Archive for August 2016

When a solution of weak electrolyte is altered by adding one of its ions from another source, the ionization of the weak electrolyte is suppressed. This behavior is termed the ____.

When a solution of weak electrolyte is altered by adding one of its ions from another source, the ionization of the weak electrolyte is suppressed. This behavior is termed the ____.




a. common ion effect
b. buffer effect
c. titration curve
d. equivalence point
e. partial neutralization effect




Answer: A

The densest phase of F2 is a

The densest phase of F2 is a




a. solid
b. liquid
c. gas



Answer: A

An unknown substance was found to have a melting point of ~300oC and was not soluble water. It is a good conductor in both the melt and solid states. Which of the following substances is the most likely?

An unknown substance was found to have a melting point of ~300oC and was not soluble water. It is a good conductor in both the melt and solid states. Which of the following substances is the most likely?




a. C6H12O6 (glucose)
b. KCl
c. Rb
d. C (diamond)
e. Si




Answer: C

Both solid and liquid CCl4 are molecular in nature. Which of the following statements is true?

Both solid and liquid CCl4 are molecular in nature. Which of the following statements is true?




a. Liquid CCl4 is much more compressible and more highly ordered than solid CCl4.
b. The liquid CCl4 molecules are attracted to one another by covalent bonds.
c. Liquid CCl4 is a slightly disordered arrangement of molecules with somewhat restricted mobility.
d. Liquid CCl4 is a state in which there is little effect contributed by intermolecular forces on the physical properties of CCl4. (The liquid CCl4 does not feel the effects of intermolecular forces).





Answer: C

When X-rays with ? = 193.7 pm are used, the second-order Bragg reflection from a set of parallel planes in a rubidium crystal occurs at an angle ? = 29.37°. Calculate the distance between the planes in the crystal.

When X-rays with ? = 193.7 pm are used, the second-order Bragg reflection from a set of parallel planes in a rubidium crystal occurs at an angle ? = 29.37°. Calculate the distance between the planes in the crystal.




a. 6.595 pm
b. 62.00 pm
c. 124.0 pm
d. 197.5 pm
e. 394.9 pm




Answer: E

As iron is heated to 1181K, it adopts one type of cubic cell (A); then, as the temperature rises to 1674K, it changes to another cubic cell (B). The iron is changing from a _______ unit cell to a _______unit cell.

As iron is heated to 1181K, it adopts one type of cubic cell (A); then, as the temperature rises to 1674K, it changes to another cubic cell (B). The iron is changing from a _______ unit cell to a _______unit cell.





a. Body-centered cubic ? simple cubic
b. Body-centered cubic ? face-centered cubic
c. Face-centered cubic ? simple cubic
d. Face-centered cubic ? body-centered cubic
e. Simple cubic ? face-centered cubic



Answer: B

The metal niobium crystallizes in a body-centered cubic unit cell. When x-rays with a wavelength of 0.8302Å are used, the second-order (n=2) Bragg reflection from a set of parallel planes in a niobium crystal is observed at an angle of ? = 14.57?. If the distance between these planes corresponds to a unit cell length (d = a), calculate the edge length of the niobium unit cell.

The metal niobium crystallizes in a body-centered cubic unit cell. When x-rays with a wavelength of 0.8302Å are used, the second-order (n=2) Bragg reflection from a set of parallel planes in a niobium crystal is observed at an angle of ? = 14.57?. If the distance between these planes corresponds to a unit cell length (d = a), calculate the edge length of the niobium unit cell.





a. 0.209Å
b. 0.915Å
c. 1.65Å
d. 3.30Å
e. 1005Å




Answer: D

You have a white, crystalline solid which melts at 88oC. It does not conduct electricity in the solid phase, and when it dissolves in water it still does not conduct electricity. Which of the following is the most likely formula for this compound?

You have a white, crystalline solid which melts at 88oC. It does not conduct electricity in the solid phase, and when it dissolves in water it still does not conduct electricity. Which of the following is the most likely formula for this compound?





a. Mg
b. Si
c. CCl4
d. AlCl3
e. C6H12O6



Answer: E

You have a white, crystalline solid which has a melting point of 800oC. It does not conduct electricity in the solid phase, but it forms a conducting solution when dissolved in water. Which of the following is the most likely formula for this compound?

