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UNIT 2
Chemical Reactions
Chapter 4: Developing
Chemical Equations
Chapter 5:Classifying
Chemical Reactions
Chapter 6:Acids and
Bases
Chemistry Review
(Pages 134-135)
There are 32 elements that you will commonly use throughout the chemistry unit.
1.
2.
3.
4.
5.
6.
7.
8.
9.
10.
Hydrogen
Helium
Lithium
Beryllium
Boron
Carbon
Nitrogen
Oxygen
Fluorine
Neon
H
He
Li
Be
B
C
N
O
F
Ne
11.
12.
13.
14.
15.
16.
17.
18.
19.
20.
Sodium
Magnesium
Aluminum
Silicon
Phosphorus
Sulfur
Chlorine
Argon
Potassium
Calcium
Na
Mg
Al
Si
P
S
Cl
Ar
K
Ca
Metals
26. Iron
28. Nickel
29. Copper
30. Zinc
35. Bromine
47. Silver
50. Tin
53. Iodine
79. Gold
80. Mercury
82. Lead
92. Uranium
Fe
Ni
Cu
Zn
Br
Ag
Sn
I
Au
Hg
Pb
U
Copyright © 2010 McGraw-Hill Ryerson Ltd.
Chemistry Review
(Pages 134-135)
Click the “Start” button to review the formation of ions and ionic compounds.
Ions are charged
particles formed
after the loss or
gain of one or
more electrons.
Copyright © 2010 McGraw-Hill Ryerson Ltd.
Chemistry Review
Metals
(Pages 134-135)
The metals are:
• Good conductors of heat (used in pots and pans)
• Good conductors of electricity (used in wires)
• Lustrous (used in jewelry and other ornamental objects)
• Almost all are solids (except for mercury)
• Malleable (can be hammered into sheets)
• Ductile (can be drawn into wires)
Examples: Gold, Aluminum, Silver, Copper, and Sodium
Copyright © 2010 McGraw-Hill Ryerson Ltd.
Chemistry Review
Non-metals
(Pages 134-135)
The non-metals are:
• Poor conductors of heat (used as insulators in construction)
• Poor conductors of electricity (used to insulate wires)
• Non-lustrous (dull in appearance)
• Either solids, liquids, or gases (there are examples of each)
• Brittle in the solid state (break easily when hammered)
• Non-ductile (cannot be drawn into wires)
Examples: Phosphorus, Sulfur, Chlorine, and Neon
Copyright © 2010 McGraw-Hill Ryerson Ltd.
Chemistry Review
Metalloids
(Pages 134-135)
Metalloids have properties of both metals and non-metals.
The metalloids show the largest variance in properties of
any group in the periodic table. They can be metallic or
non-metallic, malleable or non-malleable. The most notable
members of this group are silicon and germanium, which
have brought about revolutionary changes in the
semiconductor industry. (Semiconductors normally will not
conduct electricity but can be induced to do so at elevated
temperatures or when they are mixed with trace amounts of
other elements.)
Examples: Boron, Silicon, Arsenic,
and Antimony
Copyright © 2010 McGraw-Hill Ryerson Ltd.
Chemistry Review
(Pages 134-135)
Let’s review the use of the periodic table of the elements and how
to read the information found within it.
Ion Charges
Atomic Number
Element Symbol
Element Name
Atomic Mass
Copyright © 2010 McGraw-Hill Ryerson Ltd.
Anatomy of an Atom
•
The outermost shell is called the
valence shell. The electrons in the
valence shell are called valence
electrons.
•
The atoms of elements in Period 1 have
one shell. This shell contains a
maximum of 2 electrons.
•
The atoms of elements in Period 2 have
two shells. The valence shell contains a
maximum of 8 electrons.
•
The atoms of elements in Period 3 have
three shells. The valence shell contains
a maximum of 8 electrons.
Electron shells are fixed regions around
the nucleus where the electrons orbit.
electrons
The nucleus of the atom is a region
where protons and neutrons are found.
Recall:
• The atomic number represents the
number of protons in the nucleus of an
atom.
•
The number of electrons is equal to the
number of protons.
Worksheets– Practice with Electron Shells
Take the next 10 minutes to complete the worksheet called
“Electron shells for the first 20 elements in the periodic table”.
When you are done the first worksheet, complete “Electron
Shells”.
Patterns and Trends in The Periodic Table
•
Atoms join together with bonds (a chemical joining) to form molecules. e.g. H and
O join chemically to form H2O
•
The physical and chemical properties of individual atoms are different from those of
the compounds they form. ie. H and O have different properties than H2O
•
Understanding how the periodic table is arranged can predict how elements join
together. For example Na and Cl join to form a new compound with the formula
NaCl.
Group 1
Period 1
Period 2
Period 3
Group 18
The “staircase”
line separates the
elements into
metals and nonmetals.
Using Electron Dot Diagrams to Represent
Valence Shell Electrons
•
A simple model called an electron dot diagram (or Lewis
Diagram) is used to represent an atom and its valence
electrons.
•
The symbol of the element is used to replace the nucleus and
the inner shell electrons.
•
The electrons from the valence shell are shown as dots placed
around the symbol.
Examples: