A certain reaction is zero order in reactant A and second order in reactant B. What happens to the reaction rate when the concentrations of both reactants are doubled?

	a. The reaction rate remains the same.
	b. The reaction increases by a factor of two.
	c. The reaction increases by a factor of four.
	d. The reaction increases by a factor of eight.

.

A rate law relates which of the following?

	a. Reaction rate and temperature
	b. Reaction rate and concentration
	c. Temperature and concentration
	d. Energy and concentration

.

Determine the overall balanced equation for a reaction that has the following proposed mechanism. Which of the following is the acceptable rate law?
Step 1: B₂ + B₂ → E₃ + D slow
Step 2: E₃ + A → B₂ + C₂ fast

	a. B2 + B2 → E3 + D and R = [B2]2
	b. A + B2→ C2 + D and R = [A] [B2]2
	c. A + B2 → C2 + D and R = [B2]2
	d. A + B2→ C2+ D and R = [E3] [A]

.

Fill in the blank. A species that changes the rate of a reaction but is neither consumed nor changed in that reaction is a(n) ________________.

	a. Catalyst
	b. Activated complex
	c. Intermediate
	d. Reactant

.

If two molecules collide softly, what will most likely happen to the molecules?

	a. The molecules will be oriented favorably.
	b. The molecules will not be oriented favorably.
	c. The molecules are likely to react.
	d. The molecules may rebound without reacting.

.

The decomposition of nitrogen dioxide 2 NO₂ → 2 NO + O₂ occurs in a two-step sequence at elevated temperatures. The first step is NO₂ → NO + O. Which of the following accurately predicts the second step that, when combined with the first step, gives the complete reaction?

	a. NO2 + O → NO + O2
	b. O → NO + O2
	c. NO2→ NO
	d. O2→ NO + 3 O2

.

To be effective, a collision requires which of the following?

	a. Enough energy
	b. Favorable orientation
	c. A reaction mechanism
	d. Both A and B

.

What is the slowest step in a reaction mechanism called?

	a. The rate-determining step
	b. The uncatalyzed reaction
	c. The activation step
	d. None of the above

.

Which of the following statements most accurately describes the energy of the activated complex also called transition state?

	a. The transition state is lower than the energy of the reactants but higher than the energy of the products.
	b. The transition state is lower than the energy of both the reactants and the products.
	c. The transition state is higher than the energy of the reactants but lower than the energy of the products.
	d. The transition state is higher than the energy of both the reactants and the products.

.

Fill in the blank. The sequence of steps that occurs in a reaction process is called the _____________.

	a. Order of the reaction
	b. Reaction mechanism
	c. Overall reaction
	d. Rate law

.

A silver chloride solution is prepared with the following ion concentrations [Ag⁺] = 1.0 x 10^-6 M and [Cl^-] = 1.0 x 10^-2 M. If K_sp for AgCl = 1.8 x 10^-10, then which of the following is true?

	a. A precipitate will form.
	b. A precipitate will not form.
	c. The system is at equilibrium.
	d. None of the above

.

Acetic acid is a weak electrolyte, because it does which of the following?

	a. Becomes miscible with water
	b. Forms hydronium and hydroxide ions in aqueous solution
	c. Lowers the freezing point of water
	d. Ionizes only slightly in aqueous solution

.

How can one prepare a 1.00 L of a 0.125 M H₂SO₄ solution?

	a. Dilute 36.0 mL of 1.25 M H2SO4 to a volume of 1.00 L.
	b. Dilute 20.8 mL of 6.00 M H2SO4 to a volume of 1.00 L.
	c. Add 950. mL of water to 50.0 mL of 3.00 M H2SO4.
	d. Add 500. mL of water to 500. mL of 0.500 M H2SO4.

.

How many grams of Na₃PO₄ are there in 500. mL of a 0.250 M solution of Na₃PO₄ (molar mass = 163.94 g/mol)?

	a. 2.05 g
	b. 20.5 g
	c. 0.125 g
	d. 0.168 g

.

