Honors Chemistry Pre-Test Questions - 1986 Verified Questions

Honors Chemistry Pre-Test

Questions

Course Introduction

Honors Chemistry is an advanced introductory course designed for students with a strong interest in the fundamental principles of chemistry. The course covers key topics such as atomic structure, chemical bonding, stoichiometry, thermochemistry, kinetics, equilibrium, acids and bases, and electrochemistry. Emphasis is placed on scientific inquiry, laboratory techniques, problem-solving skills, and real-world applications of chemical concepts. Students are challenged to analyze data, formulate hypotheses, and draw evidence-based conclusions through rigorous labs and projects, preparing them for further study in science or related fields.

Recommended Textbook

Chemical Principles 6th Edition by Professor Peter Atkins

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Page 2

Chapter 1: The Quantum World

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Q1) What wavelength does radiation possess when its frequency is 2.1 * 10¹⁵ Hz?

A)4.1 * 10^-7 cm

B)1.4 * 10^-7 m

C)6.5 * 10⁶ m

D)7.0 * 10⁶ m

E)1.4 * 10^-7 nm

Answer: B

Q2) Comparing the lowest energy transition,\(\Delta\)E,in1,3-butadiene(A)and 1,3,5,7-octatetraene(B),\(\Delta\)E_A is greater than \(\Delta\)E_B.

A)True

B)False

Answer: True

Q3) The four \(\pi\) electrons of 1,3-butadiene can be modeled as particles in a box.If the length of 1,3-butadiene (L)is 0.56 nm,calculate the energy of the lowest energy transition.

Answer: 9.6 * 10^-¹⁹ J

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Chapter 2: Quantum Mechanics in Action: Atoms

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Q1) Which of the following is not a metal?

A)Ba.

B)Br.

C)Ga.

D)Al.

E)Hg.

Answer: B

Q2) Which atom has the highest first ionization energy?

A)Mg

B)Ca

C)Sr

D)Ba

Answer: A

Q3) Write the ground-state electron configuration of a europium atom.

A)[Xe]5d⁷6s²

B)[Xe]4f²5d⁵6s²

C)[Xe]4f⁹

D)[Xe]4f⁷6s²

E)[Xe]4f⁵5d²6s²

Answer: D

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Chapter 3: Chemical Bonds

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Sample Questions

Q1) Consider the following equilibrium:

S₂O₄²^-(aq) 2SO₂^-(aq)

K ~ 10^-⁹

Write a Lewis structure for each species.

Answer: The arrangement of atoms in S₂O₄²^- is O₂S-SO₂.The latter has a Lewis structure that obeys the octet rule,but SO₂^- is a radical.

Q2) Use the bond enthalpies given to estimate the heat released when ethene,CH₂=CH₂,reacts with HBr to give CH₃CH₂Br.Bond enthalpies (kJ.mol^-¹):

C-H,412; C-C,348; C=C,612; C-Br,276; Br-Br,193; H-Br,366.

A)1036 kJ.mol^-¹

B)200 kJ.mol^-¹

C)470 kJ.mol^-¹

D)424 kJ.mol^-¹

E)58 kJ.mol^-¹

Answer: E

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Page 5

Chapter 4: Molecular Shape and Structure

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Sample Questions

Q1) The bond order of O₂²⁺ is A)1.

B)2.

C)3.

D)2.5.

E)1.5.

Q2) The molecules OF₂ and O₃ both have bent shapes.What are the approximate bond angles in OF₂ and O₃,respectively?

A)109^o and 120^o

B)Both 109^o

C)Both 120^o

D)Both 180^o

E)109^o and 180^o

Q3) All the following are polar except

A)O₃.

B)ClF₃.

C)COCl₂.

D)BrO₃^-

E)CS₃²^-

Q4) What is the ground-state electron configuration of O₂^-?

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Chapter 5: The Properties of Gases

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Q1) The number of molecules in 44.8 L of nitrogen at exactly 0S1U1P1\(\circ\)S1S1P0C and 3.00 atm is

A)1.20 * 10²⁴

B)3.61 * 10²⁴

C)3.61 * 10^-23

D)2.01 * 10²³

E)18.0 * 10^-²³

Q2) Under what conditions do real gases act least like ideal gases?

A)High temperatures and low pressures.

B)High pressures and low molar masses.

C)Low temperatures and high pressures.

D)High temperatures and high pressures.

E)Low temperatures and low pressures.

Q3) What is the density of xenon gas at 750 kPa and 25S1U1P1\(\circ\)S1S1P0C?

