1. Group Reading Assignment pg 170-71
Grade 10 Chemistry Unit
Group Reading Assignment pg
Try This Activity Pg 171

2. LAB SAFETY View Safety Video at:
Count the number of safety violations in the video
Lab Equipment Checklist (CA 2)
Set up Lab Tables – Use the equipment listed in the Activities

3. LAB SAFETY Safety Quiz on the next slide
WHMIS and Safety Worksheet (CA3 , 4)
Use the internet and your textbook pg
Q 1,2 pg 179
Safety Quiz on the next slide
Number a blank piece of notepaper 1-15
Label each activity
Place an *next to the safety violations in your list

4. 12 13 11 10 14 9 8 4 7 6 5 2 3 1 15

5. Chemistry in a Bag Lab (CA 5,6)
Introductory Lab
Chemistry in a Bag Lab (CA 5,6)

6. Chapter 5 Chemicals in Action
What is chemistry?
Chemistry is the study of matter, its properties and its changes or transformations.
Matter is anything that takes up space and has mass. All types of matter have physical and chemical properties.

7. Physical properties include: state at room temperature (solid, liquid or gas), temperature, colour, odour, lustre, solubility and melting and boiling points.

8. Chemical properties include how matter reacts with: air (oxygen),acids, bases, and water

9. 5.1 Chemicals and chemical Change
There are many different types of matter that make up our world:
Pure substance – all the particles that make up this matter are the same, as a result this matter has constant properties e.g. pure water is a clear colourless substance that freezes at 0 C and boils at 100 C.

10. a) Pure substances can be classified as:
Elements – cannot be broken down into a simpler substance because they are made of only 1 kind of atom e.g. gold, oxygen, and mercury. These elements can be identified by a chemical symbol found on the periodic table (Au, O, Hg). Some elements consist of molecules, which are formed when 2 or more atoms join together; for example oxygen (O) occurs in nature as pairs of oxygen atoms or molecules of oxygen (O2)

11. Compounds – contain 2 or more different elements in a fixed proportion
Compounds – contain 2 or more different elements in a fixed proportion. Compounds can be identified with chemical formulas e.g. carbon dioxide (formula CO2) is a compound. Each molecule of carbon dioxide is made of 1 atom of carbon and 2 atoms of oxygen. Other examples of compounds are water (H2O), sodium chloride (NaCl or salt), and ammonia (NH3).

12. Mixtures can be classified as:
2)     Another type of matter is a mixture. Mixtures are made of 2 or more pure substances and can be separated by some physical method e.g. filtering, evaporation, and magnet. E.g. salt water with sand in it. The sand can be filtered with filter paper and the salt can be separated from the water by evaporating the water.
Mixtures can be classified as:

13. Solutions – a mixture where one pure substance is dissolved in another pure substance e.g. salt in water, oxygen in air, copper in a brass loonies.

14. Homogeneous mixtures – a mixture that has 2 pure substances but appears to be only 1 pure substance e.g. Kool-Aid is a mixture of flavour crystals, sugar and water

15. Heterogeneous mixture – a mixture that has 2 or more pure substances that can be seen as separate parts or layers e.g. pizza is made of cheeses tomato sauce and pepperoni

16. Matter
Pure Substance
Mixture
Element
Compound
Solution
Heterogeneous
Homogeneous

17. Properties of Matter
A physical change is a change in the size or form of a substance, which does not change the chemical properties of the substance e.g. boiling water, or dissolving sugar in water.

18. A chemical change occurs when a substance changes into a new substance with different chemical properties e.g. iron rusting or burning charcoal.

19. The starting materials in a chemical change are called reactants and the new materials made are called products.
Iron oxygen makes rust or iron (III) oxide
Fe O makes Fe2O3
Reactants Products

20. Chemical Tests
How are chemical changes useful? Chemical changes can be used to make a new substance or identify an unknown substance. There are 4 chemical tests that can be used to identify an unknown colourless gas:
1)      Oxygen Gas – a glowing splint bursts into flames
Oxygen Test

21. 2)     Hydrogen Gas – a lit splint will cause a small explosion or pop sound
Hydrogen Test
POP!!

