examview - chem 1411. review for test 3 (chapter 7, 8, 9

Name: ________________________ Class: ___________________ Date: __________ ID: A

CHEM 1411. Review for Test 3 (Chapter 7, 8, 9_Periodic Table and Bonding I & II) Ky100, page 6

CHEM 1411. Review for Test 3 (Chapter 7, 8, 9_Periodic Table and Bonding I & II) Ky100

Multiple ChoiceIdentify 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 electronsb. those electrons in s orbitalsc. those electrons in d orbitalsd. the outermost electronse. none of these

____ 2. Of the following, which periodic group(s) do not match their designation?a. d-transition metals / IIIB IIBb. halogens / VIIAc. noble gases / VIIIBd. representative metals / IA, IIAe. alkaline earth metals / IIA

____ 3. ____ is a d-transition metal.a. Snb. Gac. Crd. Sbe. Li

____ 4. ____ is an actinide.a. 22Tib. 93Npc. 36Krd. 81Tle. 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

Name: ________________________ ID: A


____ 7. The minimum energy required to remove the most loosely held electron isa. kinetic energyb. first ionization energy.c. potential energyd. electronegativity.e. electron affinity

____ 8. The first ionization energy of sulfur is less than that of phosphorus. A reasonable explanation for this fact involvesa. 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. Cb. Oc. Bd. Ne. Be

____ 10. Arrange the following elements in order of decreasing first ionization energy.F, Be, O, N, C

a. O > F > N > Be > Cb. F > O > N > C > Bec. Be > C > O > N > Fd. F > N > O > C > Bee. 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. Sib. Pc. Ted. Se. Se

____ 13. Which of the following ions is not isoelectronic with a noble gas?a. Se2

b. Mg2+

c. P2

d. Cs+

e. Ba2+

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. Rb+ > K+ > Ca2+ > Al3+ > Ga3+

b. Ga3+ > Al3+ > Ca2+ > Rb+ > K+

c. Rb+ > K+ > Ca2+ > Ga3+ > Al3+

d. Rb+ > Ga3+ > Ca2+ > K+ > Al3+

e. Rb+ > Ca2+ > K+ > Ga3+ > Al3+

____ 17. Which of these elements has the greatest attraction for electrons in a covalent bond?a. Brb. Gec. Sed. Ase. Kr

____ 18. Which pair of elements below would be least likely to form an ionic bond between them?a. Cs / Ob. C / Nc. Na / Sd. Al / Fe. 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. 3b. 6c. 5d. 4e. none of these

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. threeb. eightc. fived. foure. six

____ 21. Oxygen was discovered by Priestley in 1774 when he observed the ____.a. reaction of sulfuric acid, H2SO4, with sodiumb. electrolysis of waterc. the thermal decomposition of potassium chlorate, KClO3

d. thermal decomposition of mercury(II) oxide, HgOe. 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 oxygenoxygen bond lengths are 1.23 ? and 1.48 ?

c. Its density is about 1 12

times that of O2.

d. It is unstable.e. Its molecules are angular.

____ 23. Which one of the following oxides is amphoteric?a. BeOb. P4O6

c. CO2

d. Cl2Oe. 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. CaSb. CH4

c. NOd. H2Se. CS2

____ 25. Write the balanced formula unit equation for the reaction of dinitrogen pentoxide with water. What is the sum of the coefficients?a. 5b. 6c. 8d. 4e. 3

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. 49b. 17c. 30d. 73e. 61

____ 27. The brownish color of photochemical smog is due to ____.a. NO2

b. COc. NOd. SO2

e. SO3

____ 28. Combustion of fossil fuels contaminated with sulfur leads to what phenomena?a. ozone destructionb. greenhouse effectc. global warmingd. acid raine. photochemical smog

____ 29. An element that has the same ground state valence-shell electron configuration as silicon is

a. gallium.b. lithium.c. argon.d. magnesium.e. lead.