A)5.30 g.L^-¹

B)0.392 g.L^-¹

C)39.7 g.L^-¹

D)79.5 g.L^-¹

E)19.9 g.L^-¹

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Page 7

Chapter 6: Liquids and Solids

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Q1) If the radius of an atom is r,what is the length of the side of the body-centered cubic unit cell?

A)4r/3^½

B)2.25r

C)r

D)2r

E)8^½r

Q2) Water was found to rise to a height of 7.4 mm in a tube of internal radius 2.0 mm at room temperature.Given its density as 1.0 g.cm^-3,what is the surface tension of water?

A)0.15 N.m^-1

B)0.036 N.m^-1

C)7.3 * 10^-8 N.m^-1

D)0.073 N.m^-1

E)1.5 * 10^-7 N.m^-1

Q3) Butane and 2-propanone have approximately the same boiling points.True or false?

A)True

B)False

Q4) Sodium has a body-centered cubic unit cell.If the atomic radius of sodium is 190 pm,what is the density of sodium?

Page 8

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Chapter 7: Inorganic Materials

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Q1) Graphite and diamond are two forms of the same element,carbon.What is the term for two such forms of an element?

A)Isotopes.

B)Solid phases.

C)Physical states.

D)Allotropes.

E)Carbotropes.

Q2) What element besides iron and carbon is necessary to produced stainless steel?

A)Chromium.

B)Vanadium.

C)Phosphorus.

D)Sulfur.

E)Zinc.

Q3) Which statement about a semi-conductor is correct?

A)When it conducts,its resistance is extremely high.

B)When it conducts,it does so with 0 resistance.

C)Its resistance increases as the temperature increases.

D)Its resistance decreases as the temperature increases.

Q4) A metal sample can be considered a sea of __________________ (protons,electrons,neutrons)in an array of cations.

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Chapter 8: Thermodynamics: The First Law

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Q1) The standard enthalpy of formation of NaCl(s)is -411 kJ/mol.In a Born-Haber cycle for the formation of NaCl(s),which enthalpy change(s)is/are endothermic?

A)the lattice enthalpy of NaCl(s)

B)the electron affinity of chlorine

C)the reverse of the lattice enthalpy of NaCl(s)

D)All of the enthalpy changes are endothermic except for the standard enthalpy of formation of NaCl(s).

Q2) Give \(\Delta\)H_r values for each of the following reactions from the information below.

\(\Delta\)H_fS1U1P1\(\circ\)S1S1P0(HCl(g))= -92.31 kJ.mol^-1

H-Cl bond enthalpy = +431 kJ.mol^-1

O-H bond enthalpy = +463 kJ.mol^-1

\(\Delta\)H_fS1U1P1\(\circ\)S1S1P0(H₂O(g))= -241.8 kJ.mol^-1

(a)2H(g)+ O(g)\(\rightarrow\)H₂O(g)

(b)H₂(g)+ Cl₂(g)\(\rightarrow\) 2HCl(g) (c)H(g)+ Cl(g)\(\rightarrow\) HCl(g)

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Chapter 9: Thermodynamics: The Second and Third Laws

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Sample Questions

Q1) Which of the following has the smallest molar entropy?

A)C(diamond)

B)C₆₀(s)

C)CaCO₃(s)

D)CO₂(s)

E)C(graphite)

Q2) Which of the following would probably have a positive \(\Delta\)S value?

A)He(g,2 atm)\(\rightarrow\) He(g,10 atm)

B)H₂(g)+ I₂(s)\(\rightarrow\) 2HI(g)

C)2Ag(s)+ Br₂(l)\(\rightarrow\) 2AgBr(s)

D)O₂(g)\(\rightarrow\) O₂(aq)

E)2NO₂(g)\(\rightarrow\)N₂O₄(g)

Q3) Consider the reaction Cl₂(g)\(\rightarrow\) 2Cl(g)

Which of the following statement regarding this reaction is true?

A)The reaction is spontaneous at high temperatures.

B)The reaction is spontaneous at low temperatures.

C)The reaction is not spontaneous at any temperature.

D)The reaction is spontaneous at all temperatures.

Q4) All the halogens exist as diatomic molecules at room temperature and 1 bar.Under these conditions,which of the halogens,F to I,has the smallest molar entropy?

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Chapter 10: Physical Equilibria

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Sample Questions

Q1) Of the following,which would likely dissolve in toluene?

A)Na₂CO₃

B)NaCl

C)C₆H₁₂O₆

D)Ca(HCO₃)₂

E)Cl₂CCCl₂

Q2) Benzene would likely dissolve which of the following substances?

