1. CHEMISTRY
POWERPOINT SLIDESHOW
Covering concepts in the
Grade 9 Science Program of Studies
MATTERMATTER
&&
CHEMICAL CHANGECHEMICAL CHANGE
Supporting Science Textbook Content while enriching the Learning Process in Junior High/Middle SchoolSupporting Science Textbook Content while enriching the Learning Process in Junior High/Middle School

2. CHEMISTRY
Concept MapConcept Map
Shows the conceptsShows the concepts
coveredcovered
within the frameworkwithin the framework
of this unitof this unit
MatterMatter
&&
Chemical ChangeChemical Change
Grade 9Grade 9

3. CHEMISTRY - Lab SafetyLab Safety
Safety FirstSafety First
A good science lab is a safe one. All of the procedures,
equipment and chemicals you use have been designed to
help you understand the science principles you are
investigating. Go over the safety notes provided using the
Safety PowerPointSafety PowerPoint or online @ edquest.ca and be
prepared to take the safety test in class (do the practice test
– linked to in the PowerPoint - to help prepare you – the
test in class will be slightly different).
Notes:Notes: AccessAccess Safety NotesSafety Notes for viewing or printingfor viewing or printing @ http://edquest.ca@ http://edquest.ca
Practice Test:Practice Test: AccessAccess Safety Practice TestSafety Practice Test for viewing or printingfor viewing or printing @ http://edquest.ca@ http://edquest.ca

4. Poisonous Toxic Reactive Flammable
Corrosive Compressed Gas Biohazardous Oxidizing
CHEMISTRY - W.H.M.I.S. ReviewW.H.M.I.S. Review
WORKPLACE HAZARDOUS MATERIALS SYMBOLSWORKPLACE HAZARDOUS MATERIALS SYMBOLS

5. MATTER AND CHEMICAL CHANGE - Outline
Slides Key Concept Covered
3 - 43 - 4 Pre-Unit Teaching – Safety in the Science LabPre-Unit Teaching – Safety in the Science Lab
66 Laws, Theories, Models and ObservationsLaws, Theories, Models and Observations
7 - 97 - 9 TimelineTimeline – Early Ideas about Matter
10 - 1210 - 12 Properties of MatterProperties of Matter
1313 Organization of MatterOrganization of Matter
14 - 1714 - 17 ElementsElements: Patterns
18 - 2118 - 21 ElementsElements: Periodic Table
22 - 2722 - 27 CompoundsCompounds: Ionic and Molecular
2828 CompoundsCompounds: Comparison
29 - 3329 - 33 Chemical ReactionsChemical Reactions: Types
34 - 3534 - 35 Chemical ReactionsChemical Reactions: Reaction Rate
3636 Chemical ReactionsChemical Reactions: Identification Tests
37 - 3837 - 38 Law of Conservation of MassLaw of Conservation of Mass

6. CHEMISTRY - Developing Science Knowledge
Laws, Theories, Models, and ObservationsLaws, Theories, Models, and Observations
In science, lawslaws do not explain anything. They simply describe and summarize what
happens.
TheoriesTheories are imaginative ways to explain why something happens the way it does.
Theories are developed over the course of many observations and hundreds of
experiments before other scientists will accept it.
Scientific ideas may change over time as more evidence is gathered. Most of Dalton’s
atomic theory has stood the test of time, however, smaller particles (subatomic) have
been discovered and Dalton’s Theory needed to be revised.
Scientific modelsScientific models help others to visualize structures or processes that cannot be
seen directly.

7. CHEMISTRY - Early Ideas About Matter
8000 B.C.
Stone Age
Matter made up of solid material,
fashioned into tools.
‘tools
& implements’
6000-100 B.C.
Precious
Metals
Chemists investigated properties of
materials that were valuable to
humans.
‘gold
& copper’
4500 B.C
Bronze Age
The effect of heat on metals alloys
1200 B.C.
Iron Age
Iron combined with carbon to make
steel, for stronger tools.
Steel
350 B.C. Alchemy
Everything was made out of
Air – Water - Earth – Fire
‘atomos particles’
1500
Democritus
Theory of Matter was based more
on experimentation.
Alchemy