____ 30. An atom of which of the following elements has the largest second ionization energy?a. Pbb. Atc. Pod. Cse. Ba

____ 31. Which of the following species is isoelectronic with Ar?a. Na+

b. Ca2+

c. Ga3+

d. O2-

e. Ne

Name: ________________________ ID: A


____ 32. Which of the following species would you expect to have the largest radius?a. Se2

b. Ca2

c. Na

d. Pe. S2

____ 33. What is the oxidation state of arsenic in arsenic acid, H3AsO4?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, cesiuma. Na < K < Rb < Csb. Cs < K < Na < Rbc. Rb < Cs < Na < Kd. Na < Rb < K < Cse. 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. I and IIIb. II and IVc. I, III, and IVd. I, II, and IIIe. 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. 4b. 3c. 1d. 0e. 2

Name: ________________________ ID: A


____ 38. An atom of which element below has the most unpaired electrons?a. Alb. Pc. Od. Bae. 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. 2b. 10c. 8d. 4e. 5

____ 42. When one mole of calcium, Ca, combines with one-half mole of oxygen, O2, to form calcium oxide, CaO, ____ mole(s) of electrons are transferred from ____ atoms to ____ atoms.a. two; calcium; oxygenb. one; oxygen; calciumc. two; oxygen; calciumd. one; calcium; oxygene. one-half; oxygen; calcium

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; strongerb. more; shorter; weakerc. more; shorter; strongerd. fewer; shorter; strongere. more; greater; weaker

____ 44. Which of the following is the correct Lewis dot formula for H2S?

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 bondsc. the number of valence electronsd. the shape of the moleculee. the order the atoms are connected

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. 2b. 0c. 8d. 4e. 6

____ 48. The total number of covalent bonds in the N2 molecule is ____.a. threeb. twoc. fourd. zeroe. 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+.

a. P = 0; H = 14

+

b. P = 0; H = 1+c. P = 1+; H = 0d. P = 0; H = 0e. 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. H2Te, BeI2

b. SF4, AsF5, BeI2

c. SF4, SiCl4

d. AsF5

e. BeI2

____ 52. Which molecule exhibits resonance?a. O3

b. CO2

c. PCl3

d. H2Se. BeI2

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. I and IIb. II and IIIc. III and IVd. I and IIIe. II, III, and IV

____ 54. How many resonance structures does the nitrate ion, NO3, have?

a. 1b. 4c. 0d. 3e. 2

____ 55. Which molecule has the most polar covalent bond?a. HClb. HIc. H2

d. HBre. 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. H2Se. 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. HCNb. Na2SO4

c. Cl2

d. KCle. HF

Name: ________________________ ID: A


____ 59. Which of the following molecules has the most covalent bond character?a. NH3

b. PbOc. NaFd. IFe. IBr

____ 60. The Lewis structure of which of the following formula violates the octet rule?a. PF3

b. HFc. SiF4

d. OF2

e. ClF3

____ 61. TIn the Lewis structure of BrF5, how many lone pairs are around the central atom?a. 2b. 1c. 3d. 0e. 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 pairb. 2 single bonds, 0 double bonds, 2 lone pairsc. 2 single bonds, 0 double bonds, 1 lone paird. 1 single bond, 0 double bonds, 0 lone pairse. 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 shellb. VSEPR shellc. bonding shelld. hybridized shelle. Lewis shell

Name: ________________________ ID: A


____ 66. The valence shell isa. 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 bondsb. lone pairs on an outer atomc. double bondsd. lone pairs on the central atome. triple bonds

____ 68. What angle(s) are associated with a central atom that has tetrahedral electronic geometry?a. 90 and 180b. 109.5c. 90 and 120d. 120 and 180e. 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. spd. sp3d2

e. sp3d

____ 70. What is (are) the bond angle(s) in BeI2 molecules?a. 109b. 90 and 180c. 120d. 180e. 120 and 90

____ 71. Which of the following molecules has 120 bond angles?a. CF4

b. BI3

c. H2Od. 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

Name: ________________________ ID: A


____ 73. Consider the following statements about BCl3 molecules. Which statement is false?a. The ClBCl bond angles are 109.5.b. The BCl 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, SiF4, and no other characteristics?I. tetrahedralII. 120 bond anglesIII. sp hybridized at CIV. polar moleculeV. one unshared pair of electrons on Si

a. II and IIIb. Ic. I and Vd. II, IV, and Ve. 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. octahedralb. trigonal bipyramidalc. tetrahedrald. pyramidale. trigonal planar

____ 77. Which of the following statements about PBr3 is false?a. It is a polar molecule.b. P is sp3 hybridized.c. P has one lone pair.d. The PBr bonds are polare. 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.

