Ch.11 - Liquids, Solids & Intermolecular ForcesWorksheetSee all chapters
All Chapters
Ch.1 - Intro to General Chemistry
Ch.2 - Atoms & Elements
Ch.3 - Chemical Reactions
BONUS: Lab Techniques and Procedures
BONUS: Mathematical Operations and Functions
Ch.4 - Chemical Quantities & Aqueous Reactions
Ch.5 - Gases
Ch.6 - Thermochemistry
Ch.7 - Quantum Mechanics
Ch.8 - Periodic Properties of the Elements
Ch.9 - Bonding & Molecular Structure
Ch.10 - Molecular Shapes & Valence Bond Theory
Ch.11 - Liquids, Solids & Intermolecular Forces
Ch.12 - Solutions
Ch.13 - Chemical Kinetics
Ch.14 - Chemical Equilibrium
Ch.15 - Acid and Base Equilibrium
Ch.16 - Aqueous Equilibrium
Ch. 17 - Chemical Thermodynamics
Ch.18 - Electrochemistry
Ch.19 - Nuclear Chemistry
Ch.20 - Organic Chemistry
Ch.22 - Chemistry of the Nonmetals
Ch.23 - Transition Metals and Coordination Compounds

Intermolecular Forces are the attractive forces between 2 molecules. Intramolecular Forces are the bonding forces within a molecule. 

Intermolecular vs. Intramolecular Forces

Concept #1: Understanding the difference between intermolecular and intramolecular forces 

Intermolecular forces influence the physical properties of compounds, whereas intramolecular forces influence the chemical properties of compounds. 

Concept #2: The First and Strongest Intermolecular Force

This intermolecular force deals with the attraction between an ion and a polar compound

Concept #3: The Second Intermolecular Force

This intermolecular forces exists anytime hydrogen is directly connected to fluorine, oxygen or nitrogen

Concept #4: The Third Intermolecular Force

Concept #5: The Fourth Intermolecular Force

This intermolecular force deals with the attraction between a polar and nonpolar covalent compound

Concept #6: The Fifth Intermolecular Force

This intermolecular force is found in all compounds, but it's the main intermolecular force of nonpolar covalent compounds

Example #1: Based on the given compounds, answer each of the following questions:

CH3CH3,       KBr,        C6H5OH,           CaS,             Ne

a. Which compound will have the lowest boiling point?

 

b. Which compound will have the highest surface tension.

 

c. Which compound will have the highest vapor pressure. 

Practice: The predominant intermolecular force in C6H5NH2 is:

Practice: The predominant intermolecular force in HBr is:

Practice: The predominant intermolecular force in ZnBr2 with H2O is:

Practice: The predominant intermolecular force in Ne with H2O is:

Solubility & Intermolecular Forces

Solubility deals with the dissolving of a solute in a solvent in order to create a solution

Concept #7: Understanding the Theory of "Likes" dissolve "Likes"

In order for a solvent to dissolve a solute both components have similar polarities. 

Example #2: Identify the intermolecular forces present in both the solute and the solvent, and predict whether a solution will form between the two. 

CCl4 and P4

Example #3: Identify the intermolecular forces present in both the solute and the solvent, and predict whether a solution will form between the two. 

CH3OH and C6H6

Example #4: Identify the intermolecular forces present in both the solute and the solvent, and predict whether a solution will form between the two. 

C6H5CH2NH2 and HF

Example #5: Identify the intermolecular forces present in both the solute and the solvent, and predict whether a solution will form between the two. 

IF4­ -   and NH3

Practice: Which of the following statements is/are true?

a) Methane will dissolve completely in acetone, CH3COCH3.

b) Hydrofluoric acid (HF) will form a heterogeneous mixture with tetrachloride, CCl4.

c) Pentane will form a homogeneous mixture with CBr4.

d) Methanethiol (CH3SH) is miscible in fluoromethane (CH3F).

