Unit 2: Chemistry
5.1: Matter
What is Matter?
What is Chemistry?
Particle Theory of Matter
1. All matter is made up of _______________________________ that have ___________________
_______________________
2. All particles of one substance are __________________. Different substances are made of
___________________________________________________
3. Particles are in ______________________________________________
4. The particles of a substance _______________________________________________________
5. Particles __________________________________
States of Matter
Changes of State
Classification of Matter
5.2 & 5.3: Physical and Chemical Properties
What is a Property?
Physical Properties
Two Types of Physical Properties:
Examples of Physical Properties
Property
Definition
Example
Water is a
at room temperature
Sugar is composed of
Four is a
Aluminum foil has a
A rusty nail has a
Glass is
Sand is
The windows in the classroom are
Frosted glass is
The wall is
Glass is
Silly Putty is
Property
Definition
Example
Honey is
Water is
Wax is
Diamonds are
Aluminum is
Glass is
Copper is
Copper wires have
Plastics do not
Iron has a
Aluminum has a
Sugar is
Sand is
Sugar is
Water is
Sulfur smells like
Other examples:
Chemical Properties
Examples of Chemical Properties
Property
Definition
Example
Gasoline is
Candle wax is
Magnesium reacts with acid, producing gas
bubbles and heat
Mercury is
5.2 & 5.3 Physical and Chemical Changes
PHYSICAL CHANGE

___________________ substance is formed

The particles of the starting substance(s) _________________________________

The change can usually be _________________________________
Common Clues and Examples of a Physical Change:
Clue
Example
CHEMICAL CHANGE

at least one ___________________________ is formed

The particles in the substance(s) _____________________

Is usually _________________________________________________
Evidence for a Chemical Change:
1. Formation of _________________________ NOT caused by ____________________

The _________ is the new substance
2. Changes in _______________________________________

Could get ________________ or __________________

_______________ is often an indication that heat is produced
3. Formation of a ______________________________________

A ________________ is formed when two _____________________________ are mixed
4. Distinct _________________________

eg.

Adding blue food colouring to water is NOT a chemical change – blue was the colour of one
of the original substances (this is just __________________________)
5.
Distinct _____________________________
5.6: Characteristic Physical Properties
Characteristic Physical Properties

A physical property that is ________________ to a substance and that can be used to
______________ the substance.

For example, knowing the __________________________________ of a substance is not helpful,
because these values aren’t _______________ to substances.
1. Freezing/Melting Point and Boiling Point


Different substances ________________ and _____________________ at different temperatures.

For example, water freezes/melts at ________ and boils at ________

But, mercury melts at ________ and boils at ________
Question: How does salt melt snow and ice? Why do we put it on our roads and walkways in the
winter?
Answer!

Once salt is added to water,

Adding salt_________________________________________, so it will __________ at a
________ temperature than pure water.

Water with salt can stay a liquid until the temperature is as low as ___________

By adding salt to roads,
2. Density

A measure of _________________________________________________________________,
or how ___________________________ the particles are

Calculated by dividing ________ of a substance by its ____________


Units are __________ (solid) or __________ (liquid)
Example: a puffy marshmallow has the _________ mass as a squished marshmallow, but a
__________ density (the squished mallow takes up less volume and its particles are closer
together)
Density Calculations
Formula:
Formula Triangle:
Density Examples - Use the GRASS method
G–
(write value(s) given with symbol and units)
R–
(write symbol of what you are solving for)
A–
(write formula you will use)
S–
(sub in values to formula and solve)
S–
(write a statement that includes your final answer with UNITS!)
1. A softball has the mass of 360 g and a volume of 270 cm3. Find its density.
2. What is the mass of a silver coin which has a density of 10.0 g/cm3 and a volume of 4.0 cm3?
6.1: Introduction to The Periodic Table of the Elements
What is an Element?
What is a Compound?
What is the Periodic Table?

The Periodic Table is like a chemist’s ______________________.


The alphabet is composed of 26 letters, but these 26 letters can make up countless words.
The Periodic Table is a list of ________________ that can make up countless _______________,
in many different combinations.

“periodic” means “____________________________”
Some Basic Information about the Periodic Table
Element Symbol

an abbreviation for an element seen on the periodic table
Rules/Patterns for Element Symbols:
1. Composed of either ________________________________
2. The first letter is always ____________________. The second letter is always ______________
3. Usually contains letters from the ________________________
C=
Ca =
Cl =
4. Some symbols are based on the ___________________.
Ag stands for ___________ because its Latin name is __________________
Groups and Periods

Horizontal rows are called ___________________

Vertical columns are called __________________________________________

Which element is in:

Group 4, period 5?

