Class 10 Chemistry Cbse

Chemistry Concept Maps Class X • Chemical Reaction and Equation • Acids and Bases • Metals and Non-Metals • Carbon and Its compounds • Periodic Table

Class-X(Chemistry)

Addition of O 2Mg + O2 2MgO

N2 + O2

2NO – 180 KJ

Endothermic

Exothermic

Redox

Displacement

2H2

+

O2

Addition of H 2Na + H2 2NaH

Types of Reaction

Double

Reduction

Decomposition

2H2O

Thermal decomposition 2HgO

Compound + Compound NH3 + HCl

NH4Cl

CaO + CO2

Change of colour CuCO3

CuO + CO2 Black

CHEMICAL REACTION

Compound 2CO2

Signals for reaction

Evolution of gas

Green

Heat

2Hg + O2

Compound

Compound + Element 2CO + O2

CaCO3

Removal of O 2HgO 2Hg + O2 Addition of e– – Cl2 + 2e– 2Cl

Combination

Compound

Removal of e– 2+ Mg Mg + 2e–

Oxidation

Single

Element + Element

Removal of H 2HI I2 + H2

N2 + 3H2

Electrolysis

Photo decomposition

2H2O

2AgBr hn 2Ag + Br2

Characteristics of reaction

2NH3 + 92.2 KJ

Electric Current

2H2 + O2

Breaking & making of bonds involved

Energy changes

Change of state

Formation of ppt. AgNO3 + NaCl

Reactants White ppt

2H2(g) + O2 (g)

Products

AgCl + NaNO3

(participating species)

(Newly substances formed)

(Thermal, electrical , light, etc. energy)

Class-X(Chemistry)

Idea about weights of reactants & products

No idea about physical state

Unbalanced equation

Idea about valency

No idea about precipitate

MgO

Mg + O2

Symbol equation

Idea about Volume of gases involved

No idea about concentration

Idea about molecules

No idea about heat changes

Idea about reactants & products

No idea about reversibility

Types of chemical equation

balanced equation 2Mg + O2

2MgO

2Mg + O2

Magnesium + oxygen

2MgO

Specialities of chemical equation Precipitate represented by ppt.

Limitation of chemical equation

CHEMICAL EQUATION & REDOX REACTION IN EVERY DAY LIFE

Rectification of chemical equation

Rancidity Redox Reaction in every day life

Harms

Generally products of combustion (harmful gases)create pollution 2Fe2O3 . xH2O (Reddish brown)

Respiration

Uses

Corrosion

(Green)

Corrosion of iron

Paints

Corrosion of copper

Greasing & oiling

Heating in presence of oxygen accompained with evolution of heat & light e.g. Combustion of LPG 2C4H10 + 13O2

(Black)

Corrosion of silver

8CO2 + 10H2O + Energy

Combustion of CNG CH4+ 2O2

Galvanisation Ag2S + H2

( (

Important biochemical reaction which releases energy in the cells, accompanied by combustion of glucose

C6H12O6(s) + 6O2(g)

Combustion

Prevention Cu(OH)2. CuCO3

(

(

Favorable conditions represented on arrow

Pollution

2Ag + H2S

Heat evolution represented by + heat in RHS & heat absorbed by – heat in RHS Irreversible reaction

CH4(g) + 2O2(g)

2Cu + O2 + H2O + CO2

Concentration represented by dil. & conc.

Reversible reaction

Oxidation of fats & oil present in food

4Fe + 3O2 + xH2O

Magnesium oxide

Word equation

No idea about favourable condition

• Air tight container Prevention • By N2 • By antioxidants e.g. BHT, BHA, etc. • Refrigeration

Heat

(Coating the surface of iron objects with thin layer of zinc)

CO2 + 2H2O + Energy

6CO2 + 6H2O + Energy

Class-X(Chemistry) 2NaCl –

(i) Soap & Detergent (ii) Refining of petroleum (iii) Dye industries (iv) concentration of bauxite ore

373 K

–

–

2Cl Cl2 + 2e (Anode) + – 2Na + 2Hg + 2e 2NaHg (Cathode) 2NaHg + 2H2O 2NaOH + H2 + 2Hg

Uses CaSO4.2H2O

+

2Na + 2Cl

Preparation

Certain short contain definite amount of some H2O molecules loosely attach on moleculesthese are known as hydrated salts.

