Chemistry I Final Exam May09
Choose the best answer and mark all selections on your ScanTron with a # 2 lead pencil.
Matter & Change
1. These are 6 unique particles found in the atomic nucleus & held together by nuclear forces.
a. electrons b. neutrons c. protons d. quarks e. both B & C
2. These are found outside the nucleus in clouds or orbitals.
a. electrons b. neutrons c. protons d. quarks e. both B & C
3. The atoms of a(n) _____ are all alike.
a. compound b. element c. heterogeneous mixture d. solution e. substance
4. Physical properties include …
a. state of matter b. density c. magnetism d. A & B e. all above
5. Matter can be classified either as ___ or ___.
a. element; energy b. chemical; synthetic c. compound; solution d. solid; mixture e. substance; mixture
6. Chemical properties include the ability to …
a. corrode b. ignite (burn) c. both A & B d. be magnetic e. all the above
7. Chemical changes include …
a. melting b. magnetizing c. decomposition d. both B & C e. all the above
8. A solution is a …
a. substance b. homogeneous mixture c. heterogeneous mixture d. suspension e. colloid
9. Vertical columns on the periodic table of elements are called …
a. groups b. periods c. blocks d. families e. both a & d
10. Properties of all metals include …
a. malleability b. magnetism c. luster d. all the above e. all except B
11. The ability to be drawn into wires is known as …
a. malleability b. ductility c. luster d. conductivity e. magnetite
12. Metalloids tend to be great …
a. conductors b. insulators c. semiconductors d. radicals e. catalysts
13. The noble gas that can flow uphill is …
a. He b. Ne c. Ar d. Kr e. Xe
Scientific method & measurements
14. Proposed explanation or reason for what is observed based on knowledge from many people & experiments.
a. scientific law b. dependent variable c. hypothesis d. independent variable e. theory
15. You test if Slick50 improves gas mileage. The gas mileage is the ...
a. dependent variable b. hypothesis c. independent variable d. constant e. control
16. You test if Slick50 improves gas mileage. The Slick50 is the ...
a. dependent variable b. hypothesis c. independent variable d. constant e. control
17. The statement, “Slick50 improves gas mileage,” is the ...
a. scientific law b. dependent variable c. hypothesis d. independent variable e. theory
18. Dr. B. tested how 5 different drugs affected growth of cancer cells. Trends found would be best shown in a
a. bar graph b. line graph c. pie chart d. table e. worded document
19. Every time she treated cells, she gave exactly 10 mL of 0.1% EtOH to the cells as she should. This was …
a. accurate b. inaccurate c. imprecise d. precise e. both A & D
20. Chose the correct sequence that has volumes in increasing order (from lowest to highest volumes).
a] pL, mL, dkL, dL b] nL, mL, mL, dL c] mL, dkL, kL, mL d] pL, nL, cL, mL e] mL, nL, cL, mL
21. In scientific notation, the coefficient can be …
a. any whole real # b. any # between 0 & 10 c. any # between 1 & 9.9999 d. any # between 0 & 100
22. In scientific notation, the exponent for the power of 10 is negative if the original # is ...
a. negative b. any # < 10 c. Any # < 1 d. Any # between 0 & 1, exclusive of both e. both A&D
23. Match the SI prefix with its correct value.
a] c- 10-2; dk- 10-1; k- 103 b] c- 10-3; p- 10-12; m- 10-9 c] m- 10-6; m- 10-3; n- 10-9
d] M- 106; p- 10-9; dk- 101 e] n- 10-3; m- 106; d- 101
24. Match the SI prefix with the correct name.
a] c- centi; m- micro; n- nano b] dk- decka; d- deci; m- micro c] dk- deci; d- decka; m- milli
d] M-mega; m- micro; m- milli e] p- pico; m- milli; m- micro
25. A derived SI unit includes …
a. pounds b. liters c. density d. kelvins e. both B & C
26. The number of significant figures in 0.00430 is ...
a. 6 b. 5 c. 4 d. 3 e. 2
27. If one multiplies 12.304 x 10.624 x 420, the answer has ___ significant figures.
a. 2 b. 3 c. 4 d. 5 e. 6
28. If one adds 12.304 + 10.624 + 420, the answer has ___ significant figures.
a. 6 b. 5 c. 4 d. 3 e. 2
Atoms
29. Of the following pairs, the first man first said “atoms” compose all matter, while the 2nd man refuted it.
a. Aristotle/Democritus b. Aristotle/Socrates c. Dalton/Aufbau d. Democritus/Aristotle e. Democritus/Dalton
30. Dalton’s atomic theory is not quite correct because he proposed that atoms are…
a. Building blocks of all matter b. Indivisible particles c. In constant motion
d. Identical & unique for each element e. None of the above
31. The kinetic theory does NOT include this/these basic assumption(s).
a. All matter is composed of small particles. b. These particles are in constant random motion.
c. Small collisions produce some heat. d. Only A & B e. None of the above (all are true)
32. The atomic mass unit (amu) is based on the mass of ...
a. Calcium-20 b. Carbon-12 c. Hydrogen-1 d. Nitrogen-14 e. Oxygen-16
33. The atomic number of elements on the periodic table is always equal to the number of...
a. electrons b. neutrons c. protons d. A + B e. B + C
34. The average atomic mass listed on the periodic table is equal to ...
a. # of electrons b. # of neutrons c. # of protons d. weighted average of all isotopes e. B + C
35. Isotopes of an element have different numbers of ...
a. electrons b. neutrons c. protons d. A or C e. B & C
36. This man proposed that all moles of a pure substance have a constant # of particles.
a. Aufbau b. Avogadro c. Dalton d. Democritus e. Planck
37. ___ said an atomic orbital may describe at most 2 electrons.
