Transcript The Periodic Table - Journigan-wiki

The Periodic Table
Periodicity
Unit IV
Ch. 6
Pictionary Words
Period
Group
Metal
Metalloid
Electronegativity
Non-metal
Atomic radius
Transition metal
Reactivity
Ionization energy
Warm Up
1. What do you KNOW about the periodic table?
2. What WOULD you like to know about the
periodic table?
3. What did you like to LEARN about the
periodic table?
Warm Up
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4.
What is the law of octaves?
Identify the groups that correspond to the
following family names: alkali metals, alkali
earth metals, chalcogens, halogens, noble
gases and transition metals.
State the periodic law.
Who is credited with organizing the modern
periodic table.
Warm Up-02/19/13
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5.
Identify the family in which the following
appear: K, Cl, Pr, Ba, F, Mn, Th and W.
List 5 transition elements.
The alkili metals are also known as what?
The alkili metals are also known as what?
The noble gas family is also known as what?
Warm Up-09/24/13
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4.
Place the following elements in order from
largest to smallest: Si, Na, Ar, Al and S.
Place the following elements in order from
largest to smallest: Be, Ba, Ca, Mg, and Sr.
Repeat questions 4 and 5 for ionic radius
excluding argon.
Place the following in order from greatest to
lowest ionization energies: Kr, Ne, Xe, He
and Ar.
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Expectations:
1.) Each group will have created a neat,
colorful, and easy to read periodic table.
2.) Atomic Number, Symbol and Name must
be present.
3.) Ionization/Electronegativity/Radii value
must be written in the place of the atomic mass
4.) 3-d dimensions must be to scale
http://www.exo.net/~emuller/activities/The%20Perio
dic%20Periodic%20Table.pdf
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Atomic Radius- p. 914- 916 scale: 1 mm=
1pm.
Ionization Energy- p. 914-916 scale: 1 mm=
10 kJ/mol.
Electronegativity- p. 169 scale: 10 cm = 1
Paulings.
Ionic Radii- handout scale: 1 cm = .1
Angstroms.
Warm Up
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6.
If 1 mm= 1pm, how long would you cut a straw to represent
fluorine’s atomic radius?
If 1 mm= 1pm, how long would you cut a straw to represent
germanium’s atomic radius?
If 10 cm= 1 pauling, how long would you cut a straw to
represent silver’s electronegativity?
If 10 cm= 1 pauling, how long would you cut a straw to
represent gold’s electronegativity?
If 1 mm= 10 kJ/mol., how long would you cut a straw to
represent neon’s ionization energy?
If 1 mm= 10 kJ/mol., how long would you cut a straw to
represent potassium’s ionization energy?
Warm Up
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5.
If 1 mm= 1pm, how long would you cut a straw to represent
gallium's atomic radius?
If 1 mm= 1pm, how long would you cut a straw to represent
oxygen’s atomic radius?
If 10 cm= 1 pauling, how long would you cut a straw to
represent manganese's electronegativity?
If 1 mm= 1 pauling, how long would you cut a straw to
represent calcium’s electronegativity?
If 1 mm= 10 kJ/mol., how long would you cut a straw to
represent kripton’s ionization energy?
Johann Dobereiner, 1817
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Triads
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Groups of three elements having similar physical
and chemical properties.
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These three elements are in the same Group or
Family
John Newlands, 1863
Arranged elements in order of their atomic masses.
Noticed that their properties repeated every 8th
element
Law of Octaves
The same properties repeat every eighth element
Dmitri Mendeleev, 1869
Believed that similar properties occurred after
periods that could vary in length
Properties of the elements repeat in an orderly
way. Such a pattern is “periodic”
The Periodic Law
“The properties of the elements are a periodic
function of their atomic masses”
Henry Moseley, 1913
Using X-Rays, he showed that the nucleus had a
positive charge. Thus, the Periodic Law was
revised:
Periodic Law
Properties of the elements are a periodic
function of their atomic numbers
Electron Configuration and
The Periodic Table
Electron Configuration determines a chemical's reactivity.
s-Block Elements (Groups 1 and 2; or Groups I A and II A)
Outermost electrons are added to an s-orbital
Group 1: s1 - Alkali Metals
Group 2: s2 - Alkaline Earth Metals
Electron Configuration and
The Periodic Table
p-Block Elements (Groups 13-18; Groups III A through
VIII A)
Outermost electrons are added to a p-orbital
Group 13: p1
Group 14: p2
Group 15: p3
Group 16: p4 - Chalcogens
Group 17: p5 - Halogens
Group 18: p6 - Noble Gases (Inert Gases)
Electron Configuration and
The Periodic Table
d-Block Elements (Groups 3-12; Groups I B through VIII B)
Outermost electrons are added to a d-orbital
Known as the transition metals
All metals
Electron Configuration and
The Periodic Table
Reading the electron configuration directly off the
Periodic Table.
s-Block
p-Block
Main Group Elements (s- & p-blocks)
d-Block (Transition Elements)
f-Block (Lanthanides and Actinides)
Warm Up
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7.