Additional Problems
At room temperature, nitrogen (N 2) and oxygen (O2) are both gases, but both will condense if the temperature is lowered enough. N2 condenses at 77K, and O2 condenses at 90K. Which of these molecules experiences weaker intermolecular forces? ___________
Determine the strongest intermolecular force present in each element of compound.  a. HCl b. Br2 c. PH3 d. NH3 
What is the strongest evidence for hydrogen bonding? 1. The boiling points of NH3, H2O, and HF are abnormally high compared with the rest of the hydrides in their respective periods. 2. Hydrogen is able to accept or donate electrons, so it is the most versatile atom in the periodic chart. 3. Hydrogen has an extremely low electronegativity. 4. Hydrogen can be considered either a metal or nonmetal.
The dominant forces between molecules (intermolecular forces) are ____ in origin. 1. electrostatic 2. electrodynamic 3. electromagnetic 4. gravitational 5. magnetic
True or false: Xe is more polarizable than Ne. _________
Which of the following characteristics indicates the presence of  weak  intermolecular forces in a liquid? a) a high critical temperature  b) a low heat of vaporization c) a high boiling point d) a low vapor pressure e) None of the above
Dispersion (London) forces result from 1. distortion of the electron cloud of an atom or molecule by the presence of nearby atoms or molecules. 2. the formation of a loose covalent linkage between a hydrogen atom connected to a very electronegative atom in one molecule and another very electronegative atom in a neighboring molecule. 3. the balance of attractive and repulsive forces between two polar molecules. 4. attraction between molecules in a liquid and molecules or atoms in a solid surface with which the liquid is in contact. 5. attractive forces between a molecule at the surface of a liquid and those beneath it which are not balanced by corresponding forces from above.
In which of these compounds would you find ONLY dispersion forces existing between the molecules? I. CCl4; II. NH3; III. CO2; IV. HBr. 1. II and III only 2. I and III only  3. III and IV only 4. I and IV only 5. II only 6. III only 7. IV only 8. I and II only 9. II and IV only 10. I only
Soap has an ionic and a polar end. It works well to remove oil by A) surrounding the oil with the nonpolar end, and the water interacts with the polar end. B) surrounding the oil with the polar end, and the water interacts with the nonpolar end. C) surrounding the oil and water with the nonpolar end. D) surrounding the oil and water with the polar end.
Which one of the following substances will have both dispersion forces and dipole-dipole forces?             A)  Br2    B)  BCl3    C)  HCl    D)  H 2    E)  CO2
Which one of the following substances should exhibit hydrogen bonding in the liquid state?             A)  PH3    B)  He    C)  H2S    D)  CH4    E)  CH3OH
Which figure best describes the hydrogen bonding between two water molecules?
Identify the dominant intermolecular force in the following species, respectively: RbCl, C6H6 (benzene), HI, Fe2O3, CH2NH. a) ionic forces b) hydrogen bonding c) dipole-dipole d) instantaneous dipoles A. c, b, d, c, c B. a, c, c, d, c C. a, b, c, b, a D. a, d, c, a, b E. a, b, d, a, c F. b, d, c, d, d G. c, d, a, a, b
Acetic acid (CH3COOH) forms a molecular solid. What type of forces hold it in a solid configuration? I) London forces II) dipole-dipole III) hydrogen bonding A. II only B. I, II, and III C. II and III only D. I only E. I and II only F. II only
Which type of solid is held together only by hydrogen bonds? A. molecular crystal B. ionic crystal C. network crystal D. metallic crystal E. several of the above
"Sparkling water" is made by dissolving large amounts of carbon dioxide gas in ordinary water. What are the strongest types of intermolecular bonds between the carbon dioxide molecules and the water molecules in this mixture? a) London forces b) dipole-dipole forces c) ion-dipole forces d) dipole-induced dipole forces e) ion-ion forces
Which intermolecular force predominates in the condensation of water? a. H-bonding  b. Van der Waals c. London d. Ion-Ion e. Dipole-ion
What are the major attractive forces in an aliquot of pure carbon tetrachloride CCl 4? a) dipole-induced dipole b) dispersion c) ion-ion d) ion-dipole e) dipole-dipole
What are the major attractive forces between molecules in the “solution” in an average soda can which contains primarily water and dissolved carbon dioxide? a) dipole-induced dipole b) dispersion c) ion-ion d) ion-dipole e) dipole-dipole
The major forces holding water molecules together in the liquid state are referred to as hydrogen bonds. These are really what kind of attractive forces? a) dipole-induced dipole b) dispersion c) ion-ion d) ion-dipole e) dipole-dipole
