december 16, 2013(o)
DESCRIPTION
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? How many atoms in 0.200 grams of carbon? - PowerPoint PPT PresentationTRANSCRIPT
December 16, 2013 (O)1. Dalton is important because…2. Lavoisier is important because…3. Proust is important because…4. Boyle is important because…5. Draw a model of Rutherford’s setup6. 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.
December 16, 2013 (O)1. Review for final
HOMEWORK:2. Continue studying for final3. Have a calculator for final4. 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 ConfigurationHow do we know which are the valence electrons?
Has the highest n value, the principle quantum number
2. Electron ConfigurationWrite FULL electron configuration for Silicon, Si
2. Electron ConfigurationWrite FULL electron configuration for Silicon, Si
Si = 1s22s22p63s23p2
2. Electron ConfigurationWrite FULL electron configuration for Silicon, Si
Si = 1s22s22p63s23p2
2. Electron ConfigurationWrite FULL electron configuration for Germanium, Ge
2. Electron ConfigurationWrite FULL electron configuration for Germanium, Ge
Ge = 1s22s22p63s23p24s23d104p2
4 valence electrons
2. Electron Configuration1. Write electron configurations for the following
2. Underline the valence electrons
Barium Carbon Nitrogen Oxygen Fluorine Neon
Aluminum Tin Phosphorus Tellurium Chlorine Krypton
2. Electron Configuration1. Write electron configurations for the following
2. Underline the valence electrons
Barium
[Xe]6s2
Carbon
[He]2s22p2
Nitrogen
[He]2s22p3
Oxygen
[He]2s22p4
Fluorine
[He]2s22p5
Neon
[He]2s22p6
Aluminum Tin Phosphorus Tellurium Chlorine Krypton
2. Electron ConfigurationHow many valence electrons do you predict the last row will
have?
Do you notice a pattern?
Barium Carbon Nitrogen Oxygen Fluorine Neon
Aluminum Tin Phosphorus Tellurium Chlorine Krypton
Indium Silicon Arsenic Selenium Bromine Argon
2. Electron ConfigurationHow many valence electrons do you predict the last row will
have?
Do you notice a pattern?
Barium Carbon Nitrogen Oxygen Fluorine Neon
Aluminum Tin Phosphorus Tellurium Chlorine Krypton
Indium Silicon Arsenic Selenium 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 ConfigurationClasswork:
Workbook page 18, # 1-12Write the term
Then the letter AND phrase in your answers. You may summarize by just writing keywordsYou DO NOT have to write the entire phrase
Thomson Rutherford Bohr Schrodinger
Name of Model Nuclear Model Solar System
Drawing
Significance Electrons travel in quantized orbits
1. What can the Quantum Model of the atom show us?
2. What is an orbit and what is an orbital?3. Complete Table4. Textbook page 99, #3,4,5,6,7,95. Turn in
Thomson Rutherford Bohr Schrodinger
Name of Model Nuclear Model Solar System
Drawing
Significance Electrons travel in quantized
orbits
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 TableBrief History of the Table
• Just like class activity, different versions• 1860 - John Newlands & Octaves
3. Trendy TableBrief 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 TableBrief History of the Table
• Just like class activity, different versions• 1860 - John Newlands & Octaves• 1869 – Dimitri Mendeleev• 1913 – J. Moseley & Protons & Atomic #
3. Trendy TableBrief 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 TableBrief History of the Table
Classwork: Textbook pg 122, #2,5,6,7,8
Define the following1. Period2. Group3. Periodic Law4. Atomic Radius5. Bond Radius6. Ionization Energy7. Electronegativity
3. Trendy TableBrief History of the Table
Classwork: Textbook pg 122, #2,5,6,7,8
Define the following1. Period2. Group3. Periodic Law
3. Trendy TableBrief 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
Barium Carbon Nitrogen Oxygen Fluorine Neon
Aluminum Tin Phosphorus Tellurium Chlorine Krypton
3. Trendy TableBrief 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
Barium
[Xe]6s2
Carbon
[He]2s22p2
Nitrogen
[He]2s22p3
Oxygen
[He]2s22p4
Fluorine
[He]2s22p5
Neon
[He]2s22p6
Aluminum Tin Phosphorus Tellurium Chlorine Krypton
Indium Silicon Arsenic Selenium Bromine Argon
3. Trendy TableBrief 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
Barium
[Xe]6s2
Carbon
[He]2s22p2
Nitrogen
[He]2s22p3
Oxygen
[He]2s22p4
Fluorine
[He]2s22p5
Neon
[He]2s22p6
Aluminum Tin Phosphorus Tellurium Chlorine Krypton
3. Trendy TableBrief History of the Table
Workbook pg 23, #2-5Answer in complete sentences.
