Chemical Bonds – Ch11 | Atoms to Compounds – Test Bank - Test Bank | Foundations of College Chemistry 15e by Hein Arena by Hein Arena, Willard. DOCX document preview.
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Package Title: Hein Test Bank
Course Title: Hein 15e
Chapter Number: 11
Question Type: Multiple Choice
1) Which of the following statements is true for most atoms?
a) In general, as the atomic radius increases, the first ionization energy increases.
b) In general, as the atomic radius increases, the first ionization energy decreases.
c) In general, as the first ionization energy decreases, the electronegativity increases.
d) No correct answer is given.
Difficulty: hard
Learning Objective 1:
Section Reference 1: Section 11.1
2) Which of the following statements is false?
a) In order for a covalent bond to form, the atomic orbitals of the atoms must overlap.
b) The most common ions for the representative elements can be predicted based on their tendency to attain the same electron configuration of the closest noble gas.
c) Ionization energies show a large decrease when electrons are removed from a noble gas-like configuration.
d) Ionic compounds exist as large aggregates of positive and negative ions.
Difficulty: hard
Learning Objective 1:
Section Reference 1: Section 11.3, 11.4, and11.5
3) Which of the following pairs is incorrectly matched?
Ion | Electron Configuration | |
a | Li+ | 1s2 |
b | Ga+ | 1s22s22p63s23p64s2 |
c |
| 1s22s22p6 |
d |
| 1s22s22p63s23p6 |
Difficulty: medium
Learning Objective 1:
Section Reference 1: Section 11.3
4) Which structure represents the best Lewis structure for O2?
a) 
b) 
c) 
d) 
Difficulty: medium
Learning Objective 1:
Section Reference 1: Section 11.7
5) Choose the best Lewis structure for
.
a) [
]-
b) [ 
]-
c) [ 
]-
d) [ 
]-
Difficulty: hard
Learning Objective 1:
Section Reference 1: Section 11.8
6) As one progresses from top to bottom of a group on the periodic table, atomic radius generally
a) increases.
b) decreases.
c) remains the same.
Difficulty: easy
Learning Objective 1:
Section Reference 1: Section 11.1
7) As one progresses left to right across a period on the periodic table, atomic radius generally
a) increases.
b) decreases.
c) remains the same.
Difficulty: easy
Learning Objective 1:
Section Reference 1: Section 11.1
8) As one progresses from top to bottom of a group on the periodic table, first ionization energy generally
a) increases.
b) decreases.
c) remains the same.
Difficulty: easy
Learning Objective 1:
Section Reference 1: Section 11.1
9) As one progresses left to right across a period on the periodic table, first ionization energy generally
a) increases.
b) decreases.
c) remains the same.
Difficulty: easy
Learning Objective 1:
Section Reference 1: Section 11.1
10) Atoms of the nonmetallic elements generally form ions by
a) gaining electrons, forming positive ions.
b) gaining electrons, forming negative ions.
c) losing electrons, forming positive ions.
d) losing electrons, forming negative ions.
Difficulty: easy
Learning Objective 1:
Section Reference 1: Section 11.3
11) Atoms of the metallic elements generally form ions by
a) gaining electrons, forming positive ions.
b) gaining electrons, forming negative ions.
c) losing electrons, forming positive ions.
d) losing electrons, forming negative ions.
Difficulty: easy
Learning Objective 1:
Section Reference 1: Section 11.3
12) How many valence electrons are present in an atom of carbon in the ground state?
a) 1
b) 2
c) 4
d) 8
Difficulty: medium
Learning Objective 1:
Section Reference 1: Section 11.2
13) How many valence electrons are present in an atom of cesium in the ground state?
a) 1
b) 2
c) 3
d) 7
Difficulty: easy
Learning Objective 1:
Section Reference 1: Section 11.2
14) How many valence electrons are present in an atom of hydrogen in the ground state?
