AP Chemistry Summer Assignment Robin Stefurak, M.Ed

Welcome to AP Chemistry! This is a demanding, challenging and stimulating course, with accompanying lab, that will cover the first year of College Chemistry.

In preparation for the up and coming school year, you will want to complete the Summer Assignment before the first day of school. The material in this packet is a review of some concepts covered in a Pre-AP / Honors Level Chemistry Course. These are concepts that need to be firmly in place prior to the first day of AP Chemistry Class.

The number one indicator of how a student will perform in AP Chemistry is SELF MOTIVATION!!!!!

The Summer Assignment is very reasonable. However, DO NOT wait until the end of summer break to begin the packet.

Materials needed for class!

1. Completed Summer Assignment Packet (please have completed the first day of school)

2. Three Ring Binder (2.5 in.)3. Blue or Black Ink Pen4. A Pencil5. A Red Pen 6. A Calculator that you know how to use . A graphing calculator is not necessary. A TI-30

will suffice.

FINALLY, the first Exam will be over the material covered in the Summer Assignment. It is on the THIRD DAY of school .

Khan Academy is a wonderful resource if you need assistance with any of the material covered in this assignment. Videos for Khan Academy can be viewed directly from the site or on Youtube.

NEVER, NEVER, NEVER GIVE UP!!!!!!!!!!!!!!! W. CHURCHILL

You will need to know:

1. Polyatomic Ions. A list of relevant Polyatomic Ions is included. These need to be memorized prior to the first day of school.

2. Memorize the 7 Diatomic Molecules, N2, O2, F2, Cl2, Br2, I2, and H2 (remember, it looks like an upside down L or seven on the periodic table and H)

3. Elements #1 (H) – # 88 (Ra) AND Uranium (U) and Plutonium (Pu) on the Periodic Table. ( You will not be given a periodic table with the names of the elements in AP Chem. )

4. Know where the metals, nonmetals, metalloids are on the periodic table5. Nomenclature and formula writing6. Determine if a compound has covalent bonds, ionic bonds or both7. Naming Acids 8. Balancing 9. Reaction Types (Synthesis, Decomposition, Double Displacement, Single

Displacement, Combustion)10. Significant figures11. Scientific Notation12. Metric Conversions 13. Molar Conversions14. Lewis dot structures15. Polarity16. Electron configuration17. Stoichiometry18. Molarity19. Half-Life20. Oxidation Numbers/ Oxidation Reduction Reactions21. Net Ionic Equations

Many of life's failures are people who did not realize how close

they were to success when they gave up. T. Edison

Good Luck !!!!!

1. List the 7 diatomic molecules.

2. Name or give the symbol for the element or ion and determine if it is a metal, nonmetal or metalloid.

a. Nitrogenb. Hydrogenc. Irond. Sodiume. Brominef. Germaniumg. Bh. Ca+2

i. Lij. Mgk. Pbl. Znm. Sin. So. S-2

p. Cl-

q. Cr. Rubidiums. Silvert. Goldu. Cobaltv. Argonw. Xex. Indiumy. Fluoridez. Hydride

Don’t practice until you get it right. Practice until you can’t get it wrong. – Unknown

3. Name or give the formula for the following. Then, determine if the compounds or polyatomic ions have ionic bonds, covalent bonds, or both.

a. Calcium hydroxide b. Waterc. Copper (II) chlorided. NO3

e. NaClf. Ammonium hydroxideg. CO3

-2

h. CO2-2

i. LiHj. Zirconium (II) sulfidek. COl. Zinc sulfatem. PCl3

n. XeClo. Tin (IV) bromidep. Sulfuric acidq. iodater. Hydrochloric acids. Nitric acidt. Pb(CN)2

u. Carbon dioxidev. Carbon tetrachloridew. HClO4

x. HNO3

y. ClO3-1

z. PO4-3

Continuous effort - not strength or intelligence - is the key to unlocking our potential.

W. Churchill

4. Balance the equation for the following reactions. If the reaction is in words write-out the formulas before balancing it. Then, determine the reaction type (Synthesis, Decomposition, Single Displacement, Double Displacement or Combustion) (oxidation number for Zinc is +2, oxidation number for Silver is +1)

Type:a. H2 + N2 NH3 __________________

b. CH4 + O2 CO2 + H2O __________________

c. H2O2 H2O + O2 __________________d. zinc + hydrochloric acid hydrogen gas + zinc chloride __________________e. silver nitrate + zinc chloride silver chloride + zinc nitrate __________________

5. Molar Conversions : Solve the following. Use correct significant figures and units in your final answer. Show all work. Dimensional Analysis is preferred method for solving.

1 mole = 6.02 x 1023 molecules ( atoms, ions, formula units, etc. )( 6.02 x 1023 is Avogadro’s Number)

Molar Mass is the grams of a substance in 1 mole (g/mol) ( Ex. The m.m. of water is 18.01 g / 1 mole )

1 mole = 22.4 L (at STP) ( STP is standard temp and pressure)

a. 5.5 moles of water are how many grams of water?

b. 45 g of NaCl are how many moles of NaCl?

c. 2.35 x 1025 molecules of CO2 are how many moles of CO2?