Group 1, period 6?

Group 18, period 2?
Metals and Non-Metals

The _________________________ divides the ______________________________________

Metals are found to the _________ of the staircase (EXCEPT _________________ – it is special)

Non-Metals are found to the _____________ of the staircase

Metalloids are the elements _____________ the staircase (EXCEPT ALUMINUM and ASTATINE)
6.4: How the Periodic Table Came to Be
Textbook pg 223-224
-
In the 1860s, many scientists worked together to sort and organize the elements known at
that time.
-
One scientist stood out for his work with organizing and finding relationships among elements.
His name was ______________________________ (a Russian Chemist). Mendeleev is
known today as the _____________________________________________!
How did Mendeleev organize the periodic table? (1860s – 1870s)?
-
He made a card for each element known at the time (only 63), stating properties
like______________________________________________________________________
-
He arranged the 63 cards in order of ____________________________________________
-
He started with the ___________________________________, followed by the next
____________________________
-
He left spaces _____________________________________________________________
-
Mendeleev noticed that when he arranged the elements in order of increasing mass,
_________________________________________________________________________
-
In a brilliant move, Mendeleev decided to arrange elements with ______________________
_________________________________________________________________________
of the table, still keeping them in order of increasing atomic mass. In order to do this, he had
to force new rows of different lengths causing the table to be an ______________________!
Is the periodic table today organized like Mendeleev’s table?
-
To discover this answer, look at all the elements in period 4, then period 5.
o _____________________________________________________________________
o _____________________________________________________________________
- The elements in today’s periodic table are organized according to
___________________________ NOT _________________________
6.4: Patterns in the Periodic Table
Metals vs Non-metals
Properties
Metalloids
Metals
Non-metals
Families of Elements
Family (Group) Name
Hydrogen:
Group #
Examples
Properties
6.6 - Theories of the Atom
Scientific Theory – an expression of our best _______________________ of a phenomenon, based on
_________________________ or ____________________.
-
Theories need to be _______________ as technologies improve and new observations are made.
-
The theory of the ____________ has changed a lot over time.
400 BCE: An Indivisible Particle
Who? Democritus (a Greek Philosopher)
-
All matter can be divided into ____________________________________ until an indivisible
particle is reached. This is an ____________. Atom means “____________________________.”
-
Based on REASON, not EXPERIMENTATION
450 BCE: Earth, Water, Air, and Fire
Who? Aristotle (a Greek Philosopher)
-
Supported the theory that all matter is made up of four basic substances: earth, water, air, and fire.
-
This theory was accepted for almost ___________ years.
-
Based on REASON, not EXPERIMENTATION
1807: The Billiard Ball Model
Who? John Dalton (English Scientist and teacher)
-
Proposed that:
o
All matter is made up of tiny, indivisible particles called ________________
o
All ________________ of an ______________ are identical
o
Atoms of different elements are ________________________
o
Atoms are ______________________ to form new substances in chemical reactions, but
they are never ______________ or __________________
-
Called “billiard ball model” because he thought an atom was
_____
__________________________________________________________________.
-
Very useful because it explained ______________________________________.
-
But, it could not explain why some objects___________ each other and other objects _________
each other.
1897: The Plum Pudding Model – The Electron
Who? J.J. Thomson
-
Thomson discovered that some particles were ________________ charged and some were
_________________ charged.
-
Theorized that:
o
Atoms contain negatively charged particles called ____________________.
o
Since atoms are _____________, the rest of the atom is a _________________ charged
sphere.
o
-
Negatively charged electrons are ____________________________ throughout the atom.
Called “The Plum Pudding Model” because the ________________ embedded in an atom
resembled raisins in plum pudding. Today, we can think of it as a “Chocolate chip muffin” model.
1909: The Gold Foil Experiment – The Nucleus and the Proton
Who? Ernest Rutherford
-
Tested Thomson’s model of the atom
-
Performed an experiment involving passing particles through gold foil and observing what happens
-
Rutherford discovered:
o
The center of an atom has a _____________ charge. The center is called the __________.
It contains most of the atom’s mass but occupies a very _____________ space.
o
The nucleus is surrounded by a __________ of negatively charged __________________.
o
Most of the atom is _______________________.
o
________________ are positively charged particles contained in the nucleus.
o
Predicted that there must be a third particle in the nucleus that have approximately the
same mass as a proton.
1932: The Neutron
Who? James Chadwick (Rutherford’s Student)
-
Found a particle with ______________ charge
-
Proposed that:
o
An atom must be an ___________________ with a tiny dense central nucleus.
o
The nucleus contains protons (positively charged particles) AND _____________________
(_______________ particles).
o
The ___________ of a neutron is about the same as a ______________.
o
Negatively charged electrons ________ rapidly through the empty space around the
_____________.
o
A neutral atom as the same number of ______________ and ___________________.
1913: Electron Orbits
Who? Niels Bohr (Danish Scientist)
-
Electrons occupy ____________________ around the nucleus (much like
_____________________________________________________________________________).
6.7: Explaining the Periodic Table
What is in the atom?
 The atom is made up of three ______________________________________________
Subatomic Particle

