[ppt]grade 9 sciencelc.wnlsd.ca/~julia.strickland/fov1-0002b351/s01b8f10d.0/9... · web viewlab...
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Grade 9 Science
Unit 1: Atoms, Elements, and Compounds
Grade 9 Science
Chapter 1: Atomic theory explains the composition and behaviour of matter.
Grade 9 Science... Unit 1
Lab Safety... A Review
Safety rules and procedures MUST be your top priority.
Know them before you do the lab and use them while doing the lab.
Complete activity 1-1A pg. 9
Laboratory Safety
Safety Rules for the Science Labpages 10-11
General
Glassware
Chemicals
Hot plates and open flames
Electrical equipment
WHMIS... Page 12
Wworkplace
Hhazardous
Mmaterials
Iinformation
Ssystem
Hazard Symbols... Page 13
Dangerous Container
Dangerous Contents
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.
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.
Describing Matter
1. Physical Properties pg. 18
Characteristics of matter that are often observed or measured.
Can be either qualitative (observed) or quantitative (measured).
Color
Malleability
Lustre
Conductivity
Boilingpoint
Melting point
Texture
Magnetism
Density
2. Chemical Properties pg. 19
Observed when substances react with each other.
Determines a substances usefulness.
Reactivity
Combustibility
Core Lab Activity 1-2C pg. 20
Physical and Chemical Properties
Theory vs. Law
A law is better supported than a theory.
Most laws are supported by different and robust experimental evidence.
Theories can change or be modified
Laws rarely change
Atomic Theory
Atomic Theory
The descriptions of matter and how it behaves.
Has undergone many modifications as new facts became available.
An atom consists of a
nucleus
(of protons and neutrons)
electrons in space about the nucleus
The Atom
Inside the Atom
Subatomic ParticleChargeMassLocationProton (p+)+LargeNucleusNeutron (n)neutralLargeNucleusElectron(e-)-Very smallEnergy levels
Early ideas... 2000 years ago
Empedocles: matter was composed of four elements; earth, air, wind, and fire.
460 BC
Democritus: eventually a substance will be cut into a piece that can no longer be cut.
He called this piece atomos.
Aristotle
All matter was composed of four elements
Earth, air, water and fire
Development of Atomic Theory
John Dalton - 1808
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.
Daltons Model... Billiard Ball Model
J.J. Thomson - 1898
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.
Thomsons Model... Raisin Bun Model
Ernst Rutherford - 1910
He discovered that atoms have a nucleus.
There are two kinds of particles in the nucleus; protons (positive charge) and neutrons (neutral).
Rutherfords Model... Planetary Model
Rutherford was able to develop Thomsons 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.
Rutherfords Experiment
they fired Helium nuclei at a piece of gold foil which was only a few atoms thick.
Gold foil
Helium nuclei
They found that while most of the helium nuclei passed through the foil, a small number were deflected and, to their surprise, some helium nuclei bounced straight back.
Rutherfords new evidence allowed him to propose a more detailed model with a central nucleus.
He suggested that the positive charge was all in a central nucleus. With this holding the electrons in place by electrical attraction
However, this was not the end of the story.
Niels Bohr - 1913
He proposed that electrons surround the nucleus in specific energy levels or shells.
Each electron has a particular amount of energy.
Bohrs Model... Orbital Model
Summary...