Chemical Science Exam
Bank
Course Introduction
Chemical Science is the study of the composition, structure, properties, and changes of matter. This course explores fundamental concepts such as atomic structure, chemical bonding, stoichiometry, thermodynamics, kinetics, and equilibrium. Students learn about the periodic table, acids and bases, and the principles underlying organic and inorganic compounds. Practical laboratory work is integrated to reinforce theoretical knowledge and develop essential skills in observation, experimentation, and data analysis, preparing students for advanced study or careers in chemistry-related fields.
Recommended Textbook Chemistry 7th Edition by John E. McMurry
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23 Chapters
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Page 2
Chapter 1: Chemical Tools: Experimentation and Measurement
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Sample Questions
Q1) If 1.4% of the mass of a human body is calcium,how many kilograms of calcium are there in a 173-pound man?
A)1.1 kg Ca
B)5.3 kg Ca
C)1.1 × 10<sup>2</sup> kg Ca
D)5.3 × 10<sup>2</sup> kg Ca
Answer: A
Q2) The average distance between nitrogen and oxygen atoms is 115 pm in a compound called nitric oxide.What is this distance in nanometers?
A)1.15 × 10<sup>-2 </sup>nm
B)1.15 × 10<sup>-1 </sup>nm
C)1.15 × 10<sup>15 </sup>nm
D)1.15 × 10<sup>19</sup> nm
Answer: B
Q3) The number of significant digits in 0.01810 g is ________.
Answer: four
Q4) The difference between the boiling point and freezing point of water is 100°C,which is ________ kelvins.
Answer: 100
Page 3
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Chapter 2: Atoms, molecules, and Ions
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Sample Questions
Q1) In which pair are both formulas of binary fluorides of element D correct?
A)DF<sub>2</sub> and DF<sub>3</sub>
B)DF<sub>2</sub> and DF<sub>6</sub>
C)DF<sub>3</sub> and DF<sub>5</sub>
D)DF<sub>5</sub> and DF<sub>6</sub>
Answer: B
Q2) The chemical formula for the carbonate ion is
A)C<sup>-</sup>.
B)CO<sup>-</sup>.
C)CO<sub>3</sub><sup>2-</sup>.
D)CO<sub>2</sub><sup>2-</sup>.
Answer: C
Q3) What type of bonding is found in the compound NH<sub>3</sub>?
A)covalent bonding
B)hydrogen bonding
C)ionic bonding
D)metallic bonding
Answer: A
Q4) The symbol for mercury is ________.
Answer: Hg
Page 4
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Chapter 3: Mass Relationships in Chemical Reactions
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Sample Questions
Q1) The balanced equation for the gaseous state oxidation of ammonia is shown below. 4 NH<sub>3</sub> + 5 O<sub>2</sub> 4 NO + 6 H<sub>2</sub>O
How many moles of O<sub>2</sub> are required to react with 1.2 mole of NH<sub>3</sub>?
Answer: 1.5 mol
Q2) How many anions are in 10.0 g of sodium phosphate?
A)3.67 × 10<sup>22</sup> cations
B)1.10 × 10<sup>23</sup> cations
C)9.87 × 10<sup>24</sup> cations
D)2.96 × 10<sup>25</sup> cations
Answer: A
Q3) 9.0 g of iron is reacted with 9.0 g of water according to the chemical equation shown below.Which one of the following statements is false? 3 Fe(s)+ 4 H<sub>2</sub>O(l) Fe<sub>3</sub>O<sub>4</sub>(s)+ 4 H<sub>2</sub>(g)
A)12.4 g of Fe<sub>3</sub>O<sub>4</sub> are produced.
B)5.13 g of H<sub>2</sub>O are left over.
C)Mass is conserved in this reaction.
D)Water is the limiting reactant.
Answer: D
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Page 5
Chapter 4: Reactions in Aqueous Solutions
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Sample Questions
Q1) How many milliliters of a 9.0 M H<sub>2</sub>SO<sub>4</sub> solution are needed to make 0.45 L of a 3.5 M solution?
