front 1 1) In which set of elements would all members be expected to have very similar chemical properties? A) O, S, Se B) N, O, F C) Na, Mg, K D) S, Se, Si E) Ne, Na, Mg | back 1 A) O, S, Se |
front 2 2) In which set of elements would all members be expected to have very similar chemical properties? A) P, Se, I B) Cl, Br, Na C) Si, As, Te D) Ne, Na, Mg E) Br, I, At | back 2 E) Br, I, At |
front 3 3) Electrons in the 1s subshell are much closer to the nucleus in Ar than in He due to the larger ________ in Ar. A) nuclear charge B) paramagnetism C) diamagnetism D) Hund's rule E) azimuthal quantum number | back 3 A) nuclear charge |
front 4 Screening of the nuclear charge by core electrons in atoms is ________. A) less efficient than that by valence electrons B) more efficient than that by valence electrons C) essentially identical to that by valence electrons D) responsible for a general decrease in atomic radius going down a group E) both essentially identical to that by valence electrons and responsible for a general decrease in atomic radius going down a group | back 4 B) more efficient than that by valence electrons |
front 5 5) The effective nuclear charge of an atom is primarily affected by ________. A) inner electrons B) outer electrons C) nuclear charge D) electron distribution E) orbital radial probability | back 5 A) inner electrons |
front 6 6) The atomic radius of main-group elements generally increases down a group because ________. A) effective nuclear charge increases down a group B) effective nuclear charge decreases down a group C) effective nuclear charge zigzags down a group D) the principal quantum number of the valence orbitals increases E) both effective nuclear charge increases down a group and the principal quantum number of the valence orbitals increases | back 6 D) the principal quantum number of the valence orbitals increases |
front 7 7) Atomic radius generally increases as we move ________. A) down a group and from right to left across a period B) up a group and from left to right across a period C) down a group and from left to right across a period D) up a group and from right to left across a period E) down a group; the period position has no effect | back 7 A) down a group and from right to left across a period |
front 8 8) Atomic radius generally decreases as we move ________. A) down a group and from right to left across a period B) up a group and from left to right across a period C) down a group and from left to right across a period D) up a group and from right to left across a period E) down a group; the period position has no effect | back 8 B) up a group and from left to right across a period |
front 9 9) Of the following, which gives the correct order for atomic radius for Mg, Na, P, Si and Ar? A) Mg > Na > P > Si > Ar B) Ar > Si > P > Na > Mg C) Si > P > Ar > Na > Mg D) Na > Mg > Si > P > Ar E) Ar > P > Si > Mg > Na | back 9 D) Na > Mg > Si > P > Ar |
front 10 10) Of the following, which gives the correct order for atomic radius for Ca, K, As, Ge and Kr? A) Ca > K > As > Ge > Kr B) Kr > Ge > As > K > Ca C) Ge > As > Kr > K > Ca D) K > Ca > Ge > As > Kr E) Kr > As > Ge > Ca > K | back 10 D) K > Ca > Ge > As > Kr |
front 11 11) Of the compounds below, ________ has the smallest ionic separation. A) KF B) K2S C) RbCl D) SrBr2 E) RbF | back 11 A) KF |
front 12 12) Which of the following is an isoelectronic series? A) B5-, Si4-, As3-, Te2- B) F-, Cl-, Br-, I- C) S, Cl, Ar, K D) Si2-, P2-, S2-, Cl2- E) O2-, F-, Ne, Na+ | back 12 E) O2-, F-, Ne, Na+ |
front 13 13) Which isoelectronic series is correctly arranged in order of increasing radius? A) K+ < Ca2+ < Ar < Cl- B) Cl- < Ar < K+ < Ca2+ C) Ca2+ < Ar < K+ < Cl- D) Ca2+ < K+ < Ar < Cl- E) Ca2+ < K+ < Cl- < Ar | back 13 D) Ca2+ < K+ < Ar < Cl- |
front 14 14) Of the choices below, which gives the order for first ionization energies? A) Cl > S > Al > Ar > Si B) Ar > Cl > S > Si > Al C) Al > Si > S > Cl > Ar D) Cl > S > Al > Si > Ar E) S > Si > Cl > Al > Ar | back 14 B) Ar > Cl > S > Si > Al |
front 15 15) Of the choices below, which gives the order for first ionization energies? A) Kr > Se > Br > Ga > Ge B) Kr > Br > Se > Ge > Ga C) Ga > Br > Ge > Kr > Se D) Ga > Ge > Se > Br > Kr E) Br > Se > Ga > Kr > Ge | back 15 B) Kr > Br > Se > Ge > Ga |
