The Basic Chemistry provides learners the fundamental concept in understanding the subject matter, including matter, its states and classification, mixture, its classification and methods of separations.

1. BSc. Biology/Chemistry - MPCHS

2. Chapter Outline
• General Overview:
– Introduction to Chemistry
– The Scientific Method
• Classification of Matter:
– States of Matter
– Properties of Matter
• Mixtures:
– Homogenous mixture
– Heterogeneous mixture
• Classification of Mixture:
– Methods of separating mixtures
• Elements and the Periodic Table:
– Metal, Non-metal & Metalloid
• Compounds and its relatives:
– Inorganic compounds
– Organic compounds

3. • Upon completion, the students will be able to:
– Define Chemistry, Matter, Substance, Element, Compound
– Discus the Scientific Method and its significance
– Outline the branches of chemistry with their sub-branches
– Classify matter on the basis of physical and chemical properties
– Distinguish between the varies states of matter
– Discus the conversion among the states of matter
– Outline methods of separating mixture

4. 1. Formal sciences:
– Decision theory- economics, psychology, philosophy
– Logic- principles of valid inference & reasoning
– Mathematics - Arithmetic and Algebra
– Statistics- collection, organization, and interpretation of
data.
– Systems theory
– Theoretical computer science
2. Social Science:
– Human Behavior
– Societies
3. Natural/Pure Science:
– Physical science
• Physics
• Chemistry
• Earth science
• Space Science or Astronomy
– Science of Living Things:
• Biology
– Botany
– Zoology
The “Scientific Disciplines," are commonly divided into three major groups:
General Overview

5. • Natural and Social Sciences are empirical sciences, meaning that the
knowledge must be based on observable phenomena and must be
capable of being verified by other researchers working under the
same conditions.
• Natural, Social, and Formal science make up the fundamental
sciences, which form the basis of interdisciplinary and applied
sciences such as engineering and medicine.
General Overview

6. How to Study Chemistry
• Compared with other subjects, chemistry is commonly perceived to be
more difficult, it has a very specialized vocabulary, some of the concepts
are abstract. Nevertheless, with diligence you can complete this course
successfully:
– Attend classes regularly and take careful notes
– Always review the topics you learned in class the same day the topics are covered.
– Think critically, ask yourself if you really understand the meaning of a term or the
use of an equation.
– Don’t hesitate to Ask your Instructor for help on subject matters.

7. INTRODUCTION TO CHEMISTRY
CHEMISTRY- the branch of science concerned with the substances
of which matter is composed, the investigation of their
properties and reactions, and the use of such reactions to form
new substances.
• Chemistry is often called the CENTRAL SCIENCE…
– It is largely an Experimental Science.
• Antoine-Laurent de Lavoisier, a French chemist who is
celebrated as the “Father of Modern Chemistry"

8. • He proved that the transmutation of Water To Earth was
not possible.
• He established the Law of Conservation of Mass, which is
also called "Lavoisier's Law."
i.e. Matter retains its mass even when it changes forms.
• Mass gain = Mass lost
INTRODUCTION TO CHEMISTRY

9. INTRODUCTION TO CHEMISTRY
• He compiled the first complete (at that time) list of elements,
discovered and named Oxygen and Hydrogen along with co-
discoverer Joseph Priestley . (Dephlogisticated Air)
• He helped develop the Metric System of measurement
• He helped revise and standardize Chemical Nomenclature
• Lavoisier wrote the book Elements of Chemistry (1787).

10.  Chemistry is categorized into Five Main
Branches; Namely:
1. Organic Chemistry
2. Inorganic Chemistry
3. Analytical Chemistry
4. Physical Chemistry
5. Biochemistry
INTRODUCTION TO CHEMISTRY
Assignment # 1:
 Outline the sub-branches under
each of the five main branches of
Chemistry
• Due: Next class

11. The Scientific Method
• All sciences, including the Social sciences, employ variations of what is called
the SCIENTIFIC METHOD: (A systematic approach to research)
• The first step is carefully defining the problem
• The next step includes performing experiments
• Making careful observations
• Collecting or recording Information or Data:
• Qualitative data: consisting of general observation about the system
• Quantitative data: comprising numbers obtained by various measurements

