Fundamentals of Chemistry
Question Bank
Course Introduction
Fundamentals of Chemistry introduces students to the foundational concepts of chemical science, including the structure of matter, atomic and molecular theory, chemical bonding, stoichiometry, states of matter, and the basics of chemical reactions. The course emphasizes the principles that govern chemical behavior, such as thermodynamics, kinetics, and equilibrium, while also exploring the practical applications of chemistry in everyday life and industry. Through lectures, laboratory experiments, and problem-solving exercises, students develop a solid understanding of essential chemical principles and gain the skills necessary for further study in chemistry and related scientific fields.
Recommended Textbook Principles of General Chemistry 2nd Edition by Martin Silberberg
Available Study Resources on Quizplus
23 Chapters
1830 Verified Questions
1830 Flashcards
Source URL: https://quizplus.com/study-set/3726 Page 2
Chapter 1: Keys to the Study of Chemistry
Available Study Resources on Quizplus for this Chatper
66 Verified Questions
66 Flashcards
Source URL: https://quizplus.com/quiz/74295
Sample Questions
Q1) The average distance between the Earth and the Moon is 240,000 miles.Express this distance in kilometers.
A)6.1 \(\times\) 10<sup>5</sup> km
B)5.3 \(\times\) 10<sup>5</sup> km
C)3.9 \(\times\) l0<sup>5</sup> km
D)1.5 \(\times\) 10<sup>5</sup> km
E)9.4 \(\times\) 10<sup>4</sup> km
Answer: C
Q2) In an average year the American chemical industry produces more than 9.5 million metric tons of sodium carbonate.Over half of this is used in the manufacture of glass while another third is used in the production of detergents and other chemicals.How many pounds of sodium carbonate are produced annually?
A)2.1 \(\times\) 10<sup>10</sup> lb
B)4.3 \(\times\) 10<sup>9</sup> lb
C)1.1 \(\times\) 10<sup>7</sup> lb
D)2.2 \(\times\) 10<sup>6</sup> lb
E)2.1 \(\times\) 10<sup>4</sup> lb
Answer: A
To view all questions and flashcards with answers, click on the resource link above. Page 3
Chapter 2: The Components of Matter
Available Study Resources on Quizplus for this Chatper
91 Verified Questions
91 Flashcards
Source URL: https://quizplus.com/quiz/74296
Sample Questions
Q1) The colorless substance,MgF<sub>2</sub>,is used in the ceramics and glass industry.What is its name?
A)magnesium difluoride
B)magnesium fluoride
C)magnesium(II)fluoride
D)monomagnesium difluoride
E)none of these choices is correct,since they are all misspelled
Answer: B
Q2) Zinc acetate is used in preserving wood and in manufacturing glazes for porcelain.What is its formula?
A)ZnAc<sub>2</sub>
B)ZnCH<sub>3</sub>COO
C)Zn(CH<sub>3</sub>COO)<sub>2</sub>
D)Zn<sub>2</sub>CH<sub>3</sub>COO
E)ZnCH<sub>3</sub>COCH<sub>3 </sub>
Answer: C
Q3) In nature,some elements exist as molecules,while others do not.
A)True
B)False
Answer: True
To view all questions and flashcards with answers, click on the resource link above. Page 4
Chapter 3: Stoichiometry of Formulas and Equations
Available Study Resources on Quizplus for this Chatper
90 Verified Questions
90 Flashcards
Source URL: https://quizplus.com/quiz/74297
Sample Questions
Q1) Gadolinium oxide,a colorless powder which absorbs carbon dioxide from the air,contains 86.76 mass % Gd.Determine its empirical formula.
A)Gd<sub>2</sub>O<sub>3</sub>
B)Gd<sub>3</sub>O<sub>2</sub>
C)Gd<sub>3</sub>O<sub>4</sub>
D)Gd<sub>4</sub>O<sub>3</sub> E)GdO
Answer: A
Q2) One mole of O<sub>2</sub> has a mass of 16.0 g.
A)True
B)False
Answer: False
Q3) A solution of methanol (CH<sub>4</sub>O)in water has a concentration of 0.200
M.What mass of methanol,in grams,is present in 0.150 liters of this solution?