A solution of hydrochloric acid in water is often used to clean dirty toilets. What are the strongest intermolecular forces in this solution? a) ion-ion b) induced dipole-induced dipole c) dipole-induced dipole d) dipole-dipole e ion-dipole
Water and ethyl alcohol (CH3CH2OH, the kind people drink) mix completely with one another. What are the strongest intermolecular forces that are responsible for attracting these molecules to each other in this solution? a) ion-ion b) induced dipole-induced dipole c) dipole-induced dipole d)  dipole-dipole e) ion-dipole
London forces would be the strongest type of interaction between which of the following molecules in the gas phase? a) NaCl b) H2O c) CaCl2 d) O2 e) HCl
In which of the following compounds will the molecules not form hydrogen bonds with each other?  
INTERMOLECULAR FORCES Intermolecular forces (nonbonding forces) exist between molecules and influence the physical properties of the substance. The 5 most common intermolecular forces are: 1)  Ion-Dipole is the intermolecular force that exists between an ion and a polar compound. (Strongest) Ex:   NaCl dissolved in H2O   2)  Hydrogen Bonding is the intermolecular force that exists when hydrogen is directly connected F, O, N. (2nd Strongest) Ex:   NH3                                  H2O                  HF   3)  Dipole-Dipole is the intermolecular force that exists with polar covalent compounds. (3rd Strongest) Ex: CHCl3               HCl                   HBr                  HI   4) Dipole/Induced-Dipole is the intermolecular force that exists when a nonpolar covalent compound interacts with a polar covalent compound. (4th Strongest) Ex:       S8 (nonpolar solute) in  H2O (polar solvent)     5)  London Dispersion or Van der Waals Forces is the intermolecular force that exists with nonpolar covalent compounds. (Weakest)    
Which of the following has the strongest intermolecular forces? 1. F2 2. Ne 3. BrF 4. CO2
The strongest intermolecular forces between hydrogen sulfide (H 2S) molecules arise from  1. dipole-dipole forces 2. dispersion forces 3. hydrogen bonding 4. ion-dipole interactions 5. disulfide linkages
The strongest intermolecular forces between LiF particles are 1. dipole-dipole forces 2. dispersion forces 3. hydrogen bonding  4. ion-dipole interactions
Which of the following exhibits hydrogen bonding? 1. H3COCH3 2. CH3NH2 3. CH3SH 4. CH3Cl 5. HCl  
Which of the following compounds could not participate in hydrogen-bonding? a) H2O b) CH3NH2 c) CH3OH d) CH3Cl e) NH3
Which of the following can form intermolecular hydrogen bonds in the pure liquid? A. 1 only B. 2 only C. 3 only D. 2 and 3 only E. 1 and 2 only
Place the following compounds in order of  increasing strength of intermolecular forces. CO2      F2      NH 2CH3   A) F2  < NH 2CH 3 <  CO2 B) NH 2CH3  <  F2 <  CO2 C) CO2  < NH2CH3 <  F2 D) F2  <  CO2 <  NH2CH3 E) NH2CH3  <  CO2 <  F2
Give the major intermolecular force in seawater. A) dipole-dipole B) dispersion (London dispersion) C) hydrogen bonding D) ion-ion E) ion-dipole
Choose the molecule or compound that exhibits dispersion forces as its strongest intermolecular force.  A) CO B) Cl2 C) HF D) NaCl E) All of these have intermolecular forces stronger than dispersion. 
Identify the principal intermolecular forces that exist between molecules in each of the following species: a. C6H6   b. CH3Cl   d. CS2   e. CH3OH   f.  PF3    
 Define hydrogen bonding and indicate the hydrogen bonding interactions in water. 
List the following compounds in order of increasing strength of intermolecular forces. Cl2         F 2          NH2CH2CH3 A. NH2CH2CH3 < Cl2 < F2 B. F2 < NH2CH2CH3 < Cl2 C. NH2CH2CH3 < F2 < Cl2 D. F2 < Cl2 < NH2CH2CH3 E. Cl2 < F2 < NH2CH2CH3
What are the major attractive forces in an aliquot of pure carbon tetrachloride CCl 4? a) dipole-induced dipole b) dispersion c) ion-ion d) ion-dipole e) dipole-dipole
Which one of the following substances will have hydrogen bonding as one of its intermolecular forces?
What types of intermolecular forces exist between HI and H 2S? A) dispersion forces and dipole-dipole B) dipole-dipole and ion-dipole  C) dispersion forces, dipole-dipole, and ion-dipole  D) dispersion forces, hydrogen bonding, dipole-dipole, and ion-dipole  E) dispersion forces, dipole-dipole, and ion-dipole
Which is expected to have the largest dispersion forces?  A) C3H8 B) C12H26 C) F2 D) BeCl2
Methane (CH4) forms a molecular solid. What type of forces hold it in a solid configuration? I) London forces II) dipole-dipole forces III) hydrogen bonding 1. I only 2. II only 3. I, II, and III 4. I and II only 5. II and III only 6. III only
In general, intramolecular forces determine the __________ properties of a substance and intermolecular forces determine its __________ properties. A. chemical, physical       B. physical, chemical       C. solution, intrinsic     D. pressure, viscosity