A)0.18 mL
B)1.2 mL
C)180 mL
D)1200 mL
Q2) If the volumes in the buret and the flask are identical and the concentration of the acid in the buret is 0.250 M,what is the concentration of the base in the flask?
A)0.167 M
B)0.250 M
C)0.375 M
D)0.667 M
Q3) The reaction C<sub>6</sub>H<sub>12</sub>O<sub>6</sub>(s)+ 6 O<sub>2</sub>(g) 6 CO<sub>2</sub>(g)+ 6 H<sub>2</sub>O(l)is best classified as a(n)
A)acid-base neutralization reaction.
B)double replacement reaction.
C)oxidation-reduction reaction.
D)precipitation reaction.
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6
Chapter 5: Periodicity and the Electronic Structure of Atoms
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Sample Questions
Q1) Which one of these spheres represents an atom of Li?
A)sphere (a)
B)sphere (b)
C)sphere (c)
D)sphere (d)
Q2) An element in a ground state electron configuration has 4 electrons in the 4p orbitals.Which of the following statements can not describe the electron configurations in this atom?
A)At least one electron has an orbital angular momentum (l)of 2.
B)Six electrons are in the n=4 shell.
C)The valence electron configuration is identical to carbon.
D)No electrons have an orbital angular momentum (l)of 3.3.
Q3) Which of the following elements will have unpaired electrons in the ground state?
Ca,Li,C,F
A)Ca,Li,C,and F
B)Li,C,and F
C)Li and F
D)C and F
Q4) The highest note on a piano has a frequency of 4186 Hz.In a vacuum 4186 Hz has a corresponding wavelength of ________ m.
Page 7
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Chapter 6: Ionic Compounds: Periodic Trends and Bonding
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Sample Questions
Q1) Which of the following ionic compounds would be expected to have the highest lattice energy?
A)Li<sub> </sub>F
B)Na<sub> </sub>F
C)K<sub> </sub>F
D)Rb<sub> </sub>F
Q2) Which element has the most favorable (most negative)electron affinity?
A)K
B)Be
C)I
D)Ne
Q3) The group 4A element that always obeys the octet rule in its stable compounds is ________.
Q4) Which chemical process is associated with the lattice energy for sodium chloride?
A)NaCl(s) Na<sup>+</sup>(g)+ Cl<sup>-</sup>(g)
B)NaCl(g) Na<sup>+</sup>(g)+ Cl<sup>-</sup>(g)
C)Na(s)+ 1/2 Cl<sub>2</sub>(g) NaCl(s)
D)NaCl(s)+ H<sub>2</sub>O(l) Na<sup>+</sup>(aq)+ Cl<sup>-</sup>(aq)
Q5) The ion that has 28 protons and 26 electrons is ________.
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Chapter 7: Covalent Bonding and Electron-Dot Structures
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Sample Questions
Q1) Which molecule has the weakest bonds?
A)CF<sub>4</sub>
B)CCl<sub>4</sub>
C)CBr<sub>4</sub>
D)CI<sub>4</sub>
Q2) Of the bonds C-C,C-N,C-O,and C-F,the bond that is most polar is ________.
Q3) The electronegativity for both sulfur and carbon is 2.5.Therefore the compound
CS<sub>2</sub> would be expected to
A)be ionic with C as the anion.
B)be ionic with C as the cation.
C)have nonpolar covalent bonds between C and S.
D)have polar covalent bonds between C and S.
Q4) When melting S<sub>8</sub>,________ forces must be overcome and S<sub>8</sub> is expected to have a ________ melting point than MgS.
A)covalent bonding,higher
B)covalent bonding,lower
C)intermolecular,higher
D)intermolecular,lower
Q5) Which compound is most likely to exist as a gas at room temperature?
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Chapter 8: Covalent Compounds: Bonding Theories and Molecular Structure
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Sample Questions
Q1) What is the molecular geometry of ICl<sub>4</sub><sup>-</sup>?
A)seesaw
B)square planar
C)square pyramidal
D)tetrahedral
Q2) What is the hybridization of the carbon atom labeled C<sub>2</sub>?
