AP Chemistry --Unit 1 In Class Problemsrodensapchemistry.weebly.com/uploads/5/1/3/6/5136176/unit_1_icp...AP Chemistry Unit 1 1 Denise DeMartino & Kelly Rosier AP Chemistry --Unit 1

AP Chemistry Unit 1 1 Denise DeMartino & Kelly Rosier

AP Chemistry --Unit 1

In Class Problems

1. Figure I shows a glass cylinder containing four liquids each of different density. Two of the liquids have been

identified. A table containing a list of substances and their density (at 25 °C) has been provided. From the list

select a substance for Liquid #1 and Liquid #3. Briefly explain the reason(s) for your selections and for the

remaining substances the reason they were not selected.

Substance Density (g

mL )

Mercury 13.5

Water (polar) 1.0

Hexane (non polar) 0.660

Ethyl alcohol (polar) 0.789

Dichloromethane (non polar) 1.33

Aluminum 2.699

Bromine (non polar) 2.928

Gold 19.3

2a. Review: Compare and contrast accuracy and precision.

b) Which set(s) of measurements are precise?

c) Which set(s) of measurements are accurate?

d) Which set(s) of measurements are both precise and accurate?

3a. Explain the difference between an exact number and an inexact number.

b) For each case, indicate whether the result is an exact or inexact number.

(i) The number of faces:

(ii) The mass of six apples

(iii) The number of seeds in an apple

(iv) The number of feet in one mile

(v) The number of liters in five quarts


3. a)_____________________ b)_____________________ c)_____________________


4. Complete the following calculations and record the result using the correct number of significant figures.

Answer to correct number

Calculation of significant figures

0.347 – 0.0732

23.436 + 82.2

(8.25 x 0.14)

0.834

12.45

(6.536 – 6.476)

99.003 + 2.091


Dimensional Analysis:

Don’t memorize!

Memorize!

6. A pencil 7.00 inches long. What is its length in centimeters?

7. The speed limit on many highways in the US is 55 mph. What would the number be in km per hour?

8. A Japanese car is advertised as having a gas milage of 15 km/L. Convert this rating to miles per gallon.


9. The latest model Corvette has en engine with a displacement of 6.20 L. What is it in cubic inches?

10. The density of concentrated sulfuric acid is 1.84 g/mL. Concentrated sulfuric acid is 95 % pure sulfuric acid. What volume of concentrated sulfuric acid contains 100 g of pure sulfuric acid?

Classification of Matter:


Particulates!!!

Practice doing these kind of drawings!!!!!!


11. Each diagram (A - P) show a sample of substances as viewed at the atomic level.

Characterize the contents of the container in terms of each of the following categories:

Category I: Homogeneous mixture, heterogeneous mixture or pure substance

Category II.: Element(s), compound(s) or both

Category III: Solid, liquid, gas or combination of phases


Separation of Mixtures:

12. For each of the separation techniques listed below, describe each and how it is used to separate the components of a mixture.

a) Decantation

b) Filtration

c) Evaporation


d) Distillation

e) Paper chromatography

f) Column chromatography


13. Law of Multiple Proportions


Introduction to the Periodic Table:

9. Given the following elements determine the number of electrons, protons and neutrons.

a) 10947

Ag

b) 2412

Mg

c) 2413

Al

d) 10747

Ag+


10. Charges of common univalent cations and anions?

Charges of multivalent cations?

Binary Nomenclature:

11. NaCl CaBr2

K2S Cu3N2

AlF3 Ag2Se

CoI3 SnS2


12. Calcium sulfide __________ barium fluoride __________

Cesium hydride __________ lithium phosphide __________

Copper (I) oxide __________ bismuth (V) sulfide __________

Nickel (III) bromide __________ cadmium nitride __________

13. NO SO3

NO2 P4O10

N2O4 NF3 ___________

P3N5 CCl4 ___________

14. Silicon dioxide __________ barium fluoride __________

Boron trichloride __________ lithium phosphide __________

Xenon tetrafluoride __________ tellurium tetraiodide __________

phosphorus pentabromide __________ sulfur dichloride __________


Ternary nomenclature

15. NH4NO3 NaCN

KNO2 BaSO4

Ca(ClO4)2 Hg2O

CuCO3 NaHCO3

16. lithium carbonate __________ zinc nitrate __________

Magnesium hydroxide __________ strontium sulfate __________

Lead (II) permanganate __________ iron (III) cyanide __________

Chromium (III) chloriate__________ lithium acetate __________


MIXED PROBLEMS:

17. Na2SO3 MgSO4

SCl2 CrPO4

KMnO4 Co2(CO3)3

MnO2 SO3

18. Chromium (VI) nitrite __________ nickel (II) hydroxide __________

Sulfur dioxide __________ sodium peroxide __________

Ammonium iodide __________ osmium (VIII) oxide __________

Copper (II) Phosphide__________ gold (III) chloride __________

Acid Nomenclature:


19. HCl (g) HClO

HCl (aq) H2SO4

HClO4 H2SO3

H2CO3 H3PO4

20. Hydrosulfuric acid __________ acetic acid __________

Nitric acid __________ hydrobromic acid __________

Hydrocyanic acid __________ phosphorous acid __________

Periodic acid __________ oxalic acid __________

21. Isotope Relative Mass Per Cent Abundance

20Ne 19.992 u 90.92 21Ne 20.994 u 2.57 22Ne 21.991 u 8.82 Find the avg atomic mass!


22. Two isotopes of chlorine exist in nature. 75.77% of chlorine is 35Cl with a mass of 34.96885 amu. What is the mass of the other isotope of chlorine?

23. Simple Mole Calcs


24. Two and three steppers!


25. Complete the following table

M, Molar m, Mass of n, Moles of N, Number of atoms,

Formula Mass

g

mol sample (g) sample (mol) molecules, or formula units

H2SO4 98.0 0.825

Cr2O3 9.63 x 1023

unknown 56.8 0.476

Mo 62.8

Do work below:


% Composition

26.Determine the percent composition of each element in Ni3(PO4)2.

Empirical and Molecular Formulas 27. Determine the empirical and molecular formulas for a compound that gives the following percentages on analysis:

71.65% Cl 24.27% C 4.07% H. The molar mass is known to be 98.96 g/mol.


28. Determine the empirical formula for a compound which is 26.6 % potassium, 35.4 % chromium and 38.1 % oxygen.

The compound has a molecular weight of 294.2 g/mol. What is the molecular formula?

Balancing and Stoichiometry:

29. Balance the following equation and draw a particulate diagram of all reactants and products.

C2H5 OH (g) + O2(g) → CO2(g) + H2O(g)

30. Determine the amount of iodine produced when 145 g of KI react with excess copper (II) chloride.

2CuCl2(s) + 4KI(s) → 2CuI(s) + 4KCl(s) + I2(s)


31.

32. An industrial method for the production of elemental zinc from its ore is to ‘roast’ the crude ore in oxygen

and then react it with CO. The following reactions describe the chemical process,

2ZnS(s) + 3O2(g) → 2ZnO(s) + 2SO2(g)

ZnO(s) + CO(g) → Zn(s) + CO2(g)

A 10.0 kg sample of an ore containing ZnS was chemically treated according to the reactions described above

producing 2.85 kg of Zn. Determine the percentage of ZnS contained in the original sample of the ore.


Limiting Reactant and % yield

33. In the reaction,

2C2H6(g) + 7O2(g) → 4CO2(g)+ 6H2O(g)

Determine the moles of CO2 and H2O formed when 2.00 moles of ethane are reacted with 10.0 moles of oxygen.

34. Calculate the mass of calcium nitride formed when 50.0 g of calcium react with 50.0 g of nitrogen according to the reaction.

3Ca(s) + N2(g) → Ca3N2(s)


35.

36. A common laboratory method for determination of arsenic is described in the reaction,

As2O3(aq) + 2I2(s) + 2H2O(l) → As2O5(aq) + 4HI(aq)

a) If 2.50 g of As2O3, 4.50 g of I2 and 4.00 g of H2O are mixed, and the reaction proceeds to completion,

which reactant is the limiting reagent?

b) Calculate the mass of As2O5 which is theoretically possible.

c) If only 1.80 g of As2O5 is actually produced, determine the percent yield in the reaction.


37. A 0.00300 g sample of napthalene, a compound containing only carbon and hydrogen, was burned in excess oxygen

to give 0.0103 g of CO2. Determine the empirical formula of napthalene. The formula weight of napthalene is 128 u,

determine the molecular formula.


Review Practice Problems! Answers provided


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AP Chemistry --Unit 1 In Class Problemsrodensapchemistry.weebly.com/uploads/5/1/3/6/5136176/unit_1_icp...AP Chemistry Unit 1 1 Denise DeMartino & Kelly Rosier AP Chemistry --Unit 1