Question 1

Which of the following forces between atoms or ions or molecules is the strongest on a per mole basis?

Accepted Answer

Covalent bonds are the strongest of the forces listed on a per mole basis. They involve the sharing of electrons between atoms, leading to the formation of a stable, covalently-bonded molecule or compound. The other forces listed are weaker, and are generally considered intermolecular forces, rather than true chemical bonds.

Question 2

Arrange the following molecules in order of increasing boiling point. H₂O₂, HCl and O₂

Accepted Answer

Oxygen (O2) is non-polar and has the lowest boiling point. HCl is polar and has a higher boiling point than O2. H2O2 can form hydrogen bonds, giving it the highest boiling point among the three.

Question 3

On the basis of intermolecular forces of attraction, rank the following three compounds in terms of increasing boiling point. CH₃CH₂CH₂CH₂CH₃ (Pentane), CHCl₃ (Chloroform) and H₂O (Water)

Accepted Answer

Pentane has the lowest boiling point due to its weak van der Waals forces. Chloroform has a higher boiling point due to its dipole-dipole interactions. Water has the highest boiling point because of its strong hydrogen bonding.

Question 4

On the basis of intermolecular forces of attraction, rank the following three compounds in terms of increasing boiling point . NH₃ (Ammonia), N₂ (Nitrogen) and HCl (Hydrogen Chloride)

Accepted Answer

Nitrogen has the weakest London dispersion forces, HCl has dipole-dipole interactions, and NH3 has hydrogen bonding, leading to the highest boiling point.

Question 5

Consider the hydrogen halides, HX (where X = F, Cl, Br, and I). Based upon a comparison between the intermolecular forces for each compound, which would be expected to have the highest boiling point ?

Accepted Answer

HF has the highest boiling point among the hydrogen halides because it can form hydrogen bonds due to the high electronegativity of fluorine. This results in stronger intermolecular forces compared to HCl, HBr, and HI, which primarily exhibit dipole-dipole interactions and London dispersion forces.

Question 6

Given the three statements below, pick the best answer. I. Dipole-dipole interactions should contribute to the intermolecular bonding forces of FBr. II. London forces (instantaneous dipole) are the only intermolecular forces acting between H₂ molecules. III. London forces should be greater for I₂ than Br₂ because I₂ is more polarizable.

Accepted Answer

The answer of Given the three statements below, pick the...

Question 7

Given the three molecules listed below, which choice is best? I. CH₃OH II. H₂S III. CH₃CH₃

Accepted Answer

Hydrogen bonding is the dominant intermolecular force only for molecule I, as it is the only one that contains a hydrogen atom directly bonded to an electronegative atom (oxygen, in this case), which is a requirement for hydrogen bonding. Molecules II and III do not meet the criteria for hydrogen bonding based on the given structures.

Question 8

Three molecules are listed below. Will hydrogen bonding be important for any of them? Pick the correct answer. I. HBr II. CH₃OH III. NH₃

Accepted Answer

Hydrogen bonding occurs when there is a hydrogen atom attached to a highly electronegative atom (N, O, or F) and there is a lone pair on another electronegative atom to accept the hydrogen bond. II (CH3OH) has an -OH group, and III (NH3) has an -NH group, both of which can participate in hydrogen bonding. I (HBr) does not have hydrogen attached to N, O, or F, so it cannot hydrogen bond.

Question 9

Pick the true statement below.

Accepted Answer

Hydrogen bonding is indeed the most important intermolecular force for both HF (hydrogen fluoride) and H2O (water) due to the presence of hydrogen atoms bonded to highly electronegative atoms (F and O, respectively), which allows for the formation of hydrogen bonds.

Question 10

Based upon intermolecular forces of attraction, which is the correct order for increasing boiling points among the following three molecules? N₂, H₂, and NH₃

Accepted Answer

The correct order is based on the types of intermolecular forces present in each molecule. N₂ (N2) and H₂ (H2) are nonpolar molecules and thus exhibit London dispersion forces. NH₃ (NH3) can form hydrogen bonds, which are stronger than London dispersion forces. Since hydrogen bonds are stronger than London dispersion forces, NH3 has the highest boiling point. Between N2 and H2, H2 has a lower molecular weight, leading to weaker London dispersion forces and thus a lower boiling point. Therefore, the order from lowest to highest boiling point is H2 < N2 < NH3.

Question 11

Which molecule listed below would have its intermolecular forces dominated by dispersion forces?

Accepted Answer

N₂ (N2O) is a nonpolar molecule, so its intermolecular forces are dominated by dispersion forces. The other molecules listed have polar bonds and can exhibit dipole-dipole interactions or hydrogen bonding.

