Target Time
• An atom has 4 Protons, 4 Neutrons and 3
Electrons.
– What is this Element
– Is this an Isotope, Ion or Neutral Atom
– What is the symbol for this Element
– Draw the Bohr Model
The Periodic Table
Explore
Element Card
Element cards make up the periodic table
They show what one atom of the element
is made up of!
6
Chemical
Name
Atomic
Mass =
C
Carbon
12.0
Total mass of all
particles in atom
Atomic number =
# of protons and
# of electrons
Chemical
Symbol
To find the number of
neutrons, round the
atomic mass (mass
number) and subtract
the atomic number
So how is the Periodic Table
arranged?
• The Periodic Table is
organized like a big grid.
• The properties of an
element can be predicted
from its location in the
Periodic Table
• There are rows (left to
right) and columns (up
and down). Each row and
column mean something
different.
What do you notice about the Atomic Number of
Elements as you move Left to Right, Up to Down
on the Periodic Table of Elements?
The Atomic Mass
increases as you go left
and down
The Periodic Table can also be divided into three main
types of Elements: Metals, Metalloids, and Nonmetals
Metals make up the majority of the
table and are located on the left
Metals are shiny or lustrous
Most Metals are solid at room
temperature
Metals have high
conductivity
Metals can be flattened and not shatter
(malleable)
Metals can be pulled and stretched into
wires (ductile)
Most metals have high melting and
boiling points
Metals
• Nonmetals can be found on the
right side of the table
• Nonmetals are not shiny
• Nonmetals are mostly gaseous
at room temperature
• Generally have low melting and
boiling points
• Nonmetals are poor conductors
• Nonmetals are brittle and will
shatter easily
(not malleable or ductile)
Nonmetals
• Often described as being
located on the zig zag or the
staircase
• Metalloids have
characteristics between
metals and nonmetals
• Metalloids are solid at room
temperature
• Metalloids are semiconductors
Metalloids
Groups are Vertical Columns
Periods are Horizontal Row
 Each horizontal row of the
table is called
a period
 There are 7 period
 Each row represents the
number of energy levels
(or shells) present in the
electron cloud of an atom
of the element
 EX: The atom to the right
has 3 shells and would be
in row 3
Periods
 The Columns are called
Groups or families
 There are 18 groups
 The Elements in a group
have the same number
of electrons in their
OUTER energy level
 Groups are often
“grouped” together to
form Families because
of similar properties
Groups
(Families)
Now Lets Practice
• Pull out your Ions worksheet from yesterday
so we can review it
Groups and Valence Electrons
• You can tell a lot about an element based on its
position on the periodic table.
• The Group number for a column indicates how
many electrons are in the outer/valence shell of
that atom.
– Groups 1 and 2 – Same number of valence electrons as
the group number.
– Groups 3-12 – No rule/trick , you have to figure it out
– Groups 13-18 – Subtract 10 from the group number to
find the number of valence electrons.
Hydrogen
The properties of Hydrogen do not match the properties of any
single group, so it is set apart. It is above Group 1 because it
has 1 electron in its outer energy level like Group 1.
1: Alkali
Metals- only 1
electron in their
outer shell
making them the
most reactive
metals
• These react
strongly with water
• Easily forms bonds
with group 17
halogens
2: Alkaline-Earth Metals
Second most reactive, form bonds easily
with group 16
3-12: Transition Metals and Rare Earth Metals
Bonding and electron movement is more complicated.
Precious metals like gold, silver and copper are transition metals.
13: Boron Group- Metals and
Metalloids
Characterized by having 3 electrons in their valence shell
14: Carbon Group
Even though this group consists of nonmetals, metals and metalloids they
all still behave similarly when bonding due to four outer shell electrons
15: Nitrogen Group
5 outer shell electrons- Non-metals of the group are considered electron
accepters
16: Oxygen Group- 6 outer shell electrons.
Electron accepters.
17: Halogen Group- 7
outer shell electrons. Electron accepters.
18: Noble Gases- Have a stable outer shell full
Therefore these elements do not need or donate electrons. This makes
them non-reactive or inert.
Periodic Table and
States of Matter
Most Periodic Table models also indicate whether an element is a solid, liquid, or
gas. Look at the diagram below.
Reactivity of Elements
• Atoms will often take, give, or share electrons with
other atoms in order to have a complete set of
electrons in their outer energy level.
• Elements whose atoms undergo such processes are
called Reactive and can combine to form
compounds.
• Since “Groups” [columns] are similar because they
have the same number of electrons in their outer
energy level, the Periodic Table is also organized by
degree of reactivity.
Reactivity of Elements
Reactivity Increases
As you go down a group for metals.
As you go up a group for nonmetals.
Reactivity Decreases
As you go to the right for metals
As you go to the left for nonmetals.
Noble gases
are not
colored in
because they
do not react
with other
elements due
to the full
outer valence
shell of
electrons
Boiling and Melting Point
• There is not a specific trend, but there are
general rules regarding boiling and melting
point.
• Metals generally have high boiling and
melting points.
• Nonmetals generally have low boiling and
melting points
Elements
Matter made of one kind of atom.
f
118 elements are known or predicted
Classified in the Periodic Table
Written as symbols
Arranged by atomic #
Divided by properties
columns
rows
Metals
Nonmetals
families
periods
shiny
dull
conductors
Not conductors
malleable
brittle
Metalloids
Properties of both metals and nonmetals