1 Atom
Element
Smallest uncharged. particle that can take part in a chemical reaction
Smallest particle that cannot be broken down by chemical means
2 Molecule
3 Diffusion
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5
6
7
8
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particle made of two or more atoms joined together
Random movement of different particles so they get mixed
up Movement particles from high to low concentration.
Kinetic particle theory Particles of liquids and gases are in continuous random movement
Retardation
It is the ratio between distance travelled by sample from base line to
factor Rf
distance traveled by solvent from base line
Solution
A mixture of solute in a solvent
Solute
A substance that dissolves in a solvent
Solvent
A substance that dissolves another substance
Solubility
The amount of solute dissolved in a certain volume of solvent at a specific
temperature
10 Decanting
11 Distillation
12 Fractional distillation
pouring off the solution leaving solid behind
A method of separating a liquid from a mixture then condensing the vapors
The separation of miscible liquids due to the difference in their boiling
points
Number of protons in the nucleus
13 Atomic number
14 Mass number Nucleon The number of protons plus neutrons in the nucleus
number
A particle (proton or neutron) in the nucleus
15 Nucleon
16 Valence electrons
Electrons in the outer shell of an atom
17 Isotopes (in terms of
Atoms of same element having same atomic number. different mass
subatomic particle)
number Atoms of same element having same proton number.
different neutron
18 Radioactive
An isotope which has unstable nuclei which decompose to emit radiation
A substance made of only one type of atoms
19 Element
20 Compound
A substance made up of two or more different types elements chemically
combined
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21 Mixture
22 MaIleable
23 Ductile
24 Sonorous
25 Lustrous
26 Ion
Two or more substances mixed together but are not chemically combined
27 Ionic bonding
28 Ionic lattice
29 Covalent bonding
Electrostatic force of attraction between the positive and negative ions
Can be beaten into different sha e with a hammer
Can be drawn out into wires
Makes a ringing sound when hit
Has a shiny surface when polished
Electrically charged particle
An atom or a group of atoms that carry electric charge
Regular arrangement of ions
Attraction force between two atoms formed by sharing electrons between
them
30 Covalent lattice
Regular arrangement of atoms/molecules (according to type of structure)
31 Valency
Number of electrons lost. gained or shared by an atom to complete its
outermost shell
32 Giant ionic structure
Continuous three dimensional network of ionic bonds
33 Giant covalent structure Continuous three dimensional network of Covalent bonds
34 Allotropes
Different forms of an element having same chemical properties. different
physical properties
35 Metallic bonding
Electrostatic attraction force between metal positive ions and sea of
delocalized electrons
Formula which shows the number of each type of atoms
36 Molecular formula
37 Empirical formula
Formula which shows the simplest whole number ratio between atoms
38 Structural formula
Formula which shows how the atoms are bonded by covalent bonds
39 Diatomic Molecule
Molecule consisting of two atoms
40 Relative atomic mass (Ar) The average mass of isotopes of an atom relative to carbon-12
41 Relative formula mass
The sum of relative atomic masses of all the ions (or atoms) in a molecule
(Relative molecular
mass)
Mr
The number of particles (ions, atoms, molecules) In one mole of a substance
42 Avogadro's constant
2
43 Electrolysis
44 Electrolyte
The breakdown of an ionic compound by passing electricity through its molten
or aqueous solution
A substance which conducts electricity when molten or dissolved in water
due to the movement of free ions and breaks down during electrolysis
45 Electrodes
46 Cathode
A rod of a metal or graphite that conducts electricity to and from the electrolyte
The electrode at which reduction reaction takes place
47 Anode
48 Electroplating
49 Conductors
The electrode at which oxidation reaction takes place
50 Insulators
51 Exothermic reaction
52 Endothermic reaction
53 Bond energy
54 Fuel
55 Fuel cell
56 Catalyst
57 Activation energy