Question 12

Arrange the following elements in order of increasing boiling point. Argon, Helium, Neon

Accepted Answer

Boiling points of noble gases increase with increasing atomic number due to greater van der Waals forces in larger atoms, so Helium (He) has the lowest, followed by Neon (Ne), and then Argon (Ar) has the highest boiling point.

Question 13

Which of the following forces between atoms or ions or molecules is the strongest?

Accepted Answer

Electrostatic force between ions is the strongest type of intermolecular force because it involves the attraction between oppositely charged ions. This attraction is stronger than any of the other types of intermolecular forces.

Question 14

Given the three statements below, pick the best answer. I. Dipole-dipole forces are the main intermolecular force for I - Br. II. O₂ is a gas at room temperature because it is highly polarizable. III. London forces dominate the intermolecular forces for Br₂.

Accepted Answer

Statement I is false because I-Br molecule does not have a permanent dipole moment. Statement II is also false because O₂ is actually a liquid at room temperature despite being highly prone to polarizability. Statement III is true because Br₂ is a nonpolar molecule that only experiences London dispersion forces. Therefore, only III is true.

Question 15

Which of the following molecules cannot form hydrogen bonds as a pure liquid?

Accepted Answer

The answer of Which of the following molecules cannot form...

Question 16

On the basis of intermolecular forces of attraction, rank the following three compounds in terms of increasing boiling point . CH₃CH₂OH, CH₃OCH₃ and CH₃CH₂CH₃

Accepted Answer

The boiling point of a compound is dependent on the strength of intermolecular forces present. On analyzing the given compounds, it can be seen that they are all organic molecules with nonpolar/ polar covalent bonds. CH₃OCH₃ and CH₃CH₂CH₃ contain similar polar covalent bonds, and their boiling points are primarily decided by dispersion forces. However, CH₃CH₂OH contains a polar covalent bond and hydrogen bonding due to the presence of -OH group. The hydrogen bonding leads to higher intermolecular forces and hence a higher boiling point. Thus, the correct order of boiling point is CH₃CH₂CH₃ < CH₃OCH₃ < CH₃CH₂OH. Therefore, option C is the best choice.

Question 17

Which of the molecules shown below does not have any dipole-dipole intermolecular forces?

Accepted Answer

BeH₂ is a linear molecule and has no net dipole moment, so it does not have any dipole-dipole intermolecular forces.

Question 18

What is the most important intermolecular force in solid H₂O?

Accepted Answer

H₂O contains hydrogen atoms bonded to electronegative atoms (sulfur and oxygen) which allows for hydrogen bonding. Hydrogen bonding is a stronger force compared to London dispersion and dipole-dipole forces, and in this case there are no ions present to make ionic bonding the most important force. While covalent bonding is present in the molecule, it is not an intermolecular force, so it is not relevant to this question.

Question 19

Which of the following would have a boiling point lower than SiCl₄?

Accepted Answer

CCl₄ has a lower boiling point than SiCl₄ due to its smaller molecular size and weaker intermolecular forces compared to SiCl₄.

Question 20

Based upon an analysis of intermolecular forces of attraction among the compounds listed below, which substance would be expected to have the highest boiling point?

Accepted Answer

The compounds listed are all covalent compounds that experience intermolecular forces of attraction called London dispersion forces. The strength of these forces depends on the size of the molecules or atoms because the larger the size, the larger the electron cloud and the more likely it is to experience temporary dipoles that can induce dipoles in neighboring molecules or atoms. Among the given compounds, Iodine (I) is the largest atom and therefore will experience the strongest London dispersion forces. Stronger intermolecular forces will require more energy to break, and thus, Iodine will have the highest boiling point among the given compounds.

Quiz 11: Liquids and Solids

Which of the following forces between atoms or ions or molecules is the strongest on a per mole basis?

Arrange the following molecules in order of increasing boiling point. H₂O₂, HCl and O₂

On the basis of intermolecular forces of attraction, rank the following three compounds in terms of increasing boiling point. CH₃CH₂CH₂CH₂CH₃ (Pentane) , CHCl₃ (Chloroform) and H₂O (Water)

On the basis of intermolecular forces of attraction, rank the following three compounds in terms of increasing boiling point . NH₃ (Ammonia) , N₂ (Nitrogen) and HCl (Hydrogen Chloride)

Consider the hydrogen halides, HX (where X = F, Cl, Br, and I) . Based upon a comparison between the intermolecular forces for each compound, which would be expected to have the highest boiling point ?

Given the three molecules listed below, which choice is best? I. CH₃OH II. H₂S III. CH₃CH₃

Three molecules are listed below. Will hydrogen bonding be important for any of them? Pick the correct answer. I. HBr II. CH₃OH III. NH₃

Pick the true statement below.

