Unit Two Test Review. Click to get a new slide. Choose your answer, then click to see if you were correct.

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1 Unit Two Test Review Click to get a new slide. Choose your answer, then click to see if you were correct.

2 According to the law of definite proportions, any two samples of water, H2O, A. will be made up of only particles consisting of two atoms of hydrogen and one atom of oxygen. B. will have the same ratio of mass of hydrogen to mass of oxygen. C. will have a 2:1 ratio of mass of hydrogen to mass of oxygen. D. Both (A) and (B) (1)

3 According to the law of definite proportions, any two samples of water, H2O, A. will be made up of only particles consisting of two atoms of hydrogen and one atom of oxygen. B. will have the same ratio of mass of hydrogen to mass of oxygen. C. will have a 2:1 ratio of mass of hydrogen to mass of oxygen. D. Both (A) and (B) (1)

4 The law that states that mass cannot be created or destroyed in ordinary chemical and physical changes is known as the law of A. conservation of mass. B. mass action. C. multiple proportions. D. definite composition. (2)

5 The law that states that mass cannot be created or destroyed in ordinary chemical and physical changes is known as the law of A. conservation of mass. B. mass action. C. multiple proportions. D. definite composition. (2)

6 When two elements combine to form two or more compounds, the mass of one element that combines with a given mass of the other element is in the ratio of small whole numbers. This statement is known as the law of A. conservation of mass. B. mass action. C. multiple proportions. D. definite composition. (3)

7 When two elements combine to form two or more compounds, the mass of one element that combines with a given mass of the other element is in the ratio of small whole numbers. This statement is known as the law of A. conservation of mass. B. mass action. C. multiple proportions. D. definite composition. (3)

8 Which two compounds are examples of the law of multiple proportions? A. FeCl 3 and Fe 2 (SO 4 ) 3 B. O 2 and O 3 C. CO and CO 2 D. FeCl 2 and Fe(NO 3 ) 2 (4)

9 Which two compounds are examples of the law of multiple proportions? A. FeCl 3 and Fe 2 (SO 4 ) 3 B. O 2 and O 3 C. CO and CO 2 D. FeCl 2 and Fe(NO 3 ) 2 (4)

10 The law of multiple proportions can be partly explained by the idea that A. elements can combine in only one way to form compounds. B. whole atoms of the same two elements combine to form different compounds. C. elements in a compound always occur in a 1:1 ratio D. only atoms of the same element can combine. (5)

11 The law of multiple proportions can be partly explained by the idea that A. elements can combine in only one way to form compounds. B. whole atoms of the same two elements combine to form different compounds. C. elements in a compound always occur in a 1:1 ratio D. only atoms of the same element can combine. (5)

12 The observation that the mass of carbon dioxide formed from the reaction of carbon and oxygen equals the combined masses of the carbon and oxygen that reacted supports the law of A. mass action B. multiple proportions C. definite proportions D. conservation of mass. (6)

13 The observation that the mass of carbon dioxide formed from the reaction of carbon and oxygen equals the combined masses of the carbon and oxygen that reacted supports the law of A. mass action B. multiple proportions C. definite proportions D. conservation of mass. (6)

14 An atomic theory based on scientific observations started about A. 400 BCE. B C D (7)

15 An atomic theory based on scientific observations started about A. 400 BCE. B C D (7)

16 Dalton s atomic theory helped explain the law of conservation of mass because is stated that atoms A. could not combine. B. could not be created or destroyed. C. all had the same mass. D. were invisible. (8)

17 Dalton s atomic theory helped explain the law of conservation of mass because is stated that atoms A. could not combine. B. could not be created or destroyed. C. all had the same mass. D. were invisible. (8)

18 Dalton s atomic theory does NOT support which of the following observations? A. Matter is neither created nor destroyed in chemical and physical changes. B. Atoms of most elements are made up of protons, neutrons, and electrons. C. NO and NO 2 are compounds of nitrogen and oxygen. D. Hydrogen atoms differ from oxygen atoms. (9)