a) 1
b) 2
c) 3
d) 8
Difficulty: medium
Learning Objective 1:
Section Reference 1: Section 11.2
15) What is the total number of electrons present in a Ca+2 ion?
a) 2
b) 18
c) 20
d) 22
Difficulty: easy
Learning Objective 1:
Section Reference 1: Section 11.3
16) What is the total number of valence electrons present in a NH4 + ion?
a) 8
b) 9
c) 10
d) 11
Difficulty: medium
Learning Objective 1:
Section Reference 1: Section 11.7
17) What is the total number of valence electrons present in a NO2- ion?
a) 18
b) 16
c) 24
d) 22
Difficulty: medium
Learning Objective 1:
Section Reference 1: Section 11.7
18) What is the total number of valence electrons present in a PO43- ion?
a) 29
b) 31
c) 32
d) 36
Difficulty: medium
Learning Objective 1:
Section Reference 1: Section 11.7
19) What is the total number of electrons present in a 
ion?
a) 8
b) 10
c) 2
d) 6
Difficulty: easy
Learning Objective 1:
Section Reference 1: Section 11.3
20) When potassium fluoride forms from a potassium atom and a fluorine atom
a) a proton is transferred from the potassium atom to the fluorine atom.
b) a proton is transferred from the fluorine atom to the potassium atom.
c) an electron is transferred from the potassium atom to the fluorine atom.
d) an electron is transferred from the fluorine atom to the potassium atom.
Difficulty: easy
Learning Objective 1:
Section Reference 1: Section 11.3
21) Which element forms an ion that is larger than its atom?
a) lithium
b) calcium
c) chromium
d) nitrogen
Difficulty: medium
Learning Objective 1:
Section Reference 1: Section 11.3
22) Which element forms an ion that is smaller than its atom?
a) lead
b) sulfur
c) oxygen
d) fluorine
Difficulty: medium
Learning Objective 1:
Section Reference 1: Section 11.3
23) A Ca+2 ion has an electron configuration similar to that of
a) neon.
b) argon.
c) krypton.
d) xenon.
Difficulty: easy
Learning Objective 1:
Section Reference 1: Section 11.3
24) An S2– ion has an electron configuration similar to that of
a) chlorine.
b) argon.
c) krypton.
d) selenium.
Difficulty: easy
Learning Objective 1:
Section Reference 1: Section 11.3
25) Alkaline earth metals generally form ions with a charge of
a) +1.
b) +2.
c) –1.
d) –2.
Difficulty: easy
Learning Objective 1:
Section Reference 1: Section 11.3
26) Halogens generally form ions with a charge of
a) +1.
b) +2.
c) –1.
d) –2.
27) Alkali metals generally form ions with a charge of
a) +1.
b) +2.
c) –1.
d) –2.
Difficulty: easy
Learning Objective 1:
Section Reference 1: Section 11.3
28) Elements of Group VA generally form ions with a charge of
a) +5.
b) +3.
c) –2.
d) –3.
Difficulty: easy
Learning Objective 1:
Section Reference 1: Section 11.3
29) Elements of Group 6A generally form ions with a charge of
a) +1.
b) +2.
c) –1.
d) –2.
Difficulty: easy
Learning Objective 1:
Section Reference 1: Section 11.3
30) Given the formula Na3P, what is the formula for lithium and nitrogen?
a) Li N
b) Li3N
c) LiN3
d) Li3P
Difficulty: easy
Learning Objective 1:
Section Reference 1: Section 11.4
31) Given the formula BaS, what is the formula for calcium and oxygen?
a) CaO
b) Ca2O
c) CaO2
d) CaS
Difficulty: easy
Learning Objective 1:
Section Reference 1: Section 11.4
32) Given the formula Sr3P2, what is the formula barium and arsenic?
a) BaAs
b) Ba3AS
c) Ba2As3
d) Ba3As2
Difficulty: easy
Learning Objective 1:
Section Reference 1: Section 11.4
33) Given the formula Cs2O, what is the formula rubidium and sulfur?
