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Classifying Matter

An Introduction to the Periodic Table
During the mid 1800’s, Russian scientist ________________ invented the modern
periodic table after noticing a relationship between the ________ and ________
_____________ of the elements
...
At the time approximately ____ elements had been identified
...


Mixture

Metals are located on the _____________ and throughout the _________ of the
Periodic Table
...
All metals are ____ except for _______ (Hg), which is a _______
...
Non-metals
are _____, not _____, not very ____ and ___ conductors of ____ and ________
...

A division line known as the “_________” separates metals and non-metals
...


Physical and Chemical Changes in Matter

The name for each ____________ row of the Periodic Table is a _______
...


Physical Change –

Chemical Change –

The ________ columns in the periodic table are called _____ and range from 1-18
(these are typically written as Roman Numerals)
...

There are four families within the periodic table:

Five Clues that a Chemical Change has occurred:
1
...

3
...

5
...


54
Xe

25
26
Mn
Fe

27
Co

28
Ni

29
Cu

30
Zn

47
Ag
79
Au

50
Sn
80
Hg

82
Pb

86
Rn

An atom is the smallest particle of an element that still retains the ___________ and
______________ of the element
...
These _________ particles are _______,

__________ and ___________
...
Electrons are so ______ and _______ that they essentially contribute
no overall weight to the atom
...
Both protons and neutrons have a mass of _____
...


Examples:

Number of neutrons =

Examples:

17

7

18

Cl

Isotopes are atoms of an element that have the same number of ___________ in their nucleus,
but a different number of ___________
...


Example:

“Light” Lithium

“Heavy” Lithium

Ar

35
...
The atomic weight represents a “______________” of all the
__________ for a particular atom
...
01

39
...
In this model, the
nucleus, containing the ________ and _________, takes the central place just like the Sun takes the central place
in our solar system
...
The orbits represent the different amounts of _____ that the _______ can have
...
The first orbit holds up to
__ electrons
...
As you fill the orbits, always fill the _______
energy orbit first, then fill up the next one and the next and so on
...
Since electrons
have a _______ charge, and according the law of ____________, ________ charged particles ________ and
____ charges _____; you must place the first ____ electrons in the orbit as far apart as possible
...

Step 1: Determine the number of protons

Observations
To notice with your ______
...

Example:

The street is wet (_____________)
...


Types of Observations

Qualitative Observations:

This is equal to the atomic number of the element
Step 2: Determine the number of electrons
This is equal to the number of protons
...
For example: colour,
taste, texture etc…

DOES NOT INVOLVE NUMBERS!

Step 3: Determine the number of neutrons
...

Step 4: Draw a nucleus and write in the number of protons and neutrons
...
Always fill
the inner shells to their maximum before moving to the outer shells
...
For example: how fast,
how hot, how much etc…

ALWAYS INVOLVE THE USE OF NUMBERS!

Lewis (Electron) Dot Diagrams
Lewis Dot Diagrams are a short way to show the ____ energy shell (______) shell for an atom
...

The element ________ is used to represent, the _____, ______ and all ___________
...
The remaining four electrons (if present) can then be paired up
...
The
following is a list of some physical properties of matter that help us tell one thing from another
...
Chemical bonds are ______ that ________ atoms to each other
...

While there are only ___ naturally occurring elements, there are ___________ of different
compounds
...


Odourless, spicy, sharp, flowery
Ionic Bond
Sweet, sour, salty, bitter
1
...
Cloudy (translucent)
3
...
It usually involves a ________ and a ___________
...
Crystalline (regular shape, ex
...
Amorphous (irregular shape, ex
...
It usually involves two
_____________
...

Syrup is viscous water is not
...
To do this, an atom
will either ____________ to become an _____ or _____________ to become a ______
...
Anions and cations will
________ to one another, forming an _________
...


The chemical formula has different meanings depending on the type of _____
holding the compound together
...
The chemical
formula of a covalent compound represents exactly
_________ of each type of _____ are found in each
individual molecule
...


Ionic Compounds – Ionic compound form _________ and make a ________
structure
...
Ionic
compounds are always _________________________
...


