Chapter 5
The Periodic Table
Section 5.1
• In 1750, only ____ elements were known.
• As the rate of discovery increased, so did the
_______________________the elements
• In 1789 _________________grouped the
known elements into _______, ___________,
________, and________.
Mendeleev’s Periodic Table
• Medeleev made ______________of the 63 known
elements. (1863)
– On each card he put the ______ of the element, _______, and
________________.
– When he lined the cards up in order of increasing mass, a
___________ emerged.
– Mendeleev arranged the elements into rows in order of
___________ mass so that elements with similar properties
were in the _______________.
A deck of cards can be divided into
four suits—diamonds, spades,
hearts, and clubs. In one version of
solitaire, a player must produce an
arrangement in which each suit is
ordered from ace to king. This
arrangement is a ________for
Mendeleev's __________________.
• Periodic Table- Arrangement of elements in ________, based on a set of
properties that _______ from row to row.
• Mendeleev’s Prediction
– He could not make ________table because many of the elements
had not yet been _____________. He had to leave ________ for
those elements.
• Eka-Aluminum – one space below ___. He predicted it would be a ___
metal with a_____m.p. and a density of 5.9 g/cm3
– The close match between Mendeleev’s __________ and the
_______ properties of new elements showed how ______ the
periodic table could be.
• ________ was discovered in 1875. It’s a _____ metal, m.p. is _____ ˚C, and
has a density of 5.91 g/cm3
____ from a person's hand
can melt gallium. In some
traffic signals, there are
tiny light emitting diodes
(LEDs) that contain a
compound of gallium
Mendeleev’s Periodic Table
• How is the table organized?
– Elements are arranged in order of __________
_______.
• What do the long dashes represent?
– They represent ______________ elements.
• Why are masses listed with some of the dashes,
but not with all of them?
– He was able to ____________________for
some unknown elements based on the
properties of neighboring elements.
5.2 The Modern Periodic Table
• The sounds of musical notes that are separated by
an octave are ______, but they are not ________. In
a similar way, elements in the ______ column of the
periodic table are _______because their properties
_______ at regular intervals. But elements in
different rows are ____ identical.
Periodic Law
• Mendeleev developed his chart before the _______ was
discovered.
• In the modern periodic table, elements are arranged by
increasing __________________. (# of _____________)
• ________- Each row in the table of elements is a period.
• ________- Each column on the periodic table is called a group.
• Properties of elements repeat in a ___________ way when
atomic numbers are used to arrange elements into groups.
– Members of a group have ________ chemical properties.
• This pattern of repeating properties is called ______________.
Periods
• Periods - the _____; represent _______ levels.
– Row 1 (energy level 1) ___ elements
– Row 2 and 3 (energy level 2) ___ elements
– Row 4 and 5 (energy level 3) ___ elements
– Row 6 and 7 (energy level 4) ___ elements
• The number of available __________
increases from energy level to energy level.
• Elements change from _____ to ___________
to ___________as you move from left to right
across the period.
Groups
• Groups/Families - the _____________.
• Atomic masses __________ from top to bottom.
• Members of a group have similar electron
________________ and therefore have similar
____________ properties.
• Tells how many valence electrons are in the last energy level
of an element.***
– Valence electrons increase from _______________ on
the periodic table.
– ________________– an electron that is in the highest
occupied energy level of an atom.
Valence Electrons
• A valence electron is an
electron that is in the
____________________
energy level of an atom.
• They play a key role in
____________________.
• The # of valence electrons
increases from ____ to
______.
• Elements in a group have
similar properties because
they have the _____
__________ of valence
electrons.
Group
1A
2A
3A
4A
5A
6A
7A
8A
Valence
Electrons
Valence Electrons
• Electron configuration is the arrangement of
____________ in an atom.
• The most stable electron configuration is one in
which the ___________ electron shell is
completely _____________.
• Atoms will ____ or ____ electrons in order to
achieve the most _______ electron configuration.
