Atoms Molecules and Ions Chemistry

Atoms, Molecules, and Ions Chemistry 1) A molecule of water contains hydrogen and oxygen in a 1:8 ratio by mass. This is a statement of ________. A) the law of multiple proportions B) the law of constant composition C) the law of conservation of mass D) the law of conservation of energy E) none of the above Answer: B 2) Which one of the following is not one of the postulates of Dalton's atomic theory? A) Atoms are composed of protons, neutrons, and electrons. B) All atoms of a given element are identical; the atoms of different elements are different and have different properties. C) Atoms of an element are not changed into different types of atoms by chemical reactions: atoms are neither created nor destroyed in chemical reactions. D) Compounds are formed when atoms of more than one element combine; a given compound always has the same relative number and kind of atoms. E) Each element is composed of extremely small particles called atoms. Answer: A 3) Consider the following selected postulates of Dalton's atomic theory: (i) Each element is composed of extremely small particles called atoms. (ii) Atoms are indivisible. (iii) Atoms of a given element are identical. (iv) Atoms of different elements are different and have different properties. Which of the postulates is(are) no longer considered valid? A) (i) and (ii) B) (ii) only C) (ii) and (iii) D) (iii) only E) (iii) and (iv) Answer: C 4) Which pair of substances could be used to illustrate the law of multiple proportions? A) SO2, H2SO4 B) CO, CO2 C) H2O, O2 D) CH4, C6H12O6 E) NaCl, KCl Answer: B 5) Which statement below correctly describes the responses of alpha, beta, and gamma radiation to an electric field? A) Both beta and gamma are deflected in the same direction, while alpha shows no response. B) Both alpha and gamma are deflected in the same direction, while beta shows no response. C) Both alpha and beta are deflected in the same direction, while gamma shows no response. D) Alpha and beta are deflected in opposite directions, while gamma shows no response. E) Only alpha is deflected, while beta and gamma show no response. Answer: D 6) Which one of the following is not true concerning cathode rays? A) They originate from the negative electrode. B) They travel in straight lines in the absence of electric or magnetic fields. C) They impart a negative charge to metals exposed to them. D) They are made up of electrons. E) The characteristics of cathode rays depend on the material from which they are emitted. Answer: E 7) The charge on an electron was determined in the ________. A) cathode ray tube, by J. J. Thomson B) Rutherford gold foil experiment C) Millikan oil drop experiment D) Dalton atomic theory E) atomic theory of matter Answer: C 8) ________-rays consist of fast-moving electrons. A) Alpha B) Beta C) Gamma D) X E) none of the above Answer: B 9) 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 deflection of beta particles by gold foil E) proved the law of multiple proportions Answer: B 10) In the Rutherford nuclear-atom model, ________. A) the heavy subatomic particles, protons and neutrons, reside in the nucleus B) the three principal subatomic particles (protons, neutrons, and electrons) all have essentially the same mass C) the light subatomic particles, protons and neutrons, reside in the nucleus D) mass is spread essentially uniformly throughout the atom E) the three principal subatomic particles (protons, neutrons, and electrons) all have essentially the same mass and mass is spread essentially uniformly throughout the atom Answer: A 11) Cathode rays are ________. A) neutrons B) X-rays C) electrons D) protons E) atoms Answer: C 12) Cathode rays are deflected away from a negatively charged plate because ________. A) they are not particles B) they are positively charged particles C) they are neutral particles D) they are negatively charged particles E) they are emitted by all matter Answer: D 13) 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 Answer: B 14) Of the three types of radioactivity characterized by Rutherford, which is/are electrically charged? A) ?-rays B) ?-rays and ?-rays C) ?-rays, ?-rays, and ?-rays D) ?-rays E) ?-rays and ?-rays Answer: B 15) Of the three types of radioactivity characterized by Rutherford, which is/are not electrically charged? A) ?-rays B) ?-rays, ?-rays, and ?-rays C) ?-rays D) ?-rays and ?-rays E) ?-rays and ?-rays Answer: C 16) Of the three types of radioactivity characterized by Rutherford, which are particles? A) ?-rays B) ?-rays, ?-rays, and ?-rays C) ?-rays D) ?-rays and ?-rays E) ?-rays and ?-rays Answer: E 17) Of the three types of radioactivity characterized by Rutherford, which type does not become deflected by a magnetic field? A) ?-rays B) ?-rays and ?-rays C) ?-rays D) ?-rays E) ?-rays, ?-rays, and ?