a) RbS
b) Rb2S
c) RbS2
d) Rb3S
Difficulty: easy
Learning Objective 1:
Section Reference 1: Section 11.4
34) Given the formula GaP, what is the formula aluminum and nitrogen?
a) AlN
b) Al2N3
c) Al3N2
d) AlN3
Difficulty: easy
Learning Objective 1:
Section Reference 1: Section 11.4
35) Which type of chemical bond involves the transfer of electrons?
a) ionic
b) polar covalent
c) nonpolar covalent
Difficulty: easy
Learning Objective 1:
Section Reference 1: Section 11.3
36) Which type of chemical bond involves the equal sharing of electrons?
a) ionic
b) polar covalent
c) nonpolar covalent
Difficulty: easy
Learning Objective 1:
Section Reference 1: Section 11.6
37) Bonds between which of the following two elements would involve a complete transfer of electrons?
a) C and O
b) K and I
c) H and Br
d) N and H
Difficulty: easy
Learning Objective 1:
Section Reference 1: Section 11.6
38) Which of the following bonds is most polar?
a) O—F
b) N—F
c) O—I
d) C—N
Difficulty: medium
Learning Objective 1:
Section Reference 1: Section 11.6
39) Which of the following bonds is least polar?
a) C—O
b) C—H
c) H—I
d) C—C
Difficulty: easy
Learning Objective 1:
Section Reference 1: Section 11.6
40) As one progresses left to right across a period on the periodic table, electronegativity generally
a) increases.
b) decreases.
c) remains the same.
Difficulty: easy
Learning Objective 1:
Section Reference 1: Section 11.6
41) A bond that is principally ionic will form between
a) sulfur and hydrogen.
b) phosphorus and sulfur.
c) chlorine and iodine.
d) potassium and fluorine.
Difficulty: medium
Learning Objective 1:
Section Reference 1: Section 11.6
42) Which of the following 3rd period elements has the smallest atomic radius?
a) Na
b) Al
c) S
d) Cl
Difficulty: easy
Learning Objective 1:
Section Reference 1: Section 11.1
43) Which of the following elements have the largest atomic radius?
a) N
b) P
c) O
d) S
Difficulty: easy
Learning Objective 1:
Section Reference 1: Section 11.1
44) Which of the following ions has the smallest radius?
a) Be2+
b) Li+
c) O2-
d) F-
Difficulty: hard
Learning Objective 1:
Section Reference 1: Section 11.1
45) Which of the following ions has the largest radius?
a) Mg2+
b) Na+
c) O2-
d) F-
Difficulty: hard
Learning Objective 1:
Section Reference 1: Section 11.1
46) Which one is the correct order of the size of the iodine species?
a) I > I+ > I-
b) I > I- > I+
c) I+ > I- > I
d) I- > I > I+
Difficulty: hard
Learning Objective 1:
Section Reference 1: Section 11.1
47) Which of the following would require the largest amount of energy to remove the second electron?
a) Mg
b) Na
c) Ne
d) F
Difficulty: hard
Learning Objective 1:
Section Reference 1: Section 11.1
48) Which of the following would require the largest amount of energy to remove the second electron?
a) Ca
b) Sr
c) K
d) Ar
Difficulty: hard
Learning Objective 1:
Section Reference 1: Section 11.1
49) In any period, the highest electronegativity is found in a
a) metal.
b) nonmetal.
c) metalloid.
Difficulty: easy
Learning Objective 1:
Section Reference 1: Section 11.6
50) Which of the following would require the largest amount of energy to remove the third electron?
a) Mg
b) Na
c) Al
d) Si
Difficulty: hard
Learning Objective 1:
Section Reference 1: Section 11.1
51) A polar covalent bond will form between which two atoms as shown in the following combinations?
a) beryllium and fluorine
b) hydrogen and chlorine
c) sodium and oxygen
d) fluorine and fluorine
Difficulty: medium
Learning Objective 1:
Section Reference 1: Section 11.6
52) A nonpolar covalent bond will form between which two atoms as shown in the following combinations?
a) potassium and chlorine
b) hydrogen and chlorine
c) sodium and bromine
d) chlorine and chlorine
Difficulty: medium
Learning Objective 1:
Section Reference 1: Section 11.6
53) As the difference in electronegativity between two atoms increases, the polarity of a bond between those two atoms
a) increases.
b) decreases.
c) remains the same.
