Multiple Choice Identify the choice that best completes the statement or answers the question.

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1 Chemi1100pretest1 Multiple Choice Identify the choice that best completes the statement or answers the question. 1. Accordingly to the periodic law the properties of elements repeat at regular intervals when the elements are arranged in order of a. their increasing atomic mass. b. their increasing atomic size. c. their increasing number of neutrons in the nucleus. d. their increasing number of isotopes. e. their increasing number of protons in the nucleus. 2. Which electrons have the greatest influence on the properties of elements? a. those electrons in s orbitals b. those electrons in d orbitals c. core electrons d. the outermost electrons e. none of these 3. is a d-transition metal. a. Cr b. Ga c. Sn d. Sb e. Li 4. Which one of the following is an inner transition (f-transition) element? a. Rb b. Ho c. Co d. Ru e. Bi 5. Which of the following is not a representative element? a. Cl b. Sr c. Co d. K e. N 6. What would be the outer electron configuration of group VIA (O, S, Se,...)? a. ns 2 np 6 b. ns 2 np 2 c. ns 2 np 4 d. np 6 e. ns 0 np 6 7. What would be the outer electron configuration of alkaline earth metals? a. ns 2 np 2 b. np 2 c. ns 0 np 2

2 d. nd 2 e. ns 2 8. Choose the term that best describes all members of this series of elements: Xe, Rn, He, Ne, Kr a. metalloids b. noble gases c. alkaline earth metals d. alkali metals e. representative elements 9. Which element has the largest atomic radius? a. Al b. Si c. P d. S e. Cl 10. Arrange the following elements in order of increasing atomic radii. K, Na, Mg, Cs, Cl a. Na < Mg < Cl < K < Cs b. Cl < Mg < Na < K < Cs c. Cs < K < Cl < Mg < Na d. Cl < Mg < Cs < K < Na e. Cl < Mg < Na < Cs < K 11. Which element has the lowest first ionization energy? a. Cs b. Rb c. Ca d. Ba e. Na 12. Which of the following elements has the most negative electron affinity? a. Si b. P c. S d. Se e. Te 13. Which one of the following species is not isoelectronic with neon? a. Mg 2+ b. Na + c. O 2 d. Si 2+ e. Al Which ion has the largest radius? a. Li + b. Na + c. Be 2+

3 d. Mg 2+ e. Al Simple positively charged ions are always than the neutral atoms from which they are formed. a. smaller b. larger c. isoelectronic d. the same size e. more anionic 16. Arrange the following elements in order of decreasing electronegativities. Al, Cs, Mg, Na, P a. P > Al > Mg > Na > Cs b. Cs > Na > Mg > Al > P c. Al > Mg > Na > Cs > P d. P > Al > Mg > Cs > Na e. P > Cs > Na > Mg > Al 17. Which of the following pairs of elements would be expected to form an ionic compound? a. S / F b. H / C c. Rb / Cl d. As / Br e. C / I 18. Which of the following oxides does not give an acidic solution when dissolved in water? a. SO 2 b. CO 2 c. N 2 O 5 d. P 4 O 10 e. Na 2 O 19. An amphoteric compound exhibits a. acidic properties. b. acidic and basic properties. c. metallic properties. d. basic properties. e. ionic properties. 20. Atoms consist of three fundamental particles. What are these particles and their charges? a. proton (+1), neutron (neutral) and electron ( 1) b. proton ( 1), neutron (+1) and electron (neutral) c. proton (+1), neutron ( 1) and electron (neutral) d. proton (neutral), neutron (+1) and electron ( 1) e. proton ( 1), neutron (neutral) and electron (+1) 21. One of the following does not describe solids. Which one is it? a. Particles in definite positions. b. Definite shape. c. Easily compressed. d. Relatively high densities.

4 e. Particles compact. 22. All of the following are properties of antimony. Which one is not a physical property? a. It is a solid at room temperature. b. It has both yellow and gray forms (allotropes) in the solid state. c. It burns in an atmosphere of chlorine. d. It is one of the few substances that expands upon freezing. e. The gray form melts at 631 C. 23. The following statements describe some physical and chemical properties of sucrose (table sugar). Which response includes all that describe chemical properties, and none that describe physical properties? I. It is a colorless solid. II. It chars or blackens when heated gently. III. Its density is 1.6 g/ml. IV. It ignites and burns with a yellow flame when heated strongly. V. It is usually in the form of small crystals although it can occur as a powder. a. I, III, and IV b. II and IV c. II, IV, and V d. I and V e. another combination is the answer 24. Which of the following is not an intensive property of matter? a. color b. density c. melting point d. weight e. boiling point 25. Which response includes all of the following that involve chemical changes, and none that involve physical changes? I. converting milk to cheese II. converting water to steam III. composting leaves IV. burning of gasoline V. melting wax a. II and V b. I, III, and IV c. I, II, and III d. IV and V e. III, IV, and V 26. Which mixture is incorrectly labeled? a. homogeneous / sugar dissolved in water b. homogeneous / sand stirred into water c. heterogeneous / orange juice with pulp d. heterogeneous / chocolate chip cookie e. heterogeneous / concrete sidewalk 27. What is the symbol for the element potassium?

