Test Bank for Introductory Chemistry Essentials 5th Edition by Tro Sample Introductory Chemistry, 5e (Tro) Chapter 10 Chemical Bonding 10.1 True/False Questions 1) Bonding theories are used to predict how atoms bond together to form molecules. Diff: 1 Var: 1 Page Ref: 10.1 Global 2) Drugs to fight HIV have been developed using bonding theory models. Diff: 1 Var: 1 Page Ref: 10.1 Global 3) Li : is the proper Lewis structure (dot structure) for lithium. Diff: 1 Var: 1 Page Ref: 10.2 Learning Outcome: 10.1 Global 4) A chemical bond is classified as a covalent bond if it involves the transfer of electrons. Diff: 1 Var: 1 Page Ref: 10.2 Learning Outcome: 10.1 Global 5) The Lewis structure of oxygen should have 8 valence electrons. Diff: 1 Var: 1 Page Ref: 10.2 Learning Outcome: 10.1 Global Outcome: G1 6) Lewis structures only use the valence electrons in determining the bonding.
Diff: 1 Var: 1 Page Ref: 10.2 Learning Outcome: 10.1 Global Outcome: G1 7) Having eight valence electrons is very stable and is called an octet. Diff: 1 Var: 1 Page Ref: 10.2 Learning Outcome: 10.1 Global 8) A correct Lewis structure for an atom of carbon would have eight dots surrounding the symbol of the element. Diff: 1 Var: 1 Page Ref: 10.2 Learning Outcome: 10.1 Global 9) The correct Lewis structure for potassium in KCl is K+. Diff: 1 Var: 1 Page Ref: 10.3 Learning Outcome: 10.1 Global Outcome: G2 10) Chlorine has 8 valence electrons in the Lewis structure for KCl. Diff: 1 Var: 1 Page Ref: 10.3 Learning Outcome: 10.1 Global 11) The Lewis theory predicts that the formula for a compound of magnesium and sulfur is MgS2. Diff: 1 Var: 1 Page Ref: 10.3 Learning Outcome: 10.2 Global 12) The Lewis theory predicts that the formula for a compound made of sodium and fluorine is NaF. Diff: 1 Var: 1 Page Ref: 10.3
Learning Outcome: 10.2 Global 13) Lewis theory predicts that the formula for a compound made of aluminum and phosphorus is AlP. Diff: 1 Var: 1 Page Ref: 10.3 Learning Outcome: 10.2 Global Outcome: G2 14) The Lewis structure of water has two sets of lone pair electrons. Diff: 1 Var: 1 Page Ref: 10.4 Global 15) The structure is a proper representation of the bonding in the H2 molecule. Diff: 1 Var: 1 Page Ref: 10.4 Global Outcome: G2 16) The Lewis structure for O2 contains a triple bond. Diff: 1 Var: 1 Page Ref: 10.4 Global 17) The double bond is shorter and stronger than a single bond. Diff: 1 Var: 1 Page Ref: 10.4 Global 18) The triple bond present in diatomic nitrogen, N2, is what makes this molecule so reactive. Diff: 1 Var: 1 Page Ref: 10.4 Global
19) When calculating the number of electrons for the Lewis structure of a polyatomic ion, subtract one electron for each negative charge. Diff: 1 Var: 1 Page Ref: 10.5 Global 20) The correct Lewis structure for shows that the molecule contains two double bonds. Diff: 1 Var: 1 Page Ref: 10.5 Global 21) The correct Lewis structure for CO2 shows that the carbon atom has two sets of lone pair electrons. Diff: 1 Var: 1 Page Ref: 10.5 Global 22) When calculating the number of electrons for the Lewis structure of a polyatomic ion, you must add one electron for each negative charge and subtract one electron for each positive charge. Diff: 1 Var: 1 Page Ref: 10.5 Global Outcome: G1 23) The sulfate ion contains 28 valence electrons. Diff: 1 Var: 1 Page Ref: 10.5 Global 24) The ammonium ion contains 10 valence electrons. Diff: 1 Var: 1 Page Ref: 10.5 Global 25) Boron forms compounds that violate the octet rule.
