Term 4 Test

The molecular geometry of a water molecule is a. linear b. bent c. trigonal planar d. triangular

B

The process of changing from a solid to a gas is known as a. condensation b. sublimation c. deposition d. skim milk

B

Water's relatively high boiling point is the result of a. covalent bonding b. hydrogen bonding c. ionic bonding d. London forces

B

Which condition is necessary for most gases to behave nearly ideally? a. high pressure b. high temperature c. low compressibility d. low expansion

B

Which mixture can be separated by filtration? a. mayonnaise b. muddy water c. shaving cream d. gelatin

B

Which of the following is a colloid? a. water b. milk c. soil d. concrete

B

Which of the following is not a physical property of gases? a. absence of large volume b. large density c. high compressibility d. fluidity

B

Which of the following is not a type of crystal? a. metallic crystal b. lattice crystal c. covalent network crystal d. ionic crystal

B

Which of the following liquids is most volatile? a. water b. ether c. molten salt d. skim milk

B

A mixture that appears to be uniform while being stirred but which separates into different phases when agitation ceases is a a. solvent b. colloid c. suspension d. solute

C

A phase is defined as any part of a system that has a. the same composition throughout b. the same properties throughout c. the same properties and composition throughout d. the same temperature throughout

C

Which of the following actions does not, in general, increase the solubility of a solid in a liquid? a. increasing the temperature b. increasing the surface area of the solute c. increasing the pressure of the solution d. shaking or stirring the solution

C

Which of the following is not an example of an intermolecular force? a. hydrogen bonding b. London dispersion forces c. gravitational forces d. dipole-dipole interactions

C

Which of the following is not true about the volume of a gas? a. Most of the volume is empty space b. The volume is occupied by particles in continuous, rapid, random motion. c. The volume is about 10 times greater than that occupied by an equal number of particles in the liquid or solid state. d. Generally, the volume can be easily changed

C

Which of the following is not used in preparing 3.00 L of a 1.25 M aqueous solution? a. (3.75 mol x molar mass) of the solute b. 3.75 mol of solute c. (3.00 L x molar mass) of water d. enough water to make 3.00 L of solution

C

How can you best increase the solubility of a gas in a liquid? a. Increase both the temperature and the pressure b. Decrease both the temperature and the pressure c. Increase the temperature and decrease the pressure d. Decrease the temperature and increase the pressure

D

How many grams of CaCl₂ (molar mass = 110.98 gm/mol) are needed to prepare 1.00 L of a 1.00 M solution? a. 1.00 g b. 40.08 g c. 75.53 g d. 110.98 g

D

Liquid water forms molecular groups. How many molecules of water are there in each group? a. one to two b. two to four c. three to six d. four to eight

D

Sugar is soluble in water because sugar molecules are a. massive b. large c. nonpolar d. polar

D

The enthalpy of solution for solid AgNO₃ is positive. What does this tell you about the formation of a AgNO₃ solution? a. AgNO₃ wil not form a solution b. Energy is released during the solution process c. AgNO₃ will dissolve only under high pressure d. Energy is absorbed during the solution process

D

The smallest portion of a crystal lattice that shows the three-dimensional pattern of the entire lattice is called the a. crystal structure b. molecular structure c. formula unit d. unit cell

D

Two immiscible substances are a. water and ammonia b. water and ethanol c. carbon tetrachloride and benzene d. benzene and water

D

What type of solute-solvent combination is carbon dioxide in air? a. gas-liquid b. liquid-gas c. liquid-liquid d. gas-gas

D

Which gas deviates the most from ideal behavior? a. CH₄ b. H₂O c. Cl₂ d. He

D

Which is an example of a non-crystalline solid? a. emerald b. quartz c. ice d. glass

D

Which of the following is an assumption of the kinetic-molecular theory of gases? a. Collisions between gas particles are inelastic b. Gases consist of closely spaced particles c. Gas particles move around in an orderly manner d. The temperature of a gas depends on the average kinetic energy of the gas particles

D

Which of the following is not a physical property of crystalline solids? a. definite shape b. definite melting point c. low rate of diffusion d. high compressibility

D

Which of the following statements about concentration is true? a. A concentrated solution may be saturated b. A saturated solution may be dilute c. A dilute solution may be unsaturated d. All of the above

D

Which statement correctly represents the equilibrium between gas molecules entering and leave the liquid phase of a solution? a. gas + solution ↔ Solvent b. gas + solvent → solution c. gas ← solvent + solution d. gas + solvent ↔ solution

D

Which is an example of a solid-liquid solution? a. alcohol-water solution b. oxygen-nitrogen solution c. sugar-water solution d. copper-nickel solution

C

Surface tension does not account for which of the following phenomena? a. ability to diffuse b. meniscus formation c. capillary action d. decreasing surface area

A

Amorphous solids have no definite melting point because a. their particles are constantly changing positions b. their particles are arranged randomly. c. their particles are tightly parked. d. their particles move around each other.

