final exam
Quiz yourself by thinking what should be in
each of the black spaces below before clicking
on it to display the answer.
Help!
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| Gas molecules are easily compressed because there is a lot of _________ between the particles | empty space
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| at a given temperature, all gas particles have the same_________ | average kinetic energy
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| The SI unit of pressure is the ___________ | Pascal
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| The total pressure of a mixture of gases is ____________the sum of the partial pressures of the gases in the mixture | equal to
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| the forces that hold water molecules together in a drop of water are ______________ | intermolecular
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| Attractions between oppositely charged regions of polar molecules are ____________forces | dipole-dipole
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| A liquid is less fluid than a gas because the particles of a liquid have_________intermolecular forces | greater
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| The electrical conductivities of metallic solids are _________ than the conductivities of molecular solids | better
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| Crystals are classified into seven crystal systems based on the ______________of their unit cells | angles and dimensions
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| An ice cube melts as it ________energy from its surroundings | absorbs
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| _______________is the point on a phase diagram that represents the temperature and pressure at which three phases of a substance can coexist | triple point
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| When vaportization occurs only at the surface of a liquid, the process is called__________________ | evaporation
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| In eleastic collisions between gas molecules, | no kinetic energy is lost
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| which of the following gases will diffuse fastest through xenon? a. hydrogen b. helium c. iodine d. carbon dixoide | helium
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| methane(CH4) effuses twice as fast as sexond gas. What is the molar mass of the second gas | 64 g/mol
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| standard atomspheric pressure will support a column of mercury in a barometer to what height | 760 mm
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| Force per unit area | pressure
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| The model describing the behavior of gases in terms of particles in motion | kinetic-molecular theory
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| an instrument used to measure atmospheric pressure | barometer
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| a measure of the average kinetic energy of the particles in a sample of matter | temperature
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| states that the total pressure of a mixture of gases is equal to the sum of the pressures of each gas in the mixture | dalton's law of partial pressure
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| collisions between gas particles in which no kinetic energy is lost | elastic collisions
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| the movement of one material through another | diffusion
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| states that the rate of effusion for a gas is inversely proportional to the square root of its molar mass | graham's law of effusion
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| a manometer contains a mixture of radon and helium with partial pressures of 33.0 kPa and 346.0 kPa, respectively. WHat is the total pressure? | 379 kPa
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| In Which substance is hydrogen bonding greatest | H2O
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| Drops of dew on a spider's web illustrate which of the following statements | water has high surface tension
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| A measure of the resistance of a liquid to flow | viscosity
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| A solid whose atoms, ions, or molecules are arranged in an orderly, geometric, three-dimensional structure | crystalline solid
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| A solid in which the particles are not arranged in a regular, repeating pattern | amorphous solid
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| which of the following processes releases energy? | sublimation
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| The temperature at which a crystalline solid becomes a liquid? | melting point
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| The pressure exerted by a vapor over a liquid | vapor pressure
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| The process by which a substance changes from a gas or vapor to a solid without first becoming a liquid | deposition
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| Temperature at which a liquid become a crystalline solid | freezing point
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| temperature at which the vapor pressure of a liquid equals the external or atomospheric pressure | boiling point
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| ___________________ law states that the volume and kelvin temperature of a contained gas are directly proportional if pressure is constant | charles
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| boyles law states that the pressure and volume of a contained gas are ___________proportional if temperature is constant | inversely
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| Assuming all other variables remain constant when you squeeze a balloon the pressure inside the balloon____________ | increases
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| Which equation shows Boyle's law | P1V1=P2V2 at constant temperature
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| Which equation shows Charles law | V1/T1=V2/T2 at constant pressure
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| THe pressure of a given mass of gas varies directly with the kelvin temperature when the volume remains constant | Gay-Lussac's law
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| ______________states that the volume of one mole of any gas at STP is 22.4 L | Avogrado's Principle
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| Which of the following are the conditions known as stand temperature and pressure (STP)? | 0 degrees C and 1.00 atm
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| In the combined gas law, this variable is always constant | number of moles of gas
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| which equation shows the combined gas law? | P1V1/T1=P2V2/T2
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| What volume will one mole of a gas occupy under standard temperature and pressure | 22.4 L
