AP Chemistry Summer Study Guide

Future AP Chemistry Student:

The attached packet of information contains summer work which will review topics that were learned in Honors Chemistry and you need to know on Day 1 of AP Chem. It is imperative that you review during the summer. We will begin by applying the concepts you have already mastered this past year and begin looking at problems in a new and exciting way. You may use any resource needed to complete this review packet. You may work with your peers; in fact, I encourage you to do so. Keep in mind that copying from your peers will do you no good, as you will ultimately be responsible for knowing this material.

It is expected that ALL work is shown and completed on notebook paper or electronically, NOT on these worksheets. I will be collecting your work during the first week of school and it will be graded for completion.

If you have any questions, please e-mail me at dhardy@qcsd.org and I will get back to you. Please keep in mind that I may not check my email every day and include information in the Subject about AP Chem. If you would like to check out a textbook to use over the summer, please stop by C204 for an AP Chemistry textbook. This packet will be available on the High School Website and YouTube/Websites videos that would be helpful would be the following:

Tyler DeWitt

Bozeman Science-Chemistry

Bozeman Science-AP Chemistry

Khan Academy-Chemistry

Khan Academy-AP Chemistry

Brightstorm

Enjoy your summer and see you in August,

Ms. Hardy

Topics to Review:

Nomenclature

Mole Concept

Significant Figures

Stoichiometry

Chemical/Physical Changes

Basic Atomic Structure

Laboratory Equipment

Solutions

Thermochemistry

Equilibrium

Nomenclature

Vocabulary:

Word

Definition

Example/Equation/Diagram

Salt

Acid

Base

Binary compound

Molecule

Ion

Cation

Anion

Terinary Acid

Polyatomic ion

Oxidation Number

Diatomic

Transition Metal

Formula Unit

Name the following compounds:

1. KCN_____________________16. ICl3_____________________

2. NaCH3COO_____________________17. Pb(NO3)2_____________________

3. Cr2O3_____________________18. CH3COOH____________________

4. Hg2I2_____________________19. NaHCO3

5. N2O5_____________________20. CsOH_____________________

6. HClO4_____________________21. NH3_____________________

7. HCl(g)_____________________22. NaBr_____________________

8. HCl(aq)_____________________23. SrCO3_____________________

9. KMnO4_____________________24. Ba(OH)2_____________________

10. CO2_____________________25. Al2O3_____________________

11. CH4_____________________26. SnO2_____________________

12. CuCl2_____________________27. SF6_____________________

13. Na2CO3_____________________28. HNO3_____________________

14. H2O2_____________________29. PCl5_____________________

15. K2CrO4_____________________30. NH4NO2_____________________

Write the correct formula for each of the following compounds.

1. sodium hydroxide_____________________16. calcium nitrite_____________________

2. aluminum nitrate_____________________17. lead (II) chloride_____________________

3. antimony trichloride _____________________18. sodium permanganate_____________________

4. carbonic acid_____________________19. silver nitrate_____________________

5. ozone_____________________20. zinc sulfate_____________________

6. ammonium perchlorate_____________________21. lithium bicarbonate_____________________

7. magnesium sulfide_____________________22. iron (III) oxide_____________________

8. sodium peroxide_____________________23. potassium dichromate_____________________

9. hydrobromic acid_____________________24. nitrogen dioxide_____________________

10. copper (I) sulfide_____________________25. barium cyanide_____________________

11. diphosphorus pentoxide_____________________26. aluminum sulfate_____________________

12. hydrocyanic acid_____________________27. sodium hypochlorite_____________________

13. ammonium chloride_____________________28. hydrogen iodide_____________________

14. hydroiodic acid_____________________29. manganese (IV) oxide_____________________

15. oxalic acid_____________________30. calcium hydrogen carbonate________________

Mole Concepts

Vocabulary:

Word

Definition

Example/Equation/Diagram

Avogadros Number

Empirical Formula

Molar Mass

Molar Volume

Mole

Percent Composition

Representative Particle

Standard Temperature

Standard Pressure

Molecular Formula

1. What is the percent composition of each element in barium hydroxide?

2. A compound is found to be 63.3 percent manganese and 36.7 percent oxygen by mass. Determine the empirical formula of the compound.