Atomic Mass
• ______________is the # protons plus the # neutrons.
– It is a value that depends on the distribution of an
element’s isotopes in nature and the masses of those
isotopes.
– All atoms of the same element _________have the same
atomic _____.
– Average atomic mass of an element is a
_______________of the masses of an elements isotopes.
– The unit for atomic mass is –_______
– The standard on which the atomic mass unit is based is the
mass of a __________________.
Average Atomic Mass
• _______________– some values are more
important that other values
– For isotopes, the one that occurs more in ______
contributes ____ to the average atomic mass.
Solving for Average Atomic Mass
• When solving,
–
–
–
–
Convert the % abundance to a ___________
________________ by its mass
________ the products together
EX:
• Chlorine-35
• Chlorine-37
You Try:
75.78%
24.22%
0.7578 X 34.969 = 26.4995
0.2422 X 36.966 = +8.9532
35.4527 amu
Isotope
Mass (amu)
% abundance
27X
27.977
92.23
28X
28.976
4.67
29X
29.974
3.10
Classes of Elements
• 1. Chemical symbols are ___________by solids,
liquids, and gases.
– The symbols for solids are _____. The symbols for
liquids are _____. The symbols for gases are ____.
• 2. Elements are divided into those that occur
___________ and those that do not
– The symbols for elements that don’t occur naturally
are ______
• 3. They are also classified by their ____________
properties.
– METALS, NONMETALS, METALLOIDS
– In the periodic table, metals are located on the _____,
nonmetals are on the _____, and metalloids are in
____________.
METALS
•
•
•
•
__________ of elements
good _____________ of heat and electricity
most are _________ at room temp. (except ___)
most are ___________ and ______ –ability to be
drawn into wires
• some are _________, some are not.
– Ex. _____
Magnesium and
aluminum are typical
metals
Ex. _____
Transition Metals
• The metals in groups 3-12 are called __________
________.
• They form a _____ between the two sides of the
table. They are well known for their ability to
form compounds with _____________________
A compound of erbium
(Er) and oxygen is used to
tint glass pink.
Nonmetals
•
•
•
•
•
properties are __________ of metals.
poor ____________
many are _________ at room temp.
the solids tend to be ___________
Some are very __________, some don’t react at
all.
– Ex. __is most reactive element. Ex. __ is not reactive.
Toothpaste contains a
compound that helps to
protect teeth from tooth
decay. The compound is
formed from the
nonmetal fluorine and
the metal sodium
Metalloids
• elements with ___________ that fall between those of
metals and nonmetals.
– Ex. A metalloid’s ability to conduct electricity can vary with
___________. Si and Ge are ___________ at low temps. and
_____________ at high temps.
• Variation Across a Period
– Across a period from left to right, the elements become _____
metallic.
From left to right across
Period 3, there are three
metals (Na, Mg, and Al),
one metalloid (Si), and
four nonmetals (P, S, Cl,
and Ar). Many light bulbs
are filled with argon gas.
5.3 Representative Groups
• “___” groups are #1-8
• The number of the group is equal to the number
of ______________________in an atom of that
element.
• Valence electrons- An electron that is in the
____________ occupied energy level of an atom.
• Elements in a group have similar properties
because they have the _____________of valence
electrons.
– (This is why___is grouped with metals)
Alkali Metals
• Group 1A
• Most _________ metals
– Reactivity _________ from the
top to the bottom.
– So reactive many are kept
under ___ to prevent reacting
with ______ or oxygen.
• ____ Valence Electron
• Found in nature only in a
______________.
• Form ____ions because they
will________give up 1
electron for stability.
Element
Symbol
Hyperlink
Lithium
Li
Sodium
Na
Potassium
K
Rubidium
Rb
Cesium
Cs
Francium
Fr
Alkaline Earth Metals
• Group 2A
• Have __ Valence Electrons
• ______ than the metals in
1A.
