Chemistry
Science 10 – CHHS
Name: ___________________________________
TA: ________
Contents
Matter & Compounds ............................................................................................................................................................. 1
Chemistry in History ............................................................................................................................................................ 1
The Scientific Method ......................................................................................................................................................... 2
The Atomic Model........................................................................................................................................................... 2
Safety .................................................................................................................................................................................. 3
Universal Language ............................................................................................................................................................. 4
Compound Formation ......................................................................................................................................................... 4
Ionic Compounds ............................................................................................................................................................ 4
Polyatomic Ionic Compounds ......................................................................................................................................... 5
Molecular Compounds .................................................................................................................................................... 5
Naming & Formulas ............................................................................................................................................................ 5
Ionic Compounds ............................................................................................................................................................ 6
Molecular Compounds .................................................................................................................................................... 7
Compounds ......................................................................................................................................................................... 8
Solubility.............................................................................................................................................................................. 9
Molecular Structure ............................................................................................................................................................ 9
Toxic & Hazardous Compounds ........................................................................................................................................ 10
Chemical Reactions ............................................................................................................................................................... 11
Reactions in Daily Life ....................................................................................................................................................... 11
Essential Reactions............................................................................................................................................................ 11
Photosynthesis .............................................................................................................................................................. 11
Respiration .................................................................................................................................................................... 12
Combustion ................................................................................................................................................................... 12
Evidence of Chemical Change ........................................................................................................................................... 12
Energy Change .............................................................................................................................................................. 12
Formation of a Gas or Precipitate ................................................................................................................................. 13
Color or Odor Change ................................................................................................................................................... 13
Types of Reactions ............................................................................................................................................................ 13
Formation (Synthesis) ................................................................................................................................................... 13
Decomposition .............................................................................................................................................................. 13
Hydrocarbon combustion ............................................................................................................................................. 14
Single replacement ....................................................................................................................................................... 14
Double replacement ..................................................................................................................................................... 14
Word & Chemical Equations ............................................................................................................................................. 14
Predicting the Products..................................................................................................................................................... 14
Moles................................................................................................................................................................................. 15
Law of Conservation of Mass ............................................................................................................................................ 16
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Matter & Compounds
General Outcome A1: Students will describe the basic particles that make up the underlying structure of matter, and
investigate related technologies
Chemistry in History

I can identify historical examples of how humans worked with chemical substances to meet their basic needs
The idea that matter is made of tiny particles has been around for thousands of years. It began in ancient Greece as a
philosophical discussion. In the past several centuries, however, it has become an important topic of scientific inquiry.
Early chemists and physicists experimented, observed, hypothesized, predicted, and experimented again as they
developed theories about the tiny particles that make up matter.
For thousands of years, First Nations peoples have used the chemical properties of substances and their interactions to
make clothing, preserve food, treat illness, build tools, and adorn objects with colour.
To tan leather, First Nations peoples from various parts of North America used different techniques. Some used a
mixture of ashes and water to pre-soak the hides. Substances in the ashes helped to break down the tough layer of
mucous that coats the hide. Animal brains were applied to the hide, creating soft, water-resistant buckskin. Substances
in the brains, including emulsified fats, penetrated the hide to change its properties. This process is called brain-tanning.
Dyes for decorating fabric, wood, and other materials were obtained from local plants. Delphinium plants, for example,
produce a blue-green dye. The roots of bloodroot plants produce an orange dye. To treat illnesses and alleviate pain,
substances were extracted from local plants. For example, wild ginger was used by many Aboriginal peoples to treat a
number of ailments including coughs, colds, and flu. A tea made from the juice of juniper berries, shown here, could be
applied to the skin to soothe insect bites.
Many First Nations peoples who travelled by water, melted pine or spruce gum and mixed it with animal fat. They used
the resulting sticky resin to build waterproof canoes.
Many of these techniques and remedies work just as well as modern ones. Some First Nations people and others
interested in traditional methods still use them today. For example, many people prefer hides that have been tanned
using traditional methods. These hides are said to be softer and stronger than hides tanned using mass-production
methods. As well, traditional means of healing and herbal medicine have become more popular.
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The Scientific Method

