Date: April 2000

Sample Tests

The site will contain a sample test for each major unit.
This site was written during the spring of 99 and sometimes the order is not quite the same from semester to semester.

The order of Test Five & Test Six are switched

Try the test at your convenience; write answers then check with answer page.
Tests will be internally anchored at this site. Answers will be written on another page; just click to answer page.

Test One

Nomenclature

• binary compounds
• criss cross
• univalent elements == No valence mentioned
• divalent elements == Roman Numerals or ...ous , ....ic
• prefixes for nonmetals

Write the formula for these compounds
UNIVALENT
1. calcium sulfide
2. sodium oxide
3. zinc chloride
4. ammonium hydroxide
5. aluminum iodide

DIVALENT Compouds
6. nickel (II) phosphide
7. ferrous hydroxide
8. gold (III) bromide
9. stannous sulphide
10. plumbic oxide

Write the name of these compound given the formula
UNIVALENT
11. K₂S
12. Sr₃N₂
13. Ag₃P
14. SO₃ prefix name prefered
15. MgO

DIVALENT
16. PCl₃
17. Fe₂Se₃
18. Cr₂O₃
19. Cu₃As
20. AuN

Test Two

Chapter One: Matter

• properties of matter & its classification
• mixtures & separating them
• Laws, hypothesis, models
• Law of Constant Composition ==> with math

Match the Columns

Indicate the type of reaction that is represented. Either physical or chemical

1. Frost forms on a car's windshield
2. Saliva acts on a cracker when you are chewing it
3. A copper wire is heated untill it glows red
4. Baking soda is mixed into a cake mix
5. Leaves start to turn colour
6. A candle burns
7. An iron bar becomes a magnet
8. You have dinner

Indicate the Class of Matter

1. sugar
2. orange juice
3. smoke
4. black coffee
5. polonium
6. brass

Written or Short Answers

1. Outline the steps that would enable you to separate a water, gasoline, sand and sugar mixture.
2. Give an example of a model and why it is used.
3. Calculate the percentage composition of zinc bromide given that the is 3.726 g of zinc and 9.104 g of bromine in the sample.

Test Three

This is an Atomic Theory Test with Law of Constant Composition thrown in for go measure.

Match the Columns

Name the Scientist

Math Problems

1. If the atom Cd comes in two isotopic forms ¹¹²Cd and ¹¹⁴Cd, find the relative abundance of each isotope given that the atomic weight is 112.46 u .
2. In a reaction with sodium and chlorine, it was found that 12.3 g of sodium upon reaction with chlorine gas produced 31.3 g of sodium chloride.
   1. How much chlorine gas reacted in this experiment?
   2. If 6.45 g of chlorine gas reacted, how much sodium chloride would be produced assuming there is sufficient sodium to complete the reaction?

Short Answer

1. What are the colours of the hydrogen spectrum? Explain why or how these lines are produced. (Use the theory)
2. What's the difference between an excited state and a ground state?
3. Explain the difference between the Lyman series and the Pashen series of the hydrogen spectrum. Give both a macroscopic answer and an atomic answer.

Atom & Electron Stucture

Atom/Ion	Isotopic Nomenclature	# of p	# of e	# of n	# of shells	electron configuration	# of valence electrons
magnesium
		25
sulfide ion
					5		4
						2,8,18,10,2

Test Four

Chemical Families and Trends in the Periodic Table and Bonding
A Chapter 3, 4, 5 Test;