19 Dalton s atomic theory does NOT support which of the following observations? A. Matter is neither created nor destroyed in chemical and physical changes. B. Atoms of most elements are made up of protons, neutrons, and electrons. C. NO and NO 2 are compounds of nitrogen and oxygen. D. Hydrogen atoms differ from oxygen atoms. (9)

20 Dalton failed to recognize that substances can exist in the form A. AB B. A 2 B C. A 2 D. AB 2 (10)

21 Dalton failed to recognize that substances can exist in the form A. AB B. A 2 B C. A 2 D. AB 2 (10)

22 From observing that, within a cathode tube, cathode rays could move a paddle wheel placed in their path, J.J. Thomson concluded that A. a magnetic field was produced. B. particles were passing from the cathode to the anode. C. there was a high-pressure gas within the tube. D. atoms are indivisible. (11)

23 From observing that, within a cathode tube, cathode rays could move a paddle wheel placed in their path, J.J. Thomson concluded that A. a magnetic field was produced. B. particles were passing from the cathode to the anode. C. there was a high-pressure gas within the tube. D. atoms are indivisible. (11)

24 The rays produced in a cathode tube in early experiments were A. only affected by magnetic fields. B. only affected by electric fields. C. D. were attracted by the positive electrode. All of the above. (12)

25 The rays produced in a cathode tube in early experiments were A. only affected by magnetic fields. B. only affected by electric fields. C. D. were attracted by the positive electrode. All of the above. (12)

26 The behavior of cathode rays led scientists to conclude that the rays were composed of A. energy. B. positively charged particles. C. negatively charged particles. D. uncharged particles. (13)

27 The behavior of cathode rays led scientists to conclude that the rays were composed of A. energy. B. positively charged particles. C. negatively charged particles. D. uncharged particles. (13)

28 Because cathodes made of different metallic elements produced cathode rays, scientists generalized that A. all atoms have electrons. B. atoms are indivisible. C. atoms carry a positive charge. D. electrons vary in charge. (14)

29 Because cathodes made of different metallic elements produced cathode rays, scientists generalized that A. all atoms have electrons. B. atoms are indivisible. C. atoms carry a positive charge. D. electrons vary in charge. (14)

30 Because most of the alpha particles in Rutherford s gold-foil experiments passed through the foil, he concluded that A. atoms contained no charged particles. B. atoms were mostly empty space. C. electrons formed in the nucleus. D. atoms contained a positively charged, pudding-like material. (15)

31 Because most of the alpha particles in Rutherford s gold-foil experiments passed through the foil, he concluded that A. atoms contained no charged particles. B. atoms were mostly empty space. C. electrons formed in the nucleus. D. atoms contained a positively charged, pudding-like material. (15)

32 Because a few alpha particles were deflected back from the foil in Rutherford s gold-foil experiments, he concluded that the particles were A. striking electrons. B. indivisible. C. repelled by tiny regions of high positive charge. D. magnetic. (16)

33 Because a few alpha particles were deflected back from the foil in Rutherford s gold-foil experiments, he concluded that the particles were A. striking electrons. B. indivisible. C. repelled by tiny regions of high positive charge. D. magnetic. (16)

34 Which of the following descriptions is not a characteristic of the nucleus of an atom? A. positively charged B. contains uncharged particles C. accounts for most of the atom s volume D. accounts for most of the atom s mass (17)

35 Which of the following descriptions is not a characteristic of the nucleus of an atom? A. positively charged B. contains uncharged particles C. accounts for most of the atom s volume D. accounts for most of the atom s mass (17)

36 A neutral atom of Si A. has an atomic number of 29. B. contains a total of 43 electrons, protons, and neutrons. C. contains 15 protons and 14 neutrons. D. Both (A) and (C) (18)

37 A neutral atom of Si A. has an atomic number of 29. B. contains a total of 43 electrons, protons, and neutrons. C. contains 15 protons and 14 neutrons. D. Both (A) and (C) (18)