You have a white, crystalline solid which has a melting point of 800oC. It does not conduct electricity in the solid phase, but it forms a conducting solution when dissolved in water. Which of the following is the most likely formula for this compound?





a. Mg
b. Si
c. CCl4
d. AlCl3
e. C6H12O6



Answer: D

The electron sea model explains ______.

The electron sea model explains ______.




a. the chemical reactivity of most metals
b. why most metals are solids at room temperature
c. the thermal conductivity of metals by the easy flow of nuclei
d. the electrical conductivity of metals by the easy flow of nuclei
e. the electrical conductivity of metals by the easy flow of electrons



Answer: E

Calculate the amount of energy required to melt a 48.9g sample of cobalt at its normal melting point. Boiling point = 3097oC ? Hvap = 389 kJ/mol melting point = 1495oC ? Hfus = 15.5 kJ/mol specific heat solid = 0.418 J/goC specific heat liquid = 0.686 J/goC

Calculate the amount of energy required to melt a 48.9g sample of cobalt at its normal melting point.
Boiling point = 3097oC ? Hvap = 389 kJ/mol
melting point = 1495oC ? Hfus = 15.5 kJ/mol
specific heat solid = 0.418 J/goC specific heat liquid = 0.686 J/goC




a. 12.9 kJ
b. 18.7 kJ
c. 20.5 kJ
d. 323 kJ
e. 759 kJ



Answer: A

Choose the statement which best explains why the boiling point of ICl (97 oC) is higher than the boiling point of Br2 (59 oC):

Choose the statement which best explains why the boiling point of ICl (97 oC) is higher than the boiling point of Br2 (59 oC):




a. The molecular weight of ICl is 162.4, while that of Br2 is 159.8.
b. London dispersion forces are much stronger for ICl than for Br2.
c. ICl is an ionic compound, while Br2 is a molecular compound.
d. ICl is polar, while Br2 is nonpolar.
e. There is hydrogen bonding in ICl, but not in Br2.




Answer: D

At 10.0oC, the vapor pressure of nitric acid is 26.6 mmHg, and at 50.0oC, the vapor pressure is 208 mmHg. Using this information, calculate the heat of vaporization (?Hvap) of nitric acid.

At 10.0oC, the vapor pressure of nitric acid is 26.6 mmHg, and at 50.0oC, the vapor pressure is 208 mmHg. Using this information, calculate the heat of vaporization (?Hvap) of nitric acid.




a. 25.6 kJ/mol
b. 39.1 kJ/mol
c. 48.4 kJ/mol
d. 225 kJ/mol
e. 566 kJ/mol



Answer: B

Which of the following statements concerning the accompanying phase diagram is false?

Which of the following statements concerning the accompanying phase diagram is false?




a. The solid is less dense than the liquid.
b. Point C is the critical point of the substance.
c. Point A is the triple point of the substance.
d. The normal boiling point is below the triple point.
e. The curve AD divides the solid region from the gas region.



Answer: A

How much heat is released at constant pressure if a 18.0-L tank containing 42.0 atm of hydrogen sulfide gas condenses at its boiling point of -60.0oC? The enthalpy of vaporization of hydrogen sulfide is 18.7 kJ/mol at -60.0oC. (R = 0.0821 L • atm/(K • mol))

How much heat is released at constant pressure if a 18.0-L tank containing 42.0 atm of hydrogen sulfide gas condenses at its boiling point of -60.0oC? The enthalpy of vaporization of hydrogen sulfide is 18.7 kJ/mol at -60.0oC. (R = 0.0821 L • atm/(K • mol))




a. 1.22 × 102 J
b. 2.87 × 106 J
c. 4.33 × 102 J
d. 1.87 × 104 J
e. 8.08 × 105 J



Answer: E

Elements that have their highest energy electrons in a filled band of molecular orbitals that is separated from the lowest empty band by an energy difference much too large for electrons to jump between bands are called ____.

Elements that have their highest energy electrons in a filled band of molecular orbitals that is separated from the lowest empty band by an energy difference much too large for electrons to jump between bands are called ____.




a. semiconductors
b. metals
c. conductors
d. insulators
e. isomorphs




Answer: D

For crystal structures that contain only one kind of atom, the nearest neighbors of each atom can be visualized as lying along a line of the unit cell. For a body-centered cubic structure what is the orientation of that line with respect to the unit cell and how many atomic radii does it contain?