B

Diffusion is much slower in liquids than in gases because a. liquids exist at lower temperatures b. liquid particles are closer together c. liquid particles weigh more. d. liquids have surface tension

B

A liquid becomes a gas during a. evaporation b. condensation c. sublimation d. deposition

A

A liquid can be described as a form of matter that a. has a definite volume b. has a definite shape. c. cannot diffuse. d. has a low density.

A

A solubility table shows that almost all compounds of Group 1 metals are soluble in water. This general rule tells you that a. KI is soluble b. RbNO₃ is insoluble c. CaCl₂ is soluble d. CO₂ is soluble

A

A substance that is not soluble in a polar solvent is most likely a. nonpolar b. ionic c. polar d. hydrogen bonded

A

According to the kinetic-molecular theory, particles in solids a. vibrate around fixed points b. are loosely packed c. move rapidly around each other d. are arranged randomly

A

All of the KBr that will dissolve in a solution has dissolved, and several undissolved crystals remain on the bottom of the beaker. The solution is a. saturated b. supersaturated c. unsaturated d. at the incorrect pressure to dissolve the solid

A

All of the following are homogeneous mixtures except a. tomato soup b. a sugar-water solution c. gasoline d. a salt-water solution

A

Compared with nonpolar substances of comparable molecular mass, water's molar enthalpy of vaporization is a. higher b. lower c. similar d. equal

A

Compared with the boiling point of nonpolar substances of comparable molar mass at 1 ATM, the boiling point of water at 1 ATM is a. higher b. lower c. equal d. approximately the same

A

Equilibrium is characterized by a. opposing processes occurring at equal rates. b. an oen system. c. net change in the amount of substance in one phase d. changes in physical states.

A

If energy as heat is removed, most liquids will eventually a. freeze. b. burn. c. evaporate. d. diffuse

A

The amount of energy needed to melt one mole of a substance is its molar a. enthalpy of fusion b. enthalpy of vaporization c. entropy of fusion d. entropy of vaporization

A

The temperature at which the vapor pressure of a substance equals atmospheric pressure is its a. boiling point b. critical point c. melting point d. triple point

A

What is the reason for the relatively low density of ice? a. empty spaces between molecules b. the high number of hydrogen bonds c. the small size of hydrogen and oxygen atoms d. the low molar mass of water

A

When preparing a 2.50 m aqueous solution of KOH, you correctly calculate that you need 140.3 g of KOH and 1.000 Kg (or 1.000 L) of water. What should you do after adding 140.3 g of KOH to a large beaker? a. Add 1000. mL of water, and stir until solute dissolves b. Add 900. mL of water, dissolve solute, add to a volumetric flask, and then add water to the 1000. mL mark c. Add 900. ML of water, dissolve solute, add to a volumetric flask, add water to 1000. mL mark, and mix thoroughly. d. Add 900 mL of water, dissolve solute, add to a volumetric flask, add water to 1000. mL mark, mix thoroughly, and transfer to another container.

A

When the size of the particles in a solution and in a colloid are compared, the particle size in the solution is a. smaller b. larger c. the same size as the particle size in the colloid d. either smaller or larger, depending on the colloid and the solution

A

Which crystalline solids generally have the highest melting and boiling points? a. covalent network crystals b. nonpolar covalent molecular crystals c. ionic crystals d. polar covalent molecular crystals

A

Which is an example of a polar covalent molecular crystal? a. H₂O b. H₂ c. NaCl d. CCl₄

A

Which mixture exhibits the Tyndall effect? a. fog b. salt water c. gasoline d. sterling silver

A

Which of the following is not used in preparing a 0.300 m aqueous solution of NaBr (molar mass = 102.89 g/mol) with 1.00 Kg of solvent? a. 0.300 mol water b. 0.300 mol NaBr c. graduated cylinder d. 0.300 mol • molar mass of NaBr

A

Which of the following is the equation needed to calculated the kinetic energy, KE, of a moving particle? a. KE=1/2•mv² b. KE=2mv c. KE=mv d. KE=1/2•m²v

A

Which states of matter are fluid? a. gases and liquids b. liquids and solids c. gases only d. liquids only

A

You know the mass of solute and the volume of solution. What is the first step in finding the molarity of the solution? a. Divide the mass by molar mass to determine number of moles b. Divide the mass by the volume of solution c. Divide the volume of solution by its mass d. Divide the number of moles by the volume of solution.