38 Which of the following atoms contains the most neutrons? 43 A. Ca 20 B. 45 Sc C. Ti D. Cr (19)

39 Which of the following atoms contains the most neutrons? 43 A. Ca 20 B. 45 Sc C. Ti D. Cr (19)

40 Each of the three isotopes of hydrogen, hydrogen-1, hydrogen-2, and hydrogen-3, A. contains one neutron and one proton. B. contains at least one neutron. C. has one proton in its nucleus. D. is equally abundant. (20)

41 Each of the three isotopes of hydrogen, hydrogen-1, hydrogen-2, and hydrogen-3, A. contains one neutron and one proton. B. contains at least one neutron. C. has one proton in its nucleus. D. is equally abundant. (20)

42 Which of the following atomic models could be referred to as the solar-system model of the atom? A. Thomson s plum-pudding model B. Rutherford model C. Bohr model D. quantum model (21)

43 Which of the following atomic models could be referred to as the solar-system model of the atom? A. Thomson s plum-pudding model B. Rutherford model C. Bohr model D. quantum model (21)

44 According to the Bohr model of the atom, which particles are allowed to exist in any one of a number of energy levels? A. electrons B. protons C. neutrons D. both (A) and (B) (22)

45 According to the Bohr model of the atom, which particles are allowed to exist in any one of a number of energy levels? A. electrons B. protons C. neutrons D. both (A) and (B) (22)

46 Which model was developed in an attempt to explain hydrogen s line emission spectrum? A. Thomson s plum-pudding model B. Rutherford model C. Bohr model D. quantum model (23)

47 Which model was developed in an attempt to explain hydrogen s line emission spectrum? A. Thomson s plum-pudding model B. Rutherford model C. Bohr model D. quantum model (23)

48 The line-emission spectrum of an atom is caused by the energies released when electrons A. jump from a lower energy level to a higher energy level. B. jump from a higher energy level to a lower energy level. C. jump from the ground state to an excited state. D. None of the above. (24)

49 The line-emission spectrum of an atom is caused by the energies released when electrons A. jump from a lower energy level to a higher energy level. B. jump from a higher energy level to a lower energy level. C. jump from the ground state to an excited state. D. None of the above. (24)

50 Because excited hydrogen atoms always produced the same line-emission spectrum, scientists concluded that hydrogen A. had no electrons. B. did not release energy. C. released energy of only certain values. D. could only exist in the ground state. (25)

51 Because excited hydrogen atoms always produced the same line-emission spectrum, scientists concluded that hydrogen A. had no electrons. B. did not release energy. C. released energy of only certain values. D. could only exist in the ground state. (25)

52 The flame color produced by heated metal ions is due to electrons that A. jump from a lower energy level to a higher energy level. B. jump from a higher energy level to a lower energy level. C. jump from the ground state to an excited state. D. None of the above. (26)

53 The flame color produced by heated metal ions is due to electrons that A. jump from a lower energy level to a higher energy level. B. jump from a higher energy level to a lower energy level. C. jump from the ground state to an excited state. D. None of the above. (26)

54 If electromagnetic radiation A has a lower frequency that electromagnetic radiation B, then, compared to B A. the wavelength of A is shorter. B. the energy of A is lower. C. A is more particle-like. D. Both (A) and (C). (27)

55 If electromagnetic radiation A has a lower frequency that electromagnetic radiation B, then, compared to B A. the wavelength of A is shorter. B. the energy of A is lower. C. A is more particle-like. D. Both (A) and (C). (27)

56 Quantum number n provides what information regarding the location of electrons in an atom? A. orbital shape B. orbital orientation (tilt) C. electron spin D. energy level (28)

57 Quantum number n provides what information regarding the location of electrons in an atom? A. orbital shape B. orbital orientation (tilt) C. electron spin D. energy level (28)