Answer: 0.961 g
Q4) Analysis of a white solid produced in a reaction between chlorine and phosphorus showed that it contained 77.44% chlorine and 22.56% phosphorus.What is its empirical formula?
Answer: PCl<sub>3</sub>
To view all questions and flashcards with answers, click on the resource link above. Page 5
Chapter 4: Three Major Classes of Chemical Reactions
Available Study Resources on Quizplus for this Chatper
84 Verified Questions
84 Flashcards
Source URL: https://quizplus.com/quiz/74298
Sample Questions
Q1) A combination reaction may also be a displacement reaction.
A)True
B)False
Q2) Select the classification for the following reaction.
2Ag<sup>+</sup>(aq)+ Zn(s) \(\to\) 2Ag(s)+ Zn<sup>2+</sup>(aq)
A)displacement
B)decomposition
C)combination
D)precipitation
E)acid-base
Q3) Select the classification for the following reaction. 2I<sup>-</sup>(aq)+ Cl<sub>2</sub>(aq) \(\to\) I<sub>2</sub>(aq)+ 2Cl<sup>-</sup>(aq)
A)combination
B)displacement
C)decomposition
D)precipitation
E)acid-base
Q4) Complete and balance the equation for the following acid-base reaction. Ca(OH)<sub>2</sub>(aq)+ HCl(aq) \(\to\)
Page 6
To view all questions and flashcards with answers, click on the resource link above.
Chapter 5: Gases and the Kinetic-Molecular Theory
Available Study Resources on Quizplus for this Chatper
93 Verified Questions
93 Flashcards
Source URL: https://quizplus.com/quiz/74299
Sample Questions
Q1) A sample of oxygen gas has its absolute temperature halved while the pressure of the gas remained constant.If the initial volume is 400 mL,what is the final volume?
A)20 mL
B)133 mL
C)200 mL
D)400 mL
E)800 mL
Q2) For real gases,PV < nRT,always.
A)True
B)False
Q3) Calculate the pressure of a helium sample at -207.3°C and 768 mL if it exerts a pressure of 175 kPa at 25.0°C and 925 mL.
A)32.1 kPa
B)46.6 kPa
C)657 kPa
D)953 kPa
E)It is not possible,since the pressure would have to be negative.
Q4) Briefly state the conditions corresponding to STP (standard temperature and pressure).
To view all questions and flashcards with answers, click on the resource link above. Page 7
Chapter 6: Thermochemistry: Energy Flow and Chemical Change
Available Study Resources on Quizplus for this Chatper
71 Verified Questions
71 Flashcards
Source URL: https://quizplus.com/quiz/74300
Sample Questions
Q1) A system which undergoes an adiabatic change and does work on the surroundings has
A)w < 0,\(\Delta\)E = 0
B)w > 0,\(\Delta\)E > 0
C)w > 0,\(\Delta\)E < 0
D)w < 0,\(\Delta\)E > 0
E)w < 0,\(\Delta\)E < 0
Q2) Which of the following is not a state function?
A)internal energy
B)volume
C)work
D)pressure
E)enthalpy
Q3) A system delivers 1275 J of heat while the surroundings perform 855 J of work on it.Calculate \(\Delta\)E in J.
A)-2130 J
B)-420 J
C)420 J
D)2130 J
E)-1275 J
To view all questions and flashcards with answers, click on the resource link above. Page 8
Chapter 7: Quantum Theory and Atomic Structure
Available Study Resources on Quizplus for this Chatper
72 Verified Questions
72 Flashcards
Source URL: https://quizplus.com/quiz/74301
Sample Questions
Q1) The AM station KBOR plays your favorite music from the 20s and 30s at 1290 kHz.Find the wavelength of these waves.
A)4.30 \(\times\) 10<sup>-2</sup> m
B)0.144 m
C)6.94 m
D)232 m
E)> 10<sup>3</sup> m
Q2) What are the possible values for the following quantum numbers in an atom?
a.n
b.l
c.m<sub>l </sub>
Q3) The energy of an electron in the hydrogen atom is determined by
A)the principal quantum number (n)only.