-rays Answer: D 18) Of the following, the smallest and lightest subatomic particle is the ________. A) neutron B) proton C) electron D) nucleus E) alpha particle Answer: C 19) All atoms of a given element have the same ________. A) mass B) number of protons C) number of neutrons D) number of electrons and neutrons E) density Answer: B 20) Which atom has the smallest number of neutrons? A) carbon-14 B) nitrogen-14 C) oxygen-16 D) fluorine-19 E) neon-20 Answer: B 21) Which atom has the largest number of neutrons? A) phosphorus-30 B) chlorine-37 C) potassium-39 D) argon-40 E) calcium-40 Answer: D 22) There are ________ electrons, ________ protons, and ________ neutrons in an atom of Xe. A) 132, 132, 54 B) 54, 54, 132 C) 78, 78, 54 D) 54, 54, 78 E) 78, 78, 132 Answer: D 23) An atom of the most common isotope of gold, Au, has ________ protons, ________ neutrons, and ________ electrons. A) 197, 79, 118 B) 118, 79, 39 C) 79, 197, 197 D) 79, 118, 118 E) 79, 118, 79 Answer: E 24) Which combination of protons, neutrons, and electrons is correct for the isotope of copper, Cu A) 29 p+, 34 n°, 29 e- B) 29 p+, 29 n°, 63 e- C) 63 p+, 29 n°, 63 e- D) 34 p+, 29 n°, 34 e- E) 34 p+, 34 n°, 29 e- Answer: A 25) Which isotope has 45 neutrons? A) Kr B) Br C) Se D) Cl E) Rh Answer: B 26) Which pair of atoms constitutes a pair of isotopes of the same element? A) X X B) X X C) X X D) X X E) X X Answer: B 27) Which isotope has 36 electrons in an atom? A) Kr B) Br C) Se D) Cl E) Hg Answer: A 28) Isotopes are atoms that have the same ________ but differing ________. A) atomic masses, charges B) mass numbers, atomic numbers C) atomic numbers, mass numbers D) charges, atomic masses E) mass numbers, charges Answer: C 29) The nucleus of an atom does not contain ________. A) protons B) protons or neutrons C) neutrons D) subatomic particles E) electrons Answer: E 30) The subatomic particles located in the nucleus with no overall charges are ________. A) electrons B) protons C) neutrons D) protons and neutrons E) protons, neutrons, and electrons Answer: C 31) Different isotopes of a particular element contain the same number of ________. A) protons B) neutrons C) protons and neutrons D) protons, neutrons, and electrons E) subatomic particles Answer: A 32) Different isotopes of a particular element contain different numbers of ________. A) protons B) neutrons C) protons and neutrons D) protons, neutrons, and electrons E) None of the above is correct. Answer: B 33) In the symbol shown below, x = ________. C A) 7 B) 13 C) 12 D) 6 E) not enough information to determine Answer: D 34) In the symbol below, X = ________. X A) N B) C C) Al D) K E) not enough information to determine Answer: B 35) In the symbol below, x = ________. O A) 17 B) 8 C) 6 D) 7 E) not enough information to determine Answer: E 36) In the symbol below, x is ________. C A) the number of neutrons B) the atomic number C) the mass number D) the isotope number E) the elemental symbol Answer: C 37) Which one of the following basic forces is so small that it has no chemical significance? A) weak nuclear force B) strong nuclear force C) electromagnetism D) gravity E) Coulomb's law Answer: D 38) Gravitational forces act between objects in proportion to their ________. A) volumes B) masses C) charges D) polarizability E) densities Answer: B 39) Silver has two naturally occurring isotopes with the following isotopic masses: Ar Ar 106.90509 108.9047 The average atomic mass of silver is 107.8682 amu. The fractional abundance of the lighter of the two isotopes is ________. A) 0.24221 B) 0.48168 C) 0.51835 D) 0.75783 E) 0.90474 Answer: C Diff: 4 Page Ref: Sec. 2.4 LO: 2.4 GO: G4 40) The atomic mass unit is presently based on assigning an exact integral mass (in amu) to an isotope of ________. A) hydrogen B) oxygen C) sodium D) carbon E) helium Answer: D Page Ref: Sec. 2.4 LO: 2.4 GO: G4 41) The element X has three naturally occurring isotopes. The masses (amu) and % abundances of the isotopes are given in the table below. The average atomic mass of the element is ________ amu. A) 219.7 B) 220.4 C) 220.42 D) 218.5 E) 221.0 Answer: B Diff: 3 Page Ref: Sec. 2.4 LO: 2.4 GO: G4 42) Element X has three naturally occurring isotopes. The masses (amu) and % abundances of the isotopes are given in the table below. The average atomic mass of the element is ________ amu. A) 41.54 B) 39.68 C) 39.07 D) 38.64 E) 33.33 Answer: A Diff: 3 Page Ref: Sec. 2.4 LO: 2.4 GO: G4 43) The element X has three naturally occurring isotopes. The isotopic masses (amu) and % abundances of the isotopes are given in the table below. The average atomic mass of the element is ________ amu. A) 161.75 B) 162.03 C) 162.35 D) 163.15 E) 33.33 Answer: C Diff: 3 Page Ref: Sec. 2.4 LO: 2.4 GO: G4 44) The element X has three naturally occurring isotopes. The isotopic masses (amu) and % abundances of the isotopes are given in the table below. The average atomic mass of the element is ________ amu. A) 33.33 B) 55.74 C) 56.11 D) 57.23 E) 56.29 Answer: C Diff: 3 Page Ref: Sec. 2.4 LO: 2.4 GO: G4 45) The element X has two naturally occurring isotopes. The masses (amu) and % abundances of the isotopes are given in the table below. The average atomic mass of the element is ________ amu. A) 30.20 B) 33.20 C) 34.02 D) 35.22 E) 32.73 Answer: B Diff: 3 Page Ref: Sec. 2.4 LO: 2.4 GO: G4 46) The average atomic weight of copper, which has two naturally occurring isotopes, is 63.5. One of the isotopes has an atomic weight of 62.9 amu and constitutes 69.1% of the