Name: ________________________ Class: ___________________ Date: __________
ID: A
CHEM 1411. Review for Test 3 (Chapter 7, 8, 9_Periodic Table and Bonding I & II) Ky100
Multiple Choice
Identify the choice that best completes the statement or answers the question.
____
1. Which electrons have the greatest influence on the properties of elements?
a. core electrons
b. those electrons in s orbitals
c. those electrons in d orbitals
d. the outermost electrons
e. none of these
____
2. Of the following, which periodic group(s) do not match their designation?
a. d-transition metals / IIIB  IIB
b. halogens / VIIA
c. noble gases / VIIIB
d. representative metals / IA, IIA
e. alkaline earth metals / IIA
____
3. ____ is a d-transition metal.
a. Sn
b. Ga
c. Cr
d. Sb
e. Li
____
4. ____ is an actinide.
a. 22Ti
b. 93Np
c. 36Kr
d. 81Tl
e. 42Mo
____
5. What would be the outer electron configuration of group VIA (O, S, Se, . . .)?
a. ns0np6
b. ns2np2
c. np6
d. ns2np6
e. ns2np4
____
6. What would be the outer electron configuration of alkaline earth metals?
a. ns2np2
b. nd2
c. ns0np2
d. np2
e. ns2
CHEM 1411. Review for Test 3 (Chapter 7, 8, 9_Periodic Table and Bonding I & II) Ky100, page 6
Name: ________________________
ID: A
____
7. The minimum energy required to remove the most loosely held electron is
a. kinetic energy
b. first ionization energy.
c. potential energy
d. electronegativity.
e. electron affinity
____
8. The first ionization energy of sulfur is less than that of phosphorus. A reasonable explanation for this fact
involves
a. the smaller size of sulfur atoms relative to phosphorus atoms.
b. pairing of two electrons in one 3p orbital in sulfur atoms.
c. the higher electronegativity of sulfur relative to phosphorus.
d. the stability of the half-filled subshell in atomic sulfur.
e. the ease with which phosphorus attains a noble gas electronic configuration.
____
9. Which element has the highest first ionization energy?
a. C
b. O
c. B
d. N
e. Be
____ 10. Arrange the following elements in order of decreasing first ionization energy.
F, Be, O, N, C
a.
b.
c.
d.
e.
O > F > N > Be > C
F > O > N > C > Be
Be > C > O > N > F
F > N > O > C > Be
Be > C > N > O > F
____ 11. Which equation below depicts the reaction from which the first ionization energy would be determined?
a. Ca(g)  Ca+(g) + e
b. Ca(g)  Ca2+ + e
c. Ca(s)  Ca+(g) + e
d. Ca(s) + e  Ca-(g)
e. None of these
____ 12. Which of the following elements has the most negative electron affinity?
a. Si
b. P
c. Te
d. S
e. Se
____ 13. Which of the following ions is not isoelectronic with a noble gas?
a. Se2
b. Mg2+
c. P2
d. Cs+
e. Ba2+
CHEM 1411. Review for Test 3 (Chapter 7, 8, 9_Periodic Table and Bonding I & II) Ky100, page 2
Name: ________________________
ID: A
____ 14. Which ion has the largest radius?
a. I
b. Br
c. F
d. At
e. Cl
____ 15. Which ion has the largest radius?
a. Mg2+
b. Be2+
c. Na+
d. Al3+
e. Li+
____ 16. Arrange the following set of ions in order of decreasing ionic radii.
Al3+, Ga3+, Ca2+, Rb+, K+
a.
b.
c.
d.
e.
Rb+ > K+ > Ca2+ > Al3+ > Ga3+
Ga3+ > Al3+ > Ca2+ > Rb+ > K+
Rb+ > K+ > Ca2+ > Ga3+ > Al3+
Rb+ > Ga3+ > Ca2+ > K+ > Al3+
Rb+ > Ca2+ > K+ > Ga3+ > Al3+
____ 17. Which of these elements has the greatest attraction for electrons in a covalent bond?
a. Br
b. Ge
c. Se
d. As
e. Kr
____ 18. Which pair of elements below would be least likely to form an ionic bond between them?
a. Cs / O
b. C / N
c. Na / S
d. Al / F
e. Mg / Br
____ 19. Write the balanced formula unit equation for the reaction of magnesium with hydrogen at high temperature.
What is the sum of the coefficients? (Do not forget coefficients of one.) Use the smallest whole number
coefficients.
a. 3
b. 6
c. 5
d. 4
e. none of these
CHEM 1411. Review for Test 3 (Chapter 7, 8, 9_Periodic Table and Bonding I & II) Ky100, page 3
Name: ________________________
ID: A
____ 20. Write the balanced formula unit equation for the reaction of sodium hydride with water. What is the sum of
the coefficients in the balanced equation? Use the smallest whole numbers possible. (Do not forget
coefficients of one.)
a. three
b. eight
c. five
d. four
e. six
____ 21. Oxygen was discovered by Priestley in 1774 when he observed the ____.
a. reaction of sulfuric acid, H2SO4, with sodium
b. electrolysis of water
c. the thermal decomposition of potassium chlorate, KClO3
d. thermal decomposition of mercury(II) oxide, HgO
e. results of fractional distillation of air
____ 22. Which statement does not accurately describe ozone?
a. It is a very strong oxidizing agent.
b. Its two oxygenoxygen bond lengths are 1.23 ? and 1.48 ?
