Transcript snc1p chemistry unit review

CHEMISTRY:REVIEW
SNC1P
SAFE LAB TECHNIQUES
When lighting a Bunsen Burner, ensure all long
hair and loose clothing is out of the way
 When smelling a chemical waft it towards you.
DO NOT SMELL it directly
 Put broken glass in the designated bin
 When something is spilled. Notify Mr. Hoover
immediately
 If something breaks. Notify Mr. Hoover
immediately

SAFE LAB TECHNIQUES
Never eat or drink in the lab
 Wash hands after handling chemicals
 When performing a lab, always stay standing, do
not sit down.
 Never leave a Bunsen burner unattended
 Always use appropriate equipment
 Always wear safety goggles
 Never wear open toed shoes in the lab

WHMIS
The Workplace Hazardous Materials Information
System (WHMIS) is Canada's national hazard
communication standard.
 The key elements of the system are cautionary
labelling of containers of WHMIS "controlled
products", the provision of material safety data
sheets (MSDSs) and worker education programs

WHMIS SYMBOLS
CLASS A: COMPRESSED GAS
 This class includes compressed gases, dissolved
gases, and gases liquefied by compression or
refrigeration.
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WHMIS SYMBOLS
CLASS B: FLAMMABLE AND
COMBUSTIBLE MATERIAL
 This class includes solids, liquids, and gases
capable of catching fire in the presence of a spark
or open flame under normal working conditions.
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WHMIS SYMBOLS
CLASS C: OXIDIZING MATERIAL
 These materials increase the risk of fire if they
come in contact with flammable or combustible
materials.
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WHMIS SYMBOLS
CLASS D: POISONOUS AND INFECTIOUS
MATERIAL
Division 1: Materials Causing Immediate
and Serious Toxic Effects
 These materials can cause death or immediate
injury when a person is exposed to small
amounts. Examples: sodium cyanide, hydrogen
sulphide
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WHMIS SYMBOLS
CLASS D: POISONOUS AND INFECTIOUS
MATERIAL
Division 2: Materials Causing Other Toxic
EFFECTS
 These materials can cause life-threatening and
serious long-term health problems as well as less
severe but immediate reactions in a person who
is repeatedly exposed to small amounts.
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WHMIS SYMBOLS
CLASS D: POISONOUS AND INFECTIOUS
MATERIAL
Division 3: Biohazardous Infectious
MATERIAL
 These materials contain harmful microorganisms that have been classified into Risk
Groups 2, 3, and 4 as determined by the World
Health Organization (WHO) or the Medical
Research Council of Canada.
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WHMIS SYMBOLS
CLASS E: CORROSIVE MATERIAL
 This class includes caustic and acid materials
that can destroy the skin or eat through metals.
Examples: sodium hydroxide, hydrochloric acid,
nitric acid
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MATTER HAS MANY FORMS
Matter – anything that has mass and
volume.
 Mass is a measure of the quantity of an object. (g,
kg,)
 Volume is a measure of space taken up (mL,
L)
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Matter can be found as a solid, liquid or gas. (or
even a combination of these)
CHANGES OF STATE
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There are 3 states of matter
Solid
 Liquid
 gas
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TERMS FOR CHANGES OF STATE
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Melting – Change from a solid to a liquid
Evaporation - Change from a liquid to a gas
Condensation - Change from a gas to a
liquid
Freezing - Change from a liquid to a solid
Sublimation - Change from a solid to a
gas
Deposition - Change from a gas to a solid
TERMS FOR CHANGES OF STATE
THE PARTICLE THEORY OF MATTER (4
POINTS)
Way of describing matter.
1.
All matter is composed of very tiny objects
called particles.
2.
Each Pure substance has its own kind of
particles, different from the particles of
other pure substances.
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THE PARTICLE THEORY OF MATTER (4
POINTS)
3. Particles present in matter are always in
motion. They may be vibrating back and forth,
as in a solid, or moving in all directions, as in a
gas. In a liquid, particles stay close together but
can slide past one another.
4. The particles in a substance attract each
other. The amount of attraction is different for
different kinds of particles. All particles have
spaces between them.
THE PARTICLE THEORY OF MATTER (4
POINTS)