For crystal structures that contain only one kind of atom, the nearest neighbors of each atom can be visualized as lying along a line of the unit cell. For a body-centered cubic structure what is the orientation of that line with respect to the unit cell and how many atomic radii does it contain?




a. cell edge and 2 atomic radii
b. face diagonal and 4 atomic radii
c. body diagonal and 3 atomic radii
d. face diagonal and 2 atomic radii
e. body diagonal and 4 atomic radii




Answer: E

For crystal structures that contain only one kind of atom, the nearest neighbors of each atom can be visualized as lying along a line of the unit cell. For a simple cubic structure what is the orientation of that line with respect to the unit cell and how many atomic radii does it contain?

For crystal structures that contain only one kind of atom, the nearest neighbors of each atom can be visualized as lying along a line of the unit cell. For a simple cubic structure what is the orientation of that line with respect to the unit cell and how many atomic radii does it contain?




a. cell edge and 2 atomic radii
b. face diagonal and 4 atomic radii
c. body diagonal and 3 atomic radii
d. face diagonal and 2 atomic radii
e. body diagonal and 4 atomic radii



Answer: A

Substances have properties that are related to their structures. Which of the following statements regarding properties of solids is not expected to be correct?

Substances have properties that are related to their structures. Which of the following statements regarding properties of solids is not expected to be correct?




a. Molten KBr should be a good conductor of electricity.
b. Diamond should have a high melting point.
c. Solid sodium should be a good conductor of electricity.
d. Solid CaF2 should have a low melting point.
e. Silicon carbide, SiC, should not sublime readily.



Answer: D

Substances have properties that are related to their structures. Which of the following statements regarding properties of solids is not expected to be correct?

Substances have properties that are related to their structures. Which of the following statements regarding properties of solids is not expected to be correct?




a. Solid potassium should be a good conductor of electricity.
b. Solid CaSO4 should sublime readily.
c. Molten LiCl should be a good conductor of electricity.
d. Graphite should have a high melting point.
e. Solid CO2 should have a low melting point.




Answer: B

Which type of solid is expected for Ga?

Which type of solid is expected for Ga?




a. covalent
b. ionic
c. metallic
d. molecular
e. intensive



Answer: C

Which type of solid is expected for SO2?

Which type of solid is expected for SO2?




a. covalent
b. ionic
c. metallic
d. molecular
e. hypersaturated



Answer: D

Which one of the following is an ionic solid?

Which one of the following is an ionic solid?



a. graphite
b. nickel
c. ammonium chloride
d. silicon carbide, SiC
e. sucrose, C12H22O11



Answer: C

Which one of the following is a covalent solid?

Which one of the following is a covalent solid?




a. sulfur trioxide
b. nickel
c. ammonium chloride
d. silicon carbide, SiC
e. sucrose, C12H22O11



Answer: D

Which one of the following is not a general property of ionic solids?

Which one of the following is not a general property of ionic solids?




a. hard and brittle
b. good electrical conductors in the solid state
c. relatively high melting points
d. strongest interparticle attractions are electrostatic
e. positions of ions define the unit cell (lattice)




Answer: B

Which one of the following statements is not applicable to molecular solids?

Which one of the following statements is not applicable to molecular solids?




a. The units that occupy the lattice points are molecules.
b. The binding forces in molecular solids are dispersion forces or dispersion forces and dipole-dipole interactions.
c. Molecular solids have relatively low melting points.
d. Molecular solids are usually excellent conductors of electric current.
e. Molecular solids are soft compared to covalent solids.




Answer: D

Which one of the following statements is not applicable to metallic solids?

Which one of the following statements is not applicable to metallic solids?




a. The units that occupy the lattice points are positive ions.
b. The binding forces in metallic solids are shared electron pairs.
c. The melting points of metallic solids vary over a large range.
d. The hardness of metallic solids varies from quite soft to quite hard.
e. Metallic solids conduct electric current well.



Answer: B

Which one of the following statements is not applicable to covalent solids?

Which one of the following statements is not applicable to covalent solids?




a. The units that occupy the lattice points are atoms.
b. The binding forces in covalent solids are shared electrons.
c. Covalent solids have low melting points.
d. Covalent solids are very hard.
e. Covalent solids do not conduct electric current well.