Multiple Choice

1. Which element is the smallest?
   a) sodium, b) potassium, c) lithium, d) rubidium
2. Which element has the greatest electron affinity?
   a) oxygen, b) chlorine c) iodine, d) bromine
3. Which of these pairs are isoelectronic with each other?
   a) Ca²⁺ & Mg²⁺, b) S^2- & Ar, c) Ne & Cl^1- , d) Sr²⁺ & Br^1-
4. Which of these elements has the largest ionization energy?
   a) Ca, b) Cr, c) Zn, d) Br
5. Which of these elements will bond with potassium?
   a) sodium, b) calcium, c) krypton, d) bromine
6. How many lone pairs in the molecule CH₃CH₂CHClCH₂OH
   a) 2, b) 3, c) 4 d) 5, e) 6 .
7. Consider the elements Na, K, Cl, and Mg. Which of the following sets lists these elemnets in increasing order of ionization energy? (lowest first)
   a) Cl, Mg, Na, K . b) Mg, Na, Cl, K .
   c) Na, Mg, K , Cl . d) K, Na, Mg, Cl .
   
8. Element X is a gas at room temperature and is extremely reactive. Which of the following families might it most likely belong to?
   a) the noble gases, b) the halogens,
   c) the alkaline earth metals, d) the transition metal group.
   
9. The first five ionization energies of the element X are 0.456, 1.63, 3.06, 32.55, and 45.66 kJ/mol. Which of the following elements probably belongs to the same family as X?
   a) Sr, b) Ga, c) Ge, d) As, e) Se
10. Which of the following compounds is the most ionic?
    a) NaCl , b) MgS , c) SiCl₄ , d) Li₂S , e) NaI

Part II; Fill in the Blanks; Short answer

1. Predict how sodium will react with water. __________
2. Give two example of representative metals. ___________
3. State the Periodic Law ___________
4. Expalin why the chloride ion is larger than the chlorine atom. ___________
5. What is the shape of these molecules: ammonia NH₃, carbon tetrachloride CCl₄ , boron hydride BH₃.
6. How can one determine whether or not a bond is polar? _______________
7. Why is the sodium ion more stable than the sodium atom? ________
8. Draw a Lewis dot diagram for these
   1. atoms: aluminum, selenium and zinc
   2. molecules: carbon dioxide, hydrogen fluoride
   3. ions: ammonium & cyanide
9. What does the term isoelectronic mean and give an example _________
10. Outline an experiment to show whether or not cyclohexane C₆H₁₂ is polar or not. _______

Part III Bond formation and diagrams

1. Using Lewis structrures illustrate how the following sets of atoms bond and write the formula for each of the compunds formed.
   1. magnesium and iodine
   2. sodium and phosphorus
   3. aluminum and oxygen
2. Sketch molecular diagrams using stick structures for each of the molecules (Note: name and formula are given)
   1. CH₃CHCHCOOH ---- 2-butenoic acid
   2. C₅H₆ClCH₃ ---- 3-chloro-1-methylcyclopentene
   3. CH₃CH₂CHC₂H₅CHC₆H₅COCH₃ ---- 4-ethyl-3-phenyl -2-hexanone

Nomenclature: TEST FIVE

1. Na₂S
2. ammonium selenide
3. ferrous arsenide
4. NiO

TEST FIVE

Nomeclature & Balancing

Balancing: Insert coefficients as required

1. ___ HCl + ___ Ca(OH)₂ -------> ____ H₂O + ____ CaCl₂
2. ___ Zn + ___ H₃PO₄ -----> ___ Zn₃(PO₄)₂ + ___ H₂
3. ___ Fe(NO₃)₃ + NaOH -----> ___ Fe(OH)₃ + ___ NaNO₃
4. ___ C₄H₁₀ + ___ O₂ ----> ___ CO₂ + ___ H₂O
5. ___ Na₂CO₃ + ___ FeCl₃ + ___H₂O -----> ___ Fe(OH)₃ + ___ NaCl + ___ CO₂

Word Equation: Write balanced equations for these word equations

1. calcium hydroxide + phosphoric acid -------> calcium phosphate + water
2. potassium sulfate + ammonium nitrate ------> potassium nitrate + ammonium sulfate
3. magnesium carbonate + nitric acid ------> magnesium nitrate + carbon dioxide + water
4. plumbous nitrate + sodium sulfide -------> plumbous sulfide + sodium nitrate
5. copper + nitric acid ------> cupric nitrate + water + nitrogen monoxide

