Organizing the Elements: The Periodic Table (PT)
Development of the Periodic Table
from Steven Hawkings’ Universe: Cosmic Alchemy
a) As you view the video segment on the periodic table, jot down the answers to
the following questions. Short answers only.
1) Where and when was Mendeleev born? _____________________________
__________________________________________________________________
2) What sparked Mendeleev interest in chemistry?____________________________
__________________________________________________________________
3) What properties of the elements did Mendeleev list before he began to organize the
elements?
__________________________________________________________________
4) Explain the process Mendeleev used to help design the first periodic table.
__________________________________________________________________
5) How was Mendeleev able to predict properties of the yet to be discovered elements?
__________________________________________________________________
6) How is the modern Periodic Table organized? ______________________________
__________________________________________________________________
b) Overview of the Periodic Table
 Developed by Russian scientist Dimitri Mendeleev (1869)
 Revised based on the work of Henry Mosley (1913) and Glenn Seaborg (1940’s)
 Revised or Modern Periodic Law: The properties of the elements are periodic function of
their ATOMIC NUMBER. This means that the
o Elements are arranged by INCREASING atomic number.
o Predictable & repeating pattern to the elements’ properties (characteristics)
o Elements in the same horizontal row (PERIOD) have the same number of energy
levels (where the electrons are found). The PERIOD Number on the side of the PT
is the same as the number of energy levels.
 Period 1: ______ energy level
 Period 4: ______ energy levels
o Elements in the same vertical column (GROUP) have similar chemical properties due
to the same number of electrons in outermost energy level. In the electron
1
configuration, the number of electrons in the outermost energy level is the number
on the right in the configuration for the groups (exception: He in group 18)
 Group 1: _____ electron in the outermost energy level
 Group 2: _____ electrons in the outermost energy level
 Group 14: _____ electrons in the outermost energy level
 Group 17: _____ electrons in the outermost energy level
 Four Basic types of Elements:
1
2
3
4
5
6
7
1 H
8
9
10
11
12
13
14
15
16
17
18
He
2 Li
Be
B
C
N
O
F
Ne
3 Na
Mg
Al
Si
P
S
Cl
Ar
4 K
Ca
Sc
5 Rb
Sr
Y
6 Cs
Ba
7 Fr
Ra
La
Lu
Ac
Lr
Ti
V
Cr
Mn
Fe
Co
Ni
Cu
Zn
Ga
Ge
As
Se
Br
Kr
Zr
Nb
Mo
Tc
Ru
Rh
Pd
Ag
Cd
In
Sn
Sb
Te
I
Xe
Hf
Ta
W
Re
Os
Ir
Pt
Au
Hg
Tl
Pb
Bi
Po
At
Rn
Rf
Db
Sg
Bh
Hs
Mt
Key: Each type of element has certain properties associated with it.
Metal
Metalloid
Nonmetal
Noble gas
The most active metal and nonmetal on the PT are the two F’s in opposite corners! ___&___
Special Names of Groups on the Periodic Table:
Group 1: __________________________________
Group 2: __________________________________
(2 names= group 2)
Groups 1& 2 are so active/ reactive (unstable), these elements are always found in
compounds and never alone.
Groups 3- 11 ________________________________
Solutions of compounds containing these elements are usually colorful.
 CuSO4 (aq) : ___________________________

CoCl2 (aq) : ____________________________
Group 17: __________________________________ Has elements which are found
in all three phases of matter, (s, l & g)
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Group 18: __________________________________ Very stable (non-reactive,
inert) due to having 8 electrons in outermost energy level except for Helium (He),
which has 2 electrons.
c) Color Coding the PT on your Reference Tables- use your notes and the PTs around the
room to help you
1) On the left side, copy the following to remind yourself that vertical columns are called
GROUPS and horizontal rows are called PERIODS:
G
P E R I O D
O
U
P
2) Using a brown pencil, color lightly the elements, which are liquids.
3) Using a yellow pencil, color lightly the elements, which are gases.
4) Using an orange pencil, add two stripes to the Noble gases to remind yourself that they are
found alone as MONATOMIC molecules.
5) Using a purple pencil, color over lightly the elements’ symbols, which always come in pairs, The
“BrINClHOF” or “GEN-INE”. You should be able to still see the symbol!
6) Using a green pencil, lightly color the metalloids. Remember Al and Po are metals and NOT
metalloids. Metalloids touch one full side along the dark “crack” on the right side of the PT.