58 How many orbitals are in a p-sublevel (psubshell)? A. 1 B. 3 C. 5 D. 7 (29)

59 How many orbitals are in a p-sublevel (psubshell)? A. 1 B. 3 C. 5 D. 7 (29)

60 What is the maximum number of electrons that can be located in a d-sublevel (d-subshell)? A. 2 B. 6 C. 10 D. 14 (30)

61 What is the maximum number of electrons that can be located in a d-sublevel (d-subshell)? A. 2 B. 6 C. 10 D. 14 (30)

62 What information does an orbital give us about the location of electrons in an atom? A. The path or orbit of an electron around the nucleus. B. The location of an electron at any given point in time. C. The region of space outside of the nucleus where an electron can be found 90% of the time. D. The direction of spin of an electron. (31)

63 What information does an orbital give us about the location of electrons in an atom? A. The path or orbit of an electron around the nucleus. B. The location of an electron at any given point in time. C. The region of space outside of the nucleus where an electron can be found 90% of the time. D. The direction of spin of an electron. (31)

64 What is the maximum number of electrons that can be located in any one orbital? A. 1 B. 2 C. 6 D. 10 (32)

65 What is the maximum number of electrons that can be located in any one orbital? A. 1 B. 2 C. 6 D. 10 (32)

66 The electron configuration of Al A. 1s 2 2s 2 2p 6 3s 1 3d 2 B. 1s 2 2s 2 2p 5 3s 2 3p 2 C. 1s 2 2s 2 2p 6 3s 2 3p 1 D. [Ne]3s 1 3p 1 3d 1 (33)

67 The electron configuration of Al A. 1s 2 2s 2 2p 6 3s 1 3d 2 B. 1s 2 2s 2 2p 5 3s 2 3p 2 C. 1s 2 2s 2 2p 6 3s 2 3p 1 D. [Ne]3s 1 3p 1 3d 1 (33)

68 The electron configuration of A. 1s 2 2s 2 2p 6 3s 2 3p 6 3d 1 B. [Ar] 4s 1 C. [Kr] 4s 1 D. 1s 2 2s 2 2p 6 3s 3 3p K (34)

69 The electron configuration of A. 1s 2 2s 2 2p 6 3s 2 3p 6 3d 1 B. [Ar] 4s 1 C. [Kr] 4s 1 D. 1s 2 2s 2 2p 6 3s 3 3p K (34)

70 Which of the following orbital diagrams for phosphorus is correct? A. 1s 2s 2p 3s 3p B. 1s 2s 2p 3s 3p C. 1s 2s 2p 3s 3p D. 1s 2s 2p 3s 3p (35)

71 Which of the following orbital diagrams for phosphorus is correct? A. 1s 2s 2p 3s 3p B. 1s 2s 2p 3s 3p C. 1s 2s 2p 3s 3p D. 1s 2s 2p 3s 3p (35)

72 Which of the following pairs of atomic symbols represent isotopes? A. U and U B. P 4 and P C. P and Pb 50 Sn 51 Sb D. and (36)

73 Which of the following pairs of atomic symbols represent isotopes? A. U and U B. P 4 and P C. P and Pb 50 Sn 51 Sb D. and (36)

74 In developing his periodic table, Mendeleev listed on cards each element s name, atomic mass, and A. atomic number. B. electron configuration. C. isotopes. D. properties. (37)

75 In developing his periodic table, Mendeleev listed on cards each element s name, atomic mass, and A. atomic number. B. electron configuration. C. isotopes. D. properties. (37)

76 Mendeleev s periodic table did not always list elements in order of increasing atomic mass because he grouped together elements with similar A. properties. B. atomic numbers. C. densities. D. colors. (38)

77 Mendeleev s periodic table did not always list elements in order of increasing atomic mass because he grouped together elements with similar A. properties. B. atomic numbers. C. densities. D. colors. (38)

78 Mendeleev predicted that the gaps in his periodic table represented A. isotopes. B. radioactive elements. C. permanent gaps. D. undiscovered elements. (39)

