Chapter 6
The Periodic Table and
Periodic Law
Historical Timeline
Development of the
Periodic Table
Thursday and Friday
6.1 Development of the Periodic
Table
• Late 1790s
• Antoine Lavoisier
• compiled a list of all
elements known at the time23 elements
• 1800s- invention of electricity,
development of spectrometer, and
industrial revolution led to
explosion in the number of known
elements
• By 1870 there were 70 known
elements
• 1864
• John Newlands
• created law of octaves,
which means that properties
repeat every 8th element
• Law doesn’t work for all
elements
• 1869
• Meyer and Mendeleev
demonstrated a connection
between atomic mass and
elemental properties
• 1869
• Mendeleev organized 1st periodic
table by atomic mass and left
blank spaces where undiscovered
elements should go- not
completely correct
• 1913
• Moseley arranged elements
according to atomic number
• Periodic Law – the periodic
repetition of chemical and
physical properties of
elements when they are
arranged by increasing
atomic number
The Modern Periodic Table
• Consists of boxes containing
element name, symbol,
atomic number, and atomic
mass
Friday
• We will finish the historical timeline of the
periodic table
• We will color the two main sections of the
periodic table:
• Representative elements
• Transition elements
• We will color in the metals and the nonmetals
and the metalloids
• Representative Elements- main group
of periodic table (1,2, and 13-18), s and
p block; represent a wide range of
chemical and physical properties
• Transition Elements- groups 3-12
Classifying the Elements
• Metals- elements that are
generally shiny, solids at
room temperature, good
conductors of heat and
electricity, malleable (able to
be pounded into thin sheets),
and ductile (drawn into wires)
• Nonmetals- generally gases or
brittle, dull-looking solids; poor
conductors of electricity
• Metalloids- elements with physical
and chemical properties of both
metals and nonmetals
Monday
• We will make a foldable over the different
types of groups in the periodic table
The Families of the
modern Periodic Table
• Alkali Metals- Group 1A (1)
• Alkaline Earth Metals- Group 2A (2)
• Both groups are chemically reactive
• Transition Metals- Group B elements (d
block)
• Inner Transition Metals- (f block)
• Halogens- Group 7A (17); highly
reactive
• Noble Gases- Group 8A (18);
extremely unreactive
Classifying the Elements
• S-block elements
–groups 1A and 2A
–Holds a maximum of two electrons
• P-block elements
group 3A through 8A, or 13-18
Holds a maximum of 6 electrons
• d-block elements
– contains transition metals
– largest block
– holds maximum of 10 electrons
• f-block elements
– contains inner transition metals
– lanthanide and actinide series
– holds maximum of 14 electrons
•
Tuesday - Exploration
Activity
Lab over the periodic trends of the
Periodic Table
Wednesday
• We will do trends on the periodic table
• Compare our notes to he lab from
Tuesday
6.3 Periodic Trends
• Atomic Radius
generally increases from right to left
and increases from top to bottom of
the periodic table
• Adaptive Curriculum Clip
Atomic Size
• Ionic Radius- positive ions
decrease from left to right until
group 3A (13), then negative ions
decrease until 8A (18); generally
increases from top to bottom
• Ion- atom or bonded group of
atoms that has a positive or
negative charge
Cation
–positively charged ion (lost
electron)
–Will decrease radius because of
loss of outer energy level
–Are in groups 1-13
Anions
–negatively charged ion (gained
electron)
–will increase radius because
protons “pulling in” are the same
and with extra electrons they repel
each other and spread out
–groups 14-18
Atomic and Ionic radius
follow the same trend!!
Ionization Energy
• energy required to remove
an electron from a gaseous
atom
• generally decreases from right
to left and decreases from top to
bottom
Electronegativity
• indicates the relative ability of its
atoms to attract electrons in a
chemical bond
• decreases from right to left and
decreases from top to bottom
Follows the same trend as
electronegativity!!
Thursday
• We will finish our lab
• We will finish our review and check it
in class
Friday
• We will test on Friday