Name
Homeroom
Science 10F
Unit 2 Chemistry
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Item
Notes: Properties and Changes, A Matter of Behavior & Changes in Matter
Investigation 5-A Lab Report
CYU P169
AIMS #1 – What Is Matter Made Of?
Notes: Historical Ideas About the Nature of Matter & Models of Atomic Structure
AIMS #3 – What Parts Make Up An Atom
Timeline of Atomic Models
Notes: Bohr-Rutherford Diagrams
BLM 7-18
Bohr-Rutherford Model Practice (2 Sheets)
Drawing Bohr Model Diagrams (2 sheets)
Total Mark
5
10
10
68
5
119
10
5
6
10
60
Total for Items 1-20
308
Notes - The Periodic Table of Elements
5
108
92
*
*
5
69
50
74
102
20
AIMS #2 – How are the elements listed in special order?
AIMS #4 – How Are Electrons Arranged Around the Nucleus
Crosswords 1 & 2
Elementary My Dear Watson
Notes: Atoms & Ions
AIMS #5 - How Do Compounds Form
AIMS #6 – What Are The Properties of Metals
AIMS #7 – What Is Valence
Aims #8 – How Can Valence Help Us to Write Formulas
BLM 8-1
28
35
13
BLM 8-2 (2 Sheets)
BLM 8-3
BLM 8-4
601
909
100
Total for Items 22-34
Grand Total (Row 22 + Row 37)
Percentage
2
Chapter 5
I.
Properties and Changes
Good Scientists are: questioning, sceptical, persistent, and honest.
1. The Particle Theory of Matter
a) all matter is made up of
.
b) Each pure substance has its own kind of
, different from the particles of other
pure substances.
c) Particles
each other.
d) Particles are
.
e) Particles at a higher temperature
(on average) than particles at a
lower temperature.
2. Scientific Model – any understanding that allows a scientist to picture the processes of nature that
cannot be simply or directly seen.
Example – Particle theory of matter (see p 156)
 points 1 & 2: what matter looks like.
 points 3 – 5:
II.
how matter behaves.
A Matter of Behaviour
In nature particles may be mixed in different ways.
3
A mixture is a substance that contains more than one type of particle.
1. Mechanical mixtures (Heterogenous)
 mixtures in which particles are not
. All parts can be seen.
E.g.
2. Solutions (Homogenous)
 mixtures in which types of particles are
particle (solute) is
. One type of
in the other (solvent) material. Not all parts can be
seen.
E.g.
3. Pure substances
a) Contain only
b) Includes
III.
of particle.
&
.
Changes in Matter
1. Physical changes
a) A change in the substance, but
b) They are often
is formed.
.
 Ex)
 Change in shape – cutting or bending.
2. Chemical Changes
a) A change in a substance(s) in which at least one
(with new
properties) is formed.
b) Often
to reverse.
E.g.
3. Physical properties
-
Can be observed or measured
a chemical change happening.
Ex)
4
4. Chemical properties
– can be observed
a chemical change.
Ex)
5. Qualitative Property
a)
of a property.
b) Cannot be measure
Ex)
6. Quantitative Property
a)
using a number.
E.g.
See table 5.2 page 164
7. Evidence of a Chemical Change:
a)
or absorbed.
b) The starting material is
.
c) A
.
d) A material with
.
e)
form.
f) Grains of a
when 2 liquids are
mixed.
Activities/Assignment
- Teacher Demonstration
o Investigation 5-A, page 160-161
- Read pages 152-169
- Do CYU on page 169 1-4
- AIMS #1
5
Changes of State
GAS
VAPORIZATION/
EVAPORATION
CONDENSATION
SUBLIMATION
SUBLIMATION
LIQUID
MELTING/
FUSION
FREEZING/
SOLIDIFICATION
SOLID
The changes on this side use energy
The changes on this side give off energy
6
Teacher Demonstration - Steamboat
IV.
Historical Ideas About the Nature of Matter
1. Ancient Greek Philosophers (500 B.C.E.)
a) Wondered why
.
b) Manipulated ideas in their minds
.
c) Empidocles proposed that matter was composed of four elements:
,
,
,&
.
d) Democritus suggested that matter was made of
that could not be
. He called these
“atomos,” which means
.
e) This model was later rejected by
&
and
predominant thinking went back to the
lasted for the next
. This
years.
2. Alchemists: (500-1600 A.C.E.)
a) First people to perform
.
They were part
.
b) Three main beliefs:



7
3. Modern Chemists
a) Sir Francis Bacon (1561-1626)
 contributed the
.
 Argued that science should be based on
.
b) Robert Boyle (1627-1691)
 1661 published “
” wrote about elements as being
“
”.
 Recognized that elements could be
.
 But didn't know
.
c) Joseph Priestly (Late 1700’s)
 First person to
.
 He didn’t know
.
d) Antoine Lavoisier (1743-1794)
 Defined elements as “
. (We still use this
definition today.)

Discovered and identified
based on
.
 Identified air as
.
8
V.
Models of Atomic Structure
1. Dalton's “Billiard Ball” Model (early 1800’s) page 183
a) All
are composed of
are
. Atoms
,
,&
.
b) Atoms cannot be
.
c) All atoms of the same element are
, but they
are different in
.
d) Compounds are created when
.
2. Thomson’s “Raisin Bun” Model of the Atom (1904)
a) Discovered electrons (
) through experiments that involved
. This
disproved Dalton’s theory that
.
b) Discovered protons (
)later
using more advanced apparatus.
c) Thomson proposed the following
 Electrons have a
.
 An atom is
.
 Negative electrons are embedded in the
the resulting atom is
, so that
.
9
3. Rutherford’s “Nuclear” Model
a) Shot alpha particles (a type of radiation) through gold foil
to test Thomson’s model and discovered a
.
b) He proposed
 The nucleus is a very tiny, dense, and
.
 All of the atom’s positively charged particles, called
protons, are
.
 The nucleus is surrounded by
.
 Rapidly moving,
are scattered outside the nucleus
around the atom’s edge in what is referred to as an
.
4. Bohr’s “Planetary” Model (1913)
a) Improved on Rutherford’s model by placing electrons in
.
b) He proposed:
 Electrons move around the nucleus in nearly
, much like how
planets circle the Sun.
 Each electron in an orbit has a
. Electrons can
without loss of
energy.
 The nucleus is surrounded by
.
 Rapidly moving, negatively charged electrons are scattered
around the atom’s edge in what is referred to as an
.
10
5. Einstein’s Quantum (“Wave”) Model of the Atom –
Quantum Mechanics
a) Bohr’s model worked well in explaining the behaviour of
, that contained few
electrons, but it did not explain
.
b) The Quantum Model proposed the following:
 Electrons
like planets
around the sun.
 It is impossible to determine
.
 The probable location of an electron is
.
 Energy levels are divided into
, and each sublevel is
made up of several
.
 Electrons
called orbitals.
Assignment
- AIMS Booklet #3
- Timeline of Atomic Models Diagrams
11
Name
Timeline of Atomic Models
Use you textbook or other resources to draw a diagram of each atomic model.
Democritus (460 BCE – 370 BCE)
Dalton’s Model (Early 1800’s)
Thomson’s Model (1906)
Rutherford’s Model (1910)
Describe the Electron Cloud Model of
the atom. What are the smallest parts
of an atom known today?
Bohr’s Model (1913)
12
VI.
Bohr-Rutherford Diagrams:
1. Protons – a
charged subatomic particle.
2. Neutron – a
charged subatomic particle.
– Protons and neutrons make up the
approximately
3. Electron – a
of an atom and each one has a mass of
.
charged subatomic particle that
nucleus in
the
or SHELLS. It has a mass so small that it generally
doesn’t count.
4. Atomic mass – the
amount of mass of an atom and is equal to the # of
protons + # of neutrons.
5. Electron shells
a) The electrons move around the
in orbits called shells.
b) The more energy the electron has, the
it is from the nucleus.
c) The shells can hold:
– K shell =
electrons
– L shell =
electrons
– M shell =
electrons (18 if forced)
6. Drawing Bohr-Rutherford Diagrams
a) Find the
on the periodic table
b) The atomic
= # of
c) Find the atomic
number)
d) # n’s = atomic mass – # of p’s)
= # of
on the periodic table (round off to the nearest whole
e) Draw the nucleus as a
with the # p’s and # n’s inside.
f) Draw the same number of electrons as protons placing them in the shells (pair them up in 2s.
g) Practice
Assignment
– BLM 7-18
– Bohr-Rutherford Model Practice
– Bohr-Rutherford Diagrams for first 20 elements
13
Bohr-Rutherford Model Practice
Name: ___________________________
Part A:
Complete the Chart
Element
Name
Symbol
Atomic
Number
Atomic
Mass (2
decimals)
# of
Electrons
# of
Protons
# of
Neutrons
0
Phosphorus
9
Mercury
Ne
Silicon
Oxygen
28
Beryllium
Tungsten
65
1) How is the number of protons determined?
2) How is the number of electrons determined?
3) How is the number of neutrons determined?
14
15
16
VII. The Periodic Table of Elements
1. History
a) In the 1850s there were about
.
b) They were named by the
.
c) The lists were made in
.
d) Unfortunately that meant
the entire table when
new
.
2. Dmitri Mendeleev
a) organized elements in
(families) with similar
b) He arranged them in
with the
.
first and the
last.
c) Mendeleev’s system allowed the periodic table
for the elements that
since he could leave room
.
d) It also allowed people to “look for” the
.
3. Families
a) Alkali Metals

