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1) In the resonance form of ozone shown below, the formal charge on the central oxygen atom is ________. A) 0 B) +1 C) -1 D) +2 E) -2 2) Of the following molecules, only ________ is polar. A) CCl4 […]

1) Determine the freezing point (oC) of a 0.015 molal aqueous solution of MgSO4. Assume i = 2.0 for MgSO4. The molal freezing-point-depression constant of water is 1.86 oC/m. A) -0.056 B) -0.028 C) -0.17 D) -0.084 E) 0.000 2) […]

1) A correct name for Fe(NO3)2 is ________. A) iron nitrite B) ferrous nitrite C) ferrous nitrate D) ferric nitrite E) ferric nitrate 2) A buffer solution with a pH of 4.63 is prepared with 0.14 M formic acid and […]

1) Predict the product in the combination reaction below. Al (s) + N2 (g) → ________ A) AlN B) Al3N C) AlN2 D) Al3N2 E) AlN3 2) The nucleus of an atom does not contain ________. A) protons B) protons […]

1) Which species has 18 electrons? A) 39K B) 32S2- C) 35Cl D) 27Al3+ E) 64Cu2+ 2) The value of G o at 261.0 oC for the formation of phosphorous trichloride from its constituent elements, P2 (g) + 3Cl2 (g) […]

1) Calculate the percentage by mass of hydrogen in PtCl2(NH3)2. A) 1.558 B) 1.008 C) 0.672 D) 0.034 E) 2.016 2) The rate of a reaction depends on ________. A) collision frequency B) collision energy C) collision orientation D) all […]

1) In which of the following aqueous solutions would you expect CuBr to have the highest solubility? A) 0.0100 M KBr B) 0.040 M CuNO3 C) 0.030 M NaBr D) 0.020 M LiBr E) CuBr will have the same solubility […]

1) Which one of the following processes produces a decrease in the entropy of the system? A) freezing of Fe(l) into Fe(s) B) evaporation of liquid ethanol into gaseous ethanol C) dissolution of LiOH(s) in water D) melting ice to […]

1) Resonance structures differ by ________. A) number and placement of electrons B) number of electrons only C) placement of atoms only D) number of atoms only E) placement of electrons only 2) The ion NO– has ________ valence electrons. […]

1) Which of the following are decomposition reactions? 1. CH4 (g) + O2 (g) → CO2 (g) + H2O (l) 2. CaO (s) + CO2 (g) → CaCO3 (s) 3. Mg (s) + O2 (g) → MgO (s) 4. PbCO3 […]

1) In humans, what percent of absorbed iron is found in blood? A) 15 B) 25 C) 40 D) 60 E) 75 2) All the elements in group 8A are gases at room temperature. Of all the groups in the […]

1) The pH of a 0.15 M aqueous solution of NaZ (the sodium salt of HZ) is 10.7. What is the Ka for HZ? A) 1.6 x 10-6 B) 6.0 x 10-9 C) 8.9 x 10-4 D) 1.3 x 10-12 […]

1) Which of the following ions will act as a weak base in water? A) HS– B) F– C) NO2 – D) ClO– E) All of the above will act as a weak base in water. 2) Which combination will […]

1) The length of the side of a cube having a density of 12.6 g/ml and a mass of 7.65 g is ________ cm. A) 3.20 B) 0.847 C) 1.02 D) 0.584 E) 1.32 2) A 5.00-g sample of copper […]

1) Air containing 4% H2 can be explosive. 2) The wavelength of radio waves can be longer than a football field. Answer: TRUE 3) In some molecules and polyatomic ions, the sum of the valence electrons is odd and as […]

1) Of the following, which is most likely to form interstitial carbides? A) active metals B) transition metals C) boron and silicon D) alkaline earth metals E) alkali metals 2) A common English set of units for expressing velocity is […]

1) The rate law for a reaction is rate = k[A][B] Which one of the following statements is false? A) The reaction is first order overall. B) The reaction is first order in A. C) The reaction is first order […]

1) Which one of the following substances would be the most soluble in CCl4? A) C4H10 B) Li2O C) NH3 D) HCl E) CH3CH2CH2OH 2) According to valence bond theory, which orbitals overlap in the formation of the bond in […]

1) Which one of the following configurations depicts an excited carbon atom? A) 1s22s22p13s1 B) 1s22s22p3 C) 1s22s22p1 D) 1s22s23s1 E) 1s22s22p2 2) A carbonyl compound contains ________. A) a carbon-oxygen double bond B) a carbon-oxygen triple bond C) a […]

1) A solution is prepared by dissolving 23.7 g of CaCl2 in 375 g of water. The density of the resulting solution is 1.05 g/mL. The concentration of CaCl2 in this solution is ________ molal. A) 0.214 B) 0.569 C) […]

1) Which element has the largest bonding atomic radius? A) scandium B) titanium C) vanadium D) chromium E) manganese 2) The rate constant for this reaction is ________ s-1. A) 6.9 x 10-2 B) 3.0 x 10-2 C) 14 D) […]

1) Under ordinary conditions, a substance will sublime rather than melt if its triple point occurs at a pressure above atmospheric pressure. 2) Ammonia is a strong base. Answer: FALSE 3) Xenon can have oxidation states of 2, 4, 6, […]

1) Thermodynamic Quantities for Selected Substances at 298.15 K (25 oC) The value of G o at 25 oC for the decomposition of calcium chloride into its constituent elements, CaCl2 (s) –> Ca (s) + Cl2 (g) is ________ kJ/mol. […]

1) Transuranium elements have atomic numbers greater than ________. A) 90 B) 91 C) 92 D) 93 E) 94 2) What is the conjugate base of OH–? A) O2 B) O– C) H2O D) O2- E) H3O+ Answer: D 3) […]

1) In order to produce sp3 hybrid orbitals, ________ s atomic orbital(s) and ________ p atomic orbital(s) must be mixed. A) one, two B) one, three C) one, one D) two, two E) two, three 2) Atomic radius generally decreases […]

1) Alkali metals tend to be more reactive than alkaline earth metals because ________. A) alkali metals have lower densities B) alkali metals have lower melting points C) alkali metals have greater electron affinities D) alkali metals have lower ionization […]

1) Which one of the following substances is produced during the reaction of an acid with a metal hydroxide? A) H2 B) H2O C) CO2 D) NaOH E) O2 2) Acetic acid is a weak acid that dissociates into the […]

1) The value of ΔH° for the reaction below is -6535 kJ. ________ kJ of heat are released in the combustion of 16.0 g of C6H6 (l)? 2C6H6 (l) + 15O2 (g) → 12CO2 (g) + 6 H2O (l) A) […]

1) In the absence of magnetic or electric fields, cathode rays ________. A) do not exist B) travel in straight lines C) cannot be detected D) become positively charged E) bend toward a light source 2) In which aqueous system […]

1) The bond angle marked a in the following molecule is about ________. A) 109.5 B) 60 C) 180 D) 120 E) 90 2) For a given reaction, H = +74.6 kJ/mol, and the reaction is spontaneous at temperatures above […]

1) At what speed (m/s) must a 3.0-mg object be moving in order to have a de Broglie wavelength of 5.4 X 10-29 m? A) 1.6 X 10-28 m/s B) 3.9 X 10-4 m/s C) 2.0 X 1012 m/s D) […]