22. 3)     Carbon dioxide Gas – a chemical called limewater will turn from colourless to white if exposed to carbon dioxide

23. 4) Water Vapour (Gas) – cobalt chloride paper will change from blue to pink

24. Assignment Lab : Properties Testing Properties of Substances (CA 7,8)
Homework : Questions 1-10 pg 175
Assignment
Answer Key

25. 5.5 Elements and the Periodic Table
In Lab E1 you discovered that some substances are electrolytes and some are non electrolytes or conductors or non conductors of electricity when they are dissolved in water. What makes electrolytes different from nonelectrolytes? We can use the periodic table of Elements to help answer that question.

26. Periodic Table – an organized arrangement of elements that help us to explain and predict physical and chemical properties. The periodic table is generally arranges with metals toward the left side and the nonmetals towards the right side. One exception is hydrogen (H). Although it is located on the top left hand side of the periodic table it behaves mostly as a non-metal.

28. Chemical Families – elements have been grouped in columns or families
Chemical Families – elements have been grouped in columns or families. Chemical families are groups of elements in the same vertical column that have similar physical and chemical properties.
1)      Alkali metals (group 1) – include lithium (li) , sodium (Na), and potassium (K) and all are shiny, silvery metals. They form compounds that are white solids and very soluble in water

29. 2)     Alkaline Earth Metals (group 2) – include magnesium (Mg), calcium (Ca), and barium (Ba) and all are shiny , silvery metals, but they form compounds that are not soluble in water

30. 3)     Halogens (group 17) – include fluorine (F), chlorine (Cl), and bromine (Br) and are all poisonous elements that react easily with sodium and all other alkali metals.

31. 4) Noble Gases (group 18) – include helium (He), and neon (Ne) and do not form compounds. The other term for the noble gases is inert gases. Inert means does not react.

33. Elements and Atomic Structure
What are atoms made of?
The Bohr-Rutherford model of the atom suggests that atoms are made of 3 types of subatomic particles
1)      protons – heavy positively charged particles that are found in a dense positive core of the atom called the nucleus. The number of protons equals the atomic # of the element on the periodic table

34. 2)     Neutrons – neutral particles that have the same mass as a proton and are also found in the nucleus. The number of neutrons in an atom can vary. (atomic mass – atomic # on the periodic table)

35. 3)
Electrons – negatively charged particles with almost no mass that circle the nucleus at different energy levels, also called orbits or shells. Since atoms are electrically neutral that number of electrons equals the number of protons

37. The key to understanding the formation of compounds is to understand the arrangements of electrons around the nucleus. The farther away an electron is from the nucleus the more likely it is to be involved in a chemical change.

38. The electrons in the outer orbit (valence electrons) are involved in bonding atoms together to form compounds.

39. Bohr diagrams are used to represent the arrangement of electrons in various orbits of an atom35 17 Or Cl

40. nucleus
1st nrg level
2nd nrg level
3rd nrg level

41. Atomic Symbols     A full atomic symbol includes the symbol of the element with the atomic number at the bottom left corner and the mass number at the top left corner.     Copy Atomic Symbol Here 84 Kr 36

42. Consider what might happen to the charge of a neutral atom if the outer orbit of electrons are decreased or increased in number.

43. When this occurs the atom becomes a charged particle called an ion.
Ion’s can be positively charged (caused by a loss of electrons from the outer orbit) or negatively charged (caused by a gain of electrons in the outer orbit).

44. The symbol of the atom changes to indicate the change in ionic charge Li becomes Li +1 when a lithium atom loses 1 electron or N becomes N –3 when a nitrogen atom gains 3 electrons.
Positive ions have the same name as their original atom, but negative ions are renamed by changing the ending of atom (ine) to (ide) e.g. fluorine (F) becomes fluoride (F-1).

45. magnesium lost 2 electronsMg
Symbol of a
Magnesium
Atom
Metal Atoms to Ions
Mg 2+
Symbol of a
Magnesium
Ion
Notice 2+ means
magnesium lost 2 electrons Mg
Atom
12p+
2e-
8e- Mg
Ion
12p+
2e-
8e- Ne
2e-
8e-
Magnesium
atom
Magnesium
Ion by losing
2 electrons
becomes
To be
like
Its nearest
Noble Gas

46. sulphur gained 2 electrons
Symbol of a
Sulpur
Atom
Nonmetal Atoms to Ions
S 2-
Symbol of a
Sulphide
Ion
Notice 2- means
sulphur gained 2 electrons
And the name changed S
Atom
16p+
6e-
2e-
8e- Ar
Atom
18p+
8e-
2e- S
Ion
16p+
8e-
2e-
Its nearest
Noble Gas
Sulphur
atom
To be like
becomes
Sulphide
ion