Define the following1. Period2. Group3. Periodic Law4. Atomic Radius5. Bond Radius6. Ionization Energy7. Electronegativity
3. Trendy TableBrief History of the Table
• Just like class activity, different versions• 1860 - John Newlands & Octaves• 1869 – Dimitri Mendeleev• 1913 – J. Moseley & Protons & Atomic #
Classwork: Workbook pg 23, #2-5Answer in complete sentences.
Thomson Rutherford Bohr Schrodinger
Name of Model Nuclear Model Solar System
Drawing
Significance Electrons move in quantized
orbits
3. Trendy TablePeriodic Trends
How would you define “pattern”?How would you define “trend”?
3. Trendy TablePeriodic Trends
Objective: To recognize patterns in the PT
3. Trendy TablePeriodic Trends
Objective: To recognize patterns in the PT
3 Patterns1. Atomic Radius
2. Ionization Energy3. Electronegativity
3. Trendy TablePeriodic Trends
First, some important terms
1. Period: 2. Group:3. Periodic Law:
3. Trendy TablePeriodic Trends
First, some important terms
1. Period: 2. Group:3. Periodic Law:
3. Trendy TablePeriodic Trends
First, some important terms
1. Period: Horizontal row of elements
3. Trendy TablePeriodic Trends
First, some important terms
1. Period: elements in a period occupy SAME ENERGY LEVEL
3. Trendy TablePeriodic Trends
First, some important terms
Group: vertical column of elements
3. Trendy TablePeriodic Trends
First, some important terms
Periodic Law: predictable patterns when elements arranged by atomic number
3. Trendy TablePeriodic Trends
First, some important terms
Periodic Law: predictable patterns reoccur when elements arranged by atomic number
Patterns of what?
3. Trendy TablePeriodic Trends
Objective: To recognize patterns in the PT
3 Patterns1. Atomic Radius
2. Ionization Energy3. Electronegativity
3. Trendy TablePeriodic Trends
3 Patterns1. Atomic Radius
2. Ionization Energy3. Electronegativity
Atomic Radius
Ionization Energy
Electronegativity
Period INCREASES INCREASES INCREASES
Row INCREASES INCREASES INCREASES
3. Trendy TablePeriodic Trends
1st Pattern or Trend
Atomic Radii – Size of Atom
3. Trendy Table1st Pattern or Trend
Atomic Radii – Size of Atom
3. Trendy TablePeriodic 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 TablePeriodic Trends
Atomic Radii – Size of Atom
1. Period: Horizontal row of elements
3. Trendy TablePeriodic 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 TablePeriodic Trends
Atomic Radii – Size of Atom
WHY?Because of
Electron Shielding and
Nuclear Charge
3. Trendy TablePeriodic Trends
Atomic Radii – Size of Atom
WHY?Because of
Electron Shielding is when… Valence electrons are shielded by the core
electrons
3. Trendy TablePeriodic Trends
Atomic Radii – Size of Atom
3. Trendy TablePeriodic Trends
Atomic Radii – Size of Atom
1. Period: Horizontal row of elements
3. Trendy TablePeriodic Trends
Atomic Radii – Size of Atom
3. Trendy TablePeriodic Trends
Atomic Radii – Size of Atom
WHY?Because of
Electron Shielding is when… Valence electrons are shielded by the core
electrons
3. Trendy TablePeriodic Trends
Atomic Radii – Size of Atom
WHY?Because of
Electron Shielding is when… Valence electrons are shielded by the core
electronsFILLED inner orbitals shield electrons in the
outer orbitals
3. Trendy TablePeriodic Trends
Atomic Radii – Size of Atom
WHY?Because of Valence Electrons and filled Valence Orbitals
Atomic radius determined by valence electrons
