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Entry Task: Nov 27 th Block 1

Entry Task: Nov 27 th Block 1. Sign off Ch. 11-13 Review ws. Agenda. Discuss Ch. 11-13 review ws Clicker review on Ch. 11-13 Ch. 11-13 Exam- Next block. I can…. Ch. 11 Distinguish the type of Intermolecular forces that exist between substances.

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Entry Task: Nov 27 th Block 1

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  1. Entry Task: Nov 27th Block 1 Sign off Ch. 11-13 Review ws

  2. Agenda • Discuss Ch. 11-13 review ws • Clicker review on Ch. 11-13 • Ch. 11-13 Exam- Next block

  3. I can… Ch. 11 • Distinguish the type of Intermolecular forces that exist between substances. • Explain the relationships between a substances physical properties and IMF. • Describe how the IMF can affect the vapor pressure • Explain phase diagrams in terms of energy and phase changes

  4. I can… Ch. 13 • Explain the components and physical/chemical processes of a solution • Describe and interpret solubility curves of a substance. • State the factors that affect the solubility of a solute in solution. • Express a concentration of a solution in different ways- %, ppm, mole fraction, Molarity, & Molality • Explain how colligative properties affect the physical properties of a solution.

  5. Discuss Ch. 11-13 review

  6. Which force below is the strongest intermolecular attractive force? Hydrogen bonding Ion-dipole forces Dipole-dipole forces London dispersion forces 0 of 30

  7. Which force below increases in strength as the molecular weight of the compound increases? Hydrogen bonding Ion-dipole forces Dipole-dipole forces London dispersion forces 0 of 30

  8. Which compound below is not capable of forming hydrogen bonds? CH4 NH3 H2O d. HF 0 of 30

  9. Which compound below has the highest boiling point? H2O H2S H2Se H2Te 0 of 30

  10. Which element below has the highest boiling point? Kr F2 Cl2 Br2 0 of 30

  11. Which substance below has a greater density in its liquid state than in its solid state? Iron Glass Water Carbon dioxide 0 of 30

  12. The resistance of a liquid to flow is called the _______ of the liquid. density viscosity potential energy flow rate 0 of 30

  13. The energy required to cause a liquid to boil is called the _______ of the liquid. boiling point freezing point heat of vaporization heat of fusion 0 of 30

  14. Isopropyl alcohol feels cool to the touch because it has an (X) heat of (Y). a. X = exothermic, Y = vaporization X = endothermic, Y = vaporization X = exothermic, Y = fusion X = endothermic, Y = fusion 0 of 30

  15. When heat is added to ice at zero degrees Celsius, what will happen? The temperature will increase. The temperature will decrease. The temperature will not change. A supercritical fluid will form. 0 of 30

  16. The highest temperature at which a substance can exist in its liquid state is called its _______ point. boiling freezing triple critical 0 of 30

  17. The temperature and pressure at which all three phases exist simultaneously is called the _______ point of a substance. boiling freezing triple critical 0 of 30

  18. At high altitudes, the boiling point of water is 100 degrees Celsius. b. greater than 100 degrees Celsius. less than 100 degrees Celsius. equal to its freezing point. 0 of 30

  19. Substance X has a boiling point of 150 degrees F and a freezing point of 15 degrees F. The condensation point of X is 150 degrees F. is 15 degrees F. is 165 degrees F. is 135 degrees F. 0 of 30

  20. The rule of “like dissolves like” refers to similarities between _______ of miscible liquids. molecular weights shapes intermolecular attractive forces densities 0 of 30

  21. Which of the following compounds is miscible with water? CH3OH CH4 C6H6 CH3CH2OCH2CH3 0 of 30

  22. Which of the compounds below is the LEAST miscible with water? CH3OH CH3CH2OH CH3CH2CH2OH CH3CH2CH2CH2OH 0 of 30

  23. _______ Law says that the solubility of a gas in a liquid increases as the pressure of the gas increases. Boyle’s Charles’s Henry’s Raoult’s 0 of 30

  24. _______ Law says that the vapor pressure of a solution is proportional to the mole fraction of the solvent. Boyle’s Charles’s Henry’s d. Raoult’s 0 of 30

  25. The molality of a solution is defined as the amount of solute (in moles) divided by the volume of the solution (in liters). mass of the solvent (in kilograms). mass of the solution (in kilograms). total number of moles. 0 of 30

  26. In general, as the temperature of a solution increases, the solubility of a gaseous solute increases. decreases. remains unchanged. varies from gas to gas. 0 of 30

  27. What is the freezing point of a 2.00 m aqueous solution of sucrose? The value of Kf for water is 1.86 degrees C/molal. –3.72 degrees C –1.86 degrees C +1.86 degrees C +3.72 degrees C 0 of 30

  28. A 0.100 molal solution of which compound below will have the lowest freezing point? NaCl CaCl2 KI LiNO3 0 of 30

  29. How did we do??

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