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