copper isotopes. The other isotope has an abundance of 30.9%. The atomic weight (amu) of the second isotope is ________ amu. A) 63.2 B) 63.8 C) 64.1 D) 64.8 E) 28.1 Answer: D Diff: 4 Page Ref: Sec. 2.4 LO: 2.4 GO: G4 47) The element X has three naturally occurring isotopes. The masses (amu) and % abundances of the isotopes are given in the table below. The average atomic mass of the element is ________ amu. A) 17.20 B) 16.90 C) 17.65 D) 17.11 E) 16.90 Answer: A Diff: 3 Page Ref: Sec. 2.4 LO: 2.4 GO: G4 48) Vanadium has two naturally occurring isotopes, 50V with an atomic mass of 49.9472 amu and 51V with an atomic mass of 50.9440. The atomic weight of vanadium is 50.9415. The percent abundances of the vanadium isotopes are ________% 50V and ________% 51V. A) 0.25, 99.75 B) 99.75, 0.25 C) 49, 51 D) 1.0, 99 E) 99, 1.0 Answer: A Diff: 4 Page Ref: Sec. 2.4 LO: 2.4 GO: G4 49) An unknown element is found to have three naturally occurring isotopes with atomic masses of 35.9675 (0.337%), 37.9627 (0.063%), and 39.9624 (99.600%). Which of the following is the unknown element? A) Ar B) K C) Cl D) Ca E) None of the above could be the unknown element. Answer: A Page Ref: Sec. 2.4 LO: 2.4 GO: G4 50) In the periodic table, the elements are arranged in ________. A) alphabetical order B) order of increasing atomic number C) order of increasing metallic properties D) order of increasing neutron content E) reverse alphabetical order Answer: B 51) Elements ________ exhibit similar physical and chemical properties. A) with similar chemical symbols B) with similar atomic masses C) in the same period of the periodic table D) on opposite sides of the periodic table E) in the same group of the periodic table Answer: E 52) Which pair of elements would you expect to exhibit the greatest similarity in their physical and chemical properties? A) H, Li B) Cs, Ba C) Ca, Sr D) Ga, Ge E) C, O Answer: C 53) Which pair of elements would you expect to exhibit the greatest similarity in their physical and chemical properties? A) O, S B) C, N C) K, Ca D) H, He E) Si, P Answer: A 54) Which pair of elements would you expect to exhibit the greatest similarity in their physical and chemical properties? A) As, Br B) Mg, Al C) I, At D) Br, Kr E) N,O Answer: C 55) The elements in groups 1A, 6A, and 7A are called ________, respectively. A) alkaline earth metals, halogens, and chalcogens B) alkali metals, chalcogens, and halogens C) alkali metals, halogens, and noble gases D) alkaline earth metals, transition metals, and halogens E) halogens, transition metals, and alkali metals Answer: B 56) 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 Answer: C 57) An element in the upper right corner of the periodic table ________. A) is either a metal or metalloid B) is definitely a metal C) is either a metalloid or a nonmetal D) is definitely a nonmetal E) is definitely a metalloid Answer: D 58) An element that appears in the lower left corner of the periodic table is ________. A) either a metal or metalloid B) definitely a metal C) either a metalloid or a nonmetal D) definitely a nonmetal E) definitely a metalloid Answer: B 59) Elements in the same group of the periodic table typically have ________. A) similar mass numbers B) similar physical properties only C) similar chemical properties only D) similar atomic masses E) similar physical and chemical properties Answer: E 60) Which one of the following molecular formulas is also an empirical formula? A) C6H6O2 B) C2H6SO C) H2O2 D) H2P4O6 E) C6H6 Answer: B Page Ref: Sec. 2.6 LO: 2.6 61) Which compounds do not have the same empirical formula? A) C2H2, C6H6 B) CO, CO2 C) C2H4, C3H6 D) C2H4O2, C6H12O6 E) C2H5COOCH3, CH3CHO Answer: B Page Ref: Sec. 2.6 LO: 2.6 62) Of the choices below, which one is not an ionic compound? A) PCl5 B) MoCl6 C) RbCl D) PbCl2 E) NaCl Answer: A Page Ref: Sec. 2.6 LO: 2.6 63) Which type of formula provides the most information about a compound? A) empirical B) molecular C) simplest D) structural E) chemical Answer: D Page Ref: Sec. 2.6 LO: 2.6 64) A molecular formula always indicates ________. A) how many of each atom are in a molecule B) the simplest whole-number ratio of different atoms in a compound C) which atoms are attached to which in a molecule D) the isotope of each element in a compound E) the geometry of a molecule Answer: A Page Ref: Sec. 2.6 LO: 2.6 65) An empirical formula always indicates ________. A) which atoms are attached to which in a molecule B) how many of each atom are in a molecule C) the simplest whole-number ratio of different atoms in a compound D) the isotope of each element in a compound E) the geometry of a molecule Answer: C Page Ref: Sec. 2.6 LO: 2.6 66) 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 Answer: C Page Ref: Sec. 2.6 LO: 2.6 67) Formulas that show how atoms are attached in a molecule are called ________. A) molecular formulas B) ionic formulas C) empirical formulas D) diatomic formulas E) structural formulas Answer: E Page Ref: Sec. 2.6 LO: 2.6 68) Of the following, ________ contains the greatest number of electrons. A) P3+ B) P C) P2- D) P3- E) P2+ Answer: D 69) Which species has 54 electrons? A) Xe+ B) Te2- C) Sn2+ D) Cd