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. octahedronb. tetrahedronc. triangular planed. trigonal bipyramide. pyramid

____ 80. What is the hybridization at arsenic in AsF5 molecules?a. sp3db. sp3d2

c. spd. sp3

e. sp2

____ 81. Which one of the following molecules has sp3d hybridization at the central atom?a. HFb. 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. H2Ob. PF5

c. NH3

d. CHCl3

e. none of these

____ 84. Which one of the following is a polar molecule with nonpolar bonds?a. H2Ob. CHCl3

c. PF5

d. NH3

e. none of these

____ 85. What is the hybridization at the sulfur atom in SF6?a. sp3d2

b. sp3

c. spd. sp3de. sp2

Name: ________________________ ID: A


____ 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. I and IIIb. II and IVc. I and IVd. II and Ve. II and III

____ 90. Which one of the following molecules has a central atom that is not sp3 hybridized?a. H2Ob. CHCl3

c. SF4

d. CH4

e. NH3

Name: ________________________ ID: A


____ 91. Which species is incorrectly matched with bond angles?

Molecule / Bond Anglesa. AsF5 / 90, 120 (and 180)b. BF3 / 120c. BeI2 / slightly less than 109d. SiCl4 / 109.5e. SF6 / 90 (and 180)

____ 92. Which species is incorrectly matched with bond angles?

Molecule / Bond Anglesa. CCl4 / 109.5b. SeF6 / 90 (and 180)c. PCl5 / 120 and 90 (and 180)d. BeBr2 / 180e. 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. bentb. see-saw or distorted tetrahedralc. tetrahedrald. trigonal planare. trigonal pyramidal

Name: ________________________ ID: A


____ 95. Which of the following molecules is nonpolar?

a. sulfur dioxide, SO2

b. hydrogen fluoride, HF

c. boron trifluoride, BF3

d. sulfur tetrafluoride, SF4

e. phosphorus trifluoride, PF3

____ 96. What is the electron geometry around carbon atom C2?

a. trigonal pyramidalb. trigonal planarc. lineard. bente. tetrahedral

____ 97. What is the shape (molecular geometry) of IBr3?a. seesawb. trigonal pyramidalc. trigonal bipyramidald. trigonal planare. 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

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. bentb. trigonal bipyramidalc. trigonal planard. trigonal pyramidale. tetrahedral

ID: A


CHEM 1411. Review for Test 3 (Chapter 7, 8, 9_Periodic Table and Bonding I & II) Ky100Answer Section

MULTIPLE CHOICE

1. ANS: D PTS: 1 OBJ: Understand the importance of the outermost electrons in chemistry.TOP: More About the Periodic Table

2. ANS: C PTS: 1 OBJ: Match the family of elements with the group number(s).TOP: More About the Periodic Table

3. ANS: C PTS: 1 OBJ: Identify a d-transition metal.TOP: More About the Periodic Table

4. ANS: B PTS: 1 OBJ: Identify an actinide. TOP: More About the Periodic Table

5. ANS: E PTS: 1 OBJ: Determine the electron configuration beyond the noble gas core given the group number.TOP: More About the Periodic Table

6. ANS: E PTS: 1 OBJ: Determine the electron configuration beyond the noble gas core given the group number.TOP: More About the Periodic Table

7. ANS: B PTS: 1 OBJ: Define first ionization energy.TOP: Ionization Energy

8. ANS: B PTS: 1 OBJ: Understand the causes of differences between ionization energies. TOP: Ionization Energy

9. ANS: D PTS: 1 OBJ: Identify the atom with the highest ionization energy.TOP: Ionization Energy

10. ANS: D PTS: 1 DIF: Harder Question OBJ: Arrange the atoms according to ionization energy (five atoms). TOP: Ionization Energy

11. ANS: A PTS: 1 OBJ: Identify a chemical equation representing the first ionization energy of an atom.TOP: Ionization Energy

