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CHAPTER 1: BASIC CONCEPTS
Chemistry:
"The study of the properties of materials and the
changes that materials undergo"
INTRODUCTION TO MATTER
1. Matter"Matter is the physical material of the universe;
it is anything that occupies space and has
mass"
Audi Majdan – DMC 101 – KLIUC 1
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• Matter can be divided into pure substance
or mixture
2. Substances
• A pure substance has a fixed composition
and unique properties.• Most matter in our daily lives is not a pure
substance, but a mixture of substances.
• Pure substances are composed of either
elements or compounds.
2.1 Elements
• Definition : Substances which cannot be
decomposed into simpler substances by
chemical means
Audi Majdan – DMC 101 – KLIUC
Matter
SubstanceMixture
(2 or more substances)
ElementCompound
(2 or more elements)
2
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• Basic substances for all matter
• Everything in the world is made up from
only 109 different elements.• 90% of the human body is composed of only
three elements: Oxygen, Carbon and
Hydrogen
• Example of elements:
Element Abbreviation
Carbon C
Fluorine F
Hydrogen H
Iodine I
Nitrogen NOxygen O
Phosphorus P
Sulfur S
Aluminum Al
Barium BaCalcium Ca
Chlorine Cl
Helium He
Audi Majdan – DMC 101 – KLIUC 3
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Magnesium Mg
Platinum Pt
Silicon Si
Copper Cu (from
cuprum)
Iron Fe (from ferrum)
LeadPb (from
plumbum)
MercuryHg (from
hydrargyrum)
Potassium K (from kalium)
Silver Ag (from
argentum)
Sodium Na (fromnatrium)
TinSn (from
stannum)
2.2 Compounds
• Definition : Substance composed of two or
more elements.
Audi Majdan – DMC 101 – KLIUC 4
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• United chemically in definite proportions
by mass. For example: pure water is
composed of the elements hydrogen (H) and
oxygen (O)
3. Mixtures
• Definition : combinations of two or more
substances in which each substance retainsits own chemical identity and hence its own
properties.
• Heterogenous mixtures are not uniform
throughout the sample and have regions of
different appearance and properties
Example: Mixture of water and oil
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• Homogenous mixtures are uniform
throughout the sample and individual
substances retain their individual chemical
and physical nature.
• Homogenous mixtures are also called
solutions; the most common type of solution
is described by a solid (the solute) dissolved
in a liquid (the solvent ).
Example: Solution of water and sugar
• Individual components of mixtures retain
their physical and chemical properties.
• → the components can be separated .
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• For example: ethanol can be separated from
water by using distillation process.
• Miscible – two liquids that dissolve in one
another without separating into layers
• Immiscible – two liquids that do not mix
and form into separate layers.
Physical States of Matter
• Matter can exist in 3 physical states:
1. Gas
2. Liquid
3. Solid
Gas
• No fixed volume or shape - it takes the
volume and shape of its container.
• Can be compressed or expanded to occupy
different volumes.
Liquid
• Has a distinct volume
• No specific shape
• Takes the shape of the container
Audi Majdan – DMC 101 – KLIUC 7
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• Cannot be compressed
Solid
• Has a definite shape and volume
• Rigid
• Cannot be compressed
Physical and Chemical Properties
Audi Majdan – DMC 101 – KLIUC 8
SOLID
LIQUID
GAS
Definite
volumeDefinite
Rigid
definitevolume
NO definite
shape
NO distinct
volume NO distinct
shape
Can be
compressed
MATTER
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• Every pure substance has a unique set of
properties - characteristics which allow us to
distinguish it from other substances.
• 2 general properties: physical and chemical .
Physical properties = properties that can be
measured without changing the basic identity of
the substance.
Example: Colour, hardness & density.
Chemical properties = properties of a
substance that may change or "react" to form
other substances.
Example: to explode, to combust.
Physical and Chemical Changes
• Substances can undergo various changes in
properties; either physical or chemical.
• Physical changes - a substance changes its
physical appearance but not its basic
identity. All changes of state (e.g. solid toliquid to gas) are physical changes.
Audi Majdan – DMC 101 – KLIUC 9
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Audi Majdan – DMC 101 – KLIUC 10
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