E) Xe2+ Answer: B 70) Which species has 16 protons? A) 31P B) 34S2- C) 36Cl D) 80Br- E) 16O Answer: B 71) Which species has 18 electrons? A) 39K B) 32S2- C) 35Cl D) 27Al3+ E) 64Cu2+ Answer: B Page Ref: Sec 2.7 72) The species ________ contains 16 neutrons. A) 31P B) 34S2- C) 36Cl D) 80Br- E) 16O Answer: A 73) Which species is an isotope of 39Cl? A) 40Ar+ B) 34S2- C) 36Cl- D) 80Br E) 39Ar Answer: C 74) Which one of the following species has as many electrons as it has neutrons? A) 1H B) 40Ca2+ C) 14C D) 19F- E) 14C2+ Answer: D 75) There are ________ protons, ________ neutrons, and ________ electrons in I-. A) 131, 53, 54 B) 131, 53, 52 C) 53, 78, 54 D) 53, 131, 52 E) 78, 53, 72 Answer: C 76) There are ________ protons, ________ neutrons, and ________ electrons in U+5. A) 146, 92, 92 B) 92, 146, 87 C) 92, 146, 92 D) 92, 92, 87 E) 146, 92, 146 Answer: B 77) Which species has 48 electrons? A) Sn+2 B) Sn+4 C) Cd+2 D) Ga E) Ti Answer: A 78) Which of the following compounds would you expect to be ionic? A) H2O B) CO2 C) SrCl2 D) SO2 E) H2S Answer: C LO: 2.6 79) Which pair of elements is most apt to form an ionic compound with each other? A) barium, bromine B) calcium, sodium C) oxygen, fluorine D) sulfur, fluorine E) nitrogen, hydrogen Answer: A 80) Which pair of elements is most apt to form a molecular compound with each other? A) aluminum, oxygen B) magnesium, iodine C) sulfur, fluorine D) potassium, lithium E) barium, bromine Answer: C 81) Which species below is the nitride ion? A) Na+ B) NO3- C) NO2- D) NH4+ E) N3- Answer: E 82) Barium reacts with a polyatomic ion to form a compound with the general formula Ba3(X)2. What would be the most likely formula for the compound formed between sodium and the polyatomic ion X? A) NaX B) Na2X C) Na2X2 D) Na3X E) Na3X2 Answer: D 83) Aluminum reacts with a certain nonmetallic element to form a compound with the general formula Al2X3. Element X must be from Group ________ of the Periodic Table of Elements. A) 3A B) 4A C) 5A D) 6A E) 7A Answer: D 84) The formula for a salt is XBr. The X-ion in this salt has 46 electrons. The metal X is ________. A) Ag B) Pd C) Cd D) Cu E) Cs Answer: A 85) Which formula/name pair is incorrect? A) Mn(NO2)2 manganese(II) nitrite B) Mg(NO3)2 magnesium nitrate C) Mn(NO3)2 manganese(II) nitrate D) Mg3N2 magnesium nitrite E) Mg(MnO4)2 magnesium permanganate Answer: D 86) Which formula/name pair is incorrect? A) FeSO4 iron(II) sulfate B) Fe2(SO3)3 iron(III) sulfite C) FeS iron(II) sulfide D) FeSO3 iron(II) sulfite E) Fe2(SO4)3 iron(III) sulfide Answer: E 87) Which one of the following is the formula of hydrochloric acid? A) HClO3 B) HClO4 C) HClO D) HCl E) HClO2 Answer: D 88) The suffix -ide is used primarily ________. A) for monatomic anion names B) for polyatomic cation names C) for the name of the first element in a molecular compound D) to indicate binary acids E) for monoatomic cations Answer: A 89) Which one of the following compounds is chromium(III) oxide? A) Cr2O3 B) CrO3 C) Cr3O2 D) Cr3O E) Cr2O4 Answer: A 90) Which one of the following compounds is copper(I) chloride? A) CuCl B) CuCl2 C) Cu2Cl D) Cu2Cl3 E) Cu3Cl2 Answer: A 91) The correct name for MgF2 is ________. A) monomagnesium difluoride B) magnesium difluoride C) manganese difluoride D) manganese bifluoride E) magnesium fluoride Answer: E 92) The correct name for NaHCO3 is ________. A) sodium hydride B) persodium carbonate C) persodium hydroxide D) sodium bicarbonate E) carbonic acid Answer: D 93) A correct name for Fe(NO3)2 is ________. A) iron nitrite B) ferrous nitrite C) ferrous nitrate D) ferric nitrite E) ferric nitrate Answer: C Diff: 3 94) The correct name for HNO2 is ________. A) nitrous acid B) nitric acid C) hydrogen nitrate D) hyponitrous acid E) pernitric acid Answer: A Diff: 3 95) The proper formula for the hydronium ion is ________. A) H- B) OH- C) N3- D) H3O+ E) NH4+ Answer: D 96) The charge on the ________ ion is -3. A) sulfate B) acetate C) permanganate D) oxide E) nitride Answer: E 97) Which one of the following polyatomic ions has the same charge as the hydroxide ion? A) ammonium B) carbonate C) nitrate D) sulfate E) phosphate Answer: C 98) Which element forms an ion with the same charge as the ammonium ion? A) potassium B) chlorine C) calcium D) oxygen E) nitrogen Answer: A 99) The formula for the compound formed between aluminum ions and phosphate ions is ________. A) Al3(PO4)3 B) AlPO4 C) Al(PO4)3 D) Al2(PO4)3 E) AlP Answer: B 100) Which metal does not form cations of differing charges? A) Na B) Cu C) Co D) Fe E) Sn Answer: A 101) Which metal forms cations of differing charges? A) K B) Cs C) Ba D) Al E) Sn Answer: E 102) The correct name for Ni(CN)2 is ________. A) nickel (I) cyanide B) nickel cyanate C) nickel carbonate D) nickel (II) cyanide E) nickel (I) nitride Answer: D 103) What is the molecular formula for 1-propanol? A) CH4O B) C2H6O C) C3H8O D) C4H10O E) C5H12O Answer: C Diff: 3 Page Ref: Sec. 2.9 LO: 2.9 2.2 Bimodal Questions 1) Methane and ethane are both made up of carbon and hydrogen. In methane, there are 12.0 g of carbon for every 4.00 g of hydrogen, a ratio of 3:1 by mass. In ethane, there are 24.0 g of carbon for every 6.00 g