micro techniques are acceptable but candidates using such techniques may need to adapt the instructions given to suit the size of the apparatus being used.
(20 Marks)
Subject Teacher (Internal Examiner)
10 marks
External Examiner
10 marks
The total marks obtained out of 20 are to be sent to the Council by the Head of the school. The Head of the school will be responsible for the online entry of marks on the Council’s CAREERS portal by the due date.
NOTE: According to the recommendation of International Union of Pure and Applied Chemistry (IUPAC), the groups are numbered from 1 to 18 replacing the older notation of groups IA …. VIIA, VIII, IB …… VIIB and 0. However, for the examination both notations will be accepted. Old notation New notation
IA
IIA
IIIB
IVB
VB
VIB
VIIB
1
2
3
4
5
6
7
VIII 8
9
10
IB
IIB
IIIA
IVA
VA
VIA
VIIA
11
12
13
14
15
16
17
0 18
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7RSLFV)RXQG'LႈFXOW &RQIXVLQJ%\FDQGLGDWHV Examination Paper 2020 z Properties of Ionic and covalent compounds z Writing balanced chemical equations for the given chemical reactions z ,GHQWLÀFDWLRQRIJDVHVDQGFRPSRXQGV z Drawing structural formulae of organic compound z Drawing of isomers z Methods of preparation of salts z Identifying the salts from the given observations z Electron dot diagram z Oxidation / Reduction reaction applied to electrolysis z Reactions and observation at cathode and anode z Problems based on Mole concept z Observation based questions on practical chemistry Observation based questions on practical chemistry z Distinguishing between pairs of compound by using a particular reagent z Reaction of ammonia with excess chlorine and vice versa z Oxidation and reduction in terms of loss and gain of electrons z IUPAC names, common names and numbering of the carbon atoms in the chain z Usage of the sign < and > z (OHFWURQHJDWLYLW\DQG(OHFWURQDIÀQLW\ z Reasoning type questions Examination Paper 2019 z Observations based on practical chemistry. z Writing correct balanced chemical equations. z Methods of preparation of salts. z Structural formulae of compounds with functional groups and IUPAC nomenclature. z Distinguishing between substances on the basis of test/reagent given. z Numerical problems based on mole concept. z Conversion of molecular formula to empirical formula. z Electron dot diagram. z Arranging elements as per the trends in properties across a period and down a group. z Difference between the terms dehydration and dehydrogenation. z ,GHQWLÀFDWLRQRIWHUPVVXFKDVHOHFWURQHJDWLYLW\HWFRQWKHEDVLVRIGHVFULSWLRQVJLYHQ z Catalysts used in various industrial processes. z Components of alloys and their application. z Difference in structure of an aldehyde and alcohol. z Connecting the type of solution to its pH value based on certain observations. Examination Paper 2018 z z z z z z z z z z
6SHFLÀFWHVWVWRLGHQWLI\GLVWLQJXLVKEHWZHHQVXEVWDQFHV IUPAC names of organic compounds. 6FLHQWLÀFWHUPVIRUSURFHVVSURSHUWLHV Observations of different reactions based on practical chemistry. Reasons behind trends in properties across or down the periodic table. Ionic equations, especially involving the discharge of ions/formation of ions. Selective discharge of ions during electrolysis. 'HÀQLWLRQLIORQHSDLURIHOHFWURQV 6FLHQWLÀFUHDVRQVIRUFHUWDLQREVHUYDWLRQV (OHFWURQDIÀQLW\DQG,RQL]DWLRQSRWHQWLDO
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7RSLFV)RXQG'LႈFXOW &RQIXVLQJ%\FDQGLGDWHV z )URWKÁRDWDWLRQDQGURDVWLQJ z Method of preparations of salts in the lab. z 'LVVRFLDWLRQDQG,RQL]DWLRQ z Gases involved in reactions. z Structural formulae of organic compounds. z Difference between precipitate and solution. Examination Paper 2017 z Practical Chemistry and related observations. z Properties of ionic and covalent compounds. z Methods of preparation of salts. z Names of functional groups or their presentation. z Balancing of chemical equations. z Drawing of structural formulae. z Numerical problems based on mole concept and application of Gay Lussac's and Avogadro's Laws. z Arranging elements of periodic table as per the trends in properties across a period and down a group. z Identifying substances based on analytical chemistry. z Selective discharge of ions in electrolysis. Examination Paper 2016 z Numericals based on mole concept and Gay Lussac's Law. z Observations for different reactions. z IUPAC names and structures of organic compounds. z 6SHFLÀFWHUPVLQ3HULRGLFWDEOHDQGRUJDQLFFKHPLVWU\ z Balancing of equations. z Oxidising and reducing agents. z Hydration and hydrogenation. z Solubility of precipitates in excess NaOH and excess NH4OH. z Neutralisation and titration. z Relation between Gram molecular mass and molar volume z 'HOLTXHVFHQFHDQGHIÁRUHVFHQFH z Ionic Reactions at electrodes. z )RUPXODHRIFRPSRXQGVZKHQHOHFWURQLFFRQÀJXUDWLRQVZHUHJLYHQ z Observations when reactants are same but conditions vary. z Trends in the properties of elements across a period and down a group. Examination Paper 2015 z z z z z z z z z z z