8. CHEMISTRY - Process Inquiry Models
16601660
BoyleBoyle
Particles can be compressed.
Scientific Inquiry
ParticleParticle
ModelModel
15971597
LibauLibau
Chemical preparations and a
textbook were written
TextbookTextbook
17701770
LavoisierLavoisier
System for the naming of chemicals
was developed.
MolecularMolecular
TheoryTheory
17801780
Air is necessary for
combustion to occur.
CombustionCombustion

9. CHEMISTRY - Atomic Theory
18081808
DaltonDalton
Observation principles during
experimentation.
Billiard BallBilliard Ball
ModelModel
18971897
JJ ThomsonJJ Thomson
Raisin bun model with charged
particles.
Raison BunRaison Bun
ModelModel
19041904
H. NagaokaH. Nagaoka
Negatively charged particles orbiting
around nucleus.
Solar System ModelSolar System Model
19131913
BohrBohr
Electrons travel in shells around a
central nucleus
AtomicAtomic
TheoryTheory
ChadwickChadwick Subatomic particles
Protons, neutrons,Protons, neutrons,
electronselectrons
19221922
RutherfordRutherford
Electrons rotate randomly around the
nucleus.
ShellShell
ModelModel
‘‘Quantum Theory’Quantum Theory’
Electrons moving randomly in a cloud around the central nucleus

10. The particle model of matter is an important part of this unit. Recall that:
All matter is made up of tiny particles.
All the particles in a substance are the same; different substances are made of different particles.
There are attractive forces among particles-these attractions may be strong or weak.
The particles are always moving; the more energy the particles gain, the faster they move.
There are spaces among the particles.
The Particle Model of Matter is a scientific model which helps to visualize a process we
cannot see directly. The first two points help us to understand that particles make up
matter. The other three points help to explain density and how matter behaves when
temperature changes. Matter exists in three states: solid, liquid, or gas.
The Particle Model of Matter is useful in explaining the differences among solids, liquids, and gases.
Solids have a definite shape and volume
because the particles of a solid can move
only a little. They vibrate back and forth, but
strong forces hold them in fixed positions.
Liquids take the shape of its container
because the particles can move around
more freely than they can in solids. A
liquid's particles are held together by strong
attractions to each other, so a liquid, like a
solid, occupies a definite volume.
Gases always fill whatever container they are
in. The attractions among the particles of a
gas are so weak that individual particles are
quite far apart, with spaces among them.
Since gas particles are moving constantly
and randomly in all directions, they spread
throughout their container, no matter what its
shape and volume.
CHEMISTRY - Properties of Matter

11. CHEMISTRY - Properties of Matter
Matter can change from one form to another, or create new materials. Properties are
characteristics that can be used to describe a substance. These properties can be
physical or chemical. Physical properties include: color, luster, melting point, boiling
point, hardness, malleability, ductility, crystal shape, solubility, density and conductivity.
A physical change occurs when a material
changes state. It is reversible. No new
substances are formed.
The change is not permanent.
Dissolving is also a physical change.

12. CHEMISTRY - Properties of Matter
Chemical properties describe how a substance interacts with other substances.
Chemical properties include: reaction with acids, ability to burn, reaction with water,
behaviour in air and reaction to heat. A chemical change occurs when substances
react and create a new substance.
Evidence that a chemical change occurs includes, but is not limited to the following:
Change in colour
Change in odour
Formation of a gas (bubbles) in a liquid
Formation of a solid (precipitate) in a liquid
Release or absorption of energy (heat)
Materials you started with are used up
A new material is formed
The change is difficult to reverse

13. CHEMISTRY - Description and Organization of
Matter
Matter exists in three states: solid, liquid, or gas.
Matter undergoes a change in state when energy is gained or lost.

