1. WARMUP Get out your phone. We are doing a kahoot.
Make sure you have your periodic table ready.
Completed tests are in FOCUS, so you can look up your grades quickly first if you haven’t already looked up your test grade. Bonus points from review are already added in.

2. We will use properties to determine unknown elements.
I will complete a Mendeleev activity.
Success Criteria
Know how properties are similar and how they vary within a group
Know periodic table trends.

3. Housekeeping
All the tests that have been completed have been graded and are entered in FOCUS. Bonus points for the test review have already been added.
If you haven’t already looked up your grades, you can look up your grades now. You have two minutes to complete this task.
All work from this unit needs to be turned in by Friday this week, 11/11.
Missing assignments are on the next slide. Make sure you turn in everything, especially the LAB!

4. We are going to do a 4-2-2 with this video.
Watch for 4 minutes.
Spend 2 minutes writing what you thought were the most important facts.
Share with your table partner for 2 minutes.

6. We are going to do a 4-2-2 with this video.
Watch for 4 minutes.
Spend 2 minutes writing what you thought were the most important facts.
Share with your table partner for 2 minutes.

7. Mendeleev Activity
You will work on this activity with your table partner. If you do not have a table partner, find another student who is partnerless to work with.
If there is an odd number of students, then we will need one group of three.
Everybody has to turn in their own paper.
The next page shows you how to lay out your cards.
Do not use your phone or your notes. Only use the information on the cards.

8. Set up your cards to match the table to the right
Set up your cards to match the table to the right. You will need to look at the trends you see in each group to determine where the unknowns go.
Do not write on the cards. They will be used for every class.
When you think you have the cards arranged in the right order, call me over to check.
Write your unknown #s in the correct spaces.

9. Work on answering questions for the activity for the next 15 minutes.
Do not use your phone or your notes. Only use the information on the cards.

10. 4-2-2 with another video
Don’t write any notes. Just pay attention to the video.
After the video is over, take 2 minutes to write down what you thought was important.
At the end of 2 minutes, share with your table partner. If you are sitting alone, then share with a table that is next to you.

12. 4-2-2
Take 2 minutes to write down on the whiteboard what you thought were the most important points. NO TALKING at this time.

13. 4-2-2 Spend two minutes sharing with your table partner.
We will take notes afterward.

14. New notes section
Title this section: Periodic Trends

15. Atomic Radius
How big an atom is.

16. Increase in atomic radius

17. Atomic Radius How big an atom is. Down a group - increases
adding new energy level makes atom bigger
Across a period - decreases
adding protons increases pull on e-, pulls them closer to nucleus

18. Which element has the largest atomic radius?
S Mg K O

19. Ionic Radius
How big an ion is.

20. Increase in ionic radius

21. Ionic Radius How big an ion is. Down a group -increases
valence e- are farther from nucleus
Across a period - decreases
valence e- are closer to nucleus

22. Which element has the largest ionic radius?
Li Ca O Rb

23. Ionization Energy
Amount of energy it takes to remove an electron (become an ion)

24. Increase in ionization energy

25. Ionization Energy
Amount of energy it takes to remove an electron (become an ion)
Down a group - decreases
valence e- are far from nucleus and easy to remove
Across a period - increases
more protons pull harder on valence e- and make them harder to remove

26. Which has a higher ionization energy, metals or nonmetals? Why?

27. Electron Affinity
Amount of energy it takes to gain an electron (opposite of ionization energy)
Down a group - decreases
because each atom is larger than the atom above it
Across a period - increases
Because each atom is smaller than the atom before it

28. Increase in electron affinity

29. Electronegativity
Strength of attraction an atom has to hold onto electrons

30. Increase in electronegativity

31. Electronegativity
Strength of attraction an atom has to hold onto electrons
Down a group - decreases force of attraction
valence e- are farther away from nucleus
Across a period - increases force of attraction
more protons have more strength to pull e-

32. Which element is the most electronegative?
S Mg K O

33. Metallic characteristics
How readily an atom can lose an electron.
Down a group - metallic characteristics increase
Electron shielding causes effective nuclear charge to increase so the outer electrons ionize more readily
Across a period - metallic characteristics decrease
Decrease in atomic radius means that outer electrons ionize more readily
Metallic character relates to the ability to lose electrons, and nonmetallic character relates to the ability to gain electrons.

34. Decrease in metallic character
Increase in metallic character

35. Shielding effect
The shielding effect describes the balance between the pull of the protons on valence electrons and the repulsion forces from inner electrons.
The shielding effect explains why valence-shell electrons are more easily removed from the atom. The effect also explains atomic size. The more shielding, the further the valence shell can spread out and the bigger atoms will be.
The effective nuclear charge is the net positive charge experienced by valence electrons. It can be approximated by the equation: Zeff = Z - S, where Z is the atomic number and S is the number of shielding electrons.
Source: Boundless. “ The Shielding Effect and Effective Nuclear Charge.” Boundless Chemistry. Boundless, 08 Aug Retrieved 06 Nov from effective-nuclear-charge /

36. HAVE A NICE DAY!
Put your notebook away. Work on any missing assignments.