of hydrogen, a ratio of 4:1 by mass. This is an illustration of the law of ________. A) constant composition B) multiple proportions C) conservation of matter D) conservation of mass E) octaves Answer: B 2) ________ and ________ reside in the atomic nucleus. A) Protons, electrons B) Electrons, neutrons C) Protons, neutrons D) Neutrons, only neutrons E) none of the above Answer: C 3) 200 pm is the same as ________ Å. A) 2000 B) 20 C) 200 D) 2 E) 0.0002 Answer: D GO: G4 4) The atomic number indicates ________. A) the number of neutrons in a nucleus B) the total number of neutrons and protons in a nucleus C) the number of protons or electrons in a neutral atom D) the number of atoms in 1 g of an element E) the number of different isotopes of an element Answer: C 5) The nucleus of an atom contains ________. A) electrons B) protons, neutrons, and electrons C) protons and neutrons D) protons and electrons E) protons Answer: C 6) In the periodic table, the elements touching the steplike line are known as ________. A) transition elements B) noble gases C) metalloids D) nonmetals E) metals Answer: C 7) Which group in the periodic table contains only nonmetals? A) 1A B) 6A C) 2B D) 2A E) 8A Answer: E 8) Horizontal rows of the periodic table are known as ________. A) periods B) groups C) metalloids D) metals E) nonmetals Answer: A 9) Vertical columns of the periodic table are known as ________. A) metals B) periods C) nonmetals D) groups E) metalloids Answer: D 10) Elements in Group 1A are known as the ________. A) chalcogens B) alkaline earth metals C) alkali metals D) halogens E) noble gases Answer: C 11) Elements in Group 2A are known as the ________. A) alkaline earth metals B) alkali metals C) chalcogens D) halogens E) noble gases Answer: A 12) Elements in Group 6A are known as the ________. A) alkali metals B) chalcogens C) alkaline earth metals D) halogens E) noble gases Answer: B 13) Elements in Group 7A are known as the ________. A) chalcogens B) alkali metals C) alkaline earth metals D) halogens E) noble gases Answer: D 14) Elements in Group 8A are known as the ________. A) halogens B) alkali metals C) alkaline earth metals D) chalcogens E) noble gases Answer: E 15) Potassium is a ________ and chlorine is a ________. A) metal, nonmetal B) metal, metal C) metal, metalloid D) metalloid, nonmetal E) nonmetal, metal Answer: A 16) Lithium is a ________ and magnesium is a ________. A) nonmetal, metal B) nonmetal, nonmetal C) metal, metal D) metal, metalloid E) metalloid, metalloid Answer: C 17) Oxygen is a ________ and nitrogen is a ________. A) metal, metalloid B) nonmetal, metal C) metalloid, metalloid D) nonmetal, nonmetal E) nonmetal, metalloid Answer: D 18) Calcium is a ________ and silver is a ________. A) nonmetal, metal B) metal, metal C) metalloid, metal D) metal, metalloid E) nonmetal, metalloid Answer: B 19) ________ are found uncombined, as monatomic species in nature. A) Noble gases B) Chalcogens C) Alkali metals D) Alkaline earth metals E) Halogens Answer: A Page Ref: Sec. 2.6 LO: 2.6 20) When a metal and a nonmetal react, the ________ tends to lose electrons and the ________ tends to gain electrons. A) metal, metal B) nonmetal, nonmetal C) metal, nonmetal D) nonmetal, metal E) None of the above; these elements share electrons. Answer: C Page Ref: Sec. 2.6 LO: 2.6 21) The empirical formula of a compound with molecules containing 12 carbon atoms, 14 hydrogen atoms, and 6 oxygen atoms is ________. A) C12H14O6 B) CHO C) CH2O D) C6H7O3 E) C2H4O Answer: D Page Ref: Sec. 2.6 LO: 2.6 22) ________ typically form ions with a 2+ charge. A) Alkaline earth metals B) Halogens C) Chalcogens D) Alkali metals E) Transition metals Answer: A 23) What is the formula of the compound formed between strontium ions and nitrogen ions? A) SrN B) Sr3N2 C) Sr2N3 D) SrN2 E) SrN3 Answer: B Diff: 3 24) Magnesium reacts with a certain element to form a compound with the general formula MgX. What would the most likely formula be for the compound formed between potassium and element X? A) K2X B) KX2 C) K2X3 D) K2X2 E) KX Answer: A 25) The charge on the manganese in the salt MnF3 is ________. A) 1+ B) 1- C) 2+ D) 2- E) 3+ Answer: E 26) Aluminum reacts with a certain nonmetallic element to form a compound with the general formula AlX. Element X is a diatomic gas at room temperature. Element X must be ________. A) oxygen B) fluorine C) chlorine D) nitrogen E) sulfur Answer: D 27) Sodium forms an ion with a charge of ________. A) 1+ B) 1- C) 2+ D) 2- E) 0 Answer: A 28) Potassium forms an ion with a charge of ________. A) 2+ B) 1- C) 1+ D) 2- E) 0 Answer: C 29) Calcium forms an ion with a charge of ________. A) 1- B) 2- C) 1+ D) 2+ E) 0 Answer: D 30) Barium forms an ion with a charge of ________. A) 1+ B) 2- C) 3+ D) 3- E) 2+ Answer: E 31) Aluminum forms an ion with a charge of ________. A) 2+ B) 3- C) 1+ D) 3+ E) 1- Answer: D 32) Fluorine forms an ion with a charge of ________. A) 1- B) 1+ C) 2+ D) 3+ E) 3- Answer: A 33) Iodine forms an ion with a charge of ________. A) 7- B) 1+ C) 2- D) 2+ E) 1- Answer: E 34) Oxygen forms an ion with a charge of ________. A) 2- B) 2+ C) 3- D) 3+ E) 6+ Answer: A 35) Sulfur forms an ion