Solution A contains 0.1 mol of sucrose, C₁₂H₂₂O₁₁, dissolved in 500 g of water. Solution B contains 0.1 mol of sodium chloride, NaCl, in 500 g of water. Which of the following statements about these solutions is true?

	a. Both solutions have the same vapor pressure.
	b. Solution A would boil at a higher temperature than solution B would.
	c. Solution A would freeze at higher temperature than solution B would.
	d. Both solutions would boil at the same temperature.

.

The solubility of AgCl is 1.22 x 10^-8 mol/L. What is the value of K_sp for AgCl?

	a. 1.1 x 10⁻4
	b. 1.2 x 10⁻8
	c. 5.7 x 10⁻2
	d. 1.5 x 10⁻16

.

To make a water-soluble salt using the silver cation, Ag+, what anion should be chosen?

	a. NO3⁻
	b. CO32⁻
	c. Cl⁻
	d. PO43⁻

.

Use the solubility rules. Which salt is insoluble in water?

	a. NaBr
	b. NH4Cl
	c. FeS
	d. (NH4)2S

.

Use the solubility rules. Which salt is soluble in water?

	a. Fe(OH)3
	b. AgCl
	c. CaCl2
	d. BaSO4

.

What is the balanced, net ionic equation for the reaction of nickel(II) chloride and sodium phosphate to give nickel(II) phosphate and sodium chloride?

	a. 2 Na3PO4(aq) + 3 NiCl2(aq) → Ni3(PO4)2(s) + 6 NaCl(aq)
	b. 2 Na3PO4(aq) + 3 NiCl2(aq) → Ni3(PO4)2(aq) + 6 NaCl (aq)
	c. 2 PO43⁻(aq) + 3 Ni2⁺(aq) → Ni3(PO4)2(s)
	d. Na⁺(aq) + Cl⁻(aq) → NaCl(aq)

.

What is the balanced, net ionic equation for the reaction of aluminum sulfate with sodium hydroxide?

	a. Al2(SO4)3(aq) + 6 NaOH(aq) → 2 Al(OH)3(s) + 3 Na2SO4(aq)
	b. Al3⁺(aq) + 3 OH⁻(aq) → Al(OH)3(s)
	c. Al2(SO4)3(aq) + 6 NaOH(aq) → 2 Al(OH)3(aq) + 3 Na2SO4(s)
	d. 2 Na⁺(aq) + SO42⁻(aq) → Na2SO4(s)

.

What is the correct expression for the solubility product constant, K_sp, for FePO₄?

	a. Ksp = [Fe3⁺] / [PO43⁻]3
	b. Ksp = [Fe3⁺][P5⁻][O2⁻]3
	c. Ksp = [Fe3⁺][PO43⁻]
	d. Ksp = [Fe3⁺][PO43⁻] / [FePO4]

.

What is the molality of a 0.907 M Pb(NO₃)₂ solution? (Molar mass of Pb(NO₃)₂ = 331.2 g/mol; density of the solution = 1.252 g/mL.)

	a. 0.953 m
	b. 0.724 m
	c. 0.907 m
	d. 1.98 m

.

What is the molality of a solution containing 5.67 g glucose, C₆H₁₂O₆, dissolved in 25.2 g of water? (Molar mass of C₆H₁₂O₆ = 180.2 g/mol.)

	a. 0.00125 m
	b. 0.225 m
	c. 1.25 m
	d. 0.762 m

.

What is the molarity of a 0.273 m KCl? (Molar mass of KCl = 74.6 g/mol; density of the solution = 1.011 g/L.)

	a. 20.6 M
	b. 1.0 M
	c. 0.273 M
	d. 0.271 M

.

What is the new concentration of a nitric acid made by diluting 50. mL of a 12.0 M solution to 250. mL?

	a. 2.4 M
	b. 60. M
	c. 10. M
	d. 24 M

.

What is the total concentration of ions in a 0.0360 M solution of Na₃PO₄?

	a. 0.108 M
	b. 0.144 M
	c. 0.0360 M
	d. 0.0720 M

.

What volume in mL of 0.453 M NaCl solution contains 25.0 g of NaCl (molar mass = 58.5 g/mol)?

	a. 193 mL
	b. 1000 mL
	c. 943 mL
	d. 453 mL

.

