CHEM133 Week 11 Lesson 5 Quiz_ Answered 100% all correct_ Latest Updated 2025/26.

CHEM133 Fall 2025 Week 11 Lesson 5 Study Questions 2 1. For which of these molecules does the best Lewis structure have two or more equivalent resonance structures? CNO– CO2 SCN– HCO – – 3 2. Which of the elements listed below is most likely to exhibit an expanded octet in its compounds? N S Na C O 3. How many double and single bonds are in the resonance form for SO2 in which the formal charges on each atom are zero? Each of these choices is possible no single bonds and two double bonds one single bond and one double bond two single bonds and no double bonds 4. How many lone pairs of electrons are on the Xe atom in XeF6? NCHEM133 Fall 2025 Week 11 Lesson 5 Study Questions 3 0 1 2 5. The electron configuration of a particular diatomic species is (σ2s)2(σ*2s)2(σ2p)2(π2p)4(π*2p)4. What is the bond order for this species? 1.0 2.5 2.0 0.5 1.5 6. Which of the following diatomic molecules would the bond order become greater if an electron is removed? B2 P2 C2 Na2 F2 7. Each of the three resonance structures of NO3– has how many lone pairs of electrons? Question 7 options:CHEM133 Fall 2025 Week 11 Lesson 5 Study Questions 5 2 9 10 7 8 13 8. The hybridization of the central atom in XeF + is: sp3d sp sp3d2 sp2 sp3 9. The hybridization of the nitrogen atom in the cation NH + is: sp3d sp sp3 sp2 10. Which description fits the substance that has the following MO configuration? (σ1s)2(σ1s*)2(σ2s)2(σ2s*)2(σ2p)2(π2p)2CHEM133 Fall 2025 Week 11 Lesson 5 Study Questions paramagnetic with three unpaired electrons diamagnetic with zero unpaired electrons paramagnetic with four unpaired electrons paramagnetic with one unpaired electron paramagnetic with two unpaired electrons 11. When comparing Be2 and H2: I. Be2 is more stable because it contains both bonding and antibonding valence electrons. II. H2 has a higher bond order than Be2. III.H2 is more stable because it only contains 1s electrons. IV. H2 is more stable because it is diamagneti c, whereasCHEM133 Fall 2025 Week 11 Lesson 5 Study Questions 2 Be2 is paramagnet ic. II, III II, III, IV III only III, IV I, II 12. How many lone pairs are on the Br atom in BrF -? 2 1 3 0 13. Regarding boron trifluoride, which of these is TRUE? molecular geometry is trigonal planar the central atom does not obey the octet rule all of these are true it is not polar 14. Geometrically tetrahedral means that the electron groups have what angle? 120°CHEM133 Fall 2025 Week 11 Lesson 5 Study Questions 90° 180° 109.5° 15. Draw the Lewis structure for the carbonate polyatomic ion. How many valence electrons does it have? 18 26 22 24 23 16. If you were to use Lewis theory to predict the formula for the compound between potassium and sulfur, it would most likely be Question 16 options: KS3 KS KS2 K2S 17. According to Lewis dot theory, what types of electron pairs would you find surrounding the central atom of the nitrite ion? two bonding and two unshared pairs of electrons. three bonding and one unshared pairs of electrons.CHEM133 Fall 2025 Week 11 Lesson 5 Study Questions two bonding and one unshared pair of electrons. one bonding and three unshared pairs of electrons. 18. Regarding water, which of these is TRUE? two dipole moments are present and their effects are cancelled by one another it is not symmetrically shaped as a molecule and thus is polar. it is nonpolar it has a tetrahedal molecular geometry 19. Use Lewis theory to draw the structure of the compound containing 1 carbon and 4 chlorine atoms. What would you find surrounding the central atom of this ion? Question 19 options: 2 double bonds. no double bonds. 1 double bond. 1 triple bond. 20.We learned in this lesson that there are different types of bonds based on electronegativity. One bond type is known as polar covalent. Which choice below has this bond type? H2 NaCl H2O all of the compoundsCHEM133 Fall 2025 Week 11 Lesson 5 Study Questions none of the compounds 21. Some atoms are better at attracting electrons compared to others. Which term below best describes that? electronegativity non-polar covalent coulombic attraction polar covalent dipole moment 22. If the center atom has a double bond, a single bond, and 1 lone pair around it, what type of molecular geometry is present? bent trigonal pyramidal tetrahedral linear 23. If the center atom has three groups of electrons around it, what type of electron geometry is present? trigonal planar trigonal bipyramidal linear tetrahedralCHEM133 Fall 2025 Week 11 Lesson 5 Study Questions 24. Draw the structure of phosphorus trihydride according to VSEPR theory. What would be its associated molecular geometry? linear tetrahedral bent trigonal pyramidal 25. Draw the structure of ozone according to VSEPR theory. What would be its associated molecular geometry? tetrahedral trigonal pyramidal linear bent