I can outline the role of evidence in the development of the atomic model (protons, neutrons and electrons)
Scientists use the scientific method to determine answers to questions and
solutions to problems. This procedure consists of making observations, formulating
hypotheses, and designing experiments, which in turn lead to additional
observations, hypotheses, and experiments in repeated cycles.
Observations can be qualitative or quantitative. After an observation or a set of
observations, scientists begin an investigation by forming a hypothesis, a tentative
explanation for the observation(s).
Scientists conduct experiments to test the validity of their hypothesis. Experiments
are systematic observations or measurements, made under controlled conditions—
that is, under conditions in which a single variable changes.
A properly designed and executed experiment helps scientists to determine if the
original hypothesis was valid or if further experimentation are required.
When enough experimental data is collected and analyzed, the results may
become a law. A law says what happens; it does not address the question of why.
A law states only what happens – a theory tries to explain why. Laws are unlikely to
change too much over time. In contrast, a theory, by definition, is incomplete and
imperfect, evolving with time to explain new facts as they are discovered.
THE ATOMIC MODEL
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General Outcome A2. Students will explain, using the periodic table, how elements combine to form compounds, and
follow IUPAC guidelines for naming ionic compounds and simple molecular compounds
Safety


I can illustrate an awareness of WHMIS guidelines
I can demonstrate safe practices in the handling, storage and disposal of chemicals in the laboratory and at home
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Universal Language

I can explain the importance of, and need for, the IUPAC system of naming compounds, for scientists to
communicate clearly and precisely
Before the 18th century, without a standardized naming system for chemicals, there was confusion because the names
for chemical compounds varied from country to country and scientist to scientist. To stop the confusion, a standardized
naming system was developed.
In 1919, the International Union of Pure and Applied Chemistry (IUPAC) developed a systematic method to name
chemicals according to their composition. Today, chemists all over the world use the IUPAC system. This system makes
sure that each pure substance has a single, unique name, called its systematic name. The name of a substance describes
its composition. It also enables you to write its chemical formula and predict some of its properties. For example, the
systematic name for saltpetre is potassium nitrate (KNO3). This name identifies the substance as an ionic compound
that contains potassium and nitrate ions. From this information, a modern chemist can predict that, this potassium salt
will display properties similar to other salts.
Compound Formation

I can explain, using the periodic table, how and why elements combine to form compounds in specific ratios
As long as you understood some basic facts about the organization of the periodic table, you can predict that hydrogen
and oxygen should combine to form a new compound with the formula H2O. The periodic table can also help you
predict some properties of this new compound.
The periodic table represents patterns related to the arrangement of electrons in atoms. These patterns help explain
how substances behave during a chemical change. Neils Bohr inferred that electrons orbit the nucleus of the atom in
fixed energy levels. Each energy level can hold a certain number of electrons but no more. The second energy level can
contain a maximum of eight electrons.
Stable Octet
The arrangement of eight electrons in the outermost occupied energy level.
Valence Energy Level
The outermost occupied energy level of an atom.
Valence Electrons
The electrons in the valence energy level.
IONIC COMPOUNDS
Experimental evidence shows that many
compounds appear to be made of ions. As
the two elements react, metal atoms transfer
one or more valence electrons to atoms of
the non-metal. The resulting oppositely
charged ions attract one another, forming an
ionic bond. These ionic bonds hold the ions
in ionic compounds together. Ionic bonds are
very strong, because they result from the
strong forces of attraction between
oppositely charged ions.
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POLYATOMIC IONIC COMPOUNDS
Polyatomic Ion are a cluster of atoms that behave as a single unit in a chemical compound and are found in the table at
the top of your periodic table. Since polyatomic ions are charged particles, they have the ability to form compounds
with simple ions or with polyatomic ions:
MOLECULAR COMPOUNDS
Groups of atoms that behave as though they are made of separate groups of atoms
that share electrons are called molecules. Compounds made of molecules are called
molecular compounds. Molecular compounds contain only non-metal elements.
Molecular Elements
Nitrogen
N2
Oxygen
O2
Fluorine
F2
Atoms of the same element can form bonds, and exist as molecular elements. For
Chlorine
Cl2
example, oxygen, O2, exists as diatomic (two-atom) molecules. The table includes a
Bromine
Br2
list of the elements that form molecular elements.
Iodine
I2
Astatine
At2
Hydrogen
H2
Phosphorus
P4
Sulfur
S8
Atoms in molecules are joined by
covalent bonds. SInce they are nonmetals, no electron transfer is likely to
take place. Instead, atoms share
valence electrons. An atom can form
enough covalent bonds to complete its
valence energy level. A single covalent
bond is formed when two atoms share
a single pair of electrons.
You can predict the number of
covalent bonds an atom will form by
looking at the electrons in its valence
energy level. Each single (unpaired)
electron in the valence energy level
can form a covalent bond.
Naming & Formulas