7) Using a red pencil, lightly color groups 1 & 2 to remind yourself that these elements are so
reactive that they are never found alone in nature, only in compounds.
8) Using a blue pencil, lightly color groups 3 to 11, the TRANSITION ELEMENTS/METALS, to
remind you, that these elements often form colorful compounds and solutions.
9) Using an arrow to help, label the groups 1, 2, 17 & 18 with their special names.
10) Use a bracket ( { ) to help label groups 3 & 11, the TRANSITION ELEMENTS/ METALS.
11) At the top of the PT, label the LEFT side METALS and the RIGHT side NONMETALS.
12) Under Groups #1, #2, #13, #14, #15, #16, #17 & #18 draw the electron dot diagram, using
“X” to represent the kernel. (Remember elements in the same vertical group have the same
number of valence electrons so they have the same electron dot diagram. They will also have
similar chemical properties because of the valence electrons)
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d) Properties of Element Types
Element Type
Physical Properties
Chemical Properties
Metal
- Malleable (aluminum foil)
- Ductile (copper wire)
- Luster (aluminized glass = a mirror!)
- Excellent conductors of heat and
electricity (wires + toasters)
- Large atomic radius (big atoms)
- Phase @ 25oC: ___________
except: ________________
- Silver in color except for:
- Low electronegativity
- Lose electrons when forming bonds
- Form + charged ions (called
CATIONS)
- Low ionization energy
- Tend to tarnish or rust or form a
patina (oxide coating) in the presence
of oxygen
- Group 1 and 2 metals react violently
with water
- High electronegativity
- Gain electrons when forming bonds
with metals to form ionic bonds
- Form – charged ions (called
ANIONS)
- Share electrons with other
nonmetals to form covalent bonds
- Form molecules when bonded to
other nonmetals
- Group 17 nonmetals (halogens) are
extremely corrosive
- High ionization energy
Side of PT:
__________
about 2/3 of all
elements
Nonmetal
Side of PT:
__________
about 1/3 of all
elements
MetalloidFound along the
crack in the PT,
except for Al &
Po (dog food),
which are metals
a full side must
touch the crack
Noble GasGroup 18
- Brittle (sulfur can be crushed to a
powder)
- Dull (don’t reflect light well)
- Poor conductors of heat and
electricity (except for certain forms
of carbon)
- Small atomic radius (small atoms)
- Phase @ 25oC: ___________
_______________________
Only Liquid: ______________
Gases:
- Come in a variety of colors &
colorless
- Sometimes conduct electricity
(semiconductors)
- Used to make computer microchips
- Some have Luster (like metals)
- Brittle (like nonmetals)
- Photovoltaic (produce electricity
from light)
- Used to make solar energy panels
- Phase @ 25oC: ___________
- Low boiling points
- All gases at room temperature
- Poor conductors of heat and
electricity
- Gain electrons from metals
- Lose electrons to nonmetals
- Completely chemically nonreactive
- No electronegativity (no bonds
form)
- Extremely high ionization energy
Metallic and Nonmetallic Character
1) Metallic Character: metals lose electrons due to low ionization energy. The element with the
least ionization energy (Fr) is the most metallic, because it will lose electrons more easily than
any other metal. When comparing metals, the lower the ionization energy, the more metallic
character the element has. You can find ionization energy values on Reference Table S.
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Example: Ca has an ionization energy of 590 kJ/mol, and K has an ionization energy of 419
kJ/mol. If you heat both metals up, K will lose its electron first, as it requires less energy. K has
more metallic character than Ca.
Note: The total quantity of Francium on this planet (Earth) has been estimated to be just enough
to fit inside a small pen cap. Being so rare, we will not be using Fr during this course for any
other reason than as the most metallic element.
2) Nonmetallic Character: nonmetals tend to gain electrons due to high electronegativity. The
element with the highest electronegativity (F) is the most nonmetallic, because it will gain
electrons more easily than any other nonmetal. When comparing nonmetals, the higher the
electronegativity, the more nonmetallic character the element has. You can find
electronegativity values on Reference Table S.
