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A force that occurs between molecules is called:

A force that occurs between molecules is called:. 12.1. Intramolecular Intermolecular Molecular Covalent Ionic. A force that occurs between molecules is called:. 12.1. Intramolecular Intermolecular Molecular Covalent Ionic.

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A force that occurs between molecules is called:

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  1. A force that occurs between molecules is called: 12.1 Intramolecular Intermolecular Molecular Covalent Ionic

  2. A force that occurs between molecules is called: 12.1 Intramolecular Intermolecular Molecular Covalent Ionic

  3. A force that occurs between atoms within a compound might be: 12.2 Intramolecular Ionic Covalent All of the above Two of the above

  4. A force that occurs between atoms within a compound might be: 12.2 Intramolecular Ionic Covalent All of the above Two of the above

  5. Which pure compound has the highest total intermolecular forces per molecule at 25 °C? 12.3 Carbon dioxide Water Rubbing alcohol Table sugar Gasoline

  6. Which pure compound has the highest total intermolecular forces per molecule at 25 °C? 12.3 Carbon dioxide Water Rubbing alcohol Table sugar Gasoline

  7. Which property describes a molecular liquid? 12.4 The molecules are close together. The density is higher than its gas. It is not compressed easily. It assumes the shape of its container. All of the above

  8. Which property describes a molecular liquid? 12.4 The molecules are close together. The density is higher than its gas. It is not compressed easily. It assumes the shape of its container. All of the above

  9. Which property best describes a molecular solid? 12.5 The solid has a lower density than its gas. The solid has a lower average kinetic energy than its gas at the same temperature. The solid is easy to compress. The solid does not assume the shape of its container. All of the above

  10. Which property best describes a molecular solid? 12.5 The solid has a lower density than its gas. The solid has a lower average kinetic energy than its gas at the same temperature. The solid is easy to compress. The solid does not assume the shape of its container. All of the above

  11. Why doesn’t a paper clip sink when the clip is placed gently on water? 12.6 It is less dense than water. It is more dense than water. The repulsive forces override the attractive forces. There are strong intermolecular forces between the water and the metal. The molecules of water hold to each other and keep it from sinking.

  12. Why doesn’t a paper clip sink when the clip is placed gently on water? 12.6 It is less dense than water. It is more dense than water. The repulsive forces override the attractive forces. There are strong intermolecular forces between the water and the metal. The molecules of water hold to each other and keep it from sinking.

  13. Which of the following has the highest viscosity? 12.7 Oxygen gas Pancake syrup Running water Liquid helium Rubbing alcohol

  14. Which of the following has the highest viscosity? 12.7 Oxygen gas Pancake syrup Running water Liquid helium Rubbing alcohol

  15. The transformation from a liquid to a gas is called: 12.8 Condensation Evaporation Sublimation Vaporization Two of the above

  16. The transformation from a liquid to a gas is called: 12.8 Condensation Evaporation Sublimation Vaporization Two of the above

  17. What happens to the kinetic energy of gaseous water molecules during condensation? 12.9 It remains unchanged. It decreases. It increases. None of the above All of the above

  18. What happens to the kinetic energy of gaseous water molecules during condensation? 12.9 It remains unchanged. It decreases. It increases. None of the above All of the above

  19. Which of the following is the most volatile? 12.10 Gold Vegetable oil Water Motor oil Fingernail polish remover

  20. Which of the following is the most volatile? 12.10 Gold Vegetable oil Water Motor oil Fingernail polish remover

  21. What is the relationship between the external pressure and the boiling point of a compound? 12.11 The boiling point increases with increased pressure. The boiling point increases with decreased pressure. The boiling point decreases with increased pressure. The boiling point decreases with decreased pressure. Two of the above

  22. What is the relationship between the external pressure and the boiling point of a compound? 12.11 The boiling point increases with increased pressure. The boiling point increases with decreased pressure. The boiling point decreases with increased pressure. The boiling point decreases with decreased pressure. Two of the above

  23. What is the gas found within a bubble of boiling water? 12.12 Oxygen Water vapor Nothing Hydrogen Nitrogen

  24. What is the gas found within a bubble of boiling water? 12.12 Oxygen Water vapor Nothing Hydrogen Nitrogen

  25. Which of the following processes are exothermic? 12.13 Boiling Freezing Condensation Both 1 and 2 Both 2 and 3

  26. Which of the following processes are exothermic? 12.13 Boiling Freezing Condensation Both 1 and 2 Both 2 and 3

  27. Which of the following contains the most thermal energy? 12.14 5 grams of water at 100 °C 5 grams of water at 75 °C 5 grams of steam at 100 °C 5 grams of water at 0 °C 5 grams of ice at 0 °C