Symbol
Charge
Mass (u)
We can use the periodic table to determine the amounts of these 3 particles contained in each
element
Atomic Number
 The periodic table is arranged according to _______________________________

Tells you the ________________________________________ in an atom’s
___________________

Each atom has ________________________________________________________________
Atomic Mass
 The ___________________________________________________________

Measured in ________________________________________ (u)

This is an ___________________________________ value (use two decimal places)
Isotope

An atom with the __________ number of ______________but a _______________ number
of ______________

The atomic mass is really an __________________ mass of all the different isotopes of an
atom

Example: Isotopes of carbon can have ___________________________ neutrons. But it
only ever has __________ protons.
Mass Number
 The _____________________________________________ (to the nearest whole number)

The _________________________________________________ in an atom’s nucleus
Atomic (Standard) Notation
• A standard way to show subatomic particle information
# Protons =
# Neutrons =
# Electrons =
Ex: Fluorine
#p=
#n=
#e=
TRY: Carbon
TRY: Bromine
Standard notation:
Standard notation:
#p=
#p=
#n=
#n=
#e=
#e=
Bohr-Rutherford Diagrams

Combines Bohr and Rutherford models of the atom

A drawing that shows the _______________ and ________________ of the 3 subatomic particles

____________________ ______________ are __________________________________ and do
not move


__________________________________ around the nucleus
◦
The first orbital can hold up to _____ electrons
◦
Each orbital after that can hold up to ______ electrons
______________________________ are electrons in the outermost electron shell
How to draw:
1. Draw a ______________ for the _______________
•
inside, write the number of protons and neutrons
2. Draw a _____________ for each ____________________________ .
Add electrons (maximum of _______!) A __________ represents an electron.
3. Draw more shells as needed and add electrons (maximum of ______________!)
Practice:
Hydrogen
Carbon
Sulfur
Atoms and Ions
Lewis Dot Diagrams

Simpler diagram of an atom

Show only the _____________ (_____________) electrons in an atom


Because these are the only electrons that will ____________
Write the element ______________ and draw _________ for its number of valence electrons
around the symbol
Atoms vs Ions

Atoms have an ______________________________ (# protons = # electrons)

Most atoms by themselves are not “happy” (because they are not ________________)

They want to have their outer orbits ______________________________ with electrons
(*like the ___________________!)

ATOMS will ___________ or _______________ ELECTRONS to obtain a ________ valence shell

**_____________________ DO NOT move!

This forms an ion: ______________________________

Because ions have ______________ numbers of protons and electrons, they are not __________

Ions have a positive OR negative ____________________________:


IF e- are lost:
IF e- are gained:

Now has more ____ than ____

Now has more ____ than ____

_________________ charged ion

_________________ charged ion

Called a _____________

Called an __________

Ex: Sodium

Ex: Oxygen
Summary of Ionic Charges
1
2
Atoms And Ions
In the top of each box, Use Lewis-Dot diagrams to draw each ATOM.
In the bottom of each box, use Lewis-Dot diagrams to represent the most common ION formed by each atom.
3
4
5
6
7
8
9
10
11
12
13
14
15
16
17
18
19
20
Questions:
1. What do you notice about the amount of electrons lost/gained in each group?
2. What do you notice about the ionic charge of each group?
3. Which atoms do not form ions?
Chapter 7: Chemical Compounds
Chemical Formulas of Compounds
Chemical Formula

