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AP Chemistry: 2017-18 Semester Review: Chapters 6 Thru 9, 11.2-11.3

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AP Chemistry: 2017-18 Semester Review: Chapters 6 Thru 9, 11.2-11.3 AP Chemistry: 2017-18 Semester Review: MULTIPLE CHOICE Section Chapters 6 thru 9, 11.2-11.3 Chp. 6 1) Which one of the following is correct? A) ν ÷ λ = c B) ν = cλ C) λ = c ν D) νλ = c E) ν + λ = c Page Ref: Sec. 6.1 2) In the Bohr model of the atom, _____. A) electrons travel in circular paths called orbitals B) electron paths are controlled by probability C) electrons can have any energy D) electron energies are quantized E) both A and C Page Ref: Sec. 6.3 3) Which one of the following is an incorrect orbital notation? A) 4dxy B) 3py C) 4s D) 2s E) 3f Page Ref: Sec. 6.5 4) Which electron configuration represents a violation of the Pauli exclusion principle? A) B) C) D) E) Page Ref: Sec. 6.8 1 5) The ground state electron configuration of Ga is __________. A) B) C) D) E) [Ar] Page Ref: Sec. 6.8 6) Which electron configuration represents a violation of Hund's rule for an atom in its ground state? A) B) C) D) E) Page Ref: Sec. 6.8 7) Which two elements have the same ground-state electron configuration? A) Pd and Pt B) Fe and Cu C) Cu and Ag D) Cl and Ar E) No two elements have the same ground-state electron configuration. Page Ref: Sec. 6.8 Chp. 7 1) In which set of elements would all members be expected to have very similar chemical properties? A) O, S, Se B) S, Se, Si C) N, O, F D) Ne, Na, Mg E) Na, Mg, K Page Ref: Sec. 7.1 2) Electrons in the 1s subshell are much closer to the nucleus in Ar than in He due to the larger _____ in Ar. A) diamagnetism B) Hund's rule C) azimuthal quantum number D) nuclear charge E) paramagnetism Page Ref: Sec. 7.2 2 3) Atomic radius generally increases as we move _____. A) down a group; the period position has no effect B) down a group and from right to left 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) up a group and from left to right across a period Page Ref: Sec. 7.2 4) The atomic radius of main-group elements generally increases down a group because _____. A) effective nuclear charge decreases down a group B) effective nuclear charge increases down a group *the effective nuclear charge is the same within a group, C) effective nuclear charge zigzags down a group and increases s across the period. 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 Page Ref: Sec. 7.2 5) Which of the following correctly lists the five atoms in order of increasing size (smallest to largest)? A) O < F < S < Ba < Mg B) F < S < O < Mg < Ba C) F < O < S < Mg < Ba D) O < F < S < Mg < Ba E) F < O < S < Ba < Mg Page Ref: Sec. 7.2 5) Of the following elements, which has the largest first ionization energy? A) Na B) Al C) Se D) Br E) Cl Page Ref: Sec. 7.4 6) Which equation correctly represents the first ionization of phosphorus? A) P – (g) → P (g) + e – B) P (g) + e – → P – (g) C) P (g) → P – (g) + e – D) P (g) → P+ (g) + e – E) P+ (g) + e – → P (g) Page Ref: Sec. 7.4 7) The ion with the smallest diameter is ____. A) Why? It has a greater nuclear charge than the oxide ion with 9 protons and the valence electrons are in the second energy level while the rest of the halides increase the energy levels by one through the group. B) C) D) E) Page Ref: Sec. 7.4 8) ____ is isoelectronic with argon and _____ is isoelectronic with neon. A) , B) , C) , D) , E) F+, F – Page Ref: Sec. 7.3 3 9) Of the following elements, ____ has the most negative electron affinity. (The one that will pay out the largest energy for the electron) A) I B) S C) Se D) Cl E) Br Page Ref: Sec. 7.4 10) Sodium is much more apt to exist as a cation than is chlorine. This is because ____. 