Difficulty: easy
Learning Objective 1:
Section Reference 1: Section 11.6
54) Which of the following has the smallest ionization energy?
a) Be
b) Ca
c) Sr
d) Ba
Difficulty: easy
Learning Objective 1:
Section Reference 1: Section 11.1
55) In the periodic table, the elements having lowest ionization energy are present in _______.
a) I group
b) IV group
c) VII group
d) VIII group
Difficulty: easy
Learning Objective 1:
Section Reference 1: Section 11.1
56) Which of the following elements has the lowest ionization energy?
a) C
b) N
c) F
d) Ne
Difficulty: easy
Learning Objective 1:
Section Reference 1: Section 11.1
57) The atomic radius generally decreases as we move from left to right across a period because
a) the number of electrons in the atoms decreases from left to right.
b) the number of protons in the nucleus increases from left to right.
c) the sizes of the orbitals in the energy level decreases as we move from left to right.
d) the number of neutrons in the nucleus remains almost constant as we move from left to right.
Difficulty: medium
Learning Objective 1:
Section Reference 1: Section 11.1
58) A Lewis electron dot symbol shows
a) all the electrons in the ground-state of an atom.
b) all the core electrons in the ground-state of an atom.
c) all the valence electrons in the ground-state of an atom.
d) all the electrons in the outermost sublevel in an atom.
Difficulty: easy
Learning Objective 1:
Section Reference 1: Section 11.2
59) Bond formed between elements with electronegativities 1.2 and 3.0 would be
a) Ionic
b) Non polar covalent
c) Polar covalent
d) Metallic
Difficulty: medium
Learning Objective 1:
Section Reference 1: Section 11.5
60) Which of the following is a nonpolar molecule?
a) H2S
b) CO2
c) HF
d) NH3
Difficulty: medium
Learning Objective 1:
Section Reference 1: Section 11.7
61) Which contains both polar and non-polar bonds?
a) NH4Cl
b) HCN
c) H2O2
d) CH4
Difficulty: hard
Learning Objective 1:
Section Reference 1: Section 11.7
62) Which of the following is a nonpolar molecule?
a) CH4
b) KCl
c) HCl
d) H2O
Difficulty: medium
Learning Objective 1:
Section Reference 1: Section 11.7
63) If the electron pair forming a bond between two atoms A and B is not in the center, then the bond is
a) single bond
b) polar bond
c) non-polar bond
d) ionic bond
Difficulty: medium
Learning Objective 1:
Section Reference 1: Section 11.7
64) What is the number of valence electrons in a chlorine atom in the ground state?
a) 1
b) 2
c) 5
d) 7
Difficulty: easy
Learning Objective 1:
Section Reference 1: Section 11.2
65) What is the total number of valence electrons in a lithium sulfide formula unit?
a) 2
b) 8
c) 7
d) 19
Difficulty: medium
Learning Objective 1:
Section Reference 1: Section 11.3
66) What is the total number of valence electrons in a molecule of carbon dioxide?
a) 24
b) 16
c) 10
d) 12
Difficulty: easy
Learning Objective 1:
Section Reference 1: Section 11.7
67) What is the total number of valence electrons in a molecule of ammonia?
a) 3
b) 24
c) 6
d) 8
Difficulty: easy
Learning Objective 1:
Section Reference 1: Section 11.7
68) Which of the following contains both ionic and covalent bonds?
a) KCl
b) NH3
c) KNO3
d) [NO2]–
Difficulty: easy
Learning Objective 1:
Section Reference 1: Section 11.9
69) The shape of a carbon dioxide molecule is
a) bent.
b) linear.
c) trigonal planar.
d) tetrahedral.