12. • When the experiments have been completed, and data have been
recorded, the next step is Interpretation:
• Meaning that the scientist attempts to explain the observed phenomena,
formulating a Hypothesis – a tentative explanation for a set of observation
• Further experiments are devised to Test the Validity of the Hypothesis in as
many ways as possible, and the process begins anew.
The Scientific Method

13. • After large amount of data has been collected, it is often desirable to
summarized the information in a concise way, as a Law:
• LAW: a concise verbal or mathematical statements of a relationship between
phenomena that is always the same under the same condition.
• Ex: Sir Isaac Newton’s Second law of motion:
• Force equals mass times acceleration ( F=ma)
• Meaning an increase in mass or acceleraration of an object always increases the
object’s force proportionally and a decrease in mass or acceleration always
decreases the force.
The Scientific Method

14. • Hypothesis that survive many experimental tests of their validity
may evolve into Theory:
• It is a unifying principle that explains a body of facts and/or those laws
that are based on them.
• Theories too are constantly being tested. If a theory is disproved by
experiment, then it must be discarded or modified so that it becomes
consistent with experimental observations.
The Scientific Method

16. CLASSIFICATION OF MATTER

17. States of Matter
• All substances, at least in principle, can exist in
any of these states: Solid, Liquid, Gas, Plasma
and Bose-Einstein condensates (BEC)
• In a solid, molecules are held close together in
an orderly fashion with little freedom of motion
• Molecules in a liquid are close together but are
not held so rigidly in position and can move past
one another

18. • In a gas, the molecules are separated by
distances that are large compared with the
size of the molecules.
• These states of matter can be interconvert
without changing the composition of the
substance.
o Example: ICE

20. SOLID
The properties of solids include:
• Solids stay in one place and can
be held.
• Solids keep their shape. They do
not flow like liquids.
• Solids always take up the same
amount of space. They do not
spread out like gases.
• Solids can be cut or shaped.
• Even though they can be poured,
sugar, salt and flour are all solids.
• Each particle of salt, for example,
keeps the same shape and
volume.

21. LIQUIDS
• The properties of liquids
include:
• Liquids can flow or be poured
easily.
• They are not easy to hold.
• Liquids change their shape
depending on the container they
are in.
• Even when liquids change their
shape, they always take up the
same amount of space.
• Their volume stays the same.

22. GASES
• The properties of gases
include:
• Gases are often invisible.
• Gases do not have a fixed shape.
• They spread out and change
their shape and volume to fill up
whatever container they are in.
• Gases can be squashed.

28. Plasma

29. Bose-Einstein condensate

32. PHYSICAL AND CHEMICAL CHANGES
1. Produces no new matter
2. It is generally reversible
3. It is accompanied by great
heat change
4. Produces no change of mass
1. Always produces a new kind of matter
2. It is generally not easily reversible
3. Is usually accompanied by
considerable heat change
4. Produces individual substances whose
masses are different from those of
the original substances

33. PHYSICAL AND CHEMICAL CHANGES

34. EXTENSIVE AND INTENSIVE PROPERTIES
• The value of an extensive quantity
depends on the amount of matter
Eg: Mass, Lengths, Volume
• Does not depend on how much matter is
being considered
Eg: Density, Temperature

35. • A substance is a form of matter that
has a definite (constant) composition
and distinct properties.
• Examples include: Water, Ammonia,
Table sugar (sucrose), GOLD, and
Oxygen.
• A mixture is a combination of two
or more substances in which the
substances retain their distinct
identities.
• Mixtures are either Homogeneous
or Heterogeneous:

36. CLASSIFICATION OF MIXTURE

37. HOMOGENOUS MIXTURES
• Alloys

38. HOMOGENOUS MIXTURES
Amalgam:

39. HOMOGENOUS MIXTURES  Brass

40. CLASSIFICATION OF MIXTURE

41. HETEROGENOUS MIXTURES
• Suspension is a heterogeneous
mixture of a Liquid and a Solid. It
involve 2 phases of matter
1. It is cloudy (not as clear as a
solution).
2. It can be filtered.
3. The larger particles settle at the
bottom.
4. It is a mixture of two phases

