Introduction to Chemistry Practice Questions
Course Introduction
Introduction to Chemistry provides a foundational understanding of the principles and concepts that govern the composition, structure, properties, and changes of matter. Through a combination of theoretical concepts and practical laboratory experiences, students explore topics such as atomic structure, chemical bonding, the periodic table, chemical reactions, stoichiometry, states of matter, and basic thermochemistry. This course emphasizes problem-solving, scientific reasoning, and the development of laboratory skills, preparing students for further studies in the chemical sciences and related fields.
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Chemical Principles The Quest for Insight 7th Edition by Peter Atkins
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Page 2
Chapter 1: Atoms
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Sample Questions
Q1) What is the l corresponding to the outermost p electrons in sulfur?
A) l = 0
B) l = 1
C) l = 2
D) l = 3
E) l = 4
Answer: B
Q2) Which of the following would be most reactive with air and water?
A) Ba
B) Mg
C) Ga
D) Br
Answer: A
Q3) All the following are transition metals except:
A) Cd.
B) Cu.
C) Pd.
D) Pb.
E) Ag.
Answer: D
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Chapter 2: Molecules
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Sample Questions
Q1) For HF, the LCAO-MO, \(\Psi \)=c<sub>H</sub>\(\Psi \)<sub>H</sub> +c<sub>F</sub>\(\Psi \)<sub>F</sub>,has c<sub>H</sub> = c<sub>F</sub>.
A)True
B)False
Answer: False
Q2) Which of the following has bond angles slightly less than 109<sup>\(\circ\)</sup>?
A) CS<sub>3</sub><sup>2</sup><sup>-</sup>
B) AsF<sub>3 </sub>
C) SO<sub>2 </sub>
D) COCl<sub>2 </sub>
E) COS
Answer: B
Q3) All the following have an angular shape except A) HOCl.
B) S<sub>3</sub><sup>2-</sup>.
C) I<sub>3</sub><sup>-</sup>.
D) ClO<sub>2</sub><sup>-</sup>.
E) NH<sub>2</sub><sup>-</sup>.
Answer: C
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Page 4
Chapter 3: States of Matter
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Sample Questions
Q1) How do alloys solidify and melt?
A) At precise temperatures.
B) Over a range of temperatures.
C) At high temperatures.
D) At very low temperatures.<sup> </sup>
E) At absolute temperatures.
Answer: B
Q2) The ability of water to "wet" paper is due to hydrogen bonding between water molecules and surface molecules in the paper.
A)True
B)False
Answer: True
Q3) How is pig iron produced?
A) In a charcoal fire.
B) Through multiple heatings.
C) In a blast furnace.
D) Through molten mixing with other metals.
E) It is naturally occuring.
Answer: C
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Page 5
Chapter 4: Thermodynamics
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Sample Questions
Q1) For the reaction
2SO<sub>3</sub>(g)\(\rightarrow\)2SO<sub>2</sub>(g)+ O<sub>2</sub>(g) \(\Delta\)H<sub>r</sub>° = +198 kJ.mol<sup>-</sup><sup>1</sup> and \(\Delta\)S<sub>r</sub>° = 190 J.K<sup>-</sup><sup>1</sup>.mol<sup>-</sup><sup>1</sup> at 298 K.
The equilibrium constant for this reaction will be greater than 1 at A) all temperatures.
B) temperatures above 1315 K.
C) temperatures below 1042 K.
D) no temperature.
E) temperatures above 1042 K.
Q2) Which of the following would probably have a positive \(\Delta\)S value?
A) He(g, 2 atm) \(\rarr\) He(g, 10 atm)
B) H<sub>2</sub>(g) + I<sub>2</sub>(s) \(\rarr\) 2HI(g)
C) 2Ag(s) + Br<sub>2</sub>(l) \(\rarr\) 2AgBr(s)
D) O<sub>2</sub>(g) \(\rarr\) O<sub>2</sub>(aq)
E) 2NO<sub>2</sub>(g) \(\rarr\) N<sub>2</sub>O<sub>4</sub>(g)
Q3) What equation corresponds to the standard enthalpy of formation of gaseous hydrogen atoms,which,at 298 K is +217 kJ.mol<sup>-</sup><sup>1 </sup>?
