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DIRECTORATE OF SCHOOL EDUCATION, GOVT. OF TAMIL NADU, CHENNAI-600 006 STANDARD X

CHEMISTRY UNIT I: MATTER

Developed by Prof.Dr.V.Balasubramanian, Chair person (Chemistry) Science Syllabus Revision Committee

Chemical reactions and important chemical compounds Expected specific outcomes learning

Contents in terms of concepts

Curriculum transactional strategies

Illustrations

Evaluation

Suggested no. of periods

1

2

3

4

5

6

Recognises the role of rate of reactions in identifying the reactions.

1.1. Rate of chemical reaction.

Graph showing the Explaining the rate of chemical reactions concentration of reactants vs time. – graphical representation.

Analyses the chemical reaction as slow and fast reactions.

1.1.1 Types of reactions. 1.1.2 Slow and fast reactions.

Most of organic reactions are slow due to covalent bonds and all ionic reactions are fast due to ionic bonds. Example – decomposition of hydrogen peroxide.

Reaction with measurable rates.

Giving examples of organic reaction and ionic reaction.

Define rate of a reaction.

1

Reactions between ionic compounds are faster than that between covalent compounds. Justify.

2

1

Analyses the chemical reactions as reversible and irreversible reactions.

1.1.3 Reversible and irreversible reactions.

Meaning of reversibility and irreversibility with examples.

Understands the concept of chemical equilibrium.

1.1.4 Chemical equilibrium – Dynamic equilibrium.

Explain dynamic equilibrium to impact occurrence of reactants and products at a time.

Recognises the importance of energy changes in chemical reactions.

1.1.5. Exothermic and endothermic reactions.

Realises the importance of pH.

1.1.6. pH scale – acidic and basic nature.

Formations of ammonia and sulphur trioxide are exothermic reactions. Formation of NO from NO2 and O2 is an exothermic reaction. 1 pH =log ----- should [H+] be explained.

Formation of hydrogen iodide is a reversible reaction and formation of water is an irreversible reaction. Explain the concept of equilibrium considering the reaction H2 + I2 ? 2HI Chart showing exothermic and endothermic reactions.

What are reversible and irreversible reactions?

Chart showing pH scale

What is meant by pH? Classify the following solutions as acidic or basic or neutral. i.pH = 1.5, ii.pH=8, iii.pH=7

2

What is meant by dynamic equilibrium?

2

What are exothermic and endothermic reactions?

2

2

Unit - 2 - SOME IMPORTANT CHEMICAL COMPOUNDS Relates Science and technology to industry and in domestic life. Learns the manufacture of washing soda. Analyses the properties of washing soda.

2. Some important Naming some chemical compounds chemical compounds. 2.1. Washing soda – preparation

Manufacture by Solvay process

2.1.1. Properties

Physical properties – Existence in two forms namely washing soda and soda ash. Chemical properties – reaction with HCl and BaCl2. Uses – In softening of water, glass industry, soap preparation.

Recognises the uses of washing soda both in industry and house hold purposes.

2.1.2. Uses

Recognises the importance of baking soda

2.2. Baking soda – preparation

Manufacture – by Solvay process (outline only)

Analyses the properties of baking soda.

2.2.1. Properties

Properties like colour, solubility and action of heat can be explained

Chemical compounds are used in day to day life. Diagrammatic representation using block diagram.

2

How is washing soda prepared?

2

What is the action of sodium carbonate with HCl?

Make them to understand the importance of softening of water and how soap is wasted in hard water. Block diagrammatic representation of Solvay process.

Mention the uses of sodium carbonate.

How is baking soda manufactured?

Ask the students to What happens when bring baking sods baking soda is and ask them to heated? study its physical properties.

1

2.2.2. Uses Recognises the use of baking soda in preparing soft drinks. Recognises the importance of bleaching powder. Analyses the properties of bleaching powder.

Recognises the uses of bleaching powder. Learns the preparation and properties of Plaster of paris. Recalls the use of plaster of paris

Use – as baking soda Uses of baking soda in household in effervescent soft preparation. drinks.

Chemical nature and formula. Manufacture using slaked lime and dry chlorine. Physical –moist 2.3.1. Properties white powder, strong suffocating odour as that of chlorine. Chemical –action with HCl. Used for bleaching 2.3.2. Uses cloths, wood, pulp etc., for sterilizing water, as a disinfectant. 2.4. Plaster of paris - Preparation from gypsum. Preparation. Plasticity property 2.4.1. Property. 2.3. Bleaching powder – Manufacture

2.4.2. Uses.

Uses in surgery, for plastic moulds for statues, in dentistry, for making false ceilings.