A)Cl₂CCCl₂

B)NaCl

C)Na₂CO₃

D)Ca(HCO₃)₂

E)C₆H₁₂O₆

Q3) Which liquid would you expect to be the more volatile,CH₃CHO or CH₃OCH₃?

Q4) For a one-component system,at the triple point

A)f = 3.

B)f = 2.

C)p = 1.

D)f = 0.

E)f = 1.

Page 12

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Chapter 11: Chemical Equilibria

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Q1) Consider the reaction

4NH₃(g)+ 7O₂(g) 2N₂O₄(g)+ 6H₂O(g)

If,initially,[NH₃(g)] = [O₂(g)] = 3.60 M,at equilibrium,[N₂O₄(g)] = 0.60 M.Calculate the equilibrium concentrations of all other species.

Q2) Given: C(s)+ CO₂(g)

2CO(g) At equilibrium at a certain temperature,the partial pressures of CO(g)and CO₂(g)are 1.22 atm and 0.780 atm,respectively.Calculate the value of K for this reaction.

A)3.13

B)2.00

C)1.91

D)1.56

E)0.640

Q3) For any reaction at equilibrium,\(\Delta\)G < 0.

A)True

B)False

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Chapter 12: Acids and Bases

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Sample Questions

Q1) Calculate the hydroxide ion concentration for an aqueous solution that has a pH of 3.45.

A)3.2 * 10^-2 M

B)0.54 M

C)3.5 * 10^-4 M

D)2.8 * 10^-11 M

E)2.6 * 10^-5 M

Q2) What is the pK_a of the conjugate acid of hydrazine,given that the pK_b of hydrazine is 5.77? Write the formula of the conjugate acid of hydrazine.

Q3) Of the following,which is the strongest acid?

A)CH₃COOH (pK_a = 4.75)

B)HNO₂ (pK_a = 3.37)

C)HF (pK_a = 3.45)

D)HCN (pK_a = 9.31)

E)HIO₃ (pK_a = 0.77)

Q4) In liquid ammonia,the base B is a strong base if it is a stronger proton acceptor than NH₂^-.

A)True

B)False

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Chapter 13: Aqueous Equilibria

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Q1) Assuming no volume change on mixing,what mass of ammonium chloride should be added to 1.00 L of 0.250 M NH₃(aq)to produce a buffer of pH 10.10? The molar mass of ammonium chloride is 53.49 g/mol.

Q2) If 10.0 mmol of sodium hydroxide is added to 1.00 L of a buffer that is 0.200 M HClO(aq)and 0.155 M NaHClO(aq),the final concentrations of HClO(aq)and ClO^-(aq),respectively,are

A)0.190 M and 0.155 M.

B)0.210 M and 0.155 M.

C)0.210 M and 0.165 M.

D)0.190 M and 0.165 M.

E)0.200 M and 0.155 M

Q3) Calculate the [H⁺] in an aqueous solution that is 0.0755 M HF and 0.100 M NaF.The value of K_a for HF is 3.5 * 10^-4.

A)4.6 * 10^-4 M

B)2.6 *10^-4 M

C)3.5 * 10^-4 M

D)0.176 M

E)0.0755 M

Q4) What is the main factor that directly determines the pH of any buffer?

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Chapter 14: Electrochemistry

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Q1) The standard potential of the Cu²⁺/Cu electrode is +0.34 V and the standard potential of the cell Pb(s)|Pb²⁺(aq)m Cu²⁺(aq)|Cu(s)

Is +0.47 V.What is the standard potential of the Pb²⁺/Pb electrode?

A)-0.26 V

B)+0.81 V

C)-0.81V

D)-0.13 V

E)+0.13 V

Q2) The galvanic cell shown above uses the half-cells Pb²⁺/Pb and Zn²⁺/Zn,and a salt bridge containing KCl(aq).The voltmeter gives a positive voltage reading.Identify A and write the half-reaction that occurs in that compartment.Does the size of the electrode A increase or decrease during operation of the cell? What is the voltmeter reading?

Q3) When a sample of an unknown metal is dropped into 1 M H⁺(aq)under standard conditions,bubbles are observed.The unknown metal could be silver.

A)True

B)False

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Chapter 15: Chemical Kinetics

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Q1) The rates of first-order and second-order reactions do not change with elapsed time.

A)True

B)False

Q2) Consider the mechanism

NO₂(g)+ F₂(g)\(\rightarrow\) NO₂F(g)+

F(g)k₁ (slow)

F(g)+ NO₂(g)\(\rightarrow\) NO₂F(g)k₂ (fast) Give the molecularity of the first step and any intermediates in the mechanism.

