1. "Substance r" is more viscous as compared to "substance Z". "Substance I must have a greater integrity and/or quantit

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1. "Substance r" is more viscous as compared to "substance Z". "Substance I must have a greater integrity and/or quantity of intermolecular attractions, a) TRUE b) FALSE 2. Which of the following statements is/are TRUE concerning water? a) Water is a liquid at room temperature, b) Water has a high specific heat. c) Water has a liquid phase that is denser than the solid d) All of the above are true 3. Using the VSEPR model, the molecular geometry of the central atom in NO, is a) linear b) trigonal planar c) tetrahedral d) bent c) trigonal pyramidal 4. Using the VSEPR model, the molecular geometry of the central atom in CO, is a) lincar b) trigonal planar c) tetrahedral d) bent c) trigonal pyramidal 5. The major force between polar molecules is known as a) Van der Waal forces b) covalent forces c) dipole-dipole forces d) dispersion forces e) ionic forces 6. The strength of intermolecular attractions among molecules of a substance governs its state at room temperature. a) TRUE b) FALSE 7. The bond angle in water is _º the bond angle in ammonia is and the bond angle in CF. is a) 109.5; 109.5; 109.5 b) 109.5; 107: 104.5 C) 107: 107; 109.5 d) 107; 104,5; 109.5 e) 104.5;107: 109.5 8. Identify the total number of bonding pairs and lone pairs of electrons in the Lewis structure of N. a) 6 bonding pairs and 1 lone pair b) 4 bonding pairs and 2 lone pairs c) 3 bonding pairs and 2 lone pairs d) 2 bonding pairs and 1 lone pair e) 2 bonding pairs and 3 lone pairs 9. The carbon atom in CH is hybridized. 2) sp b) sp 10. The carbon atom in CO, is hybridized. a) sp b) sp c) sp 11. The carbon atom in CHO is hybridized. a) sp b) sp C) sp' 12. Which molecule or compound below contains a polar covalent bond? a) C;H b) NaF c) NHỊ d) NaCl e) O 13. Which of the following does NOT have multiple valid resonance structures? a) CO2 b) CIO:- °) NO; d) e) all of the above have resonance structures 14. A water molecule would be expected to have a a) 8+ on each H. b) 6- on the 0. c) 8-on cach H. d) both a and bare correct c) both b and care correct 15. A 2 M solution of KCI would require KCI in of KClay solution. a) 74.6 g:0.5L b) 2 mol; 1L c) 149.2 g; 1L d) all of the above c) none of the above 16. A 6% m/m solution of KCI would require KCl in of KCl solution A) 74.6 mol: 100 g B) 6 mol: 100g C) 6g: 100g D) all of the above e) none of the above 17. Which compound has the longest carbon-carbon bond length? a) CH.CH b) CH.CH c) HCCH 1x Which compound has the greatest carbon-carbon bond strength? a) CH.CH b) CH.CH c) HCCH c) sp

19. The Lewis structure of ammonium is shown below. What is the formal charge of any hydrogen atom? H HI -Н a)-1 b) 0 c)+1 d)-3 c)-2 20. The Lewis structure of ammonium is shown below. What is the formal charge of the nitrogen atom? H HNH a)-1 b) 0 c)+1 c)-2 21. Which of the following statements is TRUE? a) A covalent bond is formed by the sharing of electrons from one atom to another b) A pair of electrons involved in a covalent bond can be referred to as "lone pairs. c) Electrons shared are usually called core electrons as opposed to valence electrons. d) Single covalent bonds are stronger than double bonds. c) None of the above are true 22. Which of the following is the correct Lewis electron-dot structure for C2F4? a) c) d) 31-8-2-13 F-C-C-F 11 FF c) FC H 23. Which of the following is the correct Lewis electron-dot structure for CH2CH2? a) b) c) d) H H CCC C=c=c H-0----- Н H-H-8-c-o: H Н 24. Which of the following is the correct Lewis electron-dot structure for OCI2? b) )-ora: c) d) =O=C: c) <1-5-a: --- c) H-F d) H-CI e) C-H b) N: c) N: d) N: e) N. 25. Choose the compound with a bond that is most polar. a) H-1 b) H-Br 26. Which of the following represent the Lewis structure for Nitrogen? a) 27. Place the following in order of increasing bond length: C- FC-S C-ci a) C- SC-CI < C-F b) C-CI < C-FC-S c) C-F <C-S <C-CI d) C-F <C-CI < C-S e) C-S <C-F < C-CI 28. A hybridized carbon electron participates in a bond. a) sigma, o b) pi,

29. Which of the following is a correct Lewis electron-dot structure for NO3 a b) c) ) EEEE d) c) Y 30. Which statement is consistent with the data presented in these solubility curves? 100 90 NANO CC, 70 K00 NISO Solubility (s volute in 2001,0) му ) PANO KNO ka 30 20- KCIO, 10 - 00 1020 30 4050 20 90 100 Temperature a) At 40°C, 40 Nuci will not be able to completely dissolve. b) At 70°C, 70 g KNO, will not be able to completely dissolve. c) At 50°C, 60 g KCl will be able to completely dissolve. d) More Nas SO can dissolve in boiling water as compared to ice-cold water. c) Across all temperatures, more KCl can dissolve as compared to K.CO. 31. Using the VSEPR model, the molecular geometry of PCs is In this compound, phosphorous has no lone pair a) octahedral b) seesaw c) square pyramidal d) trigonal bipyramidal c) none of these 32. Using the VSEPR model, the electron group geometry of PCs is _. In this compound, phosphorous has no lone pair 3) octahedral b) soesaw c) square pyramidal d) trigonal bipyramidal c) none of these

CEC 33. Use the bond energies provided to estimate AH®rxn for: 2 Br2(1) + C2H2(B) - C2H2Br4(1) Bond Bond Energy (kJ/mol Br-Br 193 837 C-C 347 C-Br 276 C-H 414 a) +407 kJ b) -324 kJ c) +573 kJ d)-228 kJ 34. Boron (an exception to the octet rule) is stable with a valence of and BF, has a VSEPR molecular geometry described as In this compound, boron does not have any lone pair. a) three : trigonal planar b) six; octahedral c) three : octahedral d) six ; trigonal planare) six : trigonal pyramidal 35. What VSEPR electron group geometry would best describe the following Lewis structure? e) -648 kJ a) octahedral b) square planar c) square pyramidal d) seesaw e) trigonal pyramidal 36. What VSEPR molecular geometry would best describe the following Lewis structure? a a) octahedral b) square planar c) square pyramidal d) seesaw e) trigonal pyramidal 37. Liquid mercury within a cylinder is expected to have meniscus. a) a convex b) a concave c) no 38. Consider SO, and create the best Lewis structure. Calculate the formal charge on the sulfur atom. a)-2 b)-1 c) 0 d)+1 e) +2 39. Consider CO and create the best Lewis structure. Calculate the formal charge on the carbon atom. a)-2 b)-1 c) 0 d) +1 e) +2 40. Consider CO, and create the best Lewis structure. Calculate the formal charge on either oxygen atom. a) -2 b)-1 c) 0 d)+1 e) +2