Review for Final Exam
1. As you go down a group, the atomic radius of an atom tends to _______. (increase or decrease)
2. Which of the following is a lanthanide?
a. Nickel
b. Silicon
c. Beryllium
d. Cerium
3. How many electrons are there in the outer energy level of a molecule of iodine?
a. 32
b. 8
c. 24
d. 1
4. The law of conservation of mass states that the mass of a compound is
a. less than or equal to the sum of the masses of the reactants
b. less than the sum of the masses of the reactants
c. greater than the sum of the masses of the reactants
d. equal to the sum of the masses of the reactants.
5. Covalent bonds share
a. dipoles
b. ions
c. isotopes
d. electrons
6. Halogens are found in ______________. Alkali metals are found in _____________. Alkaline-earth
metals are found in ____________.
7. List the properties of metals.
8. What is the photoelectric effect?
9. How do you find the average atomic mass of an element?
10. Name an element that is similar in behavior to lithium.
11. Group 13 elements have how many valence electrons?
12. What is the formula for density?
13. If an electron has 8 electrons in its ground state, what is the correct electron configuration for the
element?
14. Which element has the smallest ionization energy?
a. As
b. Bi
c. K
d. Ga
15. What was discovered in the cathode ray tube experiment?
16. There are _________ significant figures in the measurement 3040 mm.
17. When you draw a Lewis dot structure, you must know ____________.
a. the number of valence electrons present
b. the ionization energy of each atom
c. the average atomic mass
d. the atomic radius of each atom
18. Give an example of a quantitative observation.
19. If a measurement is close to an accepted value, it is ___________.
Review for Final Exam
20. If a measurement is close to the same value every time, it is ___________.
21. Write the correct noble-gas notation for electron configuration of an atom of fluorine.
22. Give an example of a qualitative observation.
23. Noble gases have _____ valence electrons, so they fulfill the ___________ rule without bonding.
24. What tool would you use to measure the volume of a liquid in the lab?
25. Write 0.000453 cm in scientific notation.
26. The isotopic symbol for lithium, 73Li, indicates that the atomic number is ______, and the mass
number is ___.
27. The central atom of a Lewis structure generally is the __________ _____________.
28. The two most important characteristics of matter is that it _______ up ________ and has ________.
29. Name a chemical change.
30. Name a physical change.
31. What is the periodic law?
32. ___________ conceived the basic principles of the atomic theory.
33. Modern theory is different from Dalton’s atomic theory because Dalton’s theory states that atoms
cannot be __________.
34. What is a compound?
35. Neutral atoms have the same number of ___________ and ____________.
36. Which of the following is not an example of a molecular formula?
a. NH3
b. H2O
c. O2
d. Ne
37. Which experiment led a scientist to conclude there was a dense region of positive charge in atoms?
Who was the scientist?
38. 0.48 g is the same as ______ kg and _______ mg.
39. Liquids have no definite ________, but they do have definite ________.
40. What is the smallest unit of matter that maintains its chemical identity? What is the smallest unit of
a covalent compound? What is the smallest unit of an ionic compound?
41. Which group on the periodic table contains elements that have the lowest attraction for electrons?
42. How many electrons should most nonmetal elements be surrounded by in a Lewis dot structure?
43. What is the definition of a molecule?
44. Name a piece of equipment that can be safely used to remove hot glassware from heat.
Review for Final Exam
45. Which of these metric units is used to measure mass?
a. cm
b. km
c. g
d. mL
46. Name some properties of metals and nonmetals.
47. Flammable materials should never be dispensed or used near _______.
48. Multiple covalent bonds may occur in atoms of nitrogen, oxygen, or ___________.
49. The mobile electrons surrounding positive ions in metallic bonds are a ___________.
50. The word “atom” means _____________.
51. How many bonds are there in the Lewis structure of PH3?
52. Which element does the below electron configuration represent in its ground state?
1s22s22p63s23p2
53. Which have lower melting points, ionic or covalent compounds?
54. What is the ground state of an atom?
55. What is the correct orbital diagram (also known as orbital notation) for sulfur?
56. Which “block” (s, p, d, or f) are the lanthanides an actinides in?
57. Which of the following is an intensive property?
a. amount of energy
b. volume
c. density
d. mass
58. Which group on the periodic table are the halogens in?
59. Which group are the noble gases in?
60. Which group are the alkali metals in?
61. Which group are the alkaline earth metals in?
62. The electron configuration for F is 1s22s22p5. How many more electrons does it need to satisfy the
octet rule?
63. Draw the correct Lewis structure for hydrogen bromide, HBr.
64. What is the shape of PH3 according to VSEPR theory?
65. Where are the metals, nonmetals, and metalloids on the periodic table?
66. Which group of elements have a full outer energy level when in the ground state?
67. What clothing items should not be worn in a laboratory?
68. What is the distance between corresponding points on adjacent waves called?
69. What is malleability?
Review for Final Exam
70. Do metals or nonmetals usually have more valence electrons?
71. Who was the ancient Greek natural philosopher who first proposed the idea of the atom?
72. Round 0.0338790 g to three significant figures.
73. Which block(s) on the periodic table make up the main group elements?
74. How many electrons are in the outermost shell of an oxygen atom in its ground state?
75. Predict the shape of CO2 using VSEPR theory.
76. Which is not a physical change?
a. heating
b. breaking
c. burning
d. smashing
77. What types of elements are semiconductors?
78. What is the least massive particle in the atom?
79. Malleability and ductility are characteristics of substances with what type of bonds?
80. Which has the greatest atomic radius?
a. Tc
b. Ni
c. Zn
81. Which is an extensive property of matter?
a. boiling point
b. volume
c. density
82. What are the metric units of length, volume, mass, and time?
d. Ra
d. melting point
83. What is a measure of the quantity of matter?
84. What do we use to measure mass in the lab?
85. How many significant figures should we round to when dividing 75.8 by 3.20?
86. What is a statement that can be tested experimentally?
87. Horizontal rows on the periodic table are called __________.
88. Verticle columns in the periodic table are called ___________.
89. Which has the highest electronegativity?
a. Ta
b. O
c. Si
90. What property are the noble gases most known for?
d. Tc
91. Find the density of a sample which has a mass of 85.4 g and a volume of 4.32 cm3.
92. Which “block” are the transition metals in on the periodic table?
93. What is the best choice of footwear for the laboratory?
94. A phosphorus atom has 15 protons and 16 neutrons. What is the mass number?
95. VSEPR theory is used to predict __________.