Explanation through equations.

Write the uses of baking soda.

How is bleaching powder manufactured?

2

How is plaster of Paris prepared?

2

Make the students to tell the physical properties by seeing the bleaching powder. The reason for spraying bleaching powder in streets and in water. Explanation through equation.

Demonstrating, the Write the uses of plaster of paris in students how medicine? moulds are made since it expands on setting.

Recognises the Importance of cement

2.5. Cement Manufacture 2.5.1. Uses of cement

Recalls the manufacture of glass

Analyses an alloy into its constituents uses.

Cement formula Manufacture raw materials required slurry. Building materials Concrete, reinforced cement or RCC, bridges, roofs, multistoried building.

2.6. Glass Manufacture (outline) raw materials required, cooling of glass, annealing 2.6.1 Uses

Briefly explain the manufacture of glass, cooling of glass and annealing.

2.7. Steel

Composition - steel

2.7.1. Alloy steel Stainless steel composition and uses, tungsten steel Composition uses

House hold wares and cutting tools are nothing but stainless steel.

The importance of building materials

What is slurry?

1

How is cement used in construction?

What is annealing ?

1

Used in optical lenses, as mirrors and in domestic life? Role of steel in construction and in domestic life. Mention the uses and composition of steel and tungsten Steel.

1 What are the uses of steel?

1

Unit 3 – NATURAL RESOURCES STANDARD - X

METALS AND NON METALS

Expected specific

Contents in terms

Curriculum

outcomes

of concepts

transactional

no. of

strategies

periods

learning Recognizes the

3.1. Special

Nature of metals

character of metals

and nonmetals in

and nonmetals.

Illustrations

Evaluation

the form of ores. Importance of

3.1.1 Minerals and

Definition of ores and

Showing the picture of What are ores? In

Minerals and ores

ores

minerals

certain important

what way it differs

ores.

from minerals.

in day to day life. Examples of minerals-

Mention important

Bauxite, haematite,

ores of Iron and

mica & pyrolusite,

Aluminium

Some important ores, oxide ores, sulphide ores.

Suggested

Analyses the given

3.1.2. Metallurgy

Introduction-

Listing the ores of Iron

ores into its

Concentration of ores.

components.

Extraction, Refining of metals, occurrence of

Showing the three

ores. Oxide ores -

forms of Iron.

gravity separation Sulphides ores – froth floatation, roasting, smelting, refining. Recalls the

3.2

Forms of Iron

manufacturing

Metallurgy of Iron.

Extraction

from

ores

mentioning

process of iron.

chemical

Showing the picture of the reverbratory furnace.

changes Showing the Picture of

diagrammatic

Bessemer converter.

representation. Explain the

preparation

of

wrought iron from cast Iron. Explain the Preparation of steel using Bessemer converter.

Comparing

3.2.1 Properties of

Comparison of physical

different types of

iron.

properties

of

iron with reference

types of iron.

to properties and

Note

uses.

important

down

three some

chemical-

properties of iron, brief discussion

about

hardening annealing

the and

process

of

steel, mention uses of Iron. Recalls the

3.3

Occurrence in Nature,

Listing of ores.

extraction of

Metallurgy of

Extraction process of

Showing the picture of ores of Aluminum.

aluminum from its

Aluminum

Aluminium from

electrolytic method.

ores.

Mention the important How Aluminum is

bauxite ore.

extracted from

Explanation of

Bauxite.

purification of

How is Aluminum

aluminum.

purified? Give any three important

Recognises the

3.3.1 Properties of

properties and

Aluminium

uses of Aluminium

Discussion of important physical and chemical properties of Aluminum. Use of Aluminum.

chemical reactions of Aluminium? Mention the uses of Aluminium.

Importance of

3.4 Special

Definition of Alloys

Special nature of

Character of Alloys

Illustration of

What are alloys?

composition and uses

Alloys

of alloys in day to day life.

Recalls the

3.5

Explanation

importance of

Alloying of Gold.

examples,

displacement of

1.Activity Series

reacting,

metal from other

2. Displacement of reacting

salts.

one

metal

with Chart showing the high, activity series. low

moderately

from reacting

another metal

and Experiment Mercury

On what basis activity series of metals are arranged?

- tree Electroplating.

nature.