When writing chemical formula, they are typically written such that the element
found furthest to the ______ on the Periodic Table is written first
...
Therefore, ionic compounds
form when a _____ and a ________ combine
...
This is why all ionic compounds appear as ________________
...
Electricity is the movement of _________________ particles
...
When _______ or _________ in water, the ions will split apart
from each other (_________) and are then free to move around
...


The following is how you can draw atoms exchanging their electrons to become ions and therefore
form an ionic bond and thus becoming stable
...


Magnesium
and Oxygen

Which of the following metals is more reactive – lithium, sodium or potassium? Can you suggest
why?

Beryllium
and fluorine

Do you think the non-metals will follow the same pattern? For example, fluorine, chlorine and
bromine? Can you suggest why?

Aluminium
and Sulphur

EDD

EDD

Formation of Bond
(Movement of
Electrons)

Ions
formed

Chemical
Formula

Covalent Compounds
Covalent compounds typically form when two or more ___________ bond together
...
Atoms can share ________ of electrons, creating a ______ bond; __________ of
electrons, creating a _______ bond; or ________ of electrons resulting is a _________ bond
...


The following is how you can draw atoms sharing their electrons to form covalent compounds
...
There are only seven such elements that occur naturally; they are called
____________ molecules: _________________________________
Covalent compounds come in a variety of ______, solid, liquid and gas, and seem to have a wide
range of ________ when compared to ionic compounds
...
These variations within molecules
create the differences we see in covalent compounds
...
The atoms that make-up covalent molecules do not _______ __________ when they
melt or boil, but rather remain as _____________
...


Nitrogen and
Fluorine

Carbon and
Bromine

Atom
EDD

Atom
EDD

Compound EDD

Structural
Diagram

Chemical Reactions

Balancing Equations

A chemical reaction can be written in a number of different forms:

All chemical equations must be balanced so that they are consistent with the Law of Conservation of Mass
...
When balancing equations, always start with the “ugliest” molecule first (polyatomics)
...
To balance, place the desired number (coefficient) in from of the element or compound
...

3
...


Example:

4
...

Word Equation
The elements and compounds that are reacting are written first followed by the products
...


Example:

5
...


Examples:

Skeleton Equation
The Law of Conservation of Mass states that matter cannot be __________ or __________; it can only be
___________ from one form to another
...

A skeleton equation is an unbalanced equation that ______ follow the Conservation of Mass
...


Example:
H2 (g) + Cl2 (g) → HCl (g)
On the reactant side there is a total of __ atoms (__ hydrogen and __ chlorine)
On the product side there is a total of __ atoms (__ hydrogen and __ chlorine)

____ Mg (s) + ____ O2 (g) → ____ MgO (s)
Atoms
Mg
O

Example:
On the reactant side there is a total of __ atoms (__ hydrogen and __ chlorine)
On the product side there is a total of __ atoms (__ hydrogen and __ chlorine)
When there is a coefficient of “__”, it is typically not written:

H2 (g) + Cl2 (g) → 2HCl (g)

Products

____ H2 (g) + ____ O2 (g) → ____ H2O (g)
Atoms
H
O

Reactants

Products

____ Fe (s) + ____ O2 (g) → ____ Fe2O3 (s)

Balanced Chemical Equation
An equation that follows the Law of Conservation of Mass
...
In most chemical equations, numbers placed in front of the elements or compounds
(________________) are required to balance the equation
...
For example, think of appropriate storage
of chemicals…

____ Pb(NO3)2 (aq) + ____ BF3 (s) → ____ B(NO3)3 (aq) + ____ PbF2 (s)
Atoms
Pb
NO3
B
F

Reactants

Why are some chemicals stored in dark glass jars?

Products

Why is it inappropriate to store propane tanks in areas that are not airconditioned?

Sometimes to balance an equation, fractions must be used
...
To get rid of the fraction, multiply every element or compound
in the equation by the denominator of the fraction (i
...
If you use ½ as a coefficient, then multiply by 2)
...
Synthesis
A synthesis reaction occurs when 2 or more ____________ combine to form a new
_______________ or __________________
...
To balance the equation, you must first convert the elements and/or compounds into their correct
chemical formula
...
Be careful, and make sure to always check your work
...


e) Metallic oxides react with water to produce a base

2
...


