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