December 16, 2013 (O)
Dalton is important because…
Lavoisier is important because…
Proust is important because…
Boyle is important because…
Draw a model of Rutherford’s setup
What is the mass in grams of 500. atoms of
iron?
7. How many atoms in 0.200 grams of carbon?
8. Write electron configuration, draw orbital
diagram, and underline valence electrons for
cobalt.
1.
2.
3.
4.
5.
6.
December 16, 2013 (O)
1. Review for final
HOMEWORK:
1. Continue studying for final
2. Have a calculator for final
3. Periodic Table provided
2. Electron Configuration
Hydrogen Comp Simulation
2. Electron Configuration
Valence Electrons
2. Electron Configuration
What are valence electrons?
2. Electron Configuration
What are valence electrons?
electrons in its outermost orbital are
called the
valence electrons
2. Electron Configuration
How do we know which are the valence electrons?
Has the highest n value, the principle quantum number
2. Electron Configuration
Write FULL electron configuration for Silicon, Si
2. Electron Configuration
Write FULL electron configuration for Silicon, Si
Si = 1s22s22p63s23p2
2. Electron Configuration
Write FULL electron configuration for Silicon, Si
Si = 1s22s22p63s23p2
2. Electron Configuration
Write FULL electron configuration for Germanium, Ge
2. Electron Configuration
Write FULL electron configuration for Germanium, Ge
Ge = 1s22s22p63s23p24s23d104p2
4 valence electrons
2. Electron Configuration
1. Write electron configurations for the following
2. Underline the valence electrons
Barium
Carbon
Aluminum
Tin
Nitrogen
Oxygen
Phosphorus Tellurium
Fluorine
Neon
Chlorine
Krypton
2. Electron Configuration
1. Write electron configurations for the following
2. Underline the valence electrons
Barium
Carbon
Nitrogen
Oxygen
Fluorine
Neon
[Xe]6s2
[He]2s22p2
[He]2s22p3
[He]2s22p4
[He]2s22p5
[He]2s22p6
Aluminum
Tin
Phosphorus
Tellurium
Chlorine
Krypton
2. Electron Configuration
How many valence electrons do you predict the last row will
have?
Barium
Carbon
Aluminum
Tin
Indium
Silicon
Nitrogen
Oxygen
Phosphorus Tellurium
Arsenic
Selenium
Do you notice a pattern?
Fluorine
Neon
Chlorine
Krypton
Bromine
Argon
2. Electron Configuration
How many valence electrons do you predict the last row will
have?
Barium
Carbon
Aluminum
Tin
Indium
Silicon
Nitrogen
Oxygen
Phosphorus Tellurium
Arsenic
Selenium
Do you notice a pattern?
Fluorine
Neon
Chlorine
Krypton
Bromine
Argon
2. Electron Configuration
EXAMPLE:
Sodium 1s22s22p63s1 = [Ne]3s1
Lithium 1s22s1 = [He]2s1
This pattern is seen in columns 1-2 and 13-18 of the PT
What other patterns might exist within the PT?
Maybe there is a reason why the PT has that weird shape!
2. Electron Configuration
How do you identify the valence electrons?
2. Electron Configuration
Classwork:
Thomson
Name of Model
Rutherford
Bohr
Nuclear Model
Solar System
Schrodinger
Drawing
Significance
Electrons travel in
quantized orbits
Workbook page 18, # 1-12
Write the term
Then the letter AND phrase in your answers.
You may summarize by just writing keywords
You DO NOT have to write the entire phrase
1. What can the Quantum Model of the atom show
us?
2. What is an orbit and what is an orbital?
3. Complete Table
4. Textbook page 99, #3,4,5,6,7,9
5. Turn in
Thomson
Name of Model
Rutherford
Bohr
Nuclear Model
Solar System
Drawing
Significance
Electrons travel in
quantized orbits
Schrodinger
3. Trendy Table
The Periodic Table and its Trends
OBJECTIVE: Understand how the Periodic Table
is organized.
3. Trendy Table
Periodic Table
What is it?
3. Trendy Table
Periodic Table
What is it?
• a tool
• organizes information
• NOT something to memorize
• instead, learn how to use the organized
information
•See page or back of textbook
3. Trendy Table
Main Question
• How to best organize all the different
elements?
