The Current Periodic Table
• There is a periodic repetition of their physical &
chemical properties when elements are arranged
by their atomic number……this is called The
Modern Periodic Law.
Groups…Here’s Where the Periodic
Table Gets Useful!!
• Elements in the
same group
have similar
chemical and
physical
properties!!
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(Mendeleev did that on purpose.)
Why??
• They have the same
number of valence
electrons.
• They will form the same
kinds of ions.
METALS
More than ¾ of the known elements are metals.
Metals share similar properties:
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Good conductors of heat & electricity
Luster
Malleable & ductile
High densities
High boiling points & melting points
Resists stretching & twisting
Solids at room temperature
Write metal, cation, donates e in the top left corner
of your PTE
NONMETALS
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No luster
Poor conductors
May be solid, liquid or gas
Low densities
Low melting & boiling points
Write nonmetal, anion, accepts e in the top
right corner of your PTE
METALLOIDS
• Also called semimetals
• Have properties of both metals and
nonmetals
• Outline the large black line with a marker..the
elements that touch these are the metalloids
Hydrogen
• Hydrogen belongs to a family
of its own.
• Hydrogen is a diatomic,
reactive gas.
• Hydrogen was involved in the
explosion of the Hindenberg.
• Hydrogen is promising as an
alternative fuel source for
automobiles
• Color it red
• German airship (called a zeppelin- means
rigid airship)
• 804 feet long
• In 1937 it caught fire killing 35 of the 97
people on board.
• Travelling from Germany to US; caught fire
as it was landing in NJ
Alkali Metals
• 1st column on the periodic table (Group
1) not including hydrogen.
• Low densities & melting points
• React with oxygen & moisture in air
• Most reactive metals, always
combined with something else in
nature, they are not found uncombined
(like salt)
• Soft enough to cut with a butter knife
• Will react violently with water & are
stored under oil or kerosene
• Label +1 and s1 on top of Group 1A
Alkaline Earth Metals
• Second column on the
periodic table. (Group 2)
• Reactive metals that are
always combined with
nonmetals in nature.
• Several of these elements
are important mineral
nutrients (such as Mg and Ca
• Harder than alkali metals
• Less reactive than alkali
metals, not stored under oil
or kerosene
• Label +2 and s2 on top of
Group 2A
Transition Metals
• Elements in groups 3B12B
• Less reactive harder
metals
• Includes metals used in
jewelry and construction.
• Metals used “as metal.”
• Label d1-d10 on top of
transitional metals
Boron Family
• Elements in group 3A
• Aluminum metal was
once rare and expensive,
not a “disposable metal.”
• Label +3 and p1 on top of
Group 3A
Carbon Family
• Elements in group 4A
• Contains elements
important to life and
computers.
• Carbon is the basis for
an entire branch of
chemistry (Organic
Chemistry).
• Silicon and Germanium
are important
semiconductors.
• Label +/-4 and p2 on top
of Group 4A
Nitrogen Family
• Elements in group 5A
• Nitrogen makes up over
¾ of the atmosphere.
• Nitrogen and phosphorus
are both important in
living things.
• Most of the world’s
nitrogen is not available
to living things.
• The red stuff on the tip of
matches is phosphorus.
• Label -3 and p3 on top of
Group 5A
Oxygen Family
• Elements in group 6A
• Oxygen is necessary for
respiration.
• Many things that stink,
contain sulfur (rotten
eggs, garlic, skunks,etc.
• Label -2 and p4 on top of
Group 6A
• )
Halogens
• Elements in group 7A
• Very reactive, volatile,
diatomic, nonmetals
• Always found combined with
other element in nature .
• Form salts when combined
with Groups 1 or 2 metals
• Used as disinfectants and to
strengthen teeth.
• Label -1 and p5 on top of
Group 7A
The Noble Gases
The Noble Gases
• Elements in group 8A
• VERY unreactive, monatomic
gases
• Occur in atmosphere in very
small amounts
• Used in lighted “neon” signs
• Used in blimps to fix the
Hindenberg problem.
• Have a full valence shell.
• Label 0 and p6 on top of
Group 8A
• Make a dash and label s2 out
from He (see example)
Lanthanide Series
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The lanthanide family is comprised of fifteen
elements starting with lanthanum (La) at
atomic number 57 and finishing up with
lutetium (Lu) at number 71.
You might find some of these elements in
superconductors, glass production, or
lasers.
Label f1-f14 on top of these rows
Place a 4 out to the left of the row
Actinide
Series
• The actinide family is comprised of
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fifteen elements that start with
actinium (Ac) at atomic number 89
and finish up with lawrencium (Lr)
at number 103.
You have probably heard of
plutonium (Pu), since it was used in
atomic bombs.
Uranium (U) is also well known for
its radioactivity.
They aren't all used to blow up the
world. Some of them help us out
every day. You can find americium
(Am) is some metal detectors.
Label a 5 out to the left of the row
Diatomics
• 7 elements are so
reactive they are NOT
found alone in nature
• They are found in
pairs called diatomics
• H2,
N2,O2,F2,Cl2,Br2,I2
• The Magic “7”
• Color them all red
Elements as Building Blocks
• The periodic table is organized like a big grid.
• The elements are placed in specific places
because of the way they look and act.
Periods
• Even though they skip some squares in between, all of
the rows go left to right.
• When you look at a periodic table, each of the rows is
considered to be a different period (Get it? Like
PERIODic table.). There are 7 periods or rows
• In the periodic table, elements have something in
common if they are in the same row.
• All of the elements in a period have the same number of
electron orbitals.
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A pattern of repeating order is called periodicity. In the mid-1800s, Dmitri
Mendeleev, a Russian chemist, noticed a repeating pattern of chemical
properties in elements.
Mendeleev arranged the elements in order of increasing atomic mass, to form
something that resembles the modern periodic table. He was even able to
predict the properties of some of the then-unknown elements. Later, the
elements were rearranged in order of increasing atomic number.
The periodic table enables chemists and chemistry students to:
Learn the properties of families of elements (instead of learning the properties
of each element), thus saving a lot of time and effort.
Find the relationships among elements and figure out the formulas of many
different compounds.
Examine the atomic numbers, mass numbers, and information about the
number of valence electrons.
Groups (Columns)
Same group=same valence electrons
• The elements in a group have the same number
of electrons in their outer orbital or valence
electrons.
• Group One has 1 valence electron,
• Group Two has 2 valence electrons
• Group 3 has…
• Group 4, 5, 6, 7, 8….
Let’s Look at it another way… Using
Bohr Diagrams
Drawing Bohr Diagrams
Step One
• Determine the # of protons, electrons and
neutrons
• P=9
• E=9
• N=10
Step two
• Draw a circle around the number of p and n,
representing the nucleus
Step 3
• Draw the correct number
of shells
• Remember, the shells
are the same number as
the period
• F is in the 2nd period, so
it has 2 shells
Step 4
• Dots are the electrons
• 2 can go in the first
• 8 can go in the 2nd
But how do you know that there are 2 in
the 1st shell, and 7 in the 2nd??
1
2
Let’s Practice Some
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C
O
Li
Cl
Ca
Now, it is easier to see the valence electrons
Be
B
Al
4 p+
5 n°
O
5 p+
6 n°
13 p+
14 n°
Na
8 p+ 2e– 6e–
8 n°
11 p+ 2e– 8e– 1e–
12 n°