1) Which of the following liquids will have the lowest freezing point? A) pure H2O B) aqueous glucose (0.60 m) C) aqueous sucrose (0.60 m) D) aqueous FeI3 (0.24 m) E) aqueous KF (0.50 m) 2) At 333 K, which […]

1) The value of ΔE for a system that performs 139 kJ of work on its surroundings and gains 54kJ of heat is ________ kJ. A) -85 B) 193 C) 7506 D) 85 E) -193 2) The reaction of 50 […]

1) A sample of air from a home is found to contain 7.2 ppm of carbon monoxide. This means that if the total pressure is 695 torr, then the partial pressure of CO is ________ torr. A) 5.0 103 B) […]

1) The molecular formula of a compound is always ________ the empirical formula. A) more complex than B) different from C) an integral multiple of D) the same as E) simpler than 2) Which formula/name pair is incorrect? A) Mn(NO2)2manganese(II) […]

1) The gold foil experiment performed in Rutherford’s lab ________. A) confirmed the plum-pudding model of the atom B) led to the discovery of the atomic nucleus C) was the basis for Thomson’s model of the atom D) utilized the […]

1) Using the data in the table, which of the conjugate acids below is the strongest acid? A) NH4 + B) C5H5NH+ C) H3NOH+ D) NH3CH3 + E) NH4 + and NH3CH3 + 2) A substance with unpaired electrons will […]

1) Consider the following equilibrium. 2 SO2 (g) + O2 (g) 2 SO3 (g) The equilibrium cannot be established when ________ is/are placed in a 1.0-L container. A) 0.25 mol SO2 (g) and 0.25 mol O2 (g) B) 0.75 mol […]

1) A valid Lewis structure of ________ cannot be drawn without violating the octet rule. A) PO4 3- B) SiF4 C) CF4 D) SeF4 E) NF3 2) Alkenes have the general formula ________. A) CnH2n B) CnH2n-2 C) CnH2n+2 D) […]

1) Xenon has been shown to form compounds only when it is combined with ________. A) something with a tremendous ability to remove electrons from other substances B) another noble gas C) something with a tremendous ability to donate electrons […]

1) A reaction that is spontaneous as written ________. A) is very rapid B) will proceed without outside intervention C) is also spontaneous in the reverse direction D) has an equilibrium position that lies far to the left E) is […]

1) Of the following atoms, which has the largest first ionization energy? A) K B) Rb C) Sr D) Ca E) Ba 2) For the reaction 2 C4H10 (g) + 13 O2 (g) –> 8 CO2 (g) + 10 H2O […]

1) The relationship between the concentrations of reactants and products of a system at equilibrium is given by the law of mass action. 2) Possible shapes of AB3 molecules are linear, trigonal planar, and T-shaped. Answer: FALSE[/cpmembership] 3) The bond […]

1) 3.2 cm3 = 0.0032 L 2) Two deviations of real gases from ideal gases which are treated in the van der Waals equation are finite molecular volume and non-zero molecular attractions. Answer: TRUE 3) Gamma radiation only changes the […]

1) When a metal gains an electron, the process is endothermic. 2) The reduction of O2 by sodium hydride produces lye. Answer: TRUE 3) In radioactive dating, the ratio of carbon-12 to carbon-14 is related to the time of death […]

1) Thermodynamic Quantities for Selected Substances at 298.15 K (25 oC) The value of S o for the catalytic hydrogenation of acetylene to ethene, C2H2 (g) + H2 (g) –> C2H4 (g) is ________ J/K mol. A) +18.6 B) +550.8 […]

1) The reaction 4Al (s) + 3O2 → (g) 2Al2O3 (s) ΔH° = -3351 kJ is ________, and therefore heat is ________ by the reaction. A) endothermic, released B) endothermic, absorbed C) exothermic, released D) exothermic, absorbed E) thermoneutral, neither […]

1) The names of complex anions end in ________. A) -o B) -ium C) -ate D) -ous E) -ic 2) Of the following, the entropy of ________ is the largest. A) B2F4 (g) B) BF3 (g) C) B2H6 (g) D) […]

1) The square of Schrodinger’s wave equation is called an orbital. 2) Aldehydes are less reactive than ketones. Answer: FALSE 3) Radioactive decay is a first order kinetic process. Answer: TRUE 4) A gas is considered “ideal” if one mole […]

1) Metal oxides are typically ________ while nonmetal oxides are typically ________. A) basic, amphoteric B) basic, acidic C) amphoteric, basic D) acidic, basic E) amphoteric, acidic 2) Together, liquids and solids constitute ________ phases of matter. A) the compressible […]

1) The volume of an ideal gas is zero at ________. A) 0 °C B) -45 °F C) -273 K D) -363 K E) -273 °C 2) For an isothermal process, the entropy change of the surroundings is given by […]

1) Which one of the following atoms has the largest radius? A) In B) Sn C) Sb D) Te E) I 2) What is the F€Xe€F bond angle in XeF2? A) 180° B) 90° C) 109.5° D) 120° E) 60° […]

1) A combination of sand, salt, and water is an example of a ________. A) homogeneous mixture B) heterogeneous mixture C) compound D) pure substance E) solid 2) Fuel values of hydrocarbons increase as the H/C atomic ratio increases. Which […]

1) Which of the following molecules or ions will exhibit delocalized bonding? A) SO2, SO3, and SO3 2- B) SO3 2- only C) SO2 and SO3 D) SO3 and SO3 2- E) None of the above will exhibit delocalized bonding. […]

1) The molecular weight is always a whole-number multiple of the empirical formula weight. 2) The DNA double helix is held together by hydrogen bonds and London dispersion forces. Answer: TRUE 3) In the reaction BF3 + F––> BF4 – […]

1) The specific heat capacity of lead is 0.13 J/g-K. How much heat (in J) is required to raise the temperature of 15 g of lead from 22 °C to 37 °C? A) 2.0 J B) -0.13 J C) 5.8 […]

1) HA is a weak acid. Which equilibrium corresponds to the equilibrium constant Kb for A–? A) HA (aq) + H2O (l) H2A+ (aq) + OH–(aq) B) A– (aq) + H3O+ (aq) HA (aq) + H2O (l) C) HA (aq) […]

1) The name of the ionic compound NaBrO4 is ________. A) sodium perbromate B) sodium bromate C) sodium hypobromate D) sodium perbromite E) sodium bromide 2) What is/are the product(s) of photodissociation of molecular oxygen? A) molecular nitrogen B) excited […]

1) What is the oxidation state of chromium in [Cr(H2O)4Cl2]+? A) 0 B) +2 C) +3 D) -2 E) -3 2) Elements in the same group of the periodic table typically have ________. A) similar mass numbers B) similar physical […]

1) Calcium is a ________ and silver is a ________. A) nonmetal, metal B) metal, metal C) metalloid, metal D) metal, metalloid E) nonmetal, metalloid 2) Which equation correctly represents the reaction between elemental chlorine and sodium iodide? A) Cl […]

1) 1 picometer = ________ centimeters A) 1 X 1010 B) 1 X 10-10 C) 1 X 108 D) 1 X 10-8 E) 1 X 10-12 2) The solubility of nitrogen gas in water at 25 oC and a nitrogen […]

1) For molecules of the general formula ABn, n can be greater than four ________. A) for any element A B) only when A is an element from the third period or below the third period C) only when A […]

1) Bombardment of uranium-238 with a deuteron (hydrogen-2) generates neptunium-237 and ________ neutrons. A) 1 B) 2 C) 3 D) 4 E) 5 2) The reaction used to inflate automobile airbags ________. A) produces sodium gas B) is a combustion […]

