Honors Physical Science Chapter 19 & 22 Exam Review
Modified True/False
Indicate whether the statement is true or false. If false, change the identified word or phrase to make the statement true.
____ 1. The central core of an atom is called the hub. _________________________
____ 2. The chart showing the classifications of elements according to their properties and increasing atomic numbers is called the periodic table. _________________________
____ 3. The mass of an electron is about equal to the mass of a proton. _________________________
____ 4. Elements arranged in vertical columns in the periodic table are called periods. _________________________
____ 5. The region around the nucleus occupied by the electrons is called the negative zone. _________________________
____ 6. The symbol for chlorine is C. _________________________
____ 7. The maximum number of electrons in the second energy level of an atom is 4. _________________________
____ 8. Two isotopes of carbon are carbon-12 and carbon-14. These isotopes differ from one another by two protons. _________________________
____ 9. Metals are good conductors of heat and electricity. _________________________
____ 10. Scientists believe that naturally occurring elements are manufactured within Mars. _________________________
____ 11. So far, scientists have confirmed the existence of six different quarks. _________________________
____ 12. In 1926, scientists developed the Bohr model of the atom that is in use today. _________________________
____ 13. The sum of the number of protons and neutrons in an atom is the mass number. _________________________
____ 14. The symbol for fluorine is Fe. _________________________
____ 15. A very stable electron arrangement in the outer energy level is characteristic of noble gases. _________________________
____ 16. One proton and one electron are added to each element as you go across the periodic table. _________________________
____ 17. Electron cloud models are used to show how electrons in the outer energy level are bonded when elements combine to form compounds. _________________________
____ 18. The atomic number of an element is determined by its number of protons. _________________________
____ 19. According to present atomic theory, the location of an electron in an atom cannot be pinpointed exactly. _________________________
____ 20. Moving from left to right in a row of the periodic table, metallic properties increase. _________________________
____ 21. The properties of a compound are the same as the properties of the elements making up the compound. _________________________
____ 22. Because a water molecule has a slight positive charge at one end and a slight negative charge at the other end, it is a nonpolar molecule. _________________________
____ 23. Particles formed from the covalent bonding of atoms are called ions. _________________________
____ 24. Molecules are neutral. _________________________
____ 25. A term that means "without water" is anhydrous. _________________________
____ 26. When an atom gains or loses electrons, the charged particle that results is called a molecule. _________________________
____ 27. The formula SO42- stands for ammonium. _________________________
____ 28. An atom is chemically unstable when its outer energy level contains all the electrons it can hold. _________________________
____ 29. The chlorine atoms in hydrogen chloride have a stronger attraction for the electrons than the hydrogen atoms do. The hydrogen chloride molecule is therefore a nonpolar covalent molecule. _________________________
____ 30. An element's oxidation number indicates how many electrons the element must gain, lose, or share to become stable. _________________________
Multiple Choice
Identify the choice that best completes the statement or answers the question.
____ 31. Each inner energy level of an atom has a maximum number of ____ it can hold.
a. | electrons | c. | quarks |
b. | neutrons | d. | protons |
____ 32. Dot diagrams are used to represent ____.
a. | atomic numbers |
b. | atomic mass |
c. | isotopes |
d. | outer level electrons |
____ 33. Particles of matter that make up protons and neutrons are ____.
a. | electrons | c. | quarks |
b. | isotopes | d. | atoms |
____ 34. A chemical symbol represents the ____ of an element.
a. | name | c. | group |
b. | reaction | d. | structure |
____ 35. Horizontal rows of the periodic table are called ____.
a. | clusters | c. | groups |
b. | families | d. | periods |
____ 36. Atoms of the same element with different numbers of neutrons are called ____.
a. | isotopes | c. | metalloids |
b. | metals | d. | radioactive elements |
____ 37. A particle that moves around the nucleus is a(n) ____.
a. | electron | c. | neutron |
b. | proton | d. | quark |
____ 38. Elements that are gases, are brittle, and are poor conductors at room temperature are ____.
a. | metals | c. | metalloids |
b. | nonmetals | d. | isotopes |
____ 39. A ____ is used to accelerate protons in the study of subatomic particles.
a. | tevatron | c. | technology |
b. | termanite | d. | television |
____ 40. A certain atom has 26 protons, 26 electrons, and 30 neutrons. Its mass number is ____.
____ 41. In a chemical formula, the number of each type of atom in the compound is shown by numbers called ____.
a. | superscripts | c. | oxidation numbers |
b. | chemical symbols | d. | subscripts |
____ 42. A group of covalently bonded atoms that acts together as one charged atom is a ____.
a. | crystal | c. | negative ion |
b. | molecule | d. | polyatomic ion |
____ 43. The elements that make up a compound and the exact number of atoms of each element in a unit of the compound can be shown in a ____.
