1. Atoms/Atomic Structure, PTE, Valence Electrons, Gravity, Bonding
Science 81
Mr. Mullett
October 18, 2017 –
Day 33 of 180
Atoms/Atomic Structure, PTE, Valence Electrons, Gravity, Bonding

2. Homework Vocabulary Quiz WTF by 10-20
Interview Questions, Answer and Practice
Concept Layer Due
Friday 10-20/23
Tough Nuggies

3. JogNog B 1 ymohamad8 372 2 Josephgmullett 304 3 lbeaulieu8 214
4 SethD14 199
5 KSantiago8 170
6 rlambert8 168
7 Eglynn8 159
8 rbrenzel8 135
9 AMetcalf8 113
10 Valeriy Z 80
11 Amanda G 70

4. JogNog D 1 RJ_Ruiz 330 2 Josephgmullett 304 3 angie_B 300
4 stevenvelazquez3 278
5 aliceanipko 232
6 Allison14 224
7 o_lawry
8 kirill K 180
9 juliasavoy13 172
10 budbud03 160
11 lizzylovestoflip 133

5. JogNog E 1 Livia14 615 2 Josephgmullett 304 3 cdarling8 238
4 lramos8 178
5 kgagnon8 143
6 islonka8 135
7 mlatshaw8 127
8sagar t 118
9 lbryon8 117
10 Drew K 96
11 mmcdaniel8 94

6. JogNog F 1 Josephgmullett 304 2 afontanilles8 298 3 AMontovani8 270
4 iromansms8 219
5 SReed8 113
6 jwilliams8 101
7 kaden_R8 92
8 jfiddler110 79
9 DRivera8 77
10 hMetcalf8 45
11 TCarey8sms 41

7. Objective Describe the structure and components of atoms
Use Physical and Chemical properties to id elements
Understand Physical and Chemical Changes
Understand how elements are arranged on the PTE

8. Agenda Concept Layer Introduction Bell Work & Journals
Lesson of the Day
Combining elements- Bonding
Characteristic Properties
Chem/Phys Properties & Changes
Endothermic, Exothermic
States of Matter
Concept Layer Introduction
C3, C4, C6, C7

9. Scale Sizes
To understand the atomic level, we must first delve into the scale of things.
Powers of Ten Video
C1a Exit Card
C1 Worksheet Down in Comp Lab

10. Scale Sizes Large Universe (Size_______________)
Light year (speed of light traveled/yr)
300,000 km/s or 185,000 miles/s
Just over 7 times around the Earth
9.467 x 10^12km or 5.83 x 10 ^12miles
Mostly made of Hydrogen (H, 75%), Helium (He, 25%), Oxygen (O, 0.0%)

11. Scale Sizes Small Atoms/Quarks/Strings (Size_____________) Angstroms
1 A = 10^-10 meters
Strings are theoretical

12. Notes - Atoms Structure Charges Nucleus Cloud Proton (Positive)
Electron (Negative)
Neutron (Neutral)
Examples

13. PTE A way to present the Elements in an order
PTE
A way to present the Elements in an order
Based upon Atomic # and Particle Numbers
Grouped by Valence Electrons

14. Journal Entry (12)
Where did all of these elements come from? Look to the stars.
After watching the video clip, please explain how elements are created.
Now let’s talk about humans

16. Journal Entry 13
Below are some models of Atoms found on the PTE. Looking at the images, what are some things you notice? Can you ID these elements? C D A B

17. Elements on the PTE Atomic # = # of Electrons/Protons
Atomic Mass = Added Protons and Neutrons
Protons ____
Neutrons ____
Electrons ____

18.
Valence Electrons
Number of Electrons in the element’s outer orbit/shell
2, 8, 18 to fill
“Happy” when full
Wanting to Share if not full 5

19. Journal Entry (10)
Knowing that the group number at the top of the columns represents the number of valence electrons, why is Helium in the #18 Column? What might be another way to describe this column?

20. Lewis Dot Structures
Using our understanding of Valence Electrons, we will now draw in the number of electrons an atom has by using the Lewis Dot Structures.
Copy the examples

21. Journal Entry (new)
So we know that there are electrons surrounding atoms (-), why do you think that atoms are still attracted to each other so much?
Hint – Mass relation
Neutron = Proton = Electron = /1838

22. Combining Atoms
When you combine atoms you can produce both Molecules as well as Compounds
Molecule – Made of either the same or different elements, smallest unit where it still exhibits the chemical properties of a compound
Compound – Made of two different elements
All compounds are molecules, but not all molecules are compounds

23. Compounds and Molecules
Molecule – single combination of atoms. 1 water molecule
Compound – multiple molecules Many water molecules

24. Solutions and Mixtures
Mixture – A combination of 2 or more substances that are not combined chemically, can be separated. Salt/Pepper.
Solution – A well mixed mixture, saltwater, cannot be separated physically.

