MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question.

Transcription

1 Exam Name MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) In nature, sulfur is most commonly found in. 1) A) pure elemental sulfur B) H2S C) sulfuric acid D) sulfur oxides E) metal sulfides 2) Hydrogen is unique among the elements because. 1. It is not really a member of any particular group. 2. Its electron is not at all shielded from its nucleus. 3. It is the lightest element. 4. It is the only element to exist at room temperature as a diatomic gas. 5. It exhibits some chemical properties similar to those of groups 1A and 7A. A) 2, 3, 4, 5 B) 1, 2, 3, 4, 5 C) 3, 4 D) 1, 2, 3, 5 E) 1, 4, 5 2) 3) is isoelectronic with argon and is isoelectronic with neon. 3) A) Ne-, Kr+ B) Cl-, F- C) Ne-, Ar+ D) Cl-, Cl+ E) F+, F- 4) Which one of the following atoms has the largest radius? 4) A) S B) O C) Ne D) F E) Cl 5) Which of these oxides is most basic? 5) A) MgO B) K2O C) Na2O D) Al2O3 E) CO2 6) Sodium is much more apt to exist as a cation than is chlorine. This is because. 6) A) chlorine has a greater ionization energy than sodium does B) chlorine has a greater electron affinity than sodium does C) chlorine is more metallic than sodium D) chlorine is a gas and sodium is a solid E) chlorine is bigger than sodium 7) Of the elements below, is the most metallic. 7) A) magnesium B) cesium C) barium D) sodium E) calcium 8) The only noble gas that does not have the ns2np6 valence electron configuration is. 8) A) neon B) krypton C) radon D) helium E) All noble gases have the ns2np6 valence electron configuration. 1

2 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 9) 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) 9) 10) 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), (ii), and (iii) B) (ii) and (iii) C) (i), (iii,) and (iv) D) (i) and (ii) E) All statements are true. 10) 11) is credited with developing the concept of atomic numbers. 11) A) Ernest Rutherford B) Michael Faraday C) Lothar Meyer D) Henry Moseley E) Dmitri Mendeleev 12) Of the elements below, is the most metallic. 12) A) barium B) magnesium C) sodium D) calcium E) cesium 13) Hydrogen is unique among the elements because. 1. It is not really a member of any particular group. 2. Its electron is not at all shielded from its nucleus. 3. It is the lightest element. 4. It is the only element to exist at room temperature as a diatomic gas. 5. It exhibits some chemical properties similar to those of groups 1A and 7A. A) 3, 4 B) 1, 2, 3, 5 C) 1, 2, 3, 4, 5 D) 1, 4, 5 E) 2, 3, 4, 5 13) 14) Between which two elements is the difference in metallic character the greatest? 14) A) Li and Rb B) O and I C) Rb and I D) Li and O E) Rb and O 2

3 15) The first noble gas to be incorporated into a compound was. 15) A) Xe B) He C) Ne D) Kr E) Ar 16) An alkaline earth metal forms a compound with oxygen with the formula. (The symbol M represents any one of the alkaline earth metals.) A) MO2 B) MO3 C) M2O D) MO E) M2O2 16) 17) Sodium is much more apt to exist as a cation than is chlorine. This is because. 17) A) chlorine has a greater ionization energy than sodium does B) chlorine is more metallic than sodium C) chlorine is a gas and sodium is a solid D) chlorine has a greater electron affinity than sodium does E) chlorine is bigger than sodium 18) Which of the following correctly represents the second ionization of aluminum? 18) A) Al+ (g) + e- Al (g) B) Al+ (g) + e- Al2+ (g) C) Al- (g) + e- Al2- (g) D) Al+ (g) Al2+ (g) + e- E) Al (g) Al+ (g) + e- 19) Of the following elements, has the most negative electron affinity. 19) A) K B) B C) S D) Na E) O 20) Of the choices below, which gives the order for first ionization energies? 20) A) Al > Si > S > Cl > Ar B) Cl > S > Al > Si > Ar C) Ar > Cl > S > Si > Al D) Cl > S > Al > Ar > Si E) S > Si > Cl > Al > Ar 21) Which group 6A element is a metal? 21) A) sulfur B) polonium C) tellurium and polonium D) selenium E) tellurium 22) The most common and stable allotrope of sulfur is. 22) A) S2 B) S4 C) S8 D) S E) Sulfur does not form allotropes. 3