A

Dry ice sublimes into carbon dioxide gas. If the proper conditions are maintained and the system is closed, the dry ice and the carbon dioxide gas will eventually a. become the same phase b. reach equilibrium c. stop changing phase d. Both (a) and (b)

B

If the vapor pressure of water is 4.25 kPa at 30˚C, the vapor pressure of water at 10˚C is most likely to be a. 0 kPa b. 1.23 kPa c. 4.25 kPa d. 12.34 kPa

B

A 0.100 M solution of copper (II) nitrate reacts with an excess of iron. What do you need to know to calculate the number of moles of iron (II) nitrate produced? a. the amount of the other product produced b. the volume of solution c. the molar mass of copper (II) nitrate d. the molar mass of iron (II) nitrate

B

A hypothetical gas that perfectly fits all the assumptions of the kinetic-molecular theory is known as a. a real gas b. an ideal gas c. an imaginary gas d. a perfect gas

B

Which of the following solutions does not contain an electrolyte? a. potassium bromide-water solution b. sugar-water solution c. hydrochloric acid solution d. sodium chloride-water solution

B

According to the kinetic-molecular theory, particles in a liquid a. are bound together in fixed positions b. are packed together in an orderly arrangement. c. move around randomly and constantly. d. vibrate only.

C

Assume you have a substance that plots right on the liquid-vapor equilibrium line on its phase diagram. If you raise the temperature slightly and keep the same pressure, the substance will now be a. a solid b. a liquid c. a gas d. on a different equilibrium line

C

How many different types of crystal symmetry are there? a. 3 b. 5 c. 7 d. 9

C

If a gas has the same temperature throughout, which gas molecule has the highest average velocity? a. O₂ b. H₂O c. H₂ d. Xe

C

If the amount of dissolved solute in a solution at a given temperature is greater than the amount that can permanently remain in solution at that temperature, the solution is said to be a. saturated b. unsaturated c. supersaturated d. diluted

C

If water molecules were not linked by hydrogen bonds to form groups in liquid water, what would be the physical state of water at room temperature? a. solid b. liquid c. gas d. a mixture of liquid and gas

C

In some instances, the concentration os a solution is expressed as molality instead of molarity because a. molality is easier to calculate b. molarity applies only to solid-liquid solutions c. molality does not change with changes in temperature d. molarity changes with the amount of solute and molality does not

C

Liquids are more ordered than gases because liquids have a. weaker intermolecular forces and lower mobility of the particles. b. weaker intermolecular forces and greater mobility of the particles. c. stronger intermolecular forces and lower mobility of the particles d. stronger intermolecular forces and greater mobility of the particles.

C

Rate of effusion of different gases are proportional to their a. polarity b. particle charge c. particle velocities d. compressibility

C

The bond between oxygen and hydrogen in a water molecule is a. ionic b. hydrogen c. polar-covalent d. dipole-dipole

C

The molar enthalpy of fusion of ice is a. equal to the enthalpy of many other solids b. approximately the same as the enthalpy of many other solids c. larger than the enthalpy of many other solids d. smaller than the enthalpy of many other solids

C

The point on a phase diagram that indicates the temperature and pressure conditions at which the solid, liquid, and vapor of the substance can coexist at equilibrium is known as the a. critical point b. phase point c. triple point d. equilibrium point

C

The three states of matter of a particular substance, in order of strength of intermolecular forces from least to greatest, are a. solid, liquid, gas b. liquid, solid, gas c. gas, liquid, solid d. gas, solid, liquid

C

To conduct electricity, a solution must contain a. nonpolar molecules b. polar molecules c. ions d. free electrons

C

Water forms roughly spherical drops because of a. viscosity b. capillary action c. surface tension d. fluidity

C

What is the approximate angle between two hydrogen-oxygen bonds in water? a. 90˚ b. 102˚ c. 105˚ d. 120˚

C

When preparing 500. mL of a 1.35 M aqueous solution of NaCl, what should you do after adding the correct amount of solute to a large beaker? a. Add 500. mL of water, and stir until solute dissolves b. Add 500 mL of water, dissolve solute, and add to a volumetric flask c. Add 400 mL of water, dissolve solute, add to a volumetric flask, add water to 500. mL mark, and mix thoroughly. d. Add 400. mL of water, dissolve solute, add to a volumetric flask, add 100. mL of water, mix thoroughly, and transfer to another container.

C

A 0.15 M solution of HCl reacts with an excess of calcium carbonate, CaCl₃. A volume of 25.0 mL of HCl is used. To determine the number of moles of CaCl₂ produced, you need to know a. the amount of the other product produced b. the molar mass of HCl c. the molar mass of CaCl₂ d. the balanced chemical equation for the reaction

D

A mixture of alcohol, water, oil, and glycerin is poured into a graduated cylinder. The liquids separate to form layers from top to bottom: alcohol, oil, water and glycerin. Based on this observation, which liquid is the most dense? a. alcohol b. oil c. water d. glycerin

D