White

Definition

CaSO4.1/2H2O + 3/2H2

CuSO4 + 5H2O

Blue vitrol(Blue colour)

Example Blue vitrol

Preparation

CuSO4.5H2O

Caustic Soda (NaOH)

Plaster of paris (CaSO4.1/2H2O

Hydrated salts

Preparation

Uses (i) In sealing gaps (ii) Making toys, cosmetics & casts of statues (iii) Cast for setting broken bones (iv) Making moulds in pottery (v) Making design on walls & ceiling

NaOH(aq) + HCl(aq)

(i) To make wool shrink proof Uses (ii) Used as bleaching agent in paper & textile industries (iii) for disinfecting water to make it free from germs (iv) in preparation of chloroform Preparation (CHCl3)

Ca(OH)2 + Cl2

313 K

Sodium chloride(NaCl)

SOME IMPORTANT CHEMICAL COMPOUNDS

Bleaching powder Ca(OCl)Cl

Washing soda Na2CO3.10H2O

Baking soda NaHCO3

Na2SO4 + H2O + CO2 (iv) In paper, textile, ceramic etc.industries

Preparation Na2CO3 + 10H2O Na2CO3.10H2O

Preparation

Uses Ca(OCl)Cl + H2O (i) used in baking powder (ii) In medicine as soda bicarb (antacid) (iii) In fire extinguisher 2NaHCO3 + H2SO4

Uses

2NH3 + H2O + CO2

(NH4)2CO3

(NH4)2CO3 + 2NaCl

Na2CO3+NH4Cl

Na2CO3 + H2O + CO2

2NaHCO3

Uses (i) Cleansing agent (ii) Softening hardwater (iii) Manufacture of glass (iv) Consituent of several dry soap powder (v) Manufacture of borax (Na2B4O7.10H2O)

(i) In muscle contraction, in conduction of nerve impulse in the nervous system (ii) It is used as a fertilizers for sugar beet (iii) In leather industry for leather tanning (iv) Row material for chemicals like HCl, NaHCO3 etc. (v) In severe cold rock salt is spread on icy roads to melt ice.

Class-X(Chemistry) Contains three replacablehydrogen e.g. H3PO4 TriContains two replacablehydrogen e.g. H2SO4, H2CO3 etc. basic Di-basic

Weak acid

Completely ionised in aqueous solution e.g. H2SO4, HNO3, HCl etc. Strong acid

Contains one replacablehydrogen e.g. HCl, HNO3, CH3COOH etc. Mono basic Obtained from plants & animals Organic e.g CH3COOH, HCOOH etc. acid

On the basis of basicity

On the basis of strength

Dilute acid

On the basis of conc.

On the basis of source

Obtained from minerals Inorganic e.g H2SO4, HNO3, HCl etc.

Partially ionised in aqueous solution e.g. H3PO4, H2CO3, CH3COOH etc.

Little amount of water e.g. Conc. HCl, conc. H2SO4 etc.

Conc. acid

Types of acids

acid

High amount of water e.g. dil. HCl, dil. H2SO4 etc.

Reaction with base

Sour in taste Turns blue litmus to red

Chemical properties

General properties

Gives H+ ions in aqueous solution

Reaction with Metal+ acid 2Na(s) + 2HCl(aq) Metal

BASES General properties

Chemical properties

Partially ionised in aqueous solution

–

Gives OH ions in aqueous solution Donates pair of electrons

On the basis of strength

Weak base

e.g. NH4OH, Cu(OH)2 etc.

On the basis of conc. On the basis of acidity

Completely ionised in aqueous solution e.g. NaOH, KOH etc.

Strong base

Mono acidic

Contains one – replacable OH group e.g. NaOH, KOH etc.

Di-acidic Contains two replacable OH– group e.g. Ca(OH)2, Ba(OH)2 etc.

Triacidic

Conc. base

Contains three OH– group e.g. Fe(OH)3, Al(OH)3 etc.

