catalyst 9/6/13 on your catalyst sheet, please answer the following questions: 1. what happens to...
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Catalyst 9/6/13
On your Catalyst Sheet, please answer the following questions:1. What happens to electronegativity (EN) or ionization energy (IE) as you go across a period?2. Sort from lowest to highest IE: Ba, Be, Ca3. Sort from highest to lowest EN: P, Ge ,O
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Announcement #1
• Homework 1.9 – Periodic Trends due TUESDAY
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Announcement #2
TURN IN YOUR COIN DENSITY LAB REPORT (if you haven’t already)
Deadline for credit: Monday 9/9 (Periods 1/3/5); Tuesday 9/10 (Periods 2/4)
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Announcement #3• UNIT 1 EXAM NEXT MONDAY (9/9) OR
TUESDAY (9/10) (WRITE DOWN IN AGENDA)
• COVERS EVERY LEARNING TARGET IN THIS UNIT (1.1 – 1.9)– 1.1 Intro to the Atom– 1.2 Development of Atomic Theory– 1.3 Periodic Table– 1.4 Bohr Models– 1.5 Element Families– 1.6 Metals/Semimetals/Nonmetals– 1.7, 1.8, 1.9 Ionization
Energy/Electronegativity/Atomic Radius
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Lecture 1.8 – Electronegativity
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Today’s Learning Targets
• 1.8 – I can define electronegativity and explain how it relates to the charge of the nucleus and the electron. I can explain how this trend changes as you move throughout the Periodic Table.
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What is electronegativity?
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I. Electronegativity
• Electronegativity (EN) is the measure of the ability of an atom to attract electrons.
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What are the trends for electronegativity?
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I. Electronegativity Trends• As you go down a group, the
electronegativity decreases.• As you go across a period, the
electronegativity increases.
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Class Example
• Order the elements from smallest to largest electronegativity: oxygen, beryllium, lithium,
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Table Talk
• Order the elements from largest to smallest electronegativity: chlorine, bromine, fluorine
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Stop and Jot
• Order the elements from smallest to largest electronegativity: silicon, aluminum, sulfur
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Why do these trends exist?
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I. Why Electronegativity Decreases Down a Group
• As you go down a group more orbits are added.
• EN decreases because the nucleus cannot attract electrons as well due to the larger distance.
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II. Why Electronegativity Increases Across a Period
• As you move across a period you add more protons and electrons within the same orbit.
• The larger amount of protons in the nucleus and electrons in orbit show an increased attraction, which leads to increased EN
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White Board Races
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Directions
• The 5 people in your team are the line of people in front and/or behind you
• The front person in each team will answer the 1st question on the whiteboard
• Once the first person shows me a correct answer, he or she will pass it back to the second person to answer the 2nd question
• The process repeats with the board being passed back
• For the 5th question, if you only have 4 people the last person has to run the board up to the person in front
• NO HELPING TEAMMATES
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Relay Race Problems
1. Which has a larger electronegativity: chlorine or silicon?
2. Which has a smaller electronegativity magnesium or calcium?
3. Put the following elements in order from smallest electronegativity to largest: B, F, N, O.
4. Put the following elements in order from smallest electronegativity to largest: N, As, Bi, P .
5. Why does bromine do a worse job of attracting electrons than fluorine?
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Tug of War
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Justify – TPS
• Explain why there was a difference between the nucleus and electron groups’ ability to win
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• What happened to the rope as more people were added to the “nucleus”?
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Lecture 1.9 – Atomic Radius
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Today’s Learning Targets
• 1.9 – I can define atomic radius and explain how it relates to the charge of the nucleus and the electron. I can explain how this trend changes as you move throughout the Periodic Table.
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What is atomic radius?
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I. Atomic Radius
• Atomic Radius – The distance from the center of the nucleus to the edge of the electron cloud
Outer edge of electron cloud
Nucleus
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What are the trends for atomic radii?
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I. Atomic Radius Trends
• Atomic radius increases as you go down a group
• Atomic radius decreases as you go across a period
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Why do these trends exist?
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I. Why Atomic Radius Increases Down a Group
• As you go down a group, more orbits are added.
• The atom becomes bigger in size and so the radius increases.
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II. Why Atomic Radius Decreases Across a Period
• As you move across a period, more protons are added to the nucleus.
• This means there is a larger nuclear attraction and a decrease in the radius.
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SUMMARIZE
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Pick a Side• I am going to project up numerous
statements• You must decide whether you agree
or disagree.• Failure to participate, excessive
talking or touching will result in consequences
• Be prepared to defend your response!
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Pick a Side Questions
1. Atomic radius is the distance from the center of the nucleus to the first electron orbit.
2. Atomic radius increases across a period and down a group.
3. Atomic radius decreases down a group because you are adding more electron orbits.
4. Atomic radius decreases across a period because there are less electrons in the same orbit.
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Pick a Side Questions (cont.)
5. Order the following from largest to smallest atomic radius: Ca, Se, Ni
- Answer: Se, Ni, Ca6. Order the following from largest to smallest atomic radius: O, Po, S
- Answer: O, S, Po7. Order the following from smallest to largest atomic radius: Cs, F, Ga
- Answer: F, Ga, Cs
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Putting it All Together!
• With your table, create a Venn Diagram of the 3 Periodic Trends that we have been studying (ionization energy, electronegativity, atomic radius)
• Your Venn Diagram must include:– The trend as you go across a
period and down a group.– The definition of each trend– How nuclear attraction impacts
each trend– How the number of orbits
impacts the trends– An example, using elements, of
how each trend changes across a period and down a group.
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Exit Ticket
1. Define any two of the following:Ionization energyElectronegativityAtomic radius
2. Order from largest to smallest electronegativity: Ca, Se, Ni
3. Order from smallest to largest atomic radius: O, Po, S