79 Mendeleev predicted that the gaps in his periodic table represented A. isotopes. B. radioactive elements. C. permanent gaps. D. undiscovered elements. (39)

80 Moseley s work with X-ray spectral lines led to the discovery of a periodic law based on increasing A. atomic mass. B. isotopes. C. atomic number. D. properties. (40)

81 Moseley s work with X-ray spectral lines led to the discovery of a periodic law based on increasing A. atomic mass. B. isotopes. C. atomic number. D. properties. (40)

82 An electron that is found in the outermost shell of an atom and determines the atom s chemical properties is called a(n) A. paired electron. B. p electron. C. valence electron. D. octave electron. (41)

83 An electron that is found in the outermost shell of an atom and determines the atom s chemical properties is called a(n) A. paired electron. B. p electron. C. valence electron. D. octave electron. (41)

84 The periodic law states that the physical and chemical properties of elements are functions of their atomic A. masses. B. numbers. C. radii. D. structures. (42)

85 The periodic law states that the physical and chemical properties of elements are functions of their atomic A. masses. B. numbers. C. radii. D. structures. (42)

86 Refer to a periodic table. In which period is calcium? A. Period 2 B. Period 3 C. Period 4 D. Period 5 (43)

87 Refer to a periodic table. In which period is calcium? A. Period 2 B. Period 3 C. Period 4 D. Period 5 (43)

88 Refer to a periodic table. In which group is calcium? A. Group 1 (1A) B. Group 2 (2A) C. Group 17 (7A) D. Group 18 (8A) (44)

89 Refer to a periodic table. In which group is calcium? A. Group 1 (1A) B. Group 2 (2A) C. Group 17 (7A) D. Group 18 (8A) (44)

90 An element that has the electron configuration [Ne]3s 2 3p 5 is in which period? A. Period 2 B. Period 3 C. Period 5 D. Period 7 (45)

91 An element that has the electron configuration [Ne]3s 2 3p 5 is in which period? A. Period 2 B. Period 3 C. Period 5 D. Period 7 (45)

92 An element that has the electron configuration [Ne]3s 2 3p 5 is in which group? A. Group 2 (2A) B. Group 5 (5A) C. Group 7 (7B) D. Group 17 (7A) (46)

93 An element that has the electron configuration [Ne]3s 2 3p 5 is in which group? A. Group 2 (2A) B. Group 5 (5A) C. Group 7 (7B) D. Group 17 (7A) (46)

94 Elements in the s- or p- blocks of the periodic table are called A. alloys. B. main-group elements. C. metals. D. transition metals. (47)

95 Elements in the s- or p- blocks of the periodic table are called A. alloys. B. main-group elements. C. metals. D. transition metals. (47)

96 Elements in Group 18 (8A) have A. very low reactivity. B. good conductivity. C. very high reactivity. D. metallic character. (48)

97 Elements in Group 18 (8A) have A. very low reactivity. B. good conductivity. C. very high reactivity. D. metallic character. (48)

98 Nonmetallic elements in Group 17 (7A) that react with metals to form salts are A. alkali-metals. B. halogens. C. lanthanides. D. noble gases. (49)

99 Nonmetallic elements in Group 17 (7A) that react with metals to form salts are A. alkali-metals. B. halogens. C. lanthanides. D. noble gases. (49)

100 The outer shell electron configuration of an alkaline-earth metal has A. one electron in the s orbital. B. two electrons in the s orbital. C. one electron in the p orbital. D. two electrons in the p orbital. (50)

101 The outer shell electron configuration of an alkaline-earth metal has A. one electron in the s orbital. B. two electrons in the s orbital. C. one electron in the p orbital. D. two electrons in the p orbital. (50)

102 The alkali metals are found on Earth only in compounds because they A. have small atoms. B. are very reactive elements. C. are rare elements. D. are metallic elements. (51)

103 The alkali metals are found on Earth only in compounds because they A. have small atoms. B. are very reactive elements. C. are rare elements. D. are metallic elements. (51)