1
c. Its density is about 1 times that of O2.
2
d. It is unstable.
e. Its molecules are angular.
____ 23. Which one of the following oxides is amphoteric?
a. BeO
b. P4O6
c. CO2
d. Cl2O
e. Li2O
____ 24. Which one of the following compounds would be expected to react with oxygen at elevated temperatures to
produce both an acidic oxide and a basic oxide?
a. CaS
b. CH4
c. NO
d. H2S
e. CS2
____ 25. Write the balanced formula unit equation for the reaction of dinitrogen pentoxide with water. What is the
sum of the coefficients?
a. 5
b. 6
c. 8
d. 4
e. 3
CHEM 1411. Review for Test 3 (Chapter 7, 8, 9_Periodic Table and Bonding I & II) Ky100, page 4
Name: ________________________
ID: A
____ 26. Octane, C8H18, is a major component of gasoline. Write the balanced formula unit equation for the reaction
of the complete combustion of octane. What is the sum of the coefficients?
a. 49
b. 17
c. 30
d. 73
e. 61
____ 27. The brownish color of photochemical smog is due to ____.
a. NO2
b. CO
c. NO
d. SO2
e. SO3
____ 28. Combustion of fossil fuels contaminated with sulfur leads to what phenomena?
a. ozone destruction
b. greenhouse effect
c. global warming
d. acid rain
e. photochemical smog
____ 29. An element that has the same ground state valence-shell electron configuration as silicon is
a.
b.
c.
d.
e.
gallium.
lithium.
argon.
magnesium.
lead.
____ 30. An atom of which of the following elements has the largest second ionization energy?
a. Pb
b. At
c. Po
d. Cs
e. Ba
____ 31. Which of the following species is isoelectronic with Ar?
a. Na +
2+
b. Ca
3+
c. Ga
2d. O
e. Ne
CHEM 1411. Review for Test 3 (Chapter 7, 8, 9_Periodic Table and Bonding I & II) Ky100, page 5
Name: ________________________
ID: A
____ 32. Which of the following species would you expect to have the largest radius?
2
a. Se
2
b. Ca
c. Na 
d. P
2
e. S
____ 33. What is the oxidation state of arsenic in arsenic acid, H 3AsO4?
a. +1
b. -1
c. +3
d. -5
e.
+5
____ 34. Arrange the following elements in order of lowest to highest electronegativity:
Sodium, rubidium, potassium, cesium
a. Na < K < Rb < Cs
b. Cs < K < Na < Rb
c. Rb < Cs < Na < K
d. Na < Rb < K < Cs
e. Cs < Rb < K < Na
____ 35. Which response includes only the true statements concerning the characteristics of covalent compounds?
I.
These compounds can be gases, liquids, or solids with low melting points.
II.
Most are soluble in polar solvents.
III.
Liquid and molten compounds do not conduct electricity.
IV.
Aqueous solutions of these compounds are very good conductors of electricity.
a.
b.
c.
d.
e.
I and III
II and IV
I, III, and IV
I, II, and III
IV
____ 36. Which Lewis Dot Formula below is incorrect?
a.
b.
c.
d.
e.
____ 37. How many unpaired electrons are shown in a Lewis Dot Formula for silicon?
a. 4
b. 3
c. 1
d. 0
e. 2
CHEM 1411. Review for Test 3 (Chapter 7, 8, 9_Periodic Table and Bonding I & II) Ky100, page 6
Name: ________________________
ID: A
____ 38. An atom of which element below has the most unpaired electrons?
a. Al
b. P
c. O
d. Ba
e. F
____ 39. The negative ion F has the same electronic configuration as the positive ion ____.
a. K+
b. Li+
c. Ca2+
d. Mg2+
e. Sc3+
____ 40. Which Lewis dot notation for atoms and ions is correct for the reaction for the formation of calcium
phosphide?
a.
b.
c.
d.
e.
____ 41. Magnesium and nitrogen react to form Mg3N2 an ionic compound. The magnesium ion, Mg2+, has ____
electrons in its highest occupied energy level.
a. 2
b. 10
c. 8
d. 4
e. 5
____ 42. When one mole of calcium, Ca, combines with one-half mole of oxygen, O 2, to form calcium oxide, CaO,
____ mole(s) of electrons are transferred from ____ atoms to ____ atoms.
a. two; calcium; oxygen
b. one; oxygen; calcium
c. two; oxygen; calcium
d. one; calcium; oxygen
e. one-half; oxygen; calcium
CHEM 1411. Review for Test 3 (Chapter 7, 8, 9_Periodic Table and Bonding I & II) Ky100, page 7
Name: ________________________
ID: A
____ 43. The ____ bonds there are between atoms of the same two elements, the ____ the bond length and the ____ the
bond.
a. fewer; greater; stronger
b. more; shorter; weaker
c. more; shorter; stronger
d. fewer; shorter; stronger
e. more; greater; weaker
____ 44. Which of the following is the correct Lewis dot formula for H 2S?
a.
b.
c.
d.
e.
____ 45. Which of the following is the correct Lewis dash formula for carbon diselenide?
a.
b.
c.
d.
e.
