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This ppt file includes:
1. Physical and chemical properties of matter
2. Mixtures and Pure substances
3. Types of Mixtures
4. States of Matter
1.
Properties of Matter
Chapter 16
2.
Extensive = Characteristic of matter in
which the amount of the material affects the
property
Intensive = Characteristic of matter in
which the amount of the material does not
affect the property
3.
List examples of extensive and
intensive properties
4.
Measuring Matter
Measurement Unit instrument
Length Meter (m) Meter stick,
ruler, odometer
Volume Liter (l) or cubic Ruler or graduated
meter cm3 cylinder
Mass Gram (g) or Scale or balance
kilogram (kg)
Temperature Celsius (C0) or Thermometer
Kelvin (K)
density g/cm3 or g/ml Balance and ruler
or graduated
cylinder
5.
Classifying Matter: matter can be
classified into two main types
Mixture Pure Substances
contains more than is matter that cannot
one kind of matter that be separated by
can be separated by physical means
physical means
sugar
Trail mix
6.
Two Types of substances
Elements Compounds
has one kind type of atom
a substance that
contains more than one
examples: type of atom
helium (He) examples:
carbon (C) H2O (pure water)
hydrogen (H)
NaCl (sodium chloride)
oxygen (O)
7.
Matter
Examples of elements:
mercury
aluminum
iodine
9.
Examples of pure substances that are
NaCl = table salt
Water =H2O
Sugar = C6H12O6
10.
Basic units of substances are
always in motion
Atom
is the smallest possible particle of an
element
Molecule
is the smallest particle of the compound that
retains the properties of the compound
11.
Types of mixtures
Heterogeneous Homogeneous
mixture Mixture
the composition is not The composition is
uniform (different) uniform (same)
examples: examples:
chicken noodle soup salt water
mixed nuts tap water
soil brass
12.
What type of mixture is it?
homogeneous
heterogeneous
Salt water
13.
Solutions, Suspensions, and Colloids
It isn’t always easy to tell the difference
between a homogeneous or heterogeneous
mixture.
Based on the size of its largest particles, a
mixture can be classified as a solution, a
suspension, or a colloid.
14.
When substances dissolve and form a
homogeneous mixture, the mixture that
forms is called a solution.
15.
All mixtures can be separated.
Methods to separate mixtures
1. Sorting
2. Filtering
3. Heating
4. Cooling
5. distillation
16.
Matter
Substances
Heterogeneous
mixture
Homogeneous mixture Compounds
elements
17.
Two types of Properties of
1. Aphysical A chemical
property is any property can be
characteristic of a observed only when
material that can be the substances in a
observed or sample of matter
measured without are changing into
changing the different
composition of the substances.
substance in the
material.
18.
Physical Properties
Viscosity= Resistance of a liquid to
flowing
High viscosity
19.
Physical Properties of matter
Conductivity = the ability of matter to
transfer heat or electricity
20.
Physical Properties
Malleability is the
ability of a solid to
be hammered
without shattering.
Hardness is used to compare two diamond
materials. If a material can scratch
another then it is harder.
21.
Physical Properties
Melting point is the temperature at which a
substance changes from a solid to a liquid
(Water in the form of ice melts at 0 0C)
Boiling Point is the temperature at which a
substance boils. (water boils at 100 0C)
22.
Physical Properties of Matter
Density is the ratio of the mass to volume of
a substance.
23.
Chemical Properties
A chemical property is any ability to
produce a change in the composition of
matter.
Chemical properties can be observed only
when the substance in a sample of matter
are changing into different substances.
24.
Observing Chemical Properties
Flammability is a material’s ability to burn
in the presence of oxygen.
25.
Observing chemical properties
The property that describes how readily a
substance combines chemically with other
substances is reactivity.
Examples:
Rusting
Chemical reaction
26.
Indentifying Chemical Change
Common types of evidence for a chemical
change are
1. color
2. production of gas
3. formation of a precipitate
4. Thermal energy change
27.
Identifying a chemical change
28.
States of Matter
Solid
has a definite shape and definite volume
molecules vibrate slow but cannot switch
places with other molecules
29.
States of Matter
Liquid
has a definite volume but no definite shape
Molecules move faster and slip out of
position
30.
States of Matter
Gas
has no definite shape or volume
molecules move so fast that they bounce out
of the liquid state and become a gas.
31.
Temperature= the average energy of the
32.
Changing States of Matter
Melting point Boiling point
temperature at which it temperature at which it
changed from solid to changes from a liquid
liquid to a gas
33.
Changing state of matter
Evaporation Condensation
fast-moving molecules molecules in a gas
in a liquid can escape slow down and change
to become a gas into a liquid
cooling because it take
the energy (heat) away
from the substance
34.
Changes in State of Matter
Sublimation
when a solid changes directly from a solid
to a gas
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