What types of intermolecular forces exist between PH 3 and CO? A. hydrogen bonding       B. dispersion forces and hydrogen bonding       C. dispersion forces D. dipole-dipole and hydrogen bonding        E. dispersion forces and dipole-dipole
Liquid hydrogen is used as one part of the booster fuel in the space shuttle. What type of forces exist between hydrogen molecules in liquid hydrogen? 1. a mixture of all these forces 2. dispersion forces 3. hydrogen bonding 4. dipole forces
The DOMINANT intermolecular force that causes gaseous HCl molecules to attract one another is 1. dipole-dipole 2. covalent 3. None of these is dominant. 4. Ionic 5. van der Waals
Which of the following can be expected to exhibit the strongest hydrogen bonding in the liquid state? 1. CH4 2. CH3COCH3 3. CH3OCH3 4. CH3OH 5. CH3CH3
What types of intermolecular interactions does ammonia (NH 3) exhibit? I) dispersion forces II) dipole-dipole interaction III) hydrogen bonding IV) covalent bonding 1. I and II only 2. I, II, and III only 3. II and III only 4. II and IV only 5. I only 6. II only
Which option contains substances that can exhibit only London dispersion forces, and no other intermolecular forces? A) SF6        CH 4         Ne B) H2O       CH 4         Ne C) SF6        CH 4         NaCl D) NaCl       H2O        CH 4 E) BaSO4    Ne          CH 4
Consider water and glycerol , CH2( OH)CH(OH)CH2OH.List the intermolecular attractions that occur between a water molecule and a glycerol molecule.
For the homogeneous solution, consisting of Br2 and CCl4, indicate the type of forces that are involved.
Which type of intermolecular attractive force operates between all molecules?
What is the dispersion force? What does the magnitude of the dispersion force depend on? How can you predict the magnitude of the dispersion force for closely related elements or compounds?
The following data present the temperatures at which certain vapor pressures are achieved for dichloromethane (CH2 Cl2 ) and methyl iodide (CH3 I): Vapor Pressure (torr): 10.0 40.0 100.0 400.0 T for CH2 Cl2 (oC): -43.3 -22.3 -6.3 24.1 T for CH3 I(oC): -45.8 -24.2 -7.0 25.3 Which is expected to have the greater London dispersion forces?
Molecular weights, dipole moments, and boiling points of several simple organic substances.Moving from left to right, do the dispersion forces get stronger, get weaker, or stay roughly the same in the molecules shown above?
The table below shows the normal boiling points of benzene and benzene derivatives. Which of these compounds exhibit hydrogen bonding?
Which type of intermolecular attractive force operates only between the hydrogen atom of a polar bond and a nearby small electronegative atom?
Hydrogen bonding. Hydrogen bonding can occur when an H atom is bonded to an N, O, or F atom.To form a hydrogen bond, what must the non-hydrogen atom (N, O, or F) involved in the bond possess?
What is hydrogen bonding? How can you predict the presence of hydrogen bonding in a compound?
What kind of intermolecular attractive force is shown in each of the following cases? Picture (a)
What kind of intermolecular attractive force is shown in each of the following cases? Predict which of the four interactions is the weakest
What kind of intermolecular attractive force is shown in each of the following cases? Picture (b)
What kind of intermolecular attractive force is shown in each of the following cases? Picture (c)
What kind of intermolecular attractive force is shown in each of the following cases? Picture (d)
Intermolecular and intramolecular interactions.How would you expect the H-Cl distance represented by the red dotted line to compare with the H-Cl distance within the HCl molecule?
Look up and compare the normal boiling points and normal melting points of H2O and H2S.What kinds of intermolecular forces exist for H2O?
Look up and compare the normal boiling points and normal melting points of H2O and H2S.What kind of intermolecular forces exist for H2S?
The table below lists the density of O2 at various temperatures and at 1 atm. The normal melting point of O2 is 54 K. Temperature (K) Density (mol/L) 60 40.1 70 38.6 80 37.2 90 35.6 100 0.123 120 0.102 140 0.087 What intermolecular forces are operative in O2?
Melting and boiling points for benzene, toluene, and phenol.In which substance, benzene or toluene, are the intermolecular forces stronger?
Why are intermolecular forces important?
Describe the relationship between the state of a substance, its temperature, and the strength of its intermolecular forces.
From what kinds of interactions do intermolecular forces originate?
Why are intermolecular forces generally much weaker than bonding forces?
Acetone, (CH3 )2 CO, is widely used as an industrial solvent.What kinds of intermolecular attractive forces exist between acetone molecules?