I can predict formulas and write IUPAC names of compounds
Subscripts are used to indicate the number of atoms as well as whether an element or compound is currently in a solid,
liquid, or gas state. For example, H2O(s) indicates water in its solid state (ice), H20(l) is water in its liquid state, and H20(g)
is water in its gaseous form. The subscript (aq) stands for “aqueous” and means the compound is dissolved in water.
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IONIC COMPOUNDS
Since ionic compounds are joined by exchanging electrons, ionic charges must be balanced in order to write the
chemical formula since the compounds are all stable (electrically neutral).
Steps to writing the CHEMICAL FORMULA of ionic compounds
1.
2.
3.
Ex: Calcium (Ca) and Chlorine (Cl)
Print both ions’ symbols and changes. (If a polyatomic ion is being used,
its charge can be found on the list of Common Polyatomic Ions on the
periodic table.
Balance the ion charges. To balance the positive ion charges and negative
ion charges, add more ions of whichever has fewer charges. (If more of
the polyatomic ion are needed to balance charges, use the WHOLE
polyatomic ion.)
Write the formula by indicating how many ions of each ion are in it, using
subscript after the element's symbol. If there is only one atom, no
number is used. Do not include the ion charge in the formula as all
compounds are stable (electrically neutral).
Subscript:
Ca2+
Ca2+
ClCl- Cl-
CaCl2(s)
Letters, figures, or symbols written or printed below the line of the rest of the text
Steps to writing the NAME of SIMPLE ionic compounds:
Example: CaCl2(s)
1.
Write the name of the metal element.
calcium
2.
Change the last part of the non-metal element to “ide”.
chloride
3.
Combine the metal and non-metal names (in that order).
calcium chloride
Steps to writing the NAME of POLYATOMIC ionic compounds:
Example: Ca(OH)2(s)
1.
Write the name of the cation (positive ion).
calcium
2.
Write the name of the anion (negative ion).
hydroxide
3.
Combine the metal and non-metal names (in that order).
Multivalent:
calcium hydroxide
If there is more than one common ion charge for the metal, you must indicate which ion is being used. In
these cases, roman numerals are used after the name of the metal atom. For example, iron (Fe) can
form ions with either a 2+ charge or a 3+ charge. If an iron ion with a 2+ charge (Fe2+) combines, the name
iron (II) is used; if an iron ion with a 3+ charge (Fe3+) combines, the name iron (III) is used.
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ACIDS
One common feature of acids is that they all contain hydrogen. Therefore, scientist defined an acid as a substance that
reacts and releases hydrogen ions, H-(aq), in a water solution.
When naming acids, we are able to follow these general rules:
Combining Substances
Hydrogen + ______________ide
ex: hydrogen + chlorine (HCl(aq))
Hydrogen + ______________ate
ex: hydrogen + nitrate (HNO3(aq))
Hydrogen + ______________ite
ex: hydrogen + sulfite (H3SO3(aq))
IUPAC Name
Classical Name
aqueous hydrogen chloride
aqueous hydrogen nitrate
aqueous hydrogen sulfite
Hydro_______________ic acid
ex: hydrochloric acid
_______________ic acid
ex: nitric acid
_______________ous acid
ex: sulfurous acid
A list of common acids is listed below:
Name
Formula
Sulfuric ACID
H2SO4
Hydrochloric ACID
HCl
Nitric ACID
HNO3
Carbonic ACID
H2CO3
Ethanoic ACID
CH3COOH
MOLECULAR COMPOUNDS
Steps to writing the NAME of molecular compounds:
Ex: two nitrogen and three oxygen
1. The element found the further left on the periodic table is written
first, and uses the element name—just like ionic compounds
2.
The second element (further right on the periodic table) in the
compound has the suffix 'ide'—just like ionic compounds.
3.
When there is more than one atom in the formula, a prefix is used
which specifies the number of atoms. Some prefixes are listed below.
nitrogen
oxide
Dinitrogen trioxide
An exception to rule 3 is when the first element has only one atom, the prefix mono is not used.
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# of Atoms
Prefix
Examples of molecular compounds.
1
mono
2
di
N20 dinitrogen monoxide
3
tri
N 2 0 3  dinitrogen tri oxide
4
tetra
NF 3  nitrogen trifluo ride
5
penta
CC14  carbon tetrachloride
CO 2  carbon dioxide
P3F5  triphosphorus pentafluoride
Diatomic molecules are not named using the above rules. O2 (oxygen gas), H2 (hydrogen gas), and N2 (nitrogen gas), are
the most common examples.
Compounds