a. | chemical formula | c. | subscript |
b. | chemical symbol | d. | superscript |
____ 44. A chemical bond that occurs when atoms share electrons is a(n) ____ bond.
a. | covalent | c. | magnetic |
b. | ionic | d. | polyatomic |
____ 45. The ____ tells you how many electrons an atom must gain, lose, or share to become stable.
a. | atomic mass | c. | ionic number |
b. | atomic number | d. | oxidation number |
____ 46. The sum of the oxidation numbers in a neutral compound is always ____.
a. | a negative number | c. | a positive number |
b. | one | d. | zero |
____ 47. The oxidation number of an atom is shown with a ____.
a. | negative number | c. | subscript |
b. | positive number | d. | superscript |
____ 48. Which of the following correctly shows the formula for a hydrate?
a. | H2O | c. | MgSO4(H2O)7 |
b. | H2O2 | d. | MgSO4 ´ 7H2O |
____ 49. How many electrons are needed in the outer energy levels of most atoms for the atom to be chemically stable?
____ 50. What kind of chemical bond is formed when an equal exchange of electrons occurs?
a. | covalent | c. | ionic |
b. | hydrate | d. | magnetic |
____ 51. What is the total number of atoms in the compound Ca(ClO3)2?
____ 52. How many hydrogen atoms are present in one molecule of ammonium acetate, NH4C2H3O2?
____ 53. What is the name of the compound with the formula NaCl?
a. | chlorine sodiate | c. | sodium chloride |
b. | sodium chlorate | d. | sodium dichloride |
____ 54. Why do the noble gases NOT form compounds readily?
a. | They have empty outer energy levels. |
b. | They have no electrons. |
c. | They have seven electrons in the outer energy levels. |
d. | Their outer energy levels are completely filled with electrons. |
____ 55. What is the number of potassium atoms compared to oxygen atoms in a binary compound made from these two elements?
a. | One potassium atom to two oxygen atoms. |
b. | One potassium atom to three oxygen atoms. |
c. | Two potassium atoms to one oxygen atom. |
d. | Three potassium atoms to one oxygen atom. |
____ 56. What is the name of a binary compound made up of lithium and chlorine?
a. | chlorine lithiate | c. | lithium chloride |
b. | chlorine lithium | d. | lithium chlorate |
____ 57. Which of the following is the correct formula for magnesium nitrate?
a. | MgNO3 | c. | Mg(NO3)2 |
b. | Mg2NO3 | d. | Mg2(NO3)2 |
____ 58. What is the charge of phosphate in K3PO4?
____ 59. What is the correct name for K2SO4?
a. | potassium disulfide | c. | potassium sulfide |
b. | potassium sulfate | d. | potassium(II) sulfate |
____ 60. What is the correct formula for magnesium oxide?
Short Answer
61. Explain why the noble gases are stable.
62. Why is Ag the symbol for silver?
63. Use the periodic table to find the name, atomic number, and the average atomic mass of the following elements: F, O, P, S.