Practical based questions where observation had to be enumerated. Application of trends in periodic Table. Concept of g atom and g molecule and the relation with mass and volume. Enumeration of results of electrolysis. Reactions at anode and cathode. Inferences based on Practical observations. Calculations based on chemical equations. IUPAC Nomenclature and structural formulae of organic compounds. Ionic equations involving oxidation / reduction. Various functional groups and their symbolic representation. 6SHFLÀFWHUPVLQRUJDQLFFKHPLVWU\
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6XJJHVWLRQVIRU6WXGHQWV Ö Refer to the syllabus while going through each topic. ÖPractice writing balanced chemical equations. ÖFocus on the colour / solubility of precipitates formed using reagents such as Sodium hydroxide and Ammonium hydroxide. ÖPractice answering observation-based questions. Ö3UHSDUHÁRZGLDJUDPVVKRUWQRWHVWDEOHVIRUIDFWVDQGFRQFHSWV Ö/HDUQWKH/DZVDQGGHÀQLWLRQVZHOOZLWKWKHFRUUHFWWHUPVNH\ZRUGV Ö$FTXLUHNQRZOHGJHRIVROXELOLWLHVRIVDOWVHVSHFLDOO\LQGHFLGLQJWKHPHWKRGVRISUHSDUDWLRQRIVDOWV ÖExpose yourselves to variety of questions by solving past years’ Question Papers. Ö8WLOL]H WKH PLQXWHV· UHDGLQJ WLPH JLYHQ LQ WKH TXHVWLRQ SDSHU WKRURXJKO\ DQG FKRRVH WKH FRUUHFW questions to attempt. ÖDevelop the habit of solving numerical problems stepwise and try to solve as many types of numerical problems, as possible. ÖAlways write down the structural formula of organic compounds with all the bonds properly visible. ÖShow functional group in expanded form and not in the condensed form. ÖAnswer reasoning questions in points by focusing on the main reason. Ö/HDUQDOOUHDFWLRQVDORQJZLWKWKHVSHFLÀFFRQGLWLRQV ÖRemember to distinguish between a pair of compounds using a single reagent, stating that one gives the characteristic reaction while the other does not. ÖRead the questions carefully and answer what is required, e.g., do not write products for observationEDVHGTXHVWLRQVRUWKHIRUPXODIRUDTXHVWLRQZKHUH¶QDPH·LVDVNHG Ö'HYHORSDQLQWHUHVWLQH[SHULPHQWDWLRQDQGHQKDQFHWKHREVHUYDWLRQDOVNLOOVZKLFKZLOOKHOSLQOLNLQJWKH subject. ÖRead the chapters thoroughly to get a very clear concept of the subject matter. ÖEnsure all aspects of the syllabus are covered and avoid selective study of topics. Ö Practice drawing of Structural formulae of organic compounds. Ö &UHDWHFKDUWVZLWKDFRPSDUDWLYHVWXG\RQ+\GURFDUERQV²DONDQHVDONHQHVDQGDON\QHVLQFOXGLQJWKH equations and conditions and various industrial processes. Ö Learn trends in properties across a period and draw a group. Ö Be thorough with observations in practical chemistry and use colours to highlight observations along with tests to differentiate between substances. Ö In a chemical equation, write an acid with its strength(dilute/concentration) Name organic chemical compounds only using IUPAC nomenclature. Ö Select only one reagent when distinguishing between substances and state the result with each substance. Ö )ROORZFRQÀUPDWRU\WHVWIRUFRORXUOHVVJDVHV Ö )RFXV RQ REVHUYDWLRQV VXFK DV VSHFLÀF VPHOO RU VSHFLÀF FRORXU RI SUHFLSLWDWH RU FKDQJH LQ FRORXU between reactants and products. Ö Understand the role of substances used in the extraction of metals in metallurgy. Ö Practice numerical problems regularly, solve numericals stepwise with correct formula and write the answer with correct unit. Ö Pay special attention to reactions involving variations in products formed when conditions change using the same reactants. Ö 6ROYHWKHSUHYLRXV\HDUV·SDSHUVWREHFRPHIDPLOLDUZLWKWKHPRGHRITXHVWLRQLQJDQGPDUNLQJV\VWHP Ö 5HDGWKHTXHVWLRQVFDUHIXOO\DQGWKHQDQVZHUDFFRUGLQJO\ZKDWKDVEHHQDVNHG Ö Avoid selective study. Ö Prepare charts to study topics at a glance, such as Industrial processes, comparative study of Homologous series of hydrocarbons, etc. Ö Practice numerical problems regularly, solve the numericals stepwise with correct formula and write the answer with correct unit. Ö /HDUQGHÀQLWLRQVYHUEDWLPDQGKLJKOLJKWNH\ZRUGV Ö Learn symbols of elements and their valencies. Practice writing balanced chemical equations with necessary conditions. Ö In a chemical equation, write an acid with its strength(dilute/concentration) Ö Name organic chemical compounds only using IUPAC nomenclature. Ö In laboratory listen to the teacher’s instructions carefully, read the experiment thoroughly and then perform it. Ö Select only one reagent when distinguishing between substances and state the result with each substance.
