Transcript Periodic Table

Periodic Table
of Elements
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Bohr Model: and Valence electrons
http://youtu.be/trsln8RCEVo
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Casseopia
http://youtu.be/5MMWpeJ5dn4
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Dan Radcliffe
http://youtu.be/rSAaiYKF0cs
Bald Guy:
http://youtu.be/nsbXp64YPRQ
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Song:
http://youtu.be/afFw91fvNJM
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http://youtu.be/zGM-wSKFBpo
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Dmitri Mendeleev
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Russian chemist.
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Created first version of
the periodic table.
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Predicted properties of
elements yet to be
discovered.
Rockin the shaggy beard…
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Mendeleev arranged
elements according to
their atomic weights.
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Today they are arranged
by atomic number.
Periodic Law
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Properties of elements are periodic
functions of their atomic numbers.
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In other words, properties tend to repeat
as you start a new period.
Groups/Families
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Columns on the table (1-18).
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Elements have the same
number of valence electrons.
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Similar chemical properties.
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Tend to form bonds in a similar
way to get stable octet.
Periods (1-7)
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The rows on the table.
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Have the same number
of occupied energy
levels.
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They do not have similar
properties.
Get to Know Your Groups
Alkali Metals
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1 valence electron
Form +1 Ions
Very reactive
Found only in
compounds.
Rubidium
Comparing the Alkali Metals
http://youtu.be/uixxJtJPVXk
Alkaline Earth Metals
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2 valence electrons
Form +2 ions
Very reactive
Found only in
compounds
Halogens
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7 valence electrons
Form -1 ions
Very reactive
All nonmetals
Gas
Liquid
FLUORINE
Extremely reactive
gas
Solid
IODINE
solid → gas
(sublimes)
Noble Gases
Inert Gases
 Not reactive
 Have stable octet
(except He)
 Monoatomic gases
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s, p, d, f, “Blocks”
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Indicates what sublevel is being filled last
in the atom
Transition Metals
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Metals in the “lower”
columns.
(d-block metals)
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“Inner” transition
metals are the two
bottom rows
(f-block metals)
Transition Metals
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Form colored compounds and solutions.
Metals/Nonmetals/Metalloids
Metals
Have luster
 Malleable
 Ductile
 Conduct heat and electricity
 Tend to lose valence electrons and form
positive ions
 All solids (except Hg)
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Nonmetals
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No luster
Brittle (if solid)
Don’t conduct
Tend to gain valence electrons
and form negative ions
Can be solid ( I, C, P, S) , liquid (Br),
or gases (F, Cl, N, O)
Hydrogen is considered a nonmetal
Metalloids (Semimetals)
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Most elements along the
“staircase”
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Can have properties of
both metals and
nonmetals.
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B, Si, Ge, As, Sb, Te, At
Trends in the Period Table
Atomic Radius
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Distance from the nucleus of an atom to
the outer edge of it’s electron cloud.
Get out Reference
Table S
Trends in Radius
Li
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Na
Down a Group
K
Ex: Group 1 What happens?
Rb
Cs
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Fr
Across a Period
Ex: Period 2
Li
Be
B
What happens?
C
N
O
F
Ne
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Down a Group
Size increases
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You add new energy levels
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Across a Period
Size decreases
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Increasing nuclear charge pulls on the
energy levels
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http://youtu.be/ba2yN2HtPTA
Ionization Energy
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Energy required
to remove the
outermost
electron from an
atom.
Get out Reference
Table S
Trends in Ionization Energy
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Down a Group
Ex: Group 1 What happens?
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Li
Na
K
Rb
Cs
Fr
Across a Period
Ex: Period 2
Li
Be
B
C
What happens?
N
O
F
Ne
What is the trend?
Directly related to Atomic Radius.
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Large Radius = Lower Ionization Energy
Why?
The further the outmost electron to the
nuclear pull the easier to remove it.
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http://youtu.be/8F9nA4Fg3Rw
Electronegativity
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The relative
attraction an atom
has for electrons
involved in bond
formation.
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The higher the EN
value the more the
atom “pulls” on
electrons involved in
a bond.
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This can result in
“polar” and “nonpolar”
bonds.
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Fluorine has the
highest EN value = 4
(The EN scale was
created by comparing
other elements to
Fluorine)
Get out Reference
Table S
Trends in Electronegativity
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Down a Group
Ex: Group 1 What happens?
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Li
Na
K
Rb
Cs
Fr
Across a Period
Ex: Period 2
Li
Be
B
C
What happens?
N
O
F
Ne
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http://youtu.be/93G_FqpGFGY
Metallic/NonMetallic
Character
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More “Metallic”:
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Large radius
Low Ionization Energy
Low Electronegativity
More “Non Metallic”:
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Small radius
High Ionization Energy
High Electronegativity