This document contains the syllabus for a chemistry course at Durban University of Technology. The syllabus covers the following topics over one semester: basic concepts about matter including states of matter, physical and chemical properties; atomic structure and the periodic table; chemical bonding and intermolecular forces; the mole concept and balancing chemical equations; solutions; acids and bases; oxidation and reduction; and introductions to organic and inorganic chemistry. The document provides definitions and examples for key concepts like elements, compounds, mixtures, molecules, and atoms. It also outlines physical and chemical properties of metals and non-metals.

1. TXSA 111
CHEMISTRY
SEMESTER 1—JANUARY 2013
BY: MR PS NKOSI

2. SYLLABUS
 BASIC CONCEPTS ABOUT MATTER.
 ATOMIC STRUCTURE AND PERIODIC TABLE.
 CHEMICAL BONDING AND INTERMOLECULAR FORCES.
 THE MOLE CONCEPT AND BALANCING CHEMICAL
EQUATIONS.
 SOLUTION.
 ACIDS AND BASES.
 OXIDATION AND REDUCTION.
 INTRODUCTION TO ORGANIC CHEMISTRY.
 INTRODUCTION TO INORGANIC CHEMISTRY.
……....................................................................................................
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3. BASIC CONCEPTS ABOUT MATTER
 CHEMISTRY is the study of matter and the changes it
undergoes.
 Structure
 Properties
 MATTER is all substances of the universe, living and
non-living.
 It made up of molecules and atoms.
 It can be changed from one state to another by
 Adding or removing heat
 Pressurizing
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4. Matter is usually classified into three classical states of matter,
with plasma sometimes added as a fourth state for scientific purposes.
From left to right: grains of refined sucrose (a solid), water (a liquid), depiction
of particles in a gas, and a plasma globe (plasma).
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Department of Clothing and Textile Studies 4

