Archives: Quiz

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) 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 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) 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) 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) 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) 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 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) 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) 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 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) 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) 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) 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) 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) 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) 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) 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) 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) 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 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) ________ 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) 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) 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) 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 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) 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) 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 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) 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) 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 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) 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) 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) 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) 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) 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) 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) 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) 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 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) 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) 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) 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) 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) 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) 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 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) 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) 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 […]