A process used to gut a thin layer of one metal on the surface of another
metal
Substances which have a low resistance to the passage of electricity
Substances which allow electricity to pass through them easily
Substances which resist the flow of electric current through them
A reaction which gives out energy to the surrounding
A reaction which takes in energy from the surrounding
Energy needed to break a bond or released when a new bond is formed
Substance that release energy when burnt
A Cell Where hydrogen and oxygen react to produce an electric current
A substance that speed up a chemical reaction without being chemically changed
or used up
A substance that speeds up a reaction but remains chemically unchanged at the
end of the reaction
The minimum amount of energy that must be gained by molecules to react at
collision
58 Photochemical reaction A reaction that are started by ultraviolet or visible light
The process by which plants make glucose and omen from carbon dioxide and
59 Photosynthesis
60 Reversible reaction
61 Equilibrium
62 Oxidation
water in the presence of sunlight and chlorophyll which acts as a catalyst
A reaction which goes in both forward and backward directions
A reversible reaction in which the rate of forward reaction equals the rate of
backward reaction
Process of gaining oxygen, losing electrons, losing hydrogen, increase in oxidation
number
3
63 Reduction
Process of losing oxygen, gaining electrons, gaining hydrogen, decrease in
oxidation number
64 Oxidation
A number that describes how oxidized or reduced an atom is
65 Redox reaction
Reactions in which reduction and oxidation occur together
number/state
66 Oxidizing agent
67 Reducing agent
68 Acid
69 Base
A substance which removes electrons or adds oxygen to another substance
A substance which adds electrons or remove oxygen from another substance
Substance that gives hydrogen ions when dissolved in
water
Acid is a proton doner
A compound which reacts with an acid to
form a salt
Base is a proton acceptor
70 Alkali
71 pH Scale
Soluble base which has hydroxide ions dissolved in water
A scale which shows how acidic er alkaline or neutral is a solution
72 Indicator
A substance which changes color according to the PH of the solution
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Salt
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80
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Precipitation reaction
Amphoteric oxide
Alloy
Neutralization reaction
Strong acid/Base
Weak acid/Base
Reactivity series
Thermal decomposition
Ore
Roasting
Global warming
85 Greenhouse gas
Compounds formed when hydrogen in an acid is replaced by a metal or
an ammonium ion
Reaction of an acid with a base to form salt and water
Acids and alkalis that are completely ionized when dissolved in water
Acids and alkalis that are partiallyionized when dissolved in water
A reaction in which two soluble salts are mired to ether to form a solid
Precipitate
An oxide which reacts with both acids and alkalis
A mixture of two or more metals or a metal with a nonmetal
A list of elements in their order of reactivity
The breakdown of a compound into two or more substances by heat
A rock from which a metal can be extracted
Heated strongly in air
The warming of the atmosphere due to the greenhouse gases trapping infrared
radiation from the earth's surface
A as that absorbs infrared radiation from earth's surface
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86 Respiration
87 Corrosion
88 Sacrificial protection
The process by which living things get energy from food
89 Galvanization
90 Fertilizer
Coating a metal (usually iron) with a protective layer of zinc
91 Flue gas desulfurization
It is the removal of sulfur dioxide from the waste gases produced from burning
92 Homologous series
93 Functional group
94 Hydrocarbons
95 Saturated
96 unsaturated
97 Isomers
98
Fraction
99 Cracking
100 Polymerization
101 Monomer
102 Polymer
103 Addition polymerization
104 Condensation
polymerization
105 Condensation reaction
106 Non- Biodegradable
107
Biodegradable
Fermentation
The eating away of the surface of a metal by a chemical
placing a more reactive metal in contact with a less reactive metal to protect it
from corrosion
A substance added to the soil to replace essential nutrients lost when
crops are harvested
fuels
Group of organic compounds having same general formula. same functional