Q4) Work is reported in joules; and 1 joule = ____________
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Chapter 5: Equilibrium
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Sample Questions
Q1) Which of the following 1.0 M solutions contains the most particles?
A) Ethylene glycol
B) Potassium chloride
C) Magnesium sulfate
D) Glucose
E) Sodium sulfate
Q2) Calculate the vapor pressure at25<sup>\(\omicron\)</sup>C of a mixture of benzene and toluene in which the mole fraction of benzene is 0.650 .The vapor pressure at 25<sup>\(\omicron\)</sup>C of benzene is 94.6 Torr and that of toluene is 29.1 Torr.
A) 84.4 Torr
B) 124 Torr
C) 51.3 Torr
D) 71.7 Torr
E) 61.5 Torr
Q3) If a reaction mixture that is not at equilibrium contains more products than reactants,\(\Delta\)G > 0 for the forward reaction
A)True
B)False
Q4) 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) What is the pH of an aqueous solution that is 0.011 M HF (K<sub>a</sub> = 3.5 * 10<sup>-</sup><sup>4</sup>) and 0.015 M NaF?
A) 1.95
B) 3.46
C) 3.59
D) 5.27
E) 3.33
Q2) Calculate the solubility product of calcium hydroxide given that the solubility of Ca(OH)<sub>2</sub>(s) in water at 25S1U1P1\(\circ\)S1S1P0C is 0.011 M.
A) 1.5 * 10<sup>-</sup><sup>8 </sup>
B) 1.1 * 10<sup>-</sup><sup>5 </sup>
C) 2.7 * 10<sup>-</sup><sup>6 </sup>
D) 5.3 * 10<sup>-</sup><sup>6 </sup>
E) 1.2 * 10<sup>-</sup><sup>4 </sup>
Q3) True or false: the pH of 0.10 M and 0.40 M NaHCO<sub>3</sub>(aq) solutions is 8.31 for both?
A)True
B)False
Q4) What is the conjugate acid of O<sup>2</sup><sup>-</sup>?
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Chapter 7: Kinetics
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Sample Questions
Q1) The activation energy of a reaction is given by
A) +(slope of a plot of lnk vs 1/T) / R.
B) -(slope of a plot of lnk vs 1/T) / R.
C) -R / (slope of a plot of lnk vs 1/T).
D) +(slope of a plot of lnk vs 1/T) * R.
E) -(slope of a plot of lnk vs 1/T) * R.
Q2) Consider the reaction for the dimerization of butadiene(g)at a certain temperature. 2C<sub>4</sub>H<sub>6</sub>(g)\(\rightarrow\) C<sub>8</sub>H<sub>12</sub>(g) rate = k[C<sub>4</sub>H<sub>6</sub>]<sup>2</sup>.When the initial concentration of butadiene is 0.500 M, the time required for 80% dimerization is measured at 11.4 s.What is the rate constant for the dimerization?
Q3) A catalyst facilitates a reaction by
A) increasing the activation energy for the reverse reaction.
B) lowering the activation energy of the reaction.
C) shifting the position of the equilibrium of the reaction.
D) decreasing the temperature at which the reaction will proceed spontaneously.
E) making the reaction more exothermic.
Q4) What is the half-life of a second order reaction?
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Chapter 8: The Main-Group Elements
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Sample Questions
Q1) Which of the following are good reducing agents?
HNO<sub>3</sub>,PH<sub>3</sub>,HNO<sub>2</sub>,NCl<sub>3</sub>,NH<sub>3</sub>, NO
A) HNO<sub>3</sub> and NO
B) HNO<sub>2</sub> and HNO<sub>3</sub>
C) NCl<sub>3</sub> and NH<sub>3</sub>
D) NH<sub>3</sub> and PH<sub>3</sub>
E) NH<sub>3</sub> only
Q2) Which of the following reacts only as a reducing agent?
