Exam Accelerated Chemistry Study Sheet Chap12 Solids/Liquids/Intermolecular Forces

Size: px

Start display at page:

Download "Exam Accelerated Chemistry Study Sheet Chap12 Solids/Liquids/Intermolecular Forces"

Robert Harmon
5 years ago
Views:

1 Exam Accelerated Chemistry Study Sheet Chap12 Solids/Liquids/Intermolecular Forces Name /66 MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) Intermolecular forces are responsible for: 1) A) the shape of protein molecules. B) the existence of liquids and solids. C) the function of DNA. D) all of the above 2) Which state of matter has a high density and an indefinite shape? 2) A) gases B) liquids C) solids D) both solids and liquids 3) Which state of matter has a high density and a definite volume? 3) A) gases B) liquids C) solids D) both solids and liquids 4) Which state of matter has a low density and an indefinite volume? 4) A) liquids B) gases C) solids D) none of the above 5) Which state of matter has a low density and is easily compressed? 5) A) liquids B) gases C) solids D) none of the above 6) Which statement about surface tension is FALSE? 6) A) Molecules on the surface of the liquid have fewer molecules to interact with. B) Increased intermolecular forces increase surface tension. C) Items with densities lower than water will sink due to surface tension. D) Liquids tend to minimize their surface area. 7) The tendency of a liquid to minimize its surface area is called: 7) A) viscosity. B) surface tension. C) vaporization. D) capillary action. 8) The measure of the resistance to the flow of a liquid is called: 8) A) viscosity. B) condensation. C) sublimation. D) vapor pressure. 9) The change of a substance from a liquid to a gaseous form is called: 9) A) condensation. B) heat of fusion. C) dynamic equilibrium. D) vaporization. 10) A situation where two opposite processes are occurring at equal rates, and no net change is taking place, is called: A) dynamic equilibrium. B) vaporization. C) condensation. D) evaporation. 10) 1

2 11) Increasing the intermolecular forces of a liquid will do which of the following? 11) A) decrease the evaporation rate B) decrease the vapor pressure C) increase the surface tension D) all of the above 12) You can increase the vapor pressure of a liquid by: 12) A) using a nonvolatile compound. B) establishing dynamic equilibrium. C) increasing temperature. D) increasing the viscosity. 13) Which statement about boiling point is FALSE? 13) A) The boiling point is higher for compounds with a high viscosity. B) The boiling point of a compound is an absolute constant. C) The boiling point of a compound is higher for nonvolatile compounds. D) The boiling point is higher for compounds with strong intermolecular forces. 14) Evaporation is: 14) A) the opposite process as condensation. B) an endothermic process. C) increased by increasing temperature. D) all of the above 15) Which of the following statements is FALSE? 15) A) A puddle of water cools down as it evaporates. B) Evaporation is an endothermic process. C) As a liquid is converted into a gas, the liquid absorbs heat. D) All of the above are true. 16) The opposite process of freezing is: 16) A) condensation. B) boiling. C) evaporation. D) none of the above 17) The rate of vaporization of a liquid can be increased by 1. increasing the surface area 2. increasing the temperature 3. increasing the strength of the intermolecular forces A) 1 only B) 2 only C) 3 only D) 1 and 2 only 17) 18) Liquids that have high vapor pressure and low boiling points are called 18) A) abnormal liquids. B) viscous liquids. C) non-volatile liquids. D) volatile liquids. 19) The amount of heat required to melt one mole of a solid is called the: 19) A) heat of vaporization. B) heat of fusion. C) heating curve. D) none of the above 20) What is the heat of vaporization(kj/mol) if it takes 3,452 J of heat to completely vaporize 2.68 moles of the liquid at its boiling point? A) 12.2 B) 1288 C) D) ) 2

