Name: Class: Date: FINAL EXAM REVIEW I will provide all of the same sheets I provided on the quizzes this semester. True/False Indicate whether the statement is true or false. 1) Colligative properties depend on the identity of the solute. 2) True or False. Carbon dissolved in iron is an example of a solid solution of steel. 3) All compounds with polar covalent bonds are polar molecules. 4) Electrons are shared equally between two atoms in a polar bond. 5) True or False. It is possible for molecules to be attracted by two different types of intermolecular forces. 6) Liquids expand and contract in response to temperature changes much more easily than gases and solids. 7) The Kinetic Theory of Matter assumes that gas particles retain all kinetic energy when they collide with each other or the walls of their container. 8) Electrons are shared equally between two atoms in a polar bond. Multiple Choice Identify the choice that best completes the statement or answers the question. 9) This type of heterogeneous mixture has intermediate size particles. a) suspension b) colloid c) solution 10) The tyndall effect is used to differentiate a. a) suspension from a colloid b) suspension from a solution c) colloid from a solution 11) A(n) solution is formed when a saturated solution is formed at high temperature, then slowly cooled and the excess solute stays dissolved. a) unsaturated b) saturated c) supersaturated 12) Using the like dissolves like rule, which substance below is most likely to dissolve in water? a) I 2 b) CH 4 c) Al(NO 3 ) 3 13) Adding a solute to a solvent lowers the solvent s vapor pressure.why does this happen? a) The solute particles form a giant molecule that cannot be passed by the solvent molecules. b) The solute particles break into smaller pieces and bond to the water molecules. c) The solute particles prevent the solvent particles from escaping into the gas phase. 1
Name: 14) 15) The pressure of a liquid in equilibrium with its liquid is referred to as. a) vapor pressure b) boiling point elevation c) freezing point depression When a solid is dissolved in a liquid, the vapor pressure of the liquid because the molecules of the solvent are blocked by the solute from evaporating. a) is increased b) is decreased c) remains the same 16) How does the freezing point of a sugar solution compare with the freezing point of pure water? a) The pure water will freeze at a higher temperature than the sugar solution. b) The pure water will freeze at a lower temperature than the sugar solution. c) The pure water and sugar solution will freeze at the same temperature. 17) Which substance below will affect the colligative properties of a solution the most? a) NaCl b) CaCl 2 c) Al 2 (NO 3 ) 3 18) Which substance below would have the least affect on colligative properties of a solution? a) KCl b) MgBr 2 c) FeCl 3 19) Which substance below would have the greatest affect on freezing point depression of a solution? a) MgCl 2 b) Al(OH) 3 c) SnBr 4 20) Which statement below is TRUE about solutions? a) Solute will not come out of the solution upon standing. b) Solute can be filtered from the solution. c) Solute will scatter light in Tyndall effect. 21) What is the solvent in a solution of potassium chloride and water? a) potassium b) potassium chloride c) water 22) What does a hydration shell prevent? a) The hydration shell prevents crystals from dissolving in a solvent. b) The hydration shell prevents ions from reconnecting because water molecules completely surround the ion. c) The hydration shell prevents water molecules from surrounding ions. 23) What kind of solution is created when 20g of NaCl is dissolved in 100g of water at 80 C? a) unsaturated b) saturated c) supersaturated 24) In which type of solution will crystals eventually form and a saturated solution can be seen? a) unsaturated b) saturated c) supersaturated 25) The solubility of sucrose molecules in water is due to. a) sucrose being nonpolar and water being polar b) hydrogen bonding between sucrose molecules and water molecules c) sucrose being ionic and water being polar 26) Which solute below will not dissolve in alcohol(ch 3 CH 2 CH 2 CH 2 OH)? a) CaCl b) Br 2 c) NH 3 d) CH 4 2
