Name ________________________________
Periodic Table
Period ___ Date ___/___/___
PROPERTIES & TRENDS
Classifying the Elements:
The elements can be classified in two ways:
 Metals, non-metals, and semi-metals
 Chemical families (groups)
Metals are good __________________ of heat and
electricity. They are ______ and lustrous. They
are ___________ which means they can be
pounded into thin sheets. They are _________
which means they can be drawn into wires.
Metals have low ___________________ which means
that they do not hold onto their valence electrons
tightly. In their compounds they form ions with
___ charge.
Nonmetals are poor ____________________ of heat
and electricity. An important exception is pure
carbon in the form of ___________. Unlike
metals, as solids they are ___________ when hit
with a hammer.
All of the diatomic elements are nonmetals. Note that
___ is a nonmetal even though it is located with
the metals on the periodic table. Use the Gen-UIne Rule to identify the 7 elements that form
diatomic molecules.
____ ____ ____ ____ _____ ____ _____
Nonmetals have high ___________________ and
tightly hold onto their valence electrons. In their
compounds the nonmetals form ions with a ___
charge.
Semi-metals (metalloids) have properties that are in
between metals and nonmetals. They are
important in the semiconductor and computer
industries. The semimetals are: __ __ __ __ __
__ __.
Sketch the location of the semi-metals (metalloids),
metals, nonmetals and noble gases:
Properties of the Families:
Alkali Metals (1): __ __ __ __ __ __
 In their compounds they always form __ ions.
 They react with _____ to form H2(g) and OH ions.
Example: Na +

 Their chemistry involves _________ (gaining/losing)
one electron. They have one _________ electron.
 They are ______ metals and can be cut with a knife.
 They are never found uncombined in nature because
they are so reactive.
 They are stored _________ _______.
Alkaline Earth Metals (2): __ __ __ __ __ __
 In their compounds they always form __ ions.
 They slowly react with _____ to form H2(g) and
OH ions. Example: Ca +

 Their chemistry involves _________ (gaining/losing)
two electrons. They have two ________ electrons.
 __ is a component of bones and teeth.
Noble Gases (18): __ __ __ __ __ __
 These elements do not easily combine with other
elements. They are odorless, colorless and therefore
were difficult to discover.
 When air is cooled, O2 liquefies first at -182C. N2
liquefies at -195C. About 1% of the air is still gas
composed of the noble gas ________, __.
 One noble gas is radioactive and seeps up through
basement floors and walls. It is ________, __.
 One noble gas is best known for its orange color in
gas discharge tubes. It is used for signs that bear its
name. It is _______, __.
Halogens (17): __ __ __ __ (__)
 In their compounds they always form __ ions.
 They have ___ valence electrons.
 They react with ________ to form salts which gives
them their name of “salt formers.”
Example: 2 Na + Cl2 
 Their chemistry involves _________ (gaining/losing)
one electron.
 All of the members of this family are _________.
(We assume At2 would exist if there were any.)
 Halogens are very _______________. The element
on the table with the greatest attraction for electrons
is ___________, ___ (4.0).
Hydrogen, H
 Hydrogen is its own family.
 It usually forms ___ ions.
 It can combine with halogens.
Example: H2 + Cl2 
 In this case, H ______ (gains/loses) one electron.
 Hydrogen has ___ valence electron.
 H is located with the _________ ________ family.
 It has one less electron than the noble gas, ___.
 It can combine with alkali and other metals.
Example: 2Li + H2 
 In this case, H ______ (gains/loses) one electron.
 In this case, H has a ___ charge (oxidation #).
 It is diatomic like the __________ family.
Trends in the Periodic Table:
Size of the Elements:
(Sketch the trend in size)
The size of the atom is due to the size of the
___________ ___________. The two forces at
play are __________ between the electrons and
other electrons and ____________ between the
electrons and protons in the nucleus.
Left to right across the table, the atoms get _________
because there are more and more _________ in
the nucleus pulling on the valence electrons. In
any period, the valence electrons are on the same
level (floor).
Going down any group or family, the atoms get
___________ because there are more and more
__________ of electrons. Each level of electrons
is ____________ from the nucleus.
Ionization Energy (IE)
This is defined as the energy needed to remove an
electron from an atom.
Example: Na + NRG  Na+ + e
It is _________ (easier/harder) to remove an electron
from a larger atom. This is because the electron
is _________ (closer/farther) from the nucleus
and feels _______ (less/more) attraction.
(Sketch the trend in ionization energy)
Sizes of Ions:
Each time an electron is removed, the atom/ion
becomes __________ (smaller/larger) because
there is ________ (more/less) e- e repulsion.
So… each successive electron removed has a
___________ (higher/lower) ionization energy.
(Atoms that gain electrons become ___________.)
After all the valence electrons are removed, the next
electron is much __________ (closer to/farther
from) the nucleus and is much more difficult to
remove. There is a big jump in Ionization NRG.
ION Formation: each group on the periodic table will
normally gain or lose a certain number of
electrons to become an ion, Label the periodic
table below with the charges usually found on the
ions formed for each group (leave out the
transition metals)
+1
TAKS PRACTICE QUESTIONS:
1)According to the periodic table, which element most
readily accepts electrons?
A Fluorine
C Arsenic
B Nitrogen
D Aluminum
2)An unidentified element has many of the same
physical and chemical properties as
magnesium and strontium but has a lower atomic
mass than either of these elements.
What is the most likely identity of this element?
F Sodium
G Beryllium
H Calcium
J Rubidium
8) In which model of the periodic table does the
shaded area show the location of elements
that require the least energy to lose one electron?
3) The elements from which of the following
groups are most likely to react with
potassium (K)?
F Group 2
G Group 7
H Group 13
J Group 17
4) The elements of which of these groups on the
periodic table are most resistant to forming
compounds?
A Group 1
B Group 9
C Group 14
D Group 18
5) The table shows the atomic radii of some
elements in Periods 1 through 4 of the periodic
table. Which inference can be made from this
information?
F Atomic radii decrease from left to right.
G Atomic radii increase from bottom to top.
H Atomic radii decrease from right to left.
J Atomic radii double from top to bottom.
6) Which of these elements is most likely to
donate one electron?
F Be
G Cs
H Rn
J He
7) A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is a form
of the element —
A silicon
B carbon
C magnesium
D calcium
9) According to the periodic table, which of these
elements will form an ion with a –2 charge?
FS
G Mg
HF
J Rb
10) Calcium ions play an important role in the
function of neurons in the brain. Elements
that are chemically similar to calcium can
interfere with the function of neurons. Which
of the following is most likely to imitate
calcium’s role in the function of neurons?
F Sodium
G Potassium
H Strontium
J Rubidium