1) The Ka for formic acid (HCO2H) is 1.8 x 10-4. What is the pH of a 0.20 M aqueous solution of sodium formate (NaHCO2)? A) 11.64 B) 5.48 C) 3.39 D) 8.52 E) 4.26 2) 30.0 grams of argon […]

1) Heats of vaporization are greater than heats of fusion. 2) In the formula k = 0.693/t1/2, k is the decay constant. Answer: TRUE 3) The extent of ionization of a weak electrolyte is increased by adding to the solution […]

1) What volume (mL) of 142 M phosphoric acid can be neutralized with 0.367 mL of 0.0824 M sodium hydroxide? A) 211 B) 12.9 C) 1900 D) 632 E) 1570 2) Why does ozone not form in high concentrations in […]

1) Given the data in the table below, ΔH°rxn for the reaction Ca(OH)2 + 2H3AsO4 → Ca(H2AsO4)2 + 2H2O is ________ kJ. A) -744.9 B) -4519 C) -4219 D) -130.4 E) -76.4 2) A ________ liquid crystal has the least […]

1) What is the coefficient of H2O when the following equation is completed and balanced? Ba (s) + H2O (l) → A) 1 B) 2 C) 3 D) 5 E) Ba(s) does not react with H2O (l). 2) In the […]

1) As a gaseous element condenses, the atoms become ________ and they have ________ attraction for one another. A) less separated, more B) less separated, less C) more separated, more D) more separated, less E) smaller, lesser 2) Of the […]

1) Which of the following correctly represents the third ionization of aluminum? A) Al2+ (g) + e– → Al+ (g) B) Al (g) → Al+ (g) + e– C) Al2- (g) + e– → Al3- (g) D) Al2+ (g) + […]

1) If chloride is a ligand to a transition metal, it will not be precipitated by silver nitrate. 2) The principal source of the difference in the normal boiling points of ICl (97 oC; molecular mass 162 amu) and Br2 […]

1) Which formula/name pair is incorrect? A) FeSO4iron(II) sulfate B) Fe2(SO3)3 iron(III) sulfite C) FeSiron(II) sulfide D) FeSO3iron(II) sulfite E) Fe2(SO4)3 iron(III) sulfide 2) Thermodynamic Quantities for Selected Substances at 298.15 K (25 oC) The value of S o for […]

1) The majority of glucose molecules exist in ring structure. 2) Nitrogen is colorless because the minimum energy to excite an electron is in the ultraviolet section of the spectrum. Answer: TRUE 3) The color of hemoglobin changes from purple […]

1) You have to calculate the volume of a gas sample with mass of 1.000 X 103 g and density of 1.027 g/L, but you have forgotten the formula. Which way of reasoning would help you in finding the correct […]

1) ________ is a unique element and does not truly belong to any family. A) Nitrogen B) Radium C) Hydrogen D) Uranium E) Helium 2) The ________ ion has a noble gas electron configuration. A) Be2+ B) Li2+ C) Li […]

1) What is the coefficient of NO2 when the following disproportionation reaction is balanced? NO2 (g) + H2O (l) –> H+ (aq) + NO3 – (aq) + NO (g) A) 1 B) 2 C) 3 D) 5 E) 4 2) […]

1) The enthalpy change for the following reaction is -483.6 kJ: 2H2 (g) + O2 (g) → 2H2O (g) Therefore, the enthalpy change for the following reaction is ________ kJ. 4H2 (g) + 2O2 (g) → 4H2O (g) A) -483.6 […]

1) The formula weight of ammonium sulfate ((NH4)2SO4), rounded to the nearest integer, is ________ amu. A) 100 B) 118 C) 116 D) 132 E) 264 2) How many moles of Co2+ are present in 0.200 L of a 0.400 […]

1) Which one of the following is not true concerning radon? A) It decays by alpha emission. B) It decays to polonium-218, an alpha emitter. C) It is chemically active in human lungs. D) It has been implicated in lung […]

1) The melting and boiling points of hydrocarbons are determined by ________. A) ion-dipole attraction B) dipole-dipole attraction C) London forces D) hydrogen bonding E) ionic bonding 2) The value of ΔH° for the reaction below is -790 kJ. The […]

1) Which one of the following is the formula of hydrochloric acid? A) HClO3 B) HClO4 C) HClO D) HCl E) HClO2 2) Sulfur dioxide is not released into the atmosphere in any significant amount by ________. A) burning of […]

1) Thermodynamic Quantities for Selected Substances at 298.15 K (25 oC) The value of S o for the catalytic hydrogenation of acetylene to ethane, C2H2 (g) + 2H2 (g) –> C2H6 (g) is ________ J/K mol. A) -76.0 B) +440.9 […]

1) Which of the following does not have eight valence electrons? A) Ca+ B) Rb+ C) Xe D) Br– E) All of the above have eight valence electrons. 2) A solution containing 10.0 g of an unknown liquid and 90.0 […]

1) The principal quantum number for the outermost electrons in a Te atom in the ground state is ________. A) 3 B) 4 C) 5 D) 6 E) 7 2) Gaseous argon has a density of 1.40 g/L at standard […]

1) The pH of a 0.25 M aqueous solution of hydrofluoric acid, HF, at 25.0 oC is 2.03. What is the value of Ka for HF? A) 2.0 x 10-9 B) 1.1 x 10-9 C) 6.0 x 10-5 D) 3.5 […]

1) The conjugate base of NH3 is ________. A) NH2 – B) NH4 + C) NH2OH D) H3O+ E) OH– 2) Of the substances below, the highest fuel value is obtained from ________. A) charcoal B) bituminous coal C) natural […]

1) A Lewis acid is an electron-pair acceptor, and a Lewis base is an electron-pair donor. 2) The larger the principal quantum number of an orbital, the lower is the energy of the electrons in that orbital. Answer: FALSE 3) […]

1) The shape of a liquid’s meniscus is determined by ________. A) the viscosity of the liquid B) the type of material the container is made of C) the relative magnitudes of cohesive forces in the liquid and adhesive forces […]

1) Which one of the following is not amphoteric? A) Al(OH)3 B) Ca(OH)2 C) Cr(OH)3 D) Zn(OH)2 E) Sn(OH)2 2) Structural changes around a double bond in the ________ portion of the rhodopsin molecule trigger the chemical reactions that result […]

1) The elements in the ________ period of the periodic table have a core-electron configuration that is the same as the electron configuration of neon. A) first B) second C) third D) fourth E) fifth 2) The conjugate acid of […]

1) Which of the following correctly represents the electron affinity of bromine? A) Br (g) → Br+ (g) + e– B) Br (g) + e– → Br– (g) C) Br2 (g) + e– → Br– (g) D) Br2 (g) + […]

1) A borane is a ________. A) compound containing only boron and oxygen B) compound containing only boron and aluminum C) compound containing only boron and hydrogen D) compound containing only boron and carbon E) three-dimensional covalent network of boron […]

1) Which compound would produce a basic aqueous solution? A) KH B) H2S C) C2H6 D) CH3OH E) H2O 2) Calculate the pOH of a solution at 25.0 oC that contains 1.94 x 10-10 M hydronium ions. A) 1.94 B) […]

1) The value of ΔH° for the following reaction is -3351 kJ: 2Al (s) + 3O2 (g) → 2Al2O3 (s) The value of ΔH°f for Al2O3 (s) is ________ kJ. A) -3351 B) -1676 C) -32.86 D) -16.43 E) +3351 […]