Answer: C

Amorphous solids are characterized by all the following statements except:

Amorphous solids are characterized by all the following statements except:




a. Amorphous solids have no well-defined, ordered structure.
b. The intermolecular forces between their particles are constant throughout the solid.
c. Some amorphous solids are able to flow, like liquids.
d. Amorphous solids do not exhibit sharp melting points.
e. Amorphous solids shatter irregularly.




Answer: B

How much heat would be required to convert 234.3 g of solid benzene, C6H6(s), at 5.5°C into benzene vapor, C6H6(g), at 100.0°C? mp of C6H6(s) = 5.5°C bp of C6H6 = 80.1°C molar heat of fusion at 5.5°C = 9.92 kJ/mol molar heat of vaporization at 80.1°C = 30.8 kJ/mol molar heat capacity of C6H6 = 136 J/mol•°C molar heat capacity of C6H6(g) = 81.6 J/mol•°C

How much heat would be required to convert 234.3 g of solid benzene, C6H6(s), at 5.5°C into benzene vapor, C6H6(g), at 100.0°C?

mp of C6H6(s) = 5.5°C
bp of C6H6 = 80.1°C
molar heat of fusion at 5.5°C = 9.92 kJ/mol
molar heat of vaporization at 80.1°C = 30.8 kJ/mol
molar heat capacity of C6H6 = 136 J/mol•°C
molar heat capacity of C6H6(g) = 81.6 J/mol•°C




a. 106 kJ
b. 158 kJ
c. 53 kJ
d. 32 kJ
e. 5049 kJ




Answer: B

What will be the final temperature of the liquid water resulting from the mixing of 10.0 grams of steam at 130.°C with 40.0 g of ice at -10.0°C? (Sp. heat of H2O(s) = 2.09 J/g•°C, Sp. heat of H2O = 4.18 J/g•°C, Sp. heat of H2O(g) = 2.03 J/g•°C; heat of fusion of H2O(s) = 333 J/g, heat of vap. of H2O = 2260 J/g)

What will be the final temperature of the liquid water resulting from the mixing of 10.0 grams of steam at 130.°C with 40.0 g of ice at -10.0°C? (Sp. heat of H2O(s) = 2.09 J/g•°C, Sp. heat of H2O = 4.18 J/g•°C, Sp. heat of H2O(g) = 2.03 J/g•°C; heat of fusion of H2O(s) = 333 J/g, heat of vap. of H2O = 2260 J/g)




a. 80.4°C
b. 72.6°C
c. 54.3°C
d. 46.1°C
e. 63.3°C



Answer: E

A chemical reaction releases 58,500 J of heat into 150 g of water. Assuming no heat is lost to the surroundings, what is the temperature increase of the water? (Sp. heat of H2O = 4.18 J/g•°C)

A chemical reaction releases 58,500 J of heat into 150 g of water. Assuming no heat is lost to the surroundings, what is the temperature increase of the water? (Sp. heat of H2O = 4.18 J/g•°C)




a. 36.1°C
b. 93.2°C
c. 20.2°C
d. 106.4°C
e. 0.03°C




Answer: B

If 10.0 g of ice at -10.0°C is placed in 200. g of water at 80.0°C in an insulated container, what will be the temperature of the system when equilibrium is established? (Sp. heat of H2O(s) = 2.09 J/g•°C, Sp. heat of H2O = 4.18 J/g•°C, heat of fus. of H2O(s) = 333 J/g)

If 10.0 g of ice at -10.0°C is placed in 200. g of water at 80.0°C in an insulated container, what will be the temperature of the system when equilibrium is established? (Sp. heat of H2O(s) = 2.09 J/g•°C, Sp. heat of H2O = 4.18 J/g•°C, heat of fus. of H2O(s) = 333 J/g)




a. 76°C
b. 65°C
c. 27°C
d. 20°C
e. 72°C



Answer: E

Calculate the amount of heat required to convert 10.0 grams of ice at -20.°C to steam at 120.°C. (Sp. heat of H2O(s) = 2.09 J/g•°C, Sp. heat of H2O = 4.18 J/g•°C, Sp heat of H2O(g) = 2.03 J/g•°C; heat of fus. of H2O(s) = 333 J/g, heat of vap. of H2O = 2260 J/g)