Diff: 1 Var: 1 Page Ref: 10.5 Global 26) Resonance structures are the best representation we can draw but do not accurately reflect the true structure. Diff: 1 Var: 1 Page Ref: 10.6 Learning Outcome: 10.4 Global Outcome: G1 27) Carbon monoxide contains resonance Lewis structures. Diff: 1 Var: 1 Page Ref: 10.6 Learning Outcome: 10.4 Global 28) The VSEPR theory predicts that the angle between the central carbon atom and the two oxygen atoms in CO2 measures 180. Diff: 1 Var: 1 Page Ref: 10.7 Learning Outcome: 10.5 Global 29) The VSEPR theory predicts that the H-C-H angle in CH4 measures 120. Diff: 1 Var: 1 Page Ref: 10.7 30) It is important to identify lone pairs around a central atom because they do not repel other electron groups. Diff: 1 Var: 1 Page Ref: 10.7 Learning Outcome: 10.5 Global 31) The electron geometry of a molecule is never the same as its molecular geometry.
Diff: 1 Var: 1 Page Ref: 10.7 32) When you have 2 electron groups and none are lone pairs, the molecular geometry is linear. Diff: 1 Var: 1 Page Ref: 10.7 Learning Outcome: 10.5 Global 33) When you have 4 electron groups and 1 of them is a lone pair, the molecular geometry is bent. Diff: 1 Var: 1 Page Ref: 10.7 34) When you have 4 electron groups and none of them are lone pairs, the molecular geometry is trigonal pyramidal. Diff: 1 Var: 1 Page Ref: 10.7 Outcome: G1 35) When you have 4 electron groups, the electron geometry is tetrahedral. Diff: 1 Var: 1 Page Ref: 10.7 Learning Outcome: 10.5 Global 36) The compound H2S contains polar bonds but the molecule is nonpolar. Diff: 1 Var: 1 Page Ref: 10.8 Learning Outcome: 10.6 Global 37) Water and oil do not mix because water molecules are nonpolar and molecules that compose oil are generally polar.
Diff: 1 Var: 1 Page Ref: 10.8 Learning Outcome: 10.6 Global Outcome: G1 10.2 Multiple Choice Questions 1) Which of the following statements about Lewis structures is FALSE? A) An octet is when an atom has 8 valence electrons. B) A duet is a stable electron configuration for helium. C) An ionic bond occurs when electrons are transferred. D) A covalent bond occurs when electrons are shared. E) All of the above statements are true. Answer: E Diff: 2 Var: 1 Page Ref: 10.2 Learning Outcome: 10.1 Global 2) Which Lewis structure below correctly represents KCl? A) K [ ] B) K [: :] C) K : : D) : : : : Answer: B Diff: 2 Var: 1 Page Ref: 10.3 Learning Outcome: 10.2 Global 3) Which Lewis structure below correctly represents the compound formed between magnesium and sulfur? A) Mg [: :] B) Mg [: :] 2 Mg C) [: :] Mg 2 [: :] D) Mg 2 [: :] 2 Diff: 2 Var: 1 Page Ref: 10.3 Learning Outcome: 10.2 Global 4) The Lewis model predicts that the formula of a compound formed between bromine and aluminum is:
A) AlBr B) Al2Br C) AlBr3 D) AlBr2 Diff: 1 Var: 1 Page Ref: 10.3 Learning Outcome: 10.2 Global 5) The Lewis model predicts that the formula for a compound between fluorine and calcium is: A) CaF B) Ca2F C) CaF2 D) CaF3 Diff: 2 Var: 1 Page Ref: 10.3 Learning Outcome: 10.2 Global 6) The Lewis model predicts that the formula for a compound between barium and sulfur is: A) BaS B) Ba2S C) BaS2 D) BaS3 Answer: A Diff: 2 Var: 1 Page Ref: 10.3 Learning Outcome: 10.2 Global 7) The Lewis model predicts that the formula for a compound between potassium and sulfur is: A) KS B) K2S C) KS2 D) K3S Answer: B