A)sp
B)sp<sup>2</sup>
C)sp<sup>3</sup>
D)sp<sup>4</sup>
Q3) The hybrid orbital used by carbon to overlap with hydrogen in C<sub>2</sub>H<sub>2</sub> is ________.
Q4) What is the molecular geometry of SeF<sub>5</sub><sup>-</sup>?
A)octahedral
B)seesaw
C)square pyramidal
D)trigonal bipyramidal
Q5) The carbon-carbon bond in C<sub>2</sub>H<sub>2</sub> contains ________ and ________ bonds.
Page 10
Q6) The polarity of CCl<sub>4</sub> is ________.
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Chapter 9: Thermochemistry: Chemical Energy
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Sample Questions
Q1) Find E° for the reaction below if the process is carried out at a constant pressure of 1.00 atm and V (the volume change)= -24.5 L.(1 L atm = 101 J) 2 CO(g)+ O<sub>2</sub> (g) 2 CO<sub>2</sub>(g) H° = -566.kJ
A)+2.47 kJ
B)-2.47 kJ
C)-564 kJ
D)-568 kJ
Q2) Is thermal energy a form of kinetic or potential molecular energy?
Q3) Which is expected to have the lowest specific heat capacity at 25°C?
A)air
B)gold
C)ethylene glycol
D)methanol
Q4) For a system at constant pressure,19,400 calories of heat are released.This quantity of heat is equivalent to
A)6.92 × 10<sup>-5</sup> J.
B)8.12 × 10<sup>3</sup> J.
C)1.94 × 10<sup>4</sup> J.
D)8.12 × 10<sup>4</sup> J.
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Chapter 10: Gases: Their Properties and Behavior
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Sample Questions
Q1) Which one of the following is not used to describe the condition of a gas?
A)number of moles
B)electronic configuration
C)temperature
D)pressure
Q2) Which of the following instruments directly measures the pressure of a gas?
A)spectrometer
B)manometer
C)polarimeter
D)gas chromatograph
Q3) If CO<sub>2</sub> and NH<sub>3</sub> are allowed to effuse through a porous membrane under identical conditions,the rate of effusion for NH<sub>3</sub> will be ________ times that of CO<sub>2</sub>.
A)0.39
B)0.62
C)1.6
D)2.6
Q4) Gases do not behave ideally under conditions of ________ pressure and ________ temperature.
Q5) When using the ideal gas law the temperature must be expressed in ________.
Page 13
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Chapter 11: Liquids, solids, and Phase Changes
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Sample Questions
Q1) Which of the areas designated A,B,and C are smallest repeating units,analogous to two-dimensional unit cells?
A)only A
B)only B
C)only C
D)A,B,or C
Q2) How many cations and how many anions are in the unit cell?
A)4 cations and 4 anions
B)4 cations and 8 anions
C)4 cations and 14 anions
D)8 cations and 4 anions
Q3) Aluminum has a face-centered cubic structure and has a density of 2.70 g/cm<sup>3</sup>.What is its atomic radius?
A)143 pm
B)286 pm
C)405 pm
D)1150 pm
Q4) A compound having A ions on each corner and B ions on each face of a cubic unit cell has the empirical formula ________.
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Chapter 12: Solutions and Their Properties
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Sample Questions
Q1) The coolant in automobiles is often a 50/50 % by volume mixture of ethylene glycol,HOCH<sub>2</sub>CH<sub>2</sub>OH,and water.At 20°C,the density of ethylene glycol is 1.1088 g/mL and the density of water is 0.9982 g/mL.Assuming that the volumes are additive,what is the expected freezing point of a 50/50(v/v)% ethylene glycol/water solution? K<sub>f</sub> = 1.86°C/m for water.
A)-16°C
B)-17°C
C)-30°C
D)-33°C
Q2) Assume that you start with a mixture containing 0.80 mol of decane and 0.20 mol of octane,what is the vapor composition at the boiling point?