Calculate the amount of heat required to convert 10.0 grams of ice at -20.°C to steam at 120.°C. (Sp. heat of H2O(s) = 2.09 J/g•°C, Sp. heat of H2O = 4.18 J/g•°C, Sp heat of H2O(g) = 2.03 J/g•°C; heat of fus. of H2O(s) = 333 J/g, heat of vap. of H2O = 2260 J/g)




a. 18.6 kJ
b. 26.3 kJ
c. 30.9 kJ
d. 41.2 kJ
e. 46.4 kJ




Answer: C

What is the specific heat of a metal if a ten gram sample at 40.2°C is dropped into 100 grams of water at 25.4°C and the temperature rises to 28.6°C? (Sp. heat of H2O = 4.18 J/g•°C)

What is the specific heat of a metal if a ten gram sample at 40.2°C is dropped into 100 grams of water at 25.4°C and the temperature rises to 28.6°C? (Sp. heat of H2O = 4.18 J/g•°C)




a. 2.11 J/g °C
b. 0.085 J/g °C
c. 206 J/g °C
d. 1.92 J/g °C
e. 20.9 J/g °C




Answer: A

What would be the final temperature of the system if 30.0 g of lead at 150.°C is dropped into 10.0 g of water at 10.0°C in an insulated container? (Sp. heat of H2O = 4.18 J/g•°C, Sp. heat of Pb(s) = 0.128 J/g•°C)

What would be the final temperature of the system if 30.0 g of lead at 150.°C is dropped into 10.0 g of water at 10.0°C in an insulated container? (Sp. heat of H2O = 4.18 J/g•°C, Sp. heat of Pb(s) = 0.128 J/g•°C)




a. 12.4°C
b. 16.8°C
c. 19.4°C
d. 21.7°C
e. 24.6°C




Answer: D

The amount of energy associated with holding the individual particles (atoms, ions, or molecules) together in a crystal lattice is most directly related to ____.

The amount of energy associated with holding the individual particles (atoms, ions, or molecules) together in a crystal lattice is most directly related to ____.




a. the specific heat of the solid
b. the heat of fusion of the solid
c. the specific heat of the liquid
d. the density of the solid
e. the heat of condensation of the liquid



Answer: B

If 10.0 g of steam at 110.0°C is pumped into an insulated vessel containing 100. g of water at 20.0°C, what will be the equilibrium temperature of the mixture? (Sp. heat of H2O = 4.18 J/g•°C, Sp. heat of H2O(g) = 2.03 J/g•°C, heat of vap. of H2O = 2.260 kJ/g)

If 10.0 g of steam at 110.0°C is pumped into an insulated vessel containing 100. g of water at 20.0°C, what will be the equilibrium temperature of the mixture? (Sp. heat of H2O = 4.18 J/g•°C, Sp. heat of H2O(g) = 2.03 J/g•°C, heat of vap. of H2O = 2.260 kJ/g)




a. 86.8°C
b. 54.5°C
c. 58.4°C
d. 38.6°C
e. 76.9°C




Answer: E

If 100. grams of liquid water at 100.°C and 200. grams of water at 20.0°C are mixed in an insulated container, what will the final temperature of the mixture be? (Sp. heat of H2O = 4.18 J/g•°C)

If 100. grams of liquid water at 100.°C and 200. grams of water at 20.0°C are mixed in an insulated container, what will the final temperature of the mixture be? (Sp. heat of H2O = 4.18 J/g•°C)




a. 46.7°C
b. 60.0°C
c. 66.7°C
d. 73.3°C
e. 77.8°C



Answer: A

How much heat is released when 40.0 g of steam at 250.0°C cools and condenses to water at 30.0°C? (Sp. heat of H2O = 4.18 J/g•°C, Sp. heat of H2O(g) = 2.03 J/g•°C, heat of vap. of H2O = 2.260 kJ/g)

How much heat is released when 40.0 g of steam at 250.0°C cools and condenses to water at 30.0°C? (Sp. heat of H2O = 4.18 J/g•°C, Sp. heat of H2O(g) = 2.03 J/g•°C, heat of vap. of H2O = 2.260 kJ/g)




a. 24.0 kJ
b. 23.0 J
c. 32.9 kJ
d. 114 kJ
e. 122 kJ




Answer: D

Calculate the amount of heat (in joules) required to convert 92.5 g of water at 25.0°C to steam at 108.0°C. (Sp. heat of H2O = 4.18 J/g•°C, Sp. heat of H2O(g) = 2.03 J/g•°C, heat of vap. of H2O = 2.260 kJ/g)