64. Give the period and group for each of the following elements: F, O, P, S.
65. Who developed the first periodic table?
66. What are the names for the following compounds: CaBr2, CuCl, MgS.
67. What is the formula for each of the following compounds: copper(I) sulfide, calcium chloride, calcium oxide.
68. Which group of elements is the most stable? Explain.
69. What is the name of MgI2?
70. What is the name of PbO2?
Figure 20-1
71. What type of bond is formed in Figure 20-1?
Figure 20-2
72. What type of bond is formed in Figure 20-2?
73. What is the formula for calcium oxide?
74. What is the formula for magnesium chloride?
Honors Physical Science Chapter 19 & 22 Exam Review
Answer Section
MODIFIED TRUE/FALSE
1. ANS: F, nucleus
PTS: 1 DIF: B OBJ: 1/2 STA: PS2.1 CS3.1
2. ANS: T PTS: 1 DIF: B
OBJ: 3/1 STA: PS2.1 CS3.1
3. ANS: F, neutron
PTS: 1 DIF: B OBJ: 2/1 STA: PS2.1 CS3.1
4. ANS: F, groups
PTS: 1 DIF: B OBJ: 2/1 STA: PS2.1 CS3.1
5. ANS: F, electron cloud
PTS: 1 DIF: B OBJ: 1/4 STA: PS2.1 CS3.1
6. ANS: F, Cl
PTS: 1 DIF: B OBJ: 1/1 STA: PS2.1 CS3.1
7. ANS: F, 8
PTS: 1 DIF: B OBJ: 3/2 STA: PS2.1 CS3.1
8. ANS: F, neutrons
PTS: 1 DIF: B OBJ: 2/2 STA: PS2.1 CS3.1
9. ANS: T PTS: 1 DIF: B
OBJ: 3/3 STA: PS2.1 CS3.1
10. ANS: F, stars
PTS: 1 DIF: B OBJ: 3/1 STA: PS2.1 CS5.1
11. ANS: T PTS: 1 DIF: B
OBJ: 1/2 STA: PS2.1 CS3.1
12. ANS: F, electron cloud
PTS: 1 DIF: B OBJ: 1/3 STA: PS1.1 CS3.1
13. ANS: T PTS: 1 DIF: B
OBJ: 2/1 STA: PS2.1 CS3.1
14. ANS: F, iron
PTS: 1 DIF: B OBJ: 1/1 STA: PS2.1 CS3.1
15. ANS: T PTS: 1 DIF: B
OBJ: 3/2 STA: PS2.1 CS3.1
16. ANS: T PTS: 1 DIF: B
OBJ: 3/1 STA: PS2.1 CS3.1
17. ANS: F, dot diagrams
PTS: 1 DIF: B OBJ: 3/2 STA: PS2.1 CS3.1
18. ANS: T PTS: 1 DIF: B
OBJ: 2/1 STA: PS2.1 CS3.1
19. ANS: T PTS: 1 DIF: B
OBJ: 1/4 STA: PS2.1 CS3.1
20. ANS: F, decrease
PTS: 1 DIF: B OBJ: 3/2 STA: PS2.1 CS3.1
21. ANS: F, different from
PTS: 1 DIF: B OBJ: 1/1 STA: PS2.1 CS1.1
22. ANS: F, polar
PTS: 1 DIF: B OBJ: 2/3 STA: PS2.1 CS1.1
23. ANS: F, molecules
PTS: 1 DIF: B OBJ: 2/1 STA: PS2.1 CS1.1
24. ANS: T PTS: 1 DIF: B
OBJ: 2/1 STA: PS2.1 CS1.1
25. ANS: T PTS: 1 DIF: B
OBJ: 3/3 STA: PS2.1 CS1.1
26. ANS: F, an ion
PTS: 1 DIF: B OBJ: 2/1 STA: PS2.1 CS1.1
27. ANS: F, sulfate
PTS: 1 DIF: B OBJ: 3/2 STA: PS2.1 CS1.1
28. ANS: F, stable
PTS: 1 DIF: B OBJ: 1/3 STA: PS2.1 CS1.1
29. ANS: F, polar covalent
PTS: 1 DIF: A OBJ: 2/3 STA: PS2.1 CS1.1
30. ANS: T PTS: 1 DIF: B
OBJ: 3/1 STA: PS2.1 CS1.1
MULTIPLE CHOICE
31. ANS: A PTS: 1 DIF: B OBJ: 1/4
STA: PS2.1 CS3.1
32. ANS: D PTS: 1 DIF: B OBJ: 3/2
STA: PS5.3 CS3.1
33. ANS: C PTS: 1 DIF: B OBJ: 1/2
STA: PS2.1 CS3.1
34. ANS: A PTS: 1 DIF: B OBJ: 1/1
