1. PSAE Chemistry Review Part 2

2. Electrons Available for Bonding Are called __________ __________ The Electrons in the Outermost energy level Nucleus _______________ Slide 2

3. Electrons Available for Bonding Table Type #1: ROMAN NUMERALS Slide 3

4. Electrons Available for Bonding How Many Valence Electrons does each Element Have? Use the ___________ ___________ at the top of each Column. The Group Number tells you how Many Valence Electrons. Group Numbers Slide 4

5. Electrons Available for Bonding Table Type #2: Groups Numbered 1 thru 18 123456789101112131415161718 Slide 5

6. Electrons Available for Bonding How Many Valence Electrons does each Element Have? 123456789101112131415161718 Slide 6 _________________: The Number tells you the # of ValenceElectrons. Groups _______________: Subtract ________ from the Group Number. The Remainder is the # of Valence Electrons.

7. How much does an Atom Weigh? Electron Cloud is____________ ______________ ___________ Almost________ ______________ of an Atom is in the Nucleus. Even though the Nucleus is only a very small part of the Atom Slide 7

8. How much does an Atom Weigh? 12 C Carbon 12.011 ________ _________ Equals the # of Protons & Equals the # of Electrons ___________________ Average Mass of all known _______________ Slide 8

9. How much does an Atom Weigh? Isotopes: Atoms of an element that have _____________ _____________. WHY do they have Different Masses? Because of a Different Number of ____________. ParticleMass (amu) Proton1 Neutron1 Electron0 Slide 9 Note: Almost ALL of the Mass is in the Protons and Neutrons.

10. How much does an Atom Weigh? Isotope Notation Mass Number Includes: # of ____________ & # of _____________ Atomic Number # of _________________ # Neutrons = Mass Number  Atomic Number Slide 10

11. How much does an Atom Weigh? Examples of Isotopes Carbon has three Isotopes: They are all carbon atoms, but with different numbers of Neutrons Carbon – 13 ___Neutrons Slide 11 Carbon – 14 ___Neutrons Carbon – 14 ___Neutrons

12. TransUranium Elements ________________________ not found in Nature Made by Smashing Different Atoms together with _____________ Accelerators Slide 12

13. States of Matter ______ ________ Slide 13

14. States of Matter Retains a ____________________________ rigid - particles locked into place Not easily ____________________________ little free space between particles Does not _____________________________ rigid - particles cannot move/slide past one another SOLID Slide 14

15. States of Matter LIQUID Assumes _________________ of the part of the _________________ which it occupies particles can move/slide past one another Not easily _____________________ little free space between particles Flows ________________________ particles can move/slide past one another Slide 15

16. States of Matter Assumes _____________ and volume of its container particles can move past one another ___________________ lots of free space between particles Flows ________________ particles can move past one another GAS Slide 16

17. States of Matter The word "PLASMA" was first applied to _________________. Plasma consists of a collection of _______________________ electrons and ions - atoms that have lost electrons. Energy is needed to strip electrons from atoms to make plasma. PLASMA Slide 17

18. Phase Changes a.k.a. CHANGES OF STATE Slide 18 _______________ ___________________ __________________ ______________ __________________ ____________________

19. Phase Change Diagrams Time Solid Changing to Liquid _____________ Solid Temperature Liquid Gas _____________  Temperature Remains _____________ During Phase Changes No Solid Remaining Liquid Changing To Gas No Gas Remaining *Temp Increasing Slide 19

20. Phase Change Diagrams Time Liquid Changing To Solid ______________ Solid Temperature Liquid Gas _____________  Temperature Remains _____________ During Phase Changes Gas Changing To Liquid *Temp Decreasing Slide 20

21. Kinetic Molecular Theory  _________________________________ ________ Kinds of Motion  Translation – __________________ from point A to point B.  Rotation – _______________ or _______________  Vibration – ____________ and Forth Movement Gases are in Constant Random Motion Visualizing Molecular Motion 1 Video Visualizing Molecular Motion (Many) Video Diffusion of Gases Video Slide 21

22. Gas Laws  Pressure is defined as The Force per Unit Area on a Surface Slide 22 ___ N/cm 2

23. Gas Laws  Pressure is defined as The Force per Unit Area on a Surface  Gas Molecules exert pressure on any surface with which they collide.  The More Gas Molecules in a Container – the Higher the Pressure.  Ex. Double the # of Particles – ___________________ 1.0 atm2.0 atm Slide 23

24. Gas Laws  The More Gas Molecules in a Container – the ________________  This is a Direct Relationship. (Directly Proportional) # of Particles (moles) Pressure (atm) Volume Must be Held Constant Slide 24

25. Gas Laws  Boyle’s Law: _____________________ Slide 25

26. Gas Laws  Boyle’s Law: P x V = Constant  When Pressure _______________ – Volume Decreases  When Volume Increases – Pressure ________________  This is an Inversely Proportional Relationship Slide 26 Temperature Must be Held Constant

27. Gas Laws  Charles’s Law:V  T = Constant  When Temperature Increases – Volume Increases  This is a Direct Relationship. (Directly Proportional) Volume (Liters) Temperature  C Slide 27 Pressure Must be Held Constant

28. Gas Laws  Gay-Lussac’s Law: _________________  When Temperature Increases – Pressure _______________  This is a Direct Relationship. (Directly Proportional) Pressure (atm) Temperature  C Slide 28 Volume Must be Held Constant

29. Gas Laws  STP Standard _______________ & ____________  Standard Temperature: ____ Degrees Celsius ( 0  C )  Standard Pressure: _____________________ ( 1 atm) Slide 29

30. Gas Laws  Temperature  Temperature: a measure of the Average Kinetic Energies of All Molecules in a Sample  Converting From Celsius Scale To Kelvin Scale Degrees Celsius(  C ) + 273 = Kelvins (K) Ex: _____________________________  Converting From Kelvin Scale To Celsius Scale Kelvins (K) – 273 = Degrees Celsius (  C ) Ex: _____________________________ Note: The Kelvin Temperature is ALWAYS HIGHER ! Slide 30