____ 46. Lewis dot formulas for molecules show all of the following except:
a. the kinds of bonds (single, double, triple)
b. the number of bonds
c. the number of valence electrons
d. the shape of the molecule
e. the order the atoms are connected
CHEM 1411. Review for Test 3 (Chapter 7, 8, 9_Periodic Table and Bonding I & II) Ky100, page 8
Name: ________________________
ID: A
____ 47. Draw the Lewis dot formula for NH4+. How many unshared pairs of electrons are in the outer shell of the
central nitrogen atom?
a. 2
b. 0
c. 8
d. 4
e. 6
____ 48. The total number of covalent bonds in the N2 molecule is ____.
a. three
b. two
c. four
d. zero
e. one
____ 49. Which of the following guidelines for drawing Lewis formulas for covalent compounds is incorrect?
a. Representative elements (except hydrogen) usually follow the octet rule.
b. Hydrogen can never be a central atom.
c. In neutral species, nitrogen forms 3 bonds and oxygen forms 2 bonds.
d. Carbon always forms 4 bonds.
e. One carbon atom in a compound may form both a double bond and a triple bond.
____ 50. Assign a formal charge to each atom of PH4+.
1
a. P = 0; H = +
4
b. P = 0; H = 1+
c. P = 1+; H = 0
d. P = 0; H = 0
e. P = 4+; H = 1
____ 51. Which response contains all the molecules below that violate the octet rule, and no others?
SF4, SiCl4, H2Te, AsF5, BeI2
a.
b.
c.
d.
e.
H2Te, BeI2
SF4, AsF5, BeI2
SF4, SiCl4
AsF5
BeI2
____ 52. Which molecule exhibits resonance?
a. O3
b. CO2
c. PCl3
d. H2S
e. BeI2
CHEM 1411. Review for Test 3 (Chapter 7, 8, 9_Periodic Table and Bonding I & II) Ky100, page 9
Name: ________________________
ID: A
____ 53. Which numbered response lists all the molecules below that exhibit resonance and none that do not?
I.
PF5
II.
HNO3
III.
SO2
IV.
H2O
a.
b.
c.
d.
e.
I and II
II and III
III and IV
I and III
II, III, and IV
____ 54. How many resonance structures does the nitrate ion, NO 3, have?
a. 1
b. 4
c. 0
d. 3
e. 2
____ 55. Which molecule has the most polar covalent bond?
a. HCl
b. HI
c. H2
d. HBr
e. HF
____ 56. Which one of the compounds below has the bonds that are the most polar? (Electronegativities: H = 2.1, S =
2.5, P = 2.1, As = 2.1, Cl = 3.0, Si = 1.8, Sb = 1.9)
a. SiH4
b. SbCl3
c. PH3
d. H2S
e. AsCl3
____ 57. Which one of the following molecules contains bonds that are the most polar? (Electronegativities: H = 2.1,
Be = 1.5, B = 2.0, N = 3.0, F = 4.0, S = 2.5, Br = 2.8, I = 2.5)
a. BeBr2
b. BI3
c. SF6
d. NF3
e. NH3
____ 58. Which one of the following compounds involves both ionic and covalent bonding?
a. HCN
b. Na2SO4
c. Cl2
d. KCl
e. HF
CHEM 1411. Review for Test 3 (Chapter 7, 8, 9_Periodic Table and Bonding I & II) Ky100, page 10
Name: ________________________
ID: A
____ 59. Which of the following molecules has the most covalent bond character?
a. NH3
b. PbO
c. NaF
d. IF
e. IBr
____ 60. The Lewis structure of which of the following formula violates the octet rule?
a. PF3
b. HF
c. SiF4
d. OF2
e.
ClF3
____ 61. TIn the Lewis structure of BrF5, how many lone pairs are around the central atom?
a. 2
b. 1
c. 3
d. 0
e. 4
____ 62. The following Lewis structure represents the valence electron configuration of a main-group
element:
If the element is in period 4, the symbol for the element is:
a. Sc
b. Ac
c. Y
d. Ga
e.
In
____ 63. Which of the following is the correct Lewis structure for the electron configuration
1s22s22p63s23p64s23d104p65s24d105p66s2
a.
b.
c.
d.
e.
____ 64. When you draw the Lewis structure for H2O, how many single bonds, double bonds, and lone pair
electrons reside on the central oxygen atom?
a. 1 single bond, 0 double bonds, 1 lone pair
b. 2 single bonds, 0 double bonds, 2 lone pairs
c. 2 single bonds, 0 double bonds, 1 lone pair
d. 1 single bond, 0 double bonds, 0 lone pairs
e. 1 single bond, 0 double bonds, 2 lone pairs
____ 65. The electrons in the outer shell of an atom are involved in bonding. Another name for the outer shell is ____.
a. valence shell
b. VSEPR shell
c. bonding shell
d. hybridized shell
e. Lewis shell
CHEM 1411. Review for Test 3 (Chapter 7, 8, 9_Periodic Table and Bonding I & II) Ky100, page 11
Name: ________________________
ID: A
____ 66. The valence shell is
a. the orbitals belonging to the entire molecule.
b. the highest energy level occupied by electrons.
c. the set of orbitals used to make triple bonds.
d. the hard covering on crustaceans.
e. the lowest energy level occupied by electrons.