1) The density of a gold nugget is 19.3 g/cm3. If the volume of the gold nugget is 0.00369 L, the mass of the nugget is ________ g. A) 71.2 B) 0.191 C) 19.3 D) 5.23 E) none of the […]

1) Atoms surrounded by eight valence electrons tend to lose electrons. 2) At constant temperature, reducing the volume of a gaseous equilibrium mixture causes the reaction to shift in the direction that increases the number of moles of gas in […]

1) The density of nitric oxide (NO) gas at 0.970 atm and 34.9 °C is ________ g/L. A) 0.0384 B) 0.869 C) 1.15 D) 0.339 E) 10.2 2) The correct name for H2SO3 is ________. A) sulfuric acid B) sulfurous […]

1) Accuracy refers to ________. A) how close a measured number is to zero B) how close a measured number is to the calculated value C) how close a measured number is to other measured numbers D) how close a […]

1) The dissolution of 1.0 mol of ________ to 1.0 L of water at 25 °C would yield the most acidic solution. A) SO3 B) CO2 C) CO D) MgO E) CaO 2) Calculate the pH of a solution that […]

1) The hybridization of the central carbon atom in an aldehyde is ________. A) sp B) sp3 C) sp2 D) d2sp3 E) sp4 2) At a temperature of ________ °C, 0.444 mol of CO gas occupies 11.8 L at 839 […]

1) The Henry’s law constant for helium gas in water at 30 oC is 3.70 x 10-4 M/atm. When the partial pressure of helium above a sample of water is 0.400 atm, the concentration of helium in the water is […]

1) Which one of the following exhibits dipole-dipole attraction between molecules? A) NH3 B) CF4 C) C10H22 D) O2 E) SF6 2) In the Haber process, ammonia is synthesized from nitrogen and hydrogen: N2 (g) + 3H2 (g) –> 2NH3 […]

1) Predict the empirical formula of the ionic compound that forms from magnesium and oxygen. A) Mg2O B) MgO C) MgO2 D) Mg2O2 E) Mg3O2 2) What is the maximum number of double bonds that a hydrogen atom can form? […]

1) The mole fraction of urea (MW = 60.0 g/mol) in a solution prepared by dissolving 16 g of urea in 39 g of H2O is ________. A) 0.58 B) 0.37 C) 0.13 D) 0.11 E) 9.1 2) Which of […]

1) Of the following, the entropy of gaseous ________ is the largest at 25 oC and 1 atm. A) I2 B) F2 C) Cl2 D) Br2 E) O3 2) At elevated temperatures, methylisonitrile (CH3NC) isomerizes to acetonitrile (CH3CN): CH3NC (g) […]

1) In a typical multiple bond, the σ bond results from overlap of ________ orbitals and the π bond(s) result from overlap of ________ orbitals. A) hybrid, atomic B) hybrid, hybrid C) atomic, hybrid D) hybrid, hybrid or atomic E) […]

1) Round the number 3456.5 to two significant figures. A) 3400.0 B) 3400 C) 3000 D) 3500 E) 3000.0 2) Of the following, which is the strongest acid? A) HIO4 B) HIO3 C) HIO2 D) HIO E) The acid strength […]

1) The rate constant for a second-order reaction is 0.13 M-1s-1. If the initial concentration of reactant is 0.26 mol/L, it takes ________ s for the concentration to decrease to 0.07 mol/L. A) 0.017 B) 1.4 C) 14 D) 80. […]

1) The electron-domain geometry of the AsF6 – ion is octahedral. The hybrid orbitals used by the As atom for bonding are ________ orbitals. A) sp2d2 B) sp3 C) sp3d D) sp3d2 E) sp2 2) What are the respective concentrations […]

1) The photoelectric effect is ________. A) the total reflection of light by metals giving them their typical luster B) the production of current by silicon solar cells when exposed to sunlight C) the ejection of electrons by a metal […]

1) A stock solution of HNO3 is prepared and found to contain 12.7 M of HNO3. If 25.0 mL of the stock solution is diluted to a final volume of 0.500 L, the concentration of the diluted solution is ________ […]

1) What e x posure level to radiation is fatal to most humans? A) 100 rem B) 200 rem C) 600 rem D) 300 rem E) 1000 rem 2) For a given reaction, H = -24.2 kJ/mol and S = […]

1) Which of the following traits characterizes the alkali metals? A) very high melting point B) existence as diatomic molecules C) formation of dianions D) the lowest first ionization energies in a period E) the smallest atomic radius in a […]

1) Triphenylphosphine is often given the abbreviated formula PPh3. The correct name for Rh(PPh3)3Cl is ________. A) chlorotriphenylphosphinerhodium B) chlorotriphenylphosphinerhodium (I) C) tris(triphenylphosphine)chlororhodium (I) D) chlorotris(triphenylphosphine)rhodium (I) E) chlorotris(triphenylphosphine)rhodate (I) 2) Calculate the percent ionization of formic acid (HCO2H) in […]

1) The concentration of lead nitrate (Pb(NO3)2) in a 0.926 M solution is ________ molal. The density of the solution is 1.202 g/mL. A) 0.770 B) 2.13 C) 1.03 D) 0.819 E) 0.650 2) Which of the following cannot be […]

1) The correct name of H2CO3 is ________. A) hydrogen carbide B) hydrogen carbonate ion C) carbonate ion D) carbonic acid E) carboxylic acid 2) A mixture of Xe, Kr, and Ar has a total pressure of 6.69 atm. What […]

1) The kinetic energy of a 23.2-g object moving at a speed of 81.9 km/hr is ________ kcal. A) 1.43 x 10-3 B) 6.00 C) 1900 D) 454 E) 0.0251 2) 1 kilogram = ________ milligrams A) 1 X 10-6 […]

1) The correct name for HClO2 is ________. A) perchloric acid B) chloric acid C) hypochlorous acid D) hypychloric acid E) chlorous acid 2) Which one of the following could be a straight-chain alkane? A) C9H20 B) C3H3 C) C4H6 […]

1) Of the following, ΔH°f is not zero for ________. A) O2 (g) B) C (graphite) C) N2 (g) D) F2 (s) E) Cl2 (g) 2) C12H26 molecules are held together by ________. A) ion-ion interactions B) hydrogen bonding C) […]

Chemistry: The Central Science, 13e (Brown et al.) Chapter 10 Gases 10.1 Multiple Choice Questions 1) Which of the following statements about gases is false? A) Gases are highly compressible. B) Distances between molecules of gas are very large compared […]

Chemistry: The Central Science, 13e (Brown et al.) Chapter 11 Liquids and Intermolecular Forces 11.1 Multiple-Choice Questions 1) Crystalline solids ________. A) have their particles arranged randomly B) have highly ordered structures C) are usually very soft D) exist only […]

11.2 Bimodal Questions 1) Based on molecular mass and dipole moment of the five compounds in the table below, which should have the highest boiling point? A) CH3CH2CH3 B) CH3OCH3 C) CH3Cl D) CH3CHO E) CH3CN 20 Answer: E Diff: […]

Chemistry: The Central Science, 13e (Brown et al.) Chapter 13 Properties of Solutions 13.1 Multiple-Choice Questions 1) The dissolution of water in octane (C8H18) is prevented by ________. A) London dispersion forces between octane molecules B) hydrogen bonding between water […]