14. CHEMISTRY - Elements: Patterns and Order
Finding a pattern and an order in an unknown helps scientists to organize ideas and
information. It also helps them to interpret what the information means and explain
these ideas, based on what they have learned – developing theoriesdeveloping theories.
The original ‘elements’ were earth, air, fireearth, air, fire andand waterwater.
Ancient Greek philosophersAncient Greek philosophers thought matter was made out of these four ‘elements’.
They thought all things were made from these four elements with varying degrees of
hotness, coldness, dryness and wetness.
AlchemistsAlchemists (part pharmacist and part mystic) developed many useful procedures,
including distillation, and they described the properties of many different materials.
They also thought they could change lead and copper into gold. They used special
symbols to prevent others from finding out their secrets.
The current view of matter began with Sir Francis BaconSir Francis Bacon, who stated that all
science should be based on experimental evidence, rather than thought. RobertRobert
BoyleBoyle recognized that elements could combine to form compounds. Bacon and Boyle
motivated others to search for elements.
Scientists began using heating, burning, mixing, and cooling to take matter down until
it could not be broken down any further, to determine if a substance was a pure
substance or a mixture.

15. CHEMISTRY - Elements: Patterns and Order
Antoine LavoisierAntoine Lavoisier defined elements as pure substances that could not be
decomposed into simpler substances by means of a chemical change. In this way he
identified 23 pure substances as elements. Lavoisier was one of the first chemists to
use a balanced view of chemical change.
Elements were then listed in order of their atomic mass. Atomic mass is the mass of
one atom of an element. It is represented in atomic mass unitsatomic mass units (amu).
Early chemists used symbols of the sun and the planets to identify the elements. This
became a problem, when more elements were discovered than planets.
John DaltonJohn Dalton developed a new set of
symbols in the early 1800’s to improve
communication between chemists.
BerzeliusBerzelius revised Dalton’s symbols by replacing them with letters, instead of pictures
and representing each element by their first letter (capitalized), or their first two letters
(first one capitalized and the second letter lower case).

16. CHEMISTRY - Elements: Patterns and Order
In 18091809 - 47 elements were known, and scientists began to see patterns.
In 18631863 - English chemist John NewlandsJohn Newlands divided the than discovered 56 elements
into 11 groups, based on characteristics. John Newland’s “law of octaves” identified the
pattern by which properties of the elements seemed to repeat at regular intervals, similar
to the octave scale in music.
Demitri MendeleevDemitri Mendeleev later revised
the pattern in 18691869 by collecting the
63 elements known at the time and
arranging them according to their
properties. By sorting and arranging
the elements in this way, he was able
to identify gaps - for undiscovered
elements. They were later discovered
and fit where he said they would.
Mendeleev attempted to classify the elements not by some "accidental, or instinctive
reasons, but by some exact principle." He believed that this exact system should be
numerical in nature to eliminate any margin of arbitrariness. By arranging the elements
in order of increasing atomic weight he discovered that there existed a pattern of the
element properties. He used this to create his table.

17. CHEMISTRY - Elements: Patterns and Order
The Periodic Table continued to develop as new information about the elements was learned.The Periodic Table continued to develop as new information about the elements was learned.
1886 - Ernest Rutherford named three types of radiation; alpha, beta and gamma
rays. Marie and Pierre Curie started working on the radiation of uranium and thorium,
and subsequently discovered radium and polonium.
1894 - Sir William Ramsay and Lord Rayleigh discovered the noble gases, which
were added to the periodic table as group 0.
1897 - English physicist J. J. Thomson discovered electrons; small negatively charged
particles in an atom.
1903 - Rutherford announced that radioactivity is caused by the breakdown of atoms.
1911 - Rutherford and German physicist Hans Geiger discovered that electrons orbit
the nucleus of an atom.
1913 - Bohr discovered that electrons move around a nucleus in discrete energy
called orbitals. Radiation is emitted during movement from one orbital to another.
1914 - Rutherford first identified protons in the atomic nucleus.
1932 - James Chadwick first discovered neutrons, and isotopes were identified. This
was the complete basis for the periodic table.
1945 - Glenn Seaborg identified lanthanides and actinides (atomic number >92),
which are usually placed below the periodic table.

