Download 1.1 to 1.4

Science 10
Chemistry Unit
Review
1
Chemistry
is the study of matter,
its properties,
composition and
behavior
2
Matter
is anything that has mass
and occupies space. All
matter has physical and
chemical properties.
3
Physical Properties
 are
those properties that cause
a physical change in a
substance
4
• example: boiling point,
density, malleability (can
be shaped without
breaking), and ductility
(can be drawn into a thin
flexible wire)
Chemical Properties
 are
those properties that
describe how substances react
with each other in a chemical
reaction to form a new
substance with different
properties
• example: reactive and inert
(unreactive)
 Note: proof of a chemical
reaction could be a change in
5 colour, energy, state or odour.
Matter Can Be Classified
Matter
Mixtures
Pure
Substances
Elements
Metals
Compounds
Ionic
Non-metals
6
Heterogeneous
Molecular
Homogeneous
Definitions
 Pure
Substances - have fixed
properties that do not vary. Ex.
elements and compounds
 Elements - any substances that
contain only one type of atom.
Ex. C (carbon) and Al (aluminum)
 Molecular elements - whose
molecules consist of more than
one atom of the same element.
Ex. H2(g), S8(s).
7
Definitions
 Compounds
8
- any substance
that contains two or more
kinds of atoms in fixed
proportions. Ex. H2O
• can be broken down
• can be either ionic (made
up of a metal and a nonmetal) or molecular (made
up of two or more non-
Definitions
 Mixtures
- are made up of
two or more different
compounds and or
elements close together.
They do not have a
constant composition and
proportions may vary. Ex.
air, coffee, soft drinks.
9
Definitions
• Heterogeneous mixtures - are
also referred to as
mechanical mixtures because
they contain different types of
substances and states that do
not appear uniform. Ex.
concrete, this room.
10
Definitions
• Homogeneous mixtures have the same
properties throughout.
They appear uniform in
properties and can not
be filtered. Ex. solutions
and alloys.
11
Science 10 - Chemistry Unit
The Periodic Table
12
The Periodic Table
 developed
by Mendeleyev
• by arranging elements
according to atomic mass, he
discovered the Periodic Law
which is the foundation of the
Periodic Table.
 Periodic Law - patterns of
reactivity, behavior, and
properties occur in families or
13
groups of elements.
Patterns in the Periodic Table
 Elements
are organized
according to four basic
patterns:
14
• atomic number
• metals & non-metals
• period
• group/family
1. Atomic Number
 refers
to the number of
protons in an atom. Protons
are positively charged
subatomic particles in the
atom’s nucleus.
15
2. Metals & Non-metals
•
•
•
•
•
•
16
Metals
left of staircase
good conductors of
heat and electricity
shiny
malleable & ductile
form positive ions
all except mercury
are solids at SATP
•
•
•
•
•
•
Non-metals
right of staircase
poor conductors
non shiny
brittle (solids)
form negative
ions
either solids,
liquids, or gas at
SATP
SATP = Standard Ambient Temperature & Pressure
3. Periods
are
the horizontal rows of
elements whose
properties change from
metallic to non-metallic
from left to right along the
row.
17
4. Groups/Families
are
the vertical columns in
the main part of the table
whose elements have
similar chemical
properties. They are
numbered left to right #1 18.
18
4. Groups/Families
a.
alkali metals - (group 1)
– react violently with water
and get more reactive as
you move DOWN the group
–hydrogen is not a member.
19
4. Groups/Families
b. alkaline earth
metals (group2)
–light, reactive metals
c. halogens (group 17)
–extremely reactive nonmetals
–F2(g) is most reactive
20
4. Groups/Families
d. noble gases (group 18)
–extremely low chemical reactivity
or inert (very stable)
e. lanthinides (At. #57-71) and
actinides (At. # 89-103)
21
4. Groups/Families
f. representative
elements - in groups
1,2, and 13-18
g. transition elements in
groups 3-12 - exhibit a
wide range of properties
22
Science 10 Chemistry Unit
Atomic Theory
23
Atomic Theory
Matter
24
is made up of
atoms. Over the past
several hundred years,
there have been many
models of the atom. The
model that we use today is
the Bohr model, which is
named after Niels Bohr.
Parts of the Atom
 atoms
consist of three
subatomic particles, protons,
neutrons, and electrons.
• protons (p+) and neutrons
(nº) are located in the
nucleus
• electrons (e-) are located
around the nucleus
25
Parts of the Atom
Particle Symbol
proton
p+
1+
Mass
(amu)
1
neutron
nº
no chg.
1
electron
e-
1-
negligible
26
Charge
It would take 1830 electrons to
equal the mass of 1 proton or
neutron.
27
Protons
the
28
number of protons
identifies the element.
This is the element’s
atomic number. If this
number changes then
the element becomes
something else.
Protons
in
an atom, the number of
electrons always equals
the number of protons.
This makes the charge on
an atom equal to zero.
•e.g.. carbon has 6 p+
and 6e- = no charge
29
Neutrons
the
number of neutrons in
an atom can be calculated
by subtracting the number
of protons from the atomic
mass.
#nº= atomic mass - atomic
number
30
Neutrons
 isotopes
- are atoms of an
element that have the same
number of protons but the
number of neutrons will vary
from atom to atom.
 Compare
carbon -12 & carbon-14
31
32
Practice Assignment
#of
#of
#of
Name At#
.t# At. Mass protons electrons neutrons
lithium
aluminum
sulfur
chlorine
carbon
nitrogen
magnesium
calcium
33
Practice Assignment
Name
lithium
aluminum
sulfur
chlorine
carbon
nitrogen
magnesium
calcium
34
At.#
3
13
16
17
6
7
12
20
At. Mass
7
27
32
35
12
14
24
40
# of
protons
3
13
16
17
6
7
12
20
# of
# of
electrons neutrons
3
13
16
17
6
7
12
20
4
14
16
18
6
7
12
20