5 a. K b. P c. Pt d. W e. Po 28. Water is always 11.1% hydrogen and 88.9 % oxygen by mass. This is a statement of the a. Law of Conservation of Matter. b. Law of Definite Proportions. c. Law of Multiple Proportions. d. Law of Conservation of Matter and Energy. e. none of these. 29. Below is a list of physical properties and the fundamental unit used in the SI system to measure each. Which unit is not the correct fundamental unit for the property? physical property / unit a. length / meter b. time / second c. mass / gram d. temperature / kelvin e. electric current / ampere 30. Below is a list of common prefixes used in the SI and metric systems. Included with each is an abbreviation and meaning. Which set contains an error? a. mega- M 10 6 b. deci- d 10 1 c. centi- c 10 2 d. micro- m 10 6 e. kilo- k Which of the following is equivalent to 10 cm? a. 1 m b. 0.1 dm c. 100 mm d m e. 1 mm 32. Which of the following numbers has 4 significant figures? a b c d e The sum expressed to the proper number of significant figures is: a. 439 b c d e

6 34. Perform the indicated mathematical operations and express the answer in scientific notation rounded off to the proper number of significant figures: ( ) ( ) = a b c d e If neon atoms (spherical) were laid in a line, each touching the next, the line would measure 2.54 miles. What is the diameter of a neon atom in Å? (1 Å=1x10 10 m) a Å b Å c Å d Å e Å 36. What is the area in square millimeters of a rectangle that is cm long and mm wide? a mm 2 b mm 2 c mm 2 d mm 2 e mm At 25 C, one milliliter of mercury has a mass of 13.6 grams. How many liters of mercury are required to have a mass of 500 kg of mercury? a. 500 L b L c L d L e L 38. A metal cube having a mass of 112 grams is dropped into a graduated cylinder containing ml of water. This causes the water level to rise to ml. What is the density of the cube? a g/ml b g/ml c g/ml d g/ml e g/ml 39. The density of mercury is 13.6 g/cm 3. What is the mass of 6.50 cm 3 of mercury? a g b g c g d g e g 40. Gallium, a metal, has a freezing point near room temperature so it can be melted by holding it in your hands. If gallium's melting point is K, what is that temperature in C?

7 a. 0.0 C b C c C d C e C 41. If a sample of butane, C 4 H 10, contains a total of atoms of carbon, how many molecules of butane are in the sample? a b c d e Each response below lists an ion by name and by chemical symbol or formula. Also each ion is classified as monatomic or polyatomic and as a cation or anion. Which response contains an error? a. hydroxide / OH / monatomic / anion b. carbonate / CO 2 3 / polyatomic / anion c. + ammonium / NH 4 / polyatomic / cation d. magnesium / Mg 2+ / monatomic / cation e. sulfite / SO 2 3 / polyatomic / anion 43. What is the formula for ammonium fluoride? a. AlF b. Al 2 F 3 c. NH 3 F d. NH 4 F 2 e. NH 4 F 44. What is the formula for aluminum oxide? a. Al 2 O 3 b. Ag 2 O 3 c. AlO 3 d. AlO e. AlO Calculate the number of moles of oxygen atoms in 35.2 grams of oxygen. a moles b moles c moles d moles e moles 46. Determine the number of sulfur atoms in 27.1 g of molecular sulfur (S 8 ). a b c d e

8 47. Calculate the formula weight of NaHSO 4. a. 193 amu b. 104 amu c. 120 amu d. 215 amu e. 185 amu 48. What is the mass in grams of water molecules? a g b g c g d g e g 49. Which of the following has no charge? a. nucleus b. neutron c. proton d. electron e. alpha particle 50. In interpreting the results of his "oil drop" experiment in 1909, Robert Millikan was able to determine. a. the charge on a proton b. that electrically neutral particles (neutrons) are present in the nuclei of atoms c. that the masses of protons and neutrons are nearly identical d. the charge on an electron e. the extremely dense nature of the nuclei of atoms 51. In the Rutherford gold foil experiment, the fact that most of the alpha particles were not deflected as they passed through the gold foil indicates that a. the nucleus is positively charged. b. the atom is mostly empty space. c. atoms are solid spheres touching each other in the solid state. d. gold is very dense. e. none of these is correct. 52. The number of electrons in a neutral atom of an element is always equal to the of the element. a. mass number b. atomic number c. atomic mass unit d. isotope number e. Avogadro's number 53. The atomic number of an element gives the number of and in the atom while the mass number gives the total number of and. a. neutrons; protons; neutrons; electrons b. neutrons; electrons; protons; electrons c. neutrons; electrons; neutrons; protons d. protons; electrons; neutrons; electrons e. protons; electrons; neutrons; protons