18. CHEMISTRY - Elements: The Periodic Table

19. Each excerpt within the Periodic Table gives us useful information on each element
All the elements in a GroupGroup (or column) are called FamiliesFamilies.
AA periodperiod is a horizontal row in the periodic table of the elements.is a horizontal row in the periodic table of the elements.
(Group 1): The Alkali Earth Metals, all react with water in the following manner
2 Li + H2O ---> H2 + 2 LiOH
2 Na + H2O ---> H2 + 2 NaOH
2 Fr + H2O ---> H2 + 2 FrOH
(Group 8): The Noble Gases, don't react with other elements.
Atomic NumberAtomic Number Ion chargesIon charges
Element SymbolElement Symbol
Element NameElement Name
Atomic MassAtomic Mass
CHEMISTRY - Periodic Table Information

20. CHEMISTRY - Periodic Table Groupings
Group 1 - Alkali Metals – Sodium
- softer than most metals, good heat conductors and can explode if exposed to water.
Group 2 - Alkaline Earth Metals – Radium
- extremely reactive, and aren't found freely in nature.
Group 3-6-7 - Rare Earth Elements - There are 30 rare earth elements.
- many are synthetic or man-made.
Groups 3-12 - Transition Metals - Iron, cobalt and nickel
- the only elements known to produce a magnetic field.
Groups 13-15 - Other Metals - tin, aluminum and lead
-solid with a high density
Metalloids - have metal and non-metal properties. Some are semi-conductors,
meaning they can carry an electrical charge under special conditions. They are great
for computers and calculators.

21. CHEMISTRY - Periodic Table Groupings
Group 14-16 - Non-Metals –
- do not conduct heat or electricity very well and are brittle. At room temperature,
they turn into gasses and solids.
Group 17 - Halogens - "Halogen" means "salt former"
- compounds that contain a halogen are called "salts." At room temperature, they are
in three states of matter: solid, liquid and gas.
Group 18 - Noble Gases – Helium, Neon, Argon, Krypton, Xenon and Radon
- do not react with other elements, have the maximum number of electrons possible
in their outer shell (making them stable).

22. Each element in the periodic table has a chemical name. Combinations of elements
form compoundscompounds and have a chemical namechemical name and a chemical formulachemical formula. The formula
identifies which elements and how many of each are in the compound.
For example:
ethanolethanol ( C( C22 HH66 O )O )
2 carbon atoms
6 hydrogen atoms
1 oxygen atom
Guyton de MorveauGuyton de Morveau developed the chemical naming system in 1787.
IUPAC ( International Union of Pure and Applied ChemistryInternational Union of Pure and Applied Chemistry ) is now responsible for
determining the appropriate name for each compound.
IUPAC nomenclature is a systematic way of naming organic chemical compoundsorganic chemical compounds.
CHEMISTRY - Compounds

23. Molecular CompoundsMolecular Compounds
A molecule is the smallest independent unit of a pure substance. Diatomic molecules are
molecules made up of 2 atoms of the same element (oxygen Ooxygen O22, nitrogen N, nitrogen N22, hydrogen H, hydrogen H22).
Most molecular compounds do not form large structures. Of the 10 million compounds
discovered so far, about 9 million are molecular compounds. When non-metalsnon-metals combine,
they produce a pure substance called a molecule, or molecular compound. They can be
solids, liquids, or gases at room temperature. The bonding between atoms is strong, but
the attraction between the molecules is weak. Examples: sugar ( CC1212HH2222OO11 (s)11 (s) ), acetylene,
water.
Properties of molecular compounds include: low melting point, low boiling point, good
insulators, poor conductors, distinct crystal shape
A chemical formulachemical formula tells how many of each type of atom is present in the molecule.
A compound made from two elements is called a binary compoundbinary compound.
CHEMISTRY - Compounds

24. Rules for naming binary molecular compoundsbinary molecular compounds:
1. The first element in the compound uses the element name.
2. The second element has a suffix – ideide –
3. When there is more than 1 atom in the formula, a prefixprefix is used
which tells how many atoms there are.
4. Exception to #3 above – when the first element has only 1
atom the prefix mono is not used
Examples: COCO22 (g)(g) carbon didioxide CClCCl44 (l)(l) carbon tetratetrachloride SiOSiO2 (s)2 (s) Silicon didioxide
When you are changing from the written name to the chemical symbol:
Write the symbols for the elements in the same order as they appear in the name.
Use subscripts to indicate the numbers of each type of atom.
Some molecular compounds are better known by their common names rather than
their chemical names.
Examples: Water HH22 OO is actually dihydrogen oxidedihydrogen oxide, propane CC33 HH88 is tricarbon octahydridetricarbon octahydride.
The bracketed symbol following the chemical formula represents what state
(solid, liquid, gas) the compound is in. (aqaq) means aqueousaqueous (water) solution.
CHEMISTRY - Compounds
# of
Atoms Prefix
1 mono
2 di
3 tri
4 tetra
5 penta
6 hexa
7 hepta
8 octa
9 nona
10 deca