Specific examples CuSO4 + Zn ?

ZnSO4 +

Cu Recognises the

3.6

importance of

Corrosion of metals (impress that it is a about rusting of Iron.

Definition of Corrosion Showing the picture

Corrosion.

chemical change) Corrosion

of

Explain chemical reactions associated with rusting of Iron.

different

metals, rusting of Iron. Analyses the

3.7

Alloying

nature of gold,

Gold,

ornamental and

flexible

pure gold.

alloying

of Explanation

Metallurgy, character,

Importance of "carat" Explain the uses of to check the purity of

Gold Alloys.

Gold.

Why copper is added to gold to make gold

with

copper

it

ornaments.

becomes hard. Recognises the

3.8

abundance of

Introduction about

hydrogen in

Hydrogen.

Occurrence of Source.

nature. Recalls preparation

the 3.8.1. of Preparation of

Hydrogen

Hydrogen

Explanation of simple laboratory method of preparation of hydrogen.

Experiment to

How

is

hydrogen

demonstrate the

manufactured?

preparation using metal with dil. Acid.

Recalls the

3.8.2.

Explain

the

Physical Giving equations for

properties of

Properties of

and

hydrogen.

Hydrogen

properties

Recalls the uses of

3.8.3.

Industrial

hydrogen.

Uses of Hydrogen

Laboratory uses.

Chemical chemical reactions. and Preparation of Vanaspathi by hydrogenation – manufacture NH3. (Water gas) CO + 2 H2 ?

Recalls the importance of ammonia

3.9 Ammonia

CH3OH

Mention

industrial

uses of hydrogen.

Recalls the

3.9.1 Preparation

Explanation

preparation of NH3

of ammonia

laboratory

of

the Experiment to and demonstrate the

industrial

How is NH3 prepared by Haber's process?

preparation preparation.

of ammonia. Recalls the

3.9.2 Properties of

Explain

the

physical Giving equations for

properties and

NH3

and chemical Properties chemical reactions.

uses of ammonia

Experiment to show fountain experiment. 3.9.3 Uses of

Giving - industrial and

Explain the uses of

ammonia

laboratory uses.

ammonia.

Recognises the

3.10 Occurence of

Explain

importance of

sulphur

occurrence of sulphur.

Analyses the

3.10.1 Allotropy of

Demonstration

allotropic nature of

sulphur.

the three allotropes of three types of

the

natural Oral instruction

sulphur

sulphur

about Picture showing the

sulphur.

briefly

on

allotropy of sulphur?

sulphur.

Recalls the

3.10.2 Extraction

Explanation

extraction from

of sulphur

methods of extraction. 1. Sicilian method

natural sources.

Write

of

2. Frasch method.

two Diagrammatic

How

is

sulphur

representation of

extracted?

Mention

extraction of sulphur

the uses of sulphur.

Recalls the

3.10.3 Properties of Explain

properties of

sulphur

sulphur

the

and

physical Demonstrate the chemical action of heat on three

properties.

types of sulphur. Giving equation for chemical reaction.

Recalls the uses of

3.10.4 Uses of

Giving

sulphur.

Sulphur.

medicinal uses.

Recalls

the 3.11

preparation

Preparation of

industrial

and

Laboratory preparation Give of SO2.

equation of Solubility,

proerties ans uses Sulphur dioxide. of sulphur dioxide.

3.11.1 Properties

chemical How SO2 is prepared?

action

of

heat,

Explanation of physical Reaction with oxygen. and

chemical

properties. 3.11.2

Giving Industrial Uses.

Specification

user of sulphur

manufacture

dioxide

sulphuric

in

acid

the of and

bleaching nature.

Recalls the process 3.12 of

manufacturing Manufacturing

sulphuric acid.

sulphuric acid.

Explain the Preparation Illustrate

only

of of sulphuric acid (One chemical equation method)

the Explain in detail the manufacture sulphuric

acid

"contact Process"

of by

Recalls properties sulphuric acid.

the 3.12.1 of Properties of sulphuric acid.

Physical and Chemical Showing

the What happens when

properties - action with

experiments

for H2SO4

water, metal sugar and

chemical reaction

reacts

with

metal?

cellulose. Importance

of 3.12.2

using

Uses of sulphuric

sulphuric acid

Acid.

Explain the Industrial of laboratory Use.