47. Worksheet – Model of an atom (CA 11)
Homework :
Worksheet – Model of an atom (CA 11)
Worksheet – Model of an Ion (CA 12)
Activity 5.7 :Ionic Charges and Chemical Families (Use BLM 5.7a-c) (CA 9,10)
Worksheet – Table of Ions (CA 13)
Lab Testing for Ions (CA14-15)
BLM 5.1b (CA 16)
BLM 5.5b (CA 16)
Answer Key

48. 5.6 How Elements Form Compounds
There are 2 types compounds :
1)      ionic compounds – formed when a metal loses 1 or more valence electrons to a non-metal, forming a positive (cation) and a negative ion (anion)which then are attracted to each other and are held together by an attraction called an ionic bond.

49. Ionic compounds dissolve in water and separate into positive ion and negative ions. These charged particles carry electric current through the water (electrolyte)
Video

50. 2)     Molecular compounds are formed when 2 or more nonmetals combine together. When dissolved in water the molecules do not separate into charged particles and do not carry an electrical charge (non electrolyte)
Video

51. Assignment Homework : Questions 1-8pg 187 Questions 1-4 pg 189
Ionic Compound Formation Example
Homework :
Questions 1-8pg 187
Questions 1-4 pg 189

52. 5.8 Ionic Compounds
Elements in the same chemical families form ions with similar ionic charges. Such ionic charges may also be called a valence charges or carrying capacity.
Na 1+ or S 2-
Metals and non metals combine to form ionic compounds by transferring electrons from the metal to the non metal. The metal atom loses electrons and becomes positively charged and the non metal gains the electrons and becomes negatively charged.  

53. The result is a compound that is neutrally charged or the sum of the charges on the positively charged ions equals the sum of the charges on the negatively charged ions
Na 1+ S2- becomes Na2S

54. e.g. aluminum chloride
Al loses 3 electrons = Al +3
Chorine gains 1 electron = Cl –1
To make the compound electrically neutral we would need 1 aluminum and 3 chloride ions
1 aluminum(+3) + 3 chlorines(-1) = 0

55. Writing Formulas for Ionic Compounds
Follow these steps:
e.g. What is the formula for aluminum chloride
1)      write the symbols, with the metal first
Al Cl

56. 2)     write the ionic charge above each symbol to indicate the stable ion that each element forms
Al Cl

57. 3)     criss cross the charge numbers and use them as subscripts after each element. This balances the charges and makes the compound electrically neutral
Al1Cl3
1 Al (+3) and 3 Cl (-1) = 0
1(+3) (-1) = 0

58. Naming Ionic Compounds
Just as in the chemical formula the name of the metal is first followed by the name of the non-metal. However the ending of the non-metal changes to “ide”
A compound made of aluminum and chlorine AlCl3 is called aluminum chloride
Some metals can have 2 or more carrying capacities. These compounds are named the same way as other ionic compounds except a roman numeral is used after the metal to identify which ionic charge is used the metal in the formula

59. e.g.Copper has 2 carrying capacities
Cu +1 and Cu +2
When copper combines with oxygen we must identify which positive ion is being used.
Copper (I) Oxide - Cu2O
Copper (II) Oxide – CuO * notice that we have reduced from Cu2O2 to CuO because this is still electrically neutral

60. Activity : ION Dominoes (CA17)
Make a table to record your score
Cation/Anion/Formula/Name
You must play an oppositely charged ion to any domino played
Record the Cation and Anion in your table
Play continues until one player is out of dominoes
Remaining players add up superscripts(Ca2+, N3- = -1)
Play the basic game first
Play the advanced game for marks

61. Assignment Homework : Q 1-10 pg 195 Worksheet A1 (CA18)
Answer Key..\..\School\20S Notes ppt\Chemistry Unit\2008\Chemistry Activities 2009 Answer Keys.doc
Assignment
Homework : Q 1-10 pg 195
Worksheet A1 (CA18)
BLM 5.8, A3, A4 (CA19, 20)

62. 5.9 Polyatomic Compounds
Some compounds like calcium carbonate and copper (II) sulphate do not end in “ide” like other ionic compounds. Why?
Such compounds are pure substances that involve a metal ion and a polyatomic or complex ion.
Polyatomic ions are groups of atoms that tend to stay together and carry an overall charge. E.g. sulphate ion is SO4 -2