25. Ionic CompoundsIonic Compounds
Ionic compounds are pure substances formed as a result of the attraction between
particles of opposite charges, called ionsions. When an atom gains or loses electrons,
the atom is no longer neutral – it is an ion, either positively or negatively charged.
Properties of ionic compounds include: high melting point, good electrical conductivity,
distinct crystal shape, solid at room temperature.
Sodium Chloride ( table salt ) – NaClNaCl – is an ionic compoundionic compound. When it is dissolved in
water, the metal (NaNa) loses an electron – to become positively charged - and the
nonmetal (ClCl22) gains an electron – to be negatively charged - forming an aqueous
solution of ions. Conductivity is the ability of a substance to carry an electric
current. The ionic salt solution provides good conductivity. Positive sodium ions
attract negative chloride ions to form a cube-shaped arrangement (ionic model).
The force holding them together is called ionic bondsionic bonds.
CHEMISTRY - Compounds

26. 1. The chemical name of the metal or positive ion goes first, followed by the name of
the non-metal or negative ion.
2. The name of the non-metal negative ionnon-metal negative ion changes its ending to ide.
SodiumSodium Chlorideide
Some ions are called polyatomic ions (meaning “many”).
Polyatomic ions are a group of atoms acting as one.Polyatomic ions are a group of atoms acting as one.
Example: calcium carbonate (limestone)
““ate”ate” and “ite”“ite” endings indicate polyatomic ions with oxygen.
The “hypo….ite” has one less oxygen than the “ite” for the same elements
The “per…ate” has one more oxygen than the “ate” for the same elements.
Generally, elements in a group all have the same ion charge
CHEMISTRY - Rules for Naming Ionic Compounds
Hydroxide OHHydroxide OH-1-1
Carbonate COCarbonate CO22
-2-2
Phosphate POPhosphate PO44
-3-3
Nitrite NONitrite NO22
-1-1
Ammonium NHAmmonium NH44
+1+1
Sulfite SOSulfite SO33
-2-2
Nitrate NONitrate NO33
-1-1
Sulfate SOSulfate SO44
-2-2

27. CHEMISTRY - Rules for Naming Ionic Compounds
When writing an ionic formula for a metal and a nonmetal compound follow these steps:
Write the symbols for the metal and the nonmetal.
Write the valences as superscripts above each symbol.
Drop the + and - sign.
Crisscross the valences so they become the subscript for the other element.
Reduce subscripts whenever possible. Only when both are divisible by a number greater than one.
Chemical Formula for the compound between aluminum and oxygen.
Here are two examples where you must reduce:

28. CHEMISTRY - Comparing Compounds
Ionic Compounds
pure substances formed as a result of the
attraction between particles of opposite
charges, called ions.
Molecular Compounds
combined non-metals producing a
pure substance called a molecule
contains a metal doesn’t contain a metal
high melting/boiling points low melting/boiling points
distinct crystal shapesdistinct crystal shapes
solids solids, liquids, or gases
good electrical conductivity good electrical insulators
table salt ( NaCl ) sugar ( C12
H22
O11(s)
)
metal name is always first acetylene, water

29. A chemical change, which releases energy, is called EXOTHERMICEXOTHERMIC.
AmmoniaAmmonia (NH3) is formed from nitrogen and hydrogen in their gaseous forms (N2 and H2 respectively).(NH3) is formed from nitrogen and hydrogen in their gaseous forms (N2 and H2 respectively).
This is given by the equation:This is given by the equation:
3H2(g) + N2(g) → 2NH3(g)3H2(g) + N2(g) → 2NH3(g)
This reaction is exothermicThis reaction is exothermic
A chemical change, which absorbs energy, is called ENDOTHERMICENDOTHERMIC
In this reaction,In this reaction, AmmoniaAmmonia will spontaneously, split up again into its components nitrogen and hydrogen,will spontaneously, split up again into its components nitrogen and hydrogen,
given by the equation:given by the equation:
2NH3(g) → 3H2(g) + N2(g)2NH3(g) → 3H2(g) + N2(g)
This reaction is endothermicThis reaction is endothermic
CHEMISTRY - Chemical Reactions
A chemical change results from a chemical reaction. Chemical bonds are forces
that cause a group of atoms to behave as a unit. Energy is stored in these bonds.
To break the bonds energy must be added. When bonds form, energy is released.
All chemical reactions involve energy being absorbed, or released.
Photosynthesis is an endothermic reaction, because it needs light energy to occur,
whereas combustion is an exothermic reaction, because it gives off light and heat