21 18) The mole fraction of urea (MW = 60.0 g/mol) in a solution prepared by dissolving 16 g of urea in 39 g of H2O is ________. A) 0.58 B) 0.37 C) 0.13 D) 0.11 E) 9.1 19) The […]

25) A solution is prepared by dissolving 10.0 g of benzene (C6H6) in 282 g of carbon tetrachloride (CCl4). The concentration of benzene in this solution is ________ molal. The molar masses of C6H6 and CCl4 are 78.1 g/mol and […]

Chemistry: The Central Science, 13e (Brown et al.) Chapter 14 Chemical Kinetics 14.1 Multiple-Choice Questions 1) A burning splint will burn more vigorously in pure oxygen than in air because ________. A) oxygen is a reactant in combustion and concentration […]

17) At elevated temperatures, methylisonitrile (CH3NC) isomerizes to acetonitrile (CH3CN): CH3NC (g) → CH3CN (g) At the start of the experiment, there are 0.200 mol of reactant (CH3NC) and 0 mol of product (CH3CN) in the reaction vessel. After 25 […]

33 15) The rate constant for a particular zero-order reaction is 0.075 M s-1. If the initial concentration of reactant is 0.537 M it takes ________ s for the concentration to decrease to 0.100 M. A) 5.8 B) -5.8 C) […]

Chemistry: The Central Science, 13e (Brown et al.) Chapter 15 Chemical Equilibrium 15.1 Multiple-Choice Questions 1) At equilibrium, ________. A) all chemical reactions have ceased B) the rates of the forward and reverse reactions are equal C) the rate constants […]

12) The equilibrium constant (Kp) for the interconversion of PCl5 and PCl3 is 0.0121: PCl5 (g) PCl3 (g) + Cl2 (g) A vessel is charged with PCl5 giving an initial pressure of 0.123 atm. At equilibrium, the partial pressure of […]

Chemistry: The Central Science, 13e (Brown et al.) Chapter 16 Acid-Base Equilibria 16.1 Multiple-Choice Questions 1) According to the Arrhenius concept, an acid is a substance that ________. A) is capable of donating one or more H+ B) causes an […]

18) HZ is a weak acid. An aqueous solution of HZ is prepared by dissolving 0.020 mol of HZ in sufficient water to yield 1.0 L of solution. The pH of the solution was 4.93 at 25.0 °C. The Ka […]

12) What is the pOH of an aqueous solution at 25.0 °C in which [OH–] is 0.0010 M? A) 11.00 B) -3.00 C) 3.00 D) -11.00 E) 6.91 Answer: C Diff: 2 Var: 9 Page Ref: Sec. 16.4 LO: 16.4 […]

Chemistry: The Central Science, 13e (Brown et al.) Chapter 17 Additional Aspects of Aqueous Equilibria 17.1 Multiple-Choice Questions 1) Which one of the following pairs cannot be mixed together to form a buffer solution? A) HONH2, HONH3Cl B) NaCl, HCl […]

16 (KNO2). The acid dissociation constant of nitrous acid is 4.50 × 10-4. A) 3.093 B) 3.607 C) 14.26 D) 10.91 E) 4.589 5) Calculate the percent ionization of nitrous acid in a solution that is 0.241 M in nitrous […]

Chemistry: The Central Science, 13e (Brown et al.) Chapter 18 Chemistry of the Environment 18.1 Multiple-Choice Questions 1) In the troposphere, temperature ________ with increasing altitude, while in the stratosphere, temperature ________ with increasing altitude. A) increases, increases B) decreases, […]

18) Acid rain typically has a pH of about ________. A) 7 B) 5 C) 4 D) 2 E) 1 Answer: C Diff: 1 Var: 1 Page Ref: Sec. 18.2 LO: 18.2 GO: G2 19) Sulfur dioxide is not released […]

Chemistry: The Central Science, 13e (Brown et al.) Chapter 19 Chemical Thermodynamics 19.1 Multiple-Choice Questions 1) The first law of thermodynamics can be given as ________. A) ΔE = q + w B) Δ = – C) for any spontaneous […]

24) The value of ΔH° for the decomposition of gaseous sulfur dioxide to solid elemental sulfur and gaseous oxygen, SO2 (g) → S (s,rhombic) + O2 (g) is ________ kJ/mol. A) 0.0 B) +135.0 C) -135.90 D) -269.9 E) +269.9 […]

8) Of the following, the entropy of ________ is the largest. A) B2F4 (g) B) BF3 (g) C) B2H6 (g) D) BCl3 (l) E) B2O3 (s) Answer: A Diff: 2 Var: 3 Page Ref: Sec. 19.4 LO: 19.4 GO: G2 […]

Copyright © 2015 Pearson Education, Inc. 72) The species ________ contains 16 neutrons. A) 31P B) 34S2- C) 36Cl D) 80Br– E) 16O Answer: A Diff: 2 Var: 1 Page Ref: Sec. 2.7 LO: 2.7 GO: G2 73) Which species […]

Copyright © 2015 Pearson Education, Inc. 48) The correct name for H2SO4 is ________. A) sulfuric acid B) sulfurous acid C) hydrosulfuric acid D) hydrosulfic acid E) sulfur hydroxide Answer: A Diff: 2 Var: 1 Page Ref: Sec. 2.8 LO: […]

Copyright © 2015 Pearson Education, Inc. 13) How many neutrons are there in one atom of 184W? A) 74 B) 112 C) 258 D) 110 E) 184 Answer: D Diff: 3 Var: 4 Page Ref: Sec. 2.3 LO: 2.3 GO: […]

Chemistry: The Central Science, 13e (Brown et al.) Chapter 20 Electrochemistry 20.1 Multiple-Choice 1) Which element is reduced in the reaction below? Fe(CO)5 (l) + 2HI (g) → Fe(CO)4I2 (s) + CO (g) + H2 (g) A) Fe B) C […]

29) The standard cell potential (E°cell) for the voltaic cell based on the reaction below is ________ V. 2Cr (s) + 3Fe2+ (aq) → 3Fe (s) + 2Cr3+ (aq) A) +0.30 B) +2.80 C) +3.10 D) +0.83 E) -0.16 Answer: […]

Chemistry: The Central Science, 13e (Brown et al.) Chapter 21 Nuclear Chemistry 21.1 Multiple-Choice Questions 1) All atoms of a given element have the same ________. A) mass number B) number of nucleons C) atomic mass D) number of neutrons […]

A) B B) N C) C D) O E) none of the above Answer: B Diff: 2 Var: 1 Page Ref: Sec. 21.1 LO: 21.1 GO: G2 6) In balancing the nuclear reaction Br → E + e, the identity […]

6) When an atom of an element undergoes beta decay, its proton count will change by ________ and its neutron count will change by ________. A) +1, -1 B) 0, 0 C) -1, +1 D) -2, -2 E) -1, -1 […]

Chemistry: The Central Science, 13e (Brown et al.) Chapter 22 Chemistry of the Nonmetals 22.1 Multiple-Choice 1) How many oxygen atoms are bonded to each silicon atom in SiO2? A) 1 B) 2 C) 3 D) 4 E) none Answer: […]

5) Hydrogen can have oxidation states of ________. A) +1 only B) -1, 0, and +1 C) 0 and +1 only D) -1 and +1 only E) 0 only Answer: B Diff: 1 Var: 1 Page Ref: Sec. 22.2 LO: […]