I can classify ionic and molecular compounds, acids and bases on the basis of their properties
Ionic Compounds
Molecular Compounds
Acids
Bases
Conductivity
conductive (when
dissolved in water)
most: non-conductive
some: conductive
conductive (when
dissolved in water)
conductive (when
dissolved in water)
pH
n/a
n/a
0-7
7-14
Solubility
most are water soluble
many are not water
soluble
soluble
mostly insoluble
State
(at 25°C)
solid
solid, liquid, or gas
Solid
solid
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Solubility

I can predict whether an ionic compound is relatively soluble in water, using a solubility chart
How do you know whether ions will combine to form a precipitate in an aqueous solution? Scientists have tested a wide
range of ionic compounds to see how well they dissolve in water. A solubility table gives combinations of common
positive and negative ions and shows whether ionic compounds containing two types of ions are soluble in water.
If they are very soluble, they do not for a precipitate; if they are only slightly soluble, they form a precipitate.
Molecular Structure

I can relate the molecular structure of simple substances to their properties
Water has many unique properties. It exists on Earth, in large quantities, in all three states. In its solid state (ice), it is
less dense than in its liquid state – the opposite of most substances. When water freezes on the surface of a lake, the ice
floats. It insulates the water below so that the water remains liquid. If ice were denser than water, the ice would sink as
it froze. The lake would freeze solid and kill all the life within it.
Chemists explain the properties of water based on the structure of the water molecule. Two features of a water
molecule contribute to its properties: its shape and its bonding. The bent shape of a water molecule is due to the
arrangement of electrons within the molecule.
A water molecule has two O—H bonds. Each bond consists of two shared electrons. However, the oxygen atom attracts
the electrons a more strongly than the hydrogen atom. The overall effect of this difference in attraction is that the
oxygen atom has a permanent, partial negative charge, while the hydrogen atom has a permanent, partial positive
charge. Because of this, it is said to be polar. A polar bond has a negative end, or pole, and a positive pole. The bent
shape of the water molecule means that it can have a positive pole and a negative pole.
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Because water molecules are polar, they attract one another. The attraction of an oxygen atom in one water molecule
to a hydrogen atom in another water molecule is called a hydrogen bond. Water has other weird properties, such as:
•
•
•
•
•
High Boiling Point & Melting Point
It requires a great deal of energy to break the hydrogen bonds between water molecules and thus to melt ice
and to boil or evaporate liquid water. This property of water explains why perspiration, works to cool the body.
High Specific Heat Capacity
It requires a great deal of energy to increase the temperature of water. When the temperature of a substance
increases, it means that the average speed of the particles in the substance increases. For water molecules to
move more quickly, they must overcome the strong attractive forces among them. As water cools, a great deal
of energy is released.
Concave Meniscus & Capillary Action
These properties occur due to the large forces of attraction between polar water molecules and the sides of
containers. Capillary action is the force that draws water up from the roots to the leaves of tall trees.
Ice Floats
Water expands as it freezes because the polar molecules arrange themselves in an open pattern. As it forms, the
less-dense ice floats on the denser water. Substances without hydrogen bonding pack together more tightly as
they freeze, so the denser solid material sinks to the bottom of the liquid.
High Surface Tension
The hydrogen bonds between molecules on the surface of water pull them together into the smallest possible
area. A small volume of water falling through the air forms a circular drop. Water insects take advantage of
water’s surface tension to move across its surface.
Toxic & Hazardous Compounds

