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Mixed Review 2 nd Semester Midterm

Mixed Review 2 nd Semester Midterm. Overview. Question sets 1 – 4: Chapter 9 material Question sets 5 – 7: Chapter 10 material Question sets 8 – 9 : Chapter 11 material Question sets 10 – 12: Chapter 12 material Question set 13: Chapter 13 material. Question Set 1.

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Mixed Review 2 nd Semester Midterm

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  1. Mixed Review 2nd Semester Midterm

  2. Overview • Question sets 1 – 4: Chapter 9 material • Question sets 5 – 7: Chapter 10 material • Question sets 8 – 9 : Chapter 11 material • Question sets 10 – 12: Chapter 12 material • Question set 13: Chapter 13 material

  3. Question Set 1 • I. K II. F III. C • Q1. Has a higher electronegativity than Si • Q2. Can form a covalent bond with O • Q3. Would form a metallic bond with Ag • Q4. Can form an ionic bond

  4. Question Set 2 • I. Ionic II. Covalent III. Metallic • Q5. Conducts electricity • Q6. Has a crystalline structure • Q7. Has a high boiling point • Q8. Share electrons as a community

  5. Question Set 3 • What is my shape and polarity? • Q9. CH3F • Q10. HOB • Q11. NF3 • Q12. SF2

  6. Question Set 4 • I. Si II. P III. O IV. F • Q13. Has 2 lone pairs and 2 unshared electrons in its lewis dot diagram • Q14. Forms up to 3 covalent bonds • Q15. As a central atom, can produce trigonal pyramidal shapes but not tetrahedral • Q16. Is assigned a negative charge when bound to the element N

  7. Question Set 5 • I. Solid II. Liquid III. Gas • Q17. Strongest IMF’s • Q18. Condensed state of matter • Q19. Small densities under normal conditions • Q20. Has mobile bonds with neighbors

  8. Question Set 6 • I. H II. N2 III. Ne IV. Xe • Q21. Effuses faster than fluorine gas • Q22. Has largest range of motion at equal temperatures • Q23. Has the most molecules at similar energy at room temperature • Q24. Changes speed the least when temperature changes

  9. Question Set 7 • Q 25. An absolute temperature scale • Q26. Process of a gas changing to a solid • Q27. This phase change takes more energy than evaporating • Q28. A separation technique for mixed liquids

  10. Question Set 8 • Q29. Ideal gases two main tenets • Q30. Conditions of STP • Q31. A needle with cross-sectional area of 0.020 in2 has a force of 2.0 N applied to it. What is the pressure exerted on the end of the needle? • Q32. An area in the USA which experiences less atmospheric pressure than here.

  11. Question Set 9 Q33. 1 Atm = 101.325 kPa. How many kPa is 0.010 atm’s? • Q34. A gas at STP has a volume of 1.0 L. If the temperature rises to 30 C, what is the new volume? • Q35. A gas at STP has a volume of 2.0 L. If the pressure is halved, what is the new volume? • Q36. A gas has its temperature doubled and pressure quadrupled. Its new volume is changed by what factor?

  12. Question set 10 • Q37. The empirical formula of Butane (C4H10) • Q38. 10 g of Oxygen gas has the same amount of molecules as 10 g of this element. • Q39. 3 mols of propane has this many molecules • Q40. 84 grams of Carbon is this many mols of carbon

  13. Question Set 11 • Q41. 1 mol propane produces ‘x’ mols water? • Q42. 2 mols propane and 9 mols oxygen produces ‘x’ mols carbon dioxide? • Q43. 3 mols propane and 320 grams oxygen produces ‘x’ grams water? • Q44. 66 grams propane and 192 grams oxygen produces ‘x’ grams carbon dioxide C3H8 + 5 O2 3 CO2 + 4 H2O

  14. Question Set 12 • Q45. Sugar is what % carbon • Q46. A substance is found to be 20% C and 80% O. What is the empirical formula? • Q47. A substance with molecular mass of 90 grams has the empirical formula of CH3. What is its molecular formula? • Q48. A substance of mass 8.0 grams is 6.4 g C and 1.6 g H. What is the empirical formula?

  15. Question Set 13 • Q49. 250 mL of a 2.0 M NaOH solution has how many grams of NaOH? • Q50. In order to dilute a 5.0 M NaCl solution of volume 125 mL to a M of 1.0 M, how much water needs to be added to the solution? • Q51. 60 grams of sugar are dissolved in 0.50 L of water. What is the M of sugar? • Q52. A 3.0 M KCl solution is diluted down to 1 part solution and 9 parts water. What is the new M?

  16. Answers Set 1/2 • 1. II and III Both F/C closer to top right • 2. II and III Both F/C are nonmetals • 3. I Only K is a metal • 4. I and II C does not participate in Ionic • 5. III Only metallic is conductor • 6. I Ionic is crystals • 7. I and III Salts/Metals have high BP • 8. III Metals share electrons as whole

  17. Answer Set 3/4 • 9. Tetrahedral/Polar Central: C • 10. Linear/Polar Central: B • 11. Trigonal Pyramidal/Polar Central: N • 12. Bent/Polar Central: S • 13. III O has 6 VE (2 pairs, 2 alone) • 14. II P has 5 VE  3 alone  3 bonds • 15. II P can’t form four bonds • 16. III and IV O and F more electronegative

  18. Answer Set 5/6 • 17. I Solids have strong bonds • 18. I and II Solids/liquids compact • 19. III Gases have low density • 20. II Liquids have weak bonds with neighbor • 21. I, II, III These three are smaller than F2 • 22. I H is lightest, big motion • 23. IV Xe is heavy, similar speeds • 24. IV Xe too big to change much

  19. Answer Set 7/8 • 25. Kelvin • 26. Deposition Phase change is called • 27. Sublimation S  G > L  G (energy) • 28. Distillation • 29. No IMF and No Volume • 30. 1 ATM and 0 C • 31. 100 PSI P = F/A. (2.0 N)/(0.020) • 32. Higher elevation Less air above

  20. Answer Set 9/10 • 33. 1.01325 kPa Set up a proportion • 34. 1.11 L Charles law, convert to K • 35. 4.0 L Boyles Law • 36. ½ V Combined Charles/Boyles • 37. C2H5 Empirical = Lowest ratio • 38. Sulfur Sulfur has same mass as O2 • 39. 1.8 x 1024 3 mols x (6 x 1023) • 40. 7 mols 84 g / 12 mm = 7 mols

  21. Answer Set 11/12 • 41. 4 mols 1 mol propane = 4 mols water • 42. 5.4 mols Oxygen = LR. 9/5 = x/3 • 43. 144 g For 43/44. grams  mols • 44. 158.4 g LR, mol to mol, mols Grams • 45. 40% C 6 C = 72. 72 g C / 180 mm = • 46. CO3 Divide by mm, find ratio of mols • 47. C6H18 mm empirical, proportion to 90 • 48. CH3 Divide by mm, find ratio of mols

  22. Answer Set 13 • 49. 20 g NaOH M = mols/L (2.0 M = x / 0.25) • x = 0.5 mols, convert to grams • 50. 500 mL Dilution equation, subtract initial 125 mL • 51. 2/3 M M = mols/L 60g sugar is 1/3 mol. 1/3 mols in ½ L is 2/3 M • 52. 0.30 M 3.0 M diluted by a factor of 10 is 0.30 M

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