1. Introduction to Writing Formulas

2. Do Now: Consider the following ions:
Turn them into puzzle pieces and bond ONE type of CATION with ONE type of ANION
What compounds did you create?

3. Chemical Formulas represent compounds.

4. Interpreting Chemical Formulas
Coefficient
Number that is placed in front of a chemical formula or a symbol in a chemical equation that indicates the number of moles or molecules of this substance involved in the reaction
Subscript
Number placed to the lower right of a chemical symbol to indicate the number of atoms of the element in the compound.

5. Interpreting Chemical Formulas
2Na2O
2 = coefficient= 2 moles of this element
Number of atoms for each element coefficient * subscript
If you do not see a subscript, it is understood to be 1
Na = 2*2 = 4
O = 2*1 = 2
Total # of atoms = 4+2 = 6

6. Interpreting Chemical Formulas
3Ba3(PO4)2
Ba = 3*3 = 9
P = 3* (2*1) = 3*2 = 6
O = 3* (4*2) = 3*8 = 24
Total # of atoms = = 39
When you have parenthesis, you must multiply the subscript on the outside of the parenthesis by every subscript on the inside of the parenthesis before you multiply by the coefficient

7. Writing Chemical Formulas
You need to know the chemical symbol for the element
You need to know the element’s oxidation number
Oxidation number is the number of valence electrons an element gains, loses, or shares during bonding
For metals, the oxidation number is positive
For nonmetals, the oxidation number is negative
Column 14 is considered an exception; its oxidation number is +/-4 depending on what it is bonding with

8. Writing Chemical Formulas
Metals
Oxidation number = # of valence electrons it gives away when bonding (in short = number of valence electrons
Nonmetals
Oxidation number = # of valence electrons – 8
Family 14
Oxidation number is +/-4
If 1st element in compound will be +4; if second element in compound will be -4
Family 18
Oxidation number is 0

9. Common Ion Charges 1+ 2+ 3+ NA 3- 2- 1-

10. Understanding Chemical Formulas
Chemical formulas are composed of a positive half and a negative half.
Water is a compound you know to have a formula of H2O.

11. Understanding Chemical Formulas
The element with the positive oxidation number is always written first.
The element with the negative oxidation number is always written second.
H O +1 -2

12. Understanding Chemical Formulas
The total of the oxidation numbers in a compound must equal zero.
Add subscripts after a chemical symbol, when needed, to make the oxidation numbers total zero.
H2O

13. There MUST be an easier way....and there is!! Ca Cl
The easiest way to think of writing chemical formulas is to use the oxidation number (without the + or -) of one element as the subscript of the other element. +2 -1
Ca Cl

14. Writing and Understanding Chemical Formulas
Cross over the oxidation numbers without the charges!!! -1 +2
Ca Cl

15. Writing and Understanding Chemical Formulas
Ca Cl 2
Remember, DO NOT write a subscript of 1.

16. Your turn:
Decide what your level of understanding is from 1-4. (4 is the greatest level of understanding) Choose an appropriate worksheet (DO NOT WRITE ON IT) Create some formulas!

17. Exit Card:
Turn in your work from class today!

18. Naming and Formula Making!
For the next couple of slides it will be your job to take ions and from them create formulas—remember the criss-cross method (and the Lewis Dot Structures)—and then name the resulting compounds!

19. C. Ionic Nomenclature ___________________ K+ Cl-  KCl
____________________
K+ Cl-
 KCl
Mg2+ NO3-
 Mg(NO3)2
Cu2+ Cl-
 CuCl2

20. Quick Write:
Generate a list of all topics we’ve studied thus far:

21. Quick Write:
Generate a list of all topics we’ve studied thus far:

22. NOTE:
Tutoring today and tomorrow after school!

23. Rate yourself: 1—Desperately seeking help 2—I need help almost always
3—I could use some help
4—I occasionally need help
5—I can figure this stuff out on my own!

24. Move to your appropriate row:
The people at your table (and you) will choose a worksheet (max of 2 copies per group) and on your OWN paper you will answer the questions.
I will focus most of my efforts on the first row (7 minutes), then (6 minutes) for the second, 5 minutes for the third, and so on.
If you need help BEFORE I get to your row, be a problem solver and find an answer!

25. C. Molecular Nomenclature
Prefix System (binary compounds)
1. Less e-neg atom comes first.
2. Add prefixes to indicate # of atoms. Omit mono- prefix on first element.
3. Change the ending of the second element to -ide.