For example, explain why the two above reactions occur but the following reaction
does not?

The general equation for a decomposition reaction is: C → A + B

Example:

In order to determine if an element will displace another element in a single
displacement reaction you must refer to an _______________________
...


Typically, some form of ___________ or type of ____________ is needed to
initiate a decomposition reaction
...


3
...
This can occur in 2 ways, a _____ can
replace a __________ or a ____________ can replace a ___________
...
To
determine who can bump out whom, you must refer to the _____________
__________________
...
Double Displacement Reactions

Rates of Reactions and Energy Changes
Rates of Reactions
The rate of reactions is defined as the
...

The general equation for a double displacement reaction is:

In the general equation above, A and C are ______ (written first) and B and D are
___________
...
Since water is a clear, colourless, liquid, it typically
cannot be seen by looking at the reaction
...


Rates of reactions can be explained using the ____________
...
If there are a higher number of collisions in a system,
more combinations of molecules will occur
...

Reactions happen, no matter what
...
The reactions happen over and over but not always at the same speed
...

Concentration: If there is ________________ in a
system, _________________________________
_________ and speed up the rate of the reaction
...

Temperature: When you __________________ of a
system, the molecules bounce around a lot more (an ______________________)
...
That fact means they are
also more likely to combine
...
That temperature drop lowers the rate of the reaction
...
When
you __________________, the molecules have ___________________________
...
When you
_______ __________ atoms and/or molecules __________ and don't hit each other as
often
...

Surface Area: When you ________________________________________________
________, you are increasing the number of atoms/molecules that are able to
________
...


An example of this is can be seen when comparing a pack of sugar versus a sugar cube
placed in water
...
With a sugar cube, only the outer layer of sugar is in
contact with the water and therefore capable of reacting
...
Catalysts lower the energy required
(____________________) required to break the bonds that hold substances together
...


Acids and Bases
An acid is a substance that produces __________ in solution, __

(aq)
...


Energy Changes and Chemical Reactions

i) When sodium hydroxide, NaOH is placed in solution it dissociates into _______

All chemical reactions involve the ________________________
...


ii) When calcium hydroxide, Ca(OH)2 is placed in solution it dissociates into ______

You can classify reactions on the basis of whether they release or absorb more energy
...
Examples include the burning
of fossil fuels and the rusting of iron
...
________________ reactions are called
___________
...


Identify the following as exothermic or endothermic:
Ice melting - ___________________________
A match burning - __________________________
Frying an egg - _________________________
Mixing acids with water will cause a rise in temperature - __________________
Hydrogen gas and chlorine gas will explode when exposed to UV light - _________

Indicators

Strength of Acids and Bases

Most solutions of acids or bases are ____ and ________
...
The simplest way to
distinguish them from water is to use an indicator
...


Strong acid –
HCl(aq) → H+(aq) + Cl-(aq)
When hydrogen chloride molecules enter an aqueous solution, 100% of the hydrogen
chloride molecules dissociate
...
There are also a number of ________ indicators
...


Weak acid –

Concentration of Acids and Bases (pH)

Example:

Concentration is defined as the amount of _______ per quantity of __________
...
___________ is the universal solvent
...

pH stands for, “the power of hydrogen”
...
The pH scale ranges from _________
...

Notice that the arrow used in the dissociation of a weak acid points in both
directions
...
The products of the
reaction will also react to produce the original reactants
...

A change in pH from 3 to 8 is a(n) _____________ increase/decrease in [H+]
A change in pH from 11 to 2 is a(n) _____________ increase/decrease in [H+]

Neutralization Reactions
Neutralization occurs when _________________ (base) and ___________ (acid)
are mixed to make ______ and a ________
...
The general word equation for a neutralization is:

Examples:
Aqueous solutions of hydrobromic acid and beryllium hydroxide undergo a
neutralization reaction to produce water and beryllium bromide

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