B)the angular momentum quantum number (l )only.
C)the principal and angular momentum quantum numbers (n & l ).
D)the principal and magnetic quantum numbers (n & m<sub>l</sub>).
E)the principal,angular momentum and magnetic quantum numbers.
Q4) The Rydberg equation is an example of an empirical equation.
A)True
B)False
Page 9
To view all questions and flashcards with answers, click on the resource link above.
Chapter 8: Electron Configuration and Chemical Periodicity
Available Study Resources on Quizplus for this Chatper
70 Verified Questions
70 Flashcards
Source URL: https://quizplus.com/quiz/74302
Sample Questions
Q1) Energy states of atoms containing more than one electron arise from nucleus-electron and electron-electron interactions.Which of the following statements correctly describes these effects?
A)Larger nuclear charge lowers energy,more electrons in an orbital lowers energy.
B)Larger nuclear charge lowers energy,more electrons in an orbital increases energy.
C)Smaller nuclear charge lowers energy,more electrons in an orbital lowers energy.
D)Smaller nuclear charge lowers energy,more electrons in an orbital increases energy.
E)None of these statements is generally correct.
Q2) Select the most acidic compound from the following.
A)SO<sub>2</sub>
B)Al<sub>2</sub>O<sub>3</sub>
C)CaO
D)PbO
E)H<sub>2</sub>O
Q3) State Hund's rule,and show how it applies to the ground state of phosphorus atoms.
To view all questions and flashcards with answers, click on the resource link above.
Chapter 9: Models of Chemical Bonding
Available Study Resources on Quizplus for this Chatper
60 Verified Questions
60 Flashcards
Source URL: https://quizplus.com/quiz/74303
Sample Questions
Q1) Which one of the following properties is least characteristic of substances composed of small,covalently-bonded molecules?
A)low melting point
B)low boiling point
C)weak bonds
D)poor electrical conductor when solid
E)poor electrical conductor when molten
Q2) Which of the following contains covalent bonds?
A)BaO
B)IBr
C)Mg
D)LiBr
E)Cu
Q3) Electronegativities on Pauling's scale are calculated from ionization energies and electron affinities.
A)True
B)False
Q4) Using appropriate,real examples to illustrate your answer,describe the correlation between bond energy and bond length for a series of varying bond order.
To view all questions and flashcards with answers, click on the resource link above. Page 11
Chapter 10: The Shapes of Molecules
Available Study Resources on Quizplus for this Chatper
94 Verified Questions
94 Flashcards
Source URL: https://quizplus.com/quiz/74304
Sample Questions
Q1) In a Lewis structure for a molecule or ion,the sum of the formal charges on the atoms is equal to the charge on the molecule or ion.
A)True
B)False
Q2) What is the molecular shape of NH<sub>2</sub>Cl as predicted by the VSEPR theory?
A)trigonal pyramidal
B)tetrahedral
C)T-shaped
D)see-saw
E)trigonal planar
Q3) What is the molecular shape of BeH<sub>2</sub> as predicted by the VSEPR theory?
A)linear
B)bent
C)angular
D)trigonal
E)None of these choices is correct.
Q4) All possible resonance structures contribute equally to the resonance hybrid.
A)True
B)False
Page 12
To view all questions and flashcards with answers, click on the resource link above.
Chapter 11: Theories of Covalent Bonding
Available Study Resources on Quizplus for this Chatper
49 Verified Questions
49 Flashcards
Source URL: https://quizplus.com/quiz/74305
Sample Questions
Q1) In applying molecular orbital theory,the bond order is calculated in the same way as with Lewis structures.
A)True
B)False
Q2) Valence bond theory predicts that sulfur will use _____ hybrid orbitals in sulfur dioxide,SO<sub>2</sub>.
A)sp
B)sp<sup>2</sup>
C)sp<sup>3</sup>
D)sp<sup>3</sup>d
E)sp<sup>3</sup>d<sup>2</sup>
Q3) According to molecular orbital theory,what is the bond order in the O<sub>2</sub><sup>+</sup> ion?