Based upon intermolecular forces of attraction, which is the correct order for increasing boiling points among the following three molecules? N₂, H₂, and NH₃

Which molecule listed below would have its intermolecular forces dominated by dispersion forces?

Arrange the following elements in order of increasing boiling point. Argon, Helium, Neon

Which of the following forces between atoms or ions or molecules is the strongest?

Given the three statements below, pick the best answer. I. Dipole-dipole forces are the main intermolecular force for I - Br. II. O₂ is a gas at room temperature because it is highly polarizable. III. London forces dominate the intermolecular forces for Br₂.

Which of the following molecules cannot form hydrogen bonds as a pure liquid?

On the basis of intermolecular forces of attraction, rank the following three compounds in terms of increasing boiling point . CH₃CH₂OH, CH₃OCH₃ and CH₃CH₂CH₃

Which of the molecules shown below does not have any dipole-dipole intermolecular forces?

What is the most important intermolecular force in solid H₂O?

Which of the following would have a boiling point lower than SiCl₄?

Based upon an analysis of intermolecular forces of attraction among the compounds listed below, which substance would be expected to have the highest boiling point?

Quiz 11: Liquids and Solids

Which of the following forces between atoms or ions or molecules is the strongest on a per mole basis?

Arrange the following molecules in order of increasing boiling point. H2O2, HCl and O2

On the basis of intermolecular forces of attraction, rank the following three compounds in terms of increasing boiling point. CH3CH2CH2CH2CH3 (Pentane) , CHCl3 (Chloroform) and H2O (Water)

On the basis of intermolecular forces of attraction, rank the following three compounds in terms of increasing boiling point . NH3 (Ammonia) , N2 (Nitrogen) and HCl (Hydrogen Chloride)

Consider the hydrogen halides, HX (where X = F, Cl, Br, and I) . Based upon a comparison between the intermolecular forces for each compound, which would be expected to have the highest boiling point ?

Given the three molecules listed below, which choice is best? I. CH3OH II. H2S III. CH3CH3

Three molecules are listed below. Will hydrogen bonding be important for any of them? Pick the correct answer. I. HBr II. CH3OH III. NH3

Pick the true statement below.

Based upon intermolecular forces of attraction, which is the correct order for increasing boiling points among the following three molecules? N2, H2, and NH3

Which molecule listed below would have its intermolecular forces dominated by dispersion forces?

Arrange the following elements in order of increasing boiling point. Argon, Helium, Neon

Which of the following forces between atoms or ions or molecules is the strongest?

Given the three statements below, pick the best answer. I. Dipole-dipole forces are the main intermolecular force for I - Br. II. O2 is a gas at room temperature because it is highly polarizable. III. London forces dominate the intermolecular forces for Br2.

Which of the following molecules cannot form hydrogen bonds as a pure liquid?

On the basis of intermolecular forces of attraction, rank the following three compounds in terms of increasing boiling point . CH3CH2OH, CH3OCH3 and CH3CH2CH3

Which of the molecules shown below does not have any dipole-dipole intermolecular forces?

What is the most important intermolecular force in solid H2O?

Which of the following would have a boiling point lower than SiCl4?

Based upon an analysis of intermolecular forces of attraction among the compounds listed below, which substance would be expected to have the highest boiling point?

Arrange the following molecules in order of increasing boiling point. H₂O₂, HCl and O₂

On the basis of intermolecular forces of attraction, rank the following three compounds in terms of increasing boiling point. CH₃CH₂CH₂CH₂CH₃ (Pentane) , CHCl₃ (Chloroform) and H₂O (Water)

On the basis of intermolecular forces of attraction, rank the following three compounds in terms of increasing boiling point . NH₃ (Ammonia) , N₂ (Nitrogen) and HCl (Hydrogen Chloride)

Given the three molecules listed below, which choice is best? I. CH₃OH II. H₂S III. CH₃CH₃

Three molecules are listed below. Will hydrogen bonding be important for any of them? Pick the correct answer. I. HBr II. CH₃OH III. NH₃

Based upon intermolecular forces of attraction, which is the correct order for increasing boiling points among the following three molecules? N₂, H₂, and NH₃

Given the three statements below, pick the best answer. I. Dipole-dipole forces are the main intermolecular force for I - Br. II. O₂ is a gas at room temperature because it is highly polarizable. III. London forces dominate the intermolecular forces for Br₂.

On the basis of intermolecular forces of attraction, rank the following three compounds in terms of increasing boiling point . CH₃CH₂OH, CH₃OCH₃ and CH₃CH₂CH₃

What is the most important intermolecular force in solid H₂O?

Which of the following would have a boiling point lower than SiCl₄?