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PART I: Practical Mathematics (10 questions)

1. Consider the equation y = ax/b. Suppose that b is tripled, a remains constant, and y is decreased by a factor of two. The value of x has
   • decreased by a factor of 3/2
   • increased by a factor of 3
   • increased by a factor of 3/2
   • decreased by a factor of 2/3


2. Consider the equation y = az²/x³. Suppose that a remains constant, x is doubled, and z is increased by a factor of three. The value of y has
   • decreased by a factor of 1/72
   • increased by a factor of 9/8
   • decreased by a factor of 8/9
   • increased by a factor of 72


3. The product of the numbers 399.0, 0.00505, 2.01, and 10.0 is approximately
   • 40
   • 4
   • 20
   • 400


4. The sum of the numbers 1.017, 4.118, 3.993, and 3.019 is approximately
   • 48
   • 12
   • 11
   • 4


5. If we know that a (cx/b + b) = b, then x =
   • b²((1/a)-1)/c
   • c(a-1)/b²
   • ac/b² - 1
   • 1 - b²/x²


6. If we know that y = ax^-2(x - b)(x/a + b/a), then y =
   • ax⁴
   • x² + b²
   • x⁴ + b²x²
   • 1 - b²/x²


7. The equation y = 2a (x²-b²) = 0 is true for
   • x=-b
   • x=b/a
   • x=-b and +b
   • x=b and b/a²


8. Consider the following graph. The line is the graph is best described by the equation
   
   • y = x + 3
   • y = 3/x
   • y = -x/3
   • y = -x + 3


9. For the equation y = (5/9 x + 32), if y = 47 then x =
   • 29
   • 27
   • 63
   • 45


10. For the equation y = (3x - 1)(3x + 1), if x = 3 then y =
    • 80
    • 81
    • 82
    • 64

PART II: Numbers and Statistics (10 Questions)

1. The sum of 4.5 x 10^-5 and 0.05 x 10^-3 is
   • 5.45 x 10^-3
   • 4.55 x 10^-5
   • 0.50 x 10^-4
   • 9.5 x 10^-5


2. The product of the numbers 1.5 x 10^-3 and 0.5 x 10² is
   • 0.75 x 10^-3
   • 7.5 x 10^-3
   • 7.5
   • 75. x 10^-3


3. The quotient 0.63 divided by 900. is
   • 7.0 x 10^-5
   • 0.07 x 10²
   • 0.007
   • 0.0007


4. The mean of the series of numbers 1.5, 2.0, 2.7, 2.5 and 1.3 is
   • 2.0
   • 3.0
   • 1.5
   • 2.5


5. The median of the series of numbers 1.5, 2.0, 2.7, 2.5 and 1.3 is
   • 2.0
   • 2.5
   • 1.5
   • 10.0


6. A bag contains 2 red marbles and 2 white marbles. You randomly draw and remove one marble from the bag, and then draw and remove a second marble from the bag. The probability that both marbles are red is
   • 1/12
   • 1/6
   • 1/4
   • 1/2


7. You flip a coin 4 times. What is the probability that you flip 4 heads and 0 tails?
   • 0
   • 1/4
   • 1/8
   • 1/16


8. You flip a coin 2 times. The probability that you flip a head first and a tail second is
   • 1/2
   • the same as the probability of flipping two heads
   • greater than the probability of flipping two heads
   • less than the probability of flipping two heads


9. You have a bag with 17 white marbles and 54 red marbles. How many bags of 8 red marbles and 3 white marbles can you make?
   • 5
   • 6
   • 7
   • None of the above.


10. You have a bag with 11 white marbles and 39 red marbles. How many bags of 4 red marbles and 3 yellow marbles can you make?
    • 2
    • 13
    • 3
    • None of the above.