with a charge of ________. A) 2+ B) 2- C) 3+ D) 6- E) 6+ Answer: B 36) Predict the empirical formula of the ionic compound that forms from sodium and fluorine. A) NaF B) Na2F C) NaF2 D) Na2F3 E) Na3F2 Answer: A 37) Predict the empirical formula of the ionic compound that forms from magnesium and fluorine. A) Mg2F3 B) MgF C) Mg2F D) Mg3F2 E) MgF2 Answer: E 38) Predict the empirical formula of the ionic compound that forms from magnesium and oxygen. A) Mg2O B) MgO C) MgO2 D) Mg2O2 E) Mg3O2 Answer: B 39) Predict the empirical formula of the ionic compound that forms from aluminum and oxygen. A) AlO B) Al3O2 C) Al2O3 D) AlO2 E) Al2O Answer: C 40) The correct name for K2S is ________. A) potassium sulfate B) potassium disulfide C) potassium bisulfide D) potassium sulfide E) dipotassium sulfate Answer: D 41) The correct name for Al2O3 is ________. A) aluminum oxide B) dialuminum oxide C) dialuminum trioxide D) aluminum hydroxide E) aluminum trioxide Answer: A 42) The correct name for CaH2 is ________. A) hydrocalcium B) calcium dihydride C) calcium hydroxide D) calcium dihydroxide E) calcium hydride Answer: E 43) The correct name for SO is ________. A) sulfur oxide B) sulfur monoxide C) sulfoxide D) sulfate E) sulfite Answer: B 44) The correct name for CCl4 is ________. A) carbon chloride B) carbon tetrachlorate C) carbon perchlorate D) carbon tetrachloride E) carbon chlorate Answer: D 45) The correct name for N2O5 is ________. A) nitrous oxide B) nitrogen pentoxide C) dinitrogen pentoxide D) nitric oxide E) nitrogen oxide Answer: C 46) The correct name for H2CO3 is ________. A) carbonous acid B) hydrocarbonate C) carbonic acid D) carbohydrate E) carbohydric acid Answer: C 47) The correct name for H2SO3 is ________. A) sulfuric acid B) sulfurous acid C) hydrosulfuric acid D) hydrosulfic acid E) sulfur hydroxide Answer: B 48) The correct name for H2SO4 is ________. A) sulfuric acid B) sulfurous acid C) hydrosulfuric acid D) hydrosulfic acid E) sulfur hydroxide Answer: A 49) The correct name for HNO3 is ________. A) nitrous acid B) nitric acid C) hydronitroxide acid D) nitroxide acid E) nitrogen hydroxide Answer: B 50) The correct name for HClO3 is ________. A) hydrochloric acid B) perchloric acid C) chloric acid D) chlorous acid E) hydrochlorous acid Answer: C 51) The correct name for HClO is ________. A) hydrochloric acid B) perchloric acid C) chloric acid D) chlorous acid E) hypochlorous acid Answer: E 52) The correct name for HBrO4 is ________. A) hydrobromic acid B) perbromic acid C) bromic acid D) bromous acid E) hydrobromous acid Answer: B 53) The correct name for HBrO is ________. A) hydrobromic acid B) perbromic acid C) bromic acid D) bromous acid E) hypobromous acid Answer: E 54) The correct name for HBrO2 is ________. A) hydrobromic acid B) perbromic acid C) bromic acid D) bromous acid E) hydrobromous acid Answer: D 55) The correct name for HClO2 is ________. A) perchloric acid B) chloric acid C) hypochlorous acid D) hypychloric acid E) chlorous acid Answer: E 56) The correct name of the compound Na3N is ________. A) sodium nitride B) sodium azide C) sodium trinitride D) sodium(III) nitride E) trisodium nitride Answer: A 57) The formula of bromic acid is ________. A) HBr B) HBrO4 C) HBrO D) HBrO3 E) HBrO2 Answer: D 58) The correct formula for molybdenum (IV) hypochlorite is ________. A) Mo(ClO3)4 B) Mo(ClO)4 C) Mo(ClO2)4 D) Mo(ClO4)4 E) MoCl4 Answer: B 59) The name of PCl3 is ________. A) potassium chloride B) phosphorus trichloride C) phosphorous(III) chloride D) monophosphorous trichloride E) trichloro potassium Answer: B 60) The ions Ca2+ and PO43- form a salt with the formula ________. A) CaPO4 B) Ca2(PO4)3 C) Ca2PO4 D) Ca(PO4)2 E) Ca3(PO4)2 Answer: E 61) The correct formula of iron (III) bromide is ________. A) FeBr2 B) FeBr3 C) FeBr D) Fe3Br3 E) Fe3Br Answer: B 62) Magnesium and sulfur form an ionic compound with the formula ________. A) MgS B) Mg2S C) MgS2 D) Mg2S2 E) Mg2S3 Answer: A 63) The formula of ammonium carbonate is ________. A) (NH4)2CO3 B) NH4CO2 C) (NH3)2CO4 D) (NH3)2CO3 E) N2(CO3)3 Answer: A 64) The formula of the chromate ion is ________. A) CrO42- B) CrO23- C) CrO- D) CrO32- E) CrO2- Answer: A 65) The formula of the carbonate ion is ________. A) CO22- B) CO32- C) CO33- D) CO2- E) CO- Answer: B 66) The correct name for Mg(ClO3)2 is ________. A) magnesium chlorate B) manganese chlorate C) magnesium chloroxide D) magnesium perchlorate E) manganese perchlorate Answer: A 67) What is the correct formula for ammonium sulfide? A) NH4SO3 B) (NH4)2SO4 C) (NH4)2S D) NH3S E) N2S3 Answer: C 68) When calcium reacts with sulfur the compound formed is ________. A) Ca2S2 B) Ca3S2 C) CaS D) CaS2 E) Ca2S3 Answer: C 69) Chromium and chlorine form an ionic compound whose formula is CrCl3. The name of this compound is ________. A) chromium chlorine B) chromium (III) chloride C) monochromium trichloride D) chromium (III) trichloride E) chromic trichloride Answer: B 70) Iron and chlorine form an ionic compound whose formula is FeCl3. The name of this compound is ________. A) iron chlorine B) iron (III) chloride C) moniron trichloride D) iron (III) trichloride E) ferric trichloride Answer: B 