3. Trendy Table
3. Trendy Table
3. Trendy Table
3. Trendy Table
3. Trendy Table
Main Question
• How to best organize all the different
elements?
• Handout
3. Trendy Table
Main Question
• How to best organize all the different
elements?
• So a quick history…
3. Trendy Table
Brief History of the Table
• Just like class activity, different versions
• 1860 - John Newlands & Octaves
3. Trendy Table
Brief History of the Table
• Just like class activity, different versions
• 1860 - John Newlands & Octaves
3. Trendy Table
Brief History of the Table
• Just like class activity, different versions
• 1860 - John Newlands & Octaves
• 1869 – Dimitri Mendeleev
3. Trendy Table
• 1869 – Dimitri Mendeleev
3. Trendy Table
• 1869 – Dimitri Mendeleev
3. Trendy Table
• 1869 – Dimitri Mendeleev
•
•
Arranged elements into rows by atomic mass.
Arranged columns by chemical property
•
Ingenious design = left blanks, did not assume we
discovered all elements. Able to ACCURATELY
predict properties of undiscovered elements.
3. Trendy Table
Brief History of the Table
•
•
•
•
Just like class activity, different versions
1860 - John Newlands & Octaves
1869 – Dimitri Mendeleev
1913 – J. Moseley & Protons & Atomic #
3. Trendy Table
•
•
•
•
Brief History of the Table
Just like class activity, different versions
1860 - John Newlands & Octaves
1869 – Dimitri Mendeleev
1913 – J. Moseley & Protons & Atomic #
Classwork: Textbook pg 122, #2,5,6,7,8
3. Trendy Table
Brief History of the Table
Classwork: Textbook pg 122, #2,5,6,7,8
Define the following
1.
2.
3.
4.
5.
6.
7.
Period
Group
Periodic Law
Atomic Radius
Bond Radius
Ionization Energy
Electronegativity
3. Trendy Table
Brief History of the Table
Classwork: Textbook pg 122, #2,5,6,7,8
Define the following
1. Period
2. Group
3. Periodic Law
3. Trendy Table
Barium
Carbon
Nitrogen
Fluorine
Neon
Brief History
ofOxygen
the Table
• Just like class activity, different versions
•
1860
John
Newlands
&
Octaves
Aluminum
Tin
Phosphorus Tellurium
Chlorine
Krypton
• 1869 – Dimitri Mendeleev
• 1913 – J. Moseley & Protons & Atomic #
Classwork: Textbook pg 122, #2,5,6,7,8
3. Trendy Table
Barium
Nitrogen
Fluorine
Neon
Brief History
ofOxygen
the Table
2
2
22p3
22p4
22p5
[Xe]6s
[He]2s
[He]2s
[He]2s
[He]2s
[He]2s22p6
• Just
like22p
class
activity,
different
versions
• 1860 - John Newlands & Octaves
Aluminum
Phosphorus
Tellurium
Chlorine
Krypton
• 1869 –TinDimitri
Mendeleev
• 1913 – J. Moseley & Protons & Atomic #
Indium
Carbon
Silicon
Arsenic
Selenium
Bromine
Argon
Classwork: Textbook pg 122, #2,5,6,7,8
3. Trendy Table
Barium
Carbon
Nitrogen
Fluorine
Neon
Brief History
ofOxygen
the Table
2
2
22p3
22p4
22p5
[Xe]6s
[He]2s
[He]2s
[He]2s
[He]2s
[He]2s22p6
• Just
like22p
class
activity,
different
versions
• 1860 - John Newlands & Octaves
Aluminum
Phosphorus
Tellurium
Chlorine
Krypton
• 1869 –TinDimitri
Mendeleev
• 1913 – J. Moseley & Protons & Atomic #
Classwork: Textbook pg 122, #2,5,6,7,8
3. Trendy Table
1.
2.
3.
4.
5.
6.
7.
Brief History of the Table
Workbook pg 23, #2-5
Answer in complete sentences.
Define the following
Period
Group
Periodic Law
Atomic Radius
Bond Radius
Ionization Energy
Electronegativity
3. Trendy Table
Thomson
Rutherford
Bohr
Brief
History
of the Table
Name of Model
Nuclear Model
Schrodinger
Solar System
• Just like class activity, different versions
Drawing
• 1860 - John Newlands & Octaves
• Significance
1869 – Dimitri Mendeleev Electrons move
in quantized
• 1913 – J. Moseley & Protons
& Atomic #
orbits
Classwork: Workbook pg 23, #2-5
Answer in complete sentences.