26. C. Molecular Nomenclature
PREFIX mono- di- tri- tetra- penta- hexa- hepta- octa- nona- deca-
NUMBER

27. Goal of the activity? MgF2 = Magnesium Flouride
Find the piece(s) that fit its complement and build compounds!
Name them too!
It’s like a 2 for 1 Chemistry Lab!
Raise your hand if you need assistance!
MgF2 = Magnesium Flouride

28. Finished with the lab?
Turn in your group’s lab—stapled and include all papers in a single packet.
Select naming sheets to complete and do so—that way you can work to drop your lowest HW or CW grade(s)! (2 is the max. number of grades that can be dropped)

29. Exit Card:
On a half-sheet of paper—share with your partner—summarize what you have learned today and how you will apply it future interactions with ions in Chemistry.
Write 50 words or more!

30. Do Now:
What is the difference between naming ionic vs covalent compounds?
What is similar when naming them?

31. Homework: Continue creating your review!
3 days and counting until your semester exam!
Extra Credit Needed? Bring pipe cleaners or big plastic cups and you will receive a free HW pass and/or +10 points.

32. C. Molecular Nomenclature
Prefix System (binary compounds)
1. Less e-neg atom comes first.
2. Add prefixes to indicate # of atoms. Omit mono- prefix on first element.
3. Change the ending of the second element to -ide.

33. C. Molecular Nomenclature
PREFIX mono- di- tri- tetra- penta- hexa- hepta- octa- nona- deca-
NUMBER

34. C. Molecular Nomenclature
CCl4
N2O
SF6
carbon tetrachloride
dinitrogen monoxide
sulfur hexafluoride

35. C. Molecular Nomenclature
arsenic trichloride
dinitrogen pentoxide
tetraphosphorus decoxide
AsCl3
N2O5
P4O10

36. C. Molecular Nomenclature
The Seven Diatomic Elements
Br2 I2 N2 Cl2 H2 O2 F2 H N O F Cl Br I

37. C. Ionic Nomenclature Ionic Formulas
Write each ion, cation first. Don’t show charges in the final formula.
Overall charge must equal zero.
If charges cancel, just write symbols.
If not, use subscripts to balance charges.
Use parentheses to show more than one polyatomic ion.
Stock System - Roman numerals indicate the ion’s charge.

38. C. Ionic Nomenclature NaBr Na2CO3 sodium bromide FeCl3
sodium carbonate
iron(III) chloride

39. B. Acid Nomenclature

40. B. Acid Nomenclature HBr H2CO3 H2SO3 2 elements, -ide
 hydrobromic acid
3 elements, -ate
 carbonic acid
3 elements, -ite
 sulfurous acid

41. B. Acid Nomenclature hydrofluoric acid sulfuric acid nitrous acid
2 elements
 H+ F-
 HF
3 elements, -ic
 H+ SO42-
 H2SO4
3 elements, -ous
 H+ NO2-
 HNO2

42. You practice:
Grab a partner and one of the sheets from the front of the class that you HAVE NOT attempted yet.
Name the compounds and then complete as many of the formulas as possible!

43. Exit Card: Choose one Cation

44. II. Molecular Geometry (p. 183 – 187)
Ch. 6 – Molecular Structure

45. Do Now:
CH4—Draw the Lewis Dot Structure and determine what type of compound methane is…

46. Best Class Competition
1st Place: 2nd Period with 69/75 pts
2nd Place: 4th Period with 58/75 pts
3rd Place: 3rd Period with 46/75 pts (20pts!)
4th Place: 6th Period with 40/75 pts 

47. Ice Cream Sign-Up Whole Milk—1 gallon (3):
Half and Half—1/2gallon (6):
Sugar—3 lbs (3):
Toppings (6):
Napkins (1):
Plastic Bags (box of 50):
Spoons (2):
Metal Tins (2-4):
Morris: Rock Salt, Ice, Lab Quests,

48. A. VSEPR Theory Valence Shell Electron Pair Repulsion Theory
Electron pairs orient themselves in order to minimize repulsive forces.

49. Lone pairs repel more strongly than bonding pairs!!!
A. VSEPR Theory
Types of e- Pairs
Bonding pairs - form bonds
Lone pairs - nonbonding e-
Lone pairs repel more strongly than bonding pairs!!!

50. A. VSEPR Theory Bond Angle
Lone pairs reduce the bond angle between atoms.
Bond Angle

51. B. Determining Molecular Shape
Draw the Lewis Diagram.
Tally up e- pairs on central atom.
double/triple bonds = ONE pair
Shape is determined by the # of bonding pairs and lone pairs.
Know the 8 common shapes
& their bond angles!