Which of the following is NOT a colligative property?

	a. Molality
	b. Vapor-pressure lowering
	c. Boiling-point elevation
	d. Osmotic pressure

.

Which one of the following compounds is a nonelectrolyte when dissolved in water?

	a. Sodium chloride
	b. Calcium chloride
	c. Copper sulfate
	d. Sugar

.

A buffer is prepared by adding 45.0 mL of 0.15 M NaF to 35.0 mL of 0.10 HF. What is the pH of the final solution? The value of K_a for HF is 6.8 x 10^-4.

	a. 4.65
	b. 2.20
	c. 7.00
	d. 3.45

.

A solution contains 0.0128 g of HCl in 450. mL of solution. What is the pH of this solution at 25 °C?

	a. 1.00
	b. 7.00
	c. 3.10
	d. 10.89

.

A solution contains 0.384 g of KOH in 250. mL of solution. What is the pH of this solution at 25 °C?

	a. 1.56
	b. 12.44
	c. 2.67
	d. 11.33

.

An important component of blood is the buffer combination of dihydrogen phosphate ion and the hydrogen phosphate ion. The pH of blood is 7.44. What is the pH of blood, if 25% of the hydrogen phosphate is converted to dihydrogen phosphate? The value of K_a for H₂PO₄^- is 6.2 x 10^-2.

	a. 2.90
	b. 6.59
	c. 7.44
	d. 7.16

.

At 10 °C, K_w = 2.9 x 10^-15. What is [OH^-] in neutral water at 10 °C?

	a. 4.44 x 10⁻6 M
	b. 1.00 x 10⁻7 M
	c. 1.70 x 10⁻7 M
	d. 5.39 x 10⁻8 M

.

At 50 °C, K_w = 5.48 x 10^-14. What is [OH^-] in water of pH = 3 at 50 °C?

	a. 1.00 x 10⁻3 M
	b. 5.48 x 10⁻11 M
	c. 5.48 x 10⁻7 M
	d. 2.74 x 10⁻7 M

.

HC₂Cl₃O₂ is a stronger acid than HCHO₂. What is the direction of the equilibrium of the following reaction?
HC₂Cl₃O₂(aq) + CHO₂^-(aq) → C₂Cl₃O₂^-(aq) + HCHO₂(aq)

	a. The equilibrium lies to the left.
	b. The equilibrium lies to the right.
	c. The equilibrium is perfectly balanced left and right.
	d. This cannot be determined from the information given.

.

H₃PO₄ is a stronger acid than NH₄⁺. What is the direction of the equilibrium of the following reaction?
NH₄⁺(aq) + H₂PO₄^-(aq) → NH₃(aq) + H₃PO₄(aq)

	a. The equilibrium lies to the left.
	b. The equilibrium lies to the right.
	c. The equilibrium is perfectly balanced left and right.
	d. This cannot be determined from the information given.

.

The following solutions are mixed in equimolar portions. Will the resulting solution be acidic, basic, neutral, or is there not enough information given?
HCl(aq) + NaHCO₃(aq) → ?

	a. Acidic
	b. Basic
	c. Neutral
	d. This cannot be determined from the information given.

.

What are the products of the following acid-base reaction?
HCl(aq) + NaOH(aq) → ?

	a. H3O⁺(aq) + OH⁻(aq)
	b. Na⁺(aq) + Cl⁻(aq)
	c. H2O(l) + NaCl(aq)
	d. No reaction takes place.

.

What is a Brønsted-Lowry acid?

	a. A proton donor
	b. A proton acceptor
	c. An electron pair donor
	d. An electron pair acceptor

.

What is a Lewis acid?

	a. A proton donor
	b. A proton acceptor
	c. An electron pair donor
	d. An electron pair acceptor

.

What is a Lewis base?

	a. A proton donor
	b. A proton acceptor
	c. An electron pair acceptor
	d. An electron pair donor

.