STA: PS2.1 CS3.1
35. ANS: D PTS: 1 DIF: B OBJ: 3/1
STA: PS2.1 CS3.1
36. ANS: A PTS: 1 DIF: B OBJ: 2/2
STA: PS2.1 CS3.1
37. ANS: A PTS: 1 DIF: B OBJ: 1/4
STA: PS2.1 CS3.1
38. ANS: B PTS: 1 DIF: B OBJ: 3/3
STA: PS2.1 CS3.1
39. ANS: A PTS: 1 DIF: B OBJ: 1/2
STA: PS2.1 CS3.1
40. ANS: D PTS: 1 DIF: B OBJ: 2/3
STA: PS2.1 CS3.1
41. ANS: D PTS: 1 DIF: B OBJ: 1/2
STA: PS2.1 CS1.1
42. ANS: D PTS: 1 DIF: B OBJ: 3/3
STA: PS2.1 CS1.1
43. ANS: A PTS: 1 DIF: B OBJ: 1/2
STA: PS2.1 CS1.1
44. ANS: A PTS: 1 DIF: B OBJ: 2/1
STA: PS2.1 CS1.1
45. ANS: D PTS: 1 DIF: B OBJ: 3/1
STA: PS2.1 CS1.1
46. ANS: D PTS: 1 DIF: B OBJ: 3/1
STA: PS2.1 CS1.1
47. ANS: D PTS: 1 DIF: B OBJ: 3/1
STA: PS2.1 CS1.1
48. ANS: D PTS: 1 DIF: B OBJ: 3/2
STA: PS2.1 CS1.1
49. ANS: D PTS: 1 DIF: B OBJ: 1/3
STA: PS2.1 CS1.1
50. ANS: C PTS: 1 DIF: B OBJ: 2/1
STA: PS2.1 CS1.1
51. ANS: D PTS: 1 DIF: B OBJ: 1/2
STA: PS2.1 CS1.1
52. ANS: B PTS: 1 DIF: B OBJ: 1/2
STA: PS2.1 CS1.1
53. ANS: C PTS: 1 DIF: B OBJ: 3/2
STA: PS2.1 CS1.1
54. ANS: D PTS: 1 DIF: B OBJ: 1/4
STA: PS2.1 CS1.1
55. ANS: C PTS: 1 DIF: B OBJ: 1/2
STA: PS2.1 CS1.1
56. ANS: C PTS: 1 DIF: A OBJ: 3/2
STA: PS2.1 CS1.1
57. ANS: C PTS: 1 DIF: A OBJ: 3/2
STA: PS2.1 CS1.1
58. ANS: B PTS: 1 DIF: A OBJ: 3/2
STA: PS2.1 CS1.1
59. ANS: B PTS: 1 DIF: A OBJ: 3/2
STA: PS2.1 CS1.1
60. ANS: A PTS: 1 DIF: A OBJ: 3/2
STA: PS2.1 CS1.1
SHORT ANSWER
61. ANS:
Their outer energy levels are full.
PTS: 1 DIF: A OBJ: 1/4 STA: PS2.1 CS3.1
62. ANS:
Argentum is Latin for "silver."
PTS: 1 DIF: B OBJ: 1/1 STA: PS2.1 CS3.1
63. ANS:
F, fluorine, 9, 18.998; O, oxygen, 8, 15.999; P, phosphorus, 15, 30.974; S, sulfur, 16, 32.066
PTS: 1 DIF: A OBJ: 3/2 STA: PS1.2 CS2.1
64. ANS:
F, period 2, Group 17; O, period 2, Group 16; P, period 3, Group 15; S, period 3, Group 16
PTS: 1 DIF: A OBJ: 3/2 STA: PS1.2 CS2.1
65. ANS:
Dimitri Mendeleev
PTS: 1 DIF: B OBJ: 3/1 STA: PS1.2 CS2.1
66. ANS:
CaBr2—calcium bromide; CuCl—copper(I) chloride; MgS—magnesium sulfide
PTS: 1 DIF: A OBJ: 3/2 STA: PS2.1 CS1.1
67. ANS:
copper(I) sulfide—Cu2S; calcium chloride—CaCl2; calcium oxide—CaO
PTS: 1 DIF: A OBJ: 3/2 STA: PS2.1 CS1.1
68. ANS:
Group 18, the noble gases, is the most stable group. The elements in this group have outer energy levels that are completely filled.
PTS: 1 DIF: A OBJ: 1/3 STA: PS2.1 CS1.1
69. ANS:
magnesium iodide
PTS: 1 DIF: B OBJ: 3/2 STA: PS2.1 CS1.2
70. ANS:
lead(II) oxide
PTS: 1 DIF: B OBJ: 3/2 STA: PS2.1 CS1.2
71. ANS:
ionic
PTS: 1 DIF: B OBJ: 2/1 STA: PS5.1 CS1.1
72. ANS:
covalent
PTS: 1 DIF: B OBJ: 2/1 STA: PS5.1 CS1.1
73. ANS:
CaO
PTS: 1 DIF: B OBJ: 3/2 STA: PS2.1 CS1.1
74. ANS:
MgCl2
PTS: 1 DIF: B OBJ: 3/2 STA: PS2.1 CS1.1