Question 1

The term "normal" boiling point indicates ________.

Accepted Answer

A) the temperature at which water evaporates under the atmospheric pressure found at sea level. 
B) the temperature at which tap water boils under the atmospheric pressure found at sea level. 
C) the temperature at which water boils under any pressure conditions 
D) both A and B 
A) the temperature at which water evaporates under the atmospheric pressure found at sea level. 
B) the temperature at which tap water boils under the atmospheric pressure found at sea level. 
C) the temperature at which water boils under any pressure conditions 
D) both A and B

Question 2

Which intermolecular force is important for the function of the antibiotic vancomycin?

Accepted Answer

A) London forces 
B) van der Waals forces 
C) hydrogen bonding 
D) dipole forces 
A) London forces 
B) van der Waals forces 
C) hydrogen bonding 
D) dipole forces

Question 3

Which of the three phases of matter (solid, liquid, or gas)features particles that are easily compressible?

Accepted Answer

A) solid 
B) liquid 
C) gas 
D) All three phases of matter are compressible. 
A) solid 
B) liquid 
C) gas 
D) All three phases of matter are compressible.

Question 4

The main reason why carbon tetrabromide is a solid at room temperature when compared to carbon tetrachloride which is a liquid is ________.

Accepted Answer

A) carbon tetrabromide is tetrahedral in shape 
B) carbon tetrachloride has a higher molecular weight 
C) carbon tetrabromide may undergo hydrogen bonding 
D) all of the above 
A) carbon tetrabromide is tetrahedral in shape 
B) carbon tetrachloride has a higher molecular weight 
C) carbon tetrabromide may undergo hydrogen bonding 
D) all of the above

Question 5

Which of the following chemical substances would you expect to have the highest melting point?

Accepted Answer

A) water, H2O 
B) methyl alcohol, CH3OH 
C) nitrogen dioxide, NO2 
D) hydrogen sulfide, H2S 
A) water, H2O 
B) methyl alcohol, CH3OH 
C) nitrogen dioxide, NO2 
D) hydrogen sulfide, H2S

Question 6

Nonpolar molecules may exhibit ________.

Accepted Answer

A) London forces 
B) hydrogen bonding 
C) dipolar forces 
D) all of the above 
A) London forces 
B) hydrogen bonding 
C) dipolar forces 
D) all of the above

Question 7

At the freezing point the molecules are effectively frozen in place.

Accepted Answer

A) True 
 B)False

Question 8

The main reason why water has a much higher boiling point than acetone is the ability of water to undergo hydrogen bonding.

Accepted Answer

A) True 
 B)False

Question 9

Which of the following statements is true about intermolecular forces of attraction between molecules?

Accepted Answer

A) They tend to stick molecules together. 
B) Cooling is responsible for the substance's liquefaction. 
C) The solidification of a substance usually requires lower temperatures than in the case of liquefaction. 
D) All of the above are true. 
A) They tend to stick molecules together. 
B) Cooling is responsible for the substance's liquefaction. 
C) The solidification of a substance usually requires lower temperatures than in the case of liquefaction. 
D) All of the above are true.

Question 10

Solid carbon dioxide is also known as dry ice.

Accepted Answer

A) True 
 B)False

Question 11

Based upon the formulas and melting points, decide whether each of the following crystalline substances should be classified as ionic, molecular, metallic or network covalent.
-ethanol, C2H6O, m.p.: -117 °C

Accepted Answer

Question 12

Based upon the formulas and melting points, decide whether each of the following crystalline substances should be classified as ionic, molecular, metallic or network covalent.
-silicon carbide, SiC, m.p.: 2700 °C

Accepted Answer

The answer of Based upon the formulas and melting points,...

Question 13

Which of the following does not have a dipole?

Accepted Answer

A) carbon tetrachloride 
B) acetone 
C) ammonia 
D) water 
A) carbon tetrachloride 
B) acetone 
C) ammonia 
D) water

Question 14

The terms "dispersion forces" and "London forces" are interchangeable.

Accepted Answer

A) True 
 B)False

Question 15

To form hydrogen bonds, molecules must contain ________.

Accepted Answer

A) an N-H bond 
B) an O-H bond 
C) an H-F bond 
D) at least one of the above mentioned bonds 
A) an N-H bond 
B) an O-H bond 
C) an H-F bond 
D) at least one of the above mentioned bonds

Question 16

Between individual molecules of NO2 in the solid state, which of the following types of intermolecular forces would you expect to be dominant?

Accepted Answer

A) hydrogen bonding 
B) London forces 
C) van der Waals forces 
D) dipole forces 
A) hydrogen bonding 
B) London forces 
C) van der Waals forces 
D) dipole forces

Question 17

Which of the three phases of matter (solid, liquid, or gas)has particles moving at the highest average velocity?

Accepted Answer

A) solid 
B) liquid 
C) gas 
D) The particles in all three phases have about the same average speed. 
A) solid 
B) liquid 
C) gas 
D) The particles in all three phases have about the same average speed.

Question 18

Which of the following will have the lowest boiling point?