Diff: 2 Var: 1 Page Ref: 10.3 Learning Outcome: 10.2 Global 8) When a nonmetal bonds with a nonmetal: A) a molecular compound forms. B) a covalent bond is involved. C) electrons are shared. D) all of the above are true Diff: 1 Var: 1 Page Ref: 10.4 Global 9) What is the correct Lewis structure for water? A) H-: :-H B) : : C) H= =H D) H- -H Diff: 2 Var: 1 Page Ref: 10.4 Global 10) What is the correct Lewis structure for Br2? A) Br-Br B) : : C) = D) : Br Br : Answer: B Diff: 2 Var: 1 Page Ref: 10.4 Global 11) What is the correct Lewis structure for O2? A) O-O B) : : C) = D) : O O :
Diff: 2 Var: 1 Page Ref: 10.4 Global 12) What is the correct Lewis structure for N2? A) N-N B) : : C) = D) : N N : Diff: 2 Var: 1 Page Ref: 10.4 Global 13) How many bonding electrons are in the Lewis structure of N2? A) 2 B) 3 C) 4 D) 6 Diff: 1 Var: 1 Page Ref: 10.4 Global 14) How many bonding electrons are in the Lewis structure of carbon monoxide, CO? A) 2 B) 3 C) 4 D) 6 Diff: 1 Var: 1 Page Ref: 10.4 Global
15) The Lewis structure for carbon monoxide is This structures shows: A) 4 lone pairs and 1 bonding pair. B) 4 lone pairs and 3 bonding pairs. C) 2 lone pairs and 3 bonding pairs. D) 2 lone pairs and 1 bonding pair. Diff: 1 Var: 1 Page Ref: 10.4 Global 16) Which sequence below represents the proper order of increasing bond strength? A) single < double < triple B) double < single < triple C) single < triple < double D) triple < double < single Answer: A Diff: 1 Var: 1 Page Ref: 10.4 Global 17) How many valence electrons are in the nitrate ion? A) 18 B) 22 C) 23 D) 24 E) 26 Diff: 2 Var: 1 Page Ref: 10.5 Global 18) The total number of electrons to be counted for the Lewis structure of the PO43- polyatomic ion is: A) 8. B) 26. C) 29. D) 32. Diff: 1 Var: 1 Page Ref: 10.5 Global
19) The central atom in the chlorate anion, ClO3- is surrounded by: A) two bonding and two unshared pairs of electrons. B) one bonding and three unshared pairs of electrons. C) three bonding and one unshared pair of electrons. D) two double bonds and no unshared pairs of electrons.. Diff: 2 Var: 1 Page Ref: 10.5 Global 20) The central atom in the chlorite anion, ClO2- is surrounded by: A) one bonding and three unshared pairs of electrons. B) two bonding and two unshared pairs of electrons. C) two bonding and one unshared pair of electrons. D) two double bonds and no unshared pairs of electrons. Answer: B Diff: 2 Var: 1 Page Ref: 10.5 Global 21) What is the correct Lewis structure for CO2? A) : : B) : = = : C) : = C = : D) : = C = : Diff: 2 Var: 1 Page Ref: 10.5 Global 22) The Lewis structure, [: = ] best represents: A) NO2+ B) NO2- C) NO2 D) both NO2+ and NO2- E) answers A, B, and C Answer: B
Diff: 2 Var: 1 Page Ref: 10.5 Global 23) What is the correct Lewis structure for CN? A) [C-N] B) [: :] C) [ = :] D) [: C N :] Diff: 2 Var: 1 Page Ref: 10.5 Global 24) The correct Lewis structure for BF3 would have exactly: A) 1 double bond. B) 2 double bonds. C) 1 triple bond. D) no double bonds. Diff: 2 Var: 1 Page Ref: 10.5 Global 25) Which molecule below would have a Lewis structure that is an exception to the octet rule? A) BH3 B) NO C) SI6 D) PF5 E) all of these Answer: E Diff: 3 Var: 1 Page Ref: 10.5 Global 26) Which symbol should be used between two structures that represent resonance structures?