Example: O has an electronegativity of 3.5 and Cl has an electronegativity of 3.2. Since O has a
greater attraction to electrons than Cl does, it is more likely to gain electrons from a metal than
Cl is. O has greater nonmetallic character than Cl.
e) Common Element Names and Symbols (based on Reference Table S)
Symbol
Name
Significance/Use
Symbol Name
Significance/Use
H
Hydrogen
Co
Cobalt
Magnetic alloys
He
Li
C
Helium
Lithium
Carbon
Lightest element,
flammable
Balloons, radioactivity
Battery technology
Life, plastics, energy
Ni
Cu
Zn
Nickel
Copper
Zinc
N
O
F
Nitrogen
Oxygen
Fluorine
Br
Kr
Ag
Bromine
Krypton
Silver
Ne
Na
Neon
Sodium
Sn
I
Tin
Iodine
Alloys, toxic heavy metal
Disinfectant
Mg
Al
Magnesium
Aluminum
Xe
Ba
Xenon
Barium
Flashbulbs
Radiocontrast for X-rays
Si
P
Silicon
Phosphorous
Life, atmosphere
Life, atmosphere, oxides
Most nonmetallic
element
Advertising signs
Explosive metal, makes
salt
Lightweight metal, flares
Structural lightweight
metal
Microchip technology
Life, incendiary devices
Coins, alloys
Wires, pipes, alloys
Galvanized steel,
batteries
Cleaning properties
Headlamps
Jewelry, alloys
W
Au
Tungsten
Gold
S
Cl
Ar
K
Sulfur
Chlorine
Argon
Potassium
Hg
Pb
Fr
Rn
Mercury
Lead
Francium
Radon
Ca
Calcium
U
Uranium
Nuclear reactor fuel
Fe
Iron
Matches, gunpowder
Cleaning properties
Gas in windows
Nutrition, explosive
metal
Bones, minerals
(limestone)
Structural metal, rusts
Light bulb filaments
Jewelry, conductor,
alloys
Amalgams, thermostats
X-ray blankets, toxic
Most metallic element
Carcinogenic gas
Am
Americium Used in smoke detectors
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f) Important Definitions to Know for Periodic Table Unit
PERIODIC TABLE: PROPERTIES OF ELEMENTS and TRENDS
Electronegativity: ________________________________________________
_____________________________________________________________
- found on Reference Table S
- For Metals (left side of PT) it tends to be _______
- For Nonmetals (right side of PT) it tends to be ______
Ionization Energy: _______________________________________________
_____________________________________________________________
- found on Reference Table S
- For Metals (left side of PT) it tends to be _______
- For Nonmetals (right side of PT) it tends to be ______
Atomic Radii:___________________________________________________
_____________________________________________________________
- found on Reference Table S
- radii ____________ as you go across the Periodic Table Left  Right
- radii ____________ as you go down Periodic Table
Reactivity:
As a metal: _____________________________________________________
Most reactive Metal = _____________________________
As a nonmetal: __________________________________________________
Most reactive Nonmetal = __________________________
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g) FORMING IONS: When atoms gain or lose electrons their form charged
particles called ions.
The only deference between ion and its original atom is the difference in
number of electrons, protons stay the same.
EX: Hydrogen
has 1 electron: - charged
1 proton:
+ charged
If hydrogen loses an electron it becomes an ion with a charge of ______
If hydrogen gains an electron it becomes an ion with a charge of _____
Ionic Radius
An ionic bond (attraction between metal and nonmetal ion) forms when a metal
loses valence electrons to a nonmetal by forming a positive ion and the nonmetal,
which gained the electrons, forms a negative ion. These oppositely charged ions
then attract to each other. By losing or gaining electrons, each ion formed gets 8
valence electrons.
Metals: lose valence electrons when forming positive ions called: _____________
# electrons lost = _____________
This is known as OXIDATION.
For lithium (Li)
Bohr Model of the neutral atom
Bohr Model of the “+ ion”
What happens to the size of the metal atom when it forms an + ion? ________
This is known as the
IONIC RADIUS.
Ionic radius of a metal ion is _____________ then its neutral atom.
(Memory hook- lose weight, get a smaller waist; lose electrons get __________)
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Nonmetals: gain valence electrons when forming negative ions called: ___________
# electrons gained = ___________ This is known as REDUCTION.
For fluorine (F):
Bohr Model of the neutral atom
Bohr Model of the ion “-ion”
What happens to the size of the nonmetal atom when it forms an - ion? ________
This is known as the IONIC RADIUS.
Ionic radius of a nonmetal ion is ____________ then its neutral atom.