5. The properties of substance can
be used in a number of ways:
1. To identify an unknown substance, e.g in chemistry
laboratories, crime labs and medical labs.
2. To distinguish between different substances, e.g.
gold and fake gold.
3. To characterize a newly discovered substance- the
substance is new if it has a unique set of properties.
4. Predicting the usefulness of a substance for specific
applications, e.g carbon monoxide is not used as an
atmosphere in space capsules
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6. PHYSICAL PROPERTIES
 This are characteristics of matter that can be observed
or measured without altering the chemical
composition and identity of the substance.
 E.g. State, colour, density, melting point, boiling point,
volume, temperature, mass.
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7. CHEMICAL PROPERTIES
 This are properties can be observed if a change in
chemical composition and identity of a substance
occurs.
 E.g. Charcoal burns, iron rusts
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8. CLASSIFY EACH OF THE
FOLLOWING AS CHEMICAL OR
PHYSICAL
a) A substance is very hard.
b) A substance melts at 48 degrees.
c) A substance is flammable.
d) A substance is green in colour.
e) A substance does not react with chlorine.
f) A substance decomposes on hearting.
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9. Classify as : Physical or Chemical
properties.
a) Density
b) Ability to burn
c) Explosiveness
d) Solubility
e) Melting point
f) Corrosiveness
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10. A PHYSICAL CHANGE
 This is a change which causes no change in
composition.
 E.g. the melting of ice
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11. A CHEMICAL CHANGE
 Is one which is accompanied by a change in
composition.
 It involves the disappearance of one or more
substances ( reactants) and the appearance of one or
more new substance (product). These changes are
referred to as CHEMICAL REACTIONS.
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12. Classify as : Physical or chemical
changes.
a) Freezing water. f) Digesting of food.
b) Rusting of Iron. g) Absorption of a
c) Evaporation of dry vitamin from the
ice. intestinal tract.
d) Explosion of gun h) Detoxification of a
powder. drug in the liver.
e) Tearing of paper. i) Synthesis of
protein in muscle
tissue.
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13. ENERGY
 Is the capacity to do work.
 It can not be destroyed.
 It can be converted from one form into another.
 Gravitational potential energy to kinetic energy.
 Electrical to kinetic.
 Electrical to thermal (heat).
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14. A PURE SUBSTANCE
 This substance has a definite, invariable composition
and cannot be separated into simpler substance by
physical means.
 HOW IS IT TO DETERMINED WHETHER A
SUBSTANCE IS PURE OR NOT ?
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15. A MIXTURE
 Is a combination of two or more substances in which
the substances retain their identities.
 i.e. there in no chemical reaction between their
components.
 The components may be separated by physical means
 E.g. salt + water
 The components may be in any proportion
 E.g. concentrated or diluted orange juice.
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16. A HETEROGENEOUS MIXTURE
 This mixture contain two or more phases.
e.g
 Sausage and cheese pizza
 Concrete
 Sand and water
 Oil and vinegar (salad dressing)
 Blood
 Milk of magnesia
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17. A HOMOGENEOUS MIXTURE
 This mixture contain only one phase
e.g.
 Sugar dissolve in water
 Air
 Metal alloys
 Gastric juice
 Spinal tap fluid
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18. Are the following classification a
pure or as mixture?
a) Copper f) Wine
b) Air g) Sulphur
c) Milk h) Sugar solution
d) Water i) Blood
e) Concrete j) Urine
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19. Are each of the following mixture
homogeneous or heterogeneous?
a) Salt and pepper
b) Alcohol and water
c) Sulphur and iron
d) Two different salts
e) Milk of magnesia suspension
f) 5% dextrose in water (used for injection)
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20. A MOLECULE
 It made up of atoms which are chemically bonded
together.
 It can be broken down into smaller units only if
chemical changes are allowed to take place.
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21. AN ATOM
 This represents the limits of chemical subdivision of a
molecule.
 E.g. pure substance can be divided into two classes.
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22. ELEMENTS
 Are pure substance composed of homoatomic
molecules i.e atoms of one type.
e.g
 Oxygen (O2)
 Iron (Fe)
 Carbon (C)
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23. COMPOUNDS
 Are pure substances composed of heteroatomic
molecules i.e two or more kinds of atoms.
 Carbon dioxide ( CO2)
 Suphuric acid ( H2SO4)
 Sodium chloride (NaCl)
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24. Classify these classes as
heterogeneous mixture,
homogeneous mixture, pure
substance, compound, element.
a) In which of these classes must two or more substance
present?
b) Which of these classes could not possibly contain
heteroatomic molecules?
c) A variable composition is possible for which of these
classes?
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25. Classify the following as:
elements, compounds or no such
classification
a) Analysis with some elaborate instruments indicates
that substance A contains only aluminium atoms.
b) Substance B and substance C react to give a new
substance D
c) Substance E decomposes on heating to give substance
F and substance G.
d) Heating substance H to 800 degrees causes no change
in it.
e) Analysis shows that substance I contains sulphur and
oxygen.
f) Heating substance J to 620 degrees causes it to
change from a solid to a liquid.
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26. Indicate whether each of the following
statements is TRUE or FALSE. If it false,
change it to make it true.
a) Some pure substance may be decomposed into simpler
substances by chemical change.
b) The smallest characteristic unit of a pure substance is an
atom.
c) Molecules of pure substances are always heteroatomic.
d) Heterogeneous mixtures can be separated into
component substance by physical means.
e) In order for matter to be heterogeneous at least two
substances must be present.
f) Pure substance can be variable composite.
g) The limit of physical subdivision is a molecule.
h) A compound contain only one type of molecule.
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27. PROPERTIES OF METALS
 Solid (one liquid – mercury)
 Shiny
 Malleable – can be pounded into sheets.
 Ductile – can be drawn into wires.
 High electrical conductivity.
 High thermal conductivity
 Oxides, if soluble, form alkaline solutions in water.
 Tend to form positive ions
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28. PROPERTIES OF NON-METALS
 Generally gases, some solids, one liquid
 Not shiny
 Not malleable nor ductile
 Poor conductors of heat or electricity
 Oxides, if soluble, form acidic solutions in water
 Tend to form negative ions.
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29. ATOMIC STRUCTURE AND
PERIODIC TABLE.
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Department of Clothing and Textile Studies 29