3 21) How many joules of heat are needed to completely vaporize grams of water at its boiling point? Given H vap = 40.6 kj/mol A) B) C) D) ) 22) How many kilojoules of heat are needed to completely vaporize 42.8 grams of C4H10O at its boiling point? Given Hvap = 26.5kJ/mol A) 9.49 B) 16.3 C) D) ) 23) Compare a small pot of water that is boiling vigorously to a large pot of water that is boiling gently. Which statement is TRUE? A) The vapor pressure of the liquid is greater than the pressure above the pot in each case. B) The large pot is boiling at a higher temperature than the small pot. C) The small pot is boiling at higher temperature than the large pot. D) Both pots are boiling at the same temperature. 23) 24) When sufficient quantity of heat has been added to reach the boiling point of a solution, what happens to any additional heat added? A) Additional heat is used to evaporate the liquid as the process is endothermic and requires continued input of energy. B) Additional heat alters the viscosity and the surface tension of the liquid which raises the vapor pressure and increases the boiling point which is why you must continually heat the solution. C) Additional heat raises the temperature of the liquid which in turn increases the rate at which boiling occurs. D) Additional heat lowers the intermolecular forces of the liquid which in turn increases the volatility of the liquid. 24) 25) What happens as you start to add heat to a solid substance? 25) A) When the melting point is reached, the thermal energy is sufficient to overcome intermolecular forces holding the components at their stationary points. B) Heating of the now formed liquid results in increasing the liquid temperature. C) Thermal energy causes the components of the solid to vibrate faster. D) all of the above 26) If we supply additional heat to a solid in equilibrium with its liquid at the melting point, the thermal energy added is used to: A) change solid to liquid. B) overcome the intermolecular forces that hold the solid together. C) raise the temperature of the solid above its melting point. D) change the liquid back to solid. 26) 27) When you make ice cubes: 27) A) it is an exothermic process. B) the process is referred to scientifically as sublimation. C) it is an endothermic process. D) the heat of vaporization must be removed. 3

4 28) Which statement is TRUE in describing what occurs when a solid melts to a liquid? 28) A) The process is endothermic and the heat of fusion is positive. B) The process is exothermic and the heat of fusion is positive. C) The process is exothermic and the heat of fusion is negative. D) The process is endothermic and the heat of fusion is negative. 29) How much energy does it take to melt a g ice cube? H fus = 6.02 kj/mol A) 108 kj B) 936 J C) 5.64 kj D) 102 kj 29) 30) How many grams of C4H10O can be melted by J? Given Hfus =7.27 kj/mol 30) A) 14.5 B) 20.4 C) 3.64 D) ) In northern climates, it is common to have a layer of frost form on cars that have been out overnight in the winter. During the day the frost layer disappears despite its temperature remaining below freezing. How? A) The frost cycles as does the saturation level of moisture in the winter air does from night to day. B) The frost sublimes directly from solid ice to water vapor. C) The frost melts due to the sun heating the surface of the car above the melting point. D) The frost evaporates due to the sun heating the solid. 31) 32) A mothball can change directly from its solid phase to its gaseous phase. This process is known as: A) melting. B) sublimation. C) condensation. D) deposition. 32) 33) Which intermolecular force is present in all molecules and atoms? 33) A) dipole-dipole forces B) dispersion forces C) hydrogen bonding D) none of the above 34) Which intermolecular force is due to the formation of an instantaneous dipole? 34) A) hydrogen bonding B) dipole-dipole forces C) dispersion forces D) none of the above 35) Which intermolecular force increases with increasing molar mass? 35) A) dispersion forces B) hydrogen bonding C) dipole-dipole forces D) none of the above 36) Which noble gas has the highest boiling point? 36) A) Ar B) Kr C) Xe D) Ne 4

5 37) Assuming that the molecules carbon monoxide (CO) and nitrogen (N2) have similar electron clouds, which statement below is TRUE? A) CO has the higher boiling point because it experiences dipole-dipole forces. B) Both CO and N2 must have the same boiling point. C) N2 has the higher boiling point because it experiences dipole-dipole forces. D) The N2 has the higher boiling point because it has greater dispersion forces. 37) 38) Which intermolecular force is common to all polar molecules but NOT nonpolar molecules? 38) A) dispersion forces B) dipole-dipole forces C) hydrogen bonding D) none of the above 39) Substance A is a molecular compound that dissolves in gasoline but not in water. The molecules of A are very likely: A) nonmetallic. B) polar. C) nonpolar. D) metallic. 39) 40) Which substance is most likely to be miscible with water? 40) A) CF4 B) CHCl3 C) Br2 D) CS2 41) Which statement below is FALSE? 41) A) A hydrogen bond is only 2-5% the strength of a typical covalent bond. B) A hydrogen bond is the strongest of the intermolecular forces. C) The large electronegativity difference between hydrogen and an F, O, or N atom is essential for the formation of a hydrogen bond. D) none of the above 42) Which molecule below has hydrogen bonding? 42) A) CH3CH2OH B) CH4 C) HCl D) H2 43) Which molecule below has hydrogen bonding? 43) A) H2O B) CH3OH C) HF D) all of the above 44) Which compound will have the highest boiling point? 44) A) CH3CH2OH B) CH4 C) CH3CH3 D) CH3C(O)CH3 45) Which substance would be expected to have the highest boiling point? 45) A) CO B) O2 C) N2 D) CO2 46) Which compound in liquid form will have the highest vapor pressure? 46) A) CH3C(O)CH3 B) CH3CH3 C) CH4 D) CH3CH2OH 47) Which intermolecular force is the strongest? 47) A) dipole-dipole forces B) X-forces C) dispersion forces D) hydrogen bonding 5