Flowchart for determining intermolecular forces. Multiple types of intermolecular forces can be at work in a given substance or mixture. In particular, dispersion forces occur in all substances.Can the energies of multiple dispersion forces between two molecules be larger than the energy of hydrogen bonding between the two molecules?
How does the average kinetic energy of molecules compare with the average energy of attraction between molecules in solids?
How does the average kinetic energy of molecules compare with the average energy of attraction between molecules in liquids?
How does the average kinetic energy of molecules compare with the average energy of attraction between molecules in gases?
Determine the kinds of intermolecular forces that are present in each of the following elements or compounds.HCl
Determine the kinds of intermolecular forces that are present in each of the following elements or compounds.H2O
Determine the kinds of intermolecular forces that are present in each of the following elements or compounds.Br2
Determine the kinds of intermolecular forces that are present in each of the following elements or compounds.He
Water molecules in the atmosphere can form hydrogen-bonded dimers, (H2O) 2. The presence of these dimers is thought to be important in the nucleation of ice crystals in the atmosphere and in the formation of acid rain.What kind of intermolecular forces are involved in water dimer formation?
Ion-dipole forces. Why does the O side of H2O point toward the Na+ ion?
What is the ion-dipole force? Why is it important?
Which type of intermolecular attractive force operates only between polar molecules?
What is the dipole-dipole force? How can you predict the presence of dipole-dipole forces in a compound?
Two isomers of the planar compound 1,2-dichloroethylene are shown here, along with their melting and boiling points. Which of the two isomers will have the stronger dipole-dipole forces?
Which of the following intermolecular forces of attraction is the strongest? a. hydrogen bonding b. dipole-dipole forces c. dispersion forces d. London forces e. dipole-induced dipole forces
Draw out the Lewis Structure and answer the following questions. SiBr42– Number of Valence Electrons:Molecular Geometry:Electronic Geometry: Hybridization:Unhybridized Orbitals:Polarity:Bonding orbitals (Si – Br):Intermolecular Force:
List all the intermolecular forces present in pure acetone.
Draw out the Lewis Structure and answer the following questions. SF6                              Number of Valence Electrons:Molecular Geometry:Electronic Geometry:Hybridization:Unhybridized Orbitals:Polarity:Bonding orbitals (S – F):Intermolecular Force:
Why is I2 a solid while Cl2 is a gas even though they are both halogens?1. I2 is more polarizable than Cl2.2. I2 has a smaller dipole than Cl2.3. I2 is less polarizable than Cl2.4. I2 has a larger dipole than Cl2.5. I2 has H-bonding and Cl2 does not.
Identify the predominant type of intermolecular force in each of the following compounds. Drag each item to the appropriate bin.
A substance has a melting point of 1200 K, and it conducts electricity in the melted state (liquid) but not in the solid state. What is the name of the major attractive force that holds this substance together?1. hydrogen bonds2. metallic bonds3. dispersion forces4. dipole-dipole attractions5. ionic bonds
What are all of the intermolecular forces that are responsible for the existence of dry ice (solid CO2)?1. hydrogen bonding and dipole-dipole2. London forces 3. dipole-dipole, London forces, and hydrogen bonding4. dipole-dipole and ion-ion5. dipole-dipole and London forces
Which of the following molecules can form hydrogen bonds? Select one.a. NH3b. CH4c. NaHd. BH3e. HI
State the kind of intermolecular forces that would occur between the solute and solvent in barium nitrate (ionic) solution. Check all that apply.a. dispersionb. hydrogen bondingc. ion-dipoled. dipole-dipole
Select the major force between the molecules in pure, liquid acetone.A. ion-ionB. ion-dipoleC. hydrogen bondingD. dipole-dipoleE. dispersion 
Choose the molecule that exhibits London (dispersion) forces as its strongest intermolecular force.a. Cl2b. COc. HFd. NaCle. All of these have intermolecular forces stronger than dispersion
What is the strongest type of intermolecular force present in NH 2CH3?a. dispersionb. dipole-dipolec. hydrogen bondingd. ion-dipolee. none of the above
Identify the kinds of intermolecular forces that might arise between molecules of CH3OH. 1. None of these 2. dispersion forces, dipole-dipole 3. dipole-dipole 4. dispersion forces 5. hydrogen bonding 6. dispersion forces, dipole-dipole, hydrogen bonding
Determine the kinds of intermolecular forces (from below) that are present in the compound H2S. a) dispersion forces b) dipole–dipole forces c) dispersion forces and dipole–dipole forces d) hydrogen bonding
Give the major force between ethanol and waterA. dipole–dipoleB. dispersionC. hydrogen–bondingD. ion–dipoleE. ion–ion