front 16 16) ________ have the lowest first ionization energies of the groups listed. A) Alkali metals B) Transition elements C) Halogens D) Alkaline earth metals E) Noble gases | back 16 A) Alkali metals |
front 17 17) Which of the following correctly represents the second ionization of aluminum? A) Al+ (g) + e- → Al (g) B) Al (g) → Al+ (g) + e- C) Al- (g) + e- → Al2- (g) D) Al+ (g) + e- → Al2+ (g) E) Al+ (g) → Al2+ (g) + e- | back 17 E) Al+ (g) → Al2+ (g) + e- |
front 18 18) 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) + e- → Al3+ (g) E) Al2+ (g) → Al3+ (g) + e- | back 18 E) Al2+ (g) → Al3+ (g) + e- |
front 19 19) Which of the following correctly represents the second ionization of phosphorus? A) P+ (g) + e- → P2+ (g) B) P (g) → P+ (g) + e- C) P- (g) + e- → P2- (g) D) P+ (g) → P2+ (g) + e- E) P+ (g) + e- → P (g) | back 19 D) P+ (g) → P2+ (g) + e- |
front 20 20) Which equation correctly represents the first ionization of calcium? A) Ca (g) → Ca+ (g) + e- B) Ca (g) → Ca- (g) + e- C) Ca (g) + e- → Ca- (g) D) Ca- (g) → Ca (g) + e- E) Ca+ (g) + e- → Ca (g) | back 20 A) Ca (g) → Ca+ (g) + e- |
front 21 21) Which of the following correctly represents the second ionization of calcium? A) Ca (g) → Ca+ (g) + e- B) Ca+ (g) → Ca2+ (g) + e- C) Ca- (g) + e- → Ca2- (g) D) Ca+ (g) + e- → Ca2+ (g) E) Ca+ (g) + e- → Ca (g) | back 21 B) Ca+ (g) → Ca2+ (g) + e- |
front 22 22) Which of the following correctly represents the second ionization of copper? A) Cu (g) → Cu+ (g) + e- B) Cu+ (g) → Cu2+ (g) + e- C) Cu- (g) + e- → Cu2- (g) D) Cu+ (g) + e- → Cu2+ (g) E) Cu+ (g) + e- → Cu (g) | back 22 B) Cu+ (g) → Cu2+ (g) + e- |
front 23 23) Which ion below has the largest radius? A) Cl- B) K+ C) Br- D) F- E) Na+ | back 23 C) Br- |
front 24 24) Of the following species, ________ has the largest radius. A) Rb+ B) Sr2+ C) Br- D) Kr E) Ar | back 24 C) Br- |
front 25 Consider the following electron configurations to answer the questions that follow: (i)1s2 2s2 2p6 3s1 (ii)1s2 2s2 2p6 3s2 (iii)1s2 2s2 2p6 3s2 3p1 (iv)1s2 2s2 2p6 3s2 3p4 (v)1s2 2s2 2p6 3s2 3p5 25) The electron configuration belonging to the atom with the highest second ionization energy is ________. A) (i) B) (ii) C) (iii) D) (iv) E) (v) | back 25 A) (i) |
front 26 Consider the following electron configurations to answer the questions that follow: (i)1s2 2s2 2p6 3s1 (ii)1s2 2s2 2p6 3s2 (iii)1s2 2s2 2p6 3s2 3p1 (iv)1s2 2s2 2p6 3s2 3p4 (v)1s2 2s2 2p6 3s2 3p5 (26) The electron configuration that belongs to the atom with the lowest second ionization energy is ________. A) (i) B) (ii) C) (iii) D) (iv) E) (v) | back 26 B) (ii) |
front 27 Consider the following electron configurations to answer the questions that follow: (i)1s2 2s2 2p6 3s1 (ii)1s2 2s2 2p6 3s2 (iii)1s2 2s2 2p6 3s2 3p1 (iv)1s2 2s2 2p6 3s2 3p4 (v)1s2 2s2 2p6 3s2 3p5 27) The electron configuration of the atom with the most negative electron affinity is ________. A) (i) B) (ii) C) (iii) D) (iv) E) (v) | back 27 E) (v) |
front 28 Consider the following electron configurations to answer the questions that follow: (i)1s2 2s2 2p6 3s1 (ii)1s2 2s2 2p6 3s2 (iii)1s2 2s2 2p6 3s2 3p1 (iv)1s2 2s2 2p6 3s2 3p4 (v)1s2 2s2 2p6 3s2 3p5 28) The electron configuration of the atom that is expected to have a positive electron affinity is ________. A) (i) B) (ii) C) (iii) D) (iv) E) (v) | back 28 B) (ii) |
front 29 29) Of the following elements, ________ has the most negative electron affinity. A) S B) Cl C) Se D) Br E) I | back 29 B) Cl |
front 30 30) Of the following elements, ________ has the most negative electron affinity. A) P B) Al C) Si D) Cl E) B | back 30 D) Cl |
front 31 31) Of the following elements, ________ has the most negative electron affinity. A) O B) K C) B D) Na E) S | back 31 E) S |
front 32 32) Sodium is much more apt to exist as a cation than is chlorine. This is because ________. A) chlorine is a gas and sodium is a solid B) chlorine has a greater electron affinity than sodium does C) chlorine is bigger than sodium D) chlorine has a greater ionization energy than sodium does E) chlorine is more metallic than sodium | back 32 B) chlorine has a greater electron affinity than sodium does |
front 33 33) Which equation correctly represents the electron affinity of calcium? A) Ca (g) + e- → Ca- (g) B) Ca (g) → Ca+ (g) + e- C) Ca (g) → Ca- (g) + e- D) Ca- (g) → Ca (g) + e- E) Ca+ (g) + e- → Ca (g) | back 33 A) Ca (g) + e- → Ca- (g) |
