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Periodic Table Trends.

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Presentation on theme: "Periodic Table Trends."— Presentation transcript:

1 Periodic Table Trends

2 Objectives: I can review the properties of the periodic table Agenda for today:

3 Quiz Recap Homogeneous Mixture vs Heterogeneous Mixture Element vs compound Mass number, atomic number, # of neutrons ER relationship to Bohr model Using the handout Electron Configuration and Orbital diagrams

4 Utilizing the Chart

5 Quiz Correction Policy -Due by wednesday -Earn up to a 60% back

6 Lab Update -Shoes -Long pants -No droopy sleeves -safety contract due -Hair tied up, bring hair ties

7 Let’s Review the Periodic Table Properties -15 min to work, review it

8 Independent Practice -Read pg and -Take notes, on vocabulary/key terms/ideas -once finished pick up review sheet -Complete Review questions

9 Electron Configuration Battleship

10 Day 2 -Review Quiz -Lecture Review -what is the order game
-Review Wkshts -Electron Configuration Battleship HW: Due Thursday

11 Objectives: -I can order elements based on periodic trends - I can explain the key vocabulary associated with periodic trends

12 **Quiz Review **Lab reminder

13 Orbitals

14 Valence electrons **Goal of an element/atom **Octet: Noble gas ambitions when forming compound **Electron dot

15 Periodic Trend: A

16 Example: Lithium Fluorine

17 Independent Practice Name Orbital diagram Valence e- #
Electron dot structure Magnesium Carbon Nitrogen Iodine *Extra Practice Challenge Cesium *Extra Practice Challenge*

18 Ions ** Charged atom, not neutral **Differences in proton and electron numbers *Periodic Table: A

19 Cation VS Anion

20

21 Practice: Draw Orbital Diagrams
Chlorine Atom Chlorine Ion ( cation or anion ) ( charge: ) Argon

22 Electron Shielding -Occurs in electrons located between valence electrons and nucleus -Basically, as add more shells, attraction between nucleus and outer electrons decreases

23 Atomic Radius: -Measure from nucleus to outer electron cloud

24 Atomic Size Trend WHy Go across increase in electrons and protons, fill up orbital, higher attraction, shielding decreases Go down, shielding takes over, more space as fill up another level

25 ****How does the atomic radius compare?****
IONIC RADII -Cation: Smaller -Anion: Larger

26 Metallic Character: -How reactive a metal is… how likely it is to be involved in a reaction -Metals lose e- in chemical reactions -As go across, decrease in metallic character -As go down, increase in metallic character

27 Reactivity: Both Metals and Nonmetals
-As saw: Metals as go down increase in reactivity BUT Nonmetals: as go down, decrease in reactivity **nonmetals want to gain a electron rather than lose one

28 Ionization Energy

29 Ionization Energy - Energy required to remove an electron -As across, increase in value -As go down, decreases in value WHY?!?!?!?!?

30

31 Electronegativity -Ability to attract electrons -As go across, increase -As go down, decreases WHY?!?!?!?!?

32 Why does it have no values?

33 Finish Packet from yesterday
Review Worksheet -Will be collected for points, due tomorrow -If finish early, work on project Reminder: Lab day tomorrow: Hair up, Appropriate shoes and clothing

34 Break!! Electron Configuration Battleship


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