Which of the following compounds exhibits hydrogen bonding? A) CH3CH2NH2 B) C6H5OC6H5 C) CH3I D) H2S
Which intermolecular forces contribute to the dissolution of NaCl in water? Select all that apply.a. ion-dipole forcesb. ion-ion forcesc. dipole-dipole forcesd. hydrogen bonding
Which of the following statements describe hydrogen bonding between water molecules or describe properties of water that lead to hydrogen bonding between water molecules?a. The slightly negative oxygen atom of one water molecule is attracted to the slightly positive hydrogen atom of another water molecule.b. The slightly positive hydrogen atom is attracted to the slightly negative oxygen atom within a single water molecule.c. Water is polar due to its bent structure and an unequal sharing of electrons.d. Water is nonpolar due to its linear structure and unequal sharing of electrons.
Suppose that NaCl is added to hexane instead of water. Which of the following intermolecular forces will exist in the system? Select all that apply.a. Hydrogen bonding between Na+ ions and a hexane moleculeb. London dispersion force between two hexane moleculesc. Ion-dipole force between Na+ ions and a hexane moleculed. Ion-ion force between Na+ and Cl- ionse. Dipole-dipole force between two hexane molecules
What intermolecular attractive force is primarily responsible for the solubility of chlorine, Cl2, in water?a. dipole - dipoleb. hydrogen bondingc. dipole-induced dipoled. ion-dipolee. ion-induced dipole
If a solid line represents a covalent bond and a dotted line represents intermolecular attraction, which of these choices shows a hydrogen bond? Check all that apply
Consider four moleculesI) CHCl3II) CH4III) CH3ClIV) CCl4Which of these exhibit permanent dipole-dipole interactions?1. I only2. III only3. I and III only4. None of these5. I, III, and IV only
It is common to add Epson salts to bath water when one has been over exercising and has sore muscles. What is the primary intermolecular force that exists between magnesium sulfate, the primary in Epson salts, and the water in the bathtub?a) dipole-dipole forcesb) ion-dipole forcesc) London forcesd) ion-ion forcese) dipole-induced dipole forces
What is the strongest intermolecular force present in SO2 ? (EN Values: S = 2.5; O = 3.5)A) Dispersion forces (London dispersion)B) Dipole-Dipole forceC) Hydrogen-BondD) Ion-Dipole forceE) Covalent Bond
Identify which of the following are correct conditions for forming a hydrogen bond: a) A hydrogen bond is equivalent to a covalent bond. b) The CH4 molecule exhibits hydrogen bonding. c) A hydrogen bond is possible with only certain hydrogen-containing compounds. d) Hydrogen bonding occurs when a hydrogen atom is covalently bonded to an N, O or F atom. e) A hydrogen atom acquires a partial positive charge when it is covalently bonded to an F atom.
Intermolecular forces are:             A.  between molecules and weaker than a chemical bond.             B.  between two atoms within a molecule and weaker than a chemical bond.             C.  between molecules and stronger than a chemical bond.             D. between two atoms within a molecule and stronger than a chemical bond.             E. between electrons within an atom and stronger than a chemical bond.
What is the intermolecular force that exists between a calcium ion and water? a. ion-dipole b. Covalent bonding c. London dispersion forces d. ion-ion e. dipole-dipole forces
Which of the following molecules will show only intermolecular dispersion force?
Determine the kinds of intermolecular forces that is/are present in the following compound. CH3OHa) dispersion forcesb) dipole-dipole forcesc) hydrogen bondingd) dispersion forces, dipole-dipole forces, and hydrogen bonding
Sort the following events by the dominant type of force overcome or formed:
Which of the following is correct?a) The energy of dipole-dipole interactions is about 2 kJ • mol -1.b) The energy of ion-dipole interactions is about 2 kJ • mol -1.c) The energy of London forces is about 2 kJ • mol -1.d) The energy of a hydrogen bond is about 2 kJ • mol -1.e) The energy of ion-ion interactions is about 2 kJ • mol -1.
Choose the molecule or compound that exhibits dispersion forces as its strongest intermolecular force.A) O2B) COC) HFD) NaClE) All of these have intermolecular forces stronger than dispersion.
Determine the kinds of intermolecular forces present in each element or compound:N2, NH3, CO, CCl4, HCl, H2O
The predominant intermolecular force in BF3 is:  London Dispersion Hydrogen Bonding Ion-Dipole Dipole-Dipole Dipole-induced Dipole
Which of the following substances have polar interactions (dipole-dipole forces) between molecules?a) F2b) Cl2c) ClFd) NF3
What is/are the strongest intermolecular force(s) in acetone?a. H-bondingb. dipole-dipolec. dispersion