6) Which compound would produce an acidic aqueous solution? A) HF B) MgH2 C) C2H2 D) KH E) H2 Answer: A Diff: 1 Var: 50+ Page Ref: Sec. 22.2 LO: 22.2 – 22.11 GO: G2 7) The oxidation state of […]

Chemistry: The Central Science, 13e (Brown et al.) Chapter 23 Transition Metals and Coordination Chemistry 23.1 Multiple-Choice Questions 1) Chalcocite, chalcopyrite, and malachite are sources of which metal? A) manganese B) copper C) titanium D) iron E) zinc Answer: B […]

A) Ca2+ B) Fe3+ C) CN– D) Fe(CN)63- E) Fe2+ Answer: C Diff: 1 Var: 1 Page Ref: Sec. 23.2 LO: 23.2 GO: G2 11) What is the charge of the central metal ion in Ca3[Fe(CN)6]2? A) 0 B) 1+ […]

Chemistry: The Central Science, 13e (Brown et al.) Chapter 24 The Chemistry of Life: Organic and Biological Chemistry 24.1 Multiple-Choice Questions 1) Which substance would be the most soluble in gasoline? A) water B) NaNO3 C) HCl D) hexane E) […]

17) The octane number of straight-run gasoline is about ________. A) 0 B) 25 C) 50 D) 75 E) 93 Answer: C Diff: 1 Var: 1 Page Ref: Sec. 24.2 LO: 24.2 GO: G2 18) Alkenes have the general formula […]

12) When aqueous solutions of AgNO3 and KI are mixed, AgI precipitates. The balanced net ionic equation is ________. A) Ag+ (aq) + (aq) → AgI (s) B) Ag+ (aq) + NO3– (aq) → AgNO3 (s) C) Ag+ (aq) + […]

Copyright © 2015 Pearson Education, Inc. 27) The value of ΔH° for the reaction below is -1107 kJ: 2Ba (s) + O2 (g) → 2BaO (s) How many kJ of heat are released when 5.75 g of Ba (s) reacts […]

Copyright © 2015 Pearson Education, Inc. 60) Given the data in the table below and ΔH°rxn for the reaction SO2Cl2 (g) + 2H2O (l) → H2SO4 (l) + 2HCl (g) ΔH° = -62 kJ ΔH°f of HCl (g) is ________ […]

Copyright © 2015 Pearson Education, Inc. Chemistry: The Central Science, 13e (Brown et al.) Chapter 7 Periodic Properties of the Elements 7.1 Multiple-Choice Questions 1) In which set of elements would all members be expected to have very similar chemical […]

Copyright © 2015 Pearson Education, Inc. 75) Hydrogen is unique among the elements because ________. 1. It has only one valence electron. 2. It is the only element that can emit an atomic spectrum. 3. Its electron is not at […]

Copyright © 2015 Pearson Education, Inc. 5) ________ is isoelectronic with helium. A) H– B) H+ C) H D) B3- E) N3- Answer: A Diff: 1 Var: 50+ Page Ref: Sec. 7.3 LO: 7.3 GO: G2 6) ________ is isoelectronic […]

Chemistry: The Central Science, 13e (Brown et al.) Chapter 8 Basic Concepts of Chemical Bonding 8.1 Multiple-Choice Questions 1) Which of the following has eight valence electrons? A) Ti4+ B) Kr C) Cl– D) Na+ E) all of the above […]

21 67) The bond order of any molecule containing equal numbers of bonding and antibonding electrons is ________. A) 0 B) 1 C) 2 D) 3 E) 1/2 68) In comparing the same two atoms bonded together, the ________ the […]

1) A compound decomposes by a first-order process. If 13% of the compound decomposes in 60 minutes, the half-life of the compound is ________. A) 299 B) 20 C) 12 D) -18 E) -5 2) Which of the following expressions […]

1) Which of the following ions will act as a weak base in water? A) OH– B) Cl– C) NO3 – D) ClO– E) None of the above will act as a weak base in water. 2) Tetraboric acid, H2B4O7, […]

1) Which one of the following is most soluble in hexane (C6H14)? A) CH3OH B) CH3CH2CH2OH C) CH3CH2OH D) CH3CH2CH2CH2OH E) CH3CH2CH2CH2CH2OH 2) The Lewis structure of the CO3 2- ion is ________. A) B) Answer: E C) D) E) […]

1) To convert from one resonance structure to another, ________. A) only atoms can be moved B) electrons and atoms can both be moved C) only electrons can be moved D) neither electrons nor atoms can be moved E) electrons […]

1) Which of the following is soluble in water at 25 °C? A) AgNO3 B) Hg2Cl2 C) PbCl2 D) Ag2S E) AgCl 2) The value of ΔH° for the reaction below is +128.1 kJ: CH3OH (l) → CO (g) + […]

1) The de Broglie wavelength of a 84.32 gram bullet traveling at the speed of 308.6 m/s is ________ m. A) 2.546 X 10-35 B) 2.546 X 10-36 C) 2.546 X 10-37 D) 2.546 X 10-38 E) 1.724 X 10-32 […]

1) The principal component of smog is sulfur dioxide. 2) The concentration of reactants or products at any time during the reaction can be calculated from the integrated rate law. Answer: TRUE 3) Emulsifying agents typically have a hydrophobic end […]

1) Calculate the molarity of hydro xide ion in an aqueous solution that has a pOH of 3.00. A) 1.0 x 10-3 B) 11.00 C) 1.0 x 10-11 D) 3.0 x 10-14 E) 1.1 x 10-13 2) A substance that […]

1) The correct name for SO is ________. A) sulfur oxide B) sulfur monoxide C) sulfoxide D) sulfate E) sulfite 2) Which isotope has 45 neutrons? A) Kr B) Br C) Se D) Cl E) Rh Answer: B 3) Which […]

1) The angular momentum quantum number (l) value of 2 indicates the ________ subshell. A) d B) f C) s D) p E) +1/2 2) Precision refers to ________. A) how close a measured number is to other measured numbers […]

1) The ________ ion has eight valence electrons. A) Sc3+ B) Ti3+ C) V3+ D) Cr3+ E) Mn3+ 2) In a hydrogen atom, an electron in a ________ orbital can absorb a photon, but cannot emit a photon. A) 3s […]

1) In terms of binding energy per nucleon, what element divides fission and fusion processes? A) H B) He C) C D) Fe E) U 2) Which mineral contains titanium? A) pyrolusite B) chalcopyrite C) galena D) rutile E) sphalerite […]

1) How many pairs of unpaired electrons are there in one molecule of dinitrogen monoxide? A) 4 B) 3 C) 5 D) 2 E) 1 2) The following reaction is second order in [A] and the rate constant is 0.039 […]

1) Based on the equations below, which metal is the most active? Pb(NO3)2 (aq) + Ni (s) → Ni(NO3)2 (aq) + Pb (s) Pb(NO3)2 (aq) + Ag (s) → No reaction Cu(NO3)2 (aq) + Ni (s) → Ni(NO3)2 (aq) + […]

1) Thermodynamic Quantities for Selected Substances at 298.15 K (25 oC) The value of S o for the decomposition of gaseous sulfur trioxide to solid elemental sulfur and gaseous oxygen, 2SO3 (g) –> 2S (s, rhombic) + 3O2 (g) is […]

1) The central atom in ________ does not violate the octet rule. A) SF4 B) KrF2 C) CF4 D) XeF4 E) ICl4 – 2) Which atom can accommodate an octet of electrons, but doesn’t necessarily have to accommodate an octet? […]