group, same (similar) chemical properties. graduated physical properties and
each two successive members differ by CH2
An atom or a group of atoms which gives a compound characteristic properties
Organic compounds containing carbon and hydrogen atoms only
Contains only single bonds between carbon atoms
Contains a double bond between carbon atoms
Organic compounds having same molecular formula. different structural
formulae
Group Of organic compounds having similar boiling points
Group of organic compounds having limited ran e of carbon atoms
The breakdown of an organic compound into smaller molecules by heat (or
heat and a catalyst
Process of joining large number of small molecules to form a large molecule
Small molecules which join together to form a large molecule
Large molecule formed by joining a large number of small molecules
Process of joining a large number of unsaturated monomers to form a large
polymer
Process of joining two monomers having different functional groups by
eliminating a small molecule
A reaction in which two or more substances combine and a small molecule is
eliminated
Doesn't decompose by bacteria
Decompose by bacteria
Breakdown of glucose by yeast in absence of oxygen to form ethanol and
carbon dioxide
Breakdown of organic material with effervescence and release of heat
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Mole Rules
dm3
dm3
gases only
Important Rules :
 Mass of one mole is the Mr
 To get the concentration in g/dm3 you multiply the
concentration of the substance by it’s Mr
Ex
Concentration of NaoH is 0.02 mol/dm3
so Mr of NaoH = 23 + 16 + 1 = 40
Concentration of NaoH in g/dm3 = 0.02 * 40 = 0.8 g/dm3
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Colours
• All metals are silver-grey except copper (reddish-brown) & gold (yellow)
• Group I & II compounds are white – Colourless in solution
• All noble gases, as well as H2, O2 and N2 are colourless
• All acids are colourless
• Potassium iodide (reducing agent) – Colourless to Brown
• Acidified potassium manganate(VII) KMnO4 (oxidizing agent) – Purple to Colourless
• Potassium dichromate(VI) K2Cr2O7 (oxidizing agent) – Orange to Green
• Transition metals form coloured compounds
• Fe2+ salt – Green
• Cr3+ salt – Green
• Fe3+ salt: Reddish-brown
• All Cu2+ salts are Blue except CuCO3 green & CuO black
• Hydrated copper(II) sulfate – Blue
• Anhydrous cobalt(II) chloride – Blue
• Anhydrous copper(II) sulfate – white White
• Hydrated cobalt(II) chloride – Pink
❖ Group 7 halogens
• Fluorine (g) – Yellow
• Chlorine (g) – Green
• Bromine (l) – Reddish-brown
• Astatine (s) – Black
• Iodine is grey when solid, brown in solution, violet as a gas
❖ Indicators
• Litmus paper – Red (acid), Violet (neutral), Blue (base)
• Methyl orange – Red (acid), Orange (neutral), Yellow (base)
• Phenolphthalein – Colourless (acid & neutral), pink (bases)
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• Thymolphthalein – Colourless (acid), Blue (base)
• Universal indicator – Red
Strong
acid
Orange
Weak
acid
Yellow
Green
Very weak Neutral
acid
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Dark green
Very weak
alkali
Blue
Weak
alkali
Violet
Strong
alkali
Test For
Result
Purity of water
Boiling point(at 100 C) or
Melting point (at 0 C)
CuSo4 + 5H2O
(white)
Presence of water
CuSo4.5H2O
(blue)
OR
CoCl2 (blue) + 6H2O
CoCl2.6H2O(Pink)
Ethanol
Lighted Splint
Flame Produced
Alkenes
Bromine Water
Turns Colourless
Reducing agent
K2Cr2O7(V1)
turns from
orange to green
or
KMNo4(V1)
turns from
purple to colourless
Oxidizing agent
KI
Important Notes :
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turns from to colourless
brown

Antiseptic smell
Organic

Two layers

Colourless drops at the top of the tube

Flame produce

Acid

Organic Acid
Smell of Vinegar

Test for anions
Acidify first
Organic
Hydrated
Flammable
Colourless
MnO2

2H2O2
Or CuO
2H2O + O2

Ammonia & Chlorine
Soluble in Water

Colour Change then back to its original colour

Pungent or
distinctive smell
Reversible
NH3
May be Cl2 according to the test

Excess
More than the reaction needs

Saturated

Concentrated

Two layers of liquid formed

Decomposition of hydrogen peroxide
No more solid can dissolve at this temperature
Small amount of Water
organic compound
MnO2
2H2O2
Or
CuO
2H2O + O2
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