A)100% decane
B)composition at point b
C)composition at point c
D)composition at point e
Q3) Amphetamines in urine can be confirmed by mass spectroscopy at a concentration of 500 ng/mL.Assuming a urine density of 1.025 g/mL,what is this concentration in parts per million?
Q4) Molarity is defined as ________,whereas molality is defined as ________.
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Chapter 13: Chemical Kinetics
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Sample Questions
Q1) What is the species present at reaction stage 1?
A)an intermediate
B)a product
C)a reactant
D)a transition state
Q2) What is the time required to achieve the molecular mixture in drawing (d)?
A)4 min
B)5 min
C)7 min
D)8 min
Q3) The Haber process is the synthesis of ammonia gas from hydrogen and nitrogen on a hot metal surface.What is the catalyst and what type of catalysis is occurring?
A)H<sub>2</sub>,heterogeneous
B)N<sub>2</sub>,heterogeneous
C)NH<sub>3</sub>,heterogeneous
D)metal surface,heterogeneous
Q4) Platinum in the catalytic converter of an automobile catalyzes the conversion of CO to CO<sub>2</sub> is an example of a ________ (heterogeneous,homogeneous)catalyst.
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Chapter 14: Chemical Equilibrium
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Sample Questions
Q1) If additional SCN<sup>-</sup> is added to the equilibrium system shown below,Le Châtelier's principle predicts a net reaction from ________ to ________,causing the red color to become ________. Fe<sup>3+</sup>(aq)+ SCN<sup>-</sup>(aq) FeSCN<sup>2+</sup>(aq) yellow colorless red
Q2) The decomposition of nitrosyl bromide is exothermic: 2 NOBr(g) 2 NO(g)+ Br<sub>2</sub>(g).Which of the following changes in reaction condition will shift the reaction to the left?
A)remove NO<sub> </sub>
B)decrease the temperature
C)decrease the pressure
D)None of these
Q3) For the reaction H<sub>2</sub>(g)+ S(s) H<sub>2</sub>S(g),if the rate constant for the forward reaction is greater than the rate constant for the reverse reaction,the value of K<sub>c</sub> must be ________ (equal to,greater than,less than)1.
Q4) At 298 K,K<sub>p</sub> = 2.1 × 10<sup>4</sup> for the reaction CO(g)+ 2 H<sub>2</sub>(g) CH<sub>3</sub>OH(g).What is the value of K<sub>c</sub> at this temperature?
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Page 17
Chapter 15: Aqueous Equilibria: Acids and Bases
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Sample Questions
Q1) Which Br nsted-Lowry acid is not considered to be a strong acid in water?
A)HCl
B)HI<sub> </sub>
C)H<sub> </sub>ClO<sub>3</sub>
D)H<sub>2</sub>SO<sub>4</sub>
Q2) Ammonia NH<sub>3</sub>,has a base dissociation constant of 1.8 × 10<sup>-5</sup>.What is the conjugate acid of ammonia and what is its acid dissociation constant?
A)NH<sub>4</sub><sup>+</sup>,1.9 × 10<sup>9</sup>
B)NH<sub>4</sub><sup>+</sup>,1.8 × 10<sup>-5</sup>
C)NH<sub>4</sub><sup>+</sup>,5.6 × 10<sup>-10</sup> D)NH<sub>2</sub><sup>-</sup>,5.6 × 10<sup>-10</sup>
Q3) An Arrhenius base is best defined as a A)electron pair donor.
B)hydroxide acceptor.
C)substance that dissociates in water to produce aqueous hydrogen ions.
D)substance that dissociates in water to produce aqueous hydroxide ions.
