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Grade 10 Chemistry Unit

Group Reading Assignment pg 170-71Try This Activity Pg 171

Mr. Banerjee

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LAB SAFETY

»View Safety Video at:http://www.youtube.com/watch?

v=cr7roogzM8c&safety_mode=true&persist_safety_mode=1&safe=active

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

» WHMIS and Safety Worksheet (CA3 , 4)

Use the internet and your textbook pg176 -178» 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

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LAB SAFETY

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1

23

4

56

7

89

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1112 13

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Introductory Lab

• Chemistry in a Bag Lab (CA 5,6)

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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.

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

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

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5.1 Chemicals and chemical Change There are many different types of matter that make up our

world:

1) 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.

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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)

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).

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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:

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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.

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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

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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

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Matter

Pure Substance Mixture

Element Compound

Solution

Homogeneous

Heterogeneous

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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.

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

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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 + O2 makes Fe2O3

  Reactants Products

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Chemical TestsHow 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

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2)     Hydrogen Gas – a lit splint will cause a small explosion or pop sound

Hydrogen Test

POP!!

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

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

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Assignment• Lab : Properties Testing Properties of Substances

• (CA 7,8)

• Homework : Questions 1-10 pg 175 Answer Key

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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.

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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.

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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

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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

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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.

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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.

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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

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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)

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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

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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.

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

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Bohr diagrams are used to represent the arrangement of electrons in various orbits of an atom

Or

---7 e----8 e----2 e-

3517

Cl

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nucleus

1st nrg level

2nd nrg level

3rd nrg level

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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

Kr84

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

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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).

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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).

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Metal Atoms to Ions

MgAtom12p+

2e-

2e-

8e-

MgIon

12p+

2e-

8e-

Ne

2e-

8e-

Magnesium atom

becomes MagnesiumIon by losing2 electrons

To be like

Its nearest Noble Gas

MgSymbol of aMagnesium

Atom

Mg 2+

Symbol of aMagnesium

IonNotice 2+ means

magnesium lost 2 electrons

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Nonmetal Atoms to Ions

SAtom16p+

6e-

2e-

8e-

SIon

16p+

8e-

2e-

8e-

ArAtom18p+

8e-

2e-

8e-

Sulphuratom

becomes Sulphideion

To be like Its nearestNoble Gas

SSymbol of a

SulpurAtom

S 2-

Symbol of aSulphide

IonNotice 2- means

sulphur gained 2 electronsAnd the name changed

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• 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

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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.

 

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

Video

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• 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

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Assignment

• Homework :

• Questions 1-8pg 187

• Questions 1-4 pg 189

Ionic Compound Formation Example

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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.  

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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

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• 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

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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

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

+3 -1Al Cl

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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) = 01(+3) + 3 (-1) = 0

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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

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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

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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

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Assignment

• Homework : Q 1-10 pg 195

• Worksheet A1 (CA18)

• BLM 5.8, A3, A4 (CA19, 20)

Answer Key..\..\School\20S Notes ppt\Chemistry Unit\2008\Chemistry Activities 2009 Answer Keys.doc

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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

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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

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2)     write the ionic charges +2 -2

Cu SO4

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 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

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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.

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Homework

BLM 5.9, A5, A6 (CA21,22)

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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 

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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

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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 : 

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4 3 2 1H

C N O FSi P S Cl

As Se BrI

 What is the formula for the compound made of carbon and oxygen?

4 2C O = C2O4= CO2

simplify

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Naming Molecular Compounds Some molecular compounds have common names like : 

H2O = waterNH3 = ammoniaCH4 = methaneH2O2 = Hydrogen PeroxideO3 = Ozone

 

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Or they can be named using prefixes which represent the number of each atom in the compound 

H2O = diHydrogen monOxideNH3 = Nitrogen triHydrideCH4 = Carbon tetraHydride

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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) = 9Dec(a) = 10

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e.g. CO2 is carbon dioxideP2 H4 is Diphosphorous TetrahydrideCO is carbon monoxideSiO2 is silicon dioxide

P3Br8 =

= Tetrasulfur nonoxide

N2O2 =

= HeptaSelenium DecaIodie

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BLM 5.11(CA 23)A7 (CA 23)

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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 

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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 acidHydrogen _______ate becomes _____________ic acidHydrogen _______ite becomes ____________ous acid

chlor chlor

chlor chlor

chlor chlor

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Assignment• Acid Naming Worksheet (CA24)

• Review Sheet A8 (CA25)

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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).