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Study the typical reactions of acids as word equations such as Metal + Acid ® Salt + H2 OR Carbonate + Acid ® Salt + H2O + CO2 Practice structural formulae of hydrocarbons. Solve past years’ papers to understand the pattern of the paper. 5HDGHDFKTXHVWLRQFDUHIXOO\DQGWDNHQRWHRIDOOWKHLQVWUXFWLRQVDQGFRQGLWLRQVPHQWLRQHGLQWKHTXHVWLRQ When a question demands observations, it is not necessary to identify the substance. Observations could LQFOXGHVSHFLÀFVPHOORUVSHFLÀFFRORXURISUHFLSLWDWHRUORVVRIFRORXUDQGVRRQ Any distinguishing test must involve only one reagent or test that would give different results with the two substances being distinguished. :KLOHVROYLQJQXPHULFDOSUREOHPVVKRZVWHSE\VWHSZRUNLQJ :KLOHDQVZHULQJTXHVWLRQVRQSHULRGLFWDEOHGRQRWWU\LGHQWLI\LQJWKHHOHPHQWXQOHVVVSHFLÀHGLQWKH TXHVWLRQ:ULWLQJGRZQWKHHOHFWURQLFFRQÀJXUDWLRQZLWKWKHDWRPLFQXPEHUVNQRZQKHOSVLQDQVZHULQJ questions on trends in properties across the periodic table. 3UDFWLFHGUDZLQJGRWGLDJUDPVDQGPDNHQRWHRIVKDUHGSDLUVDQGORQHSDLUV Ionic bond formation must include depicting the ions formed with appropriate charges, pattern and with a little understanding, writing chemical equations becomes easy. Key words to be highlighted. Bonds should be drawn correctly in structural formulae. :KLOHOHDUQLQJWKHHTXDWLRQVFRQGLWLRQVPXVWEHNHSWLQPLQGWRR Understand ionic equations and place the electrons on the correct side so that total charge on both sides of equations tally. While learning important reactions of sulphuric acid, correctly associate the role of the acid. In metallurgy understand the role of the various substances and electrode materials used. Confusing terms must be given additional time to avoid errors. Solve the earlier Board papers to understand the pattern of questions. Read instructions carefully and avoid haste. Stating observation does not mean identifying the substance. Learn all equations with the relevant conditions. If acids are used, remember to state the concentration. 3D\DWWHQWLRQWRGHWDLOVGXULQJSUDFWLFDOZRUNDQGIRFXVRQERWKREVHUYDWLRQVDQGLQIHUHQFHV /HDUQ WKH YDULRXV WHUPV JHW WR NQRZ ,83$& 1RPHQFODWXUH ZHOO DQG HQVXUH VWUXFWXUDO IRUPXODH DUH represented correctly. ([SRVXUHWRYDULHW\RIQXPHULFDOVLVHVVHQWLDODQGKDELWRIVWHSZLVHZRUNLQJZLOOIHWFKULFKGLYLGHQGV Focus on the colours of precipitates and their solubilities in reagents such as NaOH, NH4OH. Solubilities of salts and properties of salts require special attention to understand the methods of preparation of salts. Knowledge of various types of oxides essential with relevant examples. /HDUQWKHODZVSULQFLSOHVDQGGHÀQLWLRQVYHUEDWLP Learn the tests for identifying the cations and anions and the related observations. 7DEXODWH,QGXVWULDOSUHSDUDWLRQVDQGPDNHDFRPSDUDWLYHVWXG\RIWKHGHWDLOV Study alloys in tabulated form highlighting the main component and the other metals and their special properties. Remember the rules for selective discharge of ions and learn to apply them. Various roles of different substances used must be understood in metallurgy. Ensure all aspects of the syllabus are covered and avoid selective study. Practice solving previous year's Question Papers to get an insight into the pattern of the papers. Ensure every equation written is balanced. Read questions carefully and practice application based questions. 'HYHORSVWHSZLVHZRUNLQJKDELWIRUQXPHULFDOVDQGWU\WRVROYHDVPDQ\YDULHWLHVRIQXPHULFDOVDVSRVVLEOH Read the rules of IUPAC nomenclature and practice drawing the structures of organic compounds. Various terms in metallurgy need to be understood and atleast 2 ores of each of the metal Fe, Zn and Al PXVWEHNQRZQ Learn the mechanism of the various reactions in Organic chemistry using structural formulae.
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