Periodic Table Information
Chemistry
Mr. Treanor
List of Topics
Atomic Structure – protons, neutrons,
and electrons
 Physical and chemical properties
 Metals and non-metals
 Using the periodic table
 Group Properties
 Solid/liquid/gas
 Ionic/covalent/metallic bonds
 Valence electrons/ writing formulas

Atomic Structure – protons,
neutrons, and electrons
 Atomic
Mass = # of protons + # of
neutrons
 Protons and neutrons are in the
nucleus
 The electron cloud takes up nearly
ALL of the space in an atom
Physical and chemical
properties
 Physical
properties are the
things you can sense, like
shape, texture, color,
brittleness, luster
 Chemical properties are things
that cause chemical reactions
Physical and chemical
changes
Physical changes just change the shape
– the chemical stays the same – like
boiling or melting
 Chemical changes change the
chemicals (!!) – which means there are
different chemicals and you can’t get
the original ones back (usually).
 You can tell if it is a chemical change
because they make heat, light, drastic
color changes, solid forming, or fizzing

Metals and non-metals
 Metals
are shiny, bendable, good
conductors of heat and electricity,
hard, mostly solid
 Non metals are dull, brittle, poor
conductors of heat and electricity,
soft, often liquid or gas
Using the periodic table
Find the atomic number, atomic mass,
group number, number of
protons/electrons/neutrons in an
element
 Recognize the different groups that
have names: alkali (1), alkaline earth
(2), transition metals (3-12), halogens
(17), and noble gases (18) and know
the properties of these groups…

Group Properties
Alkali: most reactive metals, soft, always
in compounds
 Alkaline earth: second most reactive
metals
 Transition metals: the ones you think of as
metals, like iron, copper, gold, silver,
chromium, zinc, platinum, etc.
 Halogens: most reactive NON metals,
always in compounds, 2 are gases, 1 liquid,
2 solid
 Noble Gases: NOT reactive because they
have full outer shells of electrons

Solid/liquid/gas
 Solids
have a rigid structure;
atoms do not move around
 Liquids have a definite volume;
atoms move around but are always
touching
 Gases have no definite shape or
size; atoms move freely and do not
touch each other all the time
Ionic/covalent/metallic
bonds
 Ionic
bonds are caused by
transferring electrons; between a
metal and a nonmetal
 Covalent bonds are caused by
sharing electrons; between 2
nonmetals
 Metallic bonds are caused by free
electrons; between 2 metals
Valence electrons/ writing
formulas
 Valence
electrons are the outer
shell electrons available for
bonding
 In groups 1 or 2, the number is 1
or 2, respectively
 In groups 13 – 18, the number is
the Group number minus 10 (3-8)
Sodium
Oxygen
Symbol
(box 1)
Atomic number
(box 2)
Valence electrons
(box 3)
Gained or lost
(box 4)
Total electrons
(box 5)
Symbol for Ion
(box 6)
Element
Determining Ionic Charge
Na
O
11
8
1
6
-1
2
10
10
Na
O
+
-2
Writing formulas
Naming Binary Compounds
 The
first element keeps its name
 The second element gets an –ide
 NaCl
is Sodium Chloride
 MgO is Magnesium Oxide
Polyatomic Ions
Some Polyatomic Ions