52. C. Common Molecular Shapes
2 total 2 bond 0 lone
BeH2
LINEAR
180°

53. C. Common Molecular Shapes
3 total 3 bond 0 lone
BF3
TRIGONAL PLANAR
120°

54. C. Common Molecular Shapes
3 total 2 bond 1 lone
SO2
BENT
<120°

55. C. Common Molecular Shapes
4 total 4 bond 0 lone
CH4
TETRAHEDRAL
109.5°

56. C. Common Molecular Shapes
4 total 3 bond 1 lone
NH3
TRIGONAL PYRAMIDAL
107°

57. C. Common Molecular Shapes
4 total 2 bond 2 lone
H2O
BENT
104.5°

58. C. Common Molecular Shapes
5 total 5 bond 0 lone
TRIGONAL BIPYRAMIDAL
120°/90°
PCl5

59. C. Common Molecular Shapes
6 total 6 bond 0 lone
SF6
OCTAHEDRAL
90°

60. D. Examples
PF3
4 total
3 bond
1 lone
TRIGONAL PYRAMIDAL
107°

61. D. Examples
CO2
2 total
2 bond
0 lone
LINEAR
180°

62. III. Molecular Polarity (p. 183)
Ch. 6 – Molecular Structure

63. + - A. Dipole Moment H Cl Direction of the polar bond in a molecule.
Arrow points toward the more e-neg atom.
H Cl + -

64. B. Determining Molecular Polarity
Depends on:
dipole moments
molecular shape

65. B. Determining Molecular Polarity
Nonpolar Molecules
Dipole moments are symmetrical and cancel out.
BF3 F B

66. B. Determining Molecular Polarity
Polar Molecules
Dipole moments are asymmetrical and don’t cancel .
H2O H O
net
dipole
moment

67. B. Determining Molecular Polarity
Therefore, polar molecules have...
asymmetrical shape (lone pairs) or
asymmetrical atoms
CHCl3 H Cl
net
dipole
moment

68. Do Now:
Choose any two ions from the periodic table and create a compound.
Repeat with two different ions.
Now using your poly atomic ion sheet, create one more compound by selecting a metal.

69. Homework: Continue creating your review! SF PPT due by Wednesday!
2 days and counting until your semester exam!
Extra Credit Needed? Bring pipe cleaners or big plastic cups and you will receive a free HW pass and/or +10 points.

70. Boys vs. Girls Competing for 5 points added to your semester exam
One writer (all thinkers), writer changes with each question
You can use any resource at your disposal!
Let’s Play!

71. Bonds: What type of bonds are there in FeNO?
What type of bonds are there in CO2?
What type of bonds are there in MgS?
What type of bond involves two of the same kind of element and is characterized by almost no solubility and a low melting point?

72. Bonds
What type of bond creates compounds that have very high melting points and high conductivity?
What type of bond is soluble? BONUS: Why is it soluble?
Describe the difference between ionic and covalent bonds.

73. Lewis Dot Structures: Draw the Lewis dot structure for:Li
Fe (II) P I
Draw CH4 ,a covalently bonded compound, as a Lewis Dot Structure
Draw a Lewis Dot Structure of an ionic bond and be able to explain what is shown in your drawing.

74. Create Compounds:
Combine oxygen and carbon to form a compound where you have one oxygen and one carbon
Name that compound
Combine Titanium +2 and Chlorine to form a compound.
Name that compound.
Combine the elements potassium (K) and sulfate (______) to form a compound.

75. Name those compounds: N2O5 Al2S3 SrO N2O H2SO4 HBr MnCl3
BONUS: Tell me what naming system did you use.

76. Make Compounds ____________ ___________ Li and S Zr (III) and OH
Co (II) and NO3
____________
___________
________ are chosen by the opposing team!

77. Do Now:
Choose any topic that we have studied so far this year and write a super succinct summary of it.
Be sure to include an example.
MANY people will be sharing, so it is in your best interest to have completed this!

78. Homework: Continue creating your review! SF PPT due by Thursday!
1 day and counting until your semester exam!

79. Jeopardy: Choose your own team of four-five people.
Generate a team name!
We will take turns answering questions.
If the answer is wrong from the team that is going—first team to hold up the correct answer steals the points.
You may ONLY use your notes—no Googling!

80. Exit Card:
Set a goal score for the exam tomorrow: _______, then explain how you will work to ensure that goal score is reached.
44 multiple choice questions
Be ready!
Never Give Up!

81. Do Now:
Study your reviews (if they exist) or your notes and ask your shoulder partners any last minute questions you have.

82. Homework:
Nada!
(Unless you haven’t turned in your Science Fair Project— then do that!)

83. Agenda: Last Minute Questions Explanation of after-test project Test
Set-up your first Ornament!
NOTE: Only one day left until Winter Break! 

84. Do Now:
Send one person from your table to get everyone there a Mid-Year Chem Survey.

85. Homework:
Nothing!
Unless you haven’t turned in your Science Fair project OR you need to remediate this 9 weeks—which I’ll talk to you about!

86. Agenda: Check the status of your snowflake
Modify or complete your set-up
Grab a page of notes to split amongst your group mates.
Write a note of thanks/appreciation/ encouragement to your teachers.
Our goal—give a note to everyone in the building! You must write one note to someone that is not listed on the board yet!
Make a card for someone important to you!
Eat Popcorn/ Drink Hot Chocolate (or Tea)!

87. Have a great break!