(HISTORY & PERIODIC TRENDS)
HOW DOES THE PERIODIC TABLE LOOK LIKE?
I GROUP/FAMILY
(vertical column)
have similar
chemical properties
II PERIODS/SERIES
(horizontal row)
- has same core
elements and number
of main energy levels
Group 1A – Alkali
Metals
 soft, malleable; lustrous,
good conductors
 MOST REACTIVE family
of metals
Group 2A – Alkaline
Earth
higher densities and
melting points than
alkali metals;
NOT as reactive as alkali
Group 3A
Boron Family
- except for Boron
which is a metalloid the
rest of the elements
are considered metals.
Group 4A
Carbon Family
 They all have 4 valence
electrons.
 They react in similar
ratios with oxygen and
other elements.
 They can form up to 4
bonds – more than any
other family!!
 Germanium is a metalloid
Group 5A
Nitrogen Family
- Nitrogen and phosphorus are
nonmetals.
- Arsenic is a metalloid with
mostly nonmetallic properties.
- Antimony is a metalloid with
mostly metallic properties.
- Bismuth is the most metallic
element in the family.
- All members of the nitrogen
family have five electrons in
their outermost energy level.
- These elements lose electrons
easily.
Group 6A
Oxygen Family/
Calcogens
- All of these have six
electrons in their
outermost energy level.
- Their properties go
from nonmetallic in
oxygen and sulfur
- Selenium and Tellurium
are metalloids
- Polonium have metallic
properties
Group 7A
Halogens
(salt-formers)
- MOST REACTIVE Non-Metals
- do not occur free in nature;
commonly found in sea water,
minerals, & living tissues
- have low melting points and boiling
points
- In the gas phase they exist as
diatomic elements
- Halogens combine readily with
metals to form a class of
compounds known as salts
Group 8A
Noble gases/Inert gases
- VERY INACTIVE elements
- used in balloons, scuba diving
tanks, light bulbs
- do not readily combine with
other elements to form
compounds
- found in small amounts in the
earth's atomsphere.
- One important property of the
noble gasses is their inactivity.
They are inactive because their
outermost energy level is full.
 COINAGE /
TRANSITION
METALS
- these elements can be
made into coins.
- able to put more than
eight electrons in the
shell that is one in from
the outermost shell.
- can use the two
outermost shells/orbitals
to bond with other
elements
OTHER SERIES
LANTHANIDE means
RARE-EARTH.
 They were thought not
scarce or rare but VERY
DIFFICULT to extract
from their ores.
ACTINIDE means
RADIOACTIVE.
 All the elements are really
radioactive.
CHEMICAL SYMBOLS
I Alchemists (1st to use symbols for different
elements)
II 1808—John Dalton introduced the framework
for the symbols
III Jons Jakob Berzelius (1st to use letter
symbols; used the 1st letter of the name of the
element)
* note: There are only 26 letters of the alphabet,
so he added a 2nd letter to the symbol of the
other elements whose sound is CONSPICUOUS
when the name of the element is pronounced.
Ex. Ca—Calcium; Cl– Chlorine
CHEMICAL SYMBOLS
IV Some symbols came from their Latin/German names:

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Gold
Silver
Lead
Potassium
Tin
Iron
Mercury
Sodium
Antimony
Copper
Tungsten
(Au)
(Ag)
(Pb)
(K)
(Sn)
(Fe)
(Hg)
(Na)
(Sb)
(Cu)
(W)
– “AURUM”
- “ARGENTUM”
- “PLUMBUM”
– “KALIUM”
- “STANNUM”
– ‘FERRUM”
– “HYDRAGYRUM”
– “NATRIUM”
– “STIBIUM”
– “CUPRUM”
– German name “WOLFRAM”
CHEMICAL SYMBOLS
V NAME of the DISCOVERER OR SCIENTIST
Ex. Einstenium (Es) - Einstein
Mendelevium (Md) – Mendeleev
VI Name of gods
Ex. Thorium (Th) - Thor
Vanadium (V) – Vanadis
VII PLACE
Ex. Francium (Fr) - France
CHEMICAL SYMBOLS
VIII For new elements without name yet the rule on
systemic name is followed.
numerical roots
0 = nil 1 = un 2 = bi 3 = tri 4 = quad
5 = pent 6 = hex 7 = sept 8 = oct
9 = enn
A) roots are assembled in the order of the digits in the
element’s number
B) suffix = IUM added after
Ex. Element 113 = un - un— tri –ium
Ununtrium (Uut)
Note: Final “n” of “enn” is omitted if before ‘nil”.
Ex. 190 = un—enn—nil –ium (Unenilium—Uen)
“i” of “bi” or “tri” omitted when it occurs before “ium”.