Calculate the amount of heat (in joules) required to convert 92.5 g of water at 25.0°C to steam at 108.0°C. (Sp. heat of H2O = 4.18 J/g•°C, Sp. heat of H2O(g) = 2.03 J/g•°C, heat of vap. of H2O = 2.260 kJ/g)




a. 2.26 × 105 J
b. 3.05 × 104 J
c. 2.40 × 105 J
d. 2.20 × 104 J
e. 6.43 × 105 J




Answer: C

On a relative basis, the weaker the intermolecular forces in a substance are,

On a relative basis, the weaker the intermolecular forces in a substance are,




a. the larger is its heat of vaporization.
b. the more it deviates from the ideal gas law.
c. the greater is its vapor pressure at a particular temperature.
d. the larger is its molar heat capacity as a liquid.
e. the higher is its boiling point.



Answer: C

Which one of the following boils at the lowest temperature?

Which one of the following boils at the lowest temperature?



a. H2O
b. H2S
c. H2Se
d. H2Te
e. H2Po




Answer: B




a. KNO3
b. XeF4
c. Kr
d. NH3
e. AsH3



Answer: C




a. CF4
b. HF
c. HCl
d. KI
e. SiF4




Answer: A


Which one of the following statements does not describe the general properties of liquids accurately?

Which one of the following statements does not describe the general properties of liquids accurately?




a. In the liquid state the close spacing of molecules leads to large intermolecular forces that are strongly dependent on the nature of the molecules involved.
b. Liquids are practically incompressible.
c. As the temperature of a liquid is increased, the vapor pressure of the liquid decreases.
d. The normal boiling point of a liquid is the temperature at which the vapor pressure of the liquid becomes equal to exactly 760 torr.
e. Vapor pressures of liquids at a given temperature differ greatly, and these differences in vapor pressure are due to the nature of the molecules in different liquids.



Answer: C

Volatile liquids are described by all of the following except:

Volatile liquids are described by all of the following except:




a. Volatile liquids are easily vaporized.
b. Volatile liquids have relatively high vapor pressures.
c. Volatile liquids have strong cohesive forces.
d. Volatile liquids have weak intermolecular forces.
e. All of these describe volatile liquids.





Answer: C

As we increase the temperature of a liquid, its properties change. Which of the following would not be an expected change in the properties of a typical liquid as we increase its temperature?

As we increase the temperature of a liquid, its properties change. Which of the following would not be an expected change in the properties of a typical liquid as we increase its temperature?




a. decrease in viscosity
b. decrease in density
c. increase in surface tension
d. increase in vapor pressure
e. increase in tendency to evaporate



Answer: C

Which liquid would evaporate most quickly at room temperature?

Which liquid would evaporate most quickly at room temperature?




a. H2O, 18 g/mol
b. Gasoline, C8H18, 114 g/mol
c. Vegetable oil, 895 g/mol
d. Mineral oil, C12H26, 170 g/mol
e. Ethylene glycol, HO-CH2-CH2-OH, 62 g/mol



Answer: B

Car wax works to repel water because ____.

Car wax works to repel water because ____.




a. wax exerts a very low adhesive force for water.
b. the cohesive forces in water are very low.
c. of capillary action present.
d. the water adheres well with the wax.
e. none of these.



Answer: A

Capillary action is ____

Capillary action is ____




a. resistance to flow.
b. the rate of collisions for gas molecules.
c. the energy required to overcome the attractive forces between molecule in the liquid state to form a gas.
d. the force required to expand the surface of a liquid.
e. the drawing of a liquid up the inside of a small-bore tube when adhesive forces exceed cohesive forces.



Answer: E

Which of the following does not correctly describe viscosity?

Which of the following does not correctly describe viscosity?




a. Viscosity is the resistance to flow of a liquid.
b. Viscosity can be measured with a viscometer.
c. The greater the ability of a liquid to hydrogen bond, the higher the viscosity.
d. The smaller the molecule, the higher the viscosity.
e. All of these correctly describe viscosity.



Answer: D

Which of the following interactions are the strongest?