Difficulty: medium
Learning Objective 1:
Section Reference 1: Section 11.10
70) The shape of an ammonia molecule is
a) bent.
b) trigonal planar.
c) pyramidal.
d) linear.
Difficulty: medium
Learning Objective 1:
Section Reference 1: Section 11.10
71) The geometry of electron pairs around the central atom of a water molecule is
a) bent.
b) pyramidal.
c) tetrahedral.
d) linear.
Difficulty: hard
Learning Objective 1:
Section Reference 1: Section 11.10
72) The shape of a boron trifluoride molecule is
a) pyramidal.
b) trigonal planar.
c) tetrahedral.
d) linear.
Difficulty: medium
Learning Objective 1:
Section Reference 1: Section 11.10
73) Which is not a linear molecule?
a) CO2
b) C2H2
c) SO2
d) BeH2
Difficulty: medium
Learning Objective 1:
Section Reference 1: Section 11.10
74) Which of the following molecules contain one lone pair of electrons on the central atom?
a) CH4
b) NH3
c) CCl4
d) H2O
Difficulty: medium
Learning Objective 1:
Section Reference 1: Section 11.10
75) The shape of a carbon tetrachloride molecule is
a) pyramidal.
b) trigonal planar.
c) bent.
d) tetrahedral.
Difficulty: medium
Learning Objective 1:
Section Reference 1: Section 11.10
76) Which one has a trigonal pyramidal structure?
a) CH4
b) NH3
c) H2O
d) CO2
Difficulty: medium
Learning Objective 1:
Section Reference 1: Section 11.10
77) Carbon dioxide is a nonpolar molecule because
a) oxygen is more electronegative than carbon.
b) the two oxygen atoms are bonded to the carbon atom.
c) the individual dipoles of the carbon-oxygen bonds are oriented 180° to each other.
d) the carbon-oxygen bonds are polar covalent.
Difficulty: hard
Learning Objective 1:
Section Reference 1: Section 11.6
78) The shape of AsH3 is
a) trigonal planar
b) linear
c) bent
d) trigonal pyramidal
Difficulty: medium
Learning Objective 1:
Section Reference 1: Section 11.10
79) Which of the following compounds contains a triple bond in its Lewis structure?
a) CO
b) SO2
c) H2S
d) 
Difficulty: medium
Learning Objective 1:
Section Reference 1: Section 11.7
80) Which of the following does not have a noble gas electron configuration?
a) Sc+3
b) Ar
c) O2–
d) K
Difficulty: easy
Learning Objective 1:
Section Reference 1: Section 11.3
81) Which of the following characterizes covalent bonding?
a) formation of ions
b) type of bond normally found between metals and nonmetals
c) loss of electrons
d) formation of true, discrete molecules
Difficulty: easy
Learning Objective 1:
Section Reference 1: Section 11.5
82) A bond with maximum covalent character between non-metallic elements is found
a) between atoms of similar radius
b) between chemically similar atoms
c) between identical atoms
d) between atoms of large electronegativity difference
Difficulty: hard
Learning Objective 1:
Section Reference 1: Section 11.5
83) Which of the following sets of atoms is arranged in order of increasing electronegativity?
a) S, Si, P
b) S, P, Si
c) Si, P, S
d) Si, S, P
Difficulty: medium
Learning Objective 1:
Section Reference 1: Section 11.6
84) Which of the following series is ranked in order of increasing electronegativity?
a) O, S, Se, Te
b) Cl, S, P, Si
c) Sr, Sn, N, O
d) C, Si, P, Se
Difficulty: medium
Learning Objective 1:
Section Reference 1: Section 11.6
85) What is the shape of CO3 2-?