Below are various rankings of intermolecular forces, which option correctly ranks the given forces from weakest to strongest? a) dipole-dipole < ion-dipole < ion-induced dipole b) dispersion < ion-induced dipole < dipole-induced dipole c) dipole-dipole < hydrogen bonding < dipole-induced dipole d) ion-induced dipole < dipole-dipole < hydrogen bonding e) dipole-induced dipole < hydrogen bonding < ion-induced dipole
Which of the responses includes all of the following that can form hydrogen bonds with water molecules?(A) Na+      (B) CH 3COOH     (C) C2H6     (D) CH 3NH21) (A) and (B)2) (A) and (C)3) (B) and (C)4) (B) and (D)5) (C) and (D)
Draw out the Lewis Structure and answer the following questions. IF2– Number of Valence Electrons:Molecular Geometry:Electronic Geometry:Hybridization:Unhybridized Orbitals:Polarity:Bonding Orbitals (I – F):Intermolecular Force:
Why is water an extraordinary substance?A) Water has a low molar mass, yet it is a liquid at room temperature.B) Water is the main solvent within living organisms.C) Water has an exceptionally high specific heat capacity.D) Water has strong hydrogen bonding.E) All of the above.
Which has the smallest dipole-dipole forces?A) CH3ClB) HBrC) O2D) NO
Determine the kinds of intermolecular forces that are present in the following element or compound: SiH4a) Dispersion forcesb) Dipole-dipole forcesc) Hydrogen bonding
What intermolecular forces are present in each of the substances?a. CH4b. C3H8c. CH3Fd. HFe. C6H5OH 
Draw out the Lewis Structure and answer the following questions. COCl2Number of Valence Electrons:Molecular Geometry:Electronic Geometry:Hybridization:Unhybridized Orbitals:Polarity:Bonding Orbitals (C – O):Intermolecular Force:
Place the following compounds in order of decreasing strength of intermolecular forces.HF        H2       CO 2A) HF > CO2 > H2B) HF > H2 > CO2C) H2 > CO2 > HD) CO2 > HF > H 2E) CO2 > H2 > HF
Draw out the Lewis Structure and answer the following questions. C2H4Number of Valence Electrons:Molecular Geometry:Electronic Geometry:Hybridization:Unhybridized Orbitals:Polarity:Bonding Orbitals (C – H):Intermolecular Force:
Identify the intermolecular forces present in each of these substances:HCl, He, CO, HFMatch these to the correct groups below.1. Hydrogen bonding, dipole-dipole and dispersion2. Dipole-dipole and dispersion only3. Dispersion only
Which of the following exhibit only london (dispersion) forces?He, HCl, H2O, Cl2
Identify the intermolecular forces present in each of these substances.NH3, CO, CO2, CH3Cl
Which interactions and processes contribute to the dissolution of ionic compounds in water? Check all that apply. A) Hydration B) Affinity of oxygen towards cations C) Ion–dipole interactions D) Hydrogen bonding E) Affinity of hydrogen towards anions F) Dipole–dipole interactions
What is the strongest intermolecular force in SO 2? a) dipole-dipole b) london dispersion c) ionic d) hydrogen bonding
Identify the intermolecular forces present in each of these substances.HF, CO, H2, and HCl.
Arrange the non-covalent interactions in order of strength.ion-ion interactionsdipole-dipole interactionsdispersion forceshydrogen bonding
Choose the molecule or compound that exhibits dipole-dipole forces as its strongest intermolecular force.a. NH3b. CF4c. SO2d. BCl3e. H2
Which of the following molecules can form intermolecular hydrogen bonds as a pure liquid? a. I, II, and III b. II and IV c. I and III d. All molecules form hydrogen bond interactions e. None of the molecules form hydrogen bond interactions
For each of the following molecules, would you expect greater solubility in water or in hexane?For each case, indicate the kinds of intermolecular forces that occur between the solute and the solvent in which the molecule is most soluble.
You may want to reference (Pages 122 - 125) Section 4.1 while completing this problem.Would you expect that an anion would be physically closer to the oxygen or to the hydrogens of water molecules that surround it in solution?
In which mixture do you expect to find ion–dipole forces between solute and solvent to exist: CH3OH in water or Ca(NO3)2 in water?
For the homogeneous solution, consisting of CH3CH2OH and H2O, indicate the type of forces that are involved.
Pick an appropriate solvent from the table below to dissolve each of the following.Common Laboratory SolventsCommon Polar SolventsCommon Nonpolar SolventsWater (H2O)Hexane (C6H14)Acetone (CH3COCH3)Diethyl ether(CH3CH2OCH2CH3 )Methanol (CH3OH)Toluene (C7H8)Ethanol (CH3CH2OH)Carbon tetrachloride(CCl4)* Diethyl ether has a small dipole moment and can be considered intermediate between polar and nonpolar.State the kind of intermolecular forces that would occur between the solute and solvent.a. motor oil (nonpolar)b. ethanol (polar, contains an OH group)c. lard (nonpolar)d. potassium chloride (ionic)