____ 67. Which of the following do not count as regions of high electron density with respect to the central atom in a
molecule?
a. single bonds
b. lone pairs on an outer atom
c. double bonds
d. lone pairs on the central atom
e. triple bonds
____ 68. What angle(s) are associated with a central atom that has tetrahedral electronic geometry?
a. 90 and 180
b. 109.5
c. 90 and 120
d. 120 and 180
e. 120
____ 69. The hybridization associated with the central atom of a molecule in which all the bond angles are 180 is
____.
a. sp2
b. sp3
c. sp
d. sp3d2
e. sp3d
____ 70. What is (are) the bond angle(s) in BeI 2 molecules?
a. 109
b. 90 and 180
c. 120
d. 180
e. 120 and 90
____ 71. Which of the following molecules has 120 bond angles?
a. CF4
b. BI3
c. H2O
d. BF4
e. NH4+
____ 72. Which one of the following molecules has only 120 bond angles?
a. NF3
b. BI3
c. PF5
d. SF6
e. PF3
CHEM 1411. Review for Test 3 (Chapter 7, 8, 9_Periodic Table and Bonding I & II) Ky100, page 12
Name: ________________________
ID: A
____ 73. Consider the following statements about BCl 3 molecules. Which statement is false?
a. The ClBCl bond angles are 109.5.
b. The BCl bonds are quite polar.
c. BCl3 molecules are nonpolar.
d. The bond dipoles exactly cancel.
e. BCl3 molecules are planar.
____ 74. Which response contains all the characteristics listed that should apply to silicon tetrafluoride, SiF 4, and no
other characteristics?
I.
tetrahedral
II.
120 bond angles
III.
sp hybridized at C
IV.
polar molecule
V.
one unshared pair of electrons on Si
a.
b.
c.
d.
e.
II and III
I
I and V
II, IV, and V
none of these
____ 75. Which one of the following molecules is polar?
a. BCl3
b. CF4
c. BF4
d. BeCl2
e. CH2F2
____ 76. The electronic geometry of the central atom in PCl3 is ____.
a. octahedral
b. trigonal bipyramidal
c. tetrahedral
d. pyramidal
e. trigonal planar
____ 77. Which of the following statements about PBr 3 is false?
a. It is a polar molecule.
b. P is sp3 hybridized.
c. P has one lone pair.
d. The PBr bonds are polar
e. The bond angles are slightly larger than 109.5.
____ 78. Consider the chlorine atom in the HCl molecule. Which statement below is true?
a. VSEPR theory and VB theory disagree about the molecular geometry of HCl.
b. The molecule is nonpolar.
c. The chlorine atom has tetrahedral electronic geometry.
d. The molecule is angular.
e. All of these are true.
CHEM 1411. Review for Test 3 (Chapter 7, 8, 9_Periodic Table and Bonding I & II) Ky100, page 13
Name: ________________________
ID: A
____ 79. An element that is sp3d hybridized and which has no lone pairs of electrons around it in a molecule is at the
center of a(n) ____ described by imaginary lines connecting the identical surrounding atoms.
a. octahedron
b. tetrahedron
c. triangular plane
d. trigonal bipyramid
e. pyramid
____ 80. What is the hybridization at arsenic in AsF 5 molecules?
a. sp3d
b. sp3d2
c. sp
d. sp3
e. sp2
____ 81. Which one of the following molecules has sp3d hybridization at the central atom?
a. HF
b. CF4
c. SF6
d. NH3
e. PF5
____ 82. Which of the following species has trigonal bipyramidal electronic geometry and trigonal bipyramidal
molecular geometry?
a. AsCl5
b. XeF2
c. SF4
d. BrF3
e. I3
____ 83. Which one of the following is a polar molecule with nonpolar bonds?
a. H2O
b. PF5
c. NH3
d. CHCl3
e. none of these
____ 84. Which one of the following is a polar molecule with nonpolar bonds?
a. H2O
b. CHCl3
c. PF5
d. NH3
e. none of these
____ 85. What is the hybridization at the sulfur atom in SF 6?
a. sp3d2
b. sp3
c. sp
d. sp3d
e. sp2
CHEM 1411. Review for Test 3 (Chapter 7, 8, 9_Periodic Table and Bonding I & II) Ky100, page 14
Name: ________________________
____ 86. Which of the following species has square pyramidal molecular geometry?
a. SiCl4
b. NH4+
c. SbCl5
d. IF5
e. PF5
____ 87. Choose the following false statement.
a. A sigma bond is a bond resulting from head-on overlap of atomic orbitals.
b. A pi bond is a bond resulting from side-on overlap of atomic orbitals.
c. A carbon atom involved in a double bond may not be sp3 hybridized.
d. A triple bond may consist of one sigma bond and two pi bonds or of two sigma bonds
and one pi bond.
e. A double bond consists of one sigma bond and one pi bond.
____ 88. Which of the following statements regarding a carbon atom involved in 2 double bonds is false?
a. There are 2 sigma and two pi bonds.
b. The hybridization is sp.
c. The geometry is linear.
d. The C atom has two unhybridized p atomic orbitals.
e. The C atom can make one more bond to complete its octet.
____ 89. Which of the following responses contains all of the true statements for ethyne?
I.