a. Aufbau b. Einstein c. Hund d. Pauli e. Rutherford
38. ___ discovered the existence of the positively charged nucleus.
a. Aufbau b. Dalton c. Hund d. Rutherford e. Thomson
39. ___ said that electrons travel around the nucleus in concentric orbitals.
a. Bohr b. Hund c. Heisenburg d. Planck e. de Broglie
40. ___ said that all matter exhibits wave-like properties.
a. Bohr b. Dalton c. de Broglie d. Heisenburg e. Planck
41. ___ said that electrons enter orbitals of lowest energy first.
a. Aufbau b. Dalton c. Heisenburg d. Hund e. Pauli
42. ___ said that electrons travel around the nucleus in concentric orbitals.
a. Bohr b. Hund c. Heisenburg d. Planck e. de Broglie
43. ___ said that it was impossible to know simultaneously both the position & velocity of an electron/ particle.
a. Bohr b. Hund c. Heisenburg d. Planck e. de Broglie
44. The principle quantum number is represented by this letter.
a] l b] m c] n d] p e] s
45. The electron configuration of 1s2 2s2 2px2 2py1 violates whole rule/ principle?
a. Aufbau’s b. Hund’s c. Heisenberg’s d. Pauli’s e. Planck’s
46. The Balmer, Lyman, & Paschen series were derived from this.
a. Bohr’s model b. Heisenberg’s principle c. H’s emission-line spectra d. Schrödinger’s equations
47. The symbol of the element whose electron configuration is 1s2 2s2 2p6 3s2 3p6 4s23d10 4p5 is
a. Br b. Se c. Cl d. I e. Lu
48. Schrödinger was responsible for this/ these contribution(s) to Bohr’s model of orbitals.
a. equations treating electrons as waves b. equations determining location & velocity of electrons
c. the 1st 3 quantum numbers d. both A & C e. both B & C
Periodic Table & Law
49. The current periodic table where elements are ordered according to increasing atomic # was made by ...
a. Dalton b. Democritus c. Einstein d. Mendeleev e. Moseley
50. The ___ group is the most stable of elements.
a. alkali & alkaline earth metals b. transition metals c. nonmetals d. halogens e. noble gases
51. Group __ is the most chemically reactive group of elements in the Periodic Table.
a. One b. Two c. Four d. Six e. Eight
52. Having 7 electrons in the outermost energy level is characteristic of ...
a. alkali metals b. alkaline earth metals c. halogens d. metalloids e. transition metals
53. Elements in which the outermost s & nearby f sublevels generally contain electrons are ...
a. alkali metals b. alkaline earth metals c. inner transition metals d. transition metals e. halogens
54. The element ___ is the most electronegative of any in the Periodic Table.
a. cesium b. fluorine c. francium d. hydrogen e. helium
55. Cations are formed when elements __ electrons.
a. lose b. gain c. both A & B d. share e. exchange
56. Ionization energies decrease as you go __ in the periodic table.
a. down b. up c. down & to the right d. down & to the left e. up & to the left
57. Atomic radii (excluding transition elements) increase as you go ____ the Periodic Table.
a. right & up b. left & up c. right & down d. left & down e. both B & C
Chemical Bonding
58. Compounds &/or molecules are bonded together when electrons are ...
a. gained b. lost c. shared d. all the above e. only A & B
59. The octet rule states that all atoms “want” to be like the ...
a. alkali metals b. metalloids c. noble Gases d. nonmetals e. transition metals
60. Covalent bonds are formed when elements ___electrons.
a. lose b. gain c. both A & B d. share e. exchange
61. Polar bonds are formed when elements unequally __ electrons
a. lose b. gain c. both A & B d. share e. exchange
62. The tendency of atoms to attract electrons when chemically combined with other atoms is ...
a. electronegativity b. ionization energy c. isomerization d. oxidation # e. none above
63. Ionic compounds are typically solids at room temperature with ____ melting points.
a. low b. medium low c. medium d. medium high e. high
64. Diatomic molecules have bonds that are perfectly ...
a. ionic b. nonpolar ionic c. polar ionic d. nonpolar covalent e. polar covalent
65. The geometric shape of a tetrahedral molecule has bond angles of ___ degrees.
a. 105 b. 107 c. 109.5 d. 120 e. 180
66. Water (H2O) has bond angles of ___ degrees.
a. 105 b. 107 c. 109.5 d. 120 e. 180
67. The molecules BF3 and AlCl3 have bond angles of ___ degrees.
a. 105 b. 107 c. 109.5 d. 120 e. 180
68. In a neutral compound/molecule, the sum of the oxidation numbers must ...
a. be positive b. be negative c. either A or B d. equal zero e. either A or D
69. The correct formula for magnesium phosphite is ...
a. MgPO3 b. Mg3 P2 c. MgPO4 d. Mg3(PO4)2 e. Mg3(PO3)2
70. The correct formula for aluminum sulfate is ...
a. AlSO4 b. Al2(SO4)3 c. Al3(SO4)2 d. AlSO3 e. Al2(SO3)3
71. The representative unit of an ionic compound is called a(n) ...
a. molecule b. formula unit c. isotope d. coordination number e. crystal
72. The attraction of free-floating valence electrons for cations is ...
a. ionic bonds b. covalent bonds c. polar bonds d. metallic bonds e. none of the above
73. Formula units are written for __, whereas molecular formulas are written for __
a. crystals; compounds b. compounds; molecules c. molecules; compounds d. crystals; molecules
74. The name for the polyatomic ion C2H3O2 – is ...
a. acetate b. acetylate c. carboxylate d. oxalate e. oxylate
75. Examples of intermolecular forces include __ forces.
a. dipole-dipole b. hydrogen bonding c. London dispersion d. instantaneous dipole e. all above