3. Trendy Table
Periodic Trends
How would you define “pattern”?
How would you define “trend”?
3. Trendy Table
Periodic Trends
Objective: To recognize patterns in the PT
3. Trendy Table
Periodic Trends
Objective: To recognize patterns in the PT
3 Patterns
1. Atomic Radius
2. Ionization Energy
3. Electronegativity
3. Trendy Table
Periodic Trends
First, some important terms
1. Period:
2. Group:
3. Periodic Law:
3. Trendy Table
Periodic Trends
First, some important terms
1. Period:
2. Group:
3. Periodic Law:
3. Trendy Table
Periodic Trends
First, some important terms
1. Period: Horizontal row of elements
3. Trendy Table
Periodic Trends
First, some important terms
1. Period: elements in a period occupy
SAME ENERGY LEVEL
3. Trendy Table
Periodic Trends
First, some important terms
Group: vertical column of elements
3. Trendy Table
Periodic Trends
First, some important terms
Periodic Law: predictable patterns when
elements arranged by atomic number
3. Trendy Table
Periodic Trends
First, some important terms
Periodic Law: predictable patterns reoccur
when elements arranged by atomic
number
Patterns of what?
3. Trendy Table
Periodic Trends
Objective: To recognize patterns in the PT
3 Patterns
1. Atomic Radius
2. Ionization Energy
3. Electronegativity
3. Trendy Table
Periodic Trends
3 Patterns
1. Atomic Radius
2. Ionization Energy
3. Electronegativity
Atomic
Radius
Ionization
Energy
Electronegativity
Period
INCREASES
INCREASES
INCREASES
Row
INCREASES
INCREASES
INCREASES
3. Trendy Table
Periodic Trends
1st Pattern or Trend
Atomic Radii – Size of Atom
3. Trendy Table
1st Pattern or Trend
Atomic Radii – Size of Atom
3. Trendy Table
Periodic Trends
1st Pattern or Trend
Atomic Radii – Size of Atom
As you go down a group, the number of
electrons _______
As you go across a period, from left to
right, the number of electrons ______
3. Trendy Table
Periodic Trends
Atomic Radii – Size of Atom
1. Period: Horizontal row of elements
3. Trendy Table
Periodic Trends
Atomic Radii – Size of Atom
So, as you go down a period, atomic radii
______.
As you go across a period…wait
WHY?
3. Trendy Table
Periodic Trends
Atomic Radii – Size of Atom
WHY?
Because of
Electron Shielding
and
Nuclear Charge
3. Trendy Table
Periodic Trends
Atomic Radii – Size of Atom
WHY?
Because of
Electron Shielding is when…
Valence electrons are shielded by the core
electrons
3. Trendy Table
Periodic Trends
Atomic Radii – Size of Atom
3. Trendy Table
Periodic Trends
Atomic Radii – Size of Atom
1. Period: Horizontal row of elements
3. Trendy Table
Periodic Trends
Atomic Radii – Size of Atom
3. Trendy Table
Periodic Trends
Atomic Radii – Size of Atom
WHY?
Because of
Electron Shielding is when…
Valence electrons are shielded by the core
electrons
3. Trendy Table
Periodic Trends
Atomic Radii – Size of Atom
WHY?
Because of
Electron Shielding is when…
Valence electrons are shielded by the core
electrons
FILLED inner orbitals shield electrons in the
outer orbitals
3. Trendy Table
Periodic Trends
Atomic Radii – Size of Atom
WHY?
