December 16, 2013(O)

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


Valence Electrons


What are valence electrons?


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


Si = 1s22s22p63s23p2


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


2. Electron ConfigurationHow many valence electrons do you predict the last row will

have?

Do you notice a pattern?



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?





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!


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



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


• Handout

3. Trendy Table

Main Question


• 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


• 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.


• 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



Define the following1. Period2. Group3. Periodic Law4. Atomic Radius5. Bond Radius6. Ionization Energy7. Electronegativity



Define the following1. Period2. Group3. Periodic Law









Barium

[Xe]6s2

Carbon

[He]2s22p2

Nitrogen

[He]2s22p3

Oxygen

[He]2s22p4

Fluorine

[He]2s22p5

Neon

[He]2s22p6






Barium

[Xe]6s2

Carbon

[He]2s22p2

Nitrogen

[He]2s22p3

Oxygen

[He]2s22p4

Fluorine

[He]2s22p5

Neon

[He]2s22p6



Workbook pg 23, #2-5Answer in complete sentences.

Define the following1. Period2. Group3. Periodic Law4. Atomic Radius5. Bond Radius6. Ionization Energy7. Electronegativity



Classwork: Workbook pg 23, #2-5Answer in complete sentences.



Drawing

Significance Electrons move in quantized

orbits

3. Trendy TablePeriodic Trends

How would you define “pattern”?How would you define “trend”?


Objective: To recognize patterns in the PT



3 Patterns1. Atomic Radius

2. Ionization Energy3. Electronegativity


First, some important terms

1. Period: 2. Group:3. Periodic Law:



1. Period: 2. Group:3. Periodic Law:



1. Period: Horizontal row of elements



1. Period: elements in a period occupy SAME ENERGY LEVEL



Group: vertical column of elements



Periodic Law: predictable patterns when elements arranged by atomic number



Periodic Law: predictable patterns reoccur when elements arranged by atomic number

Patterns of what?








Atomic Radius

Ionization Energy

Electronegativity

Period INCREASES INCREASES INCREASES

Row INCREASES INCREASES INCREASES


1st Pattern or Trend

Atomic Radii – Size of Atom

3. Trendy Table1st Pattern or Trend



1st Pattern or Trend


As you go down a group, the number of electrons _______

As you go across a period, from left to right, the number of electrons ______






So, as you go down a period, atomic radii ______.

As you go across a period…wait

WHY?



WHY?Because of

Electron Shielding and

Nuclear Charge



WHY?Because of

Electron Shielding is when… Valence electrons are shielded by the core

electrons










WHY?Because of


electrons



WHY?Because of


electronsFILLED inner orbitals shield electrons in the

outer orbitals



WHY?Because of Valence Electrons and filled Valence Orbitals

Atomic radius determined by valence electrons



Electron Shielding




Atomic Radius

Ionization Energy

Electronegativity






Atomic Radius

Ionization Energy

Electronegativity






Atomic Radius

Ionization Energy

Electronegativity





3. Trendy Table

Arrange by radius from smallest to largest1. Calcium, Magnesium, Hydrogen2. Gold, Arsenic Radon3. Carbon, Cesium, Copper, Helium, Iron,

Potassium




Atomic Radius

Ionization Energy

Electronegativity




2nd Trend: First Ionization Energy



What is this?



What is this?

Energy needed to remove an electron from an atom



What is this?


A FILLED orbital is a happy and stable orbital



What is this?


A filled orbital is a happy and stable orbitalAll elements want to be NOBLE

3. Trendy Table2nd Trend: First Ionization Energy






Atomic Radius

Ionization Energy

Electronegativity




Arrange from lowest to greatest1. Cesium, Helium, Gold2. Calcium, Copper, Potassium3. Arsenic, Carbon, Cesium, Iron,

Magnesium


3rd Trend: Electronegativity

What is this?



What is this?

Electronegativity is the ability to attract electrons when making compounds

3. Trendy Table3rd Trend: Electronegativity






Atomic Radius

Ionization Energy

Electronegativity



3. Trendy Table

Arr


Arrange from lowest to greatest electronegativity1. Cesium, Helium, Radon2. Arsenic, Copper, Gold3. Calcium, Carbon, Iron, Magnesium, Potassium

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


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,

December 16, 2013(O)

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