Introductory Chemistry Pre-Test Questions - 1997 Verified Questions

Introductory Chemistry

Pre-Test Questions

Course Introduction

Introductory Chemistry provides a foundational understanding of the key concepts in chemistry for students new to the subject. The course covers the structure and properties of matter, chemical reactions, stoichiometry, solutions, atomic theory, and bonding. Students will learn how to interpret the periodic table, perform basic laboratory experiments safely, and solve quantitative chemical problems. Emphasis is placed on developing scientific reasoning and problem-solving skills, preparing students for further study in chemistry or related sciences.

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Chemical Principles The Quest for Insight 7th Edition by Peter Atkins

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11 Chapters

1997 Verified Questions

1997 Flashcards

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Chapter 1: Atoms

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Sample Questions

Q1) Which of the following species is isoelectronic with Kr?

A) K⁺

B) Cl^-

C) Ar

D) Xe

E) Sr²⁺

Answer: E

Q2) If radiation has a frequency of 3.1 * 10¹⁶ sec^-1, what is its wavelength?

A) 1.0 * 10⁸ cm

B) 1.0 * 10^-8 cm

C) 1.0 * 10⁸ m

D) 1.0 * 10^-8 m

E) 3.0 * 10^-8 m

Answer: D

Q3) In each pair, which ionization reaction is larger?

(a)I₃ of B; or I₃ of Be

(b)I₄ of C; or I₃ of B

Answer: (a)I₃ of Be

(b)I₄ of C

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Chapter 2: Molecules

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Sample Questions

Q1) What hybrid orbitals are used by the N atoms in urea, H₂NCONH₂?

A) sp

B) sp²

C) sp³

D) dsp³

Answer: C

Q2) Predict the HNH bond angle in NH₂^-.

Answer: ~109^o

Q3) All the following have an angular shape except

A) HOCl.

B) S₃^2-.

C) I₃^-.

D) ClO₂^-.

E) NH₂^-.

Answer: C

Q4) Predict the N-O bond lengths in NO₂^- given the N-O and N=O bond lengths of 140 and 120 pm,respectively.

Answer: Both ~ 130 pm

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Chapter 3: States of Matter

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Sample Questions

Q1) How does an alloy's electrical and thermal conductivity compare to that of one of its pure elements?

A) There is generally no change.

B) They are higher.

C) They are lower.

D) Electrical is lower, thermal is higher.

E) Electrical is higher, thermal is lower.

Answer: C

Q2) How is steel defined?

A) A heterogeneous iron alloy with up to 2% carbon.

B) A homogeneous iron alloy with up to 2% carbon.

C) Any heterogeneous alloy with up to 2% carbon.

D) Any homogeneous alloy with up to 2% carbon.

E) Any iron, carbon alloy with a low melting point.

Answer: B

Q3) If the compression factor,Z,is less than one for a given gas,the van der Waals coefficient "a" is dominant for real gases

A)True

B)False

Answer: True

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Chapter 4: Thermodynamics

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Sample Questions

Q1) Calculate the change in molar entropy when the pressure of argon is allowed to double isothermally (assume ideal behavior).

A) +1.39 J.K^-¹.mol^-¹

B) -1.39 J.K^-¹.mol^-¹

C) -4.16 J.K^-¹.mol^-¹

D) -5.76 J.K^-¹.mol^-¹

E) +5.76 J.K^-¹.mol^-¹

Q2) What mass of propane, C₃H₈(g),Must be burned to supply 2580 kJ of heat? The standard enthalpy of combustion of propane at 298 K is -2220 kJ.mol^-¹

A) 25.6 g

B) 51.2 g

C) 102 g

D) 75.9 g

E) 37.9 g

Q3) Combustion reactions can be exothermic or endothermic.

A)True

B)False

Q4) Work is reported in joules; and 1 joule = ____________

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Chapter 5: Equilibrium

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Sample Questions

Q1) Consider the reaction

CO₂(g)+ C(s)\(\rightarrow\) 2CO(g)

At equilibrium,at a certain temperature,the partial pressures of CO₂(g)and CO(g)are 23.5 and 8.21 atm,respectively.Calculate the value of K_P.

Q2) The van't Hoff equation can be used to obtain the standard reaction enthalpy for a reaction if the equilibrium constant for the reaction is known at two different temperatures.

A)True

B)False

Q3) Which of the following pairs have a vant Hoff i factor of 2?

A) Sodium sulfate and potassium chloride

B) Sodium chloride and magnesium sulfate

C) Magnesium sulfate and ethylene glycol

D) Glucose and sodium chloride

E) Perchloric acid and barium hydroxide

Q4) Calculate the molality of ethanol in a solution of water,given that the mole fraction of ethanol is 0.300.

Q5) What is the vapor pressure of carbon disulfide at its normal boiling point?

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Chapter 6: Reactions

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Sample Questions

Q1) All galvanic cells require a salt bridge in order to operate.

A)True

B)False

Q2) When equilibrium is reached in an electrochemical cell,the voltage reaches its maximum value.

A)True

B)False

Q3) A cell that uses bromine to oxidize chloride ion under standard conditions at 298 K has a positive potential.