(1 e- beyond stability)



b) Alkaline Earth Metals

(2 e- beyond stability)



17
c) Halogens

(1 e- beyond stability)



d) Noble gases





e) Coinage Metals
 got their name because
 they are all
(stretched into
was made from these elements
(
) and
)
 all are
 they occur in their
(earliest metals discovered)
 they are not
 fairly high
4. Patterns in the Periodic Table
a)
b)
c)
d)
e)
f)
Assignment
- AIMS #2 & #4
- Crosswords 1 & 2 and Elementary My Dear Watson
18
ELEMENTary My Dear Watson
In the following mystery, students replace the symbol with the name of the element. If the element name
is given, they substitute the symbol. Some of the blanks involve compounds which you may leave to be
completed later, or simply provide the answers.
Twas the week before Christmas, when Inspector Lestrade came to me with a most distraught gentleman in
tow. (Helium) ________ explained that the gentleman had purchased several pieces of (Ag) ______and (Au)
________ jewelry for his wife or mistress, (iodine) ___ surmised, which had disappeared during a street
(carbon + argon) __________ ride, (nobelium) ________ doubt to see (hydrogen+erbium) _______! The
victim interrupted with "You must (Fe) _______ this out before the 24th, Mr. (Ho) ___________! I will not
(Fe2O3) _________________ until the jewels are recovered and the culprit made to (S) ___________ as
(iodine )____ have this day! (holmium and tungsten) _______________ dare someone (sulfur + tellurium +
aluminum) ____________ from me! I’d gladly (Ba) _______ with the fishes and watch him (Zn) ________ in
the Thames River! His diatribe did tend to (B) _________.
(oxygen + nitrogen) __________questioning I learned the (carbon + argon) __________ was number (Sn)
______, an express which did not stop during (hydrogen + iodine+ sulfur) _________ trip. (arsenic) ______
to unusual events, (helium) ______ remembered a (Cu) _______evicting the occupants of the seat behind
him and sitting there himself. Enjoying the ride, (helium) ___ was just thinking, "These areas (As) _____,"
when a bad jolt made the (calcium + selenium) _______ of jewelry (sulfur + lithium + phosphorus) ______
between the seat and back of the bench (helium) ____ occupied. The (Cu) ___________ retrieved it for
him. (oxygen + nitrogen) ______ checking later, he found the jewelry missing from the (calcium + selenium)
___________. (astatine) ______ their destination, (helium) ____ and the (Cu) ________ searched everyone,
and each other, (arsenic) ____ well as the (carbon + argon) _______. (nobellium) _____ jewels were found.
By this time, Lestrade seemed eager to (beryllium) _____ rid (oxygen + fluorine) ______ our pompous
victim, as (tungsten + arsenic) ____ (iodine) ____. (Indium) _____ private, the Inspector explained that he
wasn’t personally (Sb) ___________, but just wanted the theft cleared (uranium + phosophorous) ______
quickly (sulfur + oxygen) _______ he could get (oxygen + nitrogen) ______ to matters more important than
petty theft. (Iodine) ___ agreed to help, not to save the Inspector time and embarrssment (tungsten +
helium + nitrogen) __________ he failed, (arsenic) ______ I (potassium + neon + tungsten) ___________ he
would, but I had the (calcium + selenium) __________ already solved. Informed of this, the Inspector cried,
