Transcript The Periodic Table

The Periodic Table

Is a table of
elements arranged
in order of
increasing atomic
number and upward
and downward
trends.
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The Atomic Number
Is a also known as the number of
protons in an atom of an element.
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Periods

Are the rows that go
across on the table
and represents the
ENERGY LEVELS
of an atom.
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Groups

Are columns and
represent the same
number of OUTER
ENERGY LEVEL
ELECTRONS that
dictate similar
physical and
chemical properties.
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Properties such as:
Conductivity
 Reactivity
 Boiling & Melting
Point
 Density M/V
 Ionization Energy

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The Periodic Table is arranged
into four main groups:
Metals-low number of outer shell
electrons
 Nonmetals-high number of outer shell
electrons
 Metalloids-semiconductors
 Noble Gases-unreactive
 *atom arrangement depend on the outer
shell electrons

Main Group Elements
Groups 1, 2, & 13-18 have regular
electron configurations. They are
the representative elements.
Main Group Elements 1A-8A
Transition Elements 1B-8B
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Four groups within the main
group have special names:
GROUP 1 ALKALI METALS
 GROUP 2 ALKALINE EARTH METALS
 GROUP 17 HALOGENS
 GROUP 18 NOBLE GASES

METALS
Are groups 1-12 and some
elements in groups 13-16. These
are good conductors of electricity
and except for Mercury are solids
at room temperature.
GROUP 1ALKALI METALS
Are called as such because they
react with WATER to produce
alkaline solutions and because
they have metallic properties.
They are very soft and can be cut
with a knife. A newly cut surface
is shiny, but dulls quickly when
exposed to oxygen and water in
the air.
ALKAI METALS cont…
Alkali Metals have to be kept in kerosene
(heating oil) to isolate it from reacting in
the air. They are highly explosive.
Alkali metals react vigorously with cold
water forming hydrogen gas and a very
alkaline solution.
They are good conductors of electricity
because of their electron configuration.
ALKALI METALS continued

They have only one electron in their
outer shell.
 By losing this electron, the element
becomes stable like a noble gas
 *This is why these metals are very
reactive. This one electron wants to
get away from the atom and
reactive any atom around it.
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Plasmas-the fourth state of
matter
At high temperatures,
alkali metals become
plasmas, the fourth state
of matter.
They are made of ions,
electrons and neutral
particles.
Ions are atoms that have
lost or gained electrons
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Plasma continued…

As electricity flows through the ions, electrons
and neutral particles, electrons are
transferred to higher energy levels and a
photon of light is emitted (given off) as the
electron returns to its original energy state or
ground state.
 In fog lights, sodium plasma emits a yellow
glowing light. These are in many cars sold
today.
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Atom emitting a photon
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FINAL NOTE
Group 1 metals are so reactive
they are not found in nature by
themselves and have to be
produced in a laboratory for
commercial or educational
purposes.
GROUP 2
ALKALINE EARTH METALS
These metals are harder, denser, and
have higher melting points than alkali
metals.
These metals are less reactive than
those in group one. In reactions with
other metals, these metals lose two
electrons to become a noble gas. All
elements will lose or gain electrons to
achieve stability.
ALKALINE EARTH METALS
continued…
One of the most common alkaline
earth metals is CALCIUM found in
limestone and marble and and
essential to good bone structure and
health.
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CALCIUM is a metal
GROUP 17 HALOGENS
These are nonmetals that combine
with metals to produce SALTS.
The word halogen means “salt former”
in Greek.
NaCl is sodium chloride and ordinary
table salt.
*The halogens are the MOST
REACTIVE GROUP of the nonmetals.
HALOGENS continued…
When halogen atoms react
chemically, they often require ONE
electron to achieve stability. They are
said to achieve the configuration of a
noble gas.
All elements want to achieve a noble
gas configuration.
The halogens exist in all 3 states of
matter at STP.
HALOGENS
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GROUP 18 NOBLE GASES
These gases were formerly known as
inert gases because the were thought to
be completely unreactive due to having a
full outer shell of electrons.
This means that all the noble gases have
EIGHT electrons in their outer shell.
However, Xenon has been prepared as
XeF2.
HELIUM has only TWO electrons, but is
considered to have a full outer shell.
HELIUM
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HYDROGEN
In a Class of its Own
Is considered in a class of its own and
is the MOST COMMON and
NUMEROUS element in the universe.
It was the first element to form in the
universe.
It contains ONE PROTON & ONE
ELECTRON only.
HYDROGEN
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GROUPS 3-12
TRANSITION METALS
These metals have electrons used for
bonding in more than one energy level.
Therefore, they DO NOT exhibit regular
electron configurations like the Main
Group Elements who only have electrons
for bonding in the outer shell.
Bonding electrons are called VALENCE
ELECTRONS.
GROUPS 13-16
THE OTHER METALS
These metals exhibit regular electron
configurations and exhibit all the
characteristics of metals, such as luster,
malleability, electrical and heat
conductivity to various degrees.
They are all solids, have high densities,
and are opaque.
THE METALLOIDS
These semimetals as their
known, conduct electricity, but
not as well as metals.
By adding trace metals,
semiconductors are useful as
transistors and in other
electronic devices like
computers and calculators.
They contain both properties of
metals and nonmetals.
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GROUPS 14-16
THE NONMETALS
These nonmetals as their called are poor
conductors of electricity.
They are brittle and are not able to be
hammered or rolled.
They also lack luster. They are found in
solid and gas state at STP.
RARE EARTH METALS
Thirty rare earth elements are
composed of the Lanthanide and
Actinide series.
Most elements in the Actinide series
and ONE element in the Lanthanide
series are TRANSURANIUM.
Transuranium means synthetic or
manmade.
These manmade elements are made
in a particle accelerator in a
laboratory.
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VOCABULARY
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ION-an atom that has gained or lost electrons
ANION-an atom that has gained electrons.
CATION-an atom that has lost electrons.
ENERGY LEVEL-where electrons spin
around an atom. They are given numbers to
identify each of the seven levels an atom may
contain.
ORBITAL-are areas or regions in an atom
where there is a high likelihood of finding an
electron.
Orbitals contain zero, one or two elcctrons.
One or more orbitals can be found in each of
the seven energy levels.
Atom showing Energy Levels
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CONCEPTS TO KNOW

All physical and chemical properties of the
periodic table are explained by the atom itself
and the number of electrons contained in the
outer shell.
 The Periodic Table was formulated by Dmitri
Mendelev and illustrates the atom’s periodic
nature.
 Periodic means repeating. The properties of
the atoms repeat similarities when ranked
from lowest to highest by atomic number.
CONCEPTS TO KNOW
continued

The atom has a very tiny dense nucleus with
a very large diameter where electrons are
thought to reside.
 Electrons spin around the nucleus in pairs
called orbitals.
 Orbitals spin at various distances from the
nucleus. Those distances are determined by
how much energy the electron has and is
assigned an energy state
 Each energy state is an assigned energy
level.
Atom showing tiny nucleus and
orbitals
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Atom with Orbitals
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FINAL NOTE
METALS lose electrons to be stable.
NONMETALS gain electrons to be
stable.
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