44. • Emulsion is a heterogeneous mixture
of Two or More Liquids, in which one
ends up as very tiny droplets inside
the other.
• Emulsions are classified into two
categories:
1.) Oil-in-water
2.) Water-in-oil

47. SEPARATING OIL AND WATER

48. SEPARATING OIL AND WATER

50. • Colloids (also known as colloidal
dispersion) may look like a
homogenous mixture, because the
mixture looks very uniform.
Examples: Milk, Mayonnaise, Butter,
Egg Whites.
• Mayonnaise is a mixture of egg
yolk, vinegar and lemon juice.
HETEROGENOUS MIXTURES

62. METHODS OF SEPARATING MIXTURES
• Filtration - separating an insoluble solid from a liquid. An example
of such a mixture is Sand and Waters

63. METHODS OF SEPARATING MIXTURES
• Evaporation: The process by which water (and other liquids) changes
from a liquid state to a vapor or gas state.

64. METHODS OF SEPARATING MIXTURES:
• Simple Distillation separating a Liquid from a Solution.

65. METHODS OF SEPARATING MIXTURES
• Fractional Distillation - separating a Solution of Two Miscible Liquids.
(Miscible liquids are liquids that dissolve in each other). E.g. Water
and Ethanol.

66. • Magnetism - separating mixtures of two solids
with one part having magnetic properties.
• Some metals like iron, nickel and cobalt have
magnetic properties whiles gold, silver and
aluminium do not. Eg: Sand and Iron filling.
• Magnetic elements are attracted to a magnet.
METHODS OF SEPARATING MIXTURES

67. Distinguishing Mixture and Compound
1. The constituent can be separated from one
another by physical methods; chemical
reactions are not necessary
2. Mixtures may vary widely in composition
3. Mixing is not usually accompanied by
external effects such as explosion,
evolution of heat, or volume change ( for
gases)
4. The properties of a mixture are the sum of
the properties of the constituents of the
mixture
1. The constituent elements cannot be
separated by physical methods; chemical
reactions are necessary
2. Compounds are fixed in their
compositions by mass of elements present
3. Chemical combination is usually
accompanied by one or more of these
effects
4. The properties of a compound are peculiar
to itself and are usually quite different
from those of its constituent elements

68.  Pure Substances can be either
Elements and Compounds.
• An Element is a substance that
cannot be separated into simpler
substances by chemical means.
• To date, 117 elements have been
positively identified. Divided into
Metals, Non-metal and Metalloid
 Compound, a substance composed
of atoms of two or more elements
chemically united in fixed proportions
• Generally, compound is classified into:
• Organic compound and inorganic
compounds and further into ionic and
molecular compounds.

70. The Periodic Table of the Elements
• The Periodic Table is a chat showing the
arrangement of all the elements in
accordance with:
– their Increasing atomic number and
recurring Chemical properties.
– They are assorted in a tabular arrangement
wherein
• a Row is a Period and a Column is a Group.
• There are 7 Periods and 8 Groups
• Elements in the same group will have:
– The same valence electron configuration
and hence similar chemical properties
• Elements in the same period will have :
• An increasing order of valence
electrons.
• Therefore, as the energy level of the
atom increases, the number of energy
sub-levels per energy level increases

71. • The first 94 elements of the periodic
table are Naturally occurring.
• While the rest from 95 to 118 have
only been synthesized in laboratories
or nuclear reactors (Man made)
– Technetium was the first element to be
made artificially
• Dimitri Mendeleev, is widely referred
as the Father of the Periodic Table.
– Mendeleev’s periodic table was
based on Atomic weight, he was able
to predict the discovery and
properties of certain elements;
(Gallium and Germanium)
– He created the table by arranging
known elements into Rows and
Columns based on atomic weight and
Chemical Similarities
The Periodic Table of the elements

72. • The main difference between the modern periodic table and
Mendeleev's periodic table is that:
– Mendeleev's table arranged the elements in order of increasing atomic weight
– While the modern table orders the elements by increasing atomic number.
The Periodic Table of the elements

73. • The most recently discovered element,
Ununoctium, was first reported by
Russian scientists from Dubna in 2002
• The Standard Periodic Table style in
use today is attributed to Horace
Deming, an American scientist
The Periodic Table of the elements

75. Chapter Two (2)

81. References:
Primary source Secondary sources