Mixed Review 2nd 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

• 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

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

Question Set 3

• What is my shape and polarity?

• Q9. CH3F• Q10. HOB• Q11. NF3

• Q12. SF2

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

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

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

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

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.

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?

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

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

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?

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?

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

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. IIP has 5 VE 3 alone 3 bonds• 15. IIP can’t form four bonds• 16. III and IV O and F more electronegative

Answer Set 5/6

• 17. I Solids have strong bonds• 18. I and IISolids/liquids compact• 19. III Gases have low density• 20. IILiquids 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

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

Answer Set 9/10

• 33. 1.01325 kPaSet 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

Answer Set 11/12

• 41. 4 mols1 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

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