A)5.5
B)5
C)4 D)2.5
E)1.5
Q4) In one sentence state the basic principle of valence bond theory.
Q5) In one sentence state how molecular orbitals are usually obtained.
Page 13
To view all questions and flashcards with answers, click on the resource link above.
Chapter 12: Intermolecular Forces: Liquids,solids,and Phase Changes
Available Study Resources on Quizplus for this Chatper
89 Verified Questions
89 Flashcards
Source URL: https://quizplus.com/quiz/74306
Sample Questions
Q1) The strongest intermolecular interactions between pentane (C<sub>5</sub>H<sub>12</sub>)molecules arise from
A)dipole-dipole forces.
B)London dispersion forces.
C)hydrogen bonding.
D)ion-dipole interactions.
E)carbon-carbon bonds.
Q2) Select the pair of substances in which the one with the higher vapor pressure at a given temperature is listed first.
A)C<sub>7</sub>H<sub>16</sub>,C<sub>5</sub>H<sub>12</sub>
B)CCl<sub>4</sub>,CBr<sub>4</sub>
C)H<sub>2</sub>O,H<sub>2</sub>S
D)CH<sub>3</sub>CH<sub>2</sub>OH,CH<sub>3</sub>-O-CH<sub>3</sub> E)Xe,Kr
Q3) Which of the following substances will have hydrogen bonds between molecules?
A)(CH<sub>3</sub>)<sub>3</sub>N
B)CH<sub>3</sub>-O-CH<sub>3</sub>
C)CH<sub>3</sub>CH<sub>2</sub>-OH
D)CH<sub>3</sub>CH<sub>2</sub>-F E)HI
Page 14
To view all questions and flashcards with answers, click on the resource link above.
Chapter 13: The Properties of Solutions
Available Study Resources on Quizplus for this Chatper
73 Verified Questions
73 Flashcards
Source URL: https://quizplus.com/quiz/74307
Sample Questions
Q1) Which of the following sets of conditions could exist when two liquids which are completely miscible in one another are mixed?
A)(\(\Delta\)H<sub>soln</sub> > 0,entropy of system decreases)
B)(\(\Delta\)H<sub>soln</sub> \(\approx\) 0,entropy of system decreases)
C)(\(\Delta\)H<sub>soln</sub> \(\approx\) 0,entropy change of system \(\approx\) 0)
D)(\(\Delta\)H<sub>soln</sub> \(\approx\) 0,entropy of system increases)
E)None of these choices is correct.
Q2) Methane has a Henry's Law constant (k)of 9.88 \(\times\) 10<sup>-2</sup> mol/(L·atm)when dissolved in benzene at 25°C.How many grams of CH<sub>4</sub> will dissolve in 3.00 L of benzene if the partial pressure of CH<sub>4</sub> is 1.48 atm?
A)0.0667 g
B)0.146 g
C)2.34 g
D)4.83 g
E)7.02 g
Q3) The density of pure water at 25°C is 0.997 g/mL.Considering water as being both solvent and solute,calculate its molarity.
To view all questions and flashcards with answers, click on the resource link above.
15
Chapter 14: The Main-Group Elements: Applying Principles of Bonding and Structure
Available Study Resources on Quizplus for this Chatper
58 Verified Questions
58 Flashcards
Source URL: https://quizplus.com/quiz/74308
Sample Questions
Q1) The polymers containing silicon differ from polymers of carbon in which of the following ways?
A)Silicon-based polymers are larger molecules than carbon-based polymers.
B)Silicon-based polymers generally have a repeating silicon-oxygen link while carbon-based polymers can have carbon-carbon links.
C)Silicon-based polymers generally have inorganic elements attached to the chain while carbon-based polymers generally have organic groups attached.
D)Silicon-based polymers tend to be rigid while carbon-based polymers are generally flexible.
E)Silicon forms stronger bonds than carbon.