Which of the following interactions are the strongest?



a. hydrogen bonding force
b. ion-ion interactions
c. permanent dipole force
d. dispersion force
e. London force



Answer: B

Which one of the following statements does not describe the general properties of solids accurately?

Which one of the following statements does not describe the general properties of solids accurately?




a. Solids have characteristic volumes that do not change greatly with changes in temperature.
b. Solids have characteristic volumes that do not change greatly with changes in pressure.
c. Solids diffuse only very slowly when compared to liquids and gases.
d. Solids are not fluid.
e. Most solids have high vapor pressures at room temperature.



Answer: D

Identify which property liquids do not have in common with solids.

Identify which property liquids do not have in common with solids.




a. rigid shape
b. volumes do not change significantly with pressure
c. hydrogen bonding forces can be significant
d. practically incompressible
e. volumes do not change significantly with temperature


Answer: A

Which one of the following statements does NOT describe the general properties of liquids accurately?

Which one of the following statements does NOT describe the general properties of liquids accurately?




a. Liquids have characteristic volumes that do not change greatly with changes in temperature. (Assuming that the liquid is not vaporized.)
b. Liquids have characteristic volumes that do not change greatly with changes in pressure.
c. Liquids diffuse only very slowly when compared to solids.
d. The liquid state is highly disordered compared to the solid state.
e. Liquids have high densities compared to gases.



Answer: C

Molecular compounds are usually ____.

Molecular compounds are usually ____.




a. composed of two or more transition elements
b. composed of positive and negative ions
c. composed of two or more nonmetallic elements
d. exceptions to the law of definite proportions



Answer: C

What type of compound is CuSO?

What type of compound is CuSO?




a. monotomic ionic
b. polyatomic covalent
c. polyatomic ionic
d. binary molecular



Answer: C

When Group 2A elements form ions, they ____.

When Group 2A elements form ions, they ____.



a. lose two protons
b. gain two protons
c. lose two electrons
d. gain two electrons




Answer: C

Why do atoms share electrons in covalent bonds?

Why do atoms share electrons in covalent bonds?



a. to become ions and attract each other
b. to attain a noble-gas electron configuration
c. to become more polar
d. to increase their atomic numbers



Answer: B

What characteristic of metals makes them good electrical conductors?

What characteristic of metals makes them good electrical conductors?




a. They have mobile valence electrons.
b. They have mobile protons.
c. They have mobile cations.
d. Their crystal structures can be rearranged easily.



Answer: A

What is the basis of a metallic bond?

What is the basis of a metallic bond?




a. the attraction of metal ions to mobile electrons
b. the attraction between neutral metal atoms
c. the neutralization of protons by electrons
d. the attraction of oppositely charged ions


Answer: A

Which of the following occurs in an ionic bond?

Which of the following occurs in an ionic bond?



a. Oppositely charged ions attract.
b. Two atoms share two electrons.
c. Two atoms share more than two electrons.
d. Like-charged ions attract.


Answer: A

Which is the correct name for the compound N2O4?

Which is the correct name for the compound N2O4?




a. tetranitrogen dioxide
b. dinitrogen tetroxide
c. dinitrogen quadoxide
d. nitrogen oxide



Answer: B

Which is the correct name for the compound PCl5?

Which is the correct name for the compound PCl5?




a. monophosphorus tetrachloride
b. phosphorus chloride
c. phophorus pentachloride
d. pentaphophorus chloride



Answer: C

Which is the correct name for the compound N2O3?

Which is the correct name for the compound N2O3?



a. dinitro trioxide
b. nitrogen (II) oxide (III)
c. trinitrogen dioxide
d. dinitrogen trioxide



Answer: D

Covalent compound display which of these properties?

Covalent compound display which of these properties?




a. they are hard brittle soilds
b. they have high melting and boiling points
c. they display luster
d. their intermolecular forces are relatively



Answer: D

Which is the correct name for the compound NH4SO4?

Which is the correct name for the compound NH4SO4?




a. nitrogen hydrogen sulfate
b. nitrogen hydrosulfate
c. ammonium (II) sulfate
d. ammonium sulfate



Answer: D

Which is the correct name for the compound CoCO3?

Which is the correct name for the compound CoCO3?




a. carbon oxygen carbonate
b. cobolt (II) carbonate
c. cobolt carbonate
d. cobolt carbonoxide



Answer: B

Which is the correct name for the Na3P?