Q4) A 1.25 × 10<sup>-4</sup> M solution of the anti-inflammatory drug naproxen has a pH = 4.2.The K<sub>a</sub> and pK<sub>a</sub> of naproxen are ________ and
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Chapter 16: Applications of Aqueous Equilibria
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Sample Questions
Q1) What is the approximate value of the equilibrium constant,K<sub>n</sub>,for the neutralization of acetic acid with potassium hydroxide,shown in the equation below? The K<sub>a</sub> for acetic acid is 1.8 × 10<sup>-5</sup>. CH<sub>3</sub>CO<sub>2</sub>H(aq)+ KOH(aq) H<sub>2</sub>O(l)+ NaCH<sub>3</sub>CO<sub>2</sub>(aq)
A)1.8 × 10<sup>-19</sup>
B)5.6 × 10<sup>-10</sup>
C)1.8 × 10<sup>-8</sup>
D)1.8 × 10<sup>9</sup>
Q2) The dissociation equilibrium constants for the protonated form of alanine (a diprotic amino acid H<sub>2</sub>X<sup>+</sup>)are K<sub>a1</sub> = 4.6 × 10<sup>-3</sup> and K<sub>a2</sub> = 2.0 × 10<sup>-10</sup>.What is the pH of 50.00 mL of a 0.100 M solution of alanine after 100.00 mL of 0.100 M NaOH has been added?
A)9.70
B)10.69
C)11.11
D)12.70
Q3) What is the K<sub>a</sub> of the amino acid glutamine if it is 33.0% dissociated at pH = 8.82?
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Page 19
Chapter 17: Thermodynamics: Entropy, free Energy, and Equilibrium
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Sample Questions
Q1) Standard molar entropies,S°,in J/Kmol,are given below each reactant and product in the reaction shown below.The standard entropy of reaction, S°,for this reaction is ________ J/K.
2 SO<sub>2</sub>(g)+ O<sub>2</sub>(g) 2 SO<sub>3</sub>(g)
248.1 205.0 256.6
Q2) What is K if G° = -19.0 kJ for a reaction at 25°?
A)2.10 × 10<sup>3</sup>
B)2.80 × 10<sup>2</sup>
C)1.80 × 10<sup>-3</sup>
D)5.30 × 10<sup>-4</sup>
Q3) At 25°C, G°<sub>f </sub>is -620 kJ/mol for SiCl<sub>4</sub>(g)and -592 kJ/mol for MgCl<sub>2</sub>(s).Calculate G° for the reaction,SiCl<sub>4</sub>(g)+ 2 Mg(s) 2 MgCl<sub>2</sub>(s)+ Si(s)and determine if the reaction is spontaneous at 25°C if the pressure of SiCl<sub>4</sub>(g)is 1 atm.
A) G° = 28 kJ;the process is spontaneous.
B) G° = 28 kJ;the process is nonspontaneous.
C) G° = -564 kJ;the process is spontaneous.
D) G° = -564 kJ;the process is nonspontaneous.
Q4) What is the entropy of 12 molecules in a system of 100 boxes?
Page 20
Q5) What is the entropy of 50 molecules in a system of 1000 boxes?
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Chapter 18: Electrochemistry
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Q1) According to Table 17.1,which will reduce water but not Mg<sup>2+</sup>?
A)Al<sup>3+</sup>(aq)
B)Al(s)
C)Na<sup>+</sup>(aq)
D)Na(s)
Q2) If the cell reaction involves ions in solution,as the cell reaction in a galvanic cell continues,
A)E for the cell increases.
B)E for the cell decreases.
C)E° for the cell increases.
D)E° for the cell decreases.
Q3) In the shorthand notation for a galvanic cell,a double vertical line ( )represents A)a single phase boundary
B)a cathode
C)a gas
D)a salt bridge
Q4) The standard cell potential for the following galvanic cell is 0.71 V. Pb(s)|Pb<sup>2+</sup>(aq)||Al<sup>3+</sup>(aq)|Al
This reaction has an equilibrium constant,K = ________.
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Chapter 19: Nuclear Chemistry
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Sample Questions
Q1) What percentage of a radioactive substance remains after 6.00 half-lives have elapsed?
A)0.781%
B)1.56%
C)3.12%
D)6.25%
Q2) In fusion reactions to make superheavy elements,energy is required to bring the two nuclei together and to form additional mass.How much energy must be converted into mass for the alpha bombardment of <sup>253</sup>Es to form <sup>257</sup>Md?