3. A 51.36 g sample of a compound containing carbon, hydrogen and oxygen is burned. After the complete combustion of the sample, 55.90 g of carbon dioxide and 28.61 g of water are produced. What is the empirical formula of the compound?

4. Which of the following are empirical formulas?

C2H5H2OLiNO3H2O2C6H12O6

5. A 24.6 g sample of hydrated magnesium sulfate is heated to drive off the water of hydration. The sample is heated to a constant mass of 12.0 g. What is the formula of the hydrate?

Atomic Structure

Vocabulary:

Word

Definition

Example/Equation/Diagram

Isotope

Nucleus

Electron

Proton

Neutron

Mass number

Atomic number

Alkali metal

Alkaline earth metal

Noble gas

Halogen

Paramagnetic

Diamagnetic

Group/family

Period/series

Atom

1. Write the atomic/nuclear symbol, including the mass number, atomic number, and charge for each of the following species. State the number of protons, neutrons and electrons present in each.

calcium 40 atom

fluorine 19 ion

barium 137 ion

oxygen 16 atom

2. List the elements that exist as diatomic species.

3. What is the difference between a molecule and a formula unit? Why is it incorrect to refer to units of sodium chloride as molecules?

Conversions

1. Convert the following measurements:

a. 525 mmHg atmg. 80. C K

b. 25.0 g Ca(NO3)2 molesh. 3.11 x 1024 molecules CO2 grams

c. 425 mL Li. 7.2 kg/m3 g/cm3

d. 25.4 g kgj. 55.6 kPa atm

e. .55 km cmk. .68 moles of sodium atoms

f. 4.00 g/L g/mLl. 825 mg g

2. Identify the number of significant digits in each of the following measurements:

a. 4.20 m ________g. 0.0045 mL ________

b. 520 g ________h. 9.00 kg ________

c. 6.090 cm ________i. 0.020 mol ________

d. 6.0 x 1023 molecules ________j. 9.11 C ________

e. 900 m________k. 12 atoms ________

f. 8.8 g/mL ________l. 8255 kg ________

3. Write the answer to each of the following problems. Express your answer in the correct number of significant digits.

a. 3.50 g + .349 g = ____________c. 125.00 mL + 3.25 mL = _____________

b. 5.24 g 1.2 mL = _____________d. 4.2 cm x 5.25 cm x .20 cm = _____________

4. What is the volume in mL of 7.45 g of hydrogen gas at STP?

5. How many moles of calcium phosphate are equivalent to 36.45 g of calcium phosphate?

6. What is the mass of 7.23 x 1022 molecules of sulfur dioxide?

Stoichiometry

Vocabulary:

Word

Definition

Example/Equation/Diagram

Anhydrous

Hydrate

Aqueous

Coefficient

Combustion

Synthesis

Decomposition

Single Replacement

Double Displacement

Molarity

Limiting Reactant

(limiting reagent)

Percent Yield

Reactant

Product

Precipitate

Mole Ratio

Moles Chemical Given

Moles Chemical Wanted

Grams (g)

Grams (g)

Atoms/Molecules

Atoms/Molecules

Liters (L) of as at STP (0C, 1 atm)

Liters (L) of as at STP (0C, 1 atm)

Liters (L) of solution (aq)

Liters (L) of solution (aq)

Balanced Equation

Mole Ratio

Molar mass

22.4

Molar mass

22.4

M=

M=

6.02 x

6.02 x

1. How many grams of copper (II) sulfate are needed to make 500.0 mL of a .200 M CuSO4 solution.

2. How many grams of silver chloride are produced when 30.0 mL of 0.150 M calcium chloride are added to 15.0 mL of 0.100 M silver nitrate?

3. How many grams of potassium chlorate must be heated to generate 120. mL of oxygen gas at STP?

4. A 3.55 g contaminated sample of calcium carbonate is treated with hydrochloric acid. The sample required 35.5 mL of 1.50 M hydrochloric acid to completely react. Assuming that the contaminant will not react with the acid, what is the percent purity of the sample?

Misc Problems:

1. A compound having an approximate molar mass of 165 -170 g is found to have the following percent composition: 42.87% carbon, 3.598% hydrogen, 28.55% oxygen and 25.00% nitrogen. What is the molecular formula of the compound?

2. When 1.00 g of metallic chromium is heated strongly in the presence of chlorine gas,