Download Periodic Table PP revised 2014

Periodic Table
Mendeleev vs. Modern Periodic Table
• Mendeleev organized his
periodic table by
increasing atomic mass
• The modern periodic
table is organized by
increasing atomic number
• This arrangement reflects
the periodic recurrence of
similar properties as
the atomic
number increases
Groups in the Periodic Table
• Groups are the vertical columns in the periodic table
(also know as families)
• Elements in the same group will have similar chemical
and physical properties (because they have the same
number of valence electrons)
Periods in the Periodic Table
• Periods are the horizontal rows in the periodic table
• All of the elements in a period have the same number
of atomic orbitals.
• As you proceed from left to right on The Periodic Table,
a proton and an electron is added
The Element Song
• http://www.youtube.com/watch?v=K8eT-k4f7_8
Classes of Elements
• 3 main types of elements:
1. Metals
2. Nonmetals
3. Metalloids
Properties of Metals
• Good conductors of
heat and electricity
• Luster (shiny)
• Ductile (can be
drawn into thin
wires)
• Malleable (can be
hammered into a
thin foil or into
shapes)
Properties of Nonmetals
• Properties
opposite of
Metals
• Poor
conductors of
heat and
electricity
• Brittle
• Lack luster
Properties of Metalloids
• Properties
similar to both
metals and
nonmetals
• Example: have
luster and is
brittle
Alkali Metals (group 1)
• 1 valence electron (tend to lose it
very easily)
• Most reactive metals
• They are so reactive they are
only found naturally in
compounds
• Can be extracted from
compounds using electricity
• Reacts violently with water to
form H2 (g) and a base
• • Alkali means base (as opposed
to acid)
Reactivity of Alkali Metals and Water
• http://www.youtube.com/watch?v=cqeVEFFzz7E
Alkaline Earth Metals (group 2)
• 2 valence e- (tend to lose their
2e- very easily)
• Active metals
• Found naturally in compounds
• Can be extracted from
compounds using chemical
reactions
• Reacts quickly with water for
form H2 (g) and a base
Halogens (group17)
•
•
•
•
7 valence e- (tend to gain 1 e-)
Most reactive nonmetals
Found as diatomic molecules
The only group that contains all
3 phases of matter
• Can be extracted from
compounds using electricity
• Reacts violently with metals to
form halide compounds (like
NaCl)
Noble Gases (group 18)
• 8 valence e- (will not gain
or lose)
• Very stable (not reactive)
• A few compounds contain
the larger noble gases
Transition Elements
• Group 3-12
• Form colored solutions
when added to water
• Can lose different
amount of electrons or
have multiple oxidation
states (ex. Iron can lose
2 or 3 e-)(upper right
corner of each box)
• Range of reactivities,
some are quite reactive,
others are nonreactive.
• Some can be found in
pure form in nature (Cu,
Ag, Au)
Hydrogen
• 1 valence electron
• Can lose or gain 1 e• Found as a diatomic
molecule
Allotropes
• These different forms arise because of the different
conditions that elements may be found.
• Examples:
• Carbon:
• coal (amorphous mass)
• diamond (network bonded crystal)
• graphite (mineral where the carbon atoms are
bonded in weakly connected sheet structures)
• Oxygen:
• O2(diatomic oxygen),
• O3(ozone)
Trends or Patterns in the Periodic Table
Ionization Energy:
the amount of energy needed to remove a valence
electron
Electronegativity:
the measure of attraction for electrons by the nucleus
(how bad does the nucleus want to hold onto its valence
electrons
Atomic Radius:
the size of the atom
Trends or Patterns in the Periodic Table
High Electronegativity
High
____
Ionization Energy
What will the radius be, large or small?
Small Radius
Low Electronegativity
Low Ionization Energy
____
What will the radius be, large or small?
Large Radius
• http://www.youtube.com/watch?v=1PSzSTilu_s
Families
• Columns of elements are
called groups or families.
• Elements in each family
have similar but not
identical properties.
• All elements in a family
have the same number of
valence electrons.
Periods
• Each horizontal row of
elements is called a period.
• The elements in a period
are not alike in properties.
• In fact, the properties
change greatly across
every given row.
• The first element in a
period is always an
extremely active solid. The
last element in a period, is
always an inactive gas.
Trends in Ionic Size: Cations
• Cations form by losing electrons.
• Cations are smaller than the atom they
came from – not only do they lose
electrons, they lose an entire energy
level.
• Metals form cations.
• Cations of representative elements
have the noble gas configuration
before them.
Ionic size: Anions
• Anions form by gaining electrons.
• Anions are bigger than the atom
they came from – have the same
energy level, but a greater area the
nuclear charge needs to cover
• Nonmetals form anions.
• Anions of representative elements
have the noble gas configuration after
them.
Now you are almost as smart as I
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