1. CHEMISTRY
Science 9

2. WHY STUDY CHEMISTRY?
In this unit we will be studying atoms, elements and compounds
Brainstorm with a partner how you would complete the following sentences
We are studying chemistry and atoms, elements and compounds because…….
Studying chemistry is of importance in my life because…….
Some things in my everyday life that has to do with chemistry are……

3. LESSON 1: SAFETY
Science 9

4. SAFETY IN THE SCIENCE CLASSROOM
You will be assigned 1 safety rule on pages 10-11
Use the poster paper provided and felts/pencil crayons to make a poster with your safety rule
We will be putting these up in the classroom so take time to make it presentable
You will each present your safety rule to the class
We will have a short quiz at the end of the activity where you will gallery walk around the room to find the answers to the quiz

5. WHMIS SYMBOLS WHMIS: Workplace Hazardous Materials Information System
Symbols are used for chemicals
Tells us about the hazards of the chemical
There are 8 symbols
YES…you need to know these!

6. LESSON 2: INVESTIGATING MATTER
Science 9

7. What is matter? Matter: anything that has mass or volume
Mass: amount of matter in a substance or object (grams)
Volume: amount of space of a substance or object occupies (litres)
Matter can change in 2 ways:
Chemical change
Physical change

8. Chemical Change
Chemical Change: change in matter when substances combine to form new substances
Example: when you light a sparkler it glows white because it contains magnesium and it glows white
Example: Hydrogen and Oxygen combine to form water (H20)
Example: Sodium and Chloride combine to form salt (NaCl)
 in each of these examples, a new substance is formed

9. Physical Change
Physical Change: matter undergoes a change in appearance BUT no new substances are formed
Matter undergoes a change of state
3 states of matter
Solid- matter has a defined shape and volume
Example- ice
Liquid- has volume but shape is determined by its surroundings
Example- water
Gas- mass and volume are determined by its surroundings
Example- evaporated water (steam)

10. Kinetic Molecular Theory (KMT)
Kinetic Energy: energy of motion
All particles (solid, liquid and gas) are always in motion
KMT: the theory that explains what happens to particles when they change between states

11. KMT: The Main Points There are 4 main parts to the KMT theory
All matter is made up of small particles
There is empty space between all particles
Particles are constantly moving regardless of state
Solid- particles packed so close together that they only vibrate
Liquid- particles farther apart so they move more and slide against one another
Gas- particles are very far apart, they move quickly
Energy makes particles move
More energy…particles move faster

12. KMT Demo
Volunteers Please!

13. Temperature and Changes of State

14. Temperature and Changes of State
Melting: solid  liquid at a certain melting point
Evaporation: liquid  gas
Deposition: gas  solid
Sublimation: solid  gas
Condensation: gas  liquid
Solidification: liquid  solid

15. How do we describe matter?
To describe matter we observe the physical properties of a substance in 2 ways
Qualitative properties: properties can be described but not measured
Quantitative properties: characteristics that can be measured

16. How do we describe matter?
Qualitative Properties
State- solid, liquid or gas
Color- what color is the substance?
Malleability- ability to be beaten into sheets
Ductility- ability to be drawn into wires
Crystallinity- shape or appearance of crystals
Magnetism- tendency to be attracted to a magnet

17. How do we describe matter?
Quantitative Properties
Solubility- ability to dissolve in water
Conductivity- ability to conduct electricity or heat
Viscosity- resistance to flow
Density- ratio of a material’s mass to its volume
Melting/Freezing point- temperature of melting/freezing point
Boiling/Condensing Point- temperature of boiling/condensing point

18. Pure Substance
Pure Substance: a substance made up of only one kind of matter (gold, water, oxygen)
2 kinds of pure substances
Element- a pure substance that cannot be broken down or separated into smaller substances
Example: gold, oxygen
Compound- a pure substance composed of at least 2 elements
Example: water

19. Assignment
Page 27 #1-16

20. LESSON 3: ATOMIC THEORY
Science 9

21. Think-Pair-Share
Turn to a partner and discuss what you already know about atoms and the atomic theory
We will share out as a class to see what we already know about the atom