64. Writing Formulas for Polyatomic Compounds
We use the same steps that we learned in section 5.8
What is the formula for copper (II) sulphate
1)      write the symbols for the metal and the polyatomic group
Cu SO4

65. 2)     write the ionic charges
Cu SO4

66. 3)     Criss Cross and reduce the subscripts to their simplest terms if possible. (Brackets) may be needed if there is 2 or more polyatomic ions. Never change the subscript of the polyatomic group.
Cu2 SO42 = Cu2 (SO4)2
= Cu SO4

67. Naming Polyatomic Compounds
The name of the above compound is Copper (II) Sulphate
The name is simply the name of the metal (use a roman numeral if the metal has more than 1 positive charge) and the name of the polyatomic ion . Both can be found on the periodic table by looking them up.

69. Homework
BLM 5.9, A5, A6 (CA21,22)

70. Molecular Compounds (COVALENT)
Most of the compounds you encounter each day do not contain ions. Most everyday compounds are molecular or made of only nonmetals.
E.g. sugar, plastic and water

71. Molecular compounds are formed when 2 non-metal atoms share their outer electrons to fill each others outer orbits. This sharing of electrons results in a covalent bond that holds the atoms together as a molecule.
Atoms become more stable when their outer orbit is full
Some elements exist as molecules rather than atoms for this reason (Diatomic Elements)
I2 , Br2 , Cl2 , F2 , O2 , N2 , H2

73. Writing Formulas for Molecular Compounds
The method is similar to writing ionic formulas. The number of electrons an atom wants to share to become stable is a clue to the number of covalent bonds that atom will form. The combining capacity of a non-metal is a measure of the number of covalent bonds.
These combining capacities are listed below :

74. 4 3 2 1 H C N O F Si P S Cl As Se Br I C O = C2O4 = CO2 H
C N O F
Si P S Cl
As Se Br I
What is the formula for the compound made of carbon and oxygen?
4 2
C O = C2O4 = CO2
simplify

75. Naming Molecular Compounds
Some molecular compounds have common names like :
H2O = water
NH3 = ammonia
CH4 = methane
H2O2 = Hydrogen Peroxide
O3 = Ozone

76. H2O = diHydrogen monOxide NH3 = Nitrogen triHydride
Or they can be named using prefixes which represent the number of each atom in the compound
H2O = diHydrogen monOxide
NH3 = Nitrogen triHydride
CH4 = Carbon tetraHydride

77. Tri =3 Hept(a) = 7 Tetr(a) = 4 Oct(a) = 8 Pent(a) = 5 Non(a) = 9
Notice the second part of the name still ends in “ide” like many of the ionic compounds. You must know the following prefixes:
Mon(o) = 1 (optional on first name not the second)
Di =2 Hex(a) = 6
Tri =3 Hept(a) = 7
Tetr(a) = 4 Oct(a) = 8
Pent(a) = 5 Non(a) = 9
Dec(a) = 10

78. P2 H4 is Diphosphorous Tetrahydride CO is carbon monoxide
e.g.
CO2 is carbon dioxide
P2 H4 is Diphosphorous Tetrahydride
CO is carbon monoxide
SiO2 is silicon dioxide
P3Br8 =
= Tetrasulfur nonoxide
N2O2 =
= HeptaSelenium DecaIodie

79. BLM 5.11(CA 23)
A7 (CA 23)

80. Oxyacids
Oxyacids are compounds formed when hydrogen (H +1) combines with polyatomic groups that contain oxygen
E.g. HNO3 is nitric acid
H +1 NO3 –1 = HNO3

81. Use the acid naming table on the back of your periodic table to name and write the formulas of all ionic compounds that begin with hydrogen
Hydrogen _______ide becomes hydro_________ic acid
Hydrogen _______ate becomes _____________ic acid
Hydrogen _______ite becomes ____________ous acid
chlor
chlor
chlor
chlor
chlor
chlor

82. Assignment
Acid Naming Worksheet (CA24)
Review Sheet A8 (CA25)

83. 5.12Hydrocarbons : A Special Group of Molecules
Organic compounds are molecular substances that contain carbon atoms as basic building blocks.
Carbon will bond covalently with oxygen,nitrogen and hydrogen to form very stable molecules. This is due to the combining capacity of carbon (4).