The ethyne molecule has a double bond between its 2 carbon atoms.
II.
The ethyne molecule has a triple bond between its 2 carbon atoms.
III.
One pi bond is formed between the 2 carbon atoms by head-on overlap of the sp hybrid
orbitals.
IV.
One sigma bond is formed between the 2 carbon atoms by head-on overlap of the sp2
hybrid orbitals.
V.
The ethyne molecule is linear.
a.
b.
c.
d.
e.
I and III
II and IV
I and IV
II and V
II and III
____ 90. Which one of the following molecules has a central atom that is not sp3 hybridized?
a. H2O
b. CHCl3
c. SF4
d. CH4
e. NH3
CHEM 1411. Review for Test 3 (Chapter 7, 8, 9_Periodic Table and Bonding I & II) Ky100, page 15
ID: A
Name: ________________________
____ 91. Which species is incorrectly matched with bond angles?
a.
b.
c.
d.
e.
Molecule / Bond Angles
AsF5 / 90, 120 (and 180)
BF3 / 120
BeI2 / slightly less than 109
SiCl4 / 109.5
SF6 / 90 (and 180)
____ 92. Which species is incorrectly matched with bond angles?
a.
b.
c.
d.
e.
Molecule / Bond Angles
CCl4 / 109.5
SeF6 / 90 (and 180)
PCl5 / 120 and 90 (and 180)
BeBr2 / 180
NCl3 / 120
____ 93. What is the bond angle in a trigonal planar molecule or ion?
a. 109°
b. 72?
c. 180°
d. 120°
e. 90?
____ 94. What is the molecular geometry around the nitrogen atom?
a.
b.
c.
d.
e.
bent
see-saw or distorted tetrahedral
tetrahedral
trigonal planar
trigonal pyramidal
CHEM 1411. Review for Test 3 (Chapter 7, 8, 9_Periodic Table and Bonding I & II) Ky100, page 16
ID: A
Name: ________________________
ID: A
____ 95. Which of the following molecules is nonpolar?
a.
b.
c.
d.
e.
sulfur dioxide, SO2
hydrogen fluoride, HF
boron trifluoride, BF3
sulfur tetrafluoride, SF4
phosphorus trifluoride, PF3
____ 96. What is the electron geometry around carbon atom C2?
a.
b.
c.
d.
e.
trigonal pyramidal
trigonal planar
linear
bent
tetrahedral
____ 97. What is the shape (molecular geometry) of IBr3?
a. seesaw
b. trigonal pyramidal
c. trigonal bipyramidal
d. trigonal planar
e. T-shaped
Use the following Lewis structure for acetamide to answer the following questions:
____ 98. The ideal value for the C-C-N bond angle around atom 2 is:
a. 60o
b. 90o
c. 109.5o
d. 180o
e.
120o
CHEM 1411. Review for Test 3 (Chapter 7, 8, 9_Periodic Table and Bonding I & II) Ky100, page 17
Name: ________________________
ID: A
____ 99. What type of hybridization is represented in the figure below?
a.
sp3d
b.
sp3
c.
sp
d.
sp2
e.
sp3d2
____ 100. A molecule has sp3 hybridization with 1 lone pair. What is the geometry of this molecule?
a. bent
b. trigonal bipyramidal
c. trigonal planar
d. trigonal pyramidal
e. tetrahedral
CHEM 1411. Review for Test 3 (Chapter 7, 8, 9_Periodic Table and Bonding I & II) Ky100, page 18
ID: A
CHEM 1411. Review for Test 3 (Chapter 7, 8, 9_Periodic Table and Bonding I & II) Ky100
Answer Section
MULTIPLE CHOICE
1. ANS:
OBJ:
TOP:
2. ANS:
TOP:
3. ANS:
TOP:
4. ANS:
TOP:
5. ANS:
OBJ:
TOP:
6. ANS:
OBJ:
TOP:
7. ANS:
TOP:
8. ANS:
OBJ:
TOP:
9. ANS:
TOP:
10. ANS:
OBJ:
TOP:
11. ANS:
OBJ:
TOP:
12. ANS:
TOP:
13. ANS:
TOP:
14. ANS:
TOP:
15. ANS:
TOP:
16. ANS:
TOP:
17. ANS:
TOP:
18. ANS:
OBJ:
TOP:
D
PTS: 1
Understand the importance of the outermost electrons in chemistry.
More About the Periodic Table
C
PTS: 1
OBJ: Match the family of elements with the group number(s).
More About the Periodic Table
C
PTS: 1
OBJ: Identify a d-transition metal.
More About the Periodic Table
B
PTS: 1
OBJ: Identify an actinide.
More About the Periodic Table
E
PTS: 1
Determine the electron configuration beyond the noble gas core given the group number.
More About the Periodic Table
E
PTS: 1
Determine the electron configuration beyond the noble gas core given the group number.
More About the Periodic Table
B
PTS: 1
OBJ: Define first ionization energy.
Ionization Energy
B
PTS: 1
Understand the causes of differences between ionization energies.
Ionization Energy
D
PTS: 1
OBJ: Identify the atom with the highest ionization energy.
Ionization Energy
D
PTS: 1
DIF: Harder Question
Arrange the atoms according to ionization energy (five atoms).