22. Development of the Atomic Theory
The current view of the atomic theory tells us how an atom is constructed
There were 4 scientists that helped develop the current accepted atomic theory: Dalton, Thomson, Rutherford, Bohr
On a piece of paper and using pages make notes of what these 4 scientists contributed to the atomic theory
You will have 15 min to do this then we will continue with the lesson

23. JOHN DALTON (1766-1844) Dalton’s Atomic Theory
All matter is made of small particles that we call atoms
Atoms cannot be created, destroyed or divided into smaller particles
All atoms of the same element are identical in mass and size
Atoms of different elements are different in mass and size
A compound is when atoms of different elements join together in definite proportions (ex- water)

24. JJ THOMSON ( )
British physicist studied electric current in gas discharge tubes
1897- discovered the electron as streams of negatively charged particles
‘raisin bun’ model of the atom: a positively charged ball like a bun with negatively charged electrons embedded in it like raisins
This model was quickly changed with Rutherford’s research

25. ERNEST RUTHERFORD ( )
1909: Designed an experiment to probe inside the atom
Exposed a thin sheet of gold to a stream of heavy positive particles (alpha particles)
Used a fluorescent detector screen which lights up when struck by an alpha particle
Most particles went through the gold as expected
A few bounced backwards…he discovered the nucleus!
Discovered the nucleus, the proton and the neutron
A decade after his original experiment he concluded that the nucleus was made of 2 particles, a positive proton and a neutron with no electric charge

26. NEILS BOHR (1885-1962) Worked under Rutherford
He proposed that electrons surround the nucleus in energy levels or ‘shells’
When electricity is added to neon gas the electrons gain energy and jump from low to high energy levels, when they drop energy/levels the release visible light  this proved that electrons exist in energy levels

27. ATOMIC THEORY
So now we have a clear idea of what’s in an atom and how it was discovered
Atom: smallest particle of an element that still retains the properties of the element
The atom if composed of 3 subatomic particles:
Proton
Neutron
Electron

28. MASS Protons and neutrons have more mass than electrons
Electron mass is negligible compared to protons and neutrons

29. ELECTRIC CHARGE
There are 2 types of electric charges: positive and negative
Protons  positive
Electrons  negative
Therefore, protons and electrons are attracted to one another
Charges add up to zero making the atom uncharged or neutral

30. ATOMIC THEORY Subatomic particles differ in mass and electric charge
Name
Symbol
Relative Mass
Electric Charge
Location in the atom
Proton p
1836 +
Nucleus
Neutron n
1837
Electron e 1 -
Surrounding nucleus

31. NUCLEUS Tiny region at the centre of the atom
Positively charged because of protons
Contains neutrons with no charge
Protons and neutrons never leave the nucleus

32. ELECTRON Occupy shells that surround the nucleus Negligible mass
Account for 99.99% of the volume
Not a fast moving particle, rather it exists like a spread out negative charge around the nucleus

33. ASSIGNMENT
Page 37 #1-15

34. LESSON 4: THE ELEMENTS
Science 9

35. A TOUR OF THE COMMON ELEMENTS
Recall elements have physical properties (ex-state and color) as well as chemical properties (ex-its ability to react)
The periodic table has 2 main types of elements, metals and non metals
Metals: typically hard, shiny, malleable, ductile and good conductors of heat and electricity
Non-Metals: tend to not share the properties of metals and are usually gases or brittle solids at room temperature
Metals and non metals vary in their reactivity

36. A TOUR OF THE COMMON ELEMENTS
Turn to page 45-47
There are 8 common elements-4 are metals and 4 are non-metals
Use the handout provided to summarize these 8 common elements in your own words

37. THE PERIODIC TABLE The Periodic Table Overview
Organizes the elements into their properties
Listed in rows according to increasing atomic number
Rows are arranged to elements with similar properties line up in vertical columns
Rows  called periods
Columns  called families or groups
2 families of metals
Alkali metals
Alkaline earth metals
2 families of non metals
Halogens
Noble gases

38. DIMITRI MENDELEEV
A Russian teacher and chemist who was the first person to organize the elements into what has becomes today’s periodic table

39. THE PERIODIC TABLE
Atomic Number: number of protons in the nucleus of an element
Atomic Mass (weight): mass of the average atom (units are atomic mass unit)
Ion charge: when an atom gains or losses electrons and electric charge forms on the atom called the ion charge
Some atoms have more than one ion charge

40. GETTING TO KNOW THE PERIODIC TABLE
Use the handout of the Blank Periodic Table of Elements and Page 54 of your textbook
Use the information of page 54 to make your own periodic table
Use pencil crayon to color the metals, metalloids and non-metals
Be sure to include the element name, element symbol, atomic number, ion charge and atomic mass  we will learn what these are tomorrow

41. LESSON 5: THE PERIODIC TABLE
Science 9

42. Think-Pair-Share
Brainstorm with a partner what you know about the Periodic Table
What is it?
Why do we have it?
What kinds of things does it tell us?

