CEM 1211K Test III MULTIPLE COICE. (3 points each) 1) The photoelectric effect is. A) a relativistic effect B) the production of current by silicon solar cells when exposed to sunlight C) the total reflection of light by metals giving them their typical luster D) the darkening of photographic film when exposed to an electric field E) the ejection of electrons by a metal when struck by light 2) Atomic radius generally increases as we move. A) up 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; the period position has no effect D) down a group and from right to left across a period E) down a group and from left to right across a period 3) Which one of the following atoms has the largest radius? A) Ba B) Ca C) Co D) I E) Sr 4) Of the following elements, which has the largest first ionization energy? A) As B) Sb C) Ge D) Se E) S 5) Which equation correctly represents the first ionization of phosphorus? A) P (g) + e - P - (g) B) P (g) P - (g) + e - C) P - (g) P (g) + e - D) P + (g) + e - P (g) E) P (g) P + (g) + e - 6) Which of the following is an isoelectronic series? A) S,, Ar, K B) O 2-, F -, Ne, Na + C) F -, -, Br -, I - D) Si 2-, F 2-, S 2-, 2- E) B 5-, Si 4-, As 3-, Te 2-7) Of the following elements, has the most negative electron affinity. A) Al B) P C) Si D) E) B 8) Which one of the following is a metalloid? A) S B) Ge C) C D) Pb E) Br 9) Which one of the following compounds would produce an acidic solution when dissolved in water? A) Na 2 O B) MgO C) CaO D) SrO E) CO 2 10) Which of the alkali metals can react with oxygen to form a metal peroxide? A) Li and Na B) Li only C) Na, K, Rb, Cs, and Fr D) Cs only E) K, Rb, and Cs
11) Of the hydrogen halides, only is a weak acid. A) F (aq) B) I (aq) C) (aq) D) Br (aq) E) They are all weak acids. 12) Which of the following does not have eight valence electrons? A) Ca + B) Xe C) Br - D) Rb + E) none of these 13) Elements from opposite sides of the periodic table tend to form. A) ionic compounds B) covalent compounds C) compounds that are gaseous at room temperature D) homonuclear diatomic compounds E) covalent compounds that are gaseous at room temperature 14) The type of compound that is most likely to contain a covalent bond is. A) a solid metal B) one that is composed of only nonmetals C) held together by the electrostatic forces between oppositely charged ions D) one that is composed of a metal from the far left of the periodic table and a nonmetal from the far right of the periodic table E) There is no general rule to predict covalency in bonds. 15) Of the atoms below, is the least electronegative. A) Ca B) Rb C) D) Si E) F 16) A nonpolar bond will form between two atoms of electronegativity. A) different, different B) identical, different C) different, opposite D) identical, equal E) similar, different 17) Resonance structures differ by. A) number of atoms only B) number and placement of electrons C) number of electrons only D) placement of atoms only E) placement of electrons only 18) The central atom in violates the octet rule. A) AsF 3 B) SeF 2 C) N 3 D) BF 3 E) CF 4 19) Of the following transitions in the Bohr hydrogen atom, the transition results in the emission of the highest-energy photon. A) n = 6 n = 1 B) n = 1 n = 4 C) n = 6 n = 3 D) n = 3 n = 6 E) n = 1 n = 6
20) The lines in the emission spectrum of hydrogen result from. A) energy given off in the form of visible light when an electron moves from a higher energy state to a lower energy state B) electrons given off by hydrogen when it burns C) protons given off when hydrogen burns D) electrons given off by hydrogen as it cools E) decomposing hydrogen atoms 21) Which one of the following is not a valid value for the magnetic quantum number of an electron in a 5d subshell? A) 2 B) -1 C) 0 D) 1 E) 3 22) Which one of the following is an incorrect subshell notation? A) 4f B) 3d C) 2d D) 3s E) 2p 23) Which sketch represents an orbital with the quantum numbers n = 3, l = 0, and m l = 0? A) B) C) D) E) 24) The ground state electron configuration for Zn is. A) [Ar]4s 2 3d 10 B) [Ar]3s 2 3d 10 C) [Ar]4s 1 3d 10 D) [Kr]4s 2 3d 10 E) [Kr]3s 2 3d 10 25) The electron configuration of the valence electrons of an atom in its ground state is ns 2 np 3. This atom is a group element. A) 2 B) 13 C) 14 D) 15 E) 17
(5 points) Give the electron configurations for the following gas phase atoms: Bromine (Br) 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p 5 or [Ar]4s 2 3d 10 4p 5 Silicon (Si) 1s 2 2s 2 2p 6 3s 2 3p 2 or [Ne]3s 2 3p 2 (10 points) Given the Lewis Structures for the following molecules or polyatomic ions: N 4 + N + SO 2 O S P 5 P
(10 points). Using the table of average bond energies below, the for the reaction is kj. C C + 2 I I C C I Bond D (kj/mol) C=C 839 C-C 348 -I 299 C-I 240 C- 413 Bonds Broken Bonds formed C=C C-C 2 -I 2 C-I 2 C- = [(1mol(839kJ/mol))+(2mol(299kJ/mol))] [(2mol(240kJ/mol))+(2mol(413kJ/mol))=(1mol(348kJ/mol))] = [839kJ + 598kJ] [480kJ + 348kJ + 826kJ] = -217kJ