71) Copper and chlorine form an ionic compound whose formula is CuCl2. The name of this compound is ________. A) copper chlorine B) copper (III) dichloride C) monocopper dichloride D) copper (II) dichloride E) cupric chloride Answer: E 72) The name of the binary compound N2O4 is ________. A) nitrogen oxide B) nitrous oxide C) nitrogen (IV) oxide D) dinitrogen tetroxide E) oxygen nitride Answer: D 73) The formula for zinc phosphate is Zn3(PO4)2. What is the formula for cadmium arsenate? A) Cd4(AsO2)3 B) Cd3(AsO4)2 C) Cd3(AsO3)4 D) Cd2(AsO4)3 E) Cd2(AsO4)4 Answer: B 74) The formula for aluminum hydroxide is ________. A) AlOH B) Al3OH C) Al2(OH)3 D) Al(OH)3 E) Al2O3 Answer: D 75) The name of the ionic compound V2O3 is ________. A) vanadium (III) oxide B) vanadium oxide C) vanadium (II) oxide D) vanadium (III) trioxide E) divanadium trioxide Answer: A 76) The name of the ionic compound NH4CN is ________. A) nitrogen hydrogen cyanate B) ammonium carbonitride C) ammonium cyanide D) ammonium hydrogen cyanate E) cyanonitride Answer: C 77) The name of the ionic compound (NH4)3PO4 is ________. A) ammonium phosphate B) nitrogen hydrogen phosphate C) tetrammonium phosphate D) ammonia phosphide E) triammonium phosphate Answer: A 78) What is the formula for perchloric acid? A) HClO B) HClO3 C) HClO4 D) HClO2 E) HCl Answer: C 79) The correct name for HIO2 is ________. A) hypoiodic acid B) hydriodic acid C) periodous acid D) iodous acid E) periodic acid Answer: D 80) What is the molecular formula for propane? A) C2H8 B) C3H6 C) C3H8 D) C4H8 E) C4H10 Answer: C Page Ref: Sec. 2.9 LO: 2.9 81) What is the molecular formula for butane? A) C2H8 B) C3H6 C) C3H8 D) C4H8 E) C4H10 Answer: E Page Ref: Sec. 2.9 LO: 2.9 82) What is the molecular formula for octane? A) C4H10 B) C5H10 C) C6H14 D) C14H28 E) C8H18 Answer: E Page Ref: Sec. 2.9 LO: 2.9 83) What is the molecular formula for pentane? A) C2H8 B) C3H6 C) C4H8 D) C5H12 E) C5H10 Answer: D Page Ref: Sec. 2.9 LO: 2.9 84) What is the molecular formula for nonane? A) C9H18 B) C9H20 C) C10H20 D) C10H22 E) C10H24 Answer: B Page Ref: Sec. 2.9 LO: 2.9 85) What is the molecular formula for heptane? A) C6H12 B) C6H14 C) C7H14 D) C7H16 E) C7H18 Answer: D Page Ref: Sec. 2.9 LO: 2.9 86) What is the molecular formula for 1-hexanol? A) C6H13O B) C6H14O C) C6H15O D) C7H14O E) C7H15O Answer: B Page Ref: Sec. 2.9 LO: 2.9 2.3 Algorithmic Questions 1) A certain mass of carbon reacts with 128 g of oxygen to form carbon monoxide. ________ grams of oxygen would react with that same mass of carbon to form carbon dioxide, according to the law of multiple proportions. A) 25.6 B) 64.0 C) 128 D) 1280 E) 256 Answer: E Diff: 3 Var: 5 GO: G4 2) An atom of 13C contains ________ protons. A) 6 B) 19 C) 7 D) 9 E) 13 Answer: A 7 3) Of the following, the subatomic particle with the smallest mass is the ________. A) proton B) neutron C) electron D) alpha particle E) isotope Answer: C 5 4) An atom of 118Xe contains ________ neutrons. A) 54 B) 172 C) 64 D) 110 E) 118 Answer: C 7 5) There are ________ protons, ________ electrons, and ________ neutrons in an atom of Xe. A) 129, 129, 129 B) 129, 129, 75 C) 54, 75, 129 D) 54, 54, 75 E) 54, 54, 129 Answer: D Var: 5 6) An atom of 14C contains ________ electrons. A) 14 B) 20 C) 8 D) 10 E) 6 Answer: E 7 7) 87 pm is the same as ________ Angstroms. A) 870 B) 8.7 C) 87 D) .87 E) .087 Answer: D Var: 5 GO: G4 8) 200 pm is the same as ________ Å. A) 2000 B) 20 C) 200 D) 2 E) 0.0002 Answer: D Var: 5 GO: G4 9) In the symbol below, X = ________. X A) Zr B) K C) Sc D) Br E) not enough information to determine Answer: B Var: 5 10) In the symbol below, x = ________. Cl A) 17 B) 34 C) 16 D) 36 E) not enough information to determine Answer: E Var: 5 11) The mass number of an atom of 14C is ________. A) 6 B) 20 C) 8 D) 14 E) 10 Answer: D 7 12) Which atom has the largest number of neutrons? A) silicon-30 B) sulfur-36 C) argon-38 D) calcium-44 E) magnesium-24 Answer: D Diff: 3 Var: 50+ 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 14) How many protons are there in one atom of 71Ga? A) 40 B) 70 C) 71 D) 31 E) 13 Answer: D Diff: 3 Var: 5 15) How many electrons are there in one atom of 71Ga? A) 40 B) 70 C) 71 D) 31 E) 13 Answer: D Diff: 3 Var: 5 16) Which pair of atoms constitutes a pair of isotopes of the same element? A) X X B) X X C) X X D) X X E) X X Answer: B Var: 50+ 17) The atomic number of an atom of 80Br is ________. A) 115 B) 35 C) 45 D) 73 E) 80 Answer: B 7 18) How many total electrons are in the Li+ ion? A) 2 B) 3 C) 4 D) 7 E) 8 Answer: A Var: 5 19) How many total electrons are in the O2- ion? A) 10 B) 8 C) 9 D) 16 E) 18 Answer: A Var: 5 20) If a iron atom loses 2 electrons to make an ion, what is the charge on that ion? A) 2+ B) 1+ C) 3+ D) 2- E) 1- Answer: A Var: 5 21) If an atom gains 3 electrons to make an ion, what is the charge on that ion? A) 3+ B) 1+ C) 2+ D) 1- E) 3- Answer: E Var: 3 22) An ion has 26 protons, 29 neutrons, and 23 electrons. The symbol for the ion is ________. A) 55Fe3+ B) 55Fe3- C) 52Cu3+ D) 52Cu3- E) 55V3- Answer: A 0 23) The element X has three naturally occurring isotopes. The masses (amu) and % abundances of the isotopes are given in