43. THE PERIODIC TABLE The Periodic Table Overview
Organizes the elements into their properties
Listed in rows according to increasing atomic number
Rows are arranged to elements with similar properties line up in vertical columns
Rows  called periods
Columns  called families or groups
2 families of metals
Alkali metals
Alkaline earth metals
2 families of non metals
Halogens
Noble gases

44. DIMITRI MENDELEEV
A Russian teacher and chemist who was the first person to organize the elements into what has becomes today’s periodic table

45. THE PERIODIC TABLE
Atomic Number: number of protons in the nucleus of an element
Atomic Mass (weight): mass of the average atom (units are atomic mass unit)
Ion charge: when an atom gains or losses electrons and electric charge forms on the atom called the ion charge
Some atoms have more than one ion charge

46. METALS, NON METALS, METALLOIDS
Mendeleev arranged the elements according to their properties
He noticed that 3 main groups existed: metals, non metals, metalloids
State at RT
Appearance
Conductivity
Malleability and Ductility
Metals
Solid, except for mercury (a liquid)
Shiny lustre
Good conductors
Malleable
Ductile
Non Metals
Some gases
Some solids
Only Br liquid
Not very shiny
Poor conductors
Brittle
Not ductile
Metalloids
solids
Can be shiny or dull
May conduct or may not

47. PERIODS AND FAMILIES Period Family Horizontal row = period
There are 7 rows on the periodic table
Family
Vertical row = family
There are 18 columns on the periodic table
Families share similar physical and chemical properties
4 families: alkali metals, alkaline earth metals, halogens, noble gases

48. ALKALI METALS (GROUP 1 EXCLUDING HYDROGEN)
Li, Na, Rb, Cs, Fr
Highly reactive
React with water and oxygen
Reactivity increases as you go down the table
Low melting points
Soft, can be cut with a knife

49. ALKALINE EARTH METALS (GROUP 2)
Be, Mg, Ca, Sr, Ba, Ra
Less reactive than alkali metals but will burn in air if heated
Used in fireworks
Example: red fireworks caused by strontium
React with water but not as much as alkali metals

50. HALOGENS (GROUP 17) F, CL, Br, I, At Non-metals Highly reactive
Fluorine and chlorine are gases at RT
Bromine is a liquid
Iodine is a solid
Fluorine is the most reactive and iodine is the least

51. NOBLE GASES (GROUP 18) He, Ne, Ar, Kr, Xe, Rn
Most stable and unreactive elements
At RT: colorless, odourless gases
Some glow distinctive colors such as neon
Helium is lighter than air which is why helium balloons float

52. MEET THE ELEMENTS LAB Read the Meet the Elements Lab on Page 43
Work with a partner to get to “Meet the Elements”
Record your findings on the handout provided

53. LESSON 6: THE PERIODIC TABLE AND ATOMIC THEORY
SCIENCE 9

54. What do we know?
We know that the periodic table is arranged so that elements with similar properties are lined up..but why?
Patterns occur as a result of regular changes in the structure of the atoms of the elements
Elements with similar properties line up in columns because all those elements are similar in the arrangement of their electrons

55. BOHR MODEL Recall Neils Bohr...
He came up with the Bohr model diagram that shows us how electrons are in arranged in electron shells (also called valence shells)
Electron shells are arranged as follows:
First shell- 2 electrons
Second shell- 8 electrons
Third shell- 8 electrons
Fourth shell- 18 electrons

56. BOHR MODEL So how do we draw a Bohr model?
STEP 1: Figure out how many protons and electrons there are  atomic number
STEP 2: Figure out how many neutrons there are  atomic mass - atomic number
STEP 3: Write the number of protons and neutrons in the nucleus
STEP 4: arrange the electrons into shells of 2 e, 8 e, 8 e, 18 e
Example-Calcium