(Memory hook- gain weight, get a larger waist; gain electrons get __________)
Ionic Compounds
Metals
Become
Nonmetals
Cations
Become
Anions
Amount of electrons lost or gained by an atom could be found on the Periodic table.
It is called oxidation number /oxidation state
Find the charges ( oxidation nuber) for the following elements and record them the
appropriate way: Sr+2
Na
,
Sc,
Ba,
Mg,
O,
Cl,
He
Some atoms of elements can have more than one ionic charge.
Write these ions with their charges.
Fe
Cu
Sn
Mn
Au
Fe
Cu
Sn
Mn
Au
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Cation
Anion
Na+1
Cl-1
Mg+2
S-2
Sr+2
Br-1
K+1
O-2
Al+3
O-2
Try these now:
Positive Ion
Ra+2
Negative Ion
I-1
Cu+1
Se-2
Zn+2
Te-2
Sn+4
O-2
Au+3
N-3
Cs+1
F-1
Be+2
P-3
Ag+1
S-2
Formula
Formula
Use uncriss-cross method to figure it out original charges of the elements.
Formula
NaF
Cation
Anion
K2 O
SnO
Au2O3
FeO
AlCl3
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h) Trends in an “atomic shell” instead of a nutshell!
Trend
Down A
Group
(top to
bottom)
Reason for Trend
Across a
Period
(L R)
Reason for Trend
Atomic Number
Number of Valence
Electrons
Metallic
Characteristics
(Reactivity/Activity
as a metal loses
electrons)
Non-Metallic
Characteristics
(Reactivity/Activity
as a non-metal gains
electrons)
Electronegativity
(EN)
Ionization Energy
(IE)
Atomic Radius
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I) PERIODIC TABLE WORKSHEET
I. Determine the Principle Energy Level (PEL) and the number of valence electrons for
the following elements.
(PEL = Period #)
Element
PEL
# Valence Electrons
Li
Mg
Al
Ge
N
Se
Cl
Kr
II. Use the trend for atomic radii to
determine the larger atom of the pair.
Circle the larger element (You can look
up the radii on Reference Table S also)
1)
2)
3)
4)
5)
N
O
P
Mg
Li
or
or
or
or
or
O
S
As
Na
Be
III. Use the trend for electronegativity
(EN) to determine which atom of the pair
has the higher electronegativity. Circle
the element with the higher EN (You
can look up the EN on Ref. Table S also)
1)
2)
3)
4)
5)
O
N
Mg
Cl
P
or
or
or
or
or
S
O
P
I
N
IV. Using the periodic table, determine the charge of the ion formed from the element
listed and indicate if the radius of the ion is Larger (L) or Smaller (S) than the
neutral atom. Remember to use the FIRST charge listed for nonmetals.
ELEMENT
1) Mg
CHARGE
Size: L or S
ELEMENT
5) Br
2) Na
6) O
3) S
7) Sc
4) H
8) N
CHARGE
Size: L or S
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Periodic Table in Review:
1) Which two elements are the only liquids?________and __________
2) Which group, name and number, exists as monatomic molecules of gas?
Group #: ____________Name: ______________________
3) Which group, name and number, contains elements, which are solids, liquids and gases?
Group #: ____________Name: ______________________
4) Which elements exist as diatomic molecules? ___________________________
5) Which elements are gases on the periodic table?
______________________________________________________________
6) Which elements are metalloids and where are they found? __________________
_____________________________________________________________
7) Which element is the most reactive metal? ______ reactive nonmetal? _______
8) Even though iodine’s mass is less than tellurium, why was iodine (I) placed in group 17,
after tellurium (Te)? _________________________________________
9) Why is hydrogen (H) placed on top of Group 1 metals when H is not a metal?
_____________________________________________________________
10) Which elements form compounds whose aqueous solutions are colorful?
________________________________________________________________
11) Which metal groups are so reactive, they are never found alone, only in compounds?
Group #: ___Name: ___________________________________
Group #: ____Name: __________________________________
12) Metals form __________ charge ions by (losing or gaining) electrons, whose size is
________________ then the neutral atom. Loss of electrons is known as (oxidation or
reduction). [circle the correct term in the (
)]
13) Nonmetals form __________ charge ions by (losing or gaining) electrons, whose size
is ________________ then the neutral atom. Gain of electrons is known as (oxidation
or reduction). [circle the correct term in the (
)]
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