Chapter
#5
The
Periodic
Law
5-1 History of the
Periodic Table
• Cannizzaro (18261910) developed a
method for
measuring atomic
masses and
interpreting the
results of the
measurements.
Stanislao Cannizzaro
• Mendeleev
(1834-1907)
Created the
1st periodic
table by
increasing
atomic mass.
Dmitri
Mendeleev
• Moseley (18871915) set up the
periodic table
according to
increasing atomic
number.
Henry Moseley
• The word "periodic" means that there is a
repeating pattern.
• Examples of things that are periodic are,
days of the week, the months of the year,
the seasons, etc..
• In regards to the periodic table of
elements, periodic refers to the
properties of the elements that repeat
with each row (period) of the table.
• The modern periodic law states: The
chemical and physical properties of the
elements are periodic functions of their
atomic numbers.
• Put in other words, when the elements are
arranged in order of increasing atomic
number, there is a periodic repetition of
their properties.
• The periodic table is an arrangement of
the elements in order of their atomic
numbers so that elements with similar
properties fall in the same family (group).
5-2 Electron Configuration
and the Periodic Table
•
•
•
•
Families 1 & 2 = s-block
Families 3-12= d- block
Families 13-18= p-block
Lanthanide and Actinide series= f-block
• Group (Family) 1- Alkali Metals- combine
vigorously with many nonmetals very
reactive, not found in nature as free
elements. (Video)
• Group 2- AlkalineEarth Metalsthey are harder,
denser, stronger,
and have higher
melting points
than group 1
• not found in
nature as free
elements.
Copper
Iron
• Groups 3-12Transition metals
they have metallic
properties.
Cobalt
Chromium
• Main-group elements are the p-block
and s-block elements.
• Group 13- Boron's Family
• Group 14- Carbon’s Family
• Group 15- Nitrogen's Family
• Group 16- Oxygen’s Family
• Group 17- Halogens the most reactive
nonmetals they form “salts”
• Group 18- Noble Gases- Least
reactive family. WHY????
F-Block
• Lanthanides- “rare
earths” all shiny
reactive metals.
• Actinides- all
unstable and
radioactive. 1st 4
found naturally all
the rest are labmade.
Cerium
5-3 Electron configuration
and Periodic Properties
• Atomic Radius- is
one-half the
distance between
the nuclei of
identical atoms
joined in a
molecule.
BIG
Small
• Ionization Energythe energy
required to remove
1 e- from an atom
of an element (lose
electrons)
• Ion- is an atom or
group of atoms
that have a charge
(+ or -).
• Electron Affinityis the energy
change that
occurs when a
electron is
acquired by a
neutral atom (gain
e-).
Ions
• Cation- positive
ion
• Anion- negative
ion
Atom of Na
One electron is
removed
11 protons 11 electrons
Positive
because
eIon of Sodium (Na+)
11 protons 10 electrons
One eadded
Atom of Cl
Ion of Chlorine (Cl-)
17 protons 17 electrons
17 protons 18 electrons
• Valence e- (outer most) the e- available to
be lost, gained, or shared in the formation
of chemical compounds.
• Groups 13-18
• Val e- = group # - 10
ANIONS
CATIONS
• Electronegativity:
relative tendency of
an atom to attract
electrons to itself
when it is bonded to
another atom.
*It follows the same trend as electron affinity and
ionization energy. It increases across a period and up a
group.
*The most active metals (lower left) have lowest
electronegativities. Francium has the lowest
electronegativity.
*Non-metals (upper right) have the highest
electronegativities.
*Flourine has the highest electronegativity of all
other elements.
Work Cited
•
•
•
•
•
•
“Ion Cartoon”. Drawing. Aug. 8, 2006.
http://ccmm.fc.ul.pt/vnunes/ensino/quimica2.htm
“Canizzaro”. Photo. Aug. 8, 2006. http://www.unipa.it/~cheminor/
“Mendeleev”. Photo. Aug. 8, 2006.
http://academic.brooklyn.cuny.edu/chem/howell/chem11/octetSet
1.htm
“Moseley”. Photo. Aug. 8, 2006.
http://home.iitk.ac.in/~sreerup/bso203/Moseley.jpg
“Mendeleev Table and history of the periodic table”. Photo. Aug. 8,
2006.
http://www.batesville.k12.in.us/bms/Staff/smithhomepage/webqu
ests/Mendeleevtable.gif
“Periodic Table”. Gif. Aug. 8, 2006.
http://imagine.gsfc.nasa.gov/docs/features/topics/instrument_de
sign/periodic.gif
• “Blocks of the Periodic table”. Diagram. Aug. 8, 2006.
http://boomeria.org/chemlectures/menu.html
• “Sodium Pictures”. Picture. Aug. 8, 2006.
http://www.theodoregray.com/PeriodicTable/Stories/011.2
/
• “Magnesium”. Picture. Aug. 8, 2006.
http://www.theodoregray.com/PeriodicTable/Elements/012
/index.s7.html
• “Transition metal pictures”. Photo. Aug. 8, 2006.
http://www.theodoregray.com/PeriodicTable/Elements/Tra
nsitionMetals/index.s7.html
• “F-Block elements”. Photo. Aug. 8, 2006.
http://www.theodoregray.com/PeriodicTable/Elements/095
/index.s7.html
• “Periodic Table of Elements”. Chart. Aug. 9, 2006.
http://users.erols.com/kdennis/periodictable.jpg
•
•
•
•
•
•
“Atomic Radii Chart”. Diagram. Aug. 8, 2006.
http://www.colorado.edu/physics/2000/periodic_table/periodic_p
roperties.html
“Electron Affinity Chart”. Diagram. Aug. 8, 2006.
http://www.chemistry.ohiostate.edu/~grandinetti/teaching/Chem121/lectures/periodic%20tr
ends/affinity.html
“Electronegativity chart and information”. Diagram. Aug. 9, 2006.
http://www.homewood.k12.al.us/~kreaves/Chemicalbonding.htm
“Ionization energy chart”. Diagram. Aug. 9, 2006.
http://neon.mems.cmu.edu/27201/ionization-enthalpy-1-c.gif
“Sodium and Chlorine ions”. Aug. 9, 2006.
http://www.dgpc.ulaval.ca/bio90192/chap1/ions.htm
Holt, Rinehart and Winston. Modern Chemistry. Harcourt Brace &
Company. 1999.