Name: 27) Identify the type of reaction shown by this chemical equation: Al + HCl AlCl 3 + H 2 a) single replacement b) synthesis c) double replacement 28) Use the activity series to determine if this reaction will take place. Choose the correct answer below: ZnCl 2 + Na Activity Series for Metals Potassium Most Active Sodium Aluminum Zinc Copper Least Active a) NaCl + Zn b) NaZn + Cl c) No Reaction 29) The greater the electronegativity difference between two atoms bonded together, the greater the bond s. a) ionic character b) nonpolar character c) electron sharing 30) What kind of intramolecular forces are in CF 4? a) ionic b) covalent c) london dispersion forces d) hydrogen bonding 31) What type of intermolecular forces would take place between two F 2 molecules? a) hydrogen bonding b) dipole-dipole c) london dispersion forces d) ion-ion forces 32) What intramolecular forces occur between copper atoms? a) dipole-dipole b) ionic c) nonpolar covalent d) metallic 33) LiOH + MgBr 2 LiBr + Mg(OH) 2 If you start with ten grams of magnesium bromide, MgBr 2 how many grams of lithium bromide. LiBr will be produced? a) 9.43 g LiBr b) 86.85g LiBr c) 1736.9g LiBr 34) a) 56.7 g NH 3 b) 12.14g NH 3 c) 8.09g NH 3 3
Name: 35)! ""#$ %!&! '&& " ( # "! )*(" ) * +,-""! $ %. $.. a) 31.86g CO 2 b) 391.6g CO 2 c) 286.8g CO 2 36) /&))&! "" &&*) &! * ))&!"!*&!* ) 01 01 - a) 13.18g XeF 6 b) 21.5g XeF 6 c) 43.04g XeF 6 37) "!& *) "!& "!* 2$&. *%2$&*) 2$&. 2$&. a) 23.06g KClO 3 b) 46.03g KClO 3 c) 92.06g KClO 3 38) 39) $&!& &(&*%,- &(!& * & /$&$& / a) 200.3g AgCl b) 175.35g AgCl c) 99.01g AgCl &( "!, &(* &( *!. 34 435. 6 a) 25.02g AgBr b) 50.03g AgBr c) 100.23g AgBr 40) The temperature scale that has absolute zero as its zero point is the a) Celsius scale. b) Rankin scale. c) Kelvin scale. d) Fahrenheit scale. 41) What mass of oxygen will be required to react exactly with 190g of pentane, C 5 H 12 to produce carbon dioxide and water? C 5 H 12 + O 2 CO 2 + H 2 O a) 675g O 2 b) 284g O 2 c) 190 g O 2 4
Name: 42) Which two states of matter generally expand when heated? a) solids and liquids b) solids and gases c) liquids and gases 43) are defined as collisions in which not kinetic energy is lost. a) Perfect collisions b) Inelastic collisions c) Elastic collisions 44) is the average kinetic energy of of the particles in a material. a) Pressure b) Temperature c) Diffusion 45) How is the speed of a gas particle affected after is collides with the walls of its container? a) Speed is unaffected. b) Speed changes. c) Kinetic energy is lost. 46) The ability of gases to spread rapidly through other gases is explained by a) frequent inelastic collisions of the particles. b) the high density of gases. c) the high temperature of gases. d) constant random motion of particles. 47) Carbon monoxide reacts with oxygen to produce carbon dioxide. If 1.0 L of carbon monoxide reacts with oxygen at STP, how many liters of oxygen are required to react? CO(g) + O 2 (g) --> CO 2 (g) a) 1.0L O 2 b) 1.5L O 2 c) 0.5L O 2 48) Acetylene gas (C2H2) undergoes combustion to produce carbon dioxide and water vapor. How many liters of C2H2 are required to produce 75.0 L of CO2 C 2 H 2 (g) + O 2 (g) --> CO 2 (g) + H 2 O(g) a) 75 L C 2 H 2 b) 150 L C 2 H 2 c) 37.5 L C 2 H 2 49) If liquid carbon disulfide (CS2) reacts with 450 ml of oxygen to produce the gases carbon dioxide and sulfur dioxide, what volume of sulfur dioxide is produced? CS 2 (g) + O 2 (g) --> CO 2 (g) + SO 2 (g) a) 0.3 L SO 2 b) 3.0 L SO 2 c) 300 L SO 2 50) How many polar bonds are in the molecule NH 3? a) 1 b) 2 c) 3 51) Which element in the molecule NH 3 has a partial negative charge? a) N b) H c) both N and H d) neither, the molecule is nonpolar 52) Which type of intermolecular force requires the most energy to break? a) ion-ion b) dipole-dipole c) LDF 53) Which type of intermolecular force is strongest? a) LDF b) dipole-dipole c) ion-ion 5
Name: 54) Which substance below has the strongest intermolecular forces a) NH 3 b) MgCl 2 c) H 2 55) Nonpolar molecules are usually at room temperature. a) solids b) liquids c) gases 56) intermolecular forces are the strongest. a) Ion-ion b) Hydrogen bonding c) Dipole-dipole 57) Which substance below has the highest boiling point? a) CaO b) NaBr c) HCl 58) What type of intermolecular forces would take place between two molecules of CH 4? a) Hydrogen bonding b) Dipole-Dipole c) London Dispersion Forces d) polar covalent 59) The intramolecular forces in one molecule of CO 2 are. a) dipole-dipole b) ionic c) nonpolar covalent d) polar covalent 60) What kind