Transcript Slide 1

1790’s French chemist Antoine-Laurent Lavoisier
made the first periodic table.
1803- John Dalton
improved the periodic
table by assigning
symbols and masses
to each element.
1869- Dimitri Mendeleev, a
Russian chemist, arranged the
63 known element at the time,
into groups based on their
chemical properties and
atomic weights.
1912- Henry Moseley, an English
physicist improved Mendeleev’s
table by listing the elements by their
atomic number.
Glenn Seaborg- 1930's
The heaviest elements were being put up in the
body of the periodic table, and Glenn Seaborg
"plucked those out" , naming them the Actinide
series, which later permitted proper placement of
subsequently 'created' elements - the
Transactinides, changing the periodic table yet
again.
How to
Name
an
Element
In 2006, element 111 received its official name,
Roentgenium. The element's square on the periodic
table was unveiled by German science minister
Annette Schavan.
How to Name an Element
Periodic Law
When elements on the periodic table are arranged by atomic
number, relationships and similarities in properties can be seen.
This means that when the elements from the periodic table are
arranged in a certain way from lowest to highest atomic number
(the number of protons), the ones near each other will have
similar properties!
The_Periodic_Table.asf
Elements
fall into three groups
characterized by similar properties.
metals, nonmetals, and metalloids
METALS:
majority of elements…where on the periodic table???
Shiny luster
Good conductors of heat and electricity
Solid at room temperature
Malleable, or can be shaped
Ductile, or can be drawn into wires without breaking
Three or fewer
outer electrons
3/4 of all elements are metals
Most metals have one, two or
three electrons in their outer shell
During chemical reactions, metal atoms lose their outer electrons to other atoms,
usually, non metals.
The outer electrons are far from the positive pull of the protons, thus held loosely in
place.
A metal atom becomes stable, or nonreactive, when it has lost its outer electron.
NONMETALS
how many elements and where on the periodic table???
Dull in appearance
Poor conductors of heat and electricity
Many are gases at room temperature
Brittle, cannot change shape without breaking
96% of the human body is made up of nonmetals
have five or more outer electrons
METALLOIDS:
how many elements and where on the periodic table???
Have characteristics of both metals and nonmetals
Do not conduct heat and electricity as well as metals
All are solids at room temperature
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The Periodic Table
I. History
A. Lavoisier, Dalton
B. Mendeleev, Meyer
C. Rutherford, Moseley
D. Seaborg
II. Metals, Nonmetals, Metalloids
III. Organization
A. Periods
B. Groups
C. Group names and info
A Short History of the Periodic Table
Click here for more great information on th
Periodic Table
Metals, Nonmetals and Metalloids
Today’s periodic table:
arranged by atomic number
groups-columns of elements having similar chemical properties
periods-in order of atomic number, increase across the period or row
Periodic Table
Elements as Building Blocks
As you probably saw, the periodic table is organized like a big grid.
The elements are placed in specific locations because of the way
they look and act. The periodic table has rows and columns, and they
each mean something different.
Did ya notice the periodic
table sort of looks like a
calendar?
When you look at a periodic table, each of the rows is
considered to be a different period (Get it? Like PERIODic
table.).
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 atomic orbitals.
Number of orbitals or
energy shells equals
the number of the
period.
All elements in period 2
have two orbitals or
energy shells.
Period 6 elements have
six energy shells.
Group Information on the Periodic Table
What do elements in the same group have in
common?
They all have the same number of electrons in the outer
shell and thus react similarly.
(Valence electrons)
For example, all the group 1 (Alkali metals) elements react
violently with water.
