THE PERIODIC TABLE OF ELEMEI\TS
Alkali Metals
The elements in Group 1A of the periodic table.
2. AII six elements have the properties of metal
except they are softer and less dense
3. Most reactive of all the metals
4. Alkali metals are stored under oil to keep them
from reacting with oxygen
5. Alkali metals do react with water, the reaction is
1.
l^'^--+
-'Vi(rt€{rL
6.
Alkali metals have only one electron in their
outermost energy level. They form positive ions
and are very reactive because they lose their
valence electron easily.
J . Can be identified by the characteristic color each
produces in a flame test
8. Few familiar uses. They form compound such as
table salt, baking soda, and soap contain
compounds formed by them.
Alkaline Earth Metals
The elements in Group IIA of the periodic table
2.Harder and denser then alkali metals
3. Higher melting and boiling points than alkali
1.
metals
Highly reactive, but not as reactive as alkali metals
5. Alkaline earth metals are never found free in nature
4.
Magnesium and aluminum to make alloys
that are light weight and strong. Magnesium
compounds used in medicines, photographic
fiashbulbs, and flares. Calcium is an essential part
of hum anh,cay
J .Have two electrons in their outermost energy level
6. Uses:
The Boron Family
!
l.Boron (B), the first elements in the boron
family, is a metalloid
2.Other members - Ga,In, Tl , ffia metals.
3.Boron is hard and brittle, and never found in
the free state
4.Aluminum is the most abundant metal and the
third most abundant metal in the earth's crust
5. All members of this family harythree electrons
in the outennost shell
The Carbon Family
.Includes the elements C, Si, Ge, Sn, and Pb
Z.Cornpounds that contain carbon are called
organic compounds
3. Carbon has often been called "the basis for
life" because all living things contain organic
componds
4. Silicon is the second most abundant element in
the earth's crust. Also used in solar cells
.wni0ii cciiv€ri Iiis aTreT$-! CI Suniigfii iniC
electric energy
5. The densest element in the carbon family is
the metal lead
1
The Nitrogen FamilY
l.Consists of N, P, As, Sb, and Bi
z.Allmembers of this family have five elestrons
in their outermost energy level
3.Nitrogen is the most abundant element in the
earth's atmosPhere
4.Nitrogen is used in the production of
fertiLizers, explosives, drugs, and dyes
5.
Phosphorus is a nonmetal that is too active to
be found free in nature
The Orygen Family
1. The
oxygen family includes O, S, Se, Te, and
Po.
2.All these elements have six electrons in their
outermost energy level
3. Oxygen is the most abundant element in
earth's crust
4. Sulfur, selenium, and tellurium are brittle
solids at room temperafure
5. Sulfur is used in the manufacfure of such
products as clrugs, insecticicles, rrratcires,
gunpowder, and rubber
6. Selenium is used in making red glass and
enamels
T.Tellurium is useful in making alloys
8.Polonium is a very rare radioactive element
Halogens
Elements in Group VIIA
2.Include F, Cl, Br, I, At, and are the most active
nonmetals
3. Chemical reactivity of the halogens is due to
the number of electrons in the outermost
energy level of their atoms. E,ach halogen
atom has seven valence electrons
4.Fluorine is the most active halogen. F'luorine
1.
ani chiorine are gases
Halogens have low melting points and boiling
points
6. Combine readily with metals to form a class of
compounds known as salts. "Halogen" comes
from greek words halos and genos, which
mean "salt formers"
5.
Noble Gases
The six elements that make up the last family
of the periodic table, or Group VIIIA
2.Colorless gases that are extremely unreactive
3. The family of noble, also called inert, gases
includes He, Ne, Ar, Kr, Xe, and Rn
4.Because they are so scarce and so unreactive,
the noble gases were not discovered until the
end of the nineteenth century
5. The most striking property of the noble gases
1.
rs
theirrnacTlity
6.Atoms of noble gases already have complete
outermost energy levels. They do not need to
bond to other atoms
7.Balloon filled with helium
S.Radon to treat cancer, argon in light bulbs,
xenon in photographic lamps
Transition Metals
1. E,lements
between Group
IIA and Group IIIA,
30
elements
2.Common transition elements include nickel,
copper ) zrnc) platinum, gold
3. Have properties similar to one another and to other
metals, but their properties do not fit in with those
of any other family
4. Most transition metal are excellent conductors of
electricity
5. uiiiike nielais, soirro ar*,, $e:\siricn o;el;;ei:is aro
brittle
6.Transition metals are much less active than the
alkali and alkaline earth metals
7.Have more than one oxidation number.
Oxidation number is the number of electrons an
atom gains, loses, or shares during a chemical
reaction.
8. From compounds that are brightly colored.
Particular compounds of the transition metals
cobalt and cadmium are used as pigments in paint
Rare - Earth Element
1. Two rows of elements at the bottom of the
periodic table.
2. The 30 rare earth elements are similar to one
3.
another.
The elements in the first row are called the
Lanthanoid series.
4. The elements in the second row are called the
Actinoid series.
Lanthanoid series
1. Lanthanoids are soft malleable metals that
irave higir iuster anci conciuctivrry.
2. Their primary oxidation number is 3+
3. They are used in the industry to make various
alloys and high quality glass.
Actinoid series
1.
All the actinoids are radioactive.
2. Their primary oxidation number is 3+
3. The best known actinoid is uranium, which is
used as a nuclear fuel.