grade 9 science - mr. white's course...
TRANSCRIPT
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Unit 1: Atoms, Elements, and Compounds
Grade 9 Science
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Chapter 1: Atomic theory
explains the composition and
behaviour of matter.
Grade 9 Science... Unit 1
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Lab Safety... A Review
Safety MUST be your top
priority.
Know them before you do the
lab and use them while doing the
lab.
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Complete activity 1-1A pg. 9
Laboratory Safety
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Safety Rules for the Science Lab
pages 10-11
General
Glassware
Chemicals
Hot plates and open flames
Electrical equipment
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WHMIS... Page 12
W workplace
H hazardous
M materials
I information
S system
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Hazard Symbols... Page 13
Dangerous
Container
Dangerous
Contents
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Properties of Matter
Matter is anything that has mass and volume.
Mass is the amount of matter in a substance or object.
Volume is the amount of space a substance or object occupies.
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Matter is made up of elements.
Elements are substances that
contain one type of matter and
cannot be broken down or
separated into simpler
substances.
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Describing Matter
1. Physical Properties pg. 18
Characteristics
of matter that
are often
observed or
measured.
Can be either
qualitative
(observed) or
quantitative
(measured).
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•Color
•Malleability
•Lustre
•Conductivity
•Boilingpoint
•Melting point
•Texture
•Magnetism
•Density
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2. Chemical Properties pg. 19
Observed
when
substances
react with
each other.
Determines a
substances
usefulness.
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•Reactivity
•Combustibility
•Toxicity
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Core Lab Activity 1-2C pg. 20
Physical and Chemical Properties
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Theory vs. Law
A theory is less well supported
than a law.
Most laws are supported by
different and robust
experimental evidence.
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Atomic Theory
The descriptions of matter and
how it behaves.
Has undergone many
modifications as new facts
became available.
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Early ideas... 2000 years ago
Empedocles: matter was
composed of four “elements”;
earth, air, water, and fire.
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Democritus: eventually a
substance will be cut into a piece
that can no longer be cut. He
called this piece atomos.
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Development of Atomic Theory
John Dalton (1766-1844)He suggested that the particles that make up matter are like small, hard spheres that are different for different elements.
He defined an atom as the smallest particle of an element.
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Dalton’s Model... Billiard Ball
Model
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J.J. Thomson (1856-1940)
He suggested that all atoms must contain electrons (negative charge).
His model pictured a positively charged ball with the negatively charged electrons embedded in it.
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Thomson’s Model... Raisin Bun
Model
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Ernst Rutherford (1871-1937)
He discovered that atoms have a
nucleus.
There are two kinds of particles in
the nucleus; protons (positive
charge) and neutrons (neutral).
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Rutherford’s Model... Planetary
Model
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Niels Bohr (1885-1962)
He proposed that electrons
surround the nucleus in specific
energy levels or shells.
Each electron has a particular
amount of energy.
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Bohr’s Model... Orbital Model
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• Rutherford was able to develop Thomson’s model due to the development of new technologies. (gold foil experiment)
• The development of cyclotrons and proton accelerators have further developed the model accepted today.
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Summary...
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Inside the Atom
Subatomic
Particle
Charge Mass Location
Proton (p+) + Large Nucleus
Neutron (n) 0 Large Nucleus
Electron (e-) - very
small
Energy levels
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The Atom