Name ______

Paris High School AP Chemistry Summer Assignment 2016

To: All Incoming AP Chemistry Students

From: Dr. Janet Dickey, AP Chemistry, 2016 ‐ 2017

Welcome to AP Chemistry!

I am looking forward to meeting all of you and hope our year is filled with learning as well as fun. AP Chemistry is an equivalent course to Introductory Chemistry in college. Taking a college level course in high school is difficult and requires dedication in addition to extra time spent on chemistry outside of class. Come in August ready to learn!

This summer assignment is designed to review the skills you should have and background information that you are expected to know at the start of the course in August. Having not taught you Pre-AP Chemistry, we will have to work together to assure that you are ready for the AP Chemistry material. Additionally, your ability to teach yourself and be resourceful will come into play. If there is something you cannot do, you must find resources in order to figure it out.

One very good resource is Andy Allan’s website; he has generously made his resources available to any teachers or students. The site includes Powerpoints, Interactive Practice Exercises, as well as links to other helpful sources. http://www.sciencegeek.net/APchemistry/index.shtml

PART I: Memorize the names of the elements and their corresponding symbols

·  You need to know elements 1-56, plus Pt, Au, Hg, Pb, Rn, Fr, Ra, U, Pu

·  Flashcards will be helpful!

·  It’s important to know these elements because the periodic table you are provided has only the symbols and not the names of the elements.

·  A QUIZ WILL BE GIVEN THE FIRST WEEK OF SCHOOL!

PART II: Memorize the common ions and polyatomic ions (LIST INCLUDED)

Unlike introductory chemistry, these ions must be easily identifiable by name and by formula in order to write adequate, balanced chemical equations. You must be able to write the name of the ion when given the formula and charge, and you must be able to write the formula and charge when given the name. A QUIZ WILL BE GIVEN THE FIRST WEEK OF SCHOOL!

PART III: Complete the attached worksheet. DUE AUGUST 23rd, your first grade for the course.

This Part is designed to review background information from Pre-AP Chemistry. It’s okay if you have to find help online; this is for your review.

Watch my school website. As we get closer to August, I hopefully will have this summer assignment available (for those who misplaced it). Don’t wait until the night before school starts to begin memorizing and working problems; otherwise, you will start behind before class ever begins.


AP Chemistry

PART III: Summer Assignment

1. Metric Conversions. Remember 1 cm3 = 1 mL 1 L = 1 dm3

GIVEN METRIC UNIT / DESIRED METRIC UNIT
8.43 cm / mm
2.41 x 102 cm / m
294.5 nm / cm
1.445 x 104 m / km
708 mL / L
9.005 x 10-7 L / nL
456000 cm3 / L
3.45 x 10-10 L / cm3
7.60 x 1011 µg / g
0.00593 kg / mg

2. Would you expect the following atoms to gain or lose electrons when forming ions? What ion (symbol and charge) is most likely in each case?

ELEMENT / GAIN OR LOSE / ION FORMED
K
Ba
P
O
Br
Rb

3. Chemical Nomenclature: Try to complete this using a periodic table and MINIMAL help from other sources. It will be to your advantage to have already memorized the common ions and polyatomic ions.

ITEM / CHEMICAL FORMULA / CHEMICAL NAME
A / NaBr
B / CaS
C / AlI3
D / Strontium fluoride
E / Potassium nitride
F / Magnesium phosphide
G / Hg2O
H / FeBr3
I / CoS
J / TiCl4
K / Tin (II) nitride
L / Cobalt (III) iodide
M / Mercury (II) oxide
N / Chromium (VI) sulfide
O / BaSO3
P / NaNO2
Q / KMnO4
R / K2Cr2O7
S / Chromium (III) hydroxide
T / Magnesium cyanide
U / Lead (IV) carbonate
V / Ammonium acetate
W / N2O4
X / ICl3
Y / SO2
Z / P2S5
AA / Diboron trioxide
BB / Arsenic pentafluoride
CC / Dinitrogen monoxide
DD / Sulfur hexachloride
EE / HC2H3O2
FF / H3PO3
GG / HCl
HH / Hydrofluoric acid
II / Sulfurous acid
JJ / Phosphoric acid