What is the pH of a buffer solution that is 0.15 M chloroacetic acid and 0.10 M sodium chloroacetate? The value of K_a for chloroacetic acid is 1.3 x 10^-3.

	a. 11.3
	b. 3.76
	c. 2.68
	d. 3.91

.

What is the pH of the buffer solution that consists of 0.15 M pyridine and 0.10 M pyridinium bromide? The value of K_b for pyridine is 1.4 x 10⁹.

	a. 6.60
	b. 3.50
	c. 5.32
	d. 7.00

.

What is the [OH^-] of a 5.43 x 10^-4 M solution of HNO₃ at 25 °C?

	a. 1.84 x 10⁻11 M
	b. 5.43 x 10⁻10 M
	c. 5.43 x 10⁻4 M
	d. 3.67 x 10⁻8 M

.

What will happen to the pH a solution of NH₃ by adding HCl?

	a. The pH will increase.
	b. The pH will decrease.
	c. The addition of HCl will not change the pH of the solution.
	d. There is not enough information given to determine this.

.

Which of the following is an acid-base conjugate pair?

	a. HF and F⁻
	b. HNO2 and NO3⁻
	c. HClO and Cl⁻
	d. H2CO3 and CO32⁻

.

Which of the following is NOT an acid-base conjugate pair?

	a. HCN and CN⁻
	b. HNO3 and NO3⁻
	c. HCl and ClO⁻
	d. NH4⁺ and NH3

.

What is a Brønsted-Lowry base?

	a. A proton donor
	b. A proton acceptor
	c. A hydroxide donor
	d. An electron pair donor

.

A particular voltaic cell operates on the following reaction.
Zn(s) + Cl₂(g) → Zn²⁺(aq) + 2 Cl^-(aq)
Given an emf of 0.853 V, calculate the maximum electrical work generated when 20.0 g of zinc metal is consumed.

	a. -8.23 x 104 J
	b. -1.65 x 105 J
	c. -5.03 x 104 J
	d. -2.51 x 104 J

.

A voltaic cell has the following reaction.
Zn(s) + 2 Fe³⁺(aq) → 2 Fe²⁺(aq) + Zn²⁺(aq) E° = 0.72 V
What is the maximum electrical work that can be obtained from this cell per mole of iron (III) ion?

	a. +69 kJ
	b. -140 kJ
	c. -69 kJ
	d. 1.4 J

.

Cadmium reacts spontaneously with copper(II) ion.
Cd(s) + Cu²⁺(aq) → Cd²⁺(aq) + Cu(s)
What are the half reactions for this reaction?

	a. Cd(s) + 2e⁻ → Cd2⁺(aq) and Cu2⁺(aq) + 2e⁻ → Cu(s)
	b. Cd(s) → Cd2⁺(aq) + 2e⁻ and Cu2⁺(aq) → Cu(s) + 2e⁻
	c. Cd(s) → Cd2⁺(aq) + e⁻ and Cu2⁺(aq) + e⁻ → Cu(s)
	d. Cd(s) → Cd2⁺(aq) + 2e⁻ and Cu2⁺(aq) + 2e⁻ → Cu(s)

.

Calculate the emf for a cell operating with the following reaction:
Cr₂O₇^2-(aq) + 6 I^-(aq) + 14 H⁺(aq) → 2 Cr³⁺(aq) + 3 I₂(s) + 7 H₂O(l),
where [Cr₂O₇^2-] = 0.020 M, [I^-] = 0.015 M, [Cr³⁺] = 0.20 M and [H⁺] = 0.50 M, using the following standard reduction potentials:
Cr₂O₇^2-(aq) + 14 H⁺(aq) + 6 e^- → 2 Cr³⁺(aq) + 7 H₂O(l) E° = +1.33 V
I₂(s) + 2 e^- → 2 I^-(aq) E° = +0.54 V

	a. +1.87 V
	b. -1.87 V
	c. +0.79 V
	d. +0.64 V

.

Calculate the equilibrium constant K for the following reaction at 25 °C.
2 Fe³⁺(aq) + Cu(s) → 2 Fe²⁺(aq) + Cu²⁺(aq) E° = +0.43 V

	a. 7.26
	b. 0.43
	c. 3.4 x 1014
	d. 1.7 x 107

.