A)True

B)False

Q4) Given: S₂O₄²^-(aq) \(\rightarrow\)SO₃²^-(aq),Basic solution. How many electrons appear in the balanced half-reaction?

A) 3

B) 6

C) 1

D) 4

E) 2

Q5) What is the conjugate acid of O²^-?

Page 8

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Chapter 7: Kinetics

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Sample Questions

Q1) Consider the reaction

2N₂O₅(g)\(\rightarrow\)

4NO₂(g)+ O₂(g)

Rate = k[N₂O₅]

Calculate the time for the concentration of N₂O₅ to fall to one-fourth its initial value if the half-life is 133 s.

A) 133 s

B) 33.3 s

C) 266 s

D) 66.6 s

E) 533 s

Q2) If the average rate of formation of H₂(g) is 3.90 (mol H₂).L^-¹.s^-¹ for the reaction2PH₃(g)\(\rightarrow\)2P(g)+ 3H₂(g),The unique average reaction rate is

A) 3.90 mol.L^-¹.s^-¹.

B) 1.30 mol.L^-¹.s^-¹.

C) 2.60 mol.L^-¹.s^-¹.

D) 7.80 mol.L^-¹.s^-¹.

E) 11.7 mol.L^-¹.s^-¹.

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Chapter 8: The Main-Group Elements

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Sample Questions

Q1) The lattice enthalpies of ionic compounds of fluoride tend to be very high because

A) fluorine has a high electronegativity.

B) fluoride ion has an oxidation state of -1.

C) fluorine gas is very reactive.

D) the fluoride ion is small.

E) fluorine is a strong oxidant.

Q2) Phosphorous and phosphoric acids have

A) 1 and 0 hydrogens bonded to the phosphorus atom, respectively.

B) 1 hydrogen bonded to the phosphorus atom.

C) 3 hydrogens bonded to oxygen atoms.

D) 2 and 0 hydrogens bonded to the phosphorus atom.

E) 2 hydrogens bonded to the phosphorus atom.

Q3) Hydrazine is produced by the reaction of

A) nitric acid with hydrogen.

B) nitrogen dioxide with water.

C) nitrogen with water vapor at high pressure.

D) ammonia with alkaline hypochlorite solution.

E) ammonia with hydrogen.

Q4) Write an equation for the second ionization energy of magnesium.

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Chapter 9: The D-Block Elements

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Sample Questions

Q1) Which of the following is the formula of potassium hexacyanoferrate(II)?

A) [Fe(CN)₆]

B) K[Fe(CN)₆]

C) K₂[Fe(CN)₆]

D) K₃[Fe(CN)₆]

E) K₄[Fe(CN)₆]

Q2) A ligand is

A) a Lewis base.

B) necessary in a complex to balance the charge on the metal ion.

C) used to force octahedral geometry on a metal ion.

D) a Lewis acid.

E) used to precipitate metal ions from aqueous solution.

Q3) How many unpaired electrons are predicted for a tetrahedral iron (II) complex?

A) 5 or 1, depending on the ligands.

B) 0 or 4, depending on the ligands.

C) 1

D) 4

E) 5

Q4) Which complex,[CoBr₄]²1^- or [Co(NH₃)₅]³⁺,is the more highly colored?

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Chapter 10: Nuclear Chemistry

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Sample Questions

Q1) Cobalt-60, used in the radiation treatment of cancer,Is produced by absorption of 2 neutrons and emission of a \(\beta\)particle.What is the starting nuclide?

A) ⁵⁸Mn

B) ⁵⁸Ni

C) ⁵⁸Fe

D) ⁵⁹Co

E) ⁵⁹Fe

Q2) The half-life of plutonium-239 is 24 100 years .Calculate the percent of a plutonium sample left after 100 years.

A) 99.7%

B) 4.15%

C) 90.0%

D) 50.0%

E) 96.4%

Q3) A sample of carbon from the Lascaux cave in France contained 12% of the original fraction carbon-14.Estimate the age of this sample (the half-life of carbon-14 is 5.73 * 10³ year).

Q4) What is the product of the emission of a \(\beta\) particle from K-40?

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

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Chapter 11: Organic Chemistry

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Sample Questions

Q1) Which of the following is most volatile?

A) (CH₃)₂C(OH)CH₃

B) (CH₃)₃COH

C) CH₃CH(OH)CH₂CH₃

D) CH₃(CH₂)₃OH

E) CH₃CH₂CH₂CH₃

Q2) When aldehydes react with Tollens reagent,

A) a red precipitate forms.

B) a ketone is produced.

C) silver ions are produced.

D) an alcohol is produced.

E) a carboxylic acid is produced.

Q3) By what type of mechanism do alkanes undergo substitution reactions?

Q4) Which of the following has the highest boiling point?

A) C₃H₈

B) CH₃(CH₂)₇CH₃

C) CH₃(CH₂)₃CH₃

D) CH₃(CH₂)₄CH₃

E) CH₃(CH₂)₅CH₃

Q5) Acetic acetyl chloride reacts with methylamine to produce

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