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chemistry final exam review
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Chemistry
10th Grade
05/15/2012

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Term
According to the kinetic-molecular theory, particles of matter

a-have different colors
b-are in constant motion
c-are always fluid
d-have different shapes
Definition
B
Term
An ideal gas is a hypothetical gas...

a-made of motionless particles
b-whose particles have zero mass
c-that conforms to all the assumptions of the kinetic theory
d-not made of particles
Definition
C
Term
Unlike an ideal gas, in a real gas...

a-all particles move in the same direction
b-the particles cannot diffuse
c-the particles exert attractive forces on each other
d-all particles have the same kinetic energy
Definition
C
Term
According to the kinetic-molecular theory, which is the most significant difference between gases and liquids?

a-the mass of each particle
b-the distance between the particles
c-the shapes of the particles
d-the type of collision that occurs between particles
Definition
B
Term
Which is an example of gas diffusion?

a-a cylinder of oxygen stored under high pressure
b-the odor of perfume spreading throughout a room
c-inflating a flat tire
d-all of the above
Definition
B
Term
which is an example of effusion?

a-helium dispersing into a room after a balloon pops
b-oxygen and gasoline fumes mixing in an automobile carburetor
c-air slowly escaping from a pinhole on a tire
d-the aroma of a cooling pie spreading across a room
Definition
C
Term
Why does the air pressure inside the tires of a car increase when the car is driven?

a-some of the air has leaked out
b-the atmosphere compresses the tire
c-the air particles inside the tire increase their speed because their temperature rises
d-the air particles collide with the tire after the car is in motion
Definition
C
Term
What is the process by which molecules of a gas randomly encounter and pass through a small opening in a container?

a-diffusion
b-osmosis
c-distillation
d-effusion
Definition
D
Term
What does the constant bombardment of gas molecules against the inside walls of a container produce?

a-pressure
b-density
c-temperature
d-diffusion
Definition
A
Term
The intermolecular forces between particles are....

a-weaker in solids than in liquids
b-stronger in gases that in solids
c-equal in strength in gases and in liquids
d-stronger in liquids than in gases
Definition
D
Term
Which of these best describes vaporization?

a-the process by which a liquid changes to a gas
b-the process by which a solid changes to a gas
c-Both (a) and (b)
d-neither (a) nor (b)
Definition
A
Term
Which term best describes the process by which particles escape from the surface of a non-boiling liquid and enter the gas state?

a-sublimation
b-evaporation
c-surface tension
d-aeration
Definition
B
Term
Which of these can happen due to decreasing the average energy of a liquid's particles?

a-vaporization
b-evaporation
c-a random arrangement
d-freezing
Definition
D
Term
Molecules at the surface of a liquid can enter the vapor phase only if....

a-equilibrium has not been reached
b-the concentration of the vapor is zero
c-their energy is high enough to overcome the attractive forces in the liquid
d-condensation is not occurring
Definition
C
Term
Why would a camper near the top of Mt. Everest find that water boils at less than 100 degrees Celsius?

a-there is greater atmospheric pressure than at sea level
b-the flames are hotter at that elevation
c-there is less atmospheric pressure than at sea level
d-the atmosphere has less moisture
Definition
A
Term
Glycerol boils at a slightly higher temperature than water. This reveals that glycerol's attractive forces are....

a-nonexistent
b-weaker than those of water
c-the same as those of water
d-stronger than those of water
Definition
D
Term
During boiling, the temperature of a liquid...

a-remains constant
b-increases
c-decreases
d-approaches water's boiling point
Definition
B
Term
Who developed that the total pressure of a mixture of gases is the sum of their partial pressures?

a-Charles
b-Boyle
c-Kelvin
d-Dalton
Definition
D
Term
Which of the following has components in a nonuniform arrangement?

a-homogeneous mixture
b-solution
c-salt water
d-heterogeneous mixture
Definition
D
Term
Which mixture contains visible particles that settle out unless the mixture is stirred?

a-a colloid
b-a homogeneous mixture
c-a solution
d-a suspension
Definition
D
Term
Which mixture contains particles that are in a dispersed phase and do not settle out?

a-a colloid
b-a homogeneous mixture
c-a solution
d-a suspension
Definition
A
Term
A metal solution is a(n)

a-colloid
b-alloy
c-suspension
d-emulsion
Definition
B
Term
Colloids...

a-can be separated by filtering
b-settle out when allowed to stand
c-scatter light
d-contain particles larger than 1000 nm
Definition
C
Term
A substance whose water solution is a good conductor of electricity is a(n)...

a-nonelectrolyte
b-electrolyte
c-nonpolar substance
d-solute
Definition
B
Term
Which of the following is an electrolyte?

a-sodium chloride
b-sugar
c-pure water
d-glass
Definition
B
Term
Which of the following is a nonelectrolyte?

a-sodium chloride
b-hydrogen chloride
c-sugar
d-potassium chloride
Definition
A
Term
Increasing the surface area of the solute....