a) bent
b) trigonal pyramidal
c) trigonal planar
d) tetrahedral
Difficulty: medium
Learning Objective 1:
Section Reference 1: Section 11.10
86) Which of the following atoms has the largest radius?
a) Mg
b) Si
c) S
d) Cl
Difficulty: easy
Learning Objective 1:
Section Reference 1: Section 11.1
87) Which of the following atoms has the largest radius?
a) Se
b) Te
c) O
d) S
Difficulty: easy
Learning Objective 1:
Section Reference 1: Section 11.1
88) Which of the following does not have a noble gas electron configuration?
a) S-2
b) Al+3
c) Sb+5
d) Ar
Difficulty: easy
Learning Objective 1:
Section Reference 1: Section 11.3
89) Which of the following does not represent the correct formula for a compound of sodium?
a) NaCl
b) Na2O
c) NaS
d) Na3N
Difficulty: medium
Learning Objective 1:
Section Reference 1: Section 11.4
90) To break a covalent bond, energy must be
a) released.
b) absorbed.
c) both, absorbed and released.
d) neither, absorbed nor released.
Difficulty: easy
Learning Objective 1:
Section Reference 1: Section 11.5
91) The total number of valence electrons in a nitrate ion is
a) 22
b) 23
c) 24
d) 56
Difficulty: easy
Learning Objective 1:
Section Reference 1: Section 11.8
92) Which of the following does not contain a polar covalent bond?
a) CH4
b) H2O
c) CH3OH
d) Cl2
Difficulty: medium
Learning Objective 1:
Section Reference 1: Sections 11.6 and 11.7
93) The molecular shape shown in the following figure is
a) tetrahedral.
b) trigonal pyramidal.
c) bent.
d) trigonal planar.
Difficulty: medium
Learning Objective 1:
Section Reference 1: Section 11.10
94) The molecular shape shown in the following figure is
a) tetrahedral.
b) trigonal pyramidal.
c) bent.
d) trigonal planar.
Difficulty: medium
Learning Objective 1:
Section Reference 1: Section 11.10
95) In the following molecular shape, the bond angles are
a) 180°
b) 120°
c) 90°
d) 109.5°
Difficulty: medium
Learning Objective 1:
Section Reference 1: Section 11.10
96) Ionic bonds will most likely form between
a) two atoms with a high ionization energy.
b) two atoms with a low ionization energy.
c) an atom with a high ionization energy and an atom with a low ionization energy.
d) no correct answer is given.
Difficulty: hard
Learning Objective 1:
Section Reference 1: Section 11.3
97) The most predominantly ionic compound will be obtained from the combination of elements belonging to
a) IA and VIIA groups.
b) IIA and VIA groups.
c) IIIA and VA groups.
d) VIIA and VIIIA groups.
Difficulty: medium
Learning Objective 1:
Section Reference 1: Section 11.3
98) Covalent bonds will most likely form between
a) two atoms with a high ionization energy.
b) two atoms with a low ionization energy.
c) an atom with a high ionization energy and an atom with a low ionization energy.
d) no correct answer is given.
Difficulty: hard
Learning Objective 1:
Section Reference 1: Section 11.5
Question Type: True/False
99) The Ca+2 ion is larger than the Ca atom.
Difficulty: easy
Learning Objective 1:
Section Reference 1: Section 11.3
100) The Cl atom is larger than the Cl– ion
Difficulty: easy
Learning Objective 1:
Section Reference 1: Section 11.3
101) The element with the lowest electronegativity is fluorine.
Difficulty: easy
Section Reference 1: Section 11.6
102) The first ionization energy is the energy released when an atom gains an electron.
Difficulty: easy
Learning Objective 1:
Section Reference 1: Section 11.1
103) The Lewis-dot symbol for nitrogen is: N x
Difficulty: easy
Learning Objective 1:
Section Reference 1: Section 11.2
104) The series Ba, Cs, P, and O is arranged by decreasing atomic size.
Difficulty: medium
Learning Objective 1:
Section Reference 1: Section 11.1
105) The series Cl, As, Sb, In is arranged by increasing ionization energy.
