1. AP Chemistry Due Next Class: Upcoming Due Dates: Chapter 1-3 Notes
MC Ch PM)
MC Ch. 1-3 Assignment
Lab + Conclusion (9/13)
Reading Ch
Ch. 1-4 Quiz (9/15)

2. Lab Review Get back into your lab group Grab a whiteboard Group Chat
Get the Actual Formula From Ms. Bryce
Grab a whiteboard
Calculate the percent difference
Results & Analysis 1-4
List 3 possible reasons for your error.
How did you get there?
Group Chat
Patterns?
Include all info in your conclusion

3. Mastering Chemistry Sign In
1. Go to website 2. Select the link that matches the code below 3. Select the title of the Book (Chemistry, The Central Science By Brown and LeMay 13th edition) 4. Follow the on-screen instructions to register your code and create your personal login and password 5. WRITE THE LOGIN/PASSWORD DOWN INSIDE YOUR NOTEBOOK! Course ID: MCBRYCE2017 Code: SSNAST-PLUNK-BOSSY-CAVAN-BUSBY-HIKES

4. Notes

5. Solutions
Solutions: homogeneous mixtures of two or more pure substances.
Solvent: substance present in greatest abundance.
Solutes: all other substances in the solution.
Aqueous Solution: water is the solvent.
Ionic Compounds dissolve by dissociation, where water surrounds the separated ions.
Molecular compounds interact with water, but most do NOT dissociate. (Some do react with water when they dissolve).

6. Aqueous Solutions Ionic Compounds: Dissociate AND Form Ions
Molecular Compounds: Do not dissociate AND Do not form ions

7. The solvent in a sample of soda pop is
sugar.
carbon dioxide.
water.
air.
Answer: c

8. Electrolytes and Nonelectrolytes
Electrolyte: substance that dissociates into ions when dissolved in water.
Nonelectrolyte may dissolve in water, but it does not dissociate into ions when it does so.

9. Electrolytes

10. Solubility of Ionic Compounds
MUST MEMORIZE: All Na+, K+, NH4+& NO3- salts are soluble in H2O

11. Which pair of compounds will produce a precipitate if solutions of appropriate concentrations are mixed together?
H2SO4 and NaOH
HNO3 and CaCl2
Ba(NO3)2 and Na3PO4
LiCl and SrI2
Answer: c

12. Molecular Equation
The molecular equation lists the reactants and products without indicating the ionic nature of the compounds.
AgNO3(aq) + KCl(aq)  AgCl(s) + KNO3(aq)
In the complete ionic equation all strong electrolytes (strong acids, strong bases, and soluble ionic salts) are dissociated into their ions.
This more accurately reflects the species that are found in the reaction mixture.
Ag+(aq) + NO3−(aq) + K+(aq) + Cl−(aq)  AgCl(s) + K+(aq) + NO3−(aq)

13. Ag+(aq) + NO3−(aq) + K+(aq) + Cl−(aq)  AgCl(s) + K+(aq) + NO3−(aq)
Net Ionic Equation
Ag+(aq) + NO3−(aq) + K+(aq) + Cl−(aq)  AgCl(s) + K+(aq) + NO3−(aq)
Clean up! Cross out anything that does not change from the left side of the equation to the right.
The ions crossed out are called spectator ions, K+ and NO3−… since they sit back and spectate!

14. Practice- Writing Metathesis Reactions
Write the molecular, complete ionic, and net ionic equation for the precipitation reaction that occurs when aqueous solutions of calcium chloride and sodium carbonate are mixed.
CaCl2(aq) + Na2CO3(aq)  CaCO3(s) + 2NaCl(aq)
Ca2+(aq) + 2Cl-(aq) + 2Na+(aq) + CO32-(aq)  CaCO3(s) + 2Na+(aq) + 2Cl-(aq)
Ca2+(aq) + CO32-(aq)  CaCO3(s)

15. Which ions, if any, are spectator ions in this reaction?
AgNO3(aq) + NaCl(aq) ⟶ AgCl(s) + NaNO3(aq)
Ag+(aq) and Cl–(aq)
NO3–(aq) and Cl–(aq)
Na+(aq) and NO3–(aq)
No spectator ions are involved.
Answer: c

16. Precipitation Reactions
Mix solutions of soluble salts.
Sometimes, an insoluble salt is produced – or “falls” out of solution.
This solid is called a precipitate.

17. Brønsted and Lowry Acids: Proton donors

18. Brønsted and Lowry Bases: Proton acceptors

19. Strong or Weak? Strong acids: completely dissociate in water
Weak acids: partially dissociate.
Strong bases: completely dissociate to metal cations & OH- anions in water
Weak bases: only partially react to produce hydroxide anions.

20. Which compound below is not a strong acid?
HC2H3O2
H2SO4
HNO3
HBr
Answer: a

21. Comparing Acid Strengths
The following diagrams represent aqueous solutions of acids HX, HY, and HZ, with water molecules omitted for clarity. Rank the acids from strongest to weakest.
weakest
strongest
2nd strongest

22. Acid-Base Reactions
The acid (H2O above) donates a proton (H+) to the base (NH3 above).
Neutralization reactions: reactions between an acid and a base
When the base is a metal hydroxide, water and a salt (an ionic compound) are produced.

23. Neutralization Reactions
When a strong acid (like HCl) reacts with a strong base (like NaOH), the net ionic equation is circled below:
HCl(aq) + NaOH(aq)  NaCl(aq) + H2O(l)
H+(aq) + Cl−(aq) + Na+(aq) + OH−(aq)  Na+(aq) + Cl−(aq) + H2O(l)
H+(aq) + OH−(aq)  H2O(l)

24. Gas-Forming Reactions
Some metathesis reactions do not give the product expected.
When a carbonate or bicarbonate reacts with an acid, the products are a salt, carbon dioxide, and water.
CaCO3(s) + 2 HCl(aq) CaCl2(aq) + CO2(g) + H2O(l)
NaHCO3(aq) + HBr(aq) NaBr(aq) + CO2(g) + H2O(l)

25. By analogy to examples given in the text, predict what gas forms when Na2SO3(s) reacts with HCI(aq).
SO2(g)
H2(g)
CO2(g)
H2S(g)
Answer: a