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1 Chemistry Chapter 14 Review Name answer key General Concept Questions 1) is credited with developing the concept of atomic numbers. A) Dmitri Mendeleev B) Lothar Meyer C) Henry Moseley D) Ernest Rutherford E) Michael Faraday 2) Elements in the modern version of the periodic table are arranged in order of increasing. A) oxidation number B) atomic mass C) average atomic mass D) atomic number E) number of isotopes 3) 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 4) Which one of the following is a metalloid? A) Ge B) S C) Br D) Pb E) C 5) Which one of the following is a metal? A) Ge B) S C) Br D) Pb E) C 6) The only noble gas that does not have the ns 2 np 6 valence electron configuration is? A) radon B) neon C) helium D) krypton E) All noble gases have the ns 2 np 6 valence electron configuration.

2 7) To which group on the periodic table does Sulfur belong? A) Noble Gases B) Alkali Metals C) Alkaline Earthe Metals D) Chalgogens E) Halogens 8) The elements in the periodic table that have completely filled shells or subshells are the: A) Transition metals B) Noble gases C) Alkaline Earthe Metals D) Chalgogens E) Halogens 9) What is the atomic number for the element in period 3, group 2? A) 9 B) 10 C) 11 D) 12 E) 13 Z eff and Shielding 10) An electron in a(n) subshell experiences the greatest effective nuclear charge in a many-electron atom. A) 3f B) 3p C) 3d D) 3s E) 4s 11) In which orbital does an electron in a lead atom experience the greatest effective nuclear charge? A) 1s B) 4p C) 5s D) 6s E) 5d 12) In which of the following atoms is the 3s orbital closest to the nucleus? A) Se B) Br C) As D) Ga E) Ge

3 13) What is the shielding constant for Nitrogen? A) 1 B) 2 C) 3 D) 4 14) What is the effective nuclear charge on electrons in the outmost shell for nitrogen? A) 1 B) 2 C) 3 D) 4 E) 5 15) Two elements are studied. One with atomic number X and one with atomic number X+1. It isknown that element X is a Nobel Gas. Which element has the larger shielding constant? A) element X B) element X+1 C) They are both the same D) More information is needed E) There is no way to tell 16) Two elements are studied. One with atomic number X and one with atomic number X+1. Assuming element X is not a Nobel Gas, which element's outer most electrons experience the larger effective nuclear charge? A) element X B) element X+1 C) They are both the same D) More information is needed E) There is no way to tell Atomic Radius 17) Two elements are studied. One with atomic number X and one with atomic number X+1. Assuming element X is not a Nobel Gas, which element has the larger atomic radius? A) element X B) element X+1 C) They are both the same D) More information is needed E) There is no way to tell 18) 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

4 19) Of the following, which is 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 20) Which one of the following atoms has the largest radius? A) O B) F C) S D) Cl E) Ne Ionic Radius and Isoelectric Series 21) Na reacts with element X to form an ionic compound with the formula Na 3 X. Ca will react with X to form. A) CaX 2 B) CaX C) Ca 2 X 3 D) Ca 3 X 2 E) Ca 3 X 22) The most common potassium (K) ion has a charge of. A) 2- B) 1- bb D) 2+ E) potassium does not form ions. 23) is isoelectronic with argon and is isoelectronic with neon. A) Cl -, F - B) Cl -, Cl + C) F+, F - D) Ne -, Kr + E) Ne -, Ar + 24) Which isoelectronic series is correctly arranged in order of increasing radius? A) K + < Ca 2+ < Ar < Cl - B) Cl - < Ar < K + < Ca 2+ C) Ca 2+ < Ar < K + < Cl - D) Ca 2+ < K + < Ar < Cl - E) Ca 2+ < K + < Cl - < Ar

5 Ionization Energy 25) The first ionization energies of the elements as you go from left to right across a period of the periodic table, and as you go from the bottom to the top of a group in the table. A) increase, increase B) increase, decrease C) decrease, increase D) decrease, decrease E) are completely unpredictable 26) 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 27) Of the following atoms, which has the largest first ionization energy? A) Sb B) Se C) As D) S E) Ge 28) Which of the following correctly lists the six elements in order of increasing first ionization energy? A) Li < B < Be < C < O < N B) Li < Be < B < C < O < N C) Li < Be < B < O < C < N D) Li < Be < B < C < N < O E) Li < B < Be < C < N < O 29) Which of the following has the largest second ionization energy? A) Ge B) Ga C) Ca D) K E) Se 30) 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

6 31) Which equation correctly represents the first ionization of aluminum? A) Al - (g) Al (g) + e - B) Al (g) Al - (g) + e - C) Al (g) + e - Al - (g) D) Al (g) Al + (g) + e - E) Al + (g) + e - Al (g) 32) 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 - Al 2- (g) D) Al + (g) + e - Al 2+ (g) E) Al + (g) Al 2+ (g) + e - Electron Affinity 33) The have the most negative electron affinities. A) alkaline earth metals B) alkali metals C) halogens D) transition metals E) chalcogens 34) 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) Metallic Character 35) Of the elements below, is the most metallic. A) sodium B) barium C) magnesium D) calcium E) cesium

7 Reactivity 36) 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 37) 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 38) 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 energies E) alkali metals are not more reactive than alkaline earth metals

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