84. Carbon is found in many forms - plants (sugar) made from
photosynthesis
- animals (proteins)
- fossil fuels (oil)
- liquid natural gas (LNG)
All are classified as hydrocarbons (made of hydrogen and carbon)

85. -Crude oil (the source of hydrocarbons) comes from the decay of plants or the animals which fed on them. These plants and animals then died and over a period of millions of years heat and pressure turned them into crude oil

86. -When a hydrocarbon burns it must have Oxygen
-When a hydrocarbon burns it must have Oxygen. This is known as combustion or respiration. The main products of combustion are carbon dioxide and water vapor.
- Fossil fuels are a non-renewable energy source. Once used, they are gone.

87. methane + oxygen carbon dioxide + water
methane + oxygen    carbon dioxide + water. CH4(g)  + 2O2(g)         CO2(g)   +   2H2O(g)
  ethane + oxygen    carbon dioxide + water. 2C2H6(g)  + 7O2(g)         4CO2(g)   +   6H2O(g)
CO H2O + C CO
CO2 + H2O
Incomplete
Combustion
Complete
Combustion

88. Assignment Homework : Questions 1-5 pg 207
Activity : BLM 5.12 Hydrocarbons Word Search (CA 25)
Homework : Chapter 5 BLM Review (CA26)

89. Chapter 6 – Understanding Chemical reactions
How do chemical reactions happen?
How do chemists categorize the thousand’s of different chemical reactions?
In chapter 5 you saw patterns in how chemical compounds can be categorized as ionic or molecular. In this chapter you will learn to recognize patterns that will help you understand and predict different types of chemical reactions.

90. 6.1 Word Equations
Chemical reactions involve many chemicals, as in explosions of dynamite, bathroom cleaners working on a stain or as in the growth of your body. Chemists use a word equation to represent these types of reactions : it tells us what reacts and what is produced.

91. Word equation format:
Reactants and products can be separated by a (+) sign
e.g. The pop test for hydrogen gas
All the reactants All the products
Reactant Reactant Product 1 + Product 2
hydrogen + oxygen water

92. Assignment Try This Activity Pg 219 Understanding Concepts1-5 pg 219
Lab 6.2 Measuring masses in Chemical Changes
(CA27)
UC Questions 1-4 pg 221

93. 6.3 Conserving Mass
In Investigation 6.2 you saw that when two solutions react to form a solid precipitate, the mass stays the same. In all chemical reactions mass is conserved. This is because during the chemical reaction the individual atoms that make up the reactants are simply rearranged into new patterns or products, no matter is lost or added during the process. This is a scientific law that sums up the conclusions of many experiments called the Law of Conservation of Mass
The Law of Conservation of Mass states that in a chemical reaction, the total mass of the reactants is always equal to the total mass of the products
25 g g ?g
hydrogen + oxygen water

94. Assignment Understanding Concepts 1-7 pg 223
Lab 6.4 Finding the Missing Mass (CA28)
UC questions 1-4
BLM 6.5b (CA29)

95. 6.5 Balancing Chemical Equations
Because mass is always conserved in a chemical reaction we will have the same number of atoms of each element on both the reactant and product sides of a chemical equation. The equation must be balanced to make this happen.
A skeleton equation is representation of a chemical reaction in which the formulas of the reactants are connected to the formulas of the products by an arrow.
e.g. methane + oxygen carbon dioxide + water (word equation)
CH O CO H20 (skeleton equation)

96. CH4 + O2 CO2 + H20 (skeleton equation)
The problem with a skeleton equation is that it does not follow the Law of Conservation of Mass. By looking at the # of atoms on each side of the above equation we can see that they are not the same on both sides of the equation.
1 C O 1 C + 2 H
4 H 2O 1 O
16g 32g 44g 18g
48g g
(mass is not the same)

97. To make the above equation follow the Law of Conservation of Mass we must rewrite it as a balanced equation. To do this we will use multipliers at the front of each chemical formula . These multipliers are called coefficients.
By using the coefficients we have been able to show that there are the same number of atoms of the same element on each side of the equation. This would mean that the mass on each side of the equation is the same allowing us to support the Law of Conservation of Mass.
CH O CO H20
1 C O 1 C H
4 H 2O 2 O
16g 64g 44g 36g
80g = 80g
(mass is now the same)

98. How to balance an Equation
1)      write the word equation for the reaction
2)     Write the skeleton equation by replacing each name with the
correct formula
Lead (II) Nitrate + Potassium Iodide Lead(II) Iodide Potassium Nitrate
Pb(NO3) KI PbI KNO3