104 To which group does hydrogen belong? A. Group 1 (1A) B. Group 2 (2A) C. Group 18 (8A) D. None of the above. (52)

105 To which group does hydrogen belong? A. Group 1 (1A) B. Group 2 (2A) C. Group 18 (8A) D. None of the above. (52)

106 A metal is expected to be a(n) A. nonconductor. B. insulator. C. conductor. D. fluid at room temperature. (53)

107 A metal is expected to be a(n) A. nonconductor. B. insulator. C. conductor. D. fluid at room temperature. (53)

108 An element found in Groups 3 12 (3B 2B) of the periodic table is classified as a(n) A. alkali metal. B. alloy. C. actinide. D. transition metal. (54)

109 An element found in Groups 3 12 (3B 2B) of the periodic table is classified as a(n) A. alkali metal. B. alloy. C. actinide. D. transition metal. (54)

110 An element that has an outer shell electron configuration consisting of two electrons in the s orbital and two electrons in the d orbital is in which group? A. alkali metals. B. alkaline earth metals. C. transition metals. D. halogens. (55)

111 An element that has an outer shell electron configuration consisting of two electrons in the s orbital and two electrons in the d orbital is in which group? A. alkali metals. B. alkaline earth metals. C. transition metals. D. halogens. (55)

112 Lanthanide elements are found in which block of the periodic table? A. s B. p C. d D. f (56)

113 Lanthanide elements are found in which block of the periodic table? A. s B. p C. d D. f (56)

114 In which series of elements do all of the elements undergo radioactive decay? A. Period 5 B. Period 6 C. lanthanides D. actinides (57)

115 In which series of elements do all of the elements undergo radioactive decay? A. Period 5 B. Period 6 C. lanthanides D. actinides (57)

116 Ionization energy is the energy required to remove from an atom of an element. A. the electron cloud. B. all electrons. C. one electron. D. an ion. (58)

117 Ionization energy is the energy required to remove from an atom of an element. A. the electron cloud. B. all electrons. C. one electron. D. an ion. (58)

118 Across a period in the periodic table, ionization energy generally A. decreases. B. decreases then increases. C. increases. D. remains constant. (59)

119 Across a period in the periodic table, ionization energy generally A. decreases. B. decreases then increases. C. increases. D. remains constant. (59)

120 The decrease in ionization energy down a group is due to A. increased electron shielding. B. decreased charge of the nucleus. C. increased distance between the nucleus and valence electrons. D. Both (A) and (C) (60)

121 The decrease in ionization energy down a group is due to A. increased electron shielding. B. decreased charge of the nucleus. C. increased distance between the nucleus and valence electrons. D. Both (A) and (C) (60)

122 When determining the size of an atom by measuring bond radius, the radius of an atom is A. equal to the distance between nuclei. B. one-half the distance between nuclei. C. twice the distance between nuclei. D. one-fourth the distance between nuclei. (61)

123 When determining the size of an atom by measuring bond radius, the radius of an atom is A. equal to the distance between nuclei. B. one-half the distance between nuclei. C. twice the distance between nuclei. D. one-fourth the distance between nuclei. (61)

124 Across a period in the periodic table, atomic radii generally A. decrease. B. decrease, then increase. C. increase. D. increase, then decrease. (62)

125 Across a period in the periodic table, atomic radii generally A. decrease. B. decrease, then increase. C. increase. D. increase, then decrease. (62)

126 Down a group in the periodic table, atomic radii generally A. decrease. B. decrease, then increase. C. increase. D. increase, then decrease. (63)

127 Down a group in the periodic table, atomic radii generally A. decrease. B. decrease, then increase. C. increase. D. increase, then decrease. (63)

128 An element with the lowest electronegativity would be located where in the periodic table? A. Group 1 (1A), Period 7 B. Group 13 (A), Period 4 C. Group 15 (5A), Period 3 D. Group 17 (7A), Period 2 (64)