Calculate ΔG° for the following reaction at 25 °C.
3 Cu(s) + 2 NO₃^-(aq) + 8 H⁺(aq) → 3 Cu²⁺(aq) + 2 NO(g) + 4 H₂O(l) E° = +0.62 V

	a. -3.6 x 105 J
	b. -6.0 x 104 J
	c. 3.6 x 105 J
	d. 1.2 x 105 J

.

Fill in the blank. When a piece of iron is left outside, it will rust. In this situation, the iron atoms are _______________.

	a. Losing electrons
	b. Gaining electrons
	c. Staying neutral
	d. Combining with nitrogen gas from the air

.

Given the following two half reactions,
Cd²⁺(aq) + 2e^- → Cd(s) E° = -0.40 V
2 Ag⁺(aq) + 2e^- → 2 Ag(s) E° = 0.80 V
determine E° and the spontaneity of the following reaction:
2 Ag⁺(aq) + Cd(s) → 2 Ag(s) + Cd²⁺(aq)

	a. +0.40 V and not spontaneous
	b. +1.20 V and spontaneous
	c. +1.20 V and not spontaneous
	d. -0.40 V and spontaneous

.

Given the two following half reactions,
Cl₂(g) + 2e- → 2 Cl^-(aq) E° = +1.36 V
I₂(g) + 2e- → 2 I^-(s) E° = +0.54 V
calculate ΔG° for the following reaction:
2 I-(aq) + Cl₂(g) → 2 Cl-(aq) + I₂(s).

	a. -1.6 kJ
	b. -7.9 x 104 J
	c. -1.6 x 105 J
	d. -79 kJ

.

Given the two following half reactions,
Sn²⁺(aq) + 2e^- → Sn(s) E° = -0.14 V
Cu²⁺(aq) + 2e^- → Cu(s) E° = +0.34 V
calculate the standard emf for the following reaction:
Sn(s) + Cu²⁺(aq) → Sn²⁺(aq) + Cu(s).

	a. 0.96 V
	b. -0.48 V
	c. +0.20 V
	d. 0.48 V

.

Given the two following half reactions,
Cr³⁺(aq) + 3e^- → Cr(s) E° = -0.74 V
Hg2²⁺(aq) + 2e^- → Hg(l) E° = +0.80 V
calculate the standard emf for the following cell:
Cr | Cr³⁺|| Hg2²⁺| Hg

	a. -0.06 V
	b. -1.54 V
	c. +1.54 V
	d. +0.06 V

.

How many coulombs of charge are required to form 1.00 pound of Al(s) from an Al³⁺ salt?

	a. 4.87 x 106
	b. 50.5
	c. 1.62 x 106
	d. 454

.

If we wish to convert 1.00 g of Au³⁺(aq) ion into Au(s) in a “gold-plating" process, how long must we electrolyze a solution if the current passing through the circuit is 2.00 amps?

	a. 245 sec
	b. 0.50 sec
	c. 0.015 sec
	d. 735 sec

.

Of the following four reactions, how many are oxidation-reduction reactions?
NaOH + HCl → NaCl + H₂O
Cu + 2 AgNO₃ → 2 Ag + Cu(NO₃)₂
Mg(OH)₂ → MgO + H₂O
N₂ + 3 H₂ → 2 NH₃

	a. 0
	b. 1
	c. 2
	d. 3

.

The voltaic cell Cd | Cd²⁺|| Ni²⁺| Ni has an E° of 0.170 V. If the standard reduction potential of Ni²⁺/Ni is E° = -0.23 V, what is the standard reduction potential for Cd²⁺/Cd?

	a. +0.06 V
	b. -0.06 V
	c. -0.40 V
	d. +0.40 V

.

The voltaic cell Cd | Cd²⁺|| Ni²⁺ (1.0M)| Ni has an electromotive force of 0.240 V at 25 °C. What is the concentration of cadmium ion? (Please note that E° = 0.170 V.)

	a. 0.06 M
	b. 0.04 M
	c. 0.004 M
	d. 1.0 M

.