3. Trendy TablePeriodic Trends
Atomic Radii – Size of Atom
Electron Shielding
3. Trendy TablePeriodic Trends
3 Patterns1. Atomic Radius
2. Ionization Energy3. Electronegativity
Atomic Radius
Ionization Energy
Electronegativity
Period INCREASES INCREASES INCREASES
Row INCREASES INCREASES INCREASES
3. Trendy TablePeriodic Trends
3 Patterns1. Atomic Radius
2. Ionization Energy3. Electronegativity
Atomic Radius
Ionization Energy
Electronegativity
Period INCREASES INCREASES INCREASES
Row INCREASES INCREASES INCREASES
3. Trendy TablePeriodic Trends
3 Patterns1. Atomic Radius
2. Ionization Energy3. Electronegativity
Atomic Radius
Ionization Energy
Electronegativity
Period INCREASES INCREASES INCREASES
Row INCREASES INCREASES INCREASES
3. Trendy TablePeriodic Trends
Atomic Radii – Size of Atom
3. Trendy Table
Arrange by radius from smallest to largest1. Calcium, Magnesium, Hydrogen2. Gold, Arsenic Radon3. Carbon, Cesium, Copper, Helium, Iron,
Potassium
3. Trendy TablePeriodic Trends
3 Patterns1. Atomic Radius
2. Ionization Energy3. Electronegativity
Atomic Radius
Ionization Energy
Electronegativity
Period INCREASES INCREASES INCREASES
Row INCREASES INCREASES INCREASES
3. Trendy TablePeriodic Trends
2nd Trend: First Ionization Energy
3. Trendy TablePeriodic Trends
2nd Trend: First Ionization Energy
What is this?
3. Trendy TablePeriodic Trends
2nd Trend: First Ionization Energy
What is this?
Energy needed to remove an electron from an atom
3. Trendy TablePeriodic 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 TablePeriodic 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 orbitalAll elements want to be NOBLE
3. Trendy Table2nd Trend: First Ionization Energy
3. Trendy Table2nd Trend: First Ionization Energy
3. Trendy Table2nd Trend: First Ionization Energy
3. Trendy TablePeriodic Trends
3 Patterns1. Atomic Radius
2. Ionization Energy3. Electronegativity
Atomic Radius
Ionization Energy
Electronegativity
Period INCREASES INCREASES INCREASES
Row INCREASES INCREASES INCREASES
3. Trendy Table2nd Trend: First Ionization Energy
Arrange from lowest to greatest1. Cesium, Helium, Gold2. Calcium, Copper, Potassium3. Arsenic, Carbon, Cesium, Iron,
Magnesium
3. Trendy TablePeriodic Trends
3rd Trend: Electronegativity
What is this?
3. Trendy TablePeriodic Trends
3rd Trend: Electronegativity
What is this?
Electronegativity is the ability to attract electrons when making compounds
3. Trendy Table3rd Trend: Electronegativity
3. Trendy Table3rd Trend: Electronegativity
3. Trendy Table3rd Trend: Electronegativity
3. Trendy TablePeriodic Trends
3 Patterns1. Atomic Radius
2. Ionization Energy3. Electronegativity
Atomic Radius
Ionization Energy
Electronegativity
Period INCREASES INCREASES INCREASES
Row INCREASES INCREASES INCREASES
3. Trendy Table
Arr
3rd Trend: Electronegativity
Arrange from lowest to greatest electronegativity1. Cesium, Helium, Radon2. Arsenic, Copper, Gold3. Calcium, Carbon, Iron, Magnesium, Potassium
3. Trendy TableAll 3 Trends
3. Trendy TableAll 3 Trends
3. Trendy TableAll 3 Trends
Review for FinalFrom latest section
Know:Bohr
GroupsPeriod
Periodic LawValence electronsOrbital diagrams
Types of orbitals, and how many e in each?Electron configurations
Patterns for 3 trendsHund, Aufbau, Pauli
Review for FinalGreen 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 theelectrons in its outermost orbital,