What are the three largest divisions within the
periodic table?
What are the characteristics of metals?
What are the characteristics of non-metals?
What are the characteristics of metalloids?
What is the rule of thumb for metals?
What is the rule of thumb for non-metals?
State the octet rule?
Categories of Elements
Metals - hard and shiny; conduct electricity
Nonmetals - gases or brittle solids; good
insulators
Metalloids - properties of both metals and
nonmetals
Rule of Thumb:
Metals have 1-3 electrons in outer level
Nonmetals have >5 electrons in the outer level
The Octet Rule
Eight electrons in the outer level render
an atom essentially unreactive
Rule of Thumb:
An atom having a filled or half filled
sublevel is slightly more stable (less
reactive) than an atom without a filled or
half-filled sublevel.
Relative Atomic Stability
Decreasing order of stability
Full outer shell (s2 and p6)
Full sublevel (s2)
Half-filled sublevel
No special arrangement
Electron Sublevel Structure
If the last electron for an atom is in a full or
half-full sublevel, then the atom is
inherently more stable.
Periodic Properties
Atomic Radii
Ionic Radii
First Ionization Energy
Electronegativity
----------------------------Electron Affinity
Oxidation Numbers
Warm Up
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What happens to atomic radius as you go down the periodic
table?
What is ionization energy?
As atomic number increases in a period, what happens to
ionization energy?
As atomic number increases in a group, what happens to
ionization energy?
List three factors that affect ionization energy?
Define electronegativity?
What happens to electronegativity as you move left to right
across the periodic table?
What happens to electronegativity as you move top to bottom
across the periodic table?
Atomic Radius
As the principal quantum number (n) increases, the size
of the electron cloud increases. That is, the atomic
size increases as you go down the table.
The reason for this is that you are adding energy levels
as you go down the table (1, 2, 3,...).
The positive charge of the nucleus increase as you go
from left to right across the table. This increase in
nuclear charge increases the pull on the electron
cloud by the nucleus - pulling the the electron cloud
in tighter to the nucleus. Thus, the atoms decrease in
size.
Ionic Radii
Metallic Ions
Formed by the loss of electrons
Smaller than the atoms from which they
were formed
Nonmetallic Ions
Formed by the gain of electrons
Larger than the atoms from which they were
formed
First Ionization Energy
The energy required to remove the most loosely-held
electron from a neutral atom.
Increases as atomic number increases in any period.
Decreases as the atomic number increases in any
group.
Affected by:
Shielding Effect
Radius of the atom
Nuclear Charge
Electron Sublevel Structure
Factors Affecting Ionization Energy
Nuclear Charge - ionization energy is proportional to
the nuclear charge
Shielding Effect - Ionization energy is inversely
proportional to the shielding effect
Radius - Ionization energy is inversely proportional to
the distance between the nucleus and the outer
electrons
Sublevel - an electron from a full or half-full sublevel
requires additional energy to be removed
Metals - Low ionization energy
Nonmetals - High ionization energy
Electronegativity
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Electronegativity indicates the ability of an
element’s atom to attract electrons in a
chemical bond.
Electronegativity
Influenced by the same factors which affect
ionization energy and electron affinity
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Size
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Shielding effect
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Nuclear charge
The Trends (in the Periodic Table) are the same
increases from left to right
increases from bottom to top
Electronegativity
The most active metals have the lowest
electronegativity
The most active nonmetals have the highest
electronegativity
Nuclear Charge
As the positive charge of the nucleus
increases, it becomes increasingly
harder to remove an electron from an
outer shell
Tends to raise the First Ionization Energy
Shielding Effect
The effect when “inner” electrons block the
attraction of the nucleus for the outer
electrons
Tends to lower the First Ionization Energy
Radius
Ionization energy is inversely proportional to the
distance between the nucleus and the outer
electrons
Tends to lower the First Ionization Energy
Sublevel
An electron from a full or half-full sublevel requires
additional energy to be removed
If a sublevel is full or half-filled, then this tends to
raise the First Ionization Energy
Electron Affinity
The attraction an isolated atom has for an
additional electron
Shows the same trend as First Ionization
Energy (increases from left to right, and
decreases from the top down).
Oxidation Numbers
Group 1
lose 1 electron
+1
Group 2
lose 2 electrons
+2
Group 3-12
multiple gain/loss
Group 13 lose 3 electrons
+3
Group 14 lose/gain 2,4 electrons
±4, +2
Group 15 gain 3 electrons
-3
Group 16 gain 2 electrons
-2
Group 17 gain 1 electron
-1
Group 18 stable
0
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LEO says GER
Warm Up
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What is the oxidation number for group 1?
What is the oxidation number for group 2?
What is the oxidation number for group 3?
What is the oxidation number for group 15?
What is the oxidation number for group 16?
What is the oxidation number for group 17?
What is the oxidation number for group 18?
Name the following groups: 1, 2, 16,17 and 18.
Web Activity
http://www.learner.org/interacti
ves/periodic/groups_interactive
.html