How many grams of CO2?

d. 550 liters of oxygen gas (O2) at STP are how many moles of oxygen gas?

How many grams of oxygen gas?

6. Convert the following : a. 250 mg to ______gb. .00523 km to ________mc. 1.30 x 106 mm to _____kmd. 4.50 x 10-5 cm to _____kme. 1036 mg to _____µg ( µ = micro )f. 5.46 x 1015 pm to______m (p = pico )

7. Write the Electron Configuration and Lewis Dot Structure for the following atoms. Then, determine the number of Valence Electrons (the outer electrons) for each atom.

Ex. Fluorine 1s22s22p5 F. 1 valence electron

a. Hydrogenb. Lithiumc. Oxygend. Argone. Brominef. Radium

8. Draw the Lewis Dot Structure for the following. Determine if the molecule is Polar or Nonpolar. If the atom is Polar, indicate the partial positive (δ+) and partial negative ends (δ–) ends.

a. Cl2 e. N2

b. CH4 f. NH3

c. H2O g. HFd. O2 h. SO3

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Og Mandino

9. Stoichiometry: Show all work. Use the correct amount of significant figures and units in final answers. Dimensional Analysis is the preferred method of solving.

Use the following balanced equation to answer a. – d.

N2 + 3H2 2NH3

a. How many moles of hydrogen are needed to completely react with 2.0 moles of nitrogen?

b. What volume of hydrogen is necessary to react with 5.0 liters of nitrogen to produce ammonia? ( Assume STP conditions )

c. How many grams of hydrogen are necessary to react completely with 50.0 g of nitrogen?

d. What volume of NH3 at STP is produced if 25.0 g of N2 is reacted with an excess of H2?

Use the following balance equation to answer e.-g.

2KClO3 2KCl + 3O2

e. If 5.0 g of KClO3 is decomposed, what volume of O2 is produced at STP?

f. How many moles of KCl will be produced from 5.0 g of KClO3?

g. How many formula units of KCl will be produced from 5.0 g of KClO3?

10. Molarity : Solve the following. Show all work, use correct sig figs and units in final answer.

Molarity = moles of solute / liter of solution

a. What is the molarity of a solution in which 58 g of NaCl are dissolved in 1.0 L of solution?b. What is the molarity of a solution in which 10.0 g of AgNO3 is dissolved in 500. mL of

solution?

M1V1 = M2V2 ( volume needs to be in L)

c. How much concentrated 18 M sulfuric acid is needed to prepare 250 mL of a 6.0 M solution?

d. To what volume should 25 mL of 15M nitric acid be diluted to prepare a 3.0 M solution?

Education is the most powerful weapon which you can use to change the world. Nelson Mandela

11. Half-Life : Show all work. Include units in final answer.a. What is the half-life of a 100.0 g sample of nitrogen-16 that decays to 12.5 g of nitrogen-16

in 21.6 s?

b. All isotopes of technetium are radioactive, but they have widely varying half-lives. If an 800.0 g sample of technetium-99 decays to 100.0 g of technetium-99 in 639 000 y, what is its half-life?

c. A 208 g sample of sodium-24 decays to 13.0 g of sodium-24 within 60.0 h. What is the half-life of this radioactive isotope?

12. Oxidation Numbers : Determine the oxidation number for each element in the following.

a. H2O i. SO-2

b. CO2 j. F2

c. H2SO4 k. Znd. NaOH l. NH+

e. HFf. H2O2

g. MgCO3

h. LiNO3

13. Oxidation Reduction Reactions : For each reaction, determine what is being oxidized and what is being reduced ( remember: LEO, GER or OIL, RIG )

a. 2Li + CaCl2 Ca + 2LiCl

b. 2Mg + O2 2 MgO

c. HNO3 + H3PO3 NO + H3PO4

d. 4Al + 3O2 2Al2O3

14. Net-Ionic Equations : Write the balanced complete, total ionic, and net ionic equation for the following. Some will actions will require you to predict the products first. (use the Solubility Rules below)

a. AgNO3 (aq) + KCl (aq) ® AgCl (s) + KNO3 (aq)

b. manganese(II) chloride (aq) + ammonium carbonate (aq) ® manganese(II) carbonate (s) + ammonium chloride (aq)

c. K3PO4 (aq) + Al(NO3)3 (aq) ®

d. cobalt(III) bromide + potassium sulfide ®

Solubility Rules

1. All salts of Group IA, and ammonium are soluble.

2. All salts of nitrates, chlorates and acetates are soluble. 3. All salts of halides are soluble except those of silver(I), copper(I), lead(II), and mercury(I).  

4. All salts of sulfate are soluble except for barium sulfate, lead(II) sulfate, and strontium sulfate. 5. All salts of carbonate, phosphate and sulfite are insoluble, except for those of group IA and ammonium. 6. All oxides and hydroxides are insoluble except for those of group IA, calcium, strontium and barium.

7. All salts of sulfides and insoluble except for those of Group IA and IIA elements and of ammonium.