12. ANS: D PTS: 1 OBJ: Identify the atom with the most negative electron affinity.TOP: Electron Affinity

13. ANS: C PTS: 1 OBJ: Determine all atoms or ions which are isoelectronic.TOP: Ionic Radii

14. ANS: D PTS: 1 OBJ: Identify the ion with the largest radius.TOP: Ionic Radii

15. ANS: C PTS: 1 OBJ: Identify the ion with the largest radius.TOP: Ionic Radii

16. ANS: C PTS: 1 OBJ: Arrange the ions according to size (five ions).TOP: Ionic Radii

17. ANS: A PTS: 1 OBJ: Identify the atom with the highest electronegativity.TOP: Electronegativity

18. ANS: B PTS: 1 OBJ: Identify the atom pair most likely to form a covalent compound. TOP: Electronegativity

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 RadiiNOT: 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

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

ID: A


55. ANS: E PTS: 1 OBJ: Identify the most polar covalent bond.TOP: Polar and Nonpolar Covalent Bonds

56. ANS: B PTS: 1 OBJ: Identify the most polar covalent bond.TOP: Polar and Nonpolar Covalent Bonds

57. ANS: C PTS: 1 OBJ: Identify the most polar covalent bond.TOP: Polar and Nonpolar Covalent Bonds

58. ANS: B PTS: 1 OBJ: Identify the compound with both ionic and covalent bonds. TOP: The Continuous Range of Bonding Types

59. ANS: E PTS: 1 OBJ: Identify the molecule with the greatest covalent character.TOP: The Continuous Range of Bonding Types

60. ANS: E PTS: 1 OBJ: Determine the formula whose Lewis structure violates the octet rule.TOP: Lewis Formulas for Molecules and Polyatomic Ions NOT: Dynamic Question

61. ANS: B PTS: 1 OBJ: Determine the number of lone pairs around the central atom, given the formula.TOP: Lewis Formulas for Molecules and Polyatomic Ions NOT: Dynamic Question

62. ANS: D PTS: 1 OBJ: Match the an element to the Lewis Dot structure.TOP: Lewis Dot Formulas of Atoms NOT: OWL

63. ANS: E PTS: 1 OBJ: Match the Lewis Dot formula to the electron configuration. TOP: Lewis Dot Formulas of Atoms NOT: OWL

64. ANS: B PTS: 1 OBJ: Determine the Lewis structure.TOP: Lewis Formulas for Molecules and Polyatomic Ions NOT: OWL

65. ANS: A PTS: 1 OBJ: Define valence shell. TOP: Valence Electrons

66. ANS: B PTS: 1 OBJ: Define valence shell. TOP: Valence Electrons

67. ANS: B PTS: 1 OBJ: Identify electron groups which define the electron geometry around the central atom.TOP: Valence Shell Electron Pair Repulsion (VSEPR) Theory

68. ANS: B PTS: 1 OBJ: Identify the angles between electron groups given the electron geometry.TOP: Valence Shell Electron Pair Repulsion (VSEPR) Theory

69. ANS: C PTS: 1 OBJ: Identify the central atom hybridization given the bond angles. TOP: Valence Bond (VB) Theory

70. ANS: D PTS: 1 OBJ: Determine the molecule bond angles given the formula.TOP: Linear Electronic Geometry: AB2 Species

71. ANS: B PTS: 1 OBJ: Identify the formula consistent with the given bond angles. TOP: Trigonal Planar Electronic Geometry

72. ANS: B PTS: 1 OBJ: Identify the formula consistent with the given bond angles. TOP: Trigonal Planar Electronic Geometry

73. ANS: A PTS: 1 OBJ: Apply VSEPR and VB theory given the formula.TOP: Trigonal Planar Electronic Geometry

ID: A


74. ANS: B PTS: 1 OBJ: Apply VSEPR and VB theory given the formula.TOP: Tetrahedral Electronic Geometry: AB4 Species

75. ANS: E PTS: 1 OBJ: Identify the formula consistent with a polar molecule.TOP: Tetrahedral Electronic Geometry: AB4 Species

76. ANS: C PTS: 1 OBJ: Identify the central atom electron geometry given a formula. TOP: Tetrahedral Electronic Geometry: AB3U Species