Difficulty: medium
Learning Objective 1:
Section Reference 1: Section 11.1
106) The series, F, Cl, P, and K is arranged in order of decreasing electronegativity.
Difficulty: medium
Learning Objective 1:
Section Reference 1: Section 11.6
107) The size of a positive ion is larger than that of the parent atom.
Difficulty: medium
Learning Objective 1:
Section Reference 1: Section 11.1
108) The size of a negative ion is larger than that of the parent atom.
Difficulty: medium
Learning Objective 1:
Section Reference 1: Section 11.1
109) A dipole results from an unequal electron distribution between the atoms in a bond or molecule.
Difficulty: easy
Learning Objective 1:
Section Reference 1: Section 11.6
110) The bond formed between one carbon atom and one oxygen atom is a polar covalent bond.
Difficulty: easy
Learning Objective 1:
Section Reference 1: Section 11.6
Question Type: Essay
111) Arrange the following bonds in order of increasing polarity.
N—O, Br—Cl, C—O, Li—F, I—I
Difficulty: medium
Learning Objective 1:
Section Reference 1: Section 11.6
Solution: Lowest polarity I—I, Br—Cl, N—O, C—O, Li—F Highest polarity
112) Arrange the following bonds in order of increasing polarity.
F—F, N—H, Ca—O, H—O, C—H
Difficulty: medium
Learning Objective 1:
Section Reference 1: Section 11.6
Solution: Lowest polarity F—F, C—H, N—H, H—O, Ca—O Highest polarity
113) Explain how and why the following properties change as you progress from left to right across a period of the periodic table.
a) atomic radius
b) ionization energy
c) electronegativity
Difficulty: medium
Learning Objective 1:
Section Reference 1: Section 11.1
Solution: a) As one progresses from left to right across a period, atomic radius decreases. Each element in a period contains the same number of electron shells, but each successive element contains one more proton to attract those electron shells. This increasing nuclear charge pulls the electron shells closer and the atomic radius decreases.
b) As one progresses from left to right across a period, the ionization energy increases. Each successive element in a period has a smaller atomic radius and a greater nuclear charge. Both these properties work together to hold the valence electrons more tightly and to make it more difficult to remove them.
c) As one progresses from left to right across a period, electronegativity increases. This occurs because each successive element has a greater nuclear charge to attract electrons and a smaller distance between the nucleus and the valence shell. Both these properties combine to give each successive element a greater attraction on bonding electrons. The exception to this is group 8A. The noble gases generally do not form chemical bonds and are not assigned an electronegativity value.
114) Explain how and why the following properties change as you progress from the top to the bottom of a group on the periodic table.
a) atomic radius
b) ionization energy
c) electronegativity
Difficulty: medium
Learning Objective 1:
Section Reference 1: Section 11.1
Solution: a) As one progresses from top to bottom of a group, the atomic radius of each successive element increases. The reason for this increase is that each successive element contains one more electron shell than the preceding element.
b) As one progresses from top to bottom of a group, the first ionization energy decreases. The reason for this is that with each successive element the valence electrons move further out. Another factor is that the inner electron shells are able to shield the valence electrons from the attraction of the nucleus. Both of these factors allow the valence electrons to be more easily removed.
c) As one progresses from top to bottom of a group, the electronegativity of each successive element decreases. This occurs because the valence shells move further out and the inner electron shells shield the attractive force of the nucleus.
115) When an atom forms a cation its size changes. Explain how and why its size changes.
Difficulty: easy
Learning Objective 1:
Section Reference 1: Section 11.3
Solution: Cations form when atoms lose their valence electrons. Cations have one electron shell less than their atoms. In cations, a nucleus must hold fewer electrons than in an atom of the same element. The fewer electrons are held more closely. Both of these properties, fewer electron shells and fewer electrons held both combine to make the cation smaller than its atom.
