1. FLASHBACK How many electrons do all atoms want in their outer shell?
How do these atoms get those e-’s in the outer shell?
How can you tell how many valence e-’s an atom has?
If atoms gain e-’s, they become ____________ charged.
If atoms lose e-’s, they become ____________ charged.

2. Chemical Reactions!! Unit 4 Ch. 20/21 3/28/2017 2:42 AM
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3. Chemical bonds: the attractive force that holds atoms or ions together
Chemical Vocab!!
Chemical bonds: the attractive force that holds atoms or ions together

4. Why do atoms bond?
To increase stability of the atoms Group 1 and 2 metals transfer electrons to Group 16 and 17 nonmetals to create ionic bonds. Metals lose electrons & nonmetals gain electrons to achieve noble gas structure!

5. Calcium ion will give up its outer electrons to both chlorine atoms
bonding
A bond forms when… two atoms gain, lose, or share electrons in their outer energy levels. -1 -1 Cl Cl
CaCl2 +2 Ca
Calcium ion will give up its outer electrons to both chlorine atoms

6. Ionic bond
Form between two oppositely charged ions (metal to nonmetal) one gains and one loses electrons (electron transfer) Br Br +2
MgBr2 Mg
Strong bonds form

7. Ionic vs. Covalent Video
covalent bond
Form when atoms share one or more pairs of electrons = nonmetals to nonmetals
Oxygen only needs two electrons so hydrogen shares its one valence electron so that both atoms fill their outer shells. O H
H2O H
Ionic vs. Covalent Video
Weaker bonds form

8. Electron dot Diagrams Shows only valence
electrons of atom with dots around the element's symbol
What’s the point?

9. Electron dot diagrams
P=1 H
1 e-
N=0 Ca
P=20
2 e-
8 e-
8 e-
2 e-
N=20

10. Electron dot diagrams Determine # of valence electrons
Correctly place the electrons around symbol
Nitrogen: N Strontium: Sr Water: H2O

11. FLASHBACK 1. What types of elements occupy space in groups 1 and 2?
2. How many valence e-’s do these groups have, respectively?
3. What will their ionic charges be, respectively, if they lose their valence e-’s?
4. Metals will _____________ e-’s.
5. Non-metals will ________________ e-’s.
6. What e-’s do the bonding?
7. Explain difference between ionic and covalent bonds.

12. Bonding Worksheet:
4. Na Cl
7. Be Ne
11. Mg
Covalent or ionic bond?
12. HCl_________________________
14. AlO3________________________
Using electron dot diagrams, draw the ionic bonds…
17. NaCl

13. Investigating the difference between sugar and salt!
Lab time!
Ionic vs. covalent...
Which will win???
Investigating the difference between sugar and salt!
Sugar!
Salt!

14. Who knew Chemical Bonding could be so cool????
Bonding Rap…
Who knew Chemical Bonding could be so cool????
Want to give it a try???
Extra Credit by the end of the 9 weeks (March 23th) for a Chemistry Rap Video!

15. Bonds Covalent Structures: make molecules and SHARE ELECTRONS
Example: H20, CO2, C12H22O11
same charges, so no strong attraction
Ionic Structures: make ionic crystals and TRANSFER ELECTRONS
Example: NaCl, KI, CaF2
+ and – charges make a STRONG attraction!

16. IONIC Structure
When positive and negative ions surround each other, they form tightly packed structures called ionic crystals or crystal lattices
Substances with network (ionic) structures are usually strong solids with high melting and boiling points
Substances made of molecules have lower melting and boiling points

17. Electron dot Diagrams
What happens if it is not the neutral element.. But the ion??
e- diagram lose or gain e-? new (ion) e- diagram Na Cl Mg

18. SECTION 1 REVIEW
Pg. 606 # 4, 5
CHAPTER REVIEW
Pg. 626 # 4-6, 11, 14, 17, 18

19. 1. Which of the substances has the lower melting point (which melted faster)? Was this what you expected? Why or why not?
2. Relate your results to ionic and covalent bonding.
3. On a molecular level, how do the bonds in sugar and salt differ?
4. Why do atoms bond?
5. Water (H2O) contains a(n) _________________ bond.
Calcium oxide (CaO) contains a(n) ________________ bond.

20. EOC WORKBOOK!!! Pg. 38 (all) Pg. 39 (all) Pg. 36 (all) Pg. 37 (all)
FLASHBACK
EOC WORKBOOK!!!
Pg. 38 (all)
Pg. 39 (all)
Pg. 36 (all)
Pg. 37 (all)

21. FLASHBACK 1. Table salt (NaCl) has what kind of bond?
2. Table sugar (sucrose, C12H22O11) has what kind of bond?
3. When heated, what happened to the bonds in sugar?
4. When heated, what happened to the bonds in salt?
5. Provide the electron dot structure for Barium (Ba), Iodine (I), and Cesium (Cs).

