1. Bell Work
What do you use to convert grams to moles or moles to grams?
What do you use to convert particles(atoms, molecules, units) to moles or vice versa?
If I am changing from grams to particles what do I need to do?
Convert 184g of PbI2 to particles.

2. Extra Credit-Memes! Create a meme that is related to chemistry.
To create a meme, go to a meme generator website. Choose a blank meme and add your own text.
After you have created a meme save the image. Either me or print the image.
You need to include 2-3 sentences describing the science behind your meme and why it is funny and clever.
DUE BY MONDAY, DECEMBER 7

4. Unit 6: Chemical Reactions

5. What are indications that a chemical reactions has happened?

6. Bell Work
List 5 things that would indicate a chemical reaction has occurred.

7. Indicators of chemical reactions
Emission of light or heat
Formation of a gas
Formation of a precipitate
Color change
Emission of odor

8. All chemical reactions:
Have two parts
Reactants - the substances you start with
2. Products- the substances you end up with
The reactants turn into the products
Reactants ® Products

9. Describing Chemical Reactions
Can be described several ways:
1. In a sentence
Copper reacts with chlorine to form copper (II) chloride.
2. In a word equation
Copper + chlorine ® copper (II) chloride
Cu + Cl2 ® CuCl2

10. Symbols used in equations
(s) after the formula –solid Cu(s)
(g) after the formula –gas H2 (g)
(l) after the formula -liquid H2O(l)
(aq) after the formula - dissolved in water, an aqueous solution. CaCl2 (aq)
Cu(s) + Cl2(g) ® CuCl2(aq)

11. Symbols used in equations
indicates a reversible reaction
shows that heat is supplied to the reaction

12. Diatomic elements There are 7 elements that never want to be alone.
They form diatomic molecules, in gas state.
H2 , N2 , O2 , F2 , Cl2 , Br2 , and I2

14. Law of Conservation of Mass
In a chemical reaction, matter is neither created nor destroyed.
Atoms won’t change their identity (e.g. a Carbon atom can’t become an Iron atom)
This means that you have to have the same number of each type of atom on each side of the chemical equation.

15. Law of Conservation of Mass
Atoms cannot be created or destroyed!
Total mass stays the same.
The atoms are rearranged to form new materials.

16. Balancing Equations
We can see that the equation, does not follow the Law of Conservation of Mass
C2 + O2  CO2
We can see that on the product side there are two carbon atoms, but on the reactant side there is only one. This cannot possibly happen, as mass cannot be destroyed

17. Balancing Equations
To balance chemical equations follow these basic steps
Perform an atom inventory—count how many of each element you have on each side of the arrow.
Identify your problem areas
Begin adjusting the coefficients of the equation to balance the equation. You cannot change the subscripts, only the coefficients!

18. Balancing Equations C2 + O2  CO2 Atom inventory Identify Problems
Fix Problems

19. WARNING!
Don’t mess with the insides of polyatomic ions – put a square around them, or label them as X – treat the WHOLE polyatomic ion as though it were an element!
Don’t ever play around with subscripts (those little numbers that tell you how many atoms are in a molecule)
e.g. C6H22O11

20. 7.
H2 + Cl2  HCl
1H Cl2  2HCl

21. 8.
CdCO3  CdO + CO2
Already Balanced 

22. 4.
Li + FeBr2  LiBr + Fe
2Li + 1FeBr2  2LiBr + 1Fe

23. 3.
KClO3  KCl + O2
2KClO3  2KCl + 3O2

24. NaOH + FeCl3  NaCl + Fe(OH)35.
NaOH + FeCl3  NaCl + Fe(OH)3
3NaOH + 1FeCl3  3NaCl + 1Fe(OH)3

25. 2.
Na + H2O  NaOH + H2
2Na + 2H2O  2NaOH + 1H2

26. 6.
Ca2Br2 + NaCO3  CaCO3 + NaBr
1Ca2Br NaCO3  2CaCO NaBr

28. Bell Work 12-6-15 Balance the following equations:
1.___Al2(SO4)3 +___ Ca(OH)2 →__ Al(OH)3 + __ CaSO4
2. ___Cr +___ O2 →____ Cr2O3

29. Types of Reactions Synthesis reactions Decomposition reactions
Single displacement reactions
Double displacement reactions
Combustion reactions

30. 1. Synthesis General: A + B  AB Example C + O2  + O O
Definition: multiple reactants combine to form a single product

31. 2. Decomposition General: AB  A + B Example: NaCl  + Cl Na Cl Na
Definition: breakdown of one molecule into elements or simple compounds

32. 3. Single Displacement/Replacement
Example: Zn + CuCl2  Zn Cl Cu + Cl Zn Cu +
General: AB + C  AC + B
Definition: an element or ion is replaced by another in a compound

33. 4. Double displacement General: AB + CD  AD + CB Example: MgO + CaS 
Definition: two elements or ions are replaced by another in multiple compounds

34. 5. Combustion Reactions
Definition: a hydrocarbon reacts with oxygen gas.
This is also called burning!!!
In general: CxHy + O2  CO2 + H2O
Products are ALWAYS
carbon dioxide and water.

35. Bell Work 12-8-15 1.Balance the equation 2. What type of reaction?
_____ Ca + _____ O2  _____ CaO
Reaction: _______________
_____ Cu2O + _____ C  _____ Cu + _____ CO2
_____ Na + _____ MgF2  _____ NaF + _____ Mg
_____ Na + _____ HCl  _____ H2 + _____ NaCl
_____ Cl2 + _____ KI  _____ KCl + _____ I2

36. Activity Series.
Elements will replace elements below them in single rep. reactions. K Ca Na Mg Al Zn Fe Ni Pb H Cu Ag

38. Solubility Table Ion Solubility Exceptions NO3– soluble none ClO4– Cl–
except Ag+, Hg22+, *Pb2+ I–
SO42-
except Ca2+, Ba2+, Sr2+, Hg2+, Pb2+, Ag+
CO32-
insoluble
except Group IA and NH4+
PO43-
OH–
except Group IA, *Ca2+, Ba2+, Sr2+
S2-
except Group IA, IIA and NH4+
Na+ K+
NH4+

39. AgNO3(aq) CuSO4(aq) Li3N NH4NO3