10) A) chlorine is bigger than sodium B) chlorine is a gas and sodium is a solid C) chlorine has a greater ionization energy than sodium does D) chlorine is more metallic than sodium E) chlorine has a greater electron affinity than sodium does Page Ref: Sec. 7.4 11) Which of the following correctly represents the electron affinity of bromine? A) Br+ (g) + e – → Br (g) – – B) Br2 (g) + 2 e → 2 Br (g) C) Br (g) + e – → Br – (g) – – D) Br2(g) + e → Br (g) E) Br (g) → Br+ (g) + e – Page Ref: Sec. 7.4 Consider the following electron configurations to answer the questions that follow: (i) 1 2 2 3 (ii) 1 2 2 3 (because it’s almost stable) (iii) 1 2 2 3 3 (iv) 1 2 2 3 3 (v) 1 2 2 3 3 12) 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) Page Ref: Sec. 7.4 13) Of the elements below, _____ is the most metallic. A) calcium B) sodium C) barium D) magnesium E) cesium Page Ref: Sec. 7.5 14) Which one of the following compounds would produce an acidic solution when dissolved in water? A) Na2O B) CaO C) SrO D) MgO E) CO2 Page Ref: Sec. 7.5 4 15) Of the following metals, __________ exhibits multiple oxidation states. A) Na B) Cs C) Al D) Ca E) V Page Ref: Sec. 7.6 16) Which of these oxides is most basic? A) Al2O3 B) Na2O C) CO2 D) MgO E) K2O Page Ref: Sec. 7.6 17) Which of the following is not a characteristic of metals? A) malleability B) acidic oxides C) ductility D) low ionization energies E) These are all characteristics of metals. Page Ref: Sec. 7.6 18) Consider the following properties of an element: (i) It is solid at room temperature. (ii) It easily forms an oxide when exposed to air. (iii) When it reacts with water, hydrogen gas evolves. (iv) It must be stored submerged in oil. Which element fits the above description the best? A) sulfur B) magnesium C) mercury D) sodium E) copper Page Ref: Sec. 7.7 19) Which of the following generalizations cannot be made with regard to reactions of alkali metals? (The symbol M represents any one of the alkali metals.) A) M (s) + O2 (g) → MO2 (s) B) 2M (s) + S (s) → M2S (s) C) 2M (s) + 2 H2O (l) → 2MOH (aq) + H2 (g) D) 2M (s) + H2 (g) → 2MH (s) E) 2M (s) + Cl2 (g) → 2MCl (s) Page Ref: Sec. 7.7 20) All of the following are ionic compounds except __________. A) SiO2 network covalent B) NaCl C) Li3N D) Na2O4 E) K2O Page Ref: Sec. 7.7 21) In nature, the noble gases exist as A) alkali metal salts B) the gaseous fluorides C) monatomic gaseous atoms D) the sulfides E) solids in rocks and in minerals Page Ref: Sec. 7.8 5 Chp. 8 1) Of the ions below, only __________ has a noble gas electron configuration. A) B) C) D) E) Cl – Page Ref: Sec. 8.1 2) The chloride of which of the following metals should have the greatest lattice energy? A) sodium B) lithium C) rubidium D) cesium E) potassium Page Ref: Sec. 8.2 The diagram below is the Born-huber cycle for the formation of crystalline potassium fluoride. 3) Which energy change corresponds to the first ionization energy of potassium? A) 3 B) 2 C) 4 D) 6 E) 5 Page Ref: Sec. 8.2 o 4) Using the Born-Haber cycle, the ΔHf of KBr is equal to ___. o o A) ΔHf K (g)] + ΔHf Br (g)] - I1 - E(Br) + ΔHlattice o o B) ΔHf K (g)] - ΔHf [Br (g)] + I1 (K) - E(Br) + ΔHlattice o o C) ΔHf K (g)] - ΔHf [Br (g)] - I1 (K) - E(Br) - ΔHlattice o o D) ΔHf K (g)] + ΔHf [Br (g)] + I1 (K) + E(Br) + ΔHlattice o o E) ΔHf K (g)] + ΔHf [Br (g)] + I1 (K) + E(Br) - ΔHlattice Page Ref: Sec. 8.2 5) Of the atoms below, ____ is the most electronegative. A) Cl B) S C) Ca D) Si E) Rb Page Ref: Sec. 8.4 6 6) Which of the following has the bonds correctly arranged in order of increasing polarity? A) Mg-F, Be-F, N-F, O-F B) Be-F, Mg-F, N-F, O-F C) O-F, N-F, Be-F, Mg-F D) N-F, Be-F, Mg-F, O-F E) O-F, Be-F, Mg-F, N-F Page Ref: Sec. 8.4 7) Resonance structures differ by ___. A) number of atoms only B) number of electrons only C) placement of electrons only D) number and placement of electrons E) placement of atoms only Page Ref: Sec. 8.6 For the questions that follow, consider the BEST Lewis structures of the following ox_yanions: (i) (ii) (iii) (iv) (v) 8) There can be three equivalent best resonance structures of _____.
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