What are the half reactions for the electrolysis of LiCl(l)?

	a. Cathode: Li⁺(l) → Li(l) + e⁻ and Anode: 2 Cl⁻(l) → Cl2(g) + 2 e⁻
	b. Cathode: Li⁺(l) → Li(l) + e⁻ and Anode: 2 Cl⁻(l) + 2 e⁻ → Cl2(g)
	c. Cathode: 2 Cl⁻(l) → Cl2(g) + 2 e⁻ and Anode: Li⁺(l) + e⁻ → Li(l)
	d. Cathode: Li⁺(l) + e⁻ → Li(l) and Anode: 2 Cl⁻(l) → Cl2(g) + 2 e⁻

.

What is the cell notation for a voltaic cell with the following equation?
Pb²⁺(aq) + Cd(s) → Pb(s) + Cd²⁺(aq)

	a. Pb | Pb2⁺|| Cd2⁺| Cd
	b. Pb2⁺ | Pb || Cd | Cd2⁺
	c. Cd | Cd2⁺|| Pb2⁺ | Pb
	d. Cd | Pb2⁺|| Pb | Cd2⁺

.

What is the correct balanced equation for the following oxidation-reduction reaction?
Cr₂O₇^2- + C₂O₄^2- → Cr³⁺ + CO₂

	a. Cr2O72⁻ + 3 C2O42⁻ → 2 Cr3⁺ + 6 CO2
	b. 28 H⁺ + 2 Cr2O72⁻ + 3 C2O42⁻ → 4 Cr3⁺ + 6 CO2 + 14 H2O
	c. 14 H⁺ + Cr2O72⁻ + C2O42⁻ → Cr3⁺ + 2 CO2 + 7 H2O
	d. 14 H⁺ + Cr2O72⁻ + 3 C2O42⁻ → 2 Cr3⁺ + 6 CO2 + 7 H2O

.

What is the overall cell reaction for the following voltaic cell?
Fe | Fe²⁺|| Ag⁺| Ag

	a. Ag⁺(aq) + Fe(s) → Ag(s) + Fe2⁺(aq)
	b. 2 Ag⁺(aq) + Fe(s) → 2 Ag(s) + Fe2⁺(aq)
	c. 2 Ag(s) + Fe2⁺(aq) → 2 Ag⁺(aq) + Fe(s)
	d. Fe(s) + Fe2⁺(aq) → Ag⁺(aq) + Ag(s)

.

Fill in the blank. In the reaction Cu(s) + 4HNO₃(aq) → Cu(NO₃)₂(aq) + 2NO₂(g) + 2H₂O(l), copper is __________.

	a. Reduced
	b. Electrolyzed
	c. Synthesized
	d. Oxidized

.

Beta decay of the nucleus of produces which of the following nuclide?

	a. Ra
	b. Ac
	c. Pa
	d. U

.

Sodium is a very reactive metal. Its ion is found in table salt. While non-radioactive sodium is abundant, there exists a radioactive isotope of sodium, Sodium-24. Its half life is 15 hours. If after 60 hours, about 6 grams remain, then what was the original mass of the sodium-24 sample?

	a. 50 g
	b. 40 g
	c. 100 g
	d. 60 g

.

Technetium-99 has a half-life of 6.0 hrs. What fraction of Technetium-99 in the sample will remain undecayed after 36 hours?

	a. 1/8
	b. 1/64
	c. 1/32
	d. 1/16

.

The half life of Colbalt-60 is 5.2 years. What happens to an aliquot of cobalt-60 after 5.2 years?

	a. The concentration decreases by half.
	b. The cobalt changes to cobalt-30.
	c. The cobalt-60 atom breaks in half.
	d. The concentration doubles.

.

What are beta particles?

	a. Highly active electrons diffused from radioactive nuclei
	b. Less active protons diffused from standard nuclei
	c. Highly active neutrons in radioactive nuclei
	d. X-rays that allow radioactive nuclei’s to be viewed

.

What is the amount of radioactive sample that has NOT decayed after three-half lives have elapsed?

	a. 1/3 the original amount
	b. 1/9 the original amount
	c. ¼ the original amount
	d. 1/8 the original amount

.