The distances between the particles change for
different states of matter.
CLASSIFICATION OF MATTER
Matter
Pure
Substances
Element
Compound
Mixture
Mechanical
Mixture
Suspension
Solution
PURE SUBSTANCES (2)
A pure substance is made up of only
one kind of matter
 unique set of properties
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A
colour, hardness, boiling point, and
melting point.
pure substance is either an
element (gold) or a compound
(sugar).
ELEMENT
A pure substance that cannot be broken down into
any simpler substance by chemical means.
 Each element has its own name and symbol.
Example: Gold (Au)
COMPOUND
A pure substance that is made from two or more
elements that are combined together chemically.
 Example, water (H2O) is a compound containing
the elements hydrogen and oxygen.
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MIXTURES (3)
A
mixture is a combination of pure
substances.
 Each substance remains in its original,
pure form, although each is not always
easy to see distinctly once the mixture is
made.
MECHANICAL MIXTURE
(HETEROGENEOUS MIXTURE)
 Different
substances that make up the
mixture are visible
 Hetero = different
SUSPENSION
A
cloudy mixture in which tiny particles of
one substance are held within another.
 Can be separated out when the mixture is
poured through filter paper.
 A suspension is also a heterogeneous
mixture.
SOLUTION (HOMOGENEOUS MIXTURE)
 Different
substances that make it up are
not individually visible
 One substance is dissolved in another
 The prefix “homo-” means same, and all
parts of a homogeneous mixture look the
same.
PHYSICAL PROPERTIES
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-A physical property describes a
characteristic of a substance that can be
observed or measured without changing the
composition of matter.
Example: Melting Point, Boiling Point
OBSERVING PHYSICAL PROPERTIES
Property
Description
Examples
Colour and
lustre
The light the substance reflects
gives it colour and lustre
(shine)
The names for some
substances, such as gold,
are also the names of colours.
Gold has lustre; concrete is dull
Conductivity
Conductivity is the ability
of a substance to conduct
electricity or heat. A
substance that conducts
electricity or heat is called a
conductor. A substance with
little or no conductivity is an
insulator.
Most metals are good
conductors. Copper is a very
good conductor of electricity and
so is used to make electric wires.
Styrofoam® and glass are
insulators.
What it looks like
OBSERVING PHYSICAL PROPERTIES
Property
Description
Examples
Density
Density is the amount of
mass in a given volume
of
a substance.
D = m/v
Ductility
Any solid that can be
stretched into a long
wire is said to be
ductile.
The density of pure water
is 1 g/mL.
The density of gold is 19
g/mL.
Water is denser than oil,
but gold is denser than
water.
Copper is a common
example of a ductile
material.
What it looks like
OBSERVING PHYSICAL PROPERTIES
Property
Hardness
Malleability
Description
Hardness is a substance’s
ability to resist being
scratched. Hardness is
usually measured on the
Mohs hardness scale from
1 to 10.
A substance that can be
pounded or rolled into
sheets is said to be
malleable.
Examples
The mineral talc is the
softest substance on the
Mohs hardness scale (1).
Emerald is quite hard (7.5).
Diamond is the hardest
(10).
Aluminum foil is an
example of a malleable
substance.
Metals such as gold and tin
are also malleable.
What it looks like
OBSERVING PHYSICAL PROPERTIES
Property
Viscosity
Description
Examples
Viscosity is the
Honey has a high
resistance of a fluid to viscosity
flow.
Compared to water.
What it looks like
OBSERVING CHEMICAL PROPERTIES
A chemical property describes the ability of a
substance to change into a new substance or
substances.
 In order to view a chemical property a chemical
change must occur.
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Chemical change - the formation of a new
substance or substances with new properties.
A chemical reaction is a process in which a
chemical change occurs.
CHEMICAL PROPERTIES
1. Combustibility is the ability of a substance to
burn. In order to burn a substance requires
Oxygen
CHEMICAL PROPERTIES

