1. Test Corrections

2. Day 3 5-14 Goal Setting 1. Test 7 % grade = ___. I studied by …
Next time I will study by …
Goal for next time = ____
If you did not meet your goal it stays the same as last time
If you did meet your goal improve upon your score by at least 1 point
Day

3. Question of the Day Day 3 5-14 Name the following: H2SO4 FeCO3 CCl4
Write the formulas:
carbon monoxide
gold III sulfide
nitric acid

4. Day
Binders

5. Question of the Day Day 4 5-15 Name the following: Cu2SO4 HNO3
Write the formulas:
dinitrogen monoxide
aluminum oxide

6. Describing Chemical Reactions
Chemical Reactions – a process in which one or more substances are converted into new substances with different physical and chemical properties
Bonds break, and/or form, and/or rearrange!!!

7. Describing Chemical Reactions
reactants
products
H2(g) + F2(g) HF(g)
Chemical equation
Reactions are represented by chemical equations

8. Describing Chemical Reactions
reactants
products
H2(g) + F2(g) HF(g)
State of matter: g = gas, l = liquid, s = solid, aq = aqueous solution

9. Describing Chemical Reactions
reactants
products
H2(g) + F2(g) HF(g)
Coefficients – how many mols of each element react with each other – mol ratio

10. Describing Chemical Reactions
H2(g) + F2(g) HF(g)
1 mol of hydrogen gas reacts with 1 mol of fluorine gas to produce 2 mols of hydrogen fluoride gas
For now think of a mol as a piece:
1 piece of hydrogen gas reacts with 1 piece of fluorine gas to produce 2 pieces of hydrogen fluoride gas

11. Describing Chemical Reactions
Conservation of matter -
Atoms are neither created nor destroyed in ordinary chem. rxns.

12. Describing Chemical Reactions
A heads-up on diatomic gases:
If the natural state of an element is gas, assume it is always a diatomic molecule (Example: Nitrogen = N2) – NOT including the noble gases
ADD THESE TO YOUR BLUE SHEET!!!

13. What’d We Just Do? Chemical Reactions –
a process in which one or more substances are converted into new substances with different physical and chemical properties
Bonds …

14. What’d We Just Do? H2(g) + F2(g) 2HF(g) reactants products
Chemical equation

15. What’d We Just Do? H2(g) + F2(g) 2HF(g) reactants products
State of matter: g = gas, l = liquid, s = solid, aq = aqueous solution

16. What’d We Just Do? H2(g) + F2(g) 2HF(g) reactants products
Coefficients – how many mols of each element react with each other – mol ratio

17. Q Of The Day H2 Br2 O2 N2 Cl2 I2 F2 Day 5 5-18
The things you start with in a chemical reaction are called ________.
the arrow in a chemical equation stands for __________________.
Which elements on the periodic table are diatomic (list them)?
reactants
produces or yields
H2 Br2 O2 N2 Cl2 I2 F2

18. Binders
Kayla
Madison
Danielle

19. Last time Chemical Reactions –
a process in which one or more substances are converted into new substances with different physical and chemical properties
Bonds …

20. Last time Conservation of matter -
Atoms are neither created nor destroyed in ordinary chem. rxns.

21. Last time
reactants
products
H2(g) + F2(g) HF(g)
Chemical equation

22. Last time H2(g) + F2(g) 2HF(g) reactants products
State of matter: g = gas, l = liquid, s = solid, aq = aqueous solution

23. Last time 2H2(g) + O2(g) 2H2O(l) reactants products
Coefficients – how many mols of each element react with each other – mol ratio

24. Balancing Equations Writing a chemical equation:
Hydrogen gas reacts with chlorine to produce liquid hydrochloric acid.
Hydrogen gas =
Chlorine =
Liquid Hydrochloric acid =

25. Balancing Equations Writing a chemical equation: Reactants = Product =
Hydrogen gas reacts with chlorine to produce liquid hydrochloric acid.
Reactants =
Product =
Coefficients?
H2(g) + Cl2(g)  HCl(l)

26. Balancing Equations
Atoms are neither created nor destroyed in ordinary chem. rxns.
Sum of atoms on each side must be equal
Use coefficients to help

27. Balancing Equations
H2(g) + Cl2(g)  HCl(l)

28. Practice
Liquid water breaks apart into hydrogen gas and oxygen gas (electrolysis).
Equation:
Build:

29. Day
Q Of The Day
Use the following chemical reaction to answer the questions below:
4Li(s) + O2(g)  2Li2O(s)
a. lithium oxide = what state of matter?
b. What does the 4 in front of Li tell you?
c. What is produced?

30. Practice
Solid sodium reacts with chlorine gas to produce solid sodium chloride.
Equation:
Build:

31. Practice
Solid magnesium reacts with fluorine gas to produce solid magnesium fluoride.
Equation:
Notes page 3

32. Li2O(s) + H2O(l)  LiOH(aq) HCl(aq) + Mg(OH)2(aq)  MgCl2(aq) + H2O(l)
Additional Practice
1. Balance the following chemical reaction:
Li2O(s) + H2O(l)  LiOH(aq)
2. Balance the following chemical reaction:
HCl(aq) + Mg(OH)2(aq)  MgCl2(aq) + H2O(l)

33. Assignment
Read pages , define chemical equation and skeleton equation, AND complete #s 1 and 2 on page 349.
Due Wednesday!

34. 2Na(s) + 2H2O(l)  2NaOH(aq) + H2(g)
Day
Q Of The Day
Use the following chemical reaction to answer the questions below:
2Na(s) + 2H2O(l)  2NaOH(aq) + H2(g)
a. sodium hydroxide = what state of matter
b. What does the 2 in front of H2O tell you?
c. What is produced (BOTH!)?

35. Balancing Equations NOTES PAGE 3
Chemicals equations are not always balanced, sometimes we will have to balance them …
1. Balance different types of atoms one at a time
2. Start with atoms that appear only once on each side
NOTES PAGE 3

36. Balancing Equations 1. Balance different types of atoms one at a time
2. Start with atoms that appear only once on each side
3. Balance polyatomic ions that appear on both sides of the equation as a single unit
4. Balance H and O atoms last

37. If it’s not working… Balancing Equations NOTES PAGE 3 Deep breathe
Check your chemical formulas
NEVER change subscripts this changes the compounds!!!
It’s ok to start over if you get frustrated
NOTES PAGE 3

38. Balancing Equations IN NOTES!!!
F2(g) + K(s)  KF(s)
Al(s) + O2(g)  Al2O3(s)
IN NOTES!!!

39. Balancing Equations Na + Mg3(PO4)2 → Mg + Na3PO4 States of Matter?
Polyatomic Example:
Na + Mg3(PO4)2 → Mg + Na3PO4
States of Matter?

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