1) There is/are ________σ bond(s) in the molecule below. A) 1 B) 2 C) 12 D) 13 E) 18 2) The halogens, alkali metals, and alkaline earth metals have ________ valence electrons, respectively. A) 7, 4, and 6 B) 1, […]

1) At elevated temperatures, nitrogen dioxide decomposes to nitrogen oxide and oxygen: NO2 (g) –> NO (g) + O2 (g) The reaction is second order in NO2 with a rate constant of 0.543 M-1s-1at 300 oC. If the initial [NO2] […]

1) Which one of the following is false concerning pure hydrazine? A) It is an oily, colorless liquid. B) It can be made by reaction of hypochlorite and ammonia. C) It is used as a rocket fuel. D) Hydrazine is […]

1) For a first-order reaction, a plot of ________ versus ________ is linear. A) ln [A]t, B) ln [A]t, t C) , t D) [A]t, t E) t, 2) What mass (g) of AgBr is formed when 57.8 mL of […]

1) Kp = 0.0198 at 721 K for the reaction 2HI (g) H2 (g) + I2 (g) In a particular experiment, the partial pressures of H2 and I2 at equilibrium are 0.678 and 0.788 atm, respectively. The partial pressure of […]

1) The valence shell of the element X contains 2 electrons in a 5s subshell. Below that shell, element X has a partially filled 4d subshell. What type of element is X? A) main group element B) chalcogen C) halogen […]

1) How many hydrogen atoms must bond to silicon to give it an octet of valence electrons? A) 1 B) 2 C) 3 D) 4 E) 5 2) The Keq for the equilibrium below is 7.52 x 10-2 at 480.0 […]

1) According to MO theory, overlap of two s atomic orbitals produces ________. A) one bonding molecular orbital and one hybrid orbital B) two bonding molecular orbitals C) two bonding molecular orbitals and two antibonding molecular orbitals D) two bonding […]

1) What volume (mL) of a concentrated solution of magnesium chloride (9.00 M) must be diluted to 350. mL to make a 2.75 M solution of magnesium chloride? A) 2.75 B) 50.0 C) 45.0 D) 107 E) 350 2) Consider […]

1) Which of the following are strong electrolytes? HCl HC2H3O2 NH3 KCl A) HCl, KCl B) HCl, NH3, KCl C) HCl, HC2H3O2, NH3, KCl D) HCl, HC2H3O2, KCl E) HC2H3O2, KCl 2) [Ar]4s23d104p3 is the electron configuration of a(n) ________ […]

1) Oxides of the active metals combine with acid to form ________. A) hydrogen gas B) metal hydrides C) water and a salt D) oxygen gas E) metal hydroxides 2) The missing product from this reaction is ________. Se + […]

1) Solids have a ________ shape and are not appreciably ________. A) definite, compressible B) definite, incompressible C) indefinite, compressible D) indefinite, incompressible E) sharp, convertible 2) A reaction that is not spontaneous at low temperature can become spontaneous at […]

1) An ideal gas differs from a real gas in that the molecules of an ideal gas ________. A) have no attraction for one another B) have appreciable molecular volumes C) have a molecular weight of zero D) have no […]

1) The specific heat of bromine liquid is 0.226 J/g-K. The molar heat capacity (in J/mol-K) of bromine liquid is ________. A) 707 J/mol-K B) 36.1 J/mol-K C) 18.1 J/mol-K D) 9.05 J/mol-K E) 0.226 J/mol-K 2) The average rate […]

1) The oxidation state of sulfur in the SO3 molecule is ________. A) +6 B) +2 C) -2 D) +4 E) 0 2) Dinitrogentetraoxide partially decomposes according to the following equilibrium: N2O4 (g) 2 NO2 (g) A 1.00-L flask is […]

1) Given the data in the table below, ΔH°rxn for the reaction 3NO2 (g) + H2O (l) → 2HNO3 (aq) + NO (g) is ________ kJ. A) 64 B) 140 C) -140 D) -508 E) -64 2) A 25.0 mL […]

1) A 5-ounce cup of raspberry yogurt contains 6.0 g of protein, 2.0 g of fat, and 16.3 g of carbohydrate. The fuel values for protein, fat, and carbohydrate are 17, 38, and 17 kJ/g, respectively. The fuel value of […]

1) Oxalic acid is a diprotic acid. Calculate the percent of oxalic acid (H2C2O4) in a solid given that a 0.7984-g sample of that solid required 37.98 mL of 0.2283 M NaOH for neutralization. A) 48.89 B) 97.78 C) 28.59 […]

1) Which pair of elements below should be the most similar in chemical properties? A) C and O B) B and As C) I and Br D) K and Kr E) Cs and He 2) Of the following elements, ________ […]

1) CO (5.00 g) and CO2 (5.00 g) were placed in a 750.0 mL container at 50.0 °C. The total pressure in the container was ________ atm. A) 10.3 B) 4.02 C) 6.31 D) 0.292 E) 1.60 2) What are […]

1) Coordination sphere isomers ________. A) have the same molecular formula and coordination number B) have the same molecular formula but different coordination numbers C) have different molecular formulas but the same coordination number D) have different molecular formulas and […]

1) What type of reaction is known as a thermonuclear reaction? A) fission B) fusion C) transmutation D) beta emission E) neutron emission 2) In a px orbital, the subscript x denotes the ________. A) energy of the electron B) […]

1) What is the largest number of protons that can e x ist in a nucleus and still be stable? A) 206 B) 50 C) 92 D) 83 E) 84 2) Electromagnetic radiation with a wavelength of 425 nm appears […]

1) Which one of the following is the highest temperature? A) 38 °C B) 96 °F C) 302 K D) none of the above E) the freezing point of water 2) The half-life of cobalt-60 is 5.20 yr. How many […]

1) The entropy of the universe is ________. A) constant B) continually decreasing C) continually increasing D) zero E) the same as the energy, E 2) The energy of a photon of light is ________ proportional to its frequency and […]

1) The rate limiting step in a reaction is the slowest step in the reaction sequence. 2) Ca(OH)2 is a strong base. Answer: TRUE 3) To separate racemic mixtures, the isomers must be in a chiral environment. Answer: TRUE 4) […]

1) ________-rays consist of fast-moving electrons. A) Alpha B) Beta C) Gamma D) X E) none of the above 2) What radioactive element is used to diagnose medical conditions of the heart and arteries? A) cobalt-60 B) thallium-201 C) radium-226 […]

1) The product of the nuclear reaction in which 40Ar is subjected to neutron capture followed by alpha emission is ________. A) 37S B) 41Ar C) 36S D) 45Ca E) 35Ar 2) A neutralization reaction between an acid and a […]

1) Oxidation is the ________ and reduction is the ________. A) gain of oxygen, loss of electrons B) loss of oxygen, gain of electrons C) loss of electrons, gain of electrons D) gain of oxygen, loss of mass E) gain […]

1) The vapor pressure of pure water at 25 oC is 23.8 torr. What is the vapor pressure (torr) of water above a solution prepared by dissolving 18.0 g of glucose (a nonelectrolyte, MW = 180.0 g/mol) in 95.0 g […]

1) The missing product from this reaction is ________. B + _____ –> N + n A) He B) e C) n D) e E) 2) Of the reactions below, only ________ is not spontaneous. A) Mg (s) + 2HCl […]