the table below. The average atomic mass of the element is ________ amu. A) 33.333 B) 220.40 C) 220.24 D) 219.00 E) 219.67 Answer: B Diff: 3 Var: 5 Page Ref: Sec. 2.4 LO: 2.4 GO: G4 24) The element X has three naturally occurring isotopes. The masses (amu) and % abundances of the isotopes are given in the table below. The average atomic mass of the element is ________ amu. A) 159.4 B) 162.0 C) 163.1 D) 161.5 E) 163.0 Answer: B Diff: 3 Var: 5 Page Ref: Sec. 2.4 LO: 2.4 GO: G4 25) The element X has three naturally occurring isotopes. The masses (amu) and % abundances of the isotopes are given in the table below. The average atomic mass of the element is ________ amu. A) 52.62 B) 56.14 C) 55.70 D) 55.40 E) 55.74 Answer: B Diff: 3 Var: 5 Page Ref: Sec. 2.4 LO: 2.4 GO: G4 26) The element ________ is the most similar to sodium in chemical and physical properties. A) Mg B) Br C) N D) K E) Sr Answer: D Diff: 3 Var: 4 27) Which pair of elements would you expect to exhibit the greatest similarity in their physical and chemical properties? A) Li, F B) Sr, Te C) O, S D) In, Sb E) Ti, Ne Answer: C Var: 50+ 28) Which one of the following is a metalloid? A) Se B) Hf C) Zr D) Xe E) Si Answer: E Var: 5 29) The element lithium is in a group known as the _______. A) transition metals B) alkaline earth metals C) noble gases D) halogens E) alkali metals Answer: E Var: 4 30) The element chlorine is in a group known as the _______. A) transition metals B) noble gases C) alkali metals D) alkaline earth metals E) halogens Answer: E Var: 4 31) The element calcium is in a group known as the _______. A) transition metals B) alkali metals C) halogens D) noble gases E) alkaline earth metals Answer: E Var: 4 32) Of the following, only ________ is not a metalloid. A) B B) Po C) Si D) Ge E) As Answer: B Var: 4 33) Which of the following elements is a nonmetal? A) At B) Rh C) Tc D) Mo E) Zr Answer: A Var: 4 34) Which one of the following will occur as diatomic molecules in elemental form? A) helium B) argon C) chlorine D) phosphorous E) sodium Answer: C Var: 50+ Page Ref: Sec. 2.6 35) How many electrons does the As3- ion possess? A) 30 B) 36 C) 2 D) 8 E) 33 Answer: B 0 36) How many protons does the Br- ion possess? A) 34 B) 36 C) 6 D) 8 E) 35 Answer: E 0 37) Which one of the following is most likely to gain electrons when forming an ion? A) Mn B) Zn C) F D) Li E) Al Answer: C Var: 50+ 38) The formula of a salt is XCl2. The X-ion in this salt has 24 electrons. The metal X is ________. A) Ni B) Fe C) Zn D) V E) Pd Answer: B Var: 5 39) Predict the charge of the most stable ion of selenium. A) 3+ B) 1- C) 2+ D) 2- E) 1+ Answer: D 0 40) Predict the charge of the most stable ion of aluminum. A) 3- B) 1+ C) 2+ D) 1- E) 3+ Answer: E 0 41) Which of the following compounds would you expect to be ionic? A) C2H6 B) NH3 C) H2O2 D) LiBr E) None of the above. Answer: D Var: 50+ 42) Which species below is the sulfate ion? A) CN- B) SO42- C) OH- D) SO32- E) None of the above Answer: B Var: 4 43) Which species below is the nitrate ion? A) NO2- B) NO3- C) ClO3- D) ClO4- E) MnO4- Answer: B Var: 5 44) Which species below is the chromate ion? A) Cr2O72- B) CrO42- C) CH3COO- D) CO32- E) None of the above Answer: B Var: 4 45) The correct name for CaO is ________. A) calcium oxide B) calcium hydroxide C) calcium peroxide D) calcium monoxide E) calcium dioxide Answer: A Var: 4 46) Element M reacts with fluorine to form an ionic compound with the formula MF3. The M-ion has 21 electrons. Element M is ________. A) Al B) Cr C) Mn D) Fe E) Sc Answer: B Var: 5 47) The charge on the copper ion in the salt CuO is ________. A) +1 B) +2 C) +4 D) +3 E) +5 Answer: B Var: 5 48) The charge on the silver ion in the salt AgCl is ________. A) +2 B) +1 C) +3 D) +4 E) +5 Answer: B Var: 4 49) The name of the ionic compound NaBrO4 is ________. A) sodium perbromate B) sodium bromate C) sodium hypobromate D) sodium perbromite E) sodium bromide Answer: A Var: 4 50) When a bromine atom forms the bromide ion, it has the same charge as the ________ ion. A) sulfide B) ammonium C) nitrate D) phosphate E) sulfite Answer: C Var: 4 51) Which element forms an ion with the same charge as the sulfate ion? A) magnesium B) sodium C) fluorine D) vanadium E) sulfur Answer: E Var: 50+ 52) The correct name for Na2O2 is ________. A) sodium oxide B) sodium dioxide C) disodium dioxide D) sodium peroxide E) disodium oxide Answer: D Var: 4 53) Which metal is not required to have its charge specified in the names of ionic compounds it forms? A) Cr B) Ni C) Zr D) Na E) Mo Answer: D Var: 50+ 2.4 Short Answer Questions 1) What group in the periodic table would the fictitious element :: be found? Answer: VIIA 2) Which element in Group IA is the most electropositive? Answer: francium 3) The formula for potassium sulfide is ________. Answer: K2S 4) What is the name of an alcohol derived from hexane? Answer: hexanol Page Ref: Sec. 2.9 LO: 2.9 2.5 True/False Questions 1) The possible oxidation numbers for iron are +1 and +2. Answer: FALSE 2) The formula for chromium (II) iodide is CrI2. Answer: TRUE 3) H2SeO4 is called selenic acid. Answer: TRUE 4) The correct name for Na3N is sodium azide. Answer: FALSE