Archives: Quiz

1) What is the actual ratio of calcium to protein intake (mg to g) for most U.S. women? a. 3:1 b. 9:1 c. 13:1 d. 21:1 e. 36:1 2) Which of the following is an effective strategy for dealing with […]

1) Discuss several examples of naturally occurring toxicants in foods and appropriate methods to minimize exposure to them. 2) Of the following, which is used most widely as an antimicrobial agent? a. Sugar b. Saccharin c. Sodium nitrite d. Sodium […]

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

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