Grade 10 Chemistry Unit

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Grade 10 Chemistry Unit
Group Reading Assignment pg 170-71 Try This
Activity Pg 171 Mr. Banerjee
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LAB SAFETY

• View Safety Video at
• http//www.youtube.com/watch?vcr7roogzM8csafety_
  modetruepersist_safety_mode1safeactive
• 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

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LAB SAFETY

• 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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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
• 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)
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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
Heterogeneous
Homogeneous
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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 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
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2)     Hydrogen Gas a lit splint will cause a
small explosion or pop sound
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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
---7 e- ---8 e- ---2 e- 35 17
Or
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
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Kr
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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. Ions 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
Mg Symbol of a Magnesium Atom
Mg 2 Symbol of a Magnesium Ion Notice 2 means
magnesium lost 2 electrons
Magnesium atom
Magnesium Ion by losing 2 electrons
becomes
To be like
Its nearest Noble Gas
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Nonmetal Atoms to Ions
S Symbol of a Sulpur Atom
S 2- Symbol of a Sulphide Ion Notice 2- means
sulphur gained 2 electrons And the name changed
Its nearest Noble Gas
Sulphur atom
To be like
becomes
Sulphide ion
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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
Ionic Compound Formation Example

• Homework
• Questions 1-8pg 187
• Questions 1-4 pg 189

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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 -1 Al 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) 0 1(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
Answer Key..\..\School\20S Notes ppt\Chemistry
Unit\2008\Chemistry Activities 2009 Answer
Keys.doc

• Homework Q 1-10 pg 195
• Worksheet A1 (CA18)
• BLM 5.8, A3, A4 (CA19, 20)

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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 1 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
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Naming Molecular Compounds   Some molecular
compounds have common names like   H2O
water NH3 ammonia CH4
methane H2O2 Hydrogen Peroxide O3
Ozone  
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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
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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) 9 Dec(a)
10
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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
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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
acid Hydrogen _______ate becomes _____________ic
acid Hydrogen _______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)
CO2 H2O C CO
CO2 H2O
Incomplete Combustion
Complete Combustion
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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 thousands 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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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 2 O 1 C 2 H
4 H 2O 1 O
16g 32g 44g 18g
48g 62g
(mass is not the same)
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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
1 C 4 O 1 C 4 H
4 H 2O 2 O
16g 64g 44g 36g
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 1 N 2
1 K 1 1 I
1 2 O
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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  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
Pb(NO3)2 2 KI PbI2
2 KNO3
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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 products Pb
1 1 K
1 1 I 1
2 NO3 2 1
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Pb(NO3)2 2 KI PbI2
2 K(NO3)   Type of atom reactants pro
ducts Pb 1 1 K
1 1 I
2 2 NO3 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 Earths
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
Incomplete Combustion
Complete 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  
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

109
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
2H2 O2 2H2O
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
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Assignment

• 1) 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
PbCl2 2 KI 2
KCl PbI2
  In the above example the metals switched places
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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)