9 54. Isotopes are atoms of the same element that a. have different numbers of electrons. b. have different numbers of protons. c. have different atomic numbers. d. have different numbers of neutrons. e. have different nuclear charges. 55. Give the number of protons, neutrons, and electrons in an atom of the 90 Sr isotope. a. 38 p; 38 n; 38 e b. 38 p; 90 n; 38 e c. 52 p; 38 n; 52 e d. 38 p; 52 n; 38 e e. 90 p; 38 n; 90 e Chapter 4 Values The following values may be useful for solving some of the problem(s) below. speed of light = m/s 1 joule = 1 kg m 2 /s 2 Planck's constant = J s 1 Ångstrom = m 56. What is the wavelength of yellow light having a frequency of Hz? a m b m c m d m e m 57. What is the energy, in J/photon, of ultraviolet light with a frequency of Hz? a J/photon b J/photon c J/photon d J/photon e J/photon 58. Calculate the energy (J/photon) of a photon of wavelength m. a J b J c J d J e. none of these 59. The Rydberg equation is an empirical equation that describes mathematically. a. the lines in the emission spectrum of hydrogen b. the results of the oil drop experiment c. the results of the cathode ray experiments d. the Bohr model of the atom e. the possible paths of two isotopes of the same element in a mass spectrometer 60. What is the velocity of a neutron of mass kg that has a de Broglie wavelength of 2.05 Å?

10 a. 19 m/s b m/s c m/s d m/s e m/s 61. What statement regarding quantum numbers is false? a. The spin quantum number has values of either +1 or 1. b. The principle quantum number has only integer values. c. The angular momentum quantum number also has letter designations. d. The magnetic quantum number has its values restricted by the l quantum number. e. The magnetic quantum number is represented by m l. 62. Which response lists all the true statements about the four quantum numbers? I. n = principal quantum number, n = 1,2,3,... II. l = angular momentum quantum number, l = 0,1,2,3,..., (n 1) III. m l = magnetic quantum number, m l = 0, 1,..., l IV. m s = spin quantum number, m s = ± a. I, II, and IV b. I, II, and III c. I and III d. II and III e. II, III, and IV 63. The third energy level or shell of an atom can hold a maximum of electrons. a. 8 b. 2 c. 16 d. 18 e Which of the following is not a valid magnetic quantum number for the 3d set of orbitals? a. 1 b. 2 c. 0 d. 2 e What is the value of the angular momentum quantum number, l, for the following orbital? a. b. 1 c. 0 d. 1 e. 2

11 66. All orbitals of a given degenerate set must be singly occupied before pairing begins in that set is a statement of. a. the Heisenberg Uncertainty Principle b. the Bohr Theory c. the Aufbau Principle d. Planck's Theory e. Hund's Rule 67. Which element has the electron configuration below? 1s 2 2s 2 2p 6 3s 2 3p 6 3d 10 4s 2 4p 3 a. V b. Ca c. P d. As e. Se 68. What is the electron configuration of tin, Sn? a. [Kr]5s 2 3d 10 3f 14 5p 4 b. [Kr]5s 2 3d 10 4d 14 5p 4 c. [Kr]5s 2 3d 10 4f 14 5p 2 d. [Kr]5s 2 4d 10 5p 2 e. [Xe]5s 2 4d 10 5p What is the electron configuration of the iron(iii) ion? a. Fe 3+ [Ar]4s 2 3d 3 b. Fe 3+ [Ar]3d 5 c. Fe 2+ [Ar]4s 2 3d 3 d. Fe 2+ [Ar]3d 5 e. Fe 3+ [Kr]3d Which of the following sets of quantum numbers could represent the highest energy electron in V 2+? a. b. c. d. e. n l m l m s Which of the following atoms has the greatest number of unpaired electrons in its ground state? a. Fe b. N c. S d. Ti