Dilute base High amount of water e.g. dil. NaOH

Little amount of water e.g. conc. NaOH

water

Na2CO3(s)

+

Reaction with Metal Metal + Base Zn + 2NaOH(aq)

Salt

+ water

Salt + water + CO2

2HCl(aq)

Salt

+ hydrogen

2NaCl(aq) + H2O

Reaction with Metal carbonate + acid metal carbonate or bicarbonate & bicarbonate

Types of bases

Turns red litmus to blue

Salt

Reaction with Metal oxide + acid Na O(s) + 2HCl(aq) metal oxide

ACIDS

+

2NaCl(aq) + H2

2

Gains pair of electrons Generally corrosive

Bitter in taste

Salt

Acids + base HCl (aq)+ NaOH(aq)

2NaCl(aq) + H2O + CO2

+ Hydrogen

Na2ZnO2 + H2

Note : Applicable only for some metals (Zn, Sn, Pb, Al etc.)

Reaction with non-metal oxide Non-metal oxide + CO2 (g)

+

Base

2NaOH (aq)

Salt

+ Water

Na2CO3(aq) + H2O

Reaction with acid Base

+ Acid

2NaOH(aq) + H2SO4(aq)

Salt

+

Water

Na2SO4 (aq) + H2O

Solution 1. 1M Hydrochloric acid 2. Battery acid 3. Dilute hydrochloric acid 4. Gastric juices (Digestive juices in stomach) 5. Lemon juice 6. Vinegar 7. Soft drinks 8. Wine 9. Oranges

pH 0 0.5 1.0 1.0 - 3.0

Solution 14. Urine 15. Saliva 16. Blood 17. Eggs

pH 5.5 - 7.5 6.5 - 7.5 7.3 - 7.5 7.8

2.2 - 2.4 2.4 - 3.4 3.0 2.8 - 3.8 3.6

18. Baking soda solution 19. Sea-water 20. Washing soda solution 21. Lime-water 22. Milk of magnesia [Mg (OH) 2 solution]

8.4 8.5 9.0 10.5 10.5

10. Tomato juice

4.0 - 4.4

11.6

11. Beer 12. Coffee 13. Milk

4.0 - 5.0 4.5 - 5.5 6.5

23. 1 M Ammonium hydroxide (Household ammonia) 24. Dilute sodium hydroxide 25. 1 M Sodium hydroxide

13 14

+

Formula

Negative logarithm + of H ion concentration

by soap (basic)

Effect of acidity in soil is neutralised by Ca(OH)2 pH of Solution

Acidity (gastric problem) is neutralised by antacid such as NaHCO3, Mg(OH)2 etc.

Neutralization Reaction

SALTS & INDICATORS

Definition

Salts which contain two or more acidic or basic radicals Mixed Salts e.g. Ca(OCl)Cl, NaKCO3

Poisoning effect of stings of wasp (alkaline) is neutralised Poisoning effect of stings of by vinegar (acidic) ant & bees (acidic) is neutralised

Application

pH values of some common substances

pH = –log10 [H ] + –pH or [H ] = 10

Class-X(Chemistry)

Olfactory

Salt

Obtained by crystallisation Double salts of two simple salts from mixture of this saturated Basic salts solution Contains replacable OH e.g. K2SO4.Al2[SO4)3.24H2O . e.g Pb(OH)Cl, Cu(OH)NO3

Acid + Base

Indicators Normal salts Contains no replacable + – H & OH Acidic salts NaCl, K2SO4 etc. Contains replaceable H e.g. NaHCO3, KHSO4

Salt + Water

HCl(aq) + NaOH(aq)

Change its colour in different medium. e.g. Clove Oil, Vanila extract, Raw onion

Visual

Blue litmus

Original colour Blue

Colour in acidic medium Red

Colour in basic medium Blue

Red litmus

Red

Red

Blue

Indicator

Turmeric

Yellow

Yellow

Reddish-brown

China rose

Pink

Dark pink (magenta)

Green

Methyl orange

Orange

Red

Orange

Phenolphthalein Purple Cabbage juice

Colourless

Colourless

Pink

Purple

Red

Green

Lithium

Li

Potassium

K

Barium

Na + IE

Sodium

Na

Calcium

Ca

Magnesium

Mg

+e

Aluminium

Al

Zinc

Zn

Iron

Fe

Nickel

Ni

Tin

Sn

Lead

Pb

Hydrogen

H

Copper

Cu

Mercury

Hg

Silver

Ag

Gold

Au

Platinum

Pt

–

Na + Cl

+ EA

–

Non-metal + Oxygen C + O2 S

+

O2

Chemical properties of non-metal

SO2

Fe, Mo

Properties

Non-Metal

METALS & NON-METALS

Physicall properties of metal & non-metal

Metal

Reaction with oxygen Metal

+

4Na

+

Oxygen O2

2Na2O( at room temperature)

2Mg

+

O2

2MgO (heating)

2Zn

+

O2

2ZnO (Strong heating)

2Cu

+

O2

2CuO (Prolonged heating)

Metal oxide

Reaction with water Generally gaseous Low m.p. & b.p.