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| Equal volumes of gases at the same temperature and pressure contain equal numbers of particles | Avogrado's principle
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| Temperature, pressure, and volume are related for a fixed amount of gas | combined gas law
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| consider the ideal gas law and the ideal gas constant. What info do you need in order to determine the volume of the gas if you know the pressure, the temperature, and the ideal gas constant | the number of moles of the gas
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| real gases deviate most from ideal gas behavior at | extremely high pressures and low temperatures
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| Which equation shows the ideal gas law? | PV=nRT
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| What variable is mentioned in the ideal gas law that is assumed to be constant in the other gas laws? | number of moles
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| R represents the relationship among pressure, temperature, and number of moles of gas present | ideal gas constant
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| In determining the volume of a product from the volume of a reactant under constant conditions of temperature and pressure, which of the following steps is needed? | determine the mole ration of the gaseous substances
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| the volume occupied by 4 moles of Br2 at STP is___________. | 89.6L
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| Based on the following reaction, CH4(g) + 2CO2(g) -> CO2(g) + 2H2O(g), what is the volume ration of methane, CH4, to carbon dioxide, CO2? | 1:1
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| What information is NOT given by the coefficients in a balanced chemical equation? | the mass rations of reactants and products
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| A substance that dissolves in a solvent is said to be ________ in that solvent | soluble
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| Shaking and stirring __________ the rate of solvation by moving the solvated particles away from the contact areas more quickly | increases
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| the most common solvent among liquid solutions is___________ | water
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| nonpolar solutes are more soluble in nonpolar____________ | solvents
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| a supersaturated solution contains ________ dissolved solute than a saturated solution at the same temperature | more
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| A __________ solution contains a small amount of solute relative to the solute's solubility | dilute
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| A saturated solution is more _________ than an unsaturated solution | concentrated
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| Molar solutions are calculated and expressed in ____________ | moles per liter
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| THe colligative properties of a 1M aqueous solution sodium chloride (NaCl) will be ___________ the colligative properties of a 1M aqueous solution of potassium bromide (KBr) | same as
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| The _________ of the vapor pressure of a pure solvent when a solution is formed a colligative property | lowering
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| A 1m solution of a nonelectrolyte will have a _________ effect on the colligative properties of its solution than a 1m solution of an electrolyte will have on the colligative properties of its solution | lesser
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| ________________ is the temperature difference between a solution's and a pure solvent's boiling point | boiling point elevation
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| _________ are heterogeneous mixtures that contain particles between 1nm and 1000nm in diameter | colloids
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| After adding a small crystal of copper(II) sulfate to an aqueous solution of copper(II) sulfate, a large amount of copper sulfate precipitate forms. Which of the following terms describes the original solution | supersaturated solution
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| The overall energy change that occurs when a solution forms | heat of solution
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| the process of surrounding solute particles with solvent particles to form a solution | solvation
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| The statement that the solubility of a gas in a liquid is directly proportional to the pressure of the gas above the liquid | Henry's law
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| What term describes a solution in which the dissolved solute is in equilibrium with the undissolved solute | dilute solution
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| Which of the following compounds probides the most solute particles when complete dissociated in water? A. MgCl2 B. NaCl C. KBr D. Na3PO4 | Na3PO4
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| A measure of how much solute is dissolved in a specific amount of solvent or solution | concentration
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| The ration of the number of moles of solute in solution to the total number of moles of solute and solvent | mole fraction
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| The diffusion of solvent particles across a semipermeable membrane from areas of lower solute concentration to areas of higher solute concentration | osmosis
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| The amount of additional pressure caused by water molecules moving into a solution | osmotic pressure
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| the abilitity to be separated by paper filtration is a characteristic of which mixture? | suspensions
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| the erratic movement of colloid particles | brownian motion
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| the scattering of light by dispersed colloid particles | tyndall effect
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| in any chemical reaction, energy can be neither created no destroyed | law of conservation of energy
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| the ability to produce heat or do work | energy
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| energy stored in a substance because of its composition | chemical potential energy
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| heat required to raise the temperature of one gram of a substance by one degree celsius | specific heat
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| the SI unit of heat and energy | joule
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| the study of heat changes from chemical reactions and phase changes | thermochemistry
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| the change in enthalpy in a chemical reaction | enthalpy (heat) of reaction
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| standard state of a substance means the normal state of the substance at | 298K and 1 atm
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| The heat required to melt a solid substance | enthalpy of fusion
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| a balanced chemical equation that includes the physical states of all reactants and products and the energy change that accompanies the reaction | thermochemical equation
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| the enthalpy change for the complete burning of one mole of a substance | enthalpy (heat) of combustion
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| the heat of formation of a free element in its standard state is assigned a delta(triangle...change of)Hf degree symbol of exactly | 0.0kj
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| a measurement of the disorder in a system is the | entropy
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| the free energy of a reaction is a combination of the | enthalpy and entropy
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| Which of the following processes results in an increase in the entropy of the system? I. Removing 20 pennies from a box and arranging them face up on a table II. Sweeping the pennies from part I back into the box. III. Water freezing. IV. Water evaporatin | II and IV sweeping the pennies back into the box and water evaporating
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| states the spontaneous processes always proceed in such a way that the entropy of the universe increases | law of disorder
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| a physical or chemical change without outside intervention | spontaneous process
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| energy that is available to do work | free energy
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| +delta H | endothermic
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| + delta S | increase in disorder
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| +delta G | not spontaneous
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| -delta H | exothermic
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| -delta G | spontaneous
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| -delta | increase in order
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| A __________ is used to measure the amount of heat released or absorbed during a chemical process | calorimeter
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| Melting ice is an example of a spontaneous_________ process | endothermic
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| An exothermic reaction will always be spontaneous if the entropy ________ | increases
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| For the reaction NH4CL(s)-> NH3(g) + HCl(g), the entropy change is ___________ | positive
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| A(n) ___________ is used to increase the rate of a chemical reaction | catalyst
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| generally, increasing the temperature of a reaction ___________ the rate at which the reaction takes place | increases
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| reaction order for a reactant defines how the rate is affected by the____________ of the reactant | concentration
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| the reaction order for a chemical reaction is determined______________ using the mthod of initial rates | experimentally
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| In the expression Rate equals k[A], the reaction rate __________ when the concentration of A doubles | doubles
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| The complete sequence of ____________ that make up a complex reaction is called a reaction mechanism | elementary reactions
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| in a reaction, activiation energy is the amount of energy needed to | form the activated complex
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| Another name for an activated complex | transition state
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| Change in reactant concentration per unit time | reaction rate
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| States that atoms, ions, or molecules must collide in order to react | collision theory
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| Minimum amount of energy required to form the activated complex | activation energy
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| A catalyst that slows down, or inhibits, reactions rates | inhibitor
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| the rate of reaction between A and B is expressed as Rate equals k[A][B]2. To produce the greatest increas in the reaction rate | triple B while keeping A constant
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| To slow down the rate of a chemical reaction, you would | decrease the temperature of the reaction
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| Defines how a reaction rate is affected by the concentration of a reactant | reaction order
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| Mathematical relationship between the rate of a chemical reaction and the concentrations of the reactants | rate law
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| Numerical value that relates reaction rate and concentration at a given temperature | specific rate constant
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| The rate-determining step in a complex chemical raction is determined by | the slowest elementary step
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| Identify the substance at position 1 of the energy level diagram above | reactants
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| Identify the substance at position 2 of the energy level diagram above | intermediates
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| Identify the substance at position 3 of the energy leveel diagram above | activated complex
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| Identify the substance at position 4 of the energy level diagram above | products
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| chemical equilibrium is a _____ state, in which the concentrations of reactants and products are constant but not necessarily equal | dynamic
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| In a____________ chemical equilibrium, the reactants and products are present in more than one physical state | heterogeneous
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| For the equilibrium expression Keq equals [PCl3][Cl2]/[PCl5], the _______ of the forward reaction is PCl5 | ractant
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| Raising the temperature of a chemical equilibrium causes the equilibrium to shift in the direction of the _______ reaction | endothermic
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| Adding oxygen gas to the chemical equilibrium 2SO2(g)+O2(g) <-> 2SO3(g) will shift the reaction to the | right
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| The best way to be certain that any chemical equilibrium will produce the largest amount of product is to keep removing product | (blank)