TEST SIX

Mole, Empirical Formula, Percent Composition

1. Find the percent composition of each element in these compounds:
   1. stannic phosphate
   2. K₂Cr₂O₇
2. How many moles are there in 17.94 grams of cuprous sulfate?
3. How many grams does a 4.731x10^-3 mol sample of Mo₂(SiO₃)₃ weigh?
4. How many atoms are there in a 243.2 gram sample of plumbous hydroxide?
5. Find the empirical formula of a compound given these percentages:
   • Ca = 43.23 %
   • P = 22.28 %
   • O = 34.50 %
6. Find the true formula for a compound that has a formula weight of 238 g/mol and the percentages are as follows:
   • Na = 19.3 %
   • S = 26.9 %
   • O = 53.8 %

TEST SEVEN

Working With the Balanced Equation

1. When sodium metal reacts with water sodium hydroxide and hydrogen gas are produced. If 7.45x10^-2 moles of sodium react, how many moles of sodium hydroxide are produced?
2. Given this reaction: Al(NO₃)₃ + Na₂SO₄ -----> Al₂(SO₄)₃ + NaNO₃ i) If 8.97x10^-3 moles of aluminum nitrate react how many grams of aluminum sulfate are produced?
   ii) How many grams of sodium sulfate are needed to produce 2.45 mole of sodium nitrate?
3. When 65.0 grams of butane (C₄H₁₀) are burned in oxygen gas, water and carbon dioxide are produced. How many grams of water are produced in this reaction and how many moles of oxygen are need to react with all 65.0 grams of butane?
4. In a double displacement reaction of plumbous nitrate and ferric chloride, 15.6 grams of plumbous nitrate is mixed with 26.9 grams of ferric chloride. Calculate how many grams of plumbous chloride is precipitated?
5. A reaction takes place in which the percentage yield is 67.8%. Calculate the mass of zinc produced in a single displacement reaction of vanadium metal and zinc chlorite when 18.94 grams of zinc chlorite are available to react. You can use the V⁺⁵ ion in your equation.
6. In the decomposition of copper (II) sulfate pentahydrate, a student heated 6.45 grams of this compound in a test tube. After heating the student was able to collect 1.98 grams of water. Determine the percentage yield of this reaction.
7. Complete these reactions; you should also know the reaction type.
   Don't forget to Balance
   • Zn + Cu(NO₃)₂ ---->
   • H₂SO₄ + NH₄OH ------>
   • LiHCO₃ ------>
   • Mg + HCl -------->
   • Al + O₂ ------>
8. Indicate the reaction type for the following: balance as needed
   • C₆H₁₄ + O₂ -----> CO₂ + H₂O
   • Pb(NO₃)₂ + NaCH₃COO -----> Pb(CH₃COO)₂ + NaNO₃
   • Ca(OH)₂ + H₃PO₄ --------> Ca₃(PO₄)₂ + H₂O
   • Cu + Cl₂ ------> CuCl₂
   • HgO -----------> Hg + O₂

TEST EIGHT

Gas Laws

1. Define these terms or Laws
   1. Boyle's Law
   2. Dalron's Law of Partial Pressure
   3. Avogadro's Hypothesis
   4. State the main tennants of Kinetic Molecular Theory
2. Using Kinetic Molecular Theory, explain the following
   1. Why a gas compressor gets hot when in use?
   2. Why a balloon's volume decreases when placed in a freezer?
   3. What happens to the density of a gas when it is heated?
   4. Explain boiling in terms of vapour pressure.

3. A gas at 17.5 ^oC has a pressure of 99.4 kPa. The gas is cooled to -14.6 ^oC. Calculate its new pressure.
4. A 4.56 L sample of propane (C₃H₈) at STP is heated to 56.8^oC with a pressure increase to 114.8 kPa.
   1. Calculate the new volume of this gas.
   2. What is the mass of this gas?
   3. What is the density of propane at the new conditions?