12 e. Cu

13 Chemi1100pretest1 Answer Section MULTIPLE CHOICE 1. ANS: E PTS: 1 TOP: More About the Periodic Table 2. ANS: D PTS: 1 TOP: More About the Periodic Table 3. ANS: A PTS: 1 TOP: More About the Periodic Table 4. ANS: B PTS: 1 TOP: More About the Periodic Table 5. ANS: C PTS: 1 TOP: More About the Periodic Table 6. ANS: C PTS: 1 TOP: More About the Periodic Table 7. ANS: E PTS: 1 TOP: More About the Periodic Table 8. ANS: B PTS: 1 TOP: More About the Periodic Table 9. ANS: A PTS: 1 TOP: Atomic Radii 10. ANS: B PTS: 1 TOP: Atomic Radii 11. ANS: A PTS: 1 TOP: Ionization Energy 12. ANS: C PTS: 1 TOP: Electron Affinity 13. ANS: D PTS: 1 TOP: Ionic Radii 14. ANS: B PTS: 1 TOP: Ionic Radii 15. ANS: A PTS: 1 TOP: Ionic Radii 16. ANS: A PTS: 1 TOP: Electronegativity 17. ANS: C PTS: 1 TOP: Electronegativity 18. ANS: E PTS: 1 TOP: Oxygen and the Oxides 19. ANS: B PTS: 1 TOP: Oxygen and the Oxides 20. ANS: A PTS: 1 TOP: Chemistry A Molecular View of Matter 21. ANS: C PTS: 1 TOP: States of Matter 22. ANS: C PTS: 1 TOP: Chemical and Physical Properties 23. ANS: B PTS: 1 TOP: Chemical and Physical Properties 24. ANS: D PTS: 1 TOP: Chemical and Physical Properties 25. ANS: B PTS: 1 TOP: Chemical and Physical Changes 26. ANS: B PTS: 1 TOP: Mixtures, Substances, Compounds, and Elements 27. ANS: A PTS: 1 TOP: Mixtures, Substances, Compounds, and Elements 28. ANS: B PTS: 1 TOP: Mixtures, Substances, Compounds, and Elements 29. ANS: C PTS: 1 TOP: Measurements in Chemistry 30. ANS: D PTS: 1 TOP: Measurements in Chemistry 31. ANS: C PTS: 1 TOP: Measurements in Chemistry 32. ANS: A PTS: 1 TOP: Use of Numbers 33. ANS: B PTS: 1 TOP: Use of Numbers 34. ANS: D PTS: 1 TOP: Use of Numbers 35. ANS: B PTS: 1 TOP: The Unit Factor Method (Dimensional Analysis) 36. ANS: A PTS: 1 TOP: The Unit Factor Method (Dimensional Analysis)

14 37. ANS: E PTS: 1 TOP: The Unit Factor Method (Dimensional Analysis) 38. ANS: B PTS: 1 TOP: Density and Specific Gravity 39. ANS: B PTS: 1 TOP: Density and Specific Gravity 40. ANS: E PTS: 1 TOP: Heat and Temperature 41. ANS: E PTS: 1 TOP: Chemical Formulas 42. ANS: A PTS: 1 TOP: Ions and Ionic Compounds 43. ANS: E PTS: 1 TOP: Names and Formulas of Some Ionic Compounds 44. ANS: A PTS: 1 TOP: Names and Formulas of Some Ionic Compounds 45. ANS: A PTS: 1 TOP: The Mole 46. ANS: C PTS: 1 TOP: The Mole 47. ANS: C PTS: 1 TOP: Formula Weights, Molecular Weights, and Moles 48. ANS: A PTS: 1 TOP: Formula Weights, Molecular Weights, and Moles 49. ANS: B PTS: 1 TOP: Fundamental Particles 50. ANS: D PTS: 1 TOP: The Discovery of Electrons 51. ANS: B PTS: 1 TOP: Rutherford and the Nuclear Atom 52. ANS: B PTS: 1 TOP: Atomic Number 53. ANS: E PTS: 1 TOP: Mass Number and Isotopes 54. ANS: D PTS: 1 TOP: Mass Number and Isotopes 55. ANS: D PTS: 1 TOP: Mass Number and Isotopes 56. ANS: D PTS: 1 TOP: Electromagnetic Radiation 57. ANS: E PTS: 1 TOP: Electromagnetic Radiation 58. ANS: A PTS: 1 TOP: Electromagnetic Radiation 59. ANS: A PTS: 1 TOP: Atomic Spectra and the Bohr Atom 60. ANS: B PTS: 1 TOP: The Wave Nature of the Electron 61. ANS: A PTS: 1 TOP: The Quantum Mechanical Picture of the Atom 62. ANS: A PTS: 1 TOP: Quantum Numbers 63. ANS: D PTS: 1 TOP: Atomic Orbitals 64. ANS: E PTS: 1 TOP: Atomic Orbitals 65. ANS: D PTS: 1 TOP: Atomic Orbitals 66. ANS: E PTS: 1 TOP: Electron Configurations 67. ANS: D PTS: 1 TOP: Electron Configurations 68. ANS: D PTS: 1 TOP: Electron Configurations 69. ANS: B PTS: 1 TOP: Electron Configurations 70. ANS: C PTS: 1 TOP: Electron Configurations 71. ANS: A PTS: 1 TOP: Paramagnetism and Diamagnetism