• Form ___Ions because
they easily give up 2
electrons for _______.
• __________ used in
photosynthesis within the
chlorophyll.
• ___________ used in
teeth and bone.
Element
Symbol
Hyperlink
Beryllium
Be
Magnesium
Mg
Calcium
Ca
Strontium
Sr
Barium
Ba
Radium
Ra
Boron Family
 Group 3A
 Have___Valence electrons
 Form ___Ions because they
easily give up 3 electrons
for ____________.
 1 metalloid (________)
 ___ metals
 Aluminum is the most
abundant metal in the
Earth’s __________.
 People are encouraged to
________ aluminum
because it doesn’t take
that much energy to do so.
Element
Symbol
Hyperlink
Boron
B
Aluminum
Al
Gallium
Ga
Indium
In
Thallium
Tl
Ununtrium
Uut
Carbon Family
 Group 4A
 Have ___ Valence Electrons
 Form +/- 4 Ions because it will
easily lose or gain 4 electrons for
stability. (Although often doesn’t
form ionic compounds)
 1 Nonmetal ________)
 ___ Metalloids
 ___ Metals
 Metallic nature _________ from
top to bottom.
 With the exception of water,
most of the compounds in your
body contain ________.
 Silicon is the second most
abundant metal in the earth’s
__________.
Element
Symbol
Hyperlink
Carbon
C
Silicon
Si
Germanium
Ge
Tin
Sn
Lead
Pb
Ununquadium Uuq
Nitrogen Family
• Group 5A
• Have ___ Valence
Electrons
• Forms ___Ions
because it will easily
gain 3 electrons for
__________.
• ___ nonmetals
• ___ metalloids
• ___ Metals
• Nitrogen and
Phosphorus are used
in _______________.
Element
Symbol
Hyperlink
Nitrogen
N
Phosphorus
P
Arsenic
As
Antimony
Sb
Bismuth
Bi
Ununpentium
Uup
Oxygen Family
 Group 6A
 Have ___ Valence Electrons
 Forms ___Ions because it will
easily gain 2 electrons for
____________.
 ___ nonmetals
 ___ metalloids
 ___ metal
 Oxygen is the most abundant
_________ in the Earth’s _____.
 _______ is another from of
oxygen. At _______ level it can
irritate your eyes and lungs. At
higher levels it absorbs harmful
radiation from the sun.
Element
Symbol
Hyperlink
Oxygen
O
Sulfur
S
Selenium
Se
Tellurium
Te
Polonium
Po
Ununhexium Uuh
Halogens
 Group 7A
Element
 Have ___ Valence electrons
 Form ___Ions because it will
easily gain 1 electron for
Fluorine
stability.
 Most reactive ___________ Chlorine
increase from bottom to top.
 Known as “______________” Bromine
 ___ nonmetals
Iodine
 1 Unknown
 ___________ is the most
Astatine
reactive.
 React easily with most
Ununspetium
__________.
Symbol
Hyperlink
F
Cl
Br
I
At
Uus
Noble Gases
• Group 8A
• ___ Valence Electrons
• Helium is the ________
with only ___ valence
electrons.
• Extremely __________ (Do
not form Ions)
• _______ and __________.
• Used in light bulbs.
• All are used in _____ lights
except argon.
• Have the most ________
electron configuration.
Element
Helium
Symbol
Hyperlin
k
He
Neon
Ne
Argon
Ar
Krypton
Kr
Xenon
Xe
Radon
Rn
Ununoctium
Uuo
Patterns on the Periodic Table
1.
2.
3.
4.
5.
6.
7.
8.
9.
Atomic # ________________________________.
Atomic mass ________________________.
Energy level and orbitals in rows from __________.
(Physical Properties) metals
metalloids
nonmetals from _____________.
Columns atomic mass from ________________.
Columns are based on chemical properties
(________________).
Valence Electrons from _____________.
Most reactive metals are on the _______side.
Most reactive non-metals are on the _________ side.