5. A 6.78 L sample of nitrous oxide (NO₂)is at STP. How many moles is this? What's its density?
6. A 10.0 L cylinder under 500 kPa pressure contains these gases; oxygen (45.6%), argon (28.5%) and the rest carbon dioxide. What is the individual pressure of each of these gases?
7. A 350g sample of dimethyl ether (CH₃COCH₃) at 125^oC is stored in a 500 mL cylinder. What is the pressure inside this cylinder?

TEST NINE

Using Gas Laws with the Balanced Equation

1. A gas at STP has a volume of 0.623L, how many moles is this?
2. Ammonia is used to make fertilizers. A large cylinder at 22.0^oC and 5000 kPa contains 2.5 x 10² kg of ammonia. What is the volume of this cylinder?
3. Given this reaction
   Zn + HCl_(aq) ----> ZnCl_{2 (aq)} + H_{2 (g)} If this reaction takes place at STP, calculate the volume of hydrogen gas produced when 75 g of zinc completely reacts.
4. When sodium carbonate react with hydrochloric acid sodium chloride, water and carbon dioxide are produced. Calculate the volume of carbon dioxide produced when 45.6 grams of sodium carbonate react at 22.7^oC and 102.8 kPa
5. Given the following reaction
   2KMnO₄ + 16HCl ----> 2MnCl₂ + 2KCl + 5Cl₂ + 8H₂O If an laboratory needs 10.0 L of chlorine gas, how much potassium permanganate is needed to react. The lab temperature is 21.4^oC at 99.8 kPa

TEST TEN

Solutions, Acid/Bases, Dilution Problems, Solution Stoichiometry

1. Outline how a supersaturated solution can be made.
2. What is the concentration of a solution in whci 12.8 g of sugar (C₁₂H₂₂O₁₁) dissolves into 450 mL of water? Assume that the final volume of the solution is 450 mL.
3. Looking at the graph of page 331 of Understanding Chemistry answer the following
   1. Which salt is the least soluble at 30^oC?
   2. If 100 g of potassium chloride is dissolved into 250 mL of water at 40^oC, what type of solution is produced? (Unsaturated, saturated or supersaturated) Don't just guess.
   3. A saturated solution of lead (II) nitrate is carefully cooled from 75^oC to 24^oC. This results in the formation of a ______________ solution. How many grams of solute will eventually precipitate from solution?
4. How can you experimentally tell the difference between a weak electrolyte and a strong electrolyte?
5. A solution contains the following salts; lead (II) nitrate, magnesium nitrate and calcium nitrate. Outline a scheme to separate each of the cations.
6. The pH of a solution is 11.4. What is the hydrogen ion concentration?
7. How many grams of ferrous nitrate are dissolved in a 350 mL solution which has a concentration of 0.258 mol/L (M)?
8. What is the pH of a solution that has a hydrogen ion concentration of 4.62 x 10^-4 mol/L?
9. Define what an indicator is. Give two examples and state what colours they are in both acid and base solutions.
10. Given this reaction Ba(NO₃)_{2 (aq)} + Na₂SO_{4 (aq)} -----> BaSO_{4 (s)} + NaNO_{3 (aq)}
    When a 0.423 mol of barium nitrate react, a solution, with a volume of 700 mL, of sodium nitate forms. What is the concentration of this solution?
11. If 25.0 mL of 6.00 mol/l HCl reacts with excess magnesium, how many grams of MgCl₂ are produced?
12. A 400 mL solution of hydrochloric acid has a pH of 3.22. It reacts with a 300 mL of a barium hydroxide solution with a pH of 9.22. Calculate the concentration of barium chloride after neutralization assuming that 75 grams of water are produced.
13. How many mL of stock sulphuric acid (18.0 mol/L) are required to make 875 mL sulphuric acid solution to a concentration of 1.25 x 10^-1 mol/L?
14. What is the purpose of a titration?

ANSWERS Click Here