Ionization Energy
A
PTS: 1
Identify a chemical equation representing the first ionization energy of an atom.
Ionization Energy
D
PTS: 1
OBJ: Identify the atom with the most negative electron affinity.
Electron Affinity
C
PTS: 1
OBJ: Determine all atoms or ions which are isoelectronic.
Ionic Radii
D
PTS: 1
OBJ: Identify the ion with the largest radius.
Ionic Radii
C
PTS: 1
OBJ: Identify the ion with the largest radius.
Ionic Radii
C
PTS: 1
OBJ: Arrange the ions according to size (five ions).
Ionic Radii
A
PTS: 1
OBJ: Identify the atom with the highest electronegativity.
Electronegativity
B
PTS: 1
Identify the atom pair most likely to form a covalent compound.
Electronegativity
CHEM 1411. Review for Test 3 (Chapter 7, 8, 9_Periodic Table and Bonding I & II) Ky100, page 1
ID: A
19. ANS: A
PTS: 1
OBJ: Write a balanced chemical equation for the reaction of a metal with hydrogen. | Sum the coefficients.
TOP: Hydrogen and the Hydrides
20. ANS: D
PTS: 1
OBJ: Write a balanced chemical equation for the reaction of an ionic hydride with water. | Sum the
coefficients.
TOP: Hydrogen and the Hydrides
21. ANS: D
PTS: 1
OBJ: Know how Priestley discovered oxygen.
TOP: Oxygen and the Oxides
22. ANS: B
PTS: 1
OBJ: Know the structure, physical properties, and reactivity of ozone.
TOP: Oxygen and the Oxides
23. ANS: A
PTS: 1
OBJ: Identify the amphoteric oxide.
TOP: Oxygen and the Oxides
24. ANS: A
PTS: 1
OBJ: Identify the compound that combines with oxygen to form acidic and basic oxides.
TOP: Oxygen and the Oxides
25. ANS: D
PTS: 1
OBJ: Write a balanced chemical equation for the reaction of a nonmetal oxide with water. | Sum the
coefficients.
TOP: Oxygen and the Oxides
26. ANS: E
PTS: 1
OBJ: Write a balanced chemical equation for the combustion of a hydrocarbon in excess oxygen. | Sum the
coefficients.
TOP: Oxygen and the Oxides
27. ANS: A
PTS: 1
OBJ: Know the components of smog.
TOP: Oxygen and the Oxides
28. ANS: D
PTS: 1
OBJ: Know the effect of sulfur contamination in fossil fuels.
TOP: Oxygen and the Oxides
29. ANS: E
PTS: 1
DIF: Easy
OBJ: Determine the configuration of an atom using the period and group numbers.
TOP: Electronic爏 tructure爋 f燼 toms
NOT: Dynamic Question
30. ANS: D
PTS: 1
DIF: Moderate
OBJ: Identify the element with the largest second ionization energy.
TOP: Ionization Energy
NOT: Dynamic Question
31. ANS: B
PTS: 1
DIF: Easy
OBJ: Identify the atom or ion that is isoelectronic with the given element.
TOP: Electronic爏 tructure爋 f燼 toms
NOT: Dynamic Question
32. ANS: A
PTS: 1
DIF: Easy
OBJ: Identify the element or ion with the largest radius.
TOP: Ionic Radii
NOT: Dynamic Question
33. ANS: E
PTS: 1
OBJ: Determine the oxidation state of an element in a compound.
TOP: Oxidation States
NOT: OWL
34. ANS: E
PTS: 1
OBJ: Rank the elements according to electronegativity.
TOP: Electronegativity
NOT: OWL
35. ANS: A
PTS: 1
OBJ: Identify the chemical and physical properties of covalent compounds.
TOP: Ionic and Covalent Bonding
MSC: Conceptual question
36. ANS: B
PTS: 1
DIF: Harder Question
OBJ: Identify the correct Lewis Dot Formulas.
TOP: Lewis Dot Formulas of Atoms
CHEM 1411. Review for Test 3 (Chapter 7, 8, 9_Periodic Table and Bonding I & II) Ky100, page 2
ID: A
37. ANS: E
PTS: 1
OBJ: Determine the number of unpaired electrons.
TOP: Lewis Dot Formulas of Atoms
38. ANS: B
PTS: 1
DIF: Harder Question
OBJ: Determine the number of unpaired electrons.
TOP: Lewis Dot Formulas of Atoms
39. ANS: D
PTS: 1
OBJ: Identify the isoelectronic ion.
TOP: Formation of Ionic Compounds
40. ANS: E
PTS: 1
OBJ: Identify the correct Lewis Dot Formulas and reaction stoichiometry.
TOP: Formation of Ionic Compounds
41. ANS: C
PTS: 1
OBJ: Determine the number of electrons in the highest energy level.
TOP: Formation of Ionic Compounds
42. ANS: A
PTS: 1
OBJ: Determine the number of electrons transferred given the balanced reaction. | Identify the species that
lose and gain electrons.
TOP: Formation of Ionic Compounds
43. ANS: C
PTS: 1
OBJ: Understand the relationship between bond order, bond length, and bond strength.
TOP: Bond Lengths and Bond Energies
44. ANS: D
PTS: 1
OBJ: Identify the correct Lewis Dot Formula.