Accepted Answer

A) H2S 
B) H2Te 
C) H2Se 
D) H2O 
A) H2S 
B) H2Te 
C) H2Se 
D) H2O

Question 19

Match between columns
                        Premises: boron trifluoride
titanium
hydrogen fluoride
quartz
carbon tetrachloride
methane
ammonia
iron
carbon tetrabromide
sodium
diamond
water

Accepted Answer

The Answer of metallic and network covalent bonding and hydrogen is...

Question 20

Which of the following intermolecular force is the strongest?

Accepted Answer

A) London forces 
B) van der Waals forces 
C) hydrogen bonding 
D) dipole forces 
A) London forces 
B) van der Waals forces 
C) hydrogen bonding 
D) dipole forces

The term "normal" boiling point indicates ________.

Which intermolecular force is important for the function of the antibiotic vancomycin?

Which of the three phases of matter (solid, liquid, or gas)features particles that are easily compressible?

The main reason why carbon tetrabromide is a solid at room temperature when compared to carbon tetrachloride which is a liquid is ________.

Which of the following chemical substances would you expect to have the highest melting point?

Nonpolar molecules may exhibit ________.

At the freezing point the molecules are effectively frozen in place.

The main reason why water has a much higher boiling point than acetone is the ability of water to undergo hydrogen bonding.

Which of the following statements is true about intermolecular forces of attraction between molecules?

Solid carbon dioxide is also known as dry ice.

Based upon the formulas and melting points, decide whether each of the following crystalline substances should be classified as ionic, molecular, metallic or network covalent. -ethanol, C₂H₆O, m.p.: -117 °C

Based upon the formulas and melting points, decide whether each of the following crystalline substances should be classified as ionic, molecular, metallic or network covalent. -silicon carbide, SiC, m.p.: 2700 °C

Which of the following does not have a dipole?

The terms "dispersion forces" and "London forces" are interchangeable.

To form hydrogen bonds, molecules must contain ________.

Between individual molecules of NO₂ in the solid state, which of the following types of intermolecular forces would you expect to be dominant?

Which of the three phases of matter (solid, liquid, or gas)has particles moving at the highest average velocity?

Which of the following will have the lowest boiling point?

Which of the following intermolecular force is the strongest?

What Is Chemistry

The Numerical Side of Chemistry

The Evolution of Atomic Theory

The Modern Model of the Atom

Chemical Bonding and Nomenclature

The Shape of Molecules

Chemical Reactions

Stoichiometry and the Mole

Electron Transfer in Chemical Reactions

What If There Were No Intermolecular Forces the Ideal Gas

Solutions

When Reactants Turn Into Products

Chemical Equilibrium

Electrolytes, Acids, and Bases

Nuclear Chemistry

The Chemistry of Carbon

Synthetic and Biological Polymers

Filters

Exam 7: Intermolecular Forces and the Phases of Matter

The term "normal" boiling point indicates ________.

Which intermolecular force is important for the function of the antibiotic vancomycin?

Which of the three phases of matter (solid, liquid, or gas)features particles that are easily compressible?

The main reason why carbon tetrabromide is a solid at room temperature when compared to carbon tetrachloride which is a liquid is ________.

Which of the following chemical substances would you expect to have the highest melting point?

Nonpolar molecules may exhibit ________.

At the freezing point the molecules are effectively frozen in place.

The main reason why water has a much higher boiling point than acetone is the ability of water to undergo hydrogen bonding.

Which of the following statements is true about intermolecular forces of attraction between molecules?

Solid carbon dioxide is also known as dry ice.

Based upon the formulas and melting points, decide whether each of the following crystalline substances should be classified as ionic, molecular, metallic or network covalent. -ethanol, C2H6O, m.p.: -117 °C

Based upon the formulas and melting points, decide whether each of the following crystalline substances should be classified as ionic, molecular, metallic or network covalent. -silicon carbide, SiC, m.p.: 2700 °C

Which of the following does not have a dipole?

The terms "dispersion forces" and "London forces" are interchangeable.

To form hydrogen bonds, molecules must contain ________.

Between individual molecules of NO2 in the solid state, which of the following types of intermolecular forces would you expect to be dominant?

Which of the three phases of matter (solid, liquid, or gas)has particles moving at the highest average velocity?

Which of the following will have the lowest boiling point?

Which of the following intermolecular force is the strongest?

What Is Chemistry

The Numerical Side of Chemistry

The Evolution of Atomic Theory

The Modern Model of the Atom

Chemical Bonding and Nomenclature

The Shape of Molecules

Chemical Reactions

Stoichiometry and the Mole

Electron Transfer in Chemical Reactions

What If There Were No Intermolecular Forces the Ideal Gas

Solutions

When Reactants Turn Into Products

Chemical Equilibrium

Electrolytes, Acids, and Bases

Nuclear Chemistry

The Chemistry of Carbon

Synthetic and Biological Polymers

Filters

Based upon the formulas and melting points, decide whether each of the following crystalline substances should be classified as ionic, molecular, metallic or network covalent. -ethanol, C₂H₆O, m.p.: -117 °C

Between individual molecules of NO₂ in the solid state, which of the following types of intermolecular forces would you expect to be dominant?