Catalyst 9/4/13 On your Catalyst Sheet, please answer the following questions: 1. What happens to...
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Transcript of Catalyst 9/4/13 On your Catalyst Sheet, please answer the following questions: 1. What happens to...
![Page 1: Catalyst 9/4/13 On your Catalyst Sheet, please answer the following questions: 1. What happens to ionization energy as you go down a group? 2. Sort from.](https://reader035.fdocuments.in/reader035/viewer/2022062421/56649d985503460f94a82fde/html5/thumbnails/1.jpg)
Catalyst 9/4/13
On your Catalyst Sheet, please answer the following questions:1. What happens to ionization energy as you go down a group?2. Sort from lowest to highest IE: P, S, Mg3. Sort from highest to lowest IE: Kr, He, Ne
![Page 2: Catalyst 9/4/13 On your Catalyst Sheet, please answer the following questions: 1. What happens to ionization energy as you go down a group? 2. Sort from.](https://reader035.fdocuments.in/reader035/viewer/2022062421/56649d985503460f94a82fde/html5/thumbnails/2.jpg)
Announcement #1
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 #2• 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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Homework Answers
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Steal Mr. Pan’s Wallet!
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Lecture 1.7 – Ionization Energy
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Today’s Learning Target
• 1.7 – I can define ionization energy 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 ionization energy?
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I. Nuclear Attraction• Negative electrons are attracted
towards the positive nucleus.
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II. Ionization Energy
• Ionization energy is the energy that is required to remove an electron.
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What are the trends for ionization energy?
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I. IE Trends
• As you move down a group, the IE decreases.
• As you move across a period, the IE increases.
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Why do these trends exist?
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I. Why IE Decreases Down a Group
• As you go down a group more orbits are added.
• Nuclear attraction becomes weaker due to more orbits shielding the nucleus
• IE decreases because less energy is required to remove an outer electron.
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![Page 19: Catalyst 9/4/13 On your Catalyst Sheet, please answer the following questions: 1. What happens to ionization energy as you go down a group? 2. Sort from.](https://reader035.fdocuments.in/reader035/viewer/2022062421/56649d985503460f94a82fde/html5/thumbnails/19.jpg)
Electron Shielding: Explained with a Lamp and Socks
![Page 20: Catalyst 9/4/13 On your Catalyst Sheet, please answer the following questions: 1. What happens to ionization energy as you go down a group? 2. Sort from.](https://reader035.fdocuments.in/reader035/viewer/2022062421/56649d985503460f94a82fde/html5/thumbnails/20.jpg)
II. Why IE 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 show an increased nuclear attraction for electrons.
• IE increases because more energy is required to remove an electron
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Class Example
• Order the elements from smallest to largest IE: potassium, cesium, lithium.
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Table Talk
• Order the elements from largest to smallest IE: Fluorine, Carbon, Oxygen.
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Stop and Jot
• Order the elements from smallest to largest IE: phosphorus, arsenic, nitrogen.
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SUMMARIZE
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White Board Races
![Page 27: Catalyst 9/4/13 On your Catalyst Sheet, please answer the following questions: 1. What happens to ionization energy as you go down a group? 2. Sort from.](https://reader035.fdocuments.in/reader035/viewer/2022062421/56649d985503460f94a82fde/html5/thumbnails/27.jpg)
1. Order the following elements from smallest IE to largest IE: Arsenic, Gallium, Germanium.
2. Which element has a larger IE: fluorine or selenium?
3. Which element has a smaller IE: Cesium or Astatine?
4. Why does germanium have a higher ionization energy than lead?
5. Why does silicon have a lower ionization energy than phosphorus?
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Exit Slip
1. Order these from smallest to largest ionization energy: O, F, N
2. Order these from smallest to largest ionization energy: Na, Li, Cs
3. In complete sentences explain why IE decreases as you go down a group.
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Closing Time• UNIT 1 EXAM NEXT
MONDAY/TUESDAY