Archives: Quiz

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