30. Chemical reactions occur when two or more substances combine to form
new substances.
Substances at the beginning of the reaction are called reactantsreactants.
New materials produced by the reaction are called productsproducts.
Chemical reactions can be written as word equationsword equations which gives the names of all the
reactants (separated by a "plus' sign + ) followed by an arrow which points to the
names of all the products (separated by a 'plus' sign +)
eg. ( iron + oxygen + water ---» rust )
(Iron plus oxygen plus water produces rust)
CHEMISTRY - Chemical Reactions
REACTANTSREACTANTS PRODUCTSPRODUCTS

31. CHEMISTRY - Chemical Reactions
There are four types of chemical reactions:
CombinationCombination (reactants combine) - CombustionCombustion is a chemical reaction that occurs
when oxygen reacts with a substance to form a new substance and gives off energy.
CombustionCombustion is the highly exothermic combination of a substance with oxygen.
Combustion requires heat, oxygen, and fuel.
The burning of propanepropane ( CC33HH88 ) in a barbeque
is an exothermic reaction that produces heat to
cook the food. If the heat is too intense, the
products being cooked will be changed into pure
carbon (the meat will be burnt).
The products of combustion are not always beneficial. Burning fossil fuels (such as
propane) produces carbon monoxide, carbon dioxide, sulfur oxides, nitrogen oxides,
smoke, soot, ash and heat.

32. CHEMISTRY - Chemical Reactions
DecompositionDecomposition (reactants break down) - CorrosionCorrosion is a slow chemical change that
occurs when oxygen in the air reacts with a metal. Corrosion is a chemical reaction in
which the metal is decomposed (eaten away), when it reacts with other substances in
the environment.
Preventing CorrosionPreventing Corrosion
Corrosion protection (e.g. painting the metalpainting the metal)
involves protecting metal from contact with
the environment and the factors that affect
the reaction rate of this chemical reaction.
Coating a corrosive metal with a thin layer of
zinc is called galvanizationgalvanization. The process of
coating a corrosive metal with another metal
through electrolysis is called electroplating.

33. CHEMISTRY - Chemical Reactions
DisplacementDisplacement (reactants change place with each other) - Two reactants yield two
products. Silver nitrate combines with sodium chloride to produce silver chloride and
sodium nitrate - because the sodium and silver switched places.
ExchangeExchange (reactants change place) - Cellular RespirationCellular Respiration is a chemical reaction
that takes place in the cells in your body and in plant cells.
The chemical reaction for cellular respiration is ...
C6
H12
O6
+ 6O2
6CO2
+ 6H2
O (+ energy for the cell to use for other things)
A car uses fuelA car uses fuel An organism usesAn organism uses
and oxygenand oxygen Sugar to produceSugar to produce
to produceto produce COCO22
COCO22

34. The speed of a chemical reaction is called the reaction rate.
Factors affecting the reaction rate include:
 TemperatureTemperature -The higher the temperature the faster the reaction rate
 Surface AreaSurface Area -The more surface in contact, the faster the reaction rate
 ConcentrationConcentration - The higher the concentration, the faster the reaction
 CatalystsCatalysts - The presence of a catalyst (substances that help a reaction
proceed faster) also affects the reaction rate. Catalysts are not consumed in the
reaction. Types of reactions involving catalysts can be found in living and non-living
things. EnzymesEnzymes are catalysts, present in the body, that speed up reactions which
break down food. They also help to rid the body of poison. Enzymes are organic
proteins known as amino acids and are found in all living things. They are Without
enzymes, there would be no life. When there is a partial reduction of availability of
enzymes, then life is reduced. They are "activists." All activity of life depends on
them. The greening of leaves in spring, the ripening of foods, the digestion and
absorption of food, all require enzymes. Without enzymes, seeds could not sprout and
the soil could not produce, therefore fruits and crops would not ripen or grow.
CHEMISTRY - Reaction Rate