57. YOUR TURN
You are expected to know how to draw Bohr models for elements 1-20
Use only your periodic table and a piece of paper to draw the Bohr diagram for elements 1-20
You will have 20 min to work on this
This is your ticket out the door…show me your completed Bohr models

58. WHAT DO WE NOTICE?
The outer valence shell contains what we call the valence electrons
Example: calcium has 2 valence electrons
Most elements in the same family have the same number of valence electrons
Halogens have 7 valence electrons
Noble Gases have 8 valence electrons
Elements in the same period have valence electrons in the same shell
The period number indicates the number of shells that have electrons

59. NOBLE GAS STABILITY
Noble gases are unreactive and very stable, but why?
Look at the noble gases Bohr models (Helium, Neon and Argon)…what do you notice about these 3 Bohr models?

60. NOBLE GAS STABILITY
The noble gases all have full outer valence shells which makes them very stable
For a compound to be made atoms have to gain, lose or share electrons in order to make a new substance
Atoms with full valence shells do not easily trade or share electrons
This leads to noble gas stability!

61. WHAT’S SO GREAT ABOUT STABILITY???
So we know the noble gases are stable, and we know why
Most other atoms try to make themselves stable by gaining or losing electrons
Metals lose their valence electrons to become stable like the noble gases
Non-Metals gain electrons to become stable like the noble gases
The result  an ion

62. HOW ATOMS BECOME IONS
Ion: an atom that has gained or lost electrons and therefore carries a charge
An atom of any metal loses electrons  becomes a positive ion (+)
An atom of any non-metal except a noble gas gains electrons  becomes a negative ion (-)
The charge on an ion is equal to the sum of the charges of protons and electrons
Example: Mg +2- has 12 protons and 10 electrons

63. IONS Lithium Magnesium Chlorine Atom Li 3p 2, 1 Mg 12p 2, 8, 2
Cl p 2, 8, 7
Ion
Li+ 3p 2
Mg p 2, 8
Cl p 2, 8, 8
Look at Lithium…what happened to give the ion a positive charge?
Look at Magnesium…what happened to give the ion a +2 charge?
Look at Chlorine…what happened to give the ion a negative charge?

64. ASSIGNMENT
Page 71, # 1, 3-12, 14

65. LESSON 7: COMPOUNDS
SCIENCE 9

66. WHAT IS A COMPOUND?
A compound is a pure substance made up of 2 or more kinds of elements that chemically combine
Elements combine using chemical bonds which link the atoms together
2 types of compounds
Covalent compounds
Ionic compounds

67. COVALENT COMPOUNDS
Atoms combine by sharing electrons to form molecules
These shared electrons form covalent bonds that hold the atoms together
Examples: carbon dioxide, water

68. IONIC COMPOUNDS Atoms gain or lose electrons to form ions
Example: sodium chloride (NaCl)
Atoms start out neutral (with no charge) but as they move towards one another an electron is transferred
Sodium becomes a positive ion (Na+)…it loses an electron
Chlorine becomes a negative chloride ion (Cl-)…it gains an electron

69. TO RECAP

70. POLYATOMIC IONS
Sometimes a compound has both ionic and covalent bonds within the same compound
When this happens you get a molecular ion called a polyatomic ion (‘poly’ means many)
Example: potassium dichromate
Covalent bonds between oxygen and chromium
Ionic bonds between dichromate ion and potassium

71. ASSIGNMENT
Page 83 #1-7, 10-12

72. LESSON 8: NAMING COMPOUNDS
SCIENCE 9

73. REVIEW Brainstorm with a partner…
What is the main difference between an ionic and a covalent bond?
What is a polyatomic ion?

74. #1-DRAW SOME BOHR MODELS
Draw the Bohr model for Sodium
Draw the Bohr model for Chlorine
Now…try to draw the Bohr model for a compound containing sodium and chlorine called… sodium chloride
Notice the change of chlorine to chloride when written as a chemical name

75. #2-DRAW SOME BOHR MODELS
Draw the Bohr model for Potassium
Draw the Bohr model for Flourine
Now draw the Bohr model for a compound that has potassium and bromine…Potassium Flouride

76. #3-DRAW SOME BOHR MODELS
Draw a Bohr model for Calcium
Draw a Bohr model for Flourine
Now draw a Bohr model for Calcium Flouride
What do you notice about the Bohr model compound for Calcium Flouride?