1) The instability of xenon fluorides is due to its negative enthalpy of formation. 2) The quantity of product that is calculated to form when all of the limiting reagent reacts is called the actual yield. Answer: FALSE 3) Ozone […]

1) Consider the following reaction: A –> 2C The average rate of appearance of C is given by [C]/t. Comparing the rate of appearance of C and the rate of disappearance of A, we get [C]/t = ________ x (-[A]/t). […]

1) When aqueous solutions of AgNO3 and KI are mixed, AgI precipitates. The balanced net ionic equation is ________. A) Ag+ (aq) + I– → (aq) AgI (s) B) Ag+ (aq) + NO3 – (aq) → AgNO3 (s) C) Ag+ […]

1) The name of PCl3 is ________. A) potassium chloride B) phosphorus trichloride C) phosphorous(III) chloride D) monophosphorous trichloride E) trichloro potassium 2) What is the maximum amount in grams of SO3 that can be produced by the reaction of […]

1) Which compound would produce an acidic aqueous solution? A) HF B) MgH2 C) C2H2 D) KH E) H2 2) Ka for HF is 7.0 x 10-4. Kb for the fluoride ion is ________. A) 2.0 x 10-8 B) 1.4 […]

1) ________ is isoelectronic with argon, and ________ is isoelectronic with neon. A) P3-, N3- B) P2-, N2- C) P3+, N3+ D) N3-, P3- E) P, N 2) The frequency of a photon that has an energy of 3.7 X […]

1) In metallic hydrides, the oxidation number of hydrogen is considered to be ________. A) -2 B) -1 C) 0 D) +1 E) +2 2) A gas at a pressure of 10.0 Pa exerts a force of ________ N on […]

1) Classify the following compounds as weak bases (W) or strong bases (S): ammonia fluoride ion sodium hydro xide A) W W S B) S S S C) S W W D) W S S E) W S W 2) […]

1) The density of a 167.4 g sample of magnesium having a volume of 96.32 mL is ________ g/cm3. A) 0.5754 B) 7128 C) 3.625 D) 2.663 E) 1.738 2) Which solution will be the most basic? A) 0.10 M […]

1) Which one of the following is not an intensive property? A) density B) temperature C) melting point D) mass E) boiling point 2) The carbon-carbon σ bond in ethylene, , results from the overlap of ________. A) sp hybrid […]

1) How many equivalent resonance structures can be drawn for the molecule of SO3 without having to violate the octet rule on the sulfur atom? A) 5 B) 2 C) 1 D) 4 E) 3 2) A pressure of 0.500 […]

1) Element X reacts with chlorine to form a compound with the formula XCl2. The oxide of element X is basic. Element X is ________. A) Rb B) Ca C) Al D) P E) H 2) Which of the following […]

1) The pH of a solution that contains 0.800 M acetic acid (Ka = 1.76 x 10-5) and 0.172 M sodium acetate is ________. A) 4.087 B) 5.422 C) 8.578 D) 8.370 E) 9.913 2) Which one of the following […]

1) Carbon-11 decays by ________. A) alpha emission B) beta emission C) positron emission D) photon emission E) neutron capture 2) Standard temperature and pressure (STP), in the context of gases, refers to ________. A) 298.15 K and 1 atm […]

1) The bond length in an HI molecule is and the measured dipole moment is 0.44 D. What is the magnitude (in units of e) of the negative charge on I in HI? (1 debye = 3.34 x 10-30 coulomb-meters; […]

1) Glass is ________ whereas quartz is ________. A) hard, soft B) crystalline, amorphous C) amorphous, crystalline D) pure SiO2, a mixture of SiO2 and carbonates E) breakable, not breakable 2) How many isomers of C2H2Cl2 are polar? A) none […]

1) The molecular geometry of the H3O+ ion is ________. A) linear B) tetrahedral C) bent D) trigonal pyramidal E) octahedral 2) Which one of the following atoms has the largest radius? A) As B) O C) Sn D) Cs […]

1) When aqueous solutions of Pb(NO3)2 and NaCl are mixed, PbCl2 precipitates. The balanced net ionic equation is ________. A) Pb2+ (aq) + 2Cl– (aq) → PbCl2 (s) B) Pb2+ (aq) + 2NO3 – (aq) → Pb(NO3)2 (s) C) Pb2+ […]

1) Which one of the following solutions will have the greatest concentration of hydroxide ions? A) 1.10 M rubidium hydroxide B) 0.368 M calcium hydroxide C) 0.368 M ammonium hydroxide D) 0.368 M potassium hydroxide E) 0.368 M sulfuric acid […]

1) In the generation of most anions, the energy change (kJ/mol) that _______ an electron is ________. A) removes, positive B) adds, positive C) removes, negative D) adds, negative E) None of the above is correct. 2) On a phase […]

1) On a phase diagram, the critical pressure is ________. A) the pressure required to melt a solid B) the pressure below which a substance is a solid at all temperatures C) the pressure above which a substance is a […]

1) The lowest energy shell that contains f orbitals is the shell with n = ________. A) 3 B) 2 C) 4 D) 1 E) 5 2) The concentration of iodide ions in a 0.193 M solution of barium iodide […]

1) Which atom has the largest number of neutrons? A) silicon-30 B) sulfur-36 C) argon-38 D) calcium-44 E) magnesium-24 2) Which of the following are combustion reactions? 1. CH4 (g) + O2 (g) → CO2 (g) + H2O (l) 2. […]

1) Bromine is much more apt to exist as an anion than is potassium. This is because ________. A) Bromine has a greater electron affinity than potassium does B) Bromine is bigger than potassium C) Bromine has a greater ionization […]

1) All atoms of a given element have the same ________. A) mass number B) number of nucleons C) atomic mass D) number of neutrons E) atomic number 2) Thermodynamic Quantities for Selected Substances at 298.15 K (25 oC) The […]

1) Calculate the freezing point of a 0.05500 m aqueous solution of NaNO3. The molal freezing-point-depression constant of water is 1.86 oC/m. A) 0.0286 B) -0.106 C) 0.106 D) -0.0562 E) -0.205 2) How many chiral centers are there in […]

1) Of the following, a 0.2 M aqueous solution of ________ will have the highest freezing point. A) RbBr B) K2SO4 C) Sr(NO3)2 D) (NH4)2SO4 E) Fe(NO3)2 2) Of the following, ________ has a slight odor of bitter almonds and […]

1) The Lewis structure of AsH3 shows ________ nonbonding electron pair(s) on As. A) 0 B) 1 C) 2 D) 3 E) This cannot be determined from the data given. 2) Which group 6A element is a metal? A) tellurium […]

1) How many protons does the Br– ion possess? A) 34 B) 36 C) 6 D) 8 E) 35 2) CO2 from hydrocarbon combustion creates a major environmental problem that is described as ________. A) the greenhouse effect B) photochemical […]

1) The symbol for the spin magnetic quantum number is ________. A) ms B) n C) l D) ml E) sm 2) Based on the crystal-field strengths Cl– < F– < H2O < NH3 < H2NC2H4NH2, which octahedral Ti (III) […]

1) Which one of the following is an incorrect orbital notation? A) 2s B) 3py C) 3f D) 4dxy E) 4s 2) The electron configuration of a ground-state Ag atom is ________. A) [Ar]4s24d9 B) [Kr]5s14d10 C) [Kr]5s23d9 D) [Ar]4s14d10 […]