  28. Which of the following contains the most thermal energy? 12.14 5 grams of water at 100 °C 5 grams of water at 75 °C 5 grams of steam at 100 °C 5 grams of water at 0 °C 5 grams of ice at 0 °C

  29. What is the quantity of energy required to boil 45.5 g of liquid water at 100 °C at sea level? The molar heat of vaporization of water is 40.6 kJ/mol. 12.15 1.85 x 103kJ 1.12 kJ 103 kJ 2.52 kJ 40.6 kJ

  30. What is the quantity of energy required to boil 45.5 g of liquid water at 100 °C at sea level? The molar heat of vaporization of water is 40.6 kJ/mol. 12.15 1.85 x 103kJ 1.12 kJ 103 kJ 2.52 kJ 40.6 kJ

  31. What is the energy required to melt 4.50 mol of ice at 0 °C? The molar heat of fusion of water is 6.02 kJ/mol. 12.16 27.1 kJ 6.02 kJ 1.34 kJ 1.50 kJ 30.5 kJ

  32. What is the energy required to melt 4.50 mol of ice at 0 °C? The molar heat of fusion of water is 6.02 kJ/mol. 12.16 27.1 kJ 6.02 kJ 1.34 kJ 1.50 kJ 30.5 kJ

  33. Which statement is most likely true concerning an ice/water mixture kept at 0 °C? 12.17 The rate of freezing is faster. The rate of melting is faster. The ice will always melt. The water will always freeze. The rates of freezing and melting are equal.

  34. Which statement is most likely true concerning an ice/water mixture kept at 0° C? 12.17 The rate of freezing is faster. The rate of melting is faster. The ice will always melt. The water will always freeze. The rates of freezing and melting are equal.

  35. Which type of intermolecular force is the strongest? 12.18 Covalent Dipole–dipole Hydrogen bonding Ionic Dispersion

  36. Which type of intermolecular force is the strongest? 12.18 Covalent Dipole–dipole Hydrogen bonding Ionic Dispersion

  37. Which intermolecular force allows water to bead on a surface? 12.19 Ionic Dipole–dipole Hydrogen bonding Dispersion Covalent

  38. Which intermolecular force allows water to bead on a surface? 12.19 Ionic Dipole–dipole Hydrogen bonding Dispersion Covalent

  39. Which of the following has the highest boiling point? 12.20 CH3CH2CH3 CH3CH2NH2 CH3OCH3 CH4 CH3CH2OH

  40. Which of the following has the highest boiling point? 12.20 CH3CH2CH3 CH3CH2NH2 CH3OCH3 CH4 CH3CH2OH

  41. Which of the following has the least solubility in water? 12.21 CH3CH2CH3 CH3CH2NH2 CH3OCH3 H2O CH3CH2OH

  42. Which of the following has the least solubility in water? 12.21 CH3CH2CH3 CH3CH2NH2 CH3OCH3 H2O CH3CH2OH

  43. What type of intermolecular force causes today’s Saran Wrap to stick to itself? 12.22 Dipole–dipole Hydrogen bonding Dispersion Ionic Covalent

  44. What type of intermolecular force causes today’s Saran Wrap to stick to itself? 12.22 Dipole–dipole Hydrogen bonding Dispersion Ionic Covalent

  45. Arrange the following in order of increasing melting point (lowest first): CO2, Si, H2O, and NaCl. 12.23 NaCl, Si, CO2, H2O Si, NaCl, H2O, CO2 H2O, CO2, NaCl, Si CO2, H2O, NaCl, Si CO2, H2O, Si, NaCl

  46. Arrange the following in order of increasing melting point (lowest first): CO2, Si, H2O, and NaCl. 12.23 NaCl, Si, CO2, H2O Si, NaCl, H2O, CO2 H2O, CO2, NaCl, Si CO2, H2O, NaCl, Si CO2, H2O, Si, NaCl

  47. What type of crystalline solid is formed by potassium iodide? 12.24 Molecular Ionic Atomic Amorphous None of the above

  48. What type of crystalline solid is formed by potassium iodide? 12.24 Molecular Ionic Atomic Amorphous None of the above

  49. Which of the following is an example of an atomic solid? 12.25 C6H12O6 HCl S8 NaCl None of the above

  50. Which of the following is an example of an atomic solid? 12.25 C6H12O6 HCl S8 NaCl None of the above

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