Generally Solid High m.p. & b.p.

Generally soft Bad conductor of heat & electricity

Malleable

Good conductor of heat & electricity

Not ductile

ductile

Reaction with Hydrogen

Do not have any lustre

lustrous

Not sonorous Low density

Metal + Water

Sonorous High density

Metal oxide or Hydroxide + H2

2Na

+ 2H2O(cold water)

2NaOH + H2

Mg

+ H2O(boil water)

MgO + H2

Zn

+ H2O(steam)

ZnO + H2

3Fe(red hot) + 4H2O(steam)

Fe3O4 + 4H2

Reaction with dilute acid

Generally hard

Br2 + KCl(aq)

Non-Metal hydride 2H2O 2NH3

(iv) High m.p. & b.p.

(vii) Good conductor of electricity in molten and aqueous state

Chemical properties of metal

No reaction

Less reactive + Salt Non-metal

(ii) Solid & hard due to strong electrostatic forceof attraction (iii) Definite crystal structure (v) Soluble in polar solvents like H2O (vi) Brittle nature

No reaction

Reaction with salt solution

Non-Metal + Hydrogen + 2H2 O2 + 3H2 N2

Ionic compound

Non-metal oxide

Brittle

More reactive + Salt Non-metal Cl2 + KBr(aq)

(i) Consist of ions

Ionic bond

CO2

Reaction with dilute acid Non-metal + Acid

Definition

Reactivity series

Reaction with water Non-metal + Water

or NaCl Example : formaion of NaCl

Reaction with oxygen

Class-X(Chemistry)

Electrostatic force of attraction due to which positively & negatively charged ions are bonded with each other is known as ionic bond. Compound containing ionic bonds is known Definition as ionic compound e.g. NaCl, MgO etc.

(2,8,8)

(2,8,7) +

–

(2,8)

(2,8,1)

Ba

+

Na + e

Metal + dil. acid 2Na

+

Mg

+ H2SO4

2HCl

Salt + Hydrogen 2NaCl + H2 MgSO4 + H2

Reaction with salt solution More reactive metal + Salt Fe + CuSO4(aq) Fe + ZnSO4(aq)

less reactive metal + salt Cu + FeSO4(aq) No reaction

Class-X(Chemistry) Natural Substances in which metals or their compounds occur e.g. Bauxite, Haematite etc.

METALLURGY

Mineral

Impurities associated with minerals are collectively known as gangue or matrix.

Gangue

Mineral from which the metal can be conveniently and profitably extracted

Conversion of big rocks (ore) into reasonable size particles

Ore Crushiing by gyratory crusher

Crust ore particles are reduced to fine powder

Grinding or Pulverisation by stamp mill or ball mill

This methods is based on the principle on difference in the wetting properties of the ore and gangue particles with oil and water respectively

Crushiing & Grinding Hydraulic washing or gravity separation

Used for sulphide ores such as galena (PbS), HgS etc.

Froth floatation

Concentration of ore

Used for ores of iron, tin & Lead

This methods is based upon the difference in the densities of ore particles and impurites (gaunge) This method depends upon the difference in the magnetic properties of ore and gangue

Magnetic separation Used for ore of iron such as haematite (Fe2O3)

Heating of concentrated ore in absence of oxygen

Calcination Used for carbonate, oxide and hydrated ores e.g. calamine (ZnCO3), Siderite (FeCO3)

Conversion of ore into metal oxide

Roasting Used for sulphide ores e.g. galena (PbS), Cinnabar (HgS)etc.

Reduction by heating

Used for carbonate, oxide and hydrated ores e.g. calamine (ZnCO3), Siderite (FeCO3)

Electrolytic reduction

Heating of concentrated ore in presence of air(Oxygen)

Conversion of metal oxide into metal

Used for ores of low reactive metals e.g. HgS

Reduction by carbon

Chemical reduction

Reduction by carbon monoxide

Reduction by Used for ores of aluminium moderately reactive metals e.g. Fe2O3 , MnO2 etc. It is used for refining of many metals such as Cu, Sn, Ni, Ag etc.