I can outline the issues related to personal and societal use of potentially toxic or hazardous compounds
Industrial workers who handle ethanol (C2H5OH), are warned that the chemical can be harmful. The MSDS for pure
ethanol states that it can cause mutations, damage unborn children, irritate the skin and lungs, cause unconsciousness,
and damage the liver and nervous system. Despite these hazards, people expose themselves to ethanol solutions daily.
They do so every time they drink an alcoholic beverage.
Caffeine is a powerful stimulant found in coffee, tea, cocoa, and chocolate. It is a diuretic and increases blood pressure
by constricting blood vessels. Caffeine is not classified as a hazardous substance and is not regulated. On the other hand,
governments and other bodies strictly regulate the use of some substances. Many performance-enhancing drugs are
banned from athletic competitions. The use and sale of street drugs, such as cocaine, heroin, and ecstasy (MDMA), are
illegal. People under 18 cannot legally purchase alcoholic beverages and nicotine products.
The effects of alcoholic beverages and nicotine are outlined below:
Ethanol, C2H5OH (Alcohol)
Nicotine, C10H14N2
Toxicity
Drinking 50 mL of pure ethanol can lead to death
Absorbing one drop of nicotine through the tongue
can cause death.
Health Hazards









Risk of FAS if consumed during pregnancy
Damage to brain, pancreas, liver, and
kidneys
Increase risk of cancer of the stomach,
mouth and liver
Impotence and infertility
Depressant (reduces brain activity that
controls behviours)
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
Increased heart rate and blood pressure
Digestive problems and vomiting
Reduced body temperature
Increased risk of lung cancer and other lung
problems
Stimulant
Chemical Reactions
General Outcome A3: Students will identify and classify chemical changes, and write word and balanced equations for
significant chemical reactions, as applications of Lavoisier’s law of conservation of mass
Reactions in Daily Life

I can provide examples of household, commercial and industrial processes that use chemical reactions to produce
useful substances and energy
Chemical reactions involve the mixing of two or more reactants that forms one or more products.
BAKING
Baking soda reacts with acids in the dough to make carbon dioxide, which helps the dough to rise. Baking powder, which
is baking soda with an additional acidic salt, releases carbon dioxide twice during the baking process, once when it hits
water, and again when it reaches a certain temperature in the oven. Heat helps baking powder produce tiny bubbles of
carbon dioxide, which make a cake light and fluffy.
COMBUSTION
In addition to heat, it is common for a combustion reaction to release light or produce a flame. Once the reaction starts,
enough heat is produced to keep the reaction until it runs out of fuel or oxygen. As damaging as fire (combustion) can
be, when controlled and used correctly, it is very important to survival, providing a way to keep warm and to cook
meals. The fuel source in combustion reactions is most often wood, gasoline, or coal. There are other forms of
combustion reactions which are essential to life. They are used to generate power, provide heat, run motors and cook
food. In a combustion engine, the expanding gases drive the pistons in the engine of the car.
ELECTROLYSIS
Electrolysis is the use of an electric current through an electrolyte to create a non-spontaneous chemical reaction. Water
does not naturally break down into the elemental components. By passing electricity through water thought, it will
break down it into hydrogen gas and oxygen gas. This process is called electrolysis.
H2O(l) → H2(g) + O2(g)
Essential Reactions