78. #4-DRAW SOME BOHR MODELS
Draw a Bohr model for Aluminum
Draw a Bohr model for Chlorine
Now draw the Bohr model of the compound Aluminum Chloride
What do you notice about the Bohr model?

80. A COMPOUND HAS A NAME AND A FORMULA
Ionic compounds have positive and negative ions
Chemical name is how we name ionic compounds
There are 2 parts to the chemical name of an ionic compound
Positive ion is named first and is always a metal
Negative ion is named second and is always a non-metal
The suffix is always changed to “ide”
Example: flouride, chloride, bromide, iodide, oxide, nitride, phosphide

81. LET’S PUT SOME OF THESE TOGETHER…
The following elements will combine to form ionic compounds. Give the name the following ionic compounds:
Calcium and Nitrogen
Potassium and Oxygen
Lithium and Chlorine
Magnesium and Sulphur
Silver and Flourine

82. PRACTICE PROBLEMS
See page 86 and do practice problems 1a-o

83. A CHEMICAL FORMULA
Chemical formula of an ionic compound has symbols that identify each ion
It also shows the number of ions in the compound
These numbers are shown as subscript
Look back at your Bohr models for sodium chloride and potassium flouride and see if you can write the chemical formula
Look back at your Bohr models for calcium flouride and aluminum chloride and see if you can write the chemical formulas

84. A CHEMICAL FORMULA Sodium chloride  NaCl Potassium flouride  KF
There is 1 sodium atom for every 1 chlorine atom
Potassium flouride  KF
There is 1 potassium atom for every 1 flourine atom
Calcium flouride  CaF2
There is 1 calcium atom for every 2 flourine atoms
Aluminum chloride  AlCl3
There are 1 aluminum atoms for every 3 chloride atoms

85. RULES FOR WRITING CHEMICAL FORMULAS
When writing ionic compound formulas we need to balance the positive and negative charges
The easiest way is to determine the ratio of atoms in the compound
Recall calcium flouride has a calcium to every 2 flourine’s  CaF2

86. RULES FOR WRITING CHEMICAL FORMULAS
4 Step Process to Write chemical formulas:
Identify each ion and its charge
Example: zinc: Zn nitride: N3-
Determine the total charges that needed to balance positive and negative charges
Example: Zn2+ : = +6
N3- : = -6
Note the ratio of positive to negative ions
Example: 3 Zn2+ ions for every 2 N3- ions
Use subscripts to write the formula
Example: Zn3N2
You try… write the chemical formula for aluminum chloride

87. PRACTICE PROBLEMS
Page 87 #1a-f and #2a-n

88. LESSON 9: CHEMICAL FORMULAS
SCIENCE 9

89. REVIEW Name the following ionic chemical formulas CdS AgI CaSe NaF
CaI2

90. WRITING IONIC CHEMICAL FORMULAS
Step 1: Find the chemical symbols on the periodic table of the elements in the compound
Step 2: Figure out the charges on each element…recall, ionic compounds consist of charged ions
Step 3: Criss cross the charges to write the chemical formula
Example: Zinc nitride
Zn+2
N-3
Zn3N2

91. TRY THE FOLLOWING
Write the chemical formulas for the following compounds
Magnesium chloride
Zinc oxide
Aluminum phosphide
Sodium nitride
Calcium oxide
Cesium sulphide

92. WHAT ABOUT IONS WITH MORE THAN ONE CHARGE?
Look at the periodic table…which of the first 20 elements have more than one ionic charge?
How can we distinguish which ion is involved in an ionic compound if there is more than one choice of ionic charge?