A) P<sub>4 </sub>
B) NO<sub>2</sub><sup>-</sup><sup> </sup>
C) F<sub>2 </sub>
D) NH<sub>3</sub><sup> </sup>
E) S<sub>8 </sub>
Q3) All of the following contain silicates in various forms except A) asbestos.
B) mica.
C) talc.
D) molecular sieves.
E) alum.
Q4) Which of the alkaline earth metals does not form a saline hydride?
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Chapter 9: The D-Block Elements
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Sample Questions
Q1) What is the oxidation number of iron in K<sub>3</sub>[Fe(CN)<sub>6</sub>]?
A) +3
B) +2
C) +9
D) +6
Q2) Which of the following complex ions is likely to absorb at 600-700 nm?
A) [Co(OH<sub>2</sub>)<sub>6</sub>]<sup>2+ </sup>
B) [Co(NO<sub>2</sub>)<sub>6</sub>]<sup>4</sup><sup>-</sup>
C) [Co(NH<sub>3</sub>)<sub>6</sub>]<sup>2+ </sup>
D) [Co(CN)<sub>6</sub>]<sup>4</sup><sup>-</sup>
E) [CoCl<sub>4</sub>]<sup>2</sup><sup>-</sup>
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) Zinc is used to galvanize iron.Explain why a galvanized container should not be used to store sodium hydroxide.
Q5) Why is \(\Delta\)<sub>T</sub> is always greater than \(\Delta\)<sub>O</sub>?
Page 11
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Chapter 10: Nuclear Chemistry
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Sample Questions
Q1) Which of the following is likely to lie below the band of stability?
A) O-15
B) P-29
C) Li-9
D) Be-7
E) C-14
Q2) What nuclide is formed when <sup>90</sup>Sr undergoes \(\beta\) decay?
A) <sup>86</sup>Kr
B) <sup>90</sup>Y
C) <sup>94</sup>Zr
D) <sup>89</sup>Sr
E) <sup>90</sup>Rb
Q3) What type of reaction is it when a neutron becomes a proton,and the result is a nucleus that changes from Z to Z+1?
Q4) Nuclides that lie above the band of stability are proton rich.
A)True
B)False
Q5) Complete the nuclear reaction <sup>97</sup>Mo + <sup>2</sup>H \(\rarr\) _____ + 2n
Q6) What is the product of the emission of a \(\beta\) particle from K-40?
Page 12
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Chapter 11: Organic Chemistry
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Sample Questions
Q1) Both C<sub>6</sub>H<sub>5</sub>OH and C<sub>6</sub>H<sub>5</sub>CH<sub>2</sub>OH are weak acids with K<sub>a</sub> values about 10<sup>-10</sup>
A)True
B)False
Q2) Name the compound CH<sub>2</sub>=CHC(CH<sub>3</sub>)CH(CH<sub>3</sub>)<sub>2</sub>.
Q3) Name the compound (CH<sub>3</sub>CH<sub>2</sub>)<sub>2</sub>CHCH=CHCH<sub>3</sub>.
A) Diethylbutene
B) 3-ethyl-4-hexene
C) 4,4-diethyl-2-butene
D) 4-ethyl-2-hexene
E) Ethylhexene
Q4) Identify compounds 1 and 2 in the reaction scheme below. CH<sub>3</sub>CHCH<sub>2</sub> + H<sup>+</sup>/H<sub>2</sub>O \(\rarr\) 1 + K<sub>2</sub>Cr<sub>2</sub>O<sub>7</sub>/H<sup>+</sup> \(\rarr\) 2
Q5) Which atom of formaldehyde, H<sub>2</sub>CO,Is a Lewis acid site?
Q6) Why do alkanes not react with boiling nitric acid?
Q7) When amines condense with carboxylic acids,what molecule is eliminated?
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