35. CHEMISTRY - Chemical Reactions
Speeding Up a Reaction With CatalystsSpeeding Up a Reaction With Catalysts
A catalyst is a substance that help a reaction proceed faster and are not consumed in
the reaction. Types of reactions involving catalysts can be found in living and non-living
things. Enzymes are natural catalysts that help in the reactions in the body, which
break down food. They also get rid of poison in the body.
CatalaseCatalase (an enzyme found in plant and animal cells)
speeds up the breaking down of hydrogen peroxide into
harmless oxygen and water.
Slowing Down a Reaction With InhibitorsSlowing Down a Reaction With Inhibitors
Inhibitors are substances that slow down chemical reactions. Plants have natural
inhibitors in their seeds to prevent germination until the right conditions are present.
Inhibitors are added to foods to slow down their decomposition.

36. CHEMISTRY - Chemical Reaction - Identification
Tests
OXYGENOXYGEN
Light a wooden splint. Blow out the flame, allowing the splint to continue glowing. Hold
the glowing splint in a small amount of the unknown gas. If the splint bursts into flamebursts into flame,
then the gas being tested is oxygen.
HYDROGENHYDROGEN
Light a wooden splint. Hold the glowing splint in a small amount of the unknown gas. If
you hear a "poppop", then the gas being tested is Hydrogen.
CARBON DIOXIDECARBON DIOXIDE
The test for the presence of Carbon Dioxide uses limewater (a clear colorless solution of
calcium hydroxide, or slaked lime). Bubble the unknown gas (carbon dioxide) through the
limewater solution, or add a few drops of the limewater solution to the gas and swirl it
around. If the limewater turns milky, the gas is Carbon Dioxide. A solid precipitate of
calcium carbonate is formed. Calcium carbonate is chalk or limestone, and it is this, that
makes the lime water cloudy.
calcium hydroxide + carbon dioxide calcium carbonate + water.calcium hydroxide + carbon dioxide calcium carbonate + water.
Ca(OH)2(aq) + CO2(g) CaCO3(s) + H2O(l)

37. In a chemical reaction, the total mass of the reactants,In a chemical reaction, the total mass of the reactants,
is always equal to the total mass of the products.is always equal to the total mass of the products.
This law goes well with the atomic theory
Atoms (matter) are never created or destroyedAtoms (matter) are never created or destroyed
In a chemical reaction the atoms and molecules are simply rearranged.
This law of conservation of mass does not apply to nuclear reactions, because there is
some loss of mass: mass is changed into energymass is changed into energy..
This was first suggested by Albert Einstein in his famous equation:
E =MC2
(E Is Energy, M is Mass, C2
is a large number)
A very tiny amount of mass is equal to a very large amount of energyA very tiny amount of mass is equal to a very large amount of energy
In an open system some of the mass seems to disappear,
when it is in the form of a gas.
CHEMISTRY - Law of Conservation of Mass

38. Other scientists followed up on the law of conservation of mass by stating the …Other scientists followed up on the law of conservation of mass by stating the …
Law of Definite CompositionLaw of Definite Composition
Compounds are pure substances that contain two or more elementsCompounds are pure substances that contain two or more elements
combined together in fixed (or definite) proportions.combined together in fixed (or definite) proportions.
Water is an example of this law.
Pure water always contains 11% Hydrogen and 89% Oxygen.
Law of Multiple Proportions ...... states that the masses of one element, whichstates that the masses of one element, which
combine with a fixed mass of the second element, are in a ratio of whole numbers.combine with a fixed mass of the second element, are in a ratio of whole numbers.
Pure substances have constant composition and properties. An unknown substance
can be identified by measuring a property of the substance (eg. density) and
compare it to known values of other substances. If the test property matches a
known value, it is likely that substance, because each substance has its own
distinguishing properties unique to that substance.
CHEMISTRY - Law of Conservation of Mass