PART III: Units and Measures (10 Questions)

1. The top-to-bottom height of a standard 8 1/2 inch by 11 inch sheet of paper is approximately
   • 0.28 m
   • 0.32 m
   • 0.16 m
   • 0.24 m


2. The diameter of an average apple is approximately
   • 60 cm
   • 6 cm
   • 0.6 cm
   • 30 cm


3. The diameter of a hydrogen atom is approximately
   • 1 x 10⁶ m
   • 1 x 10^-2 m
   • 1 x 10^-6 m
   • 1 x 10^-10 m


4. The temperature of a normal room is approximately
   • 70 °C
   • 22 °C
   • 10 °C
   • 37 °C


5. The temperature of boiling water at sea level is approximately
   • 32 °F
   • 100 °F
   • 112 °F
   • 212 °F


6. Your body mass is approximately
   • 400 kg
   • 50 kg
   • 10 kg
   • 5 kg


7. The mass of a hydrogen atom is approximately
   • 1 x 10^-3 kg
   • 1 x 10^-10 kg
   • 1 x 10^-23 kg
   • 1 x 10^-27 kg


8. Consider the equation y = ab/c. If c is one centimeter, b is one kilometer, and a is one millimeter, then y =
   • 1000 cm
   • 0.01 km
   • 100 cm
   • 100 m


9. You are told that the speed of light is equal to the wavelength of the light multiplied by the frequency of the light wave. Take the speed of light to be 3. x 10⁸ m/s. If the wavelength of light is 3. x 10^-6cm, what is the frequency of light in Hertz (1 Hz = 1 s^-1)?
   • 9. x 10^-16 Hz
   • 9. x 10^-14 Hz
   • 1. x 10¹⁴ Hz
   • 1. x 10¹⁶ Hz


10. You are told that 4.184 joules of energy equals 1.000 calorie of energy. You read that a candy bar contains 200,000 calories of energy. How many joules of energy does the candy bar contain?
    • 5,000 joules
    • 800,000 joules
    • 50,000 joules
    • 200,000 calories

PART IV: Atoms, Elements and the Periodic Table (10 Questions)

1. The most stable isotope of carbon has
   • 6 protons and 6 neutrons
   • 6 protons and 7 neutrons
   • 4 protons and 8 neutrons
   • 4 protons and 9 neutrons


2. Naturally occurring chlorine (on Earth) is predominantly composed of a mixture of two isotopes, ³⁵Cl and ³⁷Cl. The molar mass of chlorine is approximately 35.5 g/mol. The most likely natural abundances of the two isotopes are
   • 50% chlorine-35 and 50% chlorine-37
   • 25% chlorine-35 and 75% chlorine-37
   • 60% chlorine-35 and 40% chlorine-37
   • 75% chlorine-35 and 25% chlorine-37


3. Which of the following atoms or ions is the largest?
   • Na⁺
   • Ne
   • F^-
   • He


4. Which of the following atoms or ions has the highest ionization energy?
   • H
   • He
   • Ne
   • Xe


5. Which of the following atoms or ions has the greatest electron affinity?
   • F
   • Na
   • Ne
   • S


6. Which of the following atoms or ions is the heaviest?
   • Na⁺
   • Ne
   • F^-
   • He


7. Which of the following atoms or ions is the most electronegative?
   • Na⁺
   • Cs
   • F
   • Ne


8. An atom of helium is observed to emit a photon of light. Which statement about the observation is certainly true?
   • After the transition, the helium atom is in its ground electronic state.
   • Before the emission, the helium atom was in an excited electronic state.
   • Before the emission, the helium atom was in its ground electronic state.
   • None of the above.


9. Light emissions from excited calcium ions are observed to be red. Light emissions from excited barium ions are observed to be pale green. Which statement about these observations is true?
   • The energy of the red photon is less than the energy of the green photon.
   • The energy of transition in the barium ion is greater than that in the calcium ion.
   • The energy of the photon emitted increases as the atomic number increases.
   • All of the above.


