The Periodic Table Notesheet
Applied Chemistry
Name:
Date:
Period:
A. Elements
1. There are approximately _________ elements in the periodic table.
2. _________ elements occur naturally in nature.
3. Elements exist in the following three states of matter: ______________,
________________, and ______________.
4. Elements can be found in all matter, including ___________ things and the
____________________.
5. All elements can be located in the ____________________________.
B. Properties of Elements
1. Qualitative Properties: _______________________________________________
Examples: _________________________________________________________
2. Quantitative Properties: ______________________________________________
a. Melting Point – Temperature at which a ___________ changes to a ____________.
b. Boiling Point – Temperature at which a ____________ changes to a ____________.
c. Density – a measure of the amount of ___________ of an object divided by its
_______________. Units are
.
C. Types of Elements
1. Metals
a. Properties
-
At room temperature, all are solid except for _________________________
-
_____________ (A.K.A Shininess)
-
Good ____________________ of heat and electricity (A conductor allows heat and
electricity to pass through it.)
-
High ____________ (example: dumbbell)
-
___________ melting points
-
___________________: can be drawn out into thin wires
-
___________________: can be hammered into thin sheets
b. Metals are found on the ___________ side of the periodic table.
c. Metals make up most of the periodic table.
2. Nonmetals
a. Properties
-
At room temperature, they are ______________, _______________, or __________
-
No _______________.
-
_________________ of electricity and heat. (Insulators ___________ allow heat
and electricity to pass through them.)
-
________________, easy to break.
-
Neither malleable nor ductile.
-
Lower _______________ points and _____________ points than metals
b. Located on the _____________ side of the periodic table
3. Metalloids
a. Have properties of both ________________ and _______________________.
b.
There are _______ metalloids in the periodic table: _____________________,
____________________,____________________,____________________,
_____________________, __________________, &___________________,
c. Located _______________________________________________________
D. History of the Periodic Table
Periodic - ________________________________
1. Dobereiner (1829): found that some elements have similar _______________.

Grouped the elements in groups of three called ________________.
2. Newlands (1867): saw that the properties of elements repeat every _________________
element. This is called the ________________________________.
3. Mendeleev: developed the first ________________________________ in 1869.

Arranged the periodic table in order of increasing ________________________.

Predicted the properties of ____________elements and left blank spots in the periodic
table for these elements.
1st Periodic Law: the ________________________ of the elements recur at certain
intervals of ___________________________________.
4. Moseley (1911): reorganized the periodic table in order of increasing _________________.
Modern Periodic Law – the ___________________ of elements recur at certain intervals
of _________________________________.
“Properties are Periodic”
E. Organization of the Periodic Table
1. ______________: Horizontal Rows in the periodic table

There are ________ periods in the periodic table.

Elements in a period ______ ________ have similar properties.
2. _______________ or _______________: Vertical Columns in the periodic table

There are ________ groups in the periodic table.

Numbered from ____________________________.

Elements in the same group _________ similar properties. Why?
o Elements in the same group have the same number of ____________ electrons.

_________________ electrons are those electrons in the outer energy level.

The maximum number of valence electrons is ________.
3. Groups in the periodic table:
a. Hydrogen:
Group _______
________ valence electron
b. Alkali Metals: Group ______
________ valence electron

_________ reactive metals

As you go down the group, reactivity _______________.
c. Alkaline Earth Metals: Group ________
________ valence electrons

Very reactive
d. Boron Group: Group __________
________ valence electrons
e. Carbon Group: Group _________
________ valence electrons
f. Nitrogen Group: Group _________
________ valence electrons
g. Oxygen Group or __________________________: Group _________
________ valence electrons
h. Halogen Group: Group _________
_________ valence electrons

Used in ______________.

_____________ reactive nonmetals
i. Noble Gas Group: Group ________
________ valence electrons
Helium has _______ valence electrons.

Do not react with other elements: known as ______________

Have a complete outer shell of electrons known as a ____________
_______________ _______________.
“Everyone wants to be like the noble gas group.”
j. Transition Metals: Groups _____________
k. Inner Transition Elements: Bottom of the periodic table

_________________________ Series or Rare Earth Elements
o _______________________________

_________________________ Series
o _______________________________
l. Transuranium Elements:

These elements are _________________ elements.
Members of a group have ____________________ chemical properties, because they have
the same number of ____________________ electrons.
F. Trends in the Periodic Table
1. The most reactive metals are the ________________________.
a. Metals become _______________ reactive as you move down a family.
b. The most reactive metal is ________________________.
2. The most reactive nonmetals are the _____________________.
a. Nonmetals become _______________ reactive as you move down a family.
b. The most reactive nonmetal is ______________________.
3. Atomic Radii- the distance between the ______________ and the outermost
______________ in an atom. Unit = _____________
a. ____________________ as you go down a group.
b. ____________________ as you go left to right across a period.
Examples: Which has a larger atomic radius?
Potassium
or
Cesium
Silicon
or
Lead
Sodium
or
Chlorine
Lithium
or
Oxygen
4. Ionization Energy – the energy needed to _________ a valence electron from an atom.
Unit = ________________
a. _____________________ as you go left to right across a period.
b. _____________________ as you go down a group.
c. The ionization energy for the noble gases is very _____________ because they do
not want to give up any electrons.
d. The energy needed to remove each successive electron ____________________.
Examples: Which has a higher ionization energy?
Silicon
or
Chlorine
Sulfur
or
Tellurium
Lithium
or
Rubidium
Calcium
or
Bromine