Which is the correct name for the Na3P? 




a. sodium phosphide
b. sodium phosphite
c. sodium phodphate
d. sodium (III) phophide



Answer: A

Which is the correct name for the compoud FeS?

Which is the correct name for the compoud FeS?




a. Iron sulfide
b. Iron (I) sulfide
c. Iron (II) Sulfide
d. Iron (II) Sulfide (II)



Answer: C

Which correctly describes elements in the same group?

Which correctly describes elements in the same group?




a. they have the same number of valence electrons
b. they have the electrons in the same outermosst energy level.
c. they have the same atomic radius
d. they must be in the same state of matter



Answer: A

Which element has 7 protons?

Which element has 7 protons?




a. nitrogen
b. silicon
c. aluminum
d. sulfer




Answer: A

Which one(s) have a mass of 1 amu?

Which one(s) have a mass of 1 amu? 




a. electron
b. proton
c. proton and neutron
d. electron and proton


Answer: C

Which has a charge of +1?

Which has a charge of +1?




a. proton
b. atom
c. electron
d. neutron



Answer: A

The Law of Conservation of Mass states that mass is neither created nor destroyed in an ordinary chemical reaction. When an iron nail rusts, it seems to get heaveir in mass. Does the iron nail follow the Law of Conservation of Mass?

The Law of Conservation of Mass states that mass is neither created nor destroyed in an ordinary chemical reaction. When an iron nail rusts, it seems to get heaveir in mass. Does the iron nail follow the Law of Conservation of Mass?




a. No, rusting is an exception to the law
b. yes, the iron rearranges its protons so that the masses are the same before and after the reaction and rusting follows the law
c. no, since rusting is a chemical change, it does not follow the law
d. yes, iron chemically combines with the oxygen in the air so if you add the oxygen into the mass of the chemicals before the reaction, the mass after the reaction is the same.





Answer: D

When sodium chloride reacts with calcium oxide to form sodium oxide plus calcium oxide, which of the following equations best illustrates the Law of Conservation of Mass?

When sodium chloride reacts with calcium oxide to form sodium oxide plus calcium oxide, which of the following equations best illustrates the Law of Conservation of Mass?




a. NaCl + CaCo --> Na2O + Ca Cl2
b. 4 NaCl + CaO --> 2 Na2O + CaCl2
c. 2 NaCl + CaCo --> Na20 + CaCl2
d. 3 NaCl +2 CaCo --> Na2O + 3 CaCl2




Answer: C

Which is a compound?

Which is a compound?




a. sodium
b. sea water
c. carbon dioxide
d. brass



Answer: C

According to the law of conservation of mass, in any chemical change?

According to the law of conservation of mass, in any chemical change?



a. the mass of reactants is greater than the mass of products
b. the mass of reactants is less than the mass of products
c. the mass of reactants is equal to the mass of products
d. the masses of products and reactants have no predictable relationship




Answer: C

Which of the following formations is a physical property of copper?

Which of the following formations is a physical property of copper?




a. a deep blue solution when in contact with ammonia
b. a new substance when combined with nitric acid
c. a green copper carbonate compound when in contact with moist air
d. a formation of a drill gauge and wire



Answer: D

Which is a chemical property of copper?

Which is a chemical property of copper? 




a. has a boiling point of 2567 degrees C
b. reacts in air to form a green layer
c. has the symbol Cu
d. is a solid at room temperature




Answer: B

Which is not a chemical change?

Which is not a chemical change?




a. a piece is burned
b. an egg is cooked
c. a bar of iron rusts
d. ingredients for a cake are stirred together



Answer: D

The standard english system of measurement uses units such as yards, miles, quarts, and gallons. The metric system uses units such as meters, kilometers, millimeters, and liters. Why is the metric system easier to use than the english system?

The standard english system of measurement uses units such as yards, miles, quarts, and gallons. The metric system uses units such as meters, kilometers, millimeters, and liters. Why is the metric system easier to use than the english system?




a. metric units are easier to measure than english units
b. the metric system is based on multiples of 10
c. the metric system is used by everyone in the world.
d. Metric units are smaller than English units.




Answer: B

How many meters are in 2.4 km?

How many meters are in 2.4 km?




a. 240
b. 2,400
c. 24,000
d. 240,000



Answer: B
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