front 34 34) 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) + 2e- → 2Br- (g) E) Br+ (g) + e- → Br (g) | back 34 B) Br (g) + e- → Br- (g) |
front 35 35) Which of the following correctly represents the electron affinity of phosphorus? A) P (g) → P+ (g) + e- B) P (g) + e- → P- (g) C) P4 (g) + e- → P- (g) D) P4 (g) + 4e- → 4P- (g) E) P+ (g) + e- → P (g) | back 35 B) P (g) + e- → P- (g) |
front 36 36) 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. | back 36 D) adds, negative |
front 37 37) Of the elements below, ________ is the most metallic. A) sodium B) barium C) magnesium D) calcium E) cesium | back 37 E) cesium |
front 38 38) The list that correctly indicates the order of metallic character is ________. A) B > N > C B) F > Cl > S C) Si > P > S D) P > S > Se E) Na > K > Rb | back 38 C) Si > P > S |
front 39 39) The list that correctly indicates the order of metallic character is ________. A) Sr > Ca > Mg B) F > Cl > Br C) C > Ge > Si D) Li > Na > K E) O > Se > S | back 39 A) Sr > Ca > Mg |
front 40 40) Of the elements below, ________ has the highest melting point. A) Ca B) K C) Fe D) Na E) Ba | back 40 C) Fe |
front 41 41) Of the following metals, ________ exhibits multiple oxidation states. A) Al B) Rb C) Mg D) Ni E) Cs | back 41 D) Ni |
front 42 42) Of the following oxides, ________ is the most acidic. A) CaO B) CO2 C) Al2O3 D) Li2O E) Na2O | back 42 B) CO2 |
front 43 43) The acidity of carbonated water is due to the ________. A) presence of sulfur B) reaction of CO2 and H2O C) addition of acid D) nonmetal oxides E) none of the above | back 43 B) reaction of CO2 and H2O |
front 44 44) The element in the periodic table that looks like a metal, is a poor thermal conductor, and acts as an electrical semiconductor is ________. A) Sn B) B C) As D) Si E) Ge | back 44 D) Si |
front 45 45) Transition metals within a period differ mainly in the number of ________ electrons. A) s B) p C) d D) f E) all of the above | back 45 C) d |
front 46 46) Which one of the following compounds would produce an acidic solution when dissolved in water? A) Na2O B) CaO C) MgO D) CO2 E) SrO | back 46 D) CO2 |
front 47 47) Nonmetals can be ________ at room temperature. A) solid, liquid, or gas B) solid or liquid C) solid only D) liquid only E) liquid or gas | back 47 A) solid, liquid, or gas |
front 48 48) Which of the following is not a characteristic of metals? A) acidic oxides B) low ionization energies C) malleability D) ductility E) These are all characteristics of metals. | back 48 A) acidic oxides |
front 49 49) When two elements combine to form a compound, the greater the difference in metallic character between the two elements, the greater the likelihood that the compound will be ________. A) a gas at room temperature B) a solid at room temperature C) metallic D) nonmetallic E) a liquid at room temperature | back 49 B) a solid at room temperature |
front 50 50) Alkaline earth metals ________. A) have the smallest atomic radius in a given period B) form monoanions C) form basic oxides D) exist as triatomic molecules E) form halides with the formula MX | back 50 C) form basic oxides |
front 51 51) Between which two elements is the difference in metallic character the greatest? A) Rb and O B) O and I C) Rb and I D) Li and O E) Li and Rb | back 51 A) Rb and O |
front 52 52) The oxide of which element below can react with hydrochloric acid? A) sulfur B) selenium C) nitrogen D) sodium E) carbon | back 52 D) sodium |
front 53 53) Consider the general valence electron configuration of ns2np5 and the following statements: (i)Elements with this electron configuration are expected to form -1 anions. (ii)Elements with this electron configuration are expected to have large positive electron affinities. (iii)Elements with this electron configuration are nonmetals. (iv)Elements with this electron configuration form acidic oxides. Which statements are true? A) (i) and (ii) B) (i), (ii), and (iii) C) (ii) and (iii) D) (i), (iii,) and (iv) E) All statements are true. | back 53 D) (i), (iii,) and (iv) |
front 54 54) 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 period | back 54 D) the lowest first ionization energies in a period |
front 55 55) This element is more reactive than lithium and magnesium but less reactive than potassium. This element is ________. A) Na B) Rb C) Ca D) Be E) Fr | back 55 A) Na |