of intramolecular forces are in CF 4? a) ionic b) polar covalent c) nonpolar covalent d) hydrogen bonding 61) What type of intermolecular forces would take place between two molecules of phosphorus trichloride? a) Hydrogen bonding b) Dipole-Dipole c) London Dispersion Forces d) polar covalent 62) What type of intermolecular forces would take place between two molecules of C 2 H 6? a) Hydrogen bonding b) Dipole-Dipole c) London Dispersion Forces d) polar covalent 63) Which type of bond is found in a molecule of Br 2? a) ionic b) polar covalent c) nonpolar covalent d) dispersion 64) Which type of bonding is the result of the transfer of electrons? a) ionic b) polar covalent c) nonpolar covalent d) dispersion 65) What kind of intramolecular forces take place in a molecule of PH 3? a) ionic b) polar covalent c) nonpolar covalent d) dipole-dipole 66) Which compound below has the highest boiling point? a) LiCl b) HCl c) Br 2 67) Which compound below has the highest boiling point? a) OF 2 b) CO 2 c) CaO 68) There are four factors that affect the rate of a reaction. Which statement below is TRUE about catalysts? a) A catalyst slows down the reaction rate by preventing particles from colliding with each other. b) A catalyst speeds up a reaction rate by being consumed in the reaction therefore increasing the number of particles that collide. c) A catalyst speeds up a reaction rate but does not get consumed in the reaction. 6
Name: 69) What does a high activation energy indicate about the rate of a reaction? a) A high activation energy indicates few collisions have enough energy to react so the reaction will proceed at a slow rate. b) A high activation energy indicates many collisions have enough energy to react so the reaction will proceed at a slow rate. c) A high activation energy indicates many collisions have enough energy to react so the reaction will proceed at a fast rate. 70) _ is the amount of substance present in a certain amount of space. a) Volume b) Mass c) Concentration 71) How can a water molecule be attracted to both a positive ion and a negative ion when dissolving an ionic compound? a) Because water is a liquid it can attract both positive and negative ions in a liquid. b) Because water is polar it has a slighltly positive end and a slightly negative end which attracts the positive and negative ions. c) A water molecule does not attract positive and negative ions. 72) Calculate the amount of energy in kilojoules needed to heat 25g of silver, Ag from 30 C to 50 C? specific heat of silver 0.235 J/g*C a).1175kj b) -117.5 kj c) 117.5 kj 73) How much heat in kilojoules is lost when a 640 g piece of copper cools from 375 o C, to 26 o C? (The specific heat of copper is 0.38452 J/g x o C) a) 85886 kj b) -85886 kj c) -85.886kJ 74) Which statement below is NOT true about activation energy? a) Activation energy is the amount of energy particles must have when they collide with each other. b) Activation energy is the initial amount of energy needed to initiate a reaction. c) Activation energy is the total amount of energy released or absorbed during a chemical reaction. 7
Name: 75) The graph below represents the pathway for the reaction A + B C + D What is the activation energy for the forward reaction? a) 35 kj b) 25 kj c) 10 kj 76) Which statement below is NOT true about endothermic reactions? a) Energy is a product of the reaction. b) Energy is absorbed c) The reaction vessel becomes cool. 77) The following chemical equation for the formation of water has a delta H of kj: 2H 2 + O 2 --> 2H 2 O + 483.6 kj. a) 483.6 b) -483.6 c) -241.5 78) The following chemical equation represents an change. a) endothermic b) exothermic 79) Which of the following is the correct equation for the exothermic combustion of CH 4? a) -802 kj + CH 4 + O 2 -----> CO 2 + H 2 O b) +802 kj + CH 4 + O 2 -----> CO 2 + H 2 O c) CH 4 + O 2 -----> CO 2 + H 2 O ; H = -802 kj 8
Name: 80) The graph below represents the pathway for the reaction A + B C + D What is the delta H for the reverse reaction? a) 35 kj b) 25 kj c) 10 kj 81) Choose the correct chemical equation for the forward reaction. a) N 2 + 3H 2 --> 2NH 3 + 92.4kJ b) N 2 + 3H 2 --> 2NH 3-92.4kJ c) N 2 + 3H 2 + 92.4kJ --> 2NH 3 82) Choose the correct chemical equation for the reverse reaction. a) 2NH 3 + 92.4kJ --> N 2 + 3H 2 b) 2NH 3-92.4kJ --> N 2 + 3H 2 c) 2NH 3 --> N 2 + 3H 2 + 92.4kJ 9