2. Light sensitivity is a chemical property of
that can cause new substances to form when light
hits it.
CHEMICAL PROPERTIES
3. Reacting with an acid is a chemical property
where when acid is poured on a substance it
produces a gas and bubbles.
CLUES THAT A CHEMICAL CHANGE HAS
OCCURRED
Clue
Evidence
Change in colour
Final product(s) may have a
different colour than the colours of
the starting material(s).
Formation of a
solid (precipitate)
Final materials may include a
substance in a state that differs from
the staring material(s): Precipitate
CLUES THAT A CHEMICAL CHANGE HAS
OCCURRED
Clue
Formation of a gas
Evidence
Final materials may include a substance
in a state that differs from the staring
material(s); commonly, a gas
Release / absorption Energy (light, electricity, sound or most
of heat or light
commonly heat) is given off or absorbed.
The change is difficult The change cannot be reversed or it is
to reverse
difficult to.
ATOMS ARE COMPOSED OF THREE
SUBATOMIC PARTICLES
1.
2.
3.
Protons- Heavy positively charged found in the
nucleus
Neutrons -are neutral particles that have the same
mass as protons and are located in the nucleus
Electrons- Negatively charged particles with almost
no mass. They circle the nucleus at different energy
levels.
ATOMS ARE COMPOSED OF THREE
SUBATOMIC PARTICLES

Atoms are
electronically
neutral so the
number of electrons
= the number of
protons
METALS
Found on the Left side of the periodic table
 The majority of elements on the periodic table are
metals. All metals, except for mercury are solids
at room temperature. Metals have the following
properties.
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Malleable: The ability to be hammered or bent
into a shape.
METALS
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Lustre: They are shiny in appearance.
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Ductile: They can be pulled into a wire.
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Conductor of electricity: Electricity can travel
through the metal.
METALS

A mixture of two or more metals is called an
alloy. The process of alloying different metals
together can enhance the properties of the metal.
NON-METALS
Non-metals generally have these properties:
 Non-conductor of electricity in its solid form
 At room temperature most are gasses (11) or
solids (5) and only one is liquid.
 Solids are brittle and lack the lustre of metals
METALLOIDS
Found in the middle-right of the periodic
table
 Some elements do not fit as metals or nonmetals. These fit on either side of the staircase
that divides the metals and the non-metals.
 They have some properties of metals and some
properties of non-metals. They are called
semiconductors because they do not conduct
electricity well.

ATOMIC NUMBER (Z)
Atomic number - the number of
protons in an atom of an element.
 Each element has a set number of
protons and every atom from that
element will have that many protons.
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The pattern for increasing protons moves
from left to right and then down to the
next row just like reading a book.
ATOMIC MASS (A)
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Atomic mass - the average mass of an element’s
atoms.
Atomic mass is given in atomic mass units (amu).
H has a mass of 1.01 amu. This means that iron
atoms are about 55.85 times heavier than hydrogen
atoms.
Atomic masses are always expressed as decimal
fractions. One reason that they do not have whole
number values is that, except for fluorine, atoms of
the same element have different numbers of neutrons.
ION CHARGE
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Ion charge - the electric charge that an atom
takes on when it loses or gains electrons.
An atom or group of atoms that has lost or gained
electrons is called an ion.
Electrons have a negative charge, and so an atom that
loses electrons becomes a positive ion. An atom that
gains electrons becomes a negative ion.
Metal atoms can lose electrons in certain situations.
(positive ions)
Non-metals can gain electrons in certain situations.
(negative ions)
ION CHARGE
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Elements with atoms that can form
similar ions are grouped together in the
periodic table. Metals generally lose
electrons and become positive ions.
Many non-metals can gain electrons
and so become negative ions.
CALCULATIONS
Determining the number of neutrons
 Subtract the atomic number (# of protons)
from the Atomic mass (# of protons and
neutrons)
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Atomic mass – atomic number (A – Z = N)
Example: Iron
 55.85 – 26 = 30 neutrons
BOHR DIAGRAMS
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To represent electron arrangements at various
orbits we use Bohr diagrams. Each orbit has a set
number of electrons.
Orbit #
1
2
3
4
# of Electrons
2
8
8
18
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Every row in the period contains a shell. The
farther you move down the table the more shells
you added to the diagram. H = 1 shell, Li = 2 shells,
K = 3 shells.

Moving left to right on the periodic table adds
valence electrons to the shells of that row. Na has 1
valence e-, Mg has 2 valence e-, Al has 3 valence e-,
etc.