Chemistry

Front 1

5 Main Points

Back 1

All matter is made up of tiny particles with spaces between them

Different substances are made up of different types of particles

Particles are in constant motion

Particles move faster as its temperature increases

Particles attract each other

Front 2

States of Matter

Back 2

Solid: Definite volume and shape

Lowest energy

Liquid: Definite volume and takes up the shape of the container

Gas: takes volume and shape of the container

Highest energy

Front 3

Qualitative property

Back 3

Property of a substance that is NOT measured and does NOT have a numerical value

Front 4

Quantitative Property

Back 4

Property that is measure and has a numerical value

Front 5

Physical Changes

Back 5

Change of Shape

Change of volume or size

Change of state

Front 6

5 signs of chemical change

Back 6

Change of colour

Change of odor

Bubbles are visible/gas produced

A new solid is seen (precipitate)

Change in temperature (heat or light is produced)

Front 7

Formula to find density

Back 7

D=M÷V

Front 8

Formula to find Volume

Back 8

V=M÷D

Front 9

Formula to find Mass

Back 9

M=D×V

Front 10

DEFINITION: Characteristic Physical Property

Back 10

A physical property that can identify a substance

Front 11

4 Characterisitic Physical Properties

Back 11

Density

Freezing Point

Melting Point

Boiling Point

Front 12

Effect of salt on ice

Back 12

Alter the freezing point to -16°C

Front 13

Unusual behaviour of Water

Back 13

Solid form is less dense than liquid form

Water particles occupy more space in their solid form

Front 14

Element

Back 14

A pure substance that can't be broken down into simpler chemical substance

Front 15

Element Symbol

Back 15

Abbreviation for a chemical element

Front 16

Compound

Back 16

Chemical substance composed of two or more different elements (Chemically joined)

Front 17

Metals location on P.Table

Back 17

Left side of staircase

Front 18

Non-metals location on P.Table

Back 18

Right side of staircase

Front 19

Metalloids characteristics

Back 19

Element that has properties of both metals and non metals

Front 20

Metals characteristics

Back 20

Lustrous

Malleable

Ductile

Conduct heat and electricity

Front 21

Non-metal Characterisitics

Back 21

Gas

Dull powdery solid

Don't conduct heat and electricity

Front 22

Metalloids location on P.Table

Back 22

Along the staircase

Front 23

Periods in the P.Table

Back 23

Horizontal row

Show trends of increasing or decreasing reactivity

Front 24

Groups/Columns/Families

Back 24

Vertical columns

Elements in the same group have similar properties

Front 25

# of valence electrons in Alkali Metals

Back 25

1 valence electron

Front 26

# of valence electrons for Alkaline Earth Metals

Back 26

2 valence electrons

Front 27

# of valence electrons in Halogens

Back 27

7 valence electrons

Front 28

# of valence electrons for Noble Gases

Back 28

8 valence electrons

Front 29

Reactivity trends: Metals

Back 29

Most reactive metals left side

Further down, more reactive

Front 30

Reactivity trends: Non-Metals

Back 30

Most reactive on upper right side

Further up, more reactive

Front 31

Substances made up carbon

Back 31

Charcoal

Graphite

Diamond

Front 32

Chocolate chip Muffin theory

Plum pudding

Back 32

Thompson

Front 33

Proposed that all matter can be divided into smaller pieces unil a single indivisible particle is reached

Back 33

Democritus

Front 34

Billiard Ball Model

Back 34

John Dalton

Front 35

Gold foil experiment

Back 35

Rutherford

Front 36

Discovered the neutron

Back 36

James Chadwick

Front 37

Electrons orbit the nucleus on specific orbitals/energy levels

Back 37

Niels Bohr

Front 38

Similarities and differences of Chocolate chip Muffin theory and Bohr's theory

Front 39

Atomic number

Back 39

# of protons in the nucleus

Front 40

Atomic Mass

Back 40

Mass of an atom in atomic mass units (amu)

Front 41

Mass Number

Back 41

# of protons and neutron in atoms nucleus

Front 42

Isotopes

Back 42

An atom with the same number of protons but different number of neutrons

Front 43

Standard Atomic Notation

Back 43

Front 44

Maximum # of electrons in shells

Back 44

2

8

8

18

Front 45

Molecules

Back 45

Made up of two or more atoms joined together by chemical bonds

Front 46

Molecular Elements

Back 46

Atoms of the same elements joined together

O2

Front 47

7 diatomic molecules

Back 47

O2

H2

N2

F2

Cl2

Br2

I2

Front 48

Compound

Back 48

Atoms of different elements joined together

Front 49

Chemical formulas

Back 49

Represent elements that exist as molecules and all compounds

Front 50

2 things Chemical Formulas indicate

Back 50

Which elements are present

How many atoms of each element are found

Front 51

Ion

Back 51

Form when an atom loses or gains one or more electrons without changing the # of protons

Front 52

Cation "CAT-ION"

Back 52

Positive charged ion

"PAW-sitive"

Front 53

Anion (ANion A N....)

Back 53

Negative charged ion

Front 54

Octet Rule

Back 54

Atoms gain or lose electrons in order to have a full valence shell

Front 55

Why are Noble Gases stable?

Back 55

They have full valence shells

Front 56

Why are Alkali Metals highly reactive?

Back 56

They only have one valence electron

Front 57

Metal + Metal

Back 57

Metal alloy

Front 58

Metal + Non-Metal

Back 58

Ionic Compound

Front 59

Non-Metal + Non-Metal

Back 59

Covalent Bonds