a-increases the rate of dissolution
b-decreases the rate of dissolution
c-has no effect on the rate of dissolution
d-can increase, decrease, or have no effect on the rate of dissolution
Definition
C
Term
Which of the following will dissolve most slowly?

a-large salt crystals in unstirred water
b-large salt crystals in stirred water
c-small salt crystals in unstirred water
d-small salt crystals in stirred water
Definition
A
Term
Raising solvent temperature causes a solvent-solute collisions to become....

a-less frequent and more energetic
b-more frequent and more energetic
c-less frequent and less energetic
d-more frequent and less energetic
Definition
B
Term
If the amount of solute present in a solution at a given temperature is given temperature is less than the maximum amount that can dissolve at that temperature, the solution is said to be....

a-saturated
b-unsaturated
c-supersaturated
d-concentrated
Definition
B
Term
"Like dissolves like" is a very general rule used for predicting whether....

a-one substance will form a solution with another
b-one substance will react with another
c-a reaction will reach equilibrium
d-a mixture will contain two or three phases
Definition
A
Term
Which of the following is an example of a polar solvent?

a-carbon tetrachloride
b-benzene
c-water
d-gasoline
Definition
C
Term
During the dissolving process, which particles interact?

a-solute only
b-solvent only
c-solute and solvent
d-none of the above
Definition
C
Term
Pressure has the greatest effect on the solubility of...

a-solids and liquids
b-liquids in liquids
c-gases in gases
d-gases in liquids
Definition
B
Term
The solubility of gases in liquids....

a-increases with increasing pressure
b-cannot reach equilibrium
c-decreases with increasing pressure
d-does not depend on pressure
Definition
D
Term
Henry's law relates...

a-pressure to temperature
b-pressure to gas-liquid solubility
c-temperature to gas-liquid solubility
d-pressure to liquid-solid solubility
Definition
B
Term
As temperature increases, solubility of gases in liquids....

a-increases
b-decreases
c-can increase
d-is not affected
Definition
B
Term
In the precipitation video (wow), he used lots of carbonates, phosphates, and hydroxides as they....

a-almost always form a precipitate
b-form a side variety of colors
c-were coincidently chosen
d-are inexpensive
Definition
A
Term
Electrolytes affect colligative properties differently than do nonelectrolytes because electrolytes....

a-produce more moles of solute particles per mole of solute
b-produce fewer moles of solute particles per mole of solute
c-have lower boiling points
d-are easily evaporated
Definition
A
Term
In the NaClNOSO chart, the "SO" stands for....

a-solubility
b-none of the answers are correct
c-spectator
d-SO4
Definition
D
Term
A precipitation reaction is a type of....

a-polyatomic ion dissociation
b-combustion reaction
c-acid base reaction
d-double displacement reaction
Definition
D
Term
Sugar is not an electrolyte because...

a-is too large
b-it has covalent bonds
c-it does ionize in solution
d-it has ionic bonds
Definition
C
Term
Why is a freezing-point depression a colligative property?

a-it is inversly proportional to the molal concentration of a solution
b-it is directly proportionla to the molal concentration of a solution
c-it depends on the properites of an electrolyte in a solvent
d-it does not depend on a molal freezing-point constant for each solvent
Definition
B
Term
Colligative properties depend on....

a-the boiling point and freezing point of the solution
b-the identity of the solute particles
c-the concentration of the solute particles
d-the physical properties of the solute particles
Definition
C
Term
Ionization is different that dissociation. This is because ionization involves...

a-formation of ions from a molecule with covalent bonds
b-sharing of electrons
c-transferring of electrons
d-dissociation of ions form a compound with ionic bonds
Definition
D
Term
For properties that are colligative such as boiling point, the solute particles...

a-break apart the solvent H-bonds
b-prevent the solvent molecules from leaving the surface of the solution
c-make strong covalent bonds that reuire more heat to break
d-form a "skin" over the solution
Definition
B
Term
A precipitation reaction must form a....

a-liquid or a solid
b-liquid and another reaction
c-two precipitates
d-solid and another reaction
Definition
A
Term
When writing net ionic equations,

a-write all compounds
b-none of the answers are correct
c-leave the spectators out of the equation
d-leave the precipitates out of the equation
Definition
C
Term
In order for two compounds to react they must...

a-form a solid or a liquid
b-all answers are correct
c-both be soluble
d-collide
Definition
B
Term
Acetic acid is found in....

a-lemons
b-vinegar
c-sour milk
d-apples
Definition
B
Term
Aqueous solutions of acids

a-contain only two different elements
b-carry electricity
c-have very high boiling points
d-cannot be prepared
Definition
B
Term
An acid ending with the suffix -ic produces an anion with the

a-suffix -ate
b-suffix -ite
c-prefix hydro-
d-suffix -ous
Definition
A
Term
Which acid is produced in the stomach?

a-hydrochloric acid
b-phosphoric acid
c-nitric acid
d-sulfuric acid
Definition
A
Term
Which acid is found in vinegar?

a-acetic acid
b-nitric acid
c-phosphoric acid
d-hydrochloric acid
Definition
A
Term
An Arrhenius acid contains...