10. Which of the following pairs of elements have the most similar properties?
    • K and Ca (with atomic numbers 19 and 20)
    • Na and Ne (with atomic numbers 11 and 10)
    • Cu and Zn (with atomic numbers 29 and 30)
    • S and Te (with atomic number 16 and 52)

PART V: Molecules and their Properties (10 Questions)

1. Which of the following molecules is the most polar?
   • N₂
   • F₂
   • H₂O
   • H₂S


2. In the molecule MgX₂, the most likely identity of X is
   • Na
   • Ca
   • He
   • F


3. In the molecule PX₃, the most likely identity of X is
   • I
   • N
   • O
   • B


4. In the molecule H₂X, the most likely identity of X is
   • H
   • F
   • Te
   • N


5. Consider the following formulas for possible molecules composed of nitrogen and oxygen: (I) NO, (II) NO₂, (III) N₂O, (IV) NO₃^-, and (V) NO₃^2-. Which of these species are observed in nature as "stable" molecules or ions?
   • I and IV
   • I, II and IV
   • I, II, III and IV
   • All five species.


6. Consider the following formulas for possible molecules composed of carbon and oxygen: (I) CO, (II) CO₂, (III) C₂O, (IV) CO₃^-, and (V) CO₃^2-. Which of these species are observed in nature as "stable" molecules or ions?
   • I and II
   • I, II and III
   • I, II, and IV
   • I, II, and V


7. Consider the following formulas for possible molecules composed of carbon and hydrogen: (I) CH₂, (II) C₂H₂, (III) C₂H₃, (IV) C₂H₄, and (V) C₂H₆. Which of these species are observed in nature as "stable" molecules?
   • I , II, and V
   • I, II, III and IV
   • II, IV and V
   • III, IV and V


8. The formula for iron(III) oxide is
   • Fe₃O
   • Fe₂O₃
   • Fe₃O₄
   • FeO₃


9. The most appropriate name for CuO is
   • copper oxide
   • copper(I) oxide
   • copper(II) oxide
   • copper(III) oxide


10. The most appropriate name for PCl3 is
    • lead(III) chloride
    • phosphorus(III) chloride
    • phosphorus trichloride
    • lead trichloride

PART VI: Moles, percents, stoichiometry, and limiting reagents (10 Questions)

1. How many atoms are in a molecule of Ba(NO₃)₂?
   • 3
   • 2
   • 6
   • 9


2. Approximately how many moles of hydrogen molecules are in a 2.0 gram sample of hydrogen gas?
   • 1
   • 2
   • 6.02 x 10²³
   • 12.04 x 10²³


3. Approximately how many moles of hydrogen atoms are in mole of hydrogen gas?
   • 1
   • 2
   • 6.02 x 10²³
   • 12.04 x 10²³


4. A reaction for the creation of nitrous oxide from nitrogen and oxygen is 2 N₂ + O₂ → 2 N₂O If you react x molecules of nitrogen, what is the number of oxygen molecules that react?
   • x/2
   • x
   • 2x
   • 4x


5. An equation for the formation of nitrogen triiodide is N₂ + 3 I₂ → 2 NI₃ How many moles of nitrogen triiodide are produced from a reaction of 0.4 moles of nitrogen and 1.5 moles of iodine?
   • 1.0 mol
   • 0.4 mol
   • 0.8 mol
   • 0.2 mol


6. An equation for the combustion of cyclohexane is C₆H₁₂ (g) + 9 O₂ (g) → 6 H₂O (g) + 6 CO₂ (g) Suppose that 80.0L of cyclohexane gas reacts completely with 81.0L of oxygen gas. How many liters of carbon dioxide gas are produced (assuming the same temperature and pressure for the reactants and products)?
   • 108.0 L
   • 60.0 L
   • 480.0 L
   • 54.0 L


7. What is the empirical formula of cyclohexane, C₆H₁₂?
   • CH
   • CH₂
   • C₆H₁₂
   • None of the above


8. An equation for the combustion of methane (unbalanced) is CH₄ (g) + O₂ (g) → H₂O (g) + CO₂ (g) How many moles of oxygen react with every mole of methane, CH₄?
   • 2
   • 4
   • 6
   • 8


9. In the molecule methane, CH₄, the mass percent of hydrogen is most nearly
   • 4 %
   • 12.5 %
   • 25%
   • None of the above.