The periodic table groups are as follows
(in the brackets are shown the old systems: European and American):
Group 1 (IA,IA): the Alkali metals
Group 2 (IIA,IIA): the Alkaline earth metals
Group 3 (IIIA,IIIB)
Group 4 (IVA,IVAB)
Group 5
Group 6
Group 7
Group 8
Group 9
Group 10
Group 11
Group 12 (IIB,IIB)
Group 13 (IIIB,IIIA): the Boron Group
Group 14 (IVB,IVA): the Carbon Group
Group 15 (VB,VA): Nitrogen Group
Group 16 (VIB,VIA): the Chalcogens
Group 17 (VIIB,VIIA): the Halogens
Group 18 (Group 0): the Noble gases
Group 1: The alkali metals are lithium, sodium, potassium, rubidium, cesium, and
francium. Hydrogen is also part of this group, but is only in a metal state at great
depths within Jupiter, the pressure is so great that the hydrogen atoms are broken up
and the electrons are freed so that the resulting atoms consist of bare protons. This
produces a state in which the hydrogen becomes metallic.
Alkali Metal Properties
Lower densities than other metals
One loosely bound valence electron
Largest atomic radii in their periods
Low ionization energies
Low electronegativities
Highly reactive when in contact with water
Group 2: The alkaline earth metals
All the elements are all metals with a shiny, silvery- white color.
They are all soft, low density metals, which react readily with
halgens to form ionic salts, and with water but not as rapidly as
the alkaline metals. For example, sodium and potassium react
with room temperature water, however, magnesium reacts only
with steam and calcium reacts only with hot water.
The elements have two electrons in their valance, or outermost
shell.
38 elements in groups 3 through 12 of the
periodic table are called "transition
metals". As with all metals, the transition
elements are both ductile and malleable,
and conduct electricity and heat.
The interesting thing about transition
metals is that their valence electrons, or
the electrons they use to combine with
other elements, are present in more than
one shell.
There are three noteworthy elements in
the transition metals family. These
elements are iron, cobalt, and nickel, and
they are the only elements known to
produce a magnetic field.
The Boron Group, Group 13
Except for boron itself, which is a nonmetal, the elements of
group IIIA, or Group 13, are metals (aluminum, gallium,
indium, thallium). Even boron in its elemental state is a hard
gray material that might be mistaken for a metal.
The elements of group IIIA have a valence (number of
bonds to atoms other elements) of three.
As a group, the elements of the boron group decrease in
electronegativity as one goes down the column.
Group 14: The Carbon Group has the elements change from nonmetallic in character at the top of the Group to metallic at the
bottom.
Carbon is a non-metal, silicon and germanium are metalloids, and
tin and lead are typical metals.
Diamond has a very high refractive index, also the hardest natural
substance known and so is important industrially.
Silicon is a semi-conductor and just a few millimeters square, have
revolutionized the computer and microprocessor industries.
Tin and lead, as typical metals, are good conductors of electricity.
Group 15: Nitrogen Group includes nitrogen, phosphorus,
arsenic, antimony and bismuth and ununpentium.
The name pnictogens is also sometimes used for this group; it is not
approved by IUPAC . The spelling pnicogen is also recorded. Both
spellings derive from the Greek πνίγειν (pnigein), to choke or stifle,
which is a property of nitrogen.
The chalcogens are the name for the periodic table group
16. It consists of the elements oxygen (O), sulfur (S),
selenium (Se), tellurium (Te), the radioactive polonium
(Po), and the synthetic ununhexium (Uuh).
Oxygen and sulfur are nonmetals, polonium is a true
metal, and selenium and tellurium are metalloid
semiconductors.
Group 17: the halogens are a chemical series
including: fluorine , chlorine, bromine, iodine, and
astatine. The word comes from Greek roots
meaning "salt" and "creator".
Group 18: the noble gases are a chemical series which include the
elements helium , neon , argon , krypton , xenon and radon
.
The term noble gas comes from the fact that, just like the common
view of human nobility, these gases generally sit around not doing
anything, and avoid reacting with 'common' elements.
The noble gases were previously referred to as inert gases, but
this term is not strictly accurate now that some have been shown to
take part in chemical reactions.
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