a-hydrogen that does not ionize
b-hydrogen that ionizes to form hydrogen ions
c-oxygen that ionizes to form hydroxide ions
d-oxygen that ionizes to form oxygen ions
Definition
B
Term
Which of the following is NOT a strong acid?

a-HNO3
b-CH3COOH
c-H2SO4
d-HCl
Definition
B
Term
In water, hydroxides of Group 2 metals....

a-are all strong bases
b-are all weak bases
c-are all acids
d-are nonelectrolytes
Definition
A
Term
Which of the following is a triprotic acid?

a-H2SO4
b-CH3COOOH
c-HCl
d-H3PO4
Definition
D
Term
A Bronsted-Lowry acid is a(n)

a-electron pair acceptor
b-electron pair donor
c-proton acceptor
d-proton donor
Definition
B
Term
A species that remains when an acid has lost a proton is a....

a-conjugate base
b-conjugate acid
c-strong base
d-strong acid
Definition
A
Term
The members of a conjugate acid-base pair....

a-appear on the same side of the chemical equation
b-appear on opposite sides of the chemical equation
c-might appear on the same side or on opposite sides of the equation
d-are not included in the chemical equation
Definition
B
Term
In a conjugate acid-base pair, the acid typically has....

a-one more proton than the base
b-one fewer proton than the base
c-two fewer protons than the base
d-the same number of protons as the base
Definition
A
Term
An amphoteric species is one that reacts as a(n)....

a-acid only
b-base only
c-acid or base
d-none of the above
Definition
C
Term
Pure water partially breaks down into charged particles in a process called....

a-hydration
b-hydrolysis
c-self-ionization
d-dissociation
Definition
C
Term
As a general rule, the entropy of a solid is....

a-less than that of a liquid
b-zero
c-more than that of a gas
d-more than that of a liquid
Definition
A
Term
For an exothermic reaction, delta H is always....

a-zero
b-positive
c-small
d-negative
Definition
D
Term
In water, hydroxides of Group 2 metals....

a-are all strong bases
b-are all weak bases
c-are all acids
d-are nonelectrolytes
Definition
A
Term
What is the difference between the enthalpies of the products and the reactants?

a-delta G
b-delta S
c-H
d-delta H
Definition
D
Term
What is the symbol for Gibb's free-energy change?

a-delta G
b-delta T
c-delta S
d-delta H
Definition
A
Term
Delta H=

a-Hproducts-Hreactants
b-Hreactants-Hproducts
c-Hproducts/Hreactants
d-Hreactant+Hproducts
Definition
A
Term
As a general rule, the entropy of a solid is....

a-less than that of a liquid
b-zero
c-more than that of a gas
d-more than that of a liquid
Definition
A
Term
For an exothermic reaction, delta H is always....

a-zero
b-positive
c-small
d-negative
Definition
D
Term
If a reaction is endothermic, which side of the reaction should the heat energy by written?

a-products
b-depends on the entropy
c-reactants
d-can not be determined
Definition
C
Term
If a piece of aluminum is heated from 30.0 degrees Celsius, what is the value of delta T

a-20.0 K
b-0.0 K
c- -20.0 K
d-Cannot be determined from the information given
Definition
A
Term
Which of the following substances has the highest entropy?

a-crushed ice
b-steam
c-liquid water
d-ice water
Definition
B
Term
Which of the following is a measure of the randomness in a system?

a-enthalpy
b-free energy
c-temperature
d-entropy
Definition
D
Term
Which of the following has the highest entropy when produced in a reaction?

a-a solid
b-a liquid
c-a gas
d-an aqueous solution
Definition
C
Term
What is the symbol for entropy?

a-G
b-T
c-S
d-H
Definition
C
Term
Which of the following systems has the lowest entropy?

a-oil floating in a container of water
b-sand mixed in a container of water
c-salt dissolved in a container of water
d-a container of frozen water
Definition
D
Term
Which of the following best describes temperature?

a-energy of change
b-energy as heat absorbed or released in a chemical or physical change
c-a measure of the average kinetic energy of the particles in a sample of matter
d-energy in the form of heat
Definition
C
Term
As ice melts, the water molecules...

a-stya ordered the same as in ice
b-go from a less-ordered phase to a more-ordered phase
c-go from a well-ordered phase to a less-ordered phase
d-none of the above
Definition
C
Term
The quantity of energy released or absorbed as heat during a chemical reaction is called the....

a-enthalpy of reaction
b-entropy
c-temperature
d-free energy
Definition
A
Term
Energy is measured in units of...

a-kelvin
b-joules
c-grams
d-pounds
Definition
B
Term
delta H is always positive for a....

a-spontaneous reaction
b-endothermic reaction
c-nonspontaneous reaction
d-exothermic reaction
Definition
B
Term
An equation that includes the quantity of energy released or absorbed as energy in the form of heat during the reaction is a(n)....

a-thermochemical equation
b-kinetic equation
c-energetic equation
d-temperature equation
Definition
A
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