What is the correct alternate notation for gold-197?

	a.
	b.
	c.
	d.

.

What is the half-life of a radioactive nuclide?

	a. The period of time in which 25% of the original number of atoms undergoes radioactive decay
	b. The time at which the isotope becomes non radioactive
	c. The period of time in which 50% of the original number of atoms undergoes radioactive
	d. The period of time it takes to reduce radioactivity by 100%

.

Which nuclide contains 11 protons, 11 electrons, and 14 neutrons?

	a. Silicon-11
	b. Silicon-14
	c. Sodium-11
	d. Sodium-25

.

Which of the following best describes how the atomic number changes when a nucleus captures an electron?

	a. It will increase by one.
	b. It will decrease by one.
	c. It will not change, because the electron has such a small mass.
	d. It will increase by two.

.

Which of the following elements is the daughter nuclide for the alpha decay of polonium-212?

	a. Lead-208
	b. Lead-216
	c. Radon-208
	d. Radon-216

.

Which type of radiation has the most penetrating ability?

	a. An alpha particle
	b. A beta particle
	c. A gamma ray
	d. A neutron

.

Which of the following processes is NOT an example of a spontaneous radioactive process?

	a. Alpha-decay
	b. Auto ionization
	c. Positron production
	d. Beta-decay

.

Fill in the blank. CH₃CH₂CH₂C≡CCH₂CH₂Cl is named __________.

	a. 7-chloro-4-heptyne
	b. 5-chloro-2-heptene
	c. 1-acetylenenyl-3-chloropropane
	d. 1-chloro-3-heptyne

.

How many structural isomers does butane have?

	a. 1
	b. 2
	c. 3
	d. 4

.

How many types of alkyl groups can arise from propane?

	a. 0
	b. 1
	c. 2
	d. 3

.

Kira was doing some organic chemistry nomenclature problem. She gave a molecule the following name: 2-Methyl-4-methylhexane. While one can correctly draw the molecule from the name she gave, the name violates the IUPAC rules. What is the IUPAC name of the molecule?

	a. 2,4-dimethylhexane
	b. 3-Methyl-5-methylhexane
	c. 3,5-dimethylhexane
	d. 1-isopropyl-2-methylbutane

.

Nylon is an example of which of the following?

	a. Copolymer
	b. Homopolymer
	c. Dimer
	d. None of the above

.

Teflon is an example of which of the following?

	a. Copolymer
	b. Homopolymer
	c. Dimer
	d. None of the above

.

The name methanal is the IUPAC name for which of the following?

	a. Acetone
	b. Formaldehyde
	c. Water
	d. Rubbing alcohol

.

What is the general name given to hydrocarbons with double bonds?

	a. Alkenes
	b. Alkynes
	c. Alkanes
	d. Aromatic hydrocarbons

.

What is the name of the following molecule?
CH_3-(CH₂)₇-CH₃

	a. Heptane
	b. Hexane
	c. Octane
	d. Nonane

.

Which of the following accurately provides the generalized molecular formulas for alkanes and alkenes respectively?

	a. CnH2n+2 and CnH2n
	b. CnH2n and CnH2n+2
	c. CnH2n+2 and CnH2n-2
	d. CnH2n and CnH2n+1

.

Which of the following CANNOT form alkenes?

	a. Methane
	b. Ethane
	c. Propane
	d. All of the above

.

Which of the following has the greatest number of C-O bonds?

	a. Ketone
	b. Ester
	c. Alcohol
	d. Amine

.

Which of the following has the least number of C-O bonds?

	a. Ketone
	b. Alcohol
	c. Ether
	d. Ester

.

Which of the following is known as rubbing alcohol?

	a. Methanol
	b. Ethanol
	c. Propanol
	d. Isopropanol

.

Which of the following is known as wood alcohol?

	a. Methanol
	b. Ethanol
	c. Propanol
	d. Isopropanol

.

In a triple bond, how many electrons are shared?

	a. 3
	b. 4
	c. 5
	d. 6

.