A) B) C) D) Diff: 1 Var: 1 Page Ref: 10.6 Learning Outcome: 10.4 Global 27) Which set shows the correct resonance structures for SeO2? A) : : = = B) : = : : = : C) : = Se = : O Se- : : -Se O : D) = : : = E) SeO2 does not have a resonance structure. Diff: 2 Var: 1 Page Ref: 10.6 Learning Outcome: 10.4 Global 28) Which of the following compounds have resonance structures? A) CH4 B) H2O C) NH3 D) O3 E) None of the compounds have resonance structures. Diff: 2 Var: 1 Page Ref: 10.6 Learning Outcome: 10.4 Global 29) Consider the Lewis structures for the compound SO3 and the polyatomic ions SO32- and SO42-. Which of these must exist as a set of resonance structures? A) SO3 only B) SO32- only C) SO42- only D) all of these show resonance E) none of these show resonance
Answer: A Diff: 3 Var: 1 Page Ref: 10.6 Learning Outcome: 10.4 Global 30) Which one of the following molecules is NOT capable of having resonance structures? A) SeO2 B) H2O C) SO2 D) O3 Answer: B Diff: 3 Var: 1 Page Ref: 10.6 Learning Outcome: 10.4 Global 31) What is the angle between electron groups in the linear electron geometry? A) 90 B) 109.5 C) 120 D) 180 E) not enough information Learning Outcome: 10.5 Global 32) What is the angle between electron groups in the trigonal planar electron geometry? A) 90 B) 109.5 C) 120 D) 180 E) not enough information
33) What is the angle between electron groups in the tetrahedral geometry? A) 90 B) 109.5 C) 120 D) 180 E) not enough information Answer: B 34) Which of the following is considered a single electron group? A) a lone pair of electrons B) a single bond C) a double bond D) a triple bond E) all of the above Answer: E Learning Outcome: 10.5 Global 35) What is the electron geometry if you have 4 electron groups around the center atom? A) linear B) trigonal planar C) tetrahedral D) trigonal bipyramidal E) not enough information Learning Outcome: 10.5 Global 36) What is the electron geometry if you have 2 electron groups around the center atom? A) linear B) trigonal planar C) tetrahedral D) trigonal bipyramidal E) not enough information Answer: A
Learning Outcome: 10.5 Global 37) What is the electron geometry if you have 3 electron groups around the center atom? A) linear B) trigonal planar C) tetrahedral D) trigonal bipyramidal E) not enough information Answer: B Learning Outcome: 10.5 Global 38) What is the molecular geometry if you have 3 single bonds and 1 lone pair around the central atom? A) bent B) linear C) tetrahedral D) trigonal pyramidal E) not enough information Learning Outcome: 10.5 Global 39) What is the molecular geometry if you have 4 single bonds around the central atom? A) bent B) linear C) tetrahedral D) trigonal pyramidal E) not enough information Learning Outcome: 10.5 Global 40) What is the molecular geometry if you have a double bond, a single bond and 1 lone pair around the central atom?
A) bent B) linear C) tetrahedral D) trigonal pyramidal E) not enough information Answer: A 41) What is the molecular geometry of ozone, O3? A) bent B) linear C) tetrahedral D) trigonal pyramidal E) not enough information Answer: A 42) Which of the following compounds would have a linear molecular geometry? 1. N2 2. H2S 3. CO2 A) 1 and 2 only B) 1 and 3 only C) 2 and 3 only D) 1,2 and 3 E) neither 1, 2,or 3 Answer: B 43) What is the molecular geometry of carbon dioxide,? A) bent B) linear C) tetrahedral
D) trigonal pyramidal E) not enough information Answer: B 44) What is the molecular geometry of PH3? A) bent B) linear C) tetrahedral D) trigonal pyramidal E) not enough information 45) What is the molecular geometry of SiH4? A) bent B) linear C) tetrahedral D) trigonal pyramidal E) not enough information Learning Outcome: 10.5 Global 46) What is the molecular geometry of CCl4? A) bent B) linear C) tetrahedral D) trigonal pyramidal E) not enough information 47) What is the molecular geometry of SCl2? A) bent
B) linear C) tetrahedral D) trigonal pyramidal E) not enough information Answer: A 48) What is the molecular geometry of NH4+? A) bent B) linear C) tetrahedral D) trigonal pyramidal E) not enough information Learning Outcome: 10.5 Global 49) The electron geometry and the molecular geometry of ammonia (NH3) are, respectively: A) trigonal planar, bent. B) tetrahedral, tetrahedral. C) tetrahedral, trigonal pyramidal. D) tetrahedral, bent. 50) The electron geometry and the molecular geometry of water are, respectively: A) trigonal planar, bent. B) tetrahedral, tetrahedral. C) tetrahedral, trigonal pyramidal. D) tetrahedral, bent.