4 23) Chlorine is much more apt to exist as an anion than is sodium. This is because. 23) A) chlorine is bigger than sodium B) chlorine is a gas and sodium is a solid C) chlorine has a greater electron affinity than sodium does D) chlorine has a greater ionization energy than sodium does E) chlorine is more metallic than sodium 24) All the elements in group 8A are gases at room temperature. Of all the groups in the periodic table, only group contains examples of elements that are gas, liquid, and solid at room temperature. A) 1A B) 6A C) 5A D) 7A E) 2A 24) 25) Which nonmetal exists as a diatomic solid? 25) A) bromine B) phosphorus C) boron D) antimony E) iodine 26) Of the following oxides, is the most acidic. 26) A) Li2O B) CaO C) Na2O D) CO2 E) Al2O3 27) Of the following elements, has the most negative electron affinity. 27) A) Cl B) B C) Al D) P E) Si 28) Which of the following correctly lists the five atoms in order of increasing size (smallest to largest)? 28) A) F < K < Ge < Br < Rb B) F < Br < Ge < Rb < K C) F < Br < Ge < K < Rb D) F < Ge < Br < K < Rb E) F < K < Br < Ge < Rb 29) Screening by the valence electrons in atoms is. 29) A) more efficient than that by core electrons B) responsible for a general increase in atomic radius going across a period C) essentially identical to that by core electrons D) less efficient than that by core electrons E) both more efficient than that by core electrons and responsible for a general increase in atomic radius going across a period 30) Which one of the following is a metalloid? 30) A) Pb B) Ge C) C D) S E) Br 31) Alkali metals tend to be more reactive than alkaline earth metals because. 31) A) alkali metals have lower melting points B) alkali metals have lower ionization energies C) alkali metals have lower densities D) alkali metals have greater electron affinities E) alkali metals are not more reactive than alkaline earth metals 4

5 32) In general, as you go across a period in the periodic table from left to right: (1) the atomic radius ; (2) the electron affinity becomes negative; and (3) the first ionization energy. A) decreases, decreasingly, increases B) decreases, increasingly, decreases C) increases, increasingly, increases D) decreases, increasingly, increases E) increases, increasingly, decreases 32) 33) Of the following metals, exhibits multiple oxidation states. 33) A) Cs B) V C) Ca D) Al E) Na 34) The reaction of potassium metal with elemental hydrogen produces. 34) A) K2H B) KH2 C) KH D) None of the above; potassium will not react directly with hydrogen. E) KOH 35) Which of the following correctly represents the second ionization of phosphorus? 35) A) P (g) P+ (g) + e- B) P+ (g) + e- P2+ (g) C) P- (g) + e- P2- (g) D) P+ (g) + e- P (g) E) P+ (g) P2+ (g) + e- 36) The noble gases were, until relatively recently, thought to be entirely unreactive. Experiments in the early 1960s showed that Xe could, in fact, form compounds with fluorine. The formation of compounds consisting of Xe is made possible by. A) the stability of xenon atoms B) xenon's relatively low electron affinity C) xenon's noble gas electron configuration D) the availability of xenon atoms E) xenon's relatively low ionization energy 36) 37) Which of the following correctly lists the five atoms in order of increasing size (smallest to largest)? 37) A) O < F < S < Ba < Mg B) F < S < O < Mg < Ba C) O < F < S < Mg < Ba D) F < O < S < Ba < Mg E) F < O < S < Mg < Ba 38) The element(s) could be used to produce a red or crimson color in fireworks. 38) A) Ca, Sr, or Li B) Ba C) Na or K D) Sr E) Mg or Ba 5

6 39) have the lowest first ionization energies of the groups listed. 39) A) Alkali metals B) Noble gases C) Alkaline earth metals D) Transition elements E) Halogens 40) Of the following statements, is not true for oxygen. 40) A) The chemical formula of ozone is O3. B) Dry air is about 79% oxygen. C) Oxygen forms peroxide and superoxide anions. D) Oxygen is a colorless gas at room temperature. E) The most stable allotrope of oxygen is O2. 6