10. Consider the reaction for the production of metallic iron in a "blast furnace" Fe₂O₃ (s) + 3 CO (g) → 2Fe (s) + 3 CO₂ (g) Take the molar mass of iron to be 56. g/mol, the molar mass of carbon to be 12. g/mol, and the molar mass of oxygen to be 16. g/mol. Suppose that 320. grams of Fe₂O₃ reacts in excess carbon monoxide. What is the mass of metallic iron that is produced?
    • 224 g
    • 112 g
    • 56 g
    • 48 g

PART VII: Types of Chemical Reactions (10 Questions)

1. When zinc metal is mixed with hydrochloric acid Zn (s) + HCl (aq) →
   • there is no reaction.
   • the reaction produces ZnCl and water
   • the reaction produces ZnCl and hydrogen gas
   • the reaction produces ZnCl₂ and hydrogen gas


2. The reaction of magnesium with oxygen to produce magnesium oxide is
   • an acid/base reaction.
   • a reduction/oxidation reaction.
   • a dissolution precipitation reaction.
   • none of the above, as that reaction is impossible.


3. The reaction of aqueous saturated sodium chloride solution with a solution of sodium hydroxide is
   • an acid/base reaction.
   • a reduction/oxidation reaction.
   • a dissolution precipitation reaction.
   • none of the above, as there is no reaction.


4. The decomposition of hydrogen peroxide to produce water and oxygen gas is an example of
   • an acid/base reaction.
   • a reduction/oxidation reaction.
   • a dissolution precipitation reaction.
   • a metathesis reaction.


5. The burning of paper in the air is an example of
   • an acid/base reaction.
   • a reduction/oxidation reaction.
   • a dissolution precipitation reaction.
   • none of the above.


6. The reaction of potassium nitrate with sodium iodide in aqueous solution to produce potassium iodide is an example of
   • an acid/base reaction.
   • a reduction/oxidation reaction.
   • a dissolution precipitation reaction.
   • none of the above, as the reactants and products all exist as soluble ions.


7. The reaction of lead nitrate with potassium iodide in aqueous solution to produce lead iodide is an example of
   • an acid/base reaction.
   • a reduction/oxidation reaction.
   • a dissolution precipitation reaction.
   • none of the above, as the reactants and products all exist as soluble ions.


8. The reaction of hydrofluoric acid and potassium hydroxide is an example of a reaction between
   • a strong base and a strong acid.
   • a strong base and a weak acid.
   • a weak base and a weak acid.
   • a weak base and a strong acid.


9. A 25.0 mL volume of a 0.1 M solution of ammonia is titrated with a 0.5 M solution of hydrochloric acid. When the equivalence point is reached, how much hydrochloric acid has been added?
   • 1.0 mL
   • 5.0 mL
   • 10.0 mL
   • 25.0 mL


10. Consider the reduction/oxidation reaction of zinc metal with copper sulfate to produce zinc sulfate and copper metal. In that reaction
    • the copper is the oxidant and the zinc is the reductant.
    • the copper is the reductant and the zinc is the oxidant.
    • the copper and zinc are oxidants and the sulfate is the reductant.
    • the copper is the reducing agent and the zinc is the oxidizing agent.

PART VIII: Useful Notions from the Laboratory (20 Questions)

1. The density is defined as the mass per unit volume. The density of liquid water at room temperature is approximately 1 g/cm³. What is the mass of 3 cm³ of water?
   • 1/3 g
   • 3 g
   • 18 g
   • none of the above


2. The following diagram shows a set of shots at a target. The set of shots has a
   
   • low precision and low accuracy.
   • low precision and high accuracy.
   • high precision and high accuracy.
   • high precision and low accuracy.