22. Review of Terms! Cation: positively charged ion
- Non metals or metals?
Anion: negatively charged ion

23. Chemical Formula Terms
1. Symbol: element being used
2. Subscript: shows how many of the individual atoms are present
ex. O2 CO HBr
3. Coefficient Number: placed before the element or compound, distributed to entire compound
ex. 2HBr or 2H2 + O2  2H2O
4. Oxidation Number: same as “charge”, how many electrons atoms need to gain or lose (to become stable)
**get off of periodic table!!
**write them on your P.T. (Al = +3)

24. Chemical Formulas
The chemical symbols and numbers indicating the number of atoms contained in the basic unit of a substance
Carbon = 6 atoms
C6H12O6
Hydrogen = 12 atoms
Oxygen = 6 atoms
How many atoms of each element are present in 3 molecules of glucose?
3 C6H12O6
C= H= O=18

25. Writing Ionic Formulas
The elements overall charges have to equal zero
Compounds have no net charge!!
Write the cation first with its charge, then the anion and its charge.
Al+3 F-1
Write the chemical formula, using subscripts to indicate how many of each ion are needed to make a neutral compound.
criss-cross method: Al+3 F-1 = AlF3

26. More compounds!!
Balance the formula so the compound formed has a neutral charge
Examples:
Ca Br –1
Na S –2
Al Cl-1

27. Compound Names
and
Formulas

28. Naming ionic compounds
Ionic compounds are formed by the strong attractions between cations and anions. Both ions are important to the compound’s structure, so it makes sense that both ions are included in the name
Name cation first (metal)
Name anion (nonmetal)
3. Drop the end of the anion & add suffix –ide
EXAMPLE: NaCl = sodium chloride

29. More naming practice cation anion Balance formula Compound name
Cs+1,cesium
F-1,fluorine
Ba+2, barium
Cl-1,chlorine
Al+3, aluminum
S-2, sulfur
Cesium Fluoride
CsF
Barium chloride
BaCl2
Aluminum sulfide
Al2S3

30. Naming covalent compounds
Uses prefixes!!!!
Number of atoms
prefix 1
Mono- 2
Di- 3
Tri- 4
Tetra- 5
Penta- 6
Hexa- 7
Hepta- 8
Octa- 9
Nona- 10
Deca-
If there is only one atom of the first element, it does not get a prefix
EX: BF3= boron trifluoride
Dihydrogen monoxide = ????

31. Dihydrogen Monoxide!!!!!!!!
Why????

32. Drinking, bathing, washing, swimming…
Chemistry Joke!
If H20 is water, what is H204? 
Drinking, bathing, washing, swimming…
All kinds of things!

33. The name Game What’s in a name???
How many people can you “bond” with!? 
You must turn in to me a piece of paper with…
Your element and it’s oxidation number
A total of 6 IONIC COMPOUND formulas
AND the name of those compounds
My Ion
What I am bonding with
Chemical Formula
Name
Fe+2
O-2
FeO
Iron Oxide

34. Try these covalent molecules…
Carbon monoxide CO
CO2
N5H8
TeBr2
Si3S7
Carbon dioxide
Pentanitrogen octahydride
Tellurium dibromide
Trisilicon heptasulfide

35. FLASHBACK
1. How many oxygen atoms are there in bleach, NaClO, AKA sodium hypochlorite?
2. Acetone (CH3COCH3), or nail polish remover, has how many total hydrogen atoms?
3. How do you determine oxidation #’s?
4. What is the oxidation # of Al, O, & Cl ?
5. Write ionic formulas: (find charges 1st then criss-cross!!)
Mg + F Be + N
6. Name the following compounds:
N5H SrCl2

36. More naming practice
COVALENT: NO
NO2
N2O
IONIC:
NaF
ZnCl
CaCl2

37. H O H O H Electron diagrams
1. Electron Dot Diagram: 2. Pictorial Diagrams: Hydrogen: H Oxygen: Water: H2O H O H O
Covalent bonds! H

38. and Chemical Reactions
Chemical Changes
and Chemical Reactions

39. Physical Changes
Occur when the size or shape of the substance is changed Occasionally, the color can change, too Regardless, the original substance(s) do not change Evidences of Physical Changes: - Bending, stretching, heat, and cooling can all cause a physical change ***All phase changes are physical changes

40. Chemical changes
Occurs when there is a change in the arrangement of atoms so that a different substance with different properties is produced
Very often,
there is some
kind of
evidence
(for example,
the formation
of a gas)

41. Evidence of a chemical change
Formation of a gas
Reaction with acids
(like this picture of copper reacting with nitric acid)
(Sometimes) a color change can indicate a chemical change.
- A good example of this is metal tarnishing
Is a neutralization reaction a chemical change?

42. Evidence of chemical REACTIONs
Bubbles/fizzing/formation of a gas
Precipitate formed
Energy change
Color change
Odor…

43. If you're not part of the solution… You're part of the precipitate!
Chemistry Joke!
If you're not part of the solution…
You're part of the precipitate!

44. FLASHBACK
1. What is the main difference between a chemical and physical change?
2. If a reaction forms a gas, you know it is a ______________ change.
3. If something changes color, you know it’s a chemical change. True False
4. Name the four evidences of a chemical rxn.
5. Explain a situation in which bubbling occurs, but it is NOT a chemical change.

45. Why do you burp after drinking a Coke?

46. Excuse me… Coke and other soft drinks are carbonated
Carbonation occurs when carbon dioxide is dissolved in water or solution
This gives the "fizz" to carbonated beverages
Excess gas needs out of the stomach.. So we burp!

47. Using the materials provided: 1. 2 pieces of Alka-Seltzer
Rocket Lab Time!!
Using the materials provided:
1. 2 pieces of Alka-Seltzer
2. 1 film canister
3. Water
…you are to
build a projectile!

48. Use an “If-Then” statement!
Hypothesizing
Pick ONE question to answer and generate a hypothesis and WRITE IT DOWN…
Use an “If-Then” statement!
1. How does changing the volume of water effect the time/height of rocket “launch”?
2. How does changing the amount of Alka-Seltzer effect the time/height of rocket “launch”?

49. You are to write a brief lab report on your experience…
- Skip lines between headings
- Full sentences! Alka seltzer
Title
Hypothesis: (your question)
Data: Table? List?
Conclusion: tell me what you learned (in paragraph form!)
1. What evidence did you see of a chemical reaction taking place? How does this relate to the lab?
2. Refer back to your hypothesis… was it right or wrong?? Why??
3. What would have done differently… or how would you make this lab better?

50. FLASHBACK EOC WORKBOOK Pg. 41 (all)
An exothermic reaction __________________ heat.
An endothermic reaction __________________ heat.
( A + B  AB ) is an example of a _____________ reaction

51. Naming:
2) P2O5 ___________________________
3) Mg3N ___________________________
5) SiO2 ____________________________
6) BaCl2 _______________________________
8) B2P9 _____________________________________
Formulas:
14) aluminum nitride ____________________
16) disulfur pentaphosphide ____________________
17) potassium sulfide __________________________
18) rubidium iodide ____________________________
20) hexacarbon dichloride ______________________

52. Chemical Reactions and Equations:
What do they mean?
What do they show?

53. Energy changes in reactions
During any chemical reaction, there is an energy change.
1. Exothermic reaction: heat is released during the reaction, gets hot!
2. Endothermic reaction: heat is
absorbed during the reaction,
gets cold!

54. Everyday Exothermic and Endothermic Reactions
The airbag's inflation system reacts sodium azide (NaN3) with potassium nitrate (KNO3) to produce nitrogen gas. Hot blasts of the nitrogen inflate the airbag.
                                                                                                                                                                                                                                                                       
Instant Cold Packs
Instant heat packs
AIRBAGS!
The airbag's inflation system reacts sodium azide (NaN3) with potassium nitrate (KNO3) to produce nitrogen gas. Hot blasts of the nitrogen inflate the airbag.

55. Videos
Exothermic vs. Endothermic
Endothermic Reaction

56. Reactants  Products Equation Terms
A. Reactants: original substances entering a chemical rxn
- what you started with, on the left side
B. Products: resulting substances
- what you end with, on the right side
Reactants  Products

57. Endothermic vs. Exothermic Calcium Chloride vs
Endothermic vs. Exothermic Calcium Chloride vs. Sodium Bicarbonate… who will win the temperature war???
Turn into me: Half sheet of paper

58. Classifying reactions
1. Synthesis: 2 substances combine to form 1 substance
A + B -> AB
2. Decomposition: 1 substance breaks down (decomposes) to 2 substances
AB -> A + B (opposite of synthesis)
3. Single Displacement: 1 element replaces another
A + BC -> AC + B
4. Double Displacement: positive ion of one compound replaces positive ion of another
AB + CD -> AD + CB

59. Name that equation! Synthesis Decomposition Synthesis
4Al + 3O2 --> 2Al2O3
Ca(OH)2 --> CaO + H2O
Zn + CuSO4 --> ZnSO4 + Cu
Cl2 + 2KBr --> 2KCl + Br2
BaCl2 + Na2SO4 --> 2NaCl + BaSO4
2H2 + O2 --> 2H2O
Decomposition
Single Displacement
Single Displacement
Double Displacement
Synthesis

60. FLASHBACK Label the following equations: (4types)
Zn + HCl  ZnCl2 + H2
2. Fe + O2  Fe2O3
3. SiO2 + HF  SiF4 + H2O
4. FeS + HCl  H2S + FeCl2
5. In lab yesterday, what gas produced the signature “popping” sound?
Single Displacement
Synthesis
Double Displacement
Double Displacement

61. Common Gas Lab! A. NaHCO3 + HCl  NaCl + H20 + ______ CO2
You will be conducting reactions to produce 5 different common gases and observe their chemical and physical properties.
A. NaHCO3 + HCl  NaCl + H20 + ______
B. Cu + 4HNO3  Cu(NO3)2 + 2H _____
C. NH4Cl + NaOH  NaCl + H20 + ______
D. 2H2O2  2H2O + ____
E. Mg + 2HCl  MgCl2 + ____
CO2
NO2
NH3 O2 H2

62. Section Review Pg. 645 #1, 3 EOC REVIEW Pg. 656 #1-5, 11, 15
FLASHBACK
Section Review
Pg. 645 #1, 3
EOC REVIEW
Pg. 656 #1-5, 11, 15

63. FLASHBACK
EOC WORKBOOK
Pg. 43 [all]

64. Balancing Chemical
Equations

65. Chemical Reactions
Chemical reaction - is the process of changing reactants to products by a chemical change
Chemical reactions are symbolized by
Reactants Products
(s) solid; (l) liquid; (g) gas; (aq) aqueous
are the physical states of the reactants and products

66. Equations show… The reactants which enter into a reaction.
The products which are formed by the reaction.
The amounts of each substance used and each substance produced.
___Mg(s) + __ O2(g)  __ MgO(s) 2 2

67. Subscripts and coefficients
We use subscripts to balance compounds
CaCl2
subscripts cannot be changed
We use coefficients to balance equations
2 NaCl + _ Ca(OH)2  2 NaOH + __ CaCl2

68. Balancing equations!
Goal: to get the same number of atoms on both sides of the equation
__ Al + __ O2  ___ Al2O3
__ NaCl  __ Na + __ Cl2
__ Li + __ H2O  __ LiOH + __ H2

69. What’s the point?????
A balanced chemical equation represents the process of a chemical reaction in which atoms are rearranged but not created or destroyed.
By balancing chemical equations, you show that mass is conserved…
Law of Conservation of Mass!

70. Law of Conservation of Mass
Mass is neither created nor destroyed in an ordinary chemical or physical reaction
Mass of Reactants = Mass of Products

71. LAB:
Looking at the…
Law of Conservation of mass!!!

72. FLASHBACK Balance the following equations:
___Zn + ___HCl  ___ZnCl2 + ___H2
2. ___Fe + ___O2  ___Fe2O3
3. ___SiO2 + ___HF  ___SiF4 + ___H2O
4. ___FeS + ___HCl  ___H2S + ___FeCl2
5.What is the overall goal of balancing equations?

73. FLASHBACK 1. __S8 + __O2  __SO2 2. __ HgO  __Hg + __ O2
Balance the following equations:
3. __BeCl2 + __KOH  __Be(OH)2 +__KCl
4. __S8 + __ O2  __ SO3
5. __H3PO4 + __Mg(OH)2 __Mg3(PO4)2 + __H2O
1. __S __O  __SO2
2. __ HgO  __Hg + __ O2

74. Reactions occur when particles of reactants collide with energy
Reaction Rates!
Reactions occur when particles of reactants collide with energy

75. Factors affecting reaction rates
Temperature: higher temperature, reaction rate increases
Particles moving faster, more collision between particles
Concentration: when reactants are more concentrated, rate of reaction increases
More particles mean more collisions

76. Factors affecting reaction rates [Inhibitor: slows down a reaction]
3. Surface Area: more surface area, reaction rate increases
4. Catalyst: presence of catalyst speeds up reaction without being permanently changed
[Inhibitor: slows down a reaction]
Video!

77. Thursday 10/22 - Bellringer
EOC WORKBOOK
Pg. 45 [# 2-6]
Pg. 46 [# 1-6]

78. Salt: Up close and personal
Make some observations of salt under a microscope!!