(The isotopic masses are <sup>253</sup>Es = 253.08294 amu,<sup>4</sup>He = 4.00260 amu,<sup>257</sup>Md = 257.09558 amu. )
A)3.01 × 10<sup>6</sup> kJ/mol
B)9.04 × 10<sup>8</sup> kJ/mol
C)3.59 × 10<sup>11</sup> kJ/mol
D)7.21 × 10<sup>11</sup> kJ/mol
Q3) What type of shielding can be used to protect against gamma rays?
A)paper
B)lead
C)heavy clothing
D)No shielding is effective against gamma rays.
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Chapter 20: Transition Elements and Coordination Chemistry
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Sample Questions
Q1) Which of the following chromium species is the strongest acid?
A)Cr(OH)<sub>2</sub>
B)Cr(OH)<sub>3</sub>
C)CrO<sub>2</sub>(OH)<sub>2</sub>
D)CrO<sub>4</sub><sup>2-</sup>
Q2) Which of the following elements is an inner transition metal?
A)Pm
B)Ni
C)Zr
D)Lu
Q3) Which of the above are ligands that contain two or more donor atoms?
A)All contain two or more donor atoms.
B)(a)and (b)
C)(c)and (d)
D)None contain two or more donor atoms.
Q4) What are two of the major components of stainless steel?
A)iron and carbon
B)iron and chromium
C)iron and titanium
D)iron and tungsten
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Chapter 21: Metals and Solid-State Materials
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Q1) Which picture represents an n-type Si semiconductor?
A)picture (A)
B)picture (B)
C)both picture (A)and picture (B)
D)neither picture (A)nor picture (B)
Q2) The chemical process of roasting is commonly used to facilitate the reduction of which metal ores?
A)Ag,Cu,and Hg
B)Ag,Mg,and Na
C)Hg and Pt
D)Ag,Mn,and V
Q3) Which has been found to be a three dimensional superconductor that conducts equally in all directions?
A)C (diamond)
B)C (graphite)
C)K<sub>3</sub>C<sub>60</sub>
D)YBa<sub>2</sub>Cu<sub>3</sub>O<sub>7</sub>
Q4) The number of electrons that half fill a composite s-d band is ________.
Q5) The principal source of chromium is chromite.What is the formula of chromite?
Page 24
Q6) What is the oxidation number of mercury in cinnabar?
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Chapter 22: The Main-Group Elements
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Q1) Using principles discussed in chapters 15 and 19,determine which of the following is the strongest acid.
A)HClO
B)HClO<sub>2</sub>
C)HClO<sub>3</sub>
D)HClO<sub>4</sub>
Q2) Which hydride reacts with water at 25°C to give H<sub>2</sub> gas and forms a basic solution?
A)hydride (1)
B)hydride (2)
C)hydride (3)
D)hydride (4)
Q3) Which of the following statements about helium is inconsistent with its chemistry?
A)A helium oxygen mixture is used as a deep-sea diving gas instead of compressed air.
B)In its liquid form it is used as a cryogenic coolant for superconductors.
C)It is one of the more reactive elements of its group.
D)Its melting point is -272.2°C and its boiling point is -268.9°C.
Q4) The oxidation number of the oxygen atoms in CaO<sub>2</sub> is ________.
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Chapter 23: Connections to Organic and Biological Chemistry
Available Study Resources on Quizplus for this Chatper
290 Verified Questions
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Sample Questions
Q1) Which of the following is not part of a nucleotide?
A)cyclic amine base
B)fatty acid
C)phosphoric acid
D)a sugar
Q2) Sucrose,common table sugar,when hydrolyzed will form
A)amylose and glycogen.
B)cellulose and starch.
C)glucose and fructose.
D)lactose and maltose.
Q3) What type of hybridization does a carbon atom have in a six-membered aromatic ring?
A)sp
B)sp<sup>2</sup>
C)sp<sup>3</sup>
D)sp<sup>3</sup><sup>d</sup>
Q4) The IUPAC name for the alkane shown below is ________. CH<sub>3</sub>
| CH<sub>3</sub>CHCH<sub>2</sub>CH<sub>2</sub>CH<sub>2</sub>CH<sub>3</sub>
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