"(Sulfur + oxygen) _____ fast! (Hydrogen + oxygen + tungsten) _______?! My only reply (tungsten +
arsenic) ____________ that he meet me after (I) __________d, armed, and carrying a (Ni) ________.
(Astatine) __________ dusk, the Inspector and (iodine) ____ rode the next to last streetcar of the day to
the end (oxygen + fluorine) ______ the line, the (C) _____. I used Lestrade’s (Ni) ______ to pay my fare.
(Indium) _____ the deserted (C) _______ I found number (Sn) ____ and climbed inside. Reasoning that the
culprit sat behind our victim (Pb) _______ me to examine that seat, and I found scratches on the (F)
________. Prying (uranium + phosphorus) _______ a loose piece of (F) ________, I found the missing (Ag)
______ and (Au) ___________ jewelry in a (boron + silver) ______. I substituted worthless (SiO2)
_____________ to simulate the theft of the (rhenium + aluminum) ____________ articles, and replaced the
(boron + silver) ______ under the (F) __________. The Inspector and (iodine) ______ then concealed
ourselves to await the thief. Nearly dozing (oxygen +2 fluorine) ______, I was startled by the sound of
footsteps echoing (indium) ___ the deserted (C) ________. A shadow entered number (Sn) ______ and I
heard the (F) _________ being lifted, a brief silence, then an expletive and "The jewels (Ar) _____!" The
19
Inspector yelled "Police!" and I yelled "(Cs) ________!" as we both jumped into different ends of the
streetcar. After a brief struggle, the Inspector had his (Ne) _______ the culprit, (tungsten + holmium)
________ was subdued and handcuffed. I turned (oxygen + nitrogen) ______ the torch and beheld a
uniform (oxygen + fluorine) ______ blue with (bromine + arsenic + sulfur) ________ buttons. "(Ho)
________!" exclaimed the Inspector. "It’s the (Cu) __________!" "Of course," I replied, "It’s elementary,
Inspector. He’s a (Si) __________ who found his comedy routine impersonating a (Cu) __________ in
prison to (beryllium) ____ infinitely (molybdenum + rhenium) __________ rewarding on the outside -almost."
VIII. Atoms vs. Ions
1. Atoms
a)
b)
c) are ‘happiest’ when they have
.
They are very dissatisfied they “
”
2. Ions
a) atoms which have
.
b)
. (electrons are negative!)
c)
to get empty valence shells. They
become
.
E.g. Alkali Metals like Na lose 1 e- and become
E.g. Alkaline Earth Metals like Mg lose 2 e- and become
d)
to get full valence shells. They become
.
E.g. If Cl gains 1 electron it becomes
3. Chemical Bonding
a) Atoms always bond with each other
.
b) There are 3 ways in which atoms bond together. We will only study 1 way.
c) Ionic bonds

.
 Metals happily
which happily accept the
electrons.
 Electrons transfer making
.
d) Ionic compounds are formed.
20
e) Ionic compounds:

. (strong ionic bonds)

.
 are electrolytes –
(aqueous).
Assignment – AIMS 5 & 6
4. Writing Chemical Formulas

E.g. Na + Cl
.
NaCl
Find the type/charge of ion formed
– From the family/group
Describe how many ions are needed to balance
the charges
Write the compound (metal first)
E.g. Mg + Cl
MgCl2
Find the type/charge of ion formed
– From the family/group
Describe how many ions are needed to balance
the charges
Write the compound (metal first)
21
Assignment
– AIMS 7 & 8
– BLM 8-1, 8-2 (2 pages), 8-3 & 8-4
22