Notation that tells the ___________ and ____________ of atoms in a compound
Rules for Writing and Reading Chemical Formulas:
1. The number ___ is never written. If there is no number, it’s a ___.
2. The # of atoms is written ________ the element symbol as a _____________________________
ie: H2O means __________________________________________
3. The # of molecules is written ________________ the formula.
ie: 3 H2O means _________________________________
4. If there are _______________, the subscript number applies to all atoms in __________________.
Examples
Compound
Number of
Formula
Molecules
Li2O
3 CO2
4 Al2(SO4)3
Element Symbols
Name of Element
Number of Atoms
of Each Element
How Atoms Combine
•
Atoms combine to become more ____________ and form ______________________
•
Noble gases are already stable because they have a _____________________________________,
so they do not __________________ with other elements.
•
Atoms without a full outer shell of electrons will combine with other atoms to obtain a _____________
_________________________.
•
There are 3 possible combinations that can occur:
1. Metal and Metal (Alloys)
•
Metals form ______________ with other metals to form __________________
•
Alloys are created by ___________________ two or more metals and then mixing these hot liquids.
•
These are not _____________________ because the atoms are not _________________________,
they are just metals mixed together.
•
Examples:
•
_______________ is an alloy of copper and zinc
•
_______________ is an alloy of gold, nickel, and palladium
•
___________________________ is an alloy of iron, nickel, and chromium
2. Metal and Nonmetal (Ionic Compounds)

A cation ( ) and an anion ( ) will be _____________ to each other to form an IONIC COMPOUND.

We can also think of this as ________________________ from the ________ to the _____________

Held together by ____________________
Naming Rules
1. Write the metal name
2. Write the non-metal name, but change the ending (last syllable) to “_______”
Ex:
NaCl =
BeS =
AlN =
Writing Chemical Formulas
Method 1: Diagrams

Use Lewis Dot Diagrams to show how IONIC BONDING occurs.
Rules
Examples
1. Draw each L-D diagram
Na and Cl
2. Use ________________ to show the direction
of e- movement
3. Transfer electrons until all atoms are
______________ 

K and S
If needed, add more atoms to obtain stability!
Method 2: Using Ionic Charges
Rules
Example
1. Write the SYMBOL for each element, metal then
non-metal.
2. Write the ionic CHARGES above each symbol
3. CRISS-CROSS the numbers to make subscripts

DO NOT write the + or –

DO NOT write the number 1
4. If necessary, REDUCE the subscripts to the
simplest ratio.
More examples:
a) Aluminum oxide
b) Magnesium sulfide
c) Lithium bromide
d) Potassium nitride
e) Calcium phosphide
f) Zinc oxide
Multivalent Compounds

Remember…some metals can have multiple valencies (charges).


Iron (

Copper (

Tin (

Lead (
): 2+ or 3+
): 1+ or 2+
): 2+ or 4+
): 2+ or 4+
Use a roman numeral _____________________ to indicate which charge the ion has.
Examples: FeCl2 =
FeCl3 =
Lead (IV) bromide
Lead (II) bromide
Tin (II) oxide
Tin (IV) oxide
Copper (I) nitride
3. Nonmetal + Nonmetal (Molecular Compounds)

Formed when ___________________________ join with other ________________________

Electrons are ___________________ between the non-metals
o
no charges or ions involved!

This sharing forms a ______________________________

There is no _________________________ of atoms; they can combine in many different ways.
o
Oxygen can form O2 (________________________) or O3 (________________).
o
These molecules act very _________________ from one another, even though their
formulas look _______________!
Two types of molecules:
1. Molecular Element

Contain atoms of the ________________________________

There are _______________ elements that are called __________________________________:


They do not naturally exist as _______ atom; they are always ____________!
Use the acronym ____________________ to remember these!
Naming Rules

Use their ___________________________________________________________
2. Molecular Compound

Contain of two or more ____________________________, like ___________________________

Use prefix rules for naming (see below)
Naming Rules

Many have common names
Water =

Ammonia =
Methane =
Hydrogen peroxide =
There are also standard rules that use numerical PREFIXES
Prefix
Using Prefixes
1. Write element names in same order as formula, change
ending to “______” (same as ionic)
2. Add _________ to tell the amount of each atom.
(Exception: *Do NOT use “________” before the _______ element)
Ex:
PCl3
C2Br
Writing Chemical Formulas
Method 1: Drawing Bonding Diagrams
Rules
Example
1. Draw each L-D diagram
N and F
2. Draw a circle around each pair of electrons that are
being shared
3. Continue adding bonds and/or atoms until all atoms
are full or “happy” 
Method 2: Use the Molecule Name
Rules
Example
1. Write the SYMBOL for each element, same order as in
Carbon dioxide
formula
2. The _________________ in the name become the
____________________ in the formula

Carbon monoxide
No ionic charges or criss-crossing needed!!
3. NO ______________________!
ie: N2O4 and NO2 are ____________________ molecules
Diphosphorus tetranitride
# of Atoms
Chapter 7 Summary
Metal and Nonmetal
Type of
Compound
Type of Bond
Electron
Behaviour
Composition
Nonmetal and
Nonmetal
Metal and Metal
Standard Gas Tests