3. The ideal gas constant R is defined as R = PV/nT. Suppose that you are told that the units of P are atm, the units of V are mL, the units of n are moles, and the units of T are K (degrees Kelvin). The corresponding units of R are
   • mL atm mol K
   • L atm / (mol K)
   • mL atm/ (mol K)
   • L / (atm mol K)


4. You are given two samples of metals and asked to determine if they are the same or different. Which property would you measure?
   • mass
   • temperature
   • length
   • density


5. You prepare a solution of 0.10 moles of sodium acetate in 400. mL of water. The concentration of the solution of sodium acetate is
   • 0.25 M
   • 0.025 M
   • 0.4 M
   • 0.04 M


6. You are given 100. mL of a stock solution of 0.25 M potassium hydroxide. How many mL of the stock solution will you use to prepare 25. mL of a 0.10 M solution of potassium hydroxide?
   • 25. mL
   • 40. mL
   • 20. mL
   • 10. mL


7. You observe that a gram of powdered potassium nitrate dissolves faster in water than a gram lump of potassium nitrate. That is because
   • potassium nitrate doesn't dissolve in water.
   • powders are more easily stirred than a lump.
   • powders float on the surface of the water, which is where dissolution takes place.
   • powders have a greater surface area than a lump.


8. For any aqueous solution of strong base at room temperature, you can say that
   • the pH is less than 7.
   • the concentration of hydroxide ion is less than 10^-7mol/L.
   • the concentration of hydrogen ion is greater than 10^-7mol/L.
   • the concentration of hydroxide ion is greater than the concentration of hydrogen ion.


9. The most strongly basic solution is a 0.01M solution of
   • NH₃
   • NH₄Cl
   • NaCl
   • NaOH


10. The most strongly acidic solution is a 0.01M solution of
    • NH₃
    • NH₄Cl
    • NaCl
    • NaOH


11. The total concentration of ions in a 0.1M solution of MgCl₂ is
    • 0.1 M
    • 0.2 M
    • 0.3 M
    • essentially zero as MgCl₂ is insoluble.


12. You are given an aqueous solution of chloride ions and asked to “separate the chloride ions from the water molecules” using one of the following solutions. Which solution will you use?
    • 0.1 M calcium chloride
    • 0.01 M silver nitrate
    • 0.1 M potassium sulfate
    • 1.0 M ammonium dichromate


13. You are given a 0.1 M solution of hydrochloric acid and asked to deliver 0.01 moles into a flask using one of the following. Which will you choose?
    • A pipette
    • A barette
    • A beret
    • A burette


14. You are asked to prepare a dilute solution of sulfuric acid using a concentrated solution of sulfuric acid. In your preparation, you will
    • pour the acid into the water.
    • pour the water into the acid.


15. Which of the following compounds are soluble in water?
    • sodium hydroxide
    • zinc hydroxide
    • lead iodide
    • all of the above


16. You observe that when a particular salt is dissolved in water, the solution becomes cold. If you heat the solution, the
    • salt will become more soluble in water.
    • salt will become less soluble in water.
    • solubility of the salt will not change.


17. You have two samples of water. One is in an open flask. The other is in a vacuum flask in which the pressure is one-tenth of an atmosphere. The boiling point of the water is
    • the same in each flask.
    • higher in the vacuum flask.
    • lower in the open flask.
    • higher in the open flask.


18. You prepare a 1.00 L solution by dissolving 0.05 moles of sodium chloride in water. The concentration of the solution is
    • 0.050 M
    • 0.00500 M
    • 0.05 M
    • 0.5 M


19. You are asked to compute the molar mass of water, given that the molar mass of hydrogen is 1.0079 g/mol and the molar mass of oxygen is 16.00. You should report the molar mass of water as
    • 17.0079
    • 18.0079
    • 18.00
    • 18.01


20. The pH of a solution is defined as -log₁₀ [H⁺]. The pH of a solution of hydrochloric acid is measured to be 3.00. The concentration of hydrogen ion in solution, [H⁺], should be reported as
    • 1. x 10^-3 M
    • 1.0 x 10³ M
    • 1.00 x 10^-3 M
    • 1.000 x 10^-3 M

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