77. ANS: E PTS: 1 OBJ: Apply VSEPR and VB theory given the formula.TOP: Tetrahedral Electronic Geometry: AB3U Species

78. ANS: C PTS: 1 OBJ: Apply VSEPR theory given the formula.TOP: Tetrahedral Electronic Geometry: ABU3 Species

79. ANS: D PTS: 1 OBJ: Identify the molecular geometry given the central atom hybridization and central atom lone pairs.TOP: Trigonal Bipyramidal Electronic Geometry: AB5, AB4U, AB3U2, and AB2U3

80. ANS: A PTS: 1 OBJ: Identify the central atom electron geometry given a formula. TOP: Trigonal Bipyramidal Electronic Geometry: AB5, AB4U, AB3U2, and AB2U3

81. ANS: E PTS: 1 OBJ: Identify the formula consistent with the given central atom hybridization.TOP: Trigonal Bipyramidal Electronic Geometry: AB5, AB4U, AB3U2, and AB2U3

82. ANS: A PTS: 1 OBJ: Identify the formula consistent with the given central atom electron and molecular geometry.TOP: Trigonal Bipyramidal Electronic Geometry: AB5, AB4U, AB3U2, and AB2U3

83. ANS: E PTS: 1 DIF: Harder Question OBJ: Identify the formula consistent with a nonpolar molecule. TOP: Trigonal Bipyramidal Electronic Geometry: AB5, AB4U, AB3U2, and AB2U3

84. ANS: E PTS: 1 DIF: Harder Question OBJ: Identify the formula consistent with a polar molecule. TOP: Trigonal Bipyramidal Electronic Geometry: AB5, AB4U, AB3U2, and AB2U3

85. ANS: A PTS: 1 OBJ: Identify the central atom hybridization given the formula.TOP: Octahedral Electronic Geometry: AB6, AB5U, and AB4U2

86. ANS: D PTS: 1 OBJ: Identify the formula consistent with given molecular geometry. TOP: Octahedral Electronic Geometry: AB6, AB5U, and AB4U2

87. ANS: D PTS: 1 OBJ: Understand the VBT interpretation of covalent bonding.TOP: Compounds Containing Triple Bonds

88. ANS: E PTS: 1 OBJ: Apply the VBT interpretation of covalent bonding.TOP: Compounds Containing Triple Bonds

89. ANS: D PTS: 1 OBJ: Apply VSEPR and VB theory given the molecule name.TOP: Compounds Containing Triple Bonds

90. ANS: C PTS: 1 OBJ: Identify the formula not consistent with the given central atom hybridization.TOP: A Summary of Electronic and Molecular Geometries

91. ANS: C PTS: 1 OBJ: Identify the formulas not consistent with the given bond angles. TOP: A Summary of Electronic and Molecular Geometries

ID: A


92. ANS: E PTS: 1 OBJ: Identify the formulas not consistent with the given bond angles. TOP: A Summary of Electronic and Molecular Geometries

93. ANS: D PTS: 1 DIF: Easy OBJ: Identify the bond angle of a particular molecular geometry. TOP: A Summary of Electronic and Molecular Geometries NOT: Dynamic Question

94. ANS: E PTS: 1 DIF: Moderate OBJ: Determine the molecular geometry around an atom given the Lewis structure.TOP: A Summary of Electronic and Molecular Geometries NOT: Dynamic Question

95. ANS: C PTS: 1 DIF: Moderate OBJ: Identify the nonpolar molecule.TOP: Polar and Nonpolar Molecules NOT: Dynamic Question

96. ANS: C PTS: 1 DIF: Moderate OBJ: Determine the molecular or electron geometry around the specified atom given the Lewis structure.TOP: A Summary of Electronic and Molecular Geometries NOT: Dynamic Question

97. ANS: E PTS: 1 OBJ: Apply VSEPR theory given the formula.TOP: Valence Shell Electron Pair Repulsion (VSEPR) Theory NOT: OWL

98. ANS: E PTS: 1 OBJ: Identify the ideal bond angle.TOP: Valence Shell Electron Pair Repulsion (VSEPR) Theory NOT: OWL

99. ANS: B PTS: 1 OBJ: Identify the hybrid orbital.TOP: Valence Bond (VB) Theory NOT: OWL

100. ANS: D PTS: 1 OBJ: Determine the molecular geometry given the hybridization and number of lone pairs.TOP: Valence Bond (VB) Theory NOT: OWL

examview - chem 1411. review for test 3 (chapter 7, 8, 9

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