TOP: Lewis Formulas for Molecules and Polyatomic Ions
45. ANS: E
PTS: 1
OBJ: Identify the correct Lewis Dot Formula.
TOP: Lewis Formulas for Molecules and Polyatomic Ions
46. ANS: D
PTS: 1
OBJ: Know the limits of Lewis Dot Formulas.
TOP: Lewis Formulas for Molecules and Polyatomic Ions
47. ANS: B
PTS: 1
OBJ: Draw the Lewis structure given the formula and determine the number of unshared outer shell
electrons on the central atom.
TOP: Writing Lewis Formulas: The Octet Rule
48. ANS: A
PTS: 1
OBJ: Draw the Lewis Dot Formula and determine the number of covalent bonds.
TOP: Writing Lewis Formulas: The Octet Rule
49. ANS: E
PTS: 1
OBJ: Identify the guidelines for drawing valid Lewis Dot Formulas.
TOP: Writing Lewis Formulas: The Octet Rule
50. ANS: C
PTS: 1
OBJ: Assign formal charges given the formula.
TOP: Formal Charge
51. ANS: B
PTS: 1
OBJ: Identify the molecules with Lewis structures that violate the octet rule.
TOP: Writing Lewis Formulas: Limitations of the Octet Rule for Lewis Formulas
52. ANS: A
PTS: 1
OBJ: Identify the molecule with more than one valid Lewis structure.
TOP: Resonance
53. ANS: B
PTS: 1
OBJ: Identify the molecules with more than one valid Lewis structure.
TOP: Resonance
54. ANS: D
PTS: 1
OBJ: Determine the number of valid Lewis structures given the formula.
TOP: Resonance
CHEM 1411. Review for Test 3 (Chapter 7, 8, 9_Periodic Table and Bonding I & II) Ky100, page 3
ID: A
55. ANS:
TOP:
56. ANS:
TOP:
57. ANS:
TOP:
58. ANS:
OBJ:
TOP:
59. ANS:
TOP:
60. ANS:
OBJ:
TOP:
61. ANS:
OBJ:
TOP:
62. ANS:
TOP:
63. ANS:
OBJ:
TOP:
64. ANS:
TOP:
65. ANS:
TOP:
66. ANS:
TOP:
67. ANS:
OBJ:
TOP:
68. ANS:
OBJ:
TOP:
69. ANS:
OBJ:
TOP:
70. ANS:
TOP:
71. ANS:
OBJ:
TOP:
72. ANS:
OBJ:
TOP:
73. ANS:
TOP:
E
PTS: 1
OBJ: Identify the most polar covalent bond.
Polar and Nonpolar Covalent Bonds
B
PTS: 1
OBJ: Identify the most polar covalent bond.
Polar and Nonpolar Covalent Bonds
C
PTS: 1
OBJ: Identify the most polar covalent bond.
Polar and Nonpolar Covalent Bonds
B
PTS: 1
Identify the compound with both ionic and covalent bonds.
The Continuous Range of Bonding Types
E
PTS: 1
OBJ: Identify the molecule with the greatest covalent character.
The Continuous Range of Bonding Types
E
PTS: 1
Determine the formula whose Lewis structure violates the octet rule.
Lewis Formulas for Molecules and Polyatomic Ions
NOT: Dynamic Question
B
PTS: 1
Determine the number of lone pairs around the central atom, given the formula.
Lewis Formulas for Molecules and Polyatomic Ions
NOT: Dynamic Question
D
PTS: 1
OBJ: Match the an element to the Lewis Dot structure.
Lewis Dot Formulas of Atoms
NOT: OWL
E
PTS: 1
Match the Lewis Dot formula to the electron configuration.
Lewis Dot Formulas of Atoms
NOT: OWL
B
PTS: 1
OBJ: Determine the Lewis structure.
Lewis Formulas for Molecules and Polyatomic Ions
NOT: OWL
A
PTS: 1
OBJ: Define valence shell.
Valence Electrons
B
PTS: 1
OBJ: Define valence shell.
Valence Electrons
B
PTS: 1
Identify electron groups which define the electron geometry around the central atom.
Valence Shell Electron Pair Repulsion (VSEPR) Theory
B
PTS: 1
Identify the angles between electron groups given the electron geometry.
Valence Shell Electron Pair Repulsion (VSEPR) Theory
C
PTS: 1
Identify the central atom hybridization given the bond angles.
Valence Bond (VB) Theory
D
PTS: 1
OBJ: Determine the molecule bond angles given the formula.
Linear Electronic Geometry: AB2 Species
B
PTS: 1
Identify the formula consistent with the given bond angles.
Trigonal Planar Electronic Geometry
B
PTS: 1
Identify the formula consistent with the given bond angles.
Trigonal Planar Electronic Geometry
A
PTS: 1
OBJ: Apply VSEPR and VB theory given the formula.