I can identify chemical reactions that are significant in societies
PHOTOSYNTHESIS
In photosynthesis, plants convert carbon dioxide and water to glucose (food) and oxygen. Energy from the Sun is
required for the reaction to proceed. Plants do not produce oxygen at night.
carbon dioxide + water + ENERGY  glucose + oxygen
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RESPIRATION
The reverse process of photosynthesis is cellular respiration. In cellular respiration, plants and animals convert glucose
and oxygen into carbon dioxide and water. This process releases energy in a form that the organism can use.
glucose + oxygen  carbon dioxide + water + ENERGY
COMBUSTION
Combustion Reactions often are incredible reactions that we would think of as “Burning” but in reality they are when
any substance reacts with oxygen. Hydrocarbon combustion reactions are a specific type of combustion reactions that
involves one hydrocarbon reacting with oxygen gas to form carbon dioxide and water.
“FUEL” + oxygen  carbon dioxide + water + ENERGY
Evidence of Chemical Change

I can describe the evidence for chemical changes
The following are considered to be evidence of a chemical change:
 energy change / change in temperature
 formation of a gas or precipitate,
 colour or odour change,
ENERGY CHANGE

I can differentiate between endothermic and exothermic chemical reactions
All chemical reactions release or absorb energy.
When heat is released as one of the products the reaction is said to be exothermic, like in Reaction A below. When heat
is absorbed as one of the reactants the reaction is said to be endothermic, as seen in Reaction B below.
Reaction A:
wood + oxygen  carbon dioxide + ash + light + ENERGY
Reaction B:
ammonium thiocyanate + barium hydroxide + ENERGY  barium thiocyanate + water + ammonia gas
Exothermic:
A chemical reaction where heat is released by combining two or more substances. This is
due to the formation of new bonds.
(The surrounding environment becomes hot.)
(i.e.: hydrogen + oxygen  water + energy)
Endothermic:
A chemical reaction where heat is absorbed by combining two or more substances. This
is due to the breaking of chemical bonds.
(The surrounding environment becomes cold.)
(i.e.: energy + water  hydrogen + oxygen)
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FORMATION OF A GAS OR PRECIPITATE
Precipitate:
A solid that forms when two non-solid (liquid or gas) substances are combined, which
indicates that a chemical reaction has occurred.
When two non-gas (liquid or solid) substances are combined and a gas results, this is also evidence of a chemical
reaction. When vinegar (a liquid) is combined with baking soda (a solid), carbon dioxide gas is formed.
The formation of bubbles in a solution doesn't always mean that a new gas is being produced in a chemical reaction,
and can simply indicate that the solution has begun to boil (only when in the presence of heat).
COLOR OR ODOR CHANGE
When paper is burned, the black color just seems to appear out of nowhere. This indicates a chemical change.
There are instances when a change in color occurs without a chemical reaction taking place. For example, combining
water with a red food coloring that results in a light red solution would not be a chemical change because the solution is
an intermediate color between the two, it would be possible to separate the two.
The formed of an odor different from that of the original substances can indicate that a chemical change has likely
occurred. When toast is burned, there is not only a color change, but you can smell an odor that was not there
beforehand.
NOTE: despite any of the above evidence, in ALL chemical reactions a new substance is
formed.
Types of Reactions

I can classify and identify categories of chemical reactions
FORMATION (SYNTHESIS)
Reactions involve two Elements reacting to form one compound
X + Y → XY
DECOMPOSITION
In a decomposition reaction, one compound breaks down into two or more simpler compounds or elements. The
general equation of a decomposition reaction is:
XY → X + Y
You can think of decomposition reactions as the opposite of formation reactions.
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HYDROCARBON COMBUSTION
A hydrocarbon combustion reaction involves a fossil fuels and oxygen, producing carbon dioxide gas (CO2(g)), water and
energy.
CXHYOZ + O2  CO2 + H2O + ENERGY
SINGLE REPLACEMENT
Involve one compound reacting with one element to form one new compound and one new element. The exchange can
be a metal with another metal, or a non-metal with another non-metal.
AB + C  CB + A
DOUBLE REPLACEMENT
Involve two compounds reacting to form two new compounds.
AB + CD  AD + CB
Neutralization reactions are a type of double replacement reaction that involves an acid reacting with a base to form
water and an ionic salt
HB + AOH  H2O(l) + AB
Word & Chemical Equations

