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Home
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Chemistry
WAEC 2011
Chemistry 2011 WAEC Past Questions
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Topics:
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Matter and Separation Techniques
Particulate Nature of Matter
BASIC CHEMISTRY
Chemical Combinations
Properties of Gases ( Gas Laws )
Properties of Solids and Liquids
Acids, Bases and Salts
Periodic Table
Air and Air Pollution
Water and Solubility Concept
Mass-Volume Concepts
Quantitative and Qualitative Analyses
Electrodes, Electrochemical Series and Electrolysis
Types of Reactions
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Reactions' Rates and Chemical Equilibria
Shapes of Molecules and Solids
Radioactivity ( Nuclear Chemistry )
INORGANIC CHEMISTRY
Hydrogen ( Hydrides )
Oxygen ( Oxides - Ozone )
Carbon - Carbon Compounds
Nitrogen - Nitrogen Compounds
Phosphorus - Phosphorus Compounds
Sulphur - Sulphur Compounds
Halogen Family
Silicon and its Compounds
Metals and their Compounds 1
Transition Metals and their Compounds
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Hydrocarbons
Crude Oil
Basic Concepts of Organic Chemistry
Organic Chemistry 2
Applied Chemistry
Chemical Industry
The Solar System
Separation of mixtures and purification of chemical substance
Definition and classification of matter
Elements, compounds and mixtures
Physical and chemical changes
Pure and Impure substances
Separation techniques/processes
Chemical Combination
Stoichiometry
Laws of definite and multiple proportions
Law of conservation of matter
Gay Lussac's law of combining volumes
Avogadro's law
chemical symbols, formulae, equations and their uses
Relative atomic mass based on 12C-12
The mole concept and Avogadro's number
Kinetic Theory of Matter and Gas Laws
States of matter
Change of States of matter
Phenomena Supporting Kinetic theory-Diffusion and Osmosis
Assumptions of Kinetic theory of Gases
The Gas Laws: Boyle, Charles, Graham and Dalton (law of partial pressure), combined gas law
Molar volume and atomicity of gases
The ideal gas equation (PV = nRT)
The relationship between vapour density of gases and the relative molecular mass.
Atomic Structure and Bonding
The concept of atoms, molecules and ions, the works of Dalton, Millikan, Rutherford, Moseley, Thompson and Bohr
Atomic structure, electron configuration, atomic number, mass number and isotopes.
Shapes of S and P orbitals
The Periodic table and periodicity of elements
The variation of the following properties: ionization energy, ionic radii, electron affinity and electronegativity
Chemical bonding
Van der Waals' forces.
Shapes of simple molecules
Nuclear Chemistry
Radioactivity - Types and properties of radiations
Nuclear Reactions - Natural and Artificial Radioactivity, uses and Application.
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The natural gaseous constituents and their proportion in the air
Air as a mixture and some uses of the noble gas
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Water as a product of the combustion of hydrogen and its composition by volume
Water as a solvent
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Water of crystallization, efflorescence, deliquescence and hygroscopy
Solubility
Unsaturated, saturated and supersaturated solutions
Definition of Solubility and Solubility curves and simple deductions
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Qualitative comparison of the conductances of molar solutions of strong and weak acids and bases
Relationship between conductance and amount of ions present, and Buffer solutions
pH and pOH scale; Simple calculations
Acid/base titrations.
Hydrolysis of salts
Oxidation and Reduction (REDOX) Reactions
Oxidation in terms of the addition of oxygen or removal of hydrogen.
Reduction as removal of oxygen or addition of hydrogen.
Oxidation and reduction in terms of electron transfer
Use of oxidation numbers in defining REDOX reactions and balancing simple equations.
IUPAC nomenclature of inorganic compounds using oxidation number
Tests for oxidizing and reducing agents
Electrolysis
Electrolytes and non-electrolytes, and Faraday's laws of electrolysis
Electrolysis of dilute H2SO4, aqueous CuSO4, CuCl2 solution, dilute and concentrated NaCl solutions and fused NaCl
Factors affecting discharge of ions at the electrodes
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Electrochemical cells: Redox series
Half-cell reactions and electrode potentials
Calculations on electrolysis
Corrosion as an electrolytic process
Energy changes
Energy changes accompanying physical and chemical changes
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Entropy as an order-disorder phenomenon
Spontaneity of reactions
Rates of Chemical reaction
Meaning of the rate of a chemical reaction.
Ways of measuring the rate of chemical reaction
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Arrhenius’ law and Collision theory
Reaction rate curves
Chemical equilibrium
Definition of the following terminologies: systems, reactions and dynamic equilibrium.
Properties of a system in equilibrium
Factors governing the equilibrium position
Le Chatelier’s principle
Equilibrium constant
Non-metals and their compounds
Hydrogen and Hydrides
Halogens: Chlorine as a representative element of the halogen
Oxygen and Oxides
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Nitrogen and its compounds
Carbon: Allotropes, Uses and properties.
Metals and their compounds
General properties of metals
Alkali metals e.g. sodium
Alkaline-earth metals
Aluminium and its compound
Tin Extraction from its ores
Metals of the first transition series
Iron Extraction from sulphide and oxide ores
Copper Extraction from sulphide and oxide ores
Alloy
Organic Compounds
Introduction to the tetravalency of carbon
Alkanes: Homologous series in relation to physical properties
Alkenes: Isomerism (structural and geometric isomerism)
Alkynes: Ethyne
Aromatic hydrocarbons e.g. benzene - structure, properties and uses
Alkanols: Primary, secondary, tertiary
Alkanals and alkanones
Alkanoic acids
Alkanoates
Amines (Alkanamines): Primary, Secondary, and tertiary
Carbohydrates
Proteins: Primary structures, hydrolysis and tests
Enzymes and their functions
Polymers: Natural and synthetic rubber
Industrial Chemistry
Chemical industries: Types, raw materials and relevances
Economics of Industrial process
Importance of industrial chemistry in Nigeria
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21
Which of the following statements about a molar solution is correct? it
A.
is a supersaturated solution
B.
cannot dissolve more of the solute at that temperature
C.
contains any amount of solute in a given volume of solution
D.
contains one mole of the solute in 1 dm
3
of solution
View Answer & Discuss
WAEC 2011
22
A gas that is collected by upward delivery is likely to be
A.
heavier than air
B.
insoluble in water
C.
lighter than air
D.
soluble in water
View Answer & Discuss (9)
WAEC 2011
23
Bubbling excess carbon (IV) oxide into calcium hydroxide solution results in the formaton of
A.
CaO
B.
Ca(HCO
3
)
2
C.
H
2
CO
3
D.
CaCO
3
View Answer & Discuss (7)
WAEC 2011
24
The equation P = \(\frac{K}{V}\) illustrates
A.
Boyle's law
B.
Charles' law
C.
Dalton's law
D.
Gay Lussac's law
View Answer & Discuss (1)
WAEC 2011
25
The initial volume of a gas at 300 K was 220 cm
3
Determine
its temperature if the volume became 250 cm
3
A.
183 K
B.
264 K
C.
300 K
D.
341 K
View Answer & Discuss (2)
WAEC 2011
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