25. Pure Substances
Pure Substance – Any substance that is free of contamination.
Pure Honey
Pure Hydrogen
Pure Water
Pure Copper
Pure Aluminum
If you add corn syrup to the honey, you no longer have pure honey. Pure alcohol could be ethanol, methanol or a mixture of different alcohols, but as soon as you add water (which is not an alcohol), you no longer have a pure substance. Got it?

26. TED TALK ON BONDING
Bonding
There are two types of bonds that occur often; Ionic and Covalent
Ionic Bond – Forms when one atom Gives up it’s electron (Metals and non metals)
Covalent Bond – Forms when two or more atoms Share an electron (Metals and Non Metals)
Metallic Bond – Forms when metals bond with other metals

27. Lewis Dot Structures
Using our understanding of Valence Electrons, we will now draw in the number of electrons an atom has by using the Lewis Dot Structures.
Copy the examples

28. Notes Characteristic Properties
Chemical or Physical Properties that are used to identify elements 
freezing/melting point, boiling/condensing point 
density 
magnetism
solubility

29. Journal Entry 15 (old) What do you think is happening in this video?
Why would the foil boat float on air?
Sulfur hexafluoride (SF6) = 6.17 g/L
Nitrogen (N2) = g/L
Oxygen (O2) =1.429 g/L

30. Notes
Chemical vs. Physical Properties
Chemical vs. Physical Changes

31. Physical Reaction/Change
changes affecting the form of a chemical substance, but not its chemical composition. You still have the same thing and usually you can change it back.
Examples:
Liquid water to Ice
Tree cut into smaller pieces
Shape
Size
Color
Volume

32. Chemical Reaction/Change
process that leads to the transformation of one set of chemical substances to another. You get something new, and invariably you can not change it back.
Examples:
Digested donuts
Wood to ash
Iron to rust
Statue of Liberty

33. Endo/Exo Thermic Reactions
Endothermic Reactions
When Energy Goes “In” to a reaction
Ice Cubes/Packs
Exothermic Reactions
When Energy comes “Out” during a reaction
Heat Packs, Matches

34. Conservation of Mass
When the Reactants equal the Products. Only in a closed system.
In an open System, there can be no containment of matter. Reactants might not equal Products.
Balancing Equations is a requirement of this Law.

35. Thermal Energy
Which object has more thermal energy? A B

36. Bell Work
Could you please put these states of matter in order from lowest energy to highest?
Solid
Gas
Plasma
Bose-Einstein Condensate
Liquid

37. Bell Work
Could you please put these states of matter in order according to the picture?
Solid
Gas
Liquid

38. Silly Putty
What do you think will happen?
A the ball will bounce
B the ball will shatter
C the ball will stick to the ground
D Not sure
Superliquids

39. Energy Terms
Insulator-Nature of material and it’s particles is resistant to absorbing Kinetic Energy

40. Energy Terms
Conductor-Nature of material and its particles transfers Kinetic Energy Easily!

41. Bose-Einstein, Solid, Liquid, Gas, Plasma.
All 5 Phases
Bose-Einstein, Solid, Liquid, Gas, Plasma.
All Based upon the Amount of KE

42. States of Matter There are Three Main States of Matter: Solid Liquid
Gas
However there are many states currently.

43. Solid States of Matter Particles arranged in definite order Vibrate
Close together

44. Liquid States of Matter Particles arranged in Random order
Slide past, attaching and releasing
Close together

45. Gas States of Matter Particles not arranged. Scattered, Random Fast
Very Spread out

46. Excited/ Ionized Gases
States of Matter
Other States:
Plasma-Lightening
Excited/ Ionized Gases

47. Other States of Matter Ordinary Temps Low Temps High Energy
Liquid Crystal States (Digital Watch) Mlcls pnt sm direc
Amorphous Solid (Glass, Rubber, Polystyrene)
Magnetically-ordered States (moments aligned 2 dif ways)
Low Temps
Superconductors (Cold Magnets –MRI)
Superfluids (Climbing helium 3 or 6)
Bose-Einstein Condensates (called “Fifth State” helium 4)
High Energy
Plasma (ionized gas lightning, stars, sun)
Quark-gluon Plasma (CERN 2000 Observe individual Quarks)
Proposed States
Degenerate Matter (White dwarves and Neutron Stars)
Supersolid (Solid with superfluid properties
String-net liquid (atoms have the same spin, not normal)
Rydberg Matter (condensation of excited atoms)

48. All 5 Phases

49. Other States of Matter
Solid
Liquid
Gas

50. Phase Changes

51. Temperature Scale

52. Silly Putty
What do you think will happen?
A the ball will bounce
B the ball will shatter
C the ball will stick to the ground
D Not sure
Superliquids

53. Temperature Conversions
Absolute Water Water Zero Freezes Boils F
C – K
Compare this to a Number line as in Math!

54. Phase Changes