6 48) Which intermolecular forces are found in CCl4? 48) A) dispersion forces B) dipole-dipole forces C) X-forces D) hydrogen bonding 49) Which intermolecular forces are found in CO2? 49) A) hydrogen bonding B) dipole-dipole forces C) dispersion forces and dipole-dipole forces D) dispersion forces 50) Rank the compounds NH 3, CH 4, and PH 3 in order of increasing boiling point. 50) A) CH 4 < NH 3 < PH 3 B) NH 3 < CH 4 < PH 3 C) NH 3 < PH 3 < CH 4 D) CH 4 < PH 3 < NH 3 51) Which intermolecular force found in CCl2H2 is the strongest? 51) A) dipole-dipole forces B) dispersion forces C) hydrogen bonding D) none of the above 52) What types of forces exist between I 2 molecules? 52) A) dispersion forces B) hydrogen bonding C) dipole-dipole forces D) ion-dipole forces 53) Dry ice (solid CO2) is which type of solid? 53) A) molecular solid B) nonbonding atomic solid C) metallic atomic solid D) covalent atomic solid 54) NaCl is which type of solid? 54) A) covalent atomic solid B) metallic atomic solid C) molecular solid D) ionic solid 55) Silicon is which type of solid? 55) A) metallic atomic solid B) molecular solid C) covalent atomic solid D) nonbonding atomic solid 56) Copper is which type of solid? 56) A) molecular solid B) covalent atomic solid C) nonbonding atomic solid D) metallic atomic solid 57) Which atomic solid has the highest melting point? 57) A) Si B) Xe C) Fe D) Cu 58) What are the principal forces holding ice together? 58) A) dispersion forces only B) sea of electrons C) intermolecular forces D) electrostatic attraction 6

7 59) Why is water considered an unusual molecule? 59) A) Water can dissolve many polar and ionic compounds. B) No molecule of similar size is a liquid at room temperature. C) Water expands upon freezing. D) all of the above 60) The reason for many of the unique properties of water is: 60) A) moderate viscosity and expanding upon freezing. B) the ability to form hydrogen bonds. C) high surface tension and low volatility. D) all of the above 61) Which sequence correctly shows the increasing density of the three phases of water? 61) A) gas < liquid < solid B) liquid < gas < solid C) solid < liquid < gas D) gas < solid < liquid 62) How many kj of heat are needed to completely vaporize 3.30 moles of H2O? The heat of vaporization for water at the boiling point is 40.6 kj/mole. A) 12.3 B) 134 C) 2.26 D) ) 63) How many kj of heat are needed to completely vaporize 23.4 g of H2O? The heat of vaporization for water at the boiling point is 40.6 kj/mole. A) 31.2 B) 23.4 C) 52.8 D) ) 64) A 250 gram sample of water at the boiling point had 45.0 kj of heat added. How many grams of water were vaporized? Heat of vaporization for water is 40.6 kj/mole. A) B) 1.11 C) 16.2 D) ) 65) How many kj of heat are needed to completely melt 1.70 moles of H2O, given that the water is at its melting point? The heat of fusion for water is 6.02 kj/mole. A) 63.7 B) 10.2 C) 3.54 D) ) 66) How many kj of heat are needed to completely melt 17.3 g of H2O, given that the water is at its melting point? The heat of fusion for water is 6.02 kj/mole. A) 6.26 B) C) 5.79 D) ) 7

Chapter 10 Liquids, Solids, and Intermolecular Forces

Chapter 10 Liquids, Solids, and Intermolecular Forces The Three Phases of Matter (A Macroscopic Comparison) State of Matter Shape and volume Compressibility Ability to Flow Solid Retains its own shape