Because of
Valence Electrons and filled Valence Orbitals
Atomic radius determined by valence
electrons
3. Trendy Table
Periodic Trends
Atomic Radii – Size of Atom
Electron Shielding
3. Trendy Table
Periodic Trends
3 Patterns
1. Atomic Radius
2. Ionization Energy
3. Electronegativity
Atomic
Radius
Ionization
Energy
Electronegativity
Period
INCREASES
INCREASES
INCREASES
Row
INCREASES
INCREASES
INCREASES
3. Trendy Table
Periodic Trends
3 Patterns
1. Atomic Radius
2. Ionization Energy
3. Electronegativity
Atomic
Radius
Ionization
Energy
Electronegativity
Period
INCREASES
INCREASES
INCREASES
Row
INCREASES
INCREASES
INCREASES
3. Trendy Table
Periodic Trends
3 Patterns
1. Atomic Radius
2. Ionization Energy
3. Electronegativity
Atomic
Radius
Ionization
Energy
Electronegativity
Period
INCREASES
INCREASES
INCREASES
Row
INCREASES
INCREASES
INCREASES
3. Trendy Table
Periodic Trends
Atomic Radii – Size of Atom
3. Trendy Table
Arrange by radius from smallest to largest
1. Calcium, Magnesium, Hydrogen
2. Gold, Arsenic Radon
3. Carbon, Cesium, Copper, Helium, Iron,
Potassium
3. Trendy Table
Periodic Trends
3 Patterns
1. Atomic Radius
2. Ionization Energy
3. Electronegativity
Atomic
Radius
Ionization
Energy
Electronegativity
Period
INCREASES
INCREASES
INCREASES
Row
INCREASES
INCREASES
INCREASES
3. Trendy Table
Periodic Trends
2nd Trend: First Ionization Energy
3. Trendy Table
Periodic Trends
2nd Trend: First Ionization Energy
What is this?
3. Trendy Table
Periodic Trends
2nd Trend: First Ionization Energy
What is this?
Energy needed to remove an electron from
an atom
3. Trendy Table
Periodic Trends
2nd Trend: First Ionization Energy
What is this?
Energy needed to remove an electron from
an atom
A FILLED orbital is a happy and stable
orbital
3. Trendy Table
Periodic Trends
2nd Trend: First Ionization Energy
What is this?
Energy needed to remove an electron from
an atom
A filled orbital is a happy and stable orbital
All elements want to be NOBLE
3. Trendy Table
2nd Trend: First Ionization Energy
3. Trendy Table
2nd Trend: First Ionization Energy
3. Trendy Table
2nd Trend: First Ionization Energy
3. Trendy Table
Periodic Trends
3 Patterns
1. Atomic Radius
2. Ionization Energy
3. Electronegativity
Atomic
Radius
Ionization
Energy
Electronegativity
Period
INCREASES
INCREASES
INCREASES
Row
INCREASES
INCREASES
INCREASES
3. Trendy Table
2nd Trend: First Ionization Energy
Arrange from lowest to greatest
1. Cesium, Helium, Gold
2. Calcium, Copper, Potassium
3. Arsenic, Carbon, Cesium, Iron,
Magnesium
3. Trendy Table
Periodic Trends
3rd Trend: Electronegativity
What is this?
3. Trendy Table
Periodic Trends
3rd Trend: Electronegativity
What is this?
Electronegativity is the ability to attract
electrons when making compounds
3. Trendy Table
3rd Trend: Electronegativity
3. Trendy Table
3rd Trend: Electronegativity
3. Trendy Table
3rd Trend: Electronegativity
3. Trendy Table
Periodic Trends
3 Patterns
1. Atomic Radius
2. Ionization Energy
3. Electronegativity
Atomic
Radius
Ionization
Energy
Electronegativity
Period
INCREASES
INCREASES
INCREASES
Row
INCREASES
INCREASES
INCREASES
3. Trendy Table
3rd Trend: Electronegativity
Arr
Arrange from lowest to greatest electronegativity
1. Cesium, Helium, Radon
2. Arsenic, Copper, Gold
3. Calcium, Carbon, Iron, Magnesium, Potassium
3. Trendy Table
All 3 Trends
3. Trendy Table
All 3 Trends
3. Trendy Table
All 3 Trends
Review for Final
From latest section
Know:
Bohr
Groups
Period
Periodic Law
Valence electrons
Orbital diagrams
Types of orbitals, and how many e in each?
Electron configurations
Patterns for 3 trends
Hund, Aufbau, Pauli
Review for Final
Green Workbook
Chapter 4, page 21
#2, 3, 6-7, 12, 13
Chapter 3, page 16
#1-8, 10-11, 14, 16-20
Chapter 2, page 11
# 6-8
Chapter 1, page 6
#1, 3-5, 8, 10-12, 16, 19-20
2. Electron Configuration
Because of electron shielding, electrons in the inner orbitals are closer to
the nucleus and more tightly bound to it. So they are rarely involved in
chemical reactions.
This means that the chemistry of an atom depends mostly on the
electrons in its outermost orbital,