I can translate word equations to balanced chemical equations and vice versa for chemical reactions
In a word equation, the reactants are written on the left, and the products are written on the right. They are connected
by an arrow () that is read as "yields" or "reacts to produce". Each reactant is separated from another reactant by a +
sign. When reading the + sign is read as “AND”.
Reactants  Products
Word equations are a way of writing chemical reactions using names instead of formulas.
Predicting the Products

I can predict the products of chemical reactions, when given the reactants
Remember to include your states of matter!
Elements
Refer to your periodic table.
Ionic Compounds (not in water)
Always solid.
Ionic Compounds (in water)
Refer to your solubility chart (either aqueous or solid).
Molecular Compounds (most)
Liquid or gas (not needed in Sci 10).
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MAKE SURE YOUR ION CHARGES ARE BALANCED, FORMING THE CORRECT FORMULAS FOR PRODUCTS!
FORMATION (SYNTHESIS)
IF the reactants are:
Two elements (or an element and a polyatomic ion)
THEN the product must be:
One compound (formed from the two elements)
DECOMPOSITION
IF the reactant is:
One compound
THEN the products must be:
Two elements (or an element and a polyatomic ion) that form the compound reactant
SINGLE REPLACEMENT
IF the reactants are:
One compound and one element
THEN the products must be:
One new compound and one new element
If the element reactant is a metal, then it switches with the metal in the compound
If the element reactant is a nonmetal, then it switches with the nonmetal in the compound
DOUBLE REPLACEMENT
IF the reactants are:
Two compounds
THEN the products must be:
Two new compounds
Exchange the metals in the compounds to form new compounds
HYDROCARBON COMBUSTION
IF the reactants are:
One hydrocarbon and OXYGEN
THEN the products must be:
CARBON DIOXIDE and WATER
Moles


I can define the mole as the amount of an element containing 6.02 × 1023 atoms
I can apply the concept of moles to calculate quantities of substances
A mole (mol) is a word that represents a certain number of things. Like how a dozen represents 12. A mole represents
6.02 × 1023. 6.02 × 1023 is called Avogadro’s Number. It is so large because an atom is so small, but one mole of a
substance is an observable amount.
15
The number of the moles of the elements in a molecule can be different than the number of moles of the molecule
itself. For example, one mole of water (H2O) would consist of two moles of hydrogen and one mole of oxygen. In a
balanced equation, the coefficients in front of each compound or element dictates the number of moles of each
substance required for the reaction.
The atomic mass, or molar mass, is the mass of one mole of a substance (measured in g/mol). The molar mass of sodium
is 22.99 g/mol because 1 mole of sodium has a mass of 22.99 grams. The molar mass of elements can be found on the
periodic table.
The molar mass of a compound determining by adding the molar masses of each element within the compound, and
considering the number of moles of each element in the compound.
The mass of a compound or element can be used to find the number of moles of the sample. The number of moles of a
compound or element can also be used to determine the mass of the sample.
n = # of moles
m = mass of sample
M = Molar Mass
Law of Conservation of Mass


I can interpret balanced chemical equations in terms of moles of chemicals
I can relate the mole concept to the law of conservation of mass
During a chemical reaction, the total mass of the reacting substances (the REACTANTS) is always equal to the total mass
of the resulting substances (the PRODUCTS). The Law of Conservation of Mass was developed based on a series of closed
system experiments using test tubes.
Closed Systems
does not allow exchange of matter between the system and its surroundings)
Balancing chemical reactions ensure that there is the same number of each atom on either side of the arrow in the
reaction. When balancing, only coefficients can be added into the reaction. Coefficients multiply each atom in the
compound.
When oxygen gas (O2) and hydrogen gas (H2) join they form water. Since are diatomic molecules (O2 and H2 instead of
just O or H as single atoms) you may think that two hydrogens and two oxygens would make H2O2 (a poison). Instead
two hydrogen gas (H2) molecules will always combine with one oxygen gas (O2) molecule to form two (H2O) molecules.
Chemical equation:
2H2
+
O2

2H2O

+
Models:
2 hydrogen gas
+
oxygen gas

2 water
The number of hydrogen atoms in the reactants and the product is equal. This is also true of the number of each atoms.
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