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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)

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-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   

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-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.

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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)

CompleteCombustion

Incomplete Combustion

CO2 + H2O + C + COCO2 + H2O

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Assignment

• Homework : Questions 1-5 pg 207

• Activity : BLM 5.12 Hydrocarbons Word Search (CA 25)

• Homework : Chapter 5 BLM Review (CA26)

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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.

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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.

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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 1 + Reactant 2 Product 1 + Product 2

hydrogen + oxygen water

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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

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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 10 g ?g

hydrogen + oxygen water

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Assignment

• Understanding Concepts 1-7 pg 223

• Lab 6.4 Finding the Missing Mass (CA28)– UC questions 1-4

BLM 6.5b (CA29)

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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)

CH4 + O2 CO2 + H20 (skeleton equation)

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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.

CH4 + O2 CO2 + H20 (skeleton equation)

1 C + 2 O 1 C + 2 H

16g 32g 44g 18g

4 H 2O 1 O

48g 62g

(mass is not the same)

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1 C + 4 O 1 C + 4 H

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. CH4 + 2O2 CO2 + 2H20

16g 64g 44g 36g

4 H 2O 2 O

80g = 80g (mass is now the same)

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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)2 + KI PbI2 + KNO3

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 3)     Count the # of atoms of each type in the reactants and products

Pb(NO3)2 + KI PbI2 + KNO3

 Type of atom reactants products

Pb 1 1N 2 1K 1 1I 1 2O 6 3

*** Use the ECHO rule : Count and balance the atoms in this order Element (all) then Carbon Hydrogen and finally Oxygen

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Pb(NO3)2 + 2 KI PbI2 + 2 KNO3

 

4)    multiply each of the formulas by the appropriate coefficients to balance the number of atoms

 

 

Type of atom reactants products

Pb 1 1

N 2 2

K 1 1

I 2 2

O 6 6

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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)2 + KI PbI2 + K(NO3)

Type of atom reactants productsPb 1 1K 1 1I 1 2NO3 2 1

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Pb(NO3)2 + 2 KI PbI2 + 2 K(NO3) 

Type of atom reactants productsPb 1 1K 1 1I 2 2NO3 2 2

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Assignment

• Homework – Understanding Concepts 1-3 pg 229

• A10,A11, Balancing Equations Worksheet (CA30,31)

• BLM 6.5c (CA31)

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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).

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The word equation for the combustion of a hydrocarbon is : 

Hydrocarbon + Oxygen Carbon dioxide + water + energy

Complete Combustion Incomplete Combustion

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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

C8H18 + O2 CO2 + H2O + energy

Methane + Oxygen Carbon dioxide + Water + energy

CH4 + O2 CO2 + H2O + energy

Candle Wax + Oxygen Carbon dioxide + Water + energy

C25H52 + O2 CO2 + H2O + energy

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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 

C25H52 + O2 CO2 + H2O + energy + C + CO

Candle Wax + Oxygen Carbon dioxide + Water + energy + carbon + carbon monoxide

poisonous

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Assignment

• Lab Demo – Who has the Hot Hand

• Understanding Concepts 1,3,4,5,6 pg 232

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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

2H2 + O2 2H2O

Element + Element Compound

Compound + Compound Compound

HCl + NH3 NH4Cl

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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 2H2 O2

Compound Compound + Compound NH4Cl NH3 HCl

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Assignment

1) Lab Heating Bluestone (CA32)

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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

D + BC C + BD

nonMetal + compound nonmetal + compound

F2 + 2AlCl3 Cl2 + 2FeF3

A + BC B + AC

metal + compound metal + compound

Fe + AlCl3 Al + FeCl3

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Assignment1) Lab – Single Displacement Reactions (CA33)

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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

 In the above example the metals switched places

PbCl2 + 2 KI 2 KCl + PbI2

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Lab – Double Displacement Reaction (CA34,35)

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Review Assignment

• BLM 6.13 (CA36)

• BLM Chp 6 Review (CA 36)