Ch.3 power point
By N. Mansour
Properties of matter
Substances
Matter is anything that has mass and
takes up space.
Everything around us is matter,
including things that we cannot see,
such as air and microbes.
States of matter
Solids –A solid is a form of matter
that has its own definite shape and
volume.
The particles of matter in a solid are
tightly packed
Solids are incompressible( cannot be
pressed into a smaller volume.
Liquids
Liquids –A liquid is a form of matter
that flows
Has constant volume.
Takes the shape of the container.
The particles in a liquid are not
rigidly held in place.
Liquid particles are able to move
past each other.
Gases
A gas is a form of matter that not
only flows to conform to the shape
of its container, but also fills the
entire volume of its container.
The particles of gases are very far
apart
Gases are easily compressed
Physical properties of
Matter
A physical property is a
characteristic that can be observed or
measured without changing the
sample’s composition.
Examples of physical properties:
Density, color, odor, hardness,
melting point and boiling point
Physical Change
Changes in matter
Physical Changes
Physical Changes: a change, which alters a
substance without changing its composition.
Phase change is a transition of matter from one
state to another.
Phase change is a physical change.
Examples:
* ice melting
* Water boiling
* Water evaporating
• Mixing oil and water
• Melting mercury at -39oC
Chemical change
Chemical change is when a new substance form
different from the original.
The new substances formed will have different
composition and different properties from the
original substances.
Baking soda reacts with vinegar to produce three
new substances ( carbon dioxide, water and
sodium acetate).
Decomposition of sugar ( carbohydrate)
produces water and carbon.
Burning wood produces water and carbon.
Chemical change
Homogenous mixture
The Unit Organizer
BIGGER PICTURE
Name
________________________
Date
_________________________
LAST UNIT/ExperienceCURRENT
UNITNEXT UNIT/ExperienceUnit Map
Unit Vocabulary1. 8. 2. 9. 3. 10. 4. 11. 5. 12. 6.
13. 7. 14.
Application on physical
properties
Part I. Classification - Describe each of the following properties and
either intensive or extensive.
1) Mass
2) Density
5) Reactivity
3) Length
4) Color
6) Volume
7) Malleability
8) Luster
9) Weight
Part II. Define - Use your own words to define the following
terms.
10) Intensive Properties -
11) Extensive Properties -
Answers: Part I.
1) extensive
2) intensive
Elements and Compounds
An element is a pure substance that
cannot be separated into simpler
substances by physical or chemical
means.
On Earth, 92 elements occur naturally.
A compound is made up of two or more
different elements that are combined
chemically.
Most matter in the universe exists in the
form of compounds.
Separating compounds into
components
Electrolysis –separating water into
hydrogen gas and oxygen gas by
passing a current electricity.
Separating the components of
sodium chloride(Salt) into chlorine
gas and white sodium metal.
Application on mixture and
pure substances
Science Help Online Worksheet 1-4a Classification of Matter
Name__________________________Section____________________________
Part I. Classify each of the following substances as; an element, a compound, a
solution, or a heterogeneous mixture.
1. Sand 2. Salt 3. Pure Water 4. Soil 5. Soda 6 . Pure Air
7. Carbon Dioxide 8. Gold 9. Bronze 10. Oxygen 11. Salad Dressing
12. Salt Water
Part II. In the spaces provided, describe the distinguishing characteristics of the
major categories of matter.
13. Element 14. Compound 15. Solution 16. Mixture Answers - part I.
1) mixture
2) compound
3) compound
4) mixture
5)
solution
6) solution
7) compound 8) element
9) solution
10) element 11)
mixture
12) solution Please forward all questions, comments and criticisms to
Electrolysis
Law of Definite Proportion
A compound is always composed of the
same elements in the same proportion by
mass, no matter how large or small the
sample.
Percent by mass% = mass of element X 100
mass of compound
Practice: 1. A 78.0-g of an unknown compound
contains 124g of hydrogen, what is the percent
by mass of hydrogen in the compound?
2. 1.0 g of hydrogen reacts completely with 19.0g of fluorine.
What is the percent by mass of hydrogen in the compound
that is formed?
Mixtures of Matter
A mixture is a combination of two
or more pure substances in which
each pure substance retains its
individual chemical properties.
The composition of mixture is
variable and the number of mixtures
that can be created by combining
substances is infinite.
Types of Mixtures
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Heterogeneous mixture is a mixture that does not blend smoothly
throughout and in which the individual substances remain distinct
Examples: Salad dressing, orange juice ( juice and pulp).
Homogeneous mixture is a mixture that has constant composition
throughout: it always has a single phase
Homogeneous mixtures are also referred to as solutions.
Examples of solution systems
Gas-gas –Air in a scuba tank is primarily a mixture of nitrogen, oxygen
and argon gases.
Gas-liquid –Oxygen and carbon dioxide are dissolved in seawater.
Liquid-gas -Moist air exhaled by the scuba diver contains water droplets,
Liquid-liquid –When it is raining, fresh water mixes with seawater.
Solid-liquid –Solid salts are dissolved in seawater.
Solid-solid –The air tank is made of an allow –A mixture of two metals
Separating Mixtures
Filtration –Is a technique that uses a porous barrier to
separate a solid from a liquid
Distillation –is a separation technique that is based on
differences in the boiling points of the substances
involved
Crystallisation –is a separaton technique that results in the
formation of pure solid particles of a substance from a
solution containing the dissolved subbstance.
Sublimation –process during which a solid changes to
vapor without melting
Chromatography –Is a technique that separates the
components of a mixture based on the ability of each
component to travel or be drawn across the surface of
another material.
Evidence of chemical changes
1. Color
2. Formation of gas
3. Formation of precipitate
4. Absorption of energy
5. Release of energy
Convervation Of Mass &
Matter
Convervation of Mass – Mass is neither
created nor destroyed during a chemical
reaction.
Mass of reactants = mass of products
Mass of baking soda+ vinegar before
chemical reaction = 123.92 g
Mass of carbon dioxide + water+ sodium
acetate (products) = 122.99g
Review material from last week lab/
Demo.
Extensive and intensive
properties
Extensive properties are dependent
on the amount of substance present
Examples: mass, length and volume
Intensive properties are
independent of the amount of
substance present
Example: Density
Chemical Properties of
Matter
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Chemical property is the ability of a
substance to combine with or change into
one or more other substances.
Examples
Iron and oxygen form rust
Magnesium burns brightly when ignited
Combustion
Respiration
Photosynthesis
Mixing baking soda and vinegar