Mentioning

about Mention the industrial

“King of Chemical”

uses acid.

of

sulphuric

Unit - 4 - CARBON COMPOUNDS Expected specific outcomes learning Recognises the classification of organic compounds based on functional groups

Recalls the preparation, properties and uses of alcohol

Recognises the importance of alcohol in domestic life.

Contents in terms of concepts 4.1 Functional group

Curriculum transactional strageries Classification of organic compounds based on functional group 1. alcohol 2. aldehyde 3. ketones 4. carboxylic acid

Illustrations

Evaluation

Naming of alcohols aldehydes, ketones, carboxylic acids taken from lower homologous series.

Name the functional group present in ethanal and ethanol.

4.2 Alcohol

IUPAC name and common name of lower alcohol

4.2.1 Preparation, concentration, fermentation and its importance.

Manufacture of ethanol Fermentation and its importance from "molasses" concentration. can be illustrated

How is ethanol prepared from molasses? What is rectified spirit? How is absolute alcohol prepared?

4.2.2 Properties of alcohol

Physical properties Colour, miscibility. Chemical properties reaction with oxygen, metals, esterification, oxidation, dehydrogenetion, dehydration with

what happens when enthanol is treated with 1. Sodium 2. PCl 5 3. Acetic Acid 4. O2 5. Acidified K2Cr2O7

Encourage the students by writing the chart explaining the properties of alcohols

Suggested no. of Periods 3

4

bleaching powder. 4.2.3 Uses

Recalls preparation, properties and uses of methanal.

Recalls preparation, properties and uses of acetone.

Alcoholic beverages substitute for petrol.

4.3 Aldehyde First two members methanol ethanol IUPAC name and common name 4.3.1 Preparation Preparation of HCHO Direct oxidation of alcohol. 4.3.2 Properties Physical properties of formaldehyde Nature, Boiling point Chemical properties 1. oxidation 2. reduction 3. with INH3 4.3.3 Uses Used in the preparation of bakelite, formalin, urotropine 4.4 Acetone IUPAC name and common name

Nature of alcohol content in medicine and in alcoholic beverages. Mention the IUPAC names

Which is used as substitute for petrol?

Explanation through equation

How is HCHO manufactured?

The reason for high b.p of HCHO

What happens when HCHO undergoes 1. Oxidation 2. Reduction 3. Reaction with NH3

Give the IUPAC names of 1. HCHO 2. CH3CHO

Formalin-Give its uses. Giving the IUPAC name

4.4.1 Preparation Manufacture of acetone Importance of by dehydrogenation of acetone in isopropyl alcohol medicine and in industry

Mention the IUPAC name of acetone.

How is acetone prepared?

4.4.2 Properties

What happens when acetone undergoes the following reactions 1. Reduction 2. Oxidation 3. With conc. sulphuric acid How is acetone useful in industry?

Physical properties smell, density inflammable nature Chemical properties Reduction, Oxidation Chlorination

4.4.3. Uses Recalls the importance of acids present in Natural resources. Recalls the preparation, properties and uses of acetic acid.

Uses - solvent, in the manufacture of sulphonal 4.5 Carboxylic Naming two lower acid. members of carboxylic acid - source of acetic acid 4.5.1 Preparation Carboxylic acid of acetic acid source of acetic acid

4.5.2 Properties

Recognises that acetic acid is technically important solvent.

4.5.3 Uses

Physical PropertiesColour, solubility, anhydrous nature. liquid – soluble in H2O, anhydrous acetic acid and glacial acetic acid. Chemical propertiesformation of salts, formation of esters, decarboxylation, reaction with PCl5, with NH3, with conc. H2SO4, Reduction, dehydration Solvent for cellulose and resin, preservation of food coagulation of

Naming the two members (Formic & Acetic acid) How is acetic acid prepared? Pure anhydrous acetic acid – called as glacial acetic acid

Pure anhydrous acetic acid is called as __________________

Reaction using explanation

What is esterification? Write the conversion of acetic acid to 1. Ester 2. Acetamide 3. Methane Write briefly any three uses of acetic acid.

Recalls manufacture of soaps and detergents

Recalls the properties of soaps and detergents in day to day life.

rubber. 4.6 Soap Soaps are salts of potassium or Sodium salts of long chain fally acids can be emphasized. 4.6.1 Preparation Saponification Advantages and disadvantages. 4.6.2 Detergents Explanation advantages and disadvantages over soaps

Biodegradable property can be explained. Discharge of detergents and water directly on the earth’s surface leads to ground water pollution.

Distinguish between soap and detergent