5) Which statement correctly describes the relationship of wavelength and frequency in a wave?

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1 Exam 2 Name: Multiple Choice (2 pts each) 1) Which of the following bonds is the most polar? a) C O b) N O c) O O d) Si O 2) The maximum electron capacity of an f sublevel is a) 7 c) 14 b) 6 d) 10 3) Which of the following electromagnetic radiation has the most energy? a) infrared rays b) gamma rays c) X-rays d) ultraviolet rays 4) The correct name for Fe 2 O 3 is a) iron oxide b) diiron trioxide c) Iron (III) oxide d) Iron (II) oxide 5) Which statement correctly describes the relationship of wavelength and frequency in a wave? a) Wavelength is one half of the frequency b) Wavelength is independent of the frequency c) Wavelength increases as frequency decreases d) Wavelength increases as frequency increases 6) The wavelength of the wave shown below is a) 30 cm b) 60 cm c) 80 cm d) 20 cm 1

2 7) Which of the following is the correct electron configuration for Te (Z=52)? a) [Kr] 5s 2 5d 10 5p 4 b) [Kr] 5s 2 5p 6 4d 8 c) [Kr] 5s 2 4d 10 5p 4 d) [Kr] 5s 2 4f 14 8) The number of electrons in an ion of is a) 10 b) 24 c) 12 d) 14 9) Which pair of elements would be expected to form the most polar bond? a) S and Cs b) O and H c) S and Li d) Al and H 10) Which of the following elements has the greatest metallic character? a) Ca c) Kr b) Sr d) Ga 11) The number of neutrons in one atom of 206 Pb is a) 206 b) 124 c) 288 d) 82 12) A given set of p orbitals consists of orbital(s). a) 3 b) 5 c) 1 d) 2 13) The Lewis structure of bromate ion (BrO 3 ) should contain how many electrons? a) 26 b) 25 c) 24 d) 23 2

3 14) Cobalt-60 is a radioactive isotope sometimes used in the treatment of cancer. Which of the following statements is true about an atom of cobalt-60? a) it contains 60 protons b) it contains 33 neutrons c) it contains 33 protons d) it contains 60 neutrons 15) Which of the following is the best notation for the bonding in the molecule ClF? a) Cl=F c) Cl F b) ClΞF d) Cl + F - 16) The number of unpaired electrons in a Ni atom is (are) a) 1 b) 0 c) 2 d) 3 17) What is the molecular shape of NOCl as predicted by VSEPR? a) trigonal planar b) bent c) trigonal pyramidal d) linear 18) Which of the following elements is likely to form an ion with the largest positive charge? a) nitrogen b) potassium c) calcium d) aluminum 19) Which of the following lists elements from the same group? a) C, N, O b) C, Si, Ge c) C, P, Se d) C, Al, As 20) Which of the following molecules has polar bonds but is non-polar? a) NH 3 b) CHCl 3 c) CO 2 d) N 2 3

4 21) Which of the following electromagnetic radiation has the longest wavelength? a) visible b) ultraviolet c) infrared d) radio 22) Which element has the smallest atomic radius? a) Se c) Br b) S d) Cl 23) The mass number of an atom is equal to which of the following? a) the total number of protons and neutrons in the atom b) the total number of protons, neutrons and electrons in the atom c) the number of neutrons in the atom d) the number of protons in the atom 24) Which of the following is an incorrect Lewis structure? a) (a) b) (b) c) (c) d) (d) 25) Naturally occurring copper consists of 2 isotopes: 63 Cu (atomic mass = 62.9 amu) and 65 Cu (atomic mass = 64.9 amu). The average atomic mass of copper is 63.5 amu. What is the natural abundances of these 2 isotopes? a) 20% 63 Cu and 80% 65 Cu b) 30% 63 Cu and 70% 65 Cu c) 50% 63 Cu and 50% 65 Cu d) 70% 63 Cu and 30% 65 Cu 26) Which of the following elements would be in the same group of the periodic table as the element with the electron configuration 1s 2 2s 2 2p 5? a) Ar b) S c) I d) Se 27) Which of the following is named INCORRECTLY? a) Fe 2 (SO 4 ) 3 ; iron (III) sulfate b) Cu 2 O; copper (II) oxide c) SnS 2 ; tin (IV) sulfide d) all are correct 4

5 28) How many protons, electrons and neutrons, respectively, does 127 I have? a) 53, 53, 74 b) 74, 53, 127 c) 53, 53, 127 d) 53, 74, 53 29) The molecular shape of PH 3 is a) trigonal pyramidal b) linear c) bent d) trigonal planar 30) Ca-40, K-39 and Sc-41 all have the same a) number of electrons b) number of neutrons c) atomic number d) atomic mass 31) Which subatomic particle(s) is (are) found in the nucleus? a) electrons b) protons c) neutrons d) Both b and c 32) Which experiment led to the notion that the atom contains an extremely small, positively charged nucleus? a) Thomson s cathode-ray tube experiment b) Dalton s atomic theory c) Millikan s oil drop experiment d) Rutherford s gold-foil experiment 33) Which one of these is the incorrect symbol for the pure form of the compound? a) He 2 b) F 2 c) O 2 d) N 2 5

6 34) Choose the best Lewis structure for CH 2 Cl 2. (a) (b) (c) (d) a) (a) c) (c) b) (b) d) (d) 35) The correct electron configuration for Mn is a) [Ar] 4s 2 3p 5 b) [Ar] 3d 7 c) [Ar] 4s 2 3d 5 d) [Ar] 4s 2 4p 5 36) Which of the following is an incorrect designation for an orbital? a) 1p c) 2s b) 3d d) 4f 37) In becoming a cation, an atom a) loses electrons b) gains electrons c) shares electrons d) gains protons 38) Isotopes of a given element a) have the same atomic number, but different chemical properties b) have the same mass number, but different chemical properties c) have the same number of protons, but different mass number d) have the same mass number, but different number of protons 6

7 39) Select the correct Lewis structure for nitrogen trifluoride, NF 3. a) A b) B c) C d) D (A) (B) (C) (D) 40) Which of the following structures represent isotopes? a) A and B b) A and C c) B and D d) A and D 7

8 Problems (23 Points) 41. Consider 3 elements with the following abbreviated electron configurations: X = [Ar] 4s 2 3d 10 4p 3 Y = [Ar] 4s 2 3d 3 Z = [Ne] 3s 2 3p 3 a) Identify each element as metal, metalloid or nonmetal. X = Y = Z = b) Which elements have similar properties? Explain your reasoning. 42. Which of the following pairs of diagrams is consistent with a chemical reaction according to Dalton s atomic theory? Give a brief explanation for your choice. 8

9 43. For each compound below, write the missing name or formula: a) Cu (NO 3 ) 2 b) Li 2 S c) IF 7 d) Al(OH) 3 e) H 2 CO 3 f) sodium sulfate g) magnesium iodide h) diboron tetroxide i) iron (II) bromide j) silver phosphate 9

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11 TABLE OF ELECTRONEGATIVITIES ELECTROMAGNETIC SPECTURM 11

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