Q2) Predict the products for the reaction of the following set of reactants. Sr(s)+ H<sub>2</sub>O(l) \(\to\)
A)SrO(s)+ H<sub>2</sub>(g)
B)Sr<sup>2+</sup>(aq)+ H<sub>2</sub>(g)+ O<sub>2</sub>(g)
C)Sr<sup>2+</sup>(aq)+ H<sub>3</sub>O<sup>+</sup>(aq)
D)Sr<sup>2+</sup>(aq)+ OH<sup>-</sup>(aq)+ H<sub>2</sub>(g)
E)SrH<sub>2</sub>(s)+ O<sub>2</sub>(g)
Q3) Name the three allotropes of carbon and briefly describe their properties and structures.
Page 16
To view all questions and flashcards with answers, click on the resource link above.
Chapter 15: Organic Compounds and the Atomic Properties of
Carbon
Available Study Resources on Quizplus for this Chatper
95 Verified Questions
95 Flashcards
Source URL: https://quizplus.com/quiz/74309
Sample Questions
Q1) Carboxylic acids are weak acids.
A)True
B)False
Q2) All alcohols are capable of hydrogen bonding.
A)True
B)False
Q3) Each amino acid has two functional groups in common and one of 20 other groups attached to the \(\alpha\)-carbon.The two functional groups are
A)carboxyl and amine.
B)ester and amine.
C)carboxyl and amide.
D)alcohol and amine.
E)carboxyl and peptide.
Q4) All ketones are capable of hydrogen bonding.
A)True
B)False
Q5) A characteristic reaction of alkanes is addition.
A)True
B)False
Page 17
Q6) Draw and name all stable molecules with the formula C<sub>5</sub>H<sub>12</sub>.
To view all questions and flashcards with answers, click on the resource link above.
Page 18
Chapter 16: Kinetics: Rates and Mechanisms of Chemical Reactions
Available Study Resources on Quizplus for this Chatper
76 Verified Questions
76 Flashcards
Source URL: https://quizplus.com/quiz/74310
Sample Questions
Q1) The rate law for the rearrangement of CH<sub>3</sub>NC to CH<sub>3</sub>CN at 800 K is rate = (1300 s<sup>-1</sup>)[CH<sub>3</sub>NC].What is the half-life for this reaction?
A)7.69 \(\times\) 10<sup>-4</sup> s
B)5.3 \(\times\) 10<sup>-4</sup> s
C)1.9 \(\times\) 10<sup>-3</sup> s
D)520 s
E)1920 s
Q2) Dinitrogen tetraoxide,N<sub>2</sub>O<sub>4</sub>,decomposes to nitrogen dioxide,NO<sub>2</sub>,in a first-order process.If k = 2.5 \(\times\) 10<sup>3</sup> s<sup>-1</sup> at -5°C and k = 3.5 \(\times\) 10<sup>4</sup> s<sup>-1</sup> at 25°C,what is the activation energy for the decomposition?
A)0.73 kJ/mol
B)58 kJ/mol
C)140 kJ/mol
D)580 kJ/mol
E)> 1000 kJ/mol
Q3) An elementary reaction is a simple,one-step process.
A)True
B)False
Page 19
To view all questions and flashcards with answers, click on the resource link above.
Chapter 17: Equilibrium: the Extent of Chemical Reactions
Available Study Resources on Quizplus for this Chatper
85 Verified Questions
85 Flashcards
Source URL: https://quizplus.com/quiz/74311
Sample Questions
Q1) Which of the following has an effect on the magnitude of the equilibrium constant?
A)activation energy of the forward reaction
B)concentrations of the reactants and products
C)presence of a catalyst
D)change in volume of container
E)change in temperature
Q2) The reaction quotient for a gas phase reaction has a value of 2000.If the number of moles of reactants in the reaction equation is equal to that of the products,which of the following statements is true?
A)The reaction must proceed to the left to establish equilibrium.
B)The reaction must proceed to the right to establish equilibrium.
C)When the system is at equilibrium,the concentrations of the products will be much larger than the concentrations of the reactants.
D)The concentrations of the products are generally larger than the concentrations of the reactants.
E)None of these statements is true.
To view all questions and flashcards with answers, click on the resource link above.