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| If an equilibrium reaction is started with only reactants then in time the concentrations of the reactants will | decrease
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| when an equilibrium product constant has a very high value, it means | there is a higher percentage of products than of reactants
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| A reversible reaction is | a reaction that can occur in both forward and reverse directions
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| this is the expression for the equilibrium constant for the reaction: CO(g) + H2O (g) <- -> CO2(g) +H2(g). | Keq equals [CO2][H2]/ {CO][H2O]
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| The value of any equilibrium constant is correct only at | a specific temperature
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| A state in which the forward and reverse reactions balancxe each other because they take place at equal rates | Le Chatelier's principle
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| The numerical value of the ratio of product concentrations to reactant concentrations, with the concentration of each reactant and product raised to the power corresponding to its coefficient in the balanced equation | equilibrium constant
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| Increasing the volume of the vessel containing the chemical equilibrium 2SO2 (g) + O2(g) <-> 2SO3(g) would | ch.18 number 14
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| What predicts that increasing the concentration of NH3 will shift the following reaction to the left? N2(g) + 3H2(g) <- -> 2NH3(g) | Le Chateliers principle
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| What will be the result if the volume of the reaction vessel is decreased for the reaction: H2(g) + I2 <- -> 2HI(g) | the equilibrium does not change
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| If a stress is applied to a system at equilibrium the system shifts in the direction that relieves the sress | Le Chateliers principle
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| A lesser amount of Al(OH)3 will dissolve in a solution of AlCl3 than in pure ware because | of the common ion effect
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| What can be determined if the ion product is compared to the solubility product constant | whether a substance will precipitate
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| An equilibrium constant for the dissolving of a sparingly soluble ionic compound in water | solubility product constnat
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| Bases taste | bitter
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| a(n)_______________ solution contains more hydroxide ions than it does hydrogen ions | basic
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| Who proposed the theory regarding acids and bases that states acids contain ionizable hydrogen atoms and bases contain hydroxide groups and produce hydroxide ions in solution | arrhenius
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| who proposed the theory regarding acids and bases that states an acid is a hydrogen-ion donor and a base is a hydrogen-ion acceptor | bronsted-lowry
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| the negative logarithm of the hydrogen ion concentration is | pH
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| ______________ are the products of a neutrailization reaction between a strong acid and a strong base | a salt and water
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| AN acid-base indicator changes color when which of the following is reached | a specific pH
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| A hydronium ion is a hydrated__________ion | hydrogen
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| NaOH is a strng base. The [OH-] of a .10M NaOH solution is | .10M
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| A solution of a salt of a strong acid and a weak base will be _______ | slightly acidic
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| When water self-ionizes__________ and hydroxide ions form | hydronium
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| The value of Kw at 298 K is _____e-14 | 1.0
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| A pH greater than 7 indicates a ______solution | basic
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| if the pH of a solution is 10 its pOH is_______ | 4
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| Buffers are solutions that resist changes in pH when _______amounts of acid or base are added | limited
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| Since nitric acid is a _________ acid, it completely ionizes in solution | strong
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| Which is the weakest acid: acetic, boric, hypobromous, iodic, nitrous, propanoic | boric
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| oxidation is the _______ of electrons by an atom | loss
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| sodium is the _______- agent in the folowing reaction: 2Na(S) + Cl2(g)-> SNaCl(s) | reducing
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| If the oxidation number of sulfer changes from +6 to 2, sulfur has been ________ | reduced
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| If oxidation occurs, reduction ________ occur | must also
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| When zinc metal reacts with chlorine gas, ________ is the oxidation half-reaction | Zn -> Zn 2+ + 2e-
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| In a redox reaction, electrons are | transferred from atom to atom
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| Which of the following types of reactions are always redox reactions? | single-replacement and combustion
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| THe process of reduction is the _________ of electrons by an atom | gain
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| When magnesium burns, it is oxidized. it is also____________ in the reaction | the reducing agent
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| When calcium reacts with oxygen, each calcium atom loses two electrons the oxidation number of calcium | increases by 2
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| The oxidation number of chromium can change from +6 to +3. For this change to occur, chromium ___________ extrons | gains 3
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| For one atom to gain electrons another must | lose electrons
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| A chemical reaction in which electrons are transferred from one atom to another is a | redox
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| Oxidation number of As in H3AsO4 | +5
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| Oxidation number of S in CaSO4 | +6
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| Oxidation number of Fe in Fe(NO3)2 | +2
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| Oxidation number of N in AlN | -3
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| Oxidation number of Cr in CrO4 2- | +6
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| a redox reaction will occur spontaneously if its cell standard potential is | positive
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| the two halves of an electrochemical cell are connected by a tube called a ___________ which allows ions to move between the halves | salt bridge
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| a redox reaction that occures spontaneously in an electrochemical cell ___________ electrical energy | produces
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| in the hydrogen-oxygen fuel cell, _________ is reduced | oxygen
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| the rusting of iron requires oxygen, water, and ________ ions | chapter 21 number 7
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| during the electrolysis of molten sodium chloride sodium ions are | reduced
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| a voltaic cell consisting of a moist, electrolytic paste inside a zinc shell | zinc-carbon dry cell
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| the electrode where oxidation takes place in an electrochemical cell | anode
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| one of the two main parts of an electrochemical cell where either oxidation or reduction takes place | half-cell
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| a device that converts chemical energy into electrical energy or electrical energy into chemical energy | electrochemical cell
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| the tendency of an electrode to gain electrons | reduction potentinal
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| electrode at which reduction takes place | cathode
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| the voltage measured between the electrod of a half-cell and the standard hydrogen electrode | standard reduction potential
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| the loss of metal due to a redox reaction of the metal with substances in the environment | corrosion
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| the coating of iron with a layer of zinc | galvanizing
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| why is the process of manufaction aluminum expensive | the purification process uses huge amounts of electrical energy
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| the use of electrical energy to cause a chemical reaction | electrolysis
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| a flow of charged particles such as electrons is called a | current
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| _______________ depend on reversible redox reactions | rechargable batteries
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| when copper is purified by electrolysis, the ________________- of the cell is a thin sheet of pure copper | cathode
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| ______________ produce electric energy by means of redox reactions that are not earily reversed | primary battery
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| _____________ are rechargeable and depend on reversible redox reactions for storage, computers, and cars | secondary battery
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| ________________ alkanes contain carbon atoms that are bonded to more than two otehr carbon atoms | branched-chain
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| all organic compounds contain the element | carbon
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| butane, pentane, and hexane are members of one ________________ | homologous series
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| a ____________ formula shows the structure of a hydrocarbon but saves space by not showing how the hydrogen atoms branch off the carbons atoms | condensed structural formula
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| heptane is an example of a ________ hydrocarbon | saturated
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| a hydrocarbon that has one or more triple covalent bonds between carbon atoms i called an___________ | alkyne
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| alkanes, alkenes, and alkynes are called _____________ compounds | alliphatic
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| isomers in which the atoms are bonded in different orders are known as _______________ | structural isomers
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| _______________isomers result from different arrangements of four different groups about the same carbon atom | optical
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| compounds that exist in right and left forms have a property called | chirality
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| isomers have the same molecular formula but different | molecular structures
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| organic compounds that contain benzene rings are called ___________compunds | aromatic
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| a carcinogen is a substance that causes | cancer
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| a straight chain alkane formula | CnH2n+2
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| hydrocarbons containe | carbon and hydrogen
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| in a branched alkane each branch attached to the main chain is called a | substituent group
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| choose the correct name for each of the following structures. CH3CH2CH2CH2CH3 | pentane
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| cyclohexane is an example of | a cyclic hydrocarbon
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| how many carbon atoms ar ein a straight chain alkyne with one triple bond and 16 hydrogen atoms | 9
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| CH3CH double CHCH2CH3 | 2-pentene
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| CH3CH2C triple CCH3 | 2-pentyne
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| in a polarized ligght, the light waves vibrate in | one plane
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| which substances are found in the residue collected at the bottom of a fractionating tower | paraffin, tar, asphalt
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| the boiling of petroleum to separate components is called | fractional distilllation
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| the molecular formula of a straight-chain alkene with six carbons atoms and one double bond is | C6H12
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| the structure of 3-chlorobutane would show four carbon atoms and ___________ of chlorine | one atom
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| the process called _________ breaks large alkanes from petroleum into smaller carbon compounds | cracking
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| _________ are responsible for the odors characteristic of dead, decaying organisms | amenes
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| because of their typically pleasant odors and tastes, ______ are often used in flagrances and flavorings | esters
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| the names of ketons end with suffix | -one
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| the name of aldehydes end with the suffix | -al