93. MULTIVALENT METALS Many metals have more than one ionic charge
They are called multivalent metals
When writing ionic compounds involving a multivalent metal we need to distinguish which ion charge is in the compound
We use Roman Numerals to do this
+1  I
+2  II
+3  III
+4  IV
+5  V
+6  VI
+7  VII

94. MULTIVALENT METAL FORMULAS
Step 1: Identify each ion and its charge in the formula
Step 2: Criss cross the charges
Step 3: Write the formula
Example: iron (III) suphide
Iron (III): Fe +3 sulphide: S-2
Fe2S3

95. YOU TRY
Practice Problems Page 89 1a-n

96. MULTIVALENT METAL NAMES
Step 1: Identify the metals
Step 2: Determine which ion charge will balance the non-metal
Step 3: Name the compound and include the roman numeral that states the ion charge of the metal
Example: Cu3P
Copper can be +2 or +1
The formula states that for every 1 phosphide you have 3 copper
The charge on phosphide is +3
Balance the charges!
Copper (I) phosphide

97. YOU TRY
Practice Problems Page 90 1a-o

98. LESSON 10: CHEMICAL FORMULAS CONT’D
SCIENCE 9

99. CHEMICAL FORMULAS TO KNOW…
Ionic compounds
Ionic compounds with a multivalent metal
Ionic compounds with a polyatomic ion
You are expected to know how to write the names of these types of compounds AND write the chemical formulas of these types of compounds

100. COMPOUNDS WITH POLYATOMIC IONS
Recall that a polyatomic ion is an ion that has both covalent and ionic bonds within it
They carry a charge (positive or negative)
They always pair up with ions of opposite charge
We use a list of known polyatomic ions to write chemical formulas

101. TABLE OF COMMON POLYATOMIC ION

102. WRITING FORMULAS WITH POLYATOMIC IONS
Step 1: Identify each ion (to do this you will have to use the table of polyatomic ions)
Step 2: Identify each charge
Step 3: Criss cross the charges
Example: iron (III) hydroxide
Iron: Fe 3+
Hydroxide: OH- (polyatomic ion)
Fe(OH)3

103. ANOTHER EXAMPLE Ammonium carbonate Ammonium: NH4+ Carbonate: CO32-
Criss cross the charges
(NH4)2CO3

104. LET’S PRACTICE
Practice problems: Page 91 #1 a-j and #2 a-j

105. ASSIGNMENT
PAGE 95: 1-6
You’ll be handing this in as an assignment because I need to know that YOU know how to write and name these chemical formulas…due NEXT CLASS

106. LESSON 11: PHYSICAL AND CHEMICAL CHANGES
SCIENCE 9

107. REVIEW The easiest way to think about naming chemical formulas….
Step 1: look at the elements involved, if there is one metal and one non-metal each with only 1 charge, it is a simple ionic compound
Step 2: if there is a metal with more than one charge it is a multivalent metal and you MUST add in a roman numeral
Step 3: if there is a polyatomic ion you must look at the list of polyatomic ions to find its name

108. Let‘s go back to our first lesson…
Recall we started this unit discussing matter
What did we say was a physical change?
What did we say was a chemical change?

109. PHYSICAL CHANGES A change in state No new substances are formed
No new bonds have formed or broken
Energy changes…recall KMT
Ripping, cutting, grinding and tearing are examples of physical changes
Example: chocolate left in the Sun
Chocolate will melt because of increased energy from the Sun
The atoms in the chocolate are still the same but the state has changed
Nothing new was created…its still chocolate, just melted chocolate

110. CHEMICAL CHANGES Produces new substances with new properties
Always involve energy changes
New bonds are formed and or are broken
A chemical reaction:
REACTANTS  PRODUCTS
Reactants are what you start with, they are what is going to undergo a chemical reaction
Products are what you produce after the chemical reaction has taken place

111. CHEMICAL REACTIONS Evidence of a chemical reaction:
Color change
Heat, light, sound produced or consumed
Bubbles of gas form
A precipitate may form
What are some examples you can think of?

112. CHEMICAL REACTIONS Rotten apples!
As an apple rots it gives off ethene gas (C2H4)
Ethene gas is a ‘chemical messenger’
Ethene gas tells neighboring apples to rot as well
One bad apples can spoil an entire batch of apples!!!

113. CHEMICAL AND PHYSICAL CHANGES AND ENERGY
Chemical and physical changes often occur at the same time
They also are accompanied by energy changes
Example: an explosion is a rapid release of energy
There are 2 main types of reactions:
Exothermic reaction
Endothermic reaction

114. EXO versus ENDO Exothermic Reaction “exo” means leaving
Overall release of energy by heat or light
Endothermic Reaction
“endo” means entering
Involves the overall absorption of energy