Learning Outcome: 10.5 Global 51) Which of the following has a tetrahedral electron geometry and a trigonal pyramidal molecular geometry? A) Br2O B) GeH4 C) SO2 D) PF3 Diff: 3 Var: 1 Page Ref: 10.7 52) Which term matches the definition: A separation of charge within a bond? A) coulombic attraction B) dipole moment C) pure covalent D) nonpolar covalent E) electronegativity Answer: B Learning Outcome: 10.6 Global 53) The elements with the highest electronegativity values tend to be found in the: A) upper right-side of the periodic table. B) lower right-side of the periodic table. C) upper left-side of the periodic table. D) lower left-side of the periodic table. E) center of the periodic table. Answer: A Diff: 1 Var: 1 Page Ref: 10.8 Learning Outcome: 10.6 Global
54) Which term matches the definition: The ability of an element to attract electrons within a covalent bond? A) coulombic attraction B) dipole moment C) polar covalent D) nonpolar covalent E) electronegativity Answer: E Learning Outcome: 10.6 Global 55) Which molecule listed below has a nonpolar covalent bond? A) NaCl B) H2O C) H2 D) all of the compounds E) none of the compounds Learning Outcome: 10.6 Global 56) Which molecule listed below has a polar covalent bond? A) NaCl B) H2O C) H2 D) all of the compounds E) none of the compounds Answer: B Learning Outcome: 10.6 Global 57) Which molecule listed below is a polar molecule? A) NH3 B) H2O C) HCN D) all of the compounds E) none of the compounds
Learning Outcome: 10.6 Global 58) Which substance listed below is a polar molecule? A) NH4+ B) Cl2O C) SiCl4 D) all of the compounds E) none of the compounds Answer: B Learning Outcome: 10.6 Global 59) Which molecule listed below is a nonpolar molecule? A) CCl4 B) CO2 C) BH3 D) all of the compounds E) none of the compounds Learning Outcome: 10.6 Global 60) Which compound listed below will dissolve in water? A) CCl4 B) SiO2 C) NH3 D) all of the compounds E) none of the compounds Learning Outcome: 10.6 Global 61) Which compound listed below will dissolve in NH3?
A) H2S B) CO2 C) O2 D) all of the compounds E) none of the compounds Answer: A Learning Outcome: 10.6 Global 62) Which compound listed below will dissolve in carbon tetrachloride, CCl4? A) NaCl B) CS2 C) NH3 D) all of the compounds E) none of the compounds Answer: B Learning Outcome: 10.6 Global Outcome: G2
63) Which of the following statements is TRUE for the covalent molecule HCl? A) Chlorine is more electronegative and the shared electron pair is likely to be found on the hydrogen atom. B) Chlorine is more electronegative and the shared electron pair is likely to be found on the chlorine atom. C) Hydrogen is more electronegative and the shared electron pair is likely to be found on the hydrogen atom. D) Hydrogen is more electronegative and the shared electron pair is likely to be found on the chlorine atom. Answer: B Learning Outcome: 10.6 Global 64) Which of the following statements about the water molecule is TRUE? A) A water molecule has two dipole moments and they cancel each other. B) A water molecule is symmetrical and therefore is nonpolar. C) A water molecule is asymmetric and therefore is polar. D) The electronegativities of hydrogen and oxygen are equal and therefore a water molecule is nonpolar. Learning Outcome: 10.6 Global 65) Which of the following statements are TRUE about the BF3 molecule? A) BF3 has a trigonal planar molecular geometry. B) BF3 violates the octet rule for the central atom. C) BF3 is nonpolar. D) All of the above statements are true. E) None of the above are true. Global
Learning Outcome: 10.6 66) The electronegativity value for N is 3.0 and that for O is 3.5. Based on these values, which of the following statements is TRUE about the compound NO? A) NO is an ionic compound. B) NO is a pure covalent compound. C) NO is a polar covalent compound. D) There is not enough enough information to determine the nature of NO. E) None of the above statements is true. Learning Outcome: 10.6 Global 67) The electronegativity value for Mg is 1.2 and the value for O is 3.5. Based on these values, what type of bond is expected for a compound formed between Mg and O? A) ionic B) pure covalent C) polar covalent D) not enough information Answer: A Learning Outcome: 10.6 Global 68) Consider the following electronegativity values: Which molecule below would you expect to have the more polar bond? A) H2 B) Cl2 C) F2 D) HCl E) HF Global
Answer: E Learning Outcome: 10.6 69) Which compound below is a polar molecule AND has a linear molecular geometry? A) CO B) CO2 C) CH4 D) H2O Answer: A Learning Outcome: 10.6 Global Outcome: G7 70) How does soap work? A) Soap works by breaking grease molecules into smaller molecules that dissolve in water. B) Soap works by making water into a nonpolar liquid which grease can dissolve in. C) Soap works by having a polar end and a nonpolar end which allows the water and oil to interact indirectly. D) Soap works by having a polar end which attaches to the grease molecule and polarizes it and turns the grease molecule into another soap molecule. This is a chain reaction. Learning Outcome: 10.6 Global 10.3 Algorithmic Questions 1) How many lone electron pairs does the ClO (-1 charged) polyatomic anion have? A) one B) three Global
C) six D) two Diff: 2 Var: 4 Page Ref: 10.5 Global
2) When a molecule has four electron groups with none of them lone pairs, the molecular geometry will be: A) linear B) bent C) trigonal pyramidal D) tetrahedral Diff: 1 Var: 5 Page Ref: 10.7