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| hydrogenation and hydration are both types of _________ reactions | addition
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| a reaction in which an alkyl halide is converted to an alkene, with the production of a hydrogen halide, is an example of a(n) ___________________ reaction | elimination
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| a dehydration reaction releases | water
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| in an organic molecule any atom or group of atoms that reacts in a certain way | functional group
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| organic compound containing fluorine, chlorine, bromine, or iodine | halocarbon
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| which of the following tend to be basic? ethers, amines, alcohols, amides | amides
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| ethanol with small amounts of noxious materials added | denatured alcohol
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| compound with an oxygen atom bonded to two carbon atoms | ether
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| the simplest carboxylic acid is commonly known as | formic acid
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| compound with a carbonyl group bonded to two carbon atoms | ketone
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| compound containing a carboxyl group | carboxylic acid
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| what is the structural formula of the monomer from which the polumer polyethylene is produced? | two carbon atoms double-bonded to each other and single-bonded to hydrogen atoms
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| large molecule consisting of many repeating subunits | polymer
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| a single unit molecule from which a polymer is made | monomer
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| an alpha particle has the composition of a helium__________ | nucleus
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| the loss of an aplha particle from an isotope causes its atomic number to __________________ | decrease by two
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| the mass of an atoms nucleus is always _________ the total mass of the nucleons composing it | less then
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| carbon-14 is used as a radiotracer in studies of photosynthesis because it has the same______ properties as stable carbon-12 | chemical
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| ____________ rays are particularly dangerous because they easily penetrate living tissue | gamma
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| the most penetrating form of nuclear radiation is | gamma rays
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| isotopes of atoms with unstable nuclei that emit radiation | radioisotope
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| one way to increase the stability of a nucleus with a 0.8: 1.0 neutron-to-proton ratio is to increase the number of | neutrons
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| in an atom, the strong nuclear force acts on | protons and neutrons
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| during the process of electron capture, an electron from outside the nucleus joins with a proton to form | a neutron
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| what is the symbol used for a neutron in balancing nuclear equations? | 1 over 0 n
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| a force that acts only on subatomica particles that are extremely close together | strong nuclear force
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| the area on a graph plotting neutrons and protons within which all stable nuclei are found | band of stability
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| another name for a proton or neutron | nucleon
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| a series of nuclear reactions beginning with an unstable nucleus and resulting in the formation of a stable nucleus | radioactive decay series
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|
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| an example of a transuranium element is | plutonium
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| the half-life of calcium-47 is about 5 days. starting with 64 g of this isotope, what would be the amount remaining after 20 days? | 4g
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| the process in which an atom of one element changes into an atom of another element | transmutation
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| a way of determining the age of very old objects using radioactive materials | radiochemical dating
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|
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| one advantage of a fusion raction over a fission reaction for the purpose of producing energy is that the fusion reaction | produces more energy per particle than does the fission reaction reaction
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| one product of all nuclear fission reactions is | energy
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| mass is lost or gained in | all chemical and nuclear reactions
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|
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| a chain reaction will NOT take place in a piece of uranium if | there are too few neutrons
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|
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| fusion reaction require | incredibly high temperatures
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|
||||
| the difference between the mass of a nucleus and the sum of its nucleons | mass defect
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|
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| reactors able to produce more fuel than they use | breeder ractor
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|
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| readiation damages | all kinds of cells
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|
||||
| one of the most serious problems surrounding the use of nuclear power plants is | finding a way to dispose of spent fuel rods
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|
||||
| a radioisotope that emits non-ionizing radiation and is used to signal the presence of an element of specific substance | radiotracer
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|
Review the information in the table. When you are ready to quiz yourself you can hide individual columns or the entire table. Then you can click on the empty cells to reveal the answer. Try to recall what will be displayed before clicking the empty cell.
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To hide a column, click on the column name.
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You may also shuffle the rows of the table by clicking on the "Shuffle" button.
Or sort by any of the columns using the down arrow next to any column heading.
If you know all the data on any row, you can temporarily remove it by tapping the trash can to the right of the row.
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