1

Unit 1: Atoms, Elements, and Compounds

Pages 3-105

Lithium Atom

Element Lithium

By Lester Green Smallwood Academy Gambo

2

Chapter 1: Atomic theory explains composition and behaviour of matter

Pp 6-35

3

Section 1.1 Laboratory

Safety

Pp 8-13

4

1.01 Demonstrate knowledge of WHMIS standards Safety rules for Science Lab (pp 10-11)

General Safety RulesGlassware Safety RulesChemical Safety RulesHot Plates and Open Flames Safety Rules

Electrical Equipment Safety Rules

5

1.01 continued…

Know the WHIMS symbols

Worksheet: WHMIS

6

1.01 continued…

Dangerous Container

Dangerous Product

Science Lab Safety 1.1 A Page 9

7

Pp 16-19

8

Section 1.2 Investigating matter

1.02 Describe earlier conceptions of the structure of matter with current conceptions

Early Conceptions:Composed of four

“elements”…earth, air, wind, fire.

See Did you know, page 24

9

1.02 continued…Current Conception:

Matter is composed of atoms and atoms contain electrons, protons, and neutrons

See also outcomes 1.10 and 1.11

10

1.02.1 Define matterMatterAnything that has mass and volume.

MassThe amount of matter in a substanceMeasured in grams or kilograms

VolumeThe amount of space a substance

occupiesMeasured in litres or cubic metres11

1.03 Investigate materials and describe them in terms of physical and chemical properties.

Activity 1-2A, page 17

12

1.03.1 Distinguish between chemical and physical properties.

Chemical properties

Observations and measurements of a substance when its reacts with another substance.

Example: reactivity13

1.03.1 continued…Physical properties

characteristic that can be observed or measured on its own.

Examples State Color Density14

1.03.2 List examples of physical and chemical properties. (see p.18-19)Physical Chemical

Color Combustibility

Malleability Reactivity

Electrical Conductivity Flammability

Magnetism

Luster

Density

Melting and boiling points

Texture15

1.04 Investigate materials and describe their physical and chemical properties.

Core Lab 1-2C (p 20)

16

1.05 State a prediction and hypothesis based on observed patterns.

Core Lab 1-2C (p 20)

17

1.06 Compile and display data collected on properties of materials

Core Lab 1-2C (p 20)

18

1.07 Organize data using a format that is appropriate to the experiment.

Core Lab 1-2C (p 20)

19

1.08 State a conclusion based on experimental data.

Core Lab 1-2C (p 20)

20

Pp 24-29

Section 1.3: Atomic Theory

21

1.09 Explain the importance of using the terms laws and theory in science Allows scientist to communicate their

observations Theories are proposed ideas that are supported

by reliable evidence Unlike laws, theories are subject to change if

new evidence is found

22

23

1.09.1 Distinguish between a theory and a law

TheoryExplanations of observations that are supported

by reliable evidenceTheories are subject to change given new

evidence

24

1.09.1 continuedLawsDescribes events,

patterns, or relationships that have been observed.

They state what happens with no explanation

Laws are constant and do not change25

1.10 Identify major changes in atomic theory up to and including Bohr model

26

1.10.1 Describe the contributions of scientists to the development of the atomic theory.

Early GreeksEmpedocles

claimed matter was composed of four “elements”…air, wind, earth and fire.

27

Early Greeks continued…Democritus Substance can be divided

into smaller and smaller pieces until it could be no longer divided.

He called the smallest piece “atomos”

Today we use the word atom

28

Early Greeks continued...Aristole

Agreed with the theory proposed by early Greeks but suggested there was a fifth element.

Belief of the Greek scholars FOUR elements

29

1.10.1 continuedDalton (Billard Ball Theory)Matter composed of small,

hard spheres that are different for each type of elements. Gold spheres are not like lead spheres

He defined the atom as the smallest particle of an element and it could not be divided.

30

1.10.1 continuedJ.J Thomson (Raisin Bun Model) He determined that there were streams of

negatively charged particles (electrons) He concluded that all atoms must contain

these smaller particles.

31

1.10.1 continuedJ.J Thomson (Raisin

Bun Model).He proposed a “raisin

bun” model of the atom.

The bun was positively charged and the raisins were negatively charged

32

1.10.1 continuedRutherfordHis team noticed that

when highly charged particles were fired at gold foil, some bounced back.

Reasoned that there was a concentration of particles

33

1.10.1 continuedRutherfordAn atom was much more than just empty space

of scattered electrons. (as opposed to what the "plum pudding model" proposed)

An atom must have a positively charged center that contains most of its matter

 He called this dense, concentrated center the nucleus 

The positively charged center (nucleus) was relatively small in reference to the total size of the atom  34

1.10.1 continuedRutherford (Planetary Model)

Inside the nucleus there are two kinds of particles

1 Protons…positively charged

2 Neutrons…neutral or no electric charge

35

1.10.1 continuedNeils Bohr (Orbital Model)

Discovered that electrons in an atom are arranged in energy levels or shells.

Electrons have different amounts of energy

36

1.11 Describe Rutherford’s experiment to test Thomson’s atomic model

See previous slides on Rutherford’s gold foil experiment

See page 27 and take brief notes

37

1.11.1 Recognize that the atomic theory continues to be definedEquipment used today were not available

to early scientist.This allows scientist to do different

experiment and to collect data that were not possible in the past.

New data allows scientist to continuously redefined their knowledge

38

1.12 Use models in describing the structure and components of atoms

39

1.12.1 Define atom

The smallest particle of an element that retains the properties of the element.

40

1.12.2 Distinguish among protons, neutrons and electrons.ChargeNeutrons

neutralProtons

positive chargeElectrons

negative charge41

1.12.2 continuedRelative Mass

Neutron…1837 times more than an electron

Proton…1836 times more than an electron

Electron…1

42

1.12.2 continued

Location in the atomNeutron

nucleusProton

nucleusElectron

surrounding the nucleus

43

1.13 Give examples of group settings and individual activities related to atomic structure

Worksheets: Atomic structure

44