Electrolytic refining

It is used for refining of Si, Ge etc.

Refining of metal

Zone refining

Distillation

Liquation Van arkel method It is used for refining of Ti, Zr etc.

It is used for refining of metals having low m.p. such as Sn, Pb, Bi etc.

It is used for the purification of volatile metals such as Hg, Zn etc.

Class-X(Chemistry)

(O=O)

Example N2, , C2H2 (N º N) (HC º CH)

Exhibit both Crystalline and noncrystalline structure

Physical state may be solid liquid or gas

Low m.p.& b.p.

Generally Soluble in non-polar solvent like benzene, CCl4 etc.

(H2C = CH2)

Double bond

Triple bond

(H–H)

(H3C – CH3)

Single covalent bond

Types of covalent bond

H2 molecule

Covalent bonding

Characteristics

Bad conductor of electricity

Example: H2 , C2H6

Example: O2 , C2H4

Representation

Consist of molecules

CH4 molecule

BONDING IN CARBON & ALLOTROPY

• Tetrahedral structure • Every C-atom attach with 4 another carbon atom by covalent bond

Lamp black

Charcoal

Diamond

Amorphous

Allotropes of carbon

• Fullerene (C60) shape is like Structure a soccer ball with 20 hexagonal ring and 12 pentagonal rings • It is also known as bucky ball

Crystalline

Fullerene

Uses • Act as insulator, semiconductor and super conductor under suitable condition • Catalyse the photochemical refining in industry.

• Used as dry lubricant

O

O

O=O

O2 molecule

H2O molecule

• Transparent & colourless • Refractive index = 2.45 • Specific gravity = 3.51 • Bad conductor of electricity Properties • Good conductor of heat

Structure

Coke

Cl2 molecule

• Used as a jem in jewellery • Used for glass cutting • Used as die for drawing wires from metal Uses • Used in making drill • Used in high precision thermometre & protective windows for space probes

Graphite

Properties

Structure

• Used in making crucible • Used as neutron moderator• Grey in colour & opaque • Specific gravity = 2.26 in nuclear reactor • Specific gravity = 2.26 • Used in steel, retorts & • Soft and has a soapy touch brake lining • High m.p & good conductor of electricity

• Layers with hexagonal rings present

• Each C-atom attach with another 3 C-atom with covalent bond • Each C-atom has single free electron • Two adjacent layers attach with weak vander waals forces

Class-X(Chemistry)

Unsaturated hydrocarbon burns with yellow sooty flame Non-conductor of electricity (due to higher % of carbon) Colourless liquid

Saturated hydrocarbon burns with blue clean flame (due to lower % of carbon)

boiling point 351 K Miscible with water Neutral to litmus

Terms related to alcohol

Chemical properties Conc.H2SO4

CH3CH2OH + 3O2 CrO3 CH3CH2OH Glacial acetic acid

CH3CH2OH

KMnO4

2CH3CH2OH + 2Na

Oxidation Substitution reaction Chemical Rx of carbon compounds

Alcohol (e.g. Ethanol)

Absolute alcohol

CH3CH2OH

Burning of hydrocarbons

Power alochol

Denatured alochol

Rectified spirit

Physical properties

CARBON COMPOUNDS

2CO2 + 3H2O + Heat CH3CHO By mild agent

2CH3 CH2ONa + H2

CH3– CH3

CO2 + 2H2O + Heat

CH4 + 2O2

Ethanoic acid

Esterfication

Acidic character

Oxidation

Decarboxylation Reaction with sodium

Ni

" # Heat

Combustion

CH3CH2OH + CH3COOH

CH3COOH By strong agent

CH2= CH2 + H2 "

Addition of halogen

CH2=CH2 + H2O Reaction with conc. H2SO4

Combustion

Addition of hydrogen

CaO CH3COONa + NaOH " " !" # CH4 + Na2CO3

Rx with metal carbonate

conc.H2SO4

CH3COOCH2CH3 + H2O

Rx with active 2CH3COOH + 2Na metal

Rx with base

CH3COOH + NaOH

Esterification 2CH3COOH + Na2CO3

2CH3COONa + H2O + CO2

2CH3COONa + H2

CH3COONa + H2O