129 An element with the lowest electronegativity would be located where in the periodic table? A. Group 1 (1A), Period 7 B. Group 13 (A), Period 4 C. Group 15 (5A), Period 3 D. Group 17 (7A), Period 2 (64)

130 An element with the highest electronegativity would be located where in the periodic table? A. Group 1 (1A), Period 7 B. Group 13 (A), Period 4 C. Group 15 (5A), Period 3 D. Group 17 (7A), Period 2 (65)

131 An element with the highest electronegativity would be located where in the periodic table? A. Group 1 (1A), Period 7 B. Group 13 (A), Period 4 C. Group 15 (5A), Period 3 D. Group 17 (7A), Period 2 (65)

132 Refer to a periodic table and determine which element below has the lowest electron affinity. A. Cl B. Se C. Cs D. Te (66)

133 Refer to a periodic table and determine which element below has the lowest electron affinity. A. Cl B. Se C. Cs D. Te (66)

134 As the atomic number of the metals of Group 1 (1A) increases, the ionic radius A. increases. B. decreases. C. remains the same. D. no particular trend is noted. (67)

135 As the atomic number of the metals of Group 1 (1A) increases, the ionic radius A. increases. B. decreases. C. remains the same. D. no particular trend is noted. (67)

136 An element with the smallest anionic (negative-ionic) radius would be located where in the periodic table? A. Group 1(1A), Period 7 B. Group 3 (3B), Period 4 C. Group 15 (5A), Period 3 D. Group 17 (7A), Period 2 (68)

137 An element with the smallest anionic (negative-ionic) radius would be located where in the periodic table? A. Group 1(1A), Period 7 B. Group 3 (3B), Period 4 C. Group 15 (5A), Period 3 D. Group 17 (7A), Period 2 (68)

138 Which of the following elements behaves similarly to calcium? Be able to explain your answer! A. magnesium B. sodium C. sulfur D. chlorine (69)

139 Which of the following elements behaves similarly to calcium? Be able to explain your answer! A. magnesium B. sodium C. sulfur D. chlorine (69)

140 Which of the following elements behaves most like aluminum? Be able to explain your answer! A. boron B. magnesium C. silicon D. gallium (70)

141 Which of the following elements behaves most like aluminum? Be able to explain your answer! A. boron B. magnesium C. silicon D. gallium (70)

142 How many electrons does fluorine have in its outermost shell in its ground state? A. 1 B. 5 C. 7 D. 8 (71)

143 How many electrons does fluorine have in its outermost shell in its ground state? A. 1 B. 5 C. 7 D. 8 (71)

144 How many electrons does the fluoride ion (F 1- ) have in its outermost shell in its ground state? A. 1 B. 5 C. 7 D. 8 (72)

145 How many electrons does the fluoride ion (F 1- ) have in its outermost shell in its ground state? A. 1 B. 5 C. 7 D. 8 (72)

146 Highly reactive metallic elements that react with water to form alkaline solutions are called A. actinides. B. alkali metals. C. halogens. D. noble gases. (73)

147 Highly reactive metallic elements that react with water to form alkaline solutions are called A. actinides. B. alkali metals. C. halogens. D. noble gases. (73)

148 Which of the following properties is NOT periodic, and when graphed versus atomic number would show a continuous upward trend? A. ionization energy B. electronegativity C. atomic mass D. atomic radius (74)

149 Which of the following properties is NOT periodic, and when graphed versus atomic number would show a continuous upward trend? A. ionization energy B. electronegativity C. atomic mass D. atomic radius (74)

150 Compared to a calcium atom, a calcium ion (Ca 2+ ) has A. fewer protons B. fewer electrons C. more electrons D. more protons (75)

151 Compared to a calcium atom, a calcium ion (Ca 2+ ) has A. fewer protons B. fewer electrons C. more electrons D. more protons (75)

152 What is the total charge of the nucleus of a helium atom? A. +4 B. 0 C. +2 D. -2 (76)

153 What is the total charge of the nucleus of a helium atom? A. +4 B. 0 C. +2 D. -2 (76)