Chapter 18: Acid-Base Equilibria
Available Study Resources on Quizplus for this Chatper
90 Verified Questions
90 Flashcards
Source URL: https://quizplus.com/quiz/74312
Sample Questions
Q1) According to Brønsted and Lowry,which one of the following is not a conjugate acid-base pair?
A)H<sub>3</sub>O<sup>+</sup>/OH<sup>-</sup>
B)CH<sub>3</sub>OH<sub>2</sub><sup>+</sup>/CH<sub>3</sub>OH C)HI/I<sup>-</sup>
D)HSO<sub>4</sub><sup>-</sup>/SO<sub>4</sub><sup>2-</sup>
E)H<sub>2</sub>/H<sup>-</sup>
Q2) Which of the following pairs has the stronger acid listed first?
A)H<sub>2</sub>AsO<sub>3</sub>,H<sub>2</sub>AsO<sub>4</sub>
B)HI,HBr
C)HClO,HClO<sub>3</sub>
D)H<sub>2</sub>S,HCl
E)H<sub>2</sub>SO<sub>3</sub>,H<sub>2</sub>SO<sub>4</sub>
Q3) Select the pair of substances in which an acid is listed followed by its conjugate base.
A)H<sup>+</sup>,HCl
B)NH<sub>3</sub>,NH<sub>4</sub><sup>+</sup>
C)HPO<sub>4</sub><sup>2-</sup>,H<sub>2</sub>PO<sub>4</sub><sup>-</sup>
D)HCO<sub>3</sub><sup>-</sup>,CO<sub>3</sub><sup>2-</sup>
E)CH<sub>3</sub>COOH,CH<sub>3</sub>COOH<sub>2</sub><sup>+</sup>
To view all questions and flashcards with answers, click on the resource link above. Page 21
Chapter 19: Ionic Equilibria in Aqueous Systems
Available Study Resources on Quizplus for this Chatper
96 Verified Questions
96 Flashcards
Source URL: https://quizplus.com/quiz/74313
Sample Questions
Q1) When a strong acid is titrated with a weak base,the pH at the equivalence point
A)is greater than 7.0.
B)is equal to 7.0.
C)is less than 7.0.
D)is equal to the pK<sub>a</sub> of the acid.
E)is equal to the pK<sub>b</sub> of the base.
Q2) The solubility of aluminum hydroxide in water ______________ when dilute nitric acid is added to it.
A)increases
B)decreases
C)does not change
D)first increases,then decreases
E)first decreases,then increases
Q3) Calculate the solubility of copper(II)carbonate,CuCO<sub>3</sub>,in 1.00 mol L<sup>-1</sup> NH<sub>3</sub>.K<sub>sp</sub> = 3.0 \(\times\) 10<sup>-12</sup> for CuCO<sub>3</sub>,K<sub>f</sub> = 5.6 \(\times\) 10<sup>11</sup> for Cu(NH<sub>3</sub>)<sub>4</sub><sup>2+</sup>
Q4) Make a clear distinction between buffer range and buffer capacity.
To view all questions and flashcards with answers, click on the resource link above.
Page 22
Chapter 20: Thermodynamics: Entropy,
Direction of Chemical Reactions
Available Study Resources on Quizplus for this Chatper
84 Verified Questions
84 Flashcards
Source URL: https://quizplus.com/quiz/74314
Sample Questions
Q1) For a chemical reaction to be spontaneous only at high temperatures,which of the following conditions must be met?
A)(\(\Delta\)S° > 0,\(\Delta\)H° > 0)
B)(\(\Delta\)S° > 0,\(\Delta\)H° < 0)
C)(\(\Delta\)S° < 0,\(\Delta\)H° < 0)
D)(\(\Delta\)S° < 0,\(\Delta\)H° > 0)
E)(\(\Delta\)G° > 0)
Q2) A reaction has a positive value of \(\Delta\)H° and a positive value of \(\Delta\)S°. Draw a neat,labeled schematic plot to show how \(\Delta\)G° (y-axis)will depend on absolute temperature (x-axis).
Q3) For what signs of \(\Delta\)H and \(\Delta\)S will a process a.be spontaneous at high temperatures but not at low temperatures? b.not be spontaneous at any temperatures?