99. 3)     Count the # of atoms of each type in the reactants and products
Pb(NO3) KI PbI KNO3
Type of atom reactants products Pb N K I O
*** Use the ECHO rule : Count and balance the atoms in this order Element (all) then Carbon Hydrogen and finally Oxygen

100. 4)    multiply each of the formulas by the appropriate coefficients to balance the number of atoms
Type of atom reactants products Pb N K I O
Pb(NO3) KI PbI KNO3

101. Polyatomic short cut : if you can see a polyatomic ion group that is unchanged in the reaction you could balance it as a group rather than as individual atoms
Pb(NO3) KI PbI K(NO3)
Type of atom reactants products Pb K I NO

102. Pb(NO3) KI PbI K(NO3)
Type of atom reactants products Pb K I NO

103. Assignment Homework – Understanding Concepts 1-3 pg 229
A10,A11, Balancing Equations Worksheet (CA30,31)
BLM 6.5c (CA31)

104. 6.6 Combustion
There are different types of chemical reactions. One of the most common and useful chemical reactions is combustion (burning of a fossil fuel).
  Fuel + oxygen oxides energy
For a fuel to burn we need oxygen and since the Earth’s atmosphere is 21% oxygen, combustion can occur very easily. It is combustion that gives us heat energy for our homes, electricity, and allows is to run our cars.
The most important fuels that we burn are hydrocarbons or fuels made of hydrogen and carbon like gasoline (C8H18), natural gas (CH4), and even candles (C25H52).

105. The word equation for the combustion of a hydrocarbon is :
Hydrocarbon Oxygen Carbon dioxide water energy
Complete Combustion
Incomplete Combustion

106. The only variable or change in the above equation is the type of hydrocarbon burned
 In each case we need oxygen and produce carbon dioxide and water vapour as well as energy, which we use to run our car, keep us warm or give us light.
Gasoline Oxygen Carbon dioxide Water energy
C8H O CO H2O energy
Methane Oxygen Carbon dioxide Water energy
CH O CO H2O energy
Candle Wax Oxygen Carbon dioxide Water energy
C25H O2 CO H2O energy

107. The above combustions are called complete combustions because the fuel is completely burned up. You can tell if the combustion is complete if the flame you see is a bright blue color. Sometimes the fossil fuel or hydrocarbon does not burn completely and this is called incomplete combustion. You know it is incomplete combustion if the flame color is bright yellow-orange. Candles will often burn incompletely producing other products other than carbon dioxide and water
Candle Wax Oxygen Carbon dioxide Water energy + carbon + carbon monoxide
C25H O CO H2O energy + C CO
poisonous

108. Assignment Lab Demo – Who has the Hot Hand
Understanding Concepts 1,3,4,5,6 pg 232

109. HCl + NH3 NH4Cl 6.7 Types of Chemical Reactions :
Synthesis or Combination Reaction (putting things together)
Involves the combination of smaller atoms or molecules becoming larger molecules
A B AB
Element Element Compound
2H O2 2H2O
Compound Compound Compound
HCl NH NH4Cl

110. AB A + B 6.7 Decomposition Reaction (taking things apart)
Involves the breaking apart of a larger molecule into smaller molecules
AB A B
Compound Element Element
2H2O H2 O2
Compound Compound + Compound
NH4Cl NH HCl

111. Assignment
1) Lab Heating Bluestone (CA32)

112. element + compound element + compound
6.10 Single Displacement Reaction
Involves the displacement of one element in a compound by another similar element, metals will replace metals and nonmetals will replace nonmetals
element + compound element compound
A + BC B + AC
metal + compound metal compound
Fe AlCl Al FeCl3
D + BC C + BD
nonMetal + compound nonmetal compound
F AlCl3 Cl2 + 2FeF3

113. Assignment
1) Lab – Single Displacement Reactions (CA33)

114. AY + BZ BY + AZ Compound + Compound Compound + Compound
6.10 Double Displacement
Involves the displacement of an element in one compound for a similar element in another compound
Compound + Compound Compound + Compound
AY BZ BY AZ
Lead(II) Chloride + Potassium Iodide Potassium Chloride + Lead(II) Iodide
PbCl KI KCl PbI2
In the above example the metals switched places

115. Lab – Double Displacement Reaction (CA34,35)

116. Review Assignment
BLM 6.13 (CA36)
BLM Chp 6 Review (CA 36)