A)2,and F(g)

B)2,and NO₂F(g)

C)2,and NO₂(g)

D)1,and no intermediate

E)2,and no intermediate

Q3) For a zero-order reaction,the rate constant has the same units as the rate of reaction.

A)True

B)False

Q4) What is the half-life of a second order reaction?

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Chapter 16: The Elements: the Main Group Elements

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Q1) What two types of bonds involving hydrogen does diborane exhibit?

Q2) Which of the following is a saline carbide?

A)SiC

B)CaC₂

C)Mo₂C

D)Fe₃C

E)W₂C

Q3) Order the following ions according to their radii from largest to smallest: H^-,Cl^-,^-.

Q4) What is the shape of XeOF₄?

A)trigonal bipyramidal

B)square planar

C)T-shaped

D)square pyramidal

E)octahedral

Q5) What is the function of aluminum in the thermite reaction?

Q6) In the following reaction,what role does CO play?

PbO(s)+ CO(g)\(\rightarrow\) Pb(s)+ CO₂(g).

Q7) Sulfur dioxide can act as both an oxidizing agent and a reducing agent; explain.

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Q8) When phosphoric acid is heated it undergoes a ________________ reaction.

Chapter 17: The Elements: The D Block

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Q1) The ligand field splitting energy is greater for complexes of \(\pi\)-acid ligands than for complexes of \(\pi\)-base ligands.

A)True

B)False

Q2) Which of the following complexes is chiral?

A)[Co(en)₃]³⁺

B)[RuCl₃(CN)₃]^3-

C)[Co(NH₃)₆]³⁺

D)trans-[Cr(en)₃]³⁺

Q3) Which of the following is expected to be the best oxidizing agent?

A)Cu⁺(aq)

B)Ti³⁺(aq)

C)CrO₄^2-(aq)

D)VO₂⁺

E)Cr²⁺(aq)

Q4) rhodium complexes are high spin?

A)True

B)False

Q5) In the following reaction,what acts as the Lewis acid? MgO(s)+ SO₂(g)\(\rightarrow\) MgSO₃(s)

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Chapter 18: Nuclear Chemistry

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Q1) Radioactive decay is a

A)first-order process.

B)second-order process.

C)nonspontaneous process.

D)temperature-dependent process.

E)zero-order process.

Q2) Heavy elements are more likely to give off \(\alpha\) radiation.

A)True

B)False

Q3) Bombarding ⁵⁴Fe with a neutron results in emission of a proton and formation of

A)⁵⁵Fe.

B)⁵⁴Cr.

C)⁵⁴Co.

D)⁵⁴Mn.

E)⁴⁹Ti.

Q4) Nuclides that lie below the band of stability are proton rich and can form more stable nuclei by _______________,___________________,and

Q5) Why does the band of stability curve upward at high atomic number?

Page 20

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Chapter 19: Organic Chemistry I

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Q1) Arenes undergo predominantly addition reactions.

A)True

B)False

Q2) When 2-methyl-1-butene reacts with HBr,the reaction occurs in two steps.What is the major product? (Hint: Intermediate carbocations are most stable when formed at tertiary carbons.)

Q3) The alkene CH₃CH=CHCH₂CH₃ cannot exist as cis and trans isomers.

A)True

B)False

Q4) The product of the reaction of 2-butene with Cl₂ is

A)3,3-dichlorobutane.

B)2,3-dichlorobutane.

C)butane.

D)2-chlorobutane.

E)2,2-dichlorobutane.

Q5) A racemic mixture is an equal mixture of enantiomers and therefore is optically active.

A)True

B)False

Page 21

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Chapter 20: Organic Chemistry II

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Q1) The product of the reaction of CH₃CH₂CHO with excess KMnO₄(aq)in acidic solution is

A)CH₃CH₂COOH.

B)CH₃CH₂COCH₂CH₃.

C)CH₃COOH.

D)CH₃CH₂CH₃.

E)CH₃CH₂OH.

Q2) Oxidation of secondary alcohols produces A)acids.

B)aldehydes.

C)ketones.

D)Secondary alcohols cannot be oxidized.

E)ethers.

Q3) All the following produce a silver mirror with Tollens reagent except A)HCHO.

B)CH₃CH₂CH(CHO)CH₃.

C)CH₃CH₂COCH₃.

D)CH₃(CH₂)₃CHO.

E)CH₃CH₂CHO.

Q4) What reactants would be used to synthesize diethyl ether?

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