Q4) In the expression,S = k ln W,W is called the number of microstates.Explain clearly the meaning of the word "microstate",and why a system under a given set of conditions normally has many microstates.
Q5) State the second and third laws of thermodynamics.
To view all questions and flashcards with answers, click on the resource link above. Page 23
Chapter 21: Electrochemistry: Chemical Change and Electrical Work
Available Study Resources on Quizplus for this Chatper
97 Verified Questions
97 Flashcards
Source URL: https://quizplus.com/quiz/74315
Sample Questions
Q1) a.Write a balanced equation to represent the overall reaction you would expect to occur in the electrolysis of molten KCl.
b.Write a balanced equation to represent the overall reaction you would expect to occur in the electrolysis of aqueous KCl.
c.Clearly explain why the products of the two processes are not the same.
Q2) Which of the following statements about voltaic and electrolytic cells is correct?
A)The anode will definitely gain weight in a voltaic cell.
B)Oxidation occurs at the cathode of both cells.
C)The free energy change,\(\Delta\)G,is negative for the voltaic cell.
D)The electrons in the external wire flow from cathode to anode in an electrolytic cell.
E)None of these statements is correct.
Q3) Write down equations representing the anode half-reaction,the cathode half-reaction and the overall cell reaction for the lead-acid battery.
Q4) Explain what is meant by a fuel cell.Provide a balanced equation to represent the reaction in any fuel cell of your choice.
To view all questions and flashcards with answers, click on the resource link above. Page 24
Chapter 22: The Transition Elements and Their Coordination Compounds
Available Study Resources on Quizplus for this Chatper
72 Verified Questions
72 Flashcards
Source URL: https://quizplus.com/quiz/74316
Sample Questions
Q1) a.How many unpaired 3d electrons will there be in (i)high and (ii)low-spin complexes of Co(II)?
b.How can high and low-spin complexes be recognized and distinguished experimentally?
Q2) a.How can the formation of a complex ion be described in terms of a theory of acids and bases?
b.What is the essential requirement for a molecule or ion to act as a ligand?
Q3) What is the highest possible oxidation state for palladium,Pd?
A)+1
B)+2
C)+3
D)+4
E)+6
Q4) Which of the following will be diamagnetic?
A)Ni<sup>2+</sup>
B)Cr<sup>2+</sup>
C)Mn<sup>2+</sup>
D)Co<sup>3+</sup>
E)Ti<sup>4+</sup>
Page 25
Q5) What is the difference between a coordination compound and a complex ion?
To view all questions and flashcards with answers, click on the resource link above.
Chapter 23: Nuclear Reactions and Their Applications
Available Study Resources on Quizplus for this Chatper
75 Verified Questions
75 Flashcards
Source URL: https://quizplus.com/quiz/74317
Sample Questions
Q1) A 55-kg person exposed to thorium-234 receives 7.5 \(\times\) 10<sup>4</sup> \(\beta\) particles,each with an energy of 1.6 \(\times\) 10<sup>-14</sup> J.How many rads does the person receive?
A)2.1 \(\times\) 10<sup>-19</sup>
B)1.2 \(\times\) 10<sup>-17</sup>
C)2.2 \(\times\) 10<sup>-9</sup>
D)1.2 \(\times\) 10<sup>-9</sup>
E)None of these choices is correct.
Q2) A 30.0-kg child receives 2.65 \(\times\) 10<sup>7</sup> \(\beta\) particles,each with an energy of 4.60 \(\times\)0 10<sup>-13</sup> J.If the RBE = 0.78,how many millirem did the child receive?
A)3.2 \(\times\) 10<sup>-7</sup>
B)5.2 \(\times\) 10<sup>-7</sup>
C)5.2 \(\times\) 10<sup>-4</sup>
D)3.2 \(\times\) 10<sup>-2</sup>
E)None of these choices is correct.
Q3) Radioactive decay follows zero-order kinetics.
A)True
B)False
Q4) Write a complete,balanced equation to represent the alpha decay of radon-210.
To view all questions and flashcards with answers, click on the resource link above. Page 26