4. Chemical Reactions – Write and balance the following reactions.

a. Glucose (C6H12O6) reacts with oxygen gas to produce gaseous carbon dioxide and water vapor.

b. Solid iron (III) sulfide reacts with gaseous hydrogen chloride to form solid iron (III) chloride and hydrogen sulfide gas.

c. Carbon disulfide liquid reacts with ammonia gas to produce hydrogen sulfide gas and solid ammonium thiocyanate (NH4SCN).

d. Aqueous solutions of lead (II) nitrate and sodium phosphate are mixed resulting in the precipitate formation of lead (II) phosphate and aqueous sodium nitrate as the other product.

e. Solid zinc reacts with aqueous hydrochloric acid to form aqueous zinc chloride and hydrogen gas.

f. Aqueous calcium hydroxide is neutralized by aqueous phosphoric acid to produce solid calcium phosphate and water.

5. Chemical Calculations – You must show the work (on a separate sheet of paper) that leads to your answer to receive credit. Write your answers in the blanks to the left of the question.

Remember that: 1 mole element = 6.022 x 1023 atoms

1 mole compound = 6.022 x 1023 molecules or formula units

·  molecules refer to covalent compounds while formula units refer to ionic compounds (mathematically they mean the same thing)

A. Bauxite, the principle ore used in the production of aluminum, has the molecular formula of Al2O3·2H2O (aluminum oxide dihydrate).

______(i) What is the molar mass of bauxite?

______(ii) What is the mass of aluminum in 0.580 mol bauxite?

______(iii) How many atoms of aluminum are in 0.580 mol bauxite?

______(iv) What is the mass of 2.10 x 1024 formula units of bauxite?

B. Chloral hydrate (C2H3Cl3O2) is a drug formerly used as a sedative and hypnotic.

______(i) Calculate the molar mass of chloral hydrate.

______(ii) How many moles of chloral hydrate molecules are in 500.0 g of chloral hydrate?

______(iii) What is the mass in grams of 2.00 x 10-2 mol chloral hydrate?

______(iv) What number of chlorine atoms are in 5.00 g chloral hydrate?

______(v) What mass of chloral hydrate would contain 1.00 g Cl?

______(vi) What is the mass of exactly 500 molecules of chloral hydrate?

6. Stoichiometry –Show your work on a separate sheet of paper but write the answer in the blank to the left of the question. Remember the equation must be balanced.

A. The reaction between potassium chlorate and red phosphorus (P4) takes place when you strike a match on a matchbox. The products are tetraphosphorus decaoxide and potassium chloride. Answer the following questions using this reaction.

(i) Write the balanced chemical equation for this reaction.

______(ii) What mass of tetraphosphorus decaoxide is formed when 52.9 g of potassium chlorate reacts with an excess of red phosphorus?

______(iii) If the reaction produces 32.5 grams of tetraphosphorus decaoxide, what is the percent yield?

B. Phosphorus (P4) can be prepared from calcium phosphate by the following reaction:

Ca3(PO4)2 + SiO2 + C CaSiO3 + P4 + CO

(i) Balance the equation. [Hint: start with phosphorus]

______(ii) How many grams of carbon is need to react with 73.5 mg of silicon dioxide?

______(iii) Phosphorite is a mineral that contains Ca3(PO4)2 plus other non-phosphorus containing compounds. What is the maximum amount of P4 that can be produced from 1.00 kg of phosphorite if the phosphorite sample is 75% calcium phosphate by mass? Assume an excess of the other reactants.

C. 500 g sulfuric acid reacts with 400 g barium hydroxide producing a barium sulfate solid precipitate and water.

(i)Write and balance the equation for this reaction.

______(ii) Determine the limiting reactant.

______(iii) Calculate the mass of water produced.

______(iv) Calculate the mass of the excess reactant remaining after the reaction goes to completion.