116) When an atom forms an anion its size changes. Explain how and why its size changes.
Difficulty: easy
Learning Objective 1:
Section Reference 1: Section 11.3
Solution: Anions form when atoms gain one or more electrons. The nuclear charge, which holds electrons, must be spread over more electrons. Each electron is held more loosely in the anion causing its size to increase. Anions are larger than their atoms.
117) Explain how magnesium sulfide forms from its elements. Be sure to include the following:
a) how the anion and cation form
b) ground state electron configuration for both atoms
c) ground state electron configuration for both ions.
d) Balanced chemical equation for the entire process.
Difficulty: hard
Learning Objective 1:
Section Reference 1: Section 11.3
Solution: Magnesium sulfide forms from magnesium and sulfur. Electrons are transferred from the magnesium atoms to the sulfur atoms. The magnesium atoms have the electron configuration 1s2 2s2 2p6 3s2. These atoms lose two electrons forming the cation Mg+2. These cations have the electron configuration 1s2 2s2 2p6. The sulfur atoms have the electron configuration 1s2 2s2 2p6 3s23p4. These atoms gain two electrons forming the anion S-2. These anions have the electron configuration 1s2 2s2 2p6 3s2 3p6. The balanced chemical equation for this process is as follows:
Mg + S → MgS
118) Explain how magnesium chloride forms from its elements. Be sure to include the following: a) how the anion and cation form
b) ground state electron configuration for both atoms
c) ground state electron configuration for both ions
d) balanced chemical equation for the entire process
Difficulty: hard
Learning Objective 1:
Section Reference 1: Section 11.3
Solution: Magnesium chloride forms from magnesium and chlorine. Electrons are transferred from the magnesium atoms to the chlorine atoms. The magnesium atoms have the electron configuration 1s2 2s2 2p6 3s2. These atoms lose two electrons forming the cation Mg+2. These cations have the electron configuration 1s2 2s2 2p6. The chlorine atoms have the electron configuration 1s2 2s2 2p6 3s23p5. These atoms gain one electron forming the anion 
. These anions have the electron configuration 1s2 2s2 2p6 3s2 3p6. The balanced chemical equation for this process is as follows:
Mg + Cl2 → MgCl2
119) For each of the following compounds, choose its molecular shape from the list of shapes. (Shapes can be used more than once.)
COMPOUNDS SHAPES
a) H2O 1. Linear
b) CO2 2. Bent
c) CH4 3. Trigonal Planar
d) BF3 4. Trigonal Pyramidal
e) N2 5. Tetrahedral
Difficulty: medium
Learning Objective 1:
Section Reference 1: Section 11.10
Solution: a) H2O is bent (2); b) CO2 is linear (1); c) CH4 is tetrahedral (5); d) BF3 is trigonal planar (3); e) N2 is linear (1)
120) For each of the following compounds, choose its molecular shape from the list of shapes. (Shapes can be used more than once.)
COMPOUNDS SHAPES
a) NH3 1. Linear
b) H2S 2. Bent
c) AlCl3 3. Trigonal Planar
d) CCl4 4. Trigonal Pyramidal
e) HCN 5. Tetrahedral
Difficulty: medium
Learning Objective 1:
Section Reference 1: Section 11.10
Solution: a) NH3 is a trigonal pyramidal (4); b) H2S is bent (2); c) AlCl3 is (ionic compound, shapes are coming from crystal lattice structures) trigonal planar (3); d) CCl4 is tetrahedral (5); e) HCN is linear (1)
121) Using Lewis electron dot symbols, show how magnesium chloride forms from its elements.
Difficulty: medium
Learning Objective 1:
Section Reference 1: Section 11.3
Solution: 
122) Using Lewis electron dot symbols, show how potassium sulfide forms from its elements.
Difficulty: medium
Learning Objective 1:
Section Reference 1: Section 11.3
Solution: 
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Test Bank | Foundations of College Chemistry 15e by Hein Arena
By Hein Arena, Willard
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