Trigonal Planar Electronic Geometry
CHEM 1411. Review for Test 3 (Chapter 7, 8, 9_Periodic Table and Bonding I & II) Ky100, page 4
ID: A
74. ANS:
TOP:
75. ANS:
TOP:
76. ANS:
OBJ:
TOP:
77. ANS:
TOP:
78. ANS:
TOP:
79. ANS:
OBJ:
TOP:
80. ANS:
OBJ:
TOP:
81. ANS:
OBJ:
TOP:
82. ANS:
OBJ:
TOP:
83. ANS:
OBJ:
TOP:
84. ANS:
OBJ:
TOP:
85. ANS:
TOP:
86. ANS:
OBJ:
TOP:
87. ANS:
TOP:
88. ANS:
TOP:
89. ANS:
TOP:
90. ANS:
OBJ:
TOP:
91. ANS:
OBJ:
TOP:
B
PTS: 1
OBJ: Apply VSEPR and VB theory given the formula.
Tetrahedral Electronic Geometry: AB4 Species
E
PTS: 1
OBJ: Identify the formula consistent with a polar molecule.
Tetrahedral Electronic Geometry: AB4 Species
C
PTS: 1
Identify the central atom electron geometry given a formula.
Tetrahedral Electronic Geometry: AB3U Species
E
PTS: 1
OBJ: Apply VSEPR and VB theory given the formula.
Tetrahedral Electronic Geometry: AB3U Species
C
PTS: 1
OBJ: Apply VSEPR theory given the formula.
Tetrahedral Electronic Geometry: ABU3 Species
D
PTS: 1
Identify the molecular geometry given the central atom hybridization and central atom lone pairs.
Trigonal Bipyramidal Electronic Geometry: AB5, AB4U, AB3U2, and AB2U3
A
PTS: 1
Identify the central atom electron geometry given a formula.
Trigonal Bipyramidal Electronic Geometry: AB5, AB4U, AB3U2, and AB2U3
E
PTS: 1
Identify the formula consistent with the given central atom hybridization.
Trigonal Bipyramidal Electronic Geometry: AB5, AB4U, AB3U2, and AB2U3
A
PTS: 1
Identify the formula consistent with the given central atom electron and molecular geometry.
Trigonal Bipyramidal Electronic Geometry: AB5, AB4U, AB3U2, and AB2U3
E
PTS: 1
DIF: Harder Question
Identify the formula consistent with a nonpolar molecule.
Trigonal Bipyramidal Electronic Geometry: AB5, AB4U, AB3U2, and AB2U3
E
PTS: 1
DIF: Harder Question
Identify the formula consistent with a polar molecule.
Trigonal Bipyramidal Electronic Geometry: AB5, AB4U, AB3U2, and AB2U3
A
PTS: 1
OBJ: Identify the central atom hybridization given the formula.
Octahedral Electronic Geometry: AB6, AB5U, and AB4U2
D
PTS: 1
Identify the formula consistent with given molecular geometry.
Octahedral Electronic Geometry: AB6, AB5U, and AB4U2
D
PTS: 1
OBJ: Understand the VBT interpretation of covalent bonding.
Compounds Containing Triple Bonds
E
PTS: 1
OBJ: Apply the VBT interpretation of covalent bonding.
Compounds Containing Triple Bonds
D
PTS: 1
OBJ: Apply VSEPR and VB theory given the molecule name.
Compounds Containing Triple Bonds
C
PTS: 1
Identify the formula not consistent with the given central atom hybridization.
A Summary of Electronic and Molecular Geometries
C
PTS: 1
Identify the formulas not consistent with the given bond angles.
A Summary of Electronic and Molecular Geometries
CHEM 1411. Review for Test 3 (Chapter 7, 8, 9_Periodic Table and Bonding I & II) Ky100, page 5
ID: A
92. ANS:
OBJ:
TOP:
93. ANS:
OBJ:
TOP:
94. ANS:
OBJ:
TOP:
95. ANS:
TOP:
96. ANS:
OBJ:
TOP:
97. ANS:
TOP:
98. ANS:
TOP:
99. ANS:
TOP:
100. ANS:
OBJ:
TOP:
E
PTS: 1
Identify the formulas not consistent with the given bond angles.
A Summary of Electronic and Molecular Geometries
D
PTS: 1
DIF: Easy
Identify the bond angle of a particular molecular geometry.
A Summary of Electronic and Molecular Geometries
NOT: Dynamic Question
E
PTS: 1
DIF: Moderate
Determine the molecular geometry around an atom given the Lewis structure.
A Summary of Electronic and Molecular Geometries
NOT: Dynamic Question
C
PTS: 1
DIF: Moderate
OBJ: Identify the nonpolar molecule.
Polar and Nonpolar Molecules
NOT: Dynamic Question
C
PTS: 1
DIF: Moderate
Determine the molecular or electron geometry around the specified atom given the Lewis structure.
A Summary of Electronic and Molecular Geometries
NOT: Dynamic Question
E
PTS: 1
OBJ: Apply VSEPR theory given the formula.
Valence Shell Electron Pair Repulsion (VSEPR) Theory NOT: OWL
E
PTS: 1
OBJ: Identify the ideal bond angle.
Valence Shell Electron Pair Repulsion (VSEPR) Theory NOT: OWL
B
PTS: 1
OBJ: Identify the hybrid orbital.
Valence Bond (VB) Theory
NOT: OWL
D
PTS: 1
Determine the molecular geometry given the hybridization and number of lone pairs.
Valence Bond (VB) Theory
NOT: OWL
CHEM 1411. Review for Test 3 (Chapter 7, 8, 9_Periodic Table and Bonding I & II) Ky100, page 6