Pick an appropriate solvent from the table below to dissolve each substance. State the kind of intermolecular forces that would occur between the solute and solvent in isopropyl alcohol (polar, contains an OH group).Common polar solventsCommon nonpolar solventsWater (H2O)Hexane (C6H14)Acetone (CH3COCH3)Diethyl ether (CH3CH2OCH2CH3)Methanol (CH3OH)Toluene (C7H8)Ethanol (CH3CH2OH)Carbon tetrachloride (CCl4)
Pick an appropriate solvent from the table below to dissolve each substance.  State the kind of intermolecular forces that would occur between the solute and solvent in sodium chloride (ionic).Common polar solventsCommon nonpolar solventsWater (H2O)Hexane (C6H14)Acetone (CH3COCH3)Diethyl ether (CH3CH2OCH2CH3)Methanol (CH3OH)Toluene (C7H8)Ethanol (CH3CH2OH)Carbon tetrachloride (CCl4)
What is the strongest type of intermolecular force between solute and solvent in each solution?(b) Ne(g) in H2O(l)
Pick an appropriate solvent from the table below to dissolve each substance. State the kind of intermolecular forces that would occur between the solute and solvent in paraffine oil (nonpolar).Common polar solventsCommon nonpolar solventsWater (H2O)Hexane (C6H14)Acetone (CH3COCH3)Diethyl ether (CH3CH2OCH2CH3)Methanol (CH3OH)Toluene (C7H8)Ethanol (CH3CH2OH)Carbon tetrachloride (CCl4)
Pick an appropriate solvent from the table below to dissolve each substance. State the kind of intermolecular forces that would occur between the solute and solvent in sodium nitrate (ionic).Common polar solventsCommon nonpolar solventsWater (H2O)Hexane (C6H14)Acetone (CH3COCH3)Diethyl ether (CH3CH2OCH2CH3)Methanol (CH3OH)Toluene (C7H8)Ethanol (CH3CH2OH)Carbon tetrachloride (CCl4)
Which of the following pairs of compounds would you expect to form homogeneous solutions when combined?a. CH3CH2CH2CH2CH3 and CH3CH2CH2CH2CH2CH3b. CBr4 and H2Oc. LiNO3 and H2Od. CH3OH and CH3CH2CH2CH2CH3
Indicate the types of forces that are involved when forming a homogeneous solution between CH3CH2CH2CH2CH3 and CH3CH2CH2CH2CH2CH3.
Indicate the types of forces that are involved when forming a homogeneous solution between LiNO3 and H2O.
Explain the cleansing action of soap.
Indicate the kinds of intermolecular forces that would occur between the toluene and hexane:
Indicate the kinds of intermolecular forces that would occur between the sucrose and water:
Indicate the kinds of intermolecular forces that would occur between the isobutene and hexane:
Indicate the kinds of intermolecular forces that would occur between the ethylene glycol and water:
Which species in each pair has the greater polarizability? Explain.(a) Br− or I−
Which species in each pair has the greater polarizability? Explain.(b) CH2=CH2 or CH3—CH3
Which species in each pair has the greater polarizability? Explain.(c) H2O or H2Se
Which species in each pair has the greater polarizability? Explain.(a) Ca2+ or Ca
Which species in each pair has the greater polarizability? Explain.(b) CH3CH3 or CH3CH2CH3
Which species in each pair has the greater polarizability? Explain.(c) CCl4 or CF4
Define the following and give an example of each:(a) dispersion force
Put the following molecules in order of increasing polarizability: GeCl4, CH4, SiCl4, SiH4, and GeBr4.
Which member of the following pairs has the larger London dispersion forces?H2O or H2S?
Which member of the following pairs has the larger London dispersion forces?CO2 or CO?
Given each pair, complete the sentences to determine which member of each has the stronger intermolecular dispersion forces.
Which type(s) of bonding is (are) found within hydrocarbon molecules? a. Hydrogen Bonding b. Covalent Bonding c. Van der Waals d. Metallic e. Ionic
Consider the following enthalpy changes:F2 + HF → FHF -                                              ΔH = -155 kJ/mol(CH3)2C=O + HF → (CH 3)2C=O---HF             ΔH = -46 kJ/molH2O (g) +  HOH (g) → H2O---HOH (in ice)       ΔH = -21 kJ/molHow do the strengths of hydrogen bonds vary with the electronegativity of the element to which hydrogen is bonded? Where in the preceding series would you expect hydrogen bonds of the following type to fall?
Which member of each pair of compounds forms intermolecular H bonds? Draw the H-bonded structures in each case:a.  or CH3SCH3
Which member of each pair of compounds forms intermolecular H bonds? Draw the H-bonded structures in each case:(b) HF or HBr
Which member of each pair of compounds forms intermolecular H bonds? Draw the H-bonded structures in each case:(a) (CH3)2NH or (CH3)3N
Which member of each pair of compounds forms intermolecular H bonds? Draw the H-bonded structures in each case:(b) HOCH2CH2OH or FCH2CH2F
The table below shows the normal boiling points of benzene and benzene derivatives.Which of these compounds exhibit dipole-dipole interactions?
The following molecules have the same molecular formula (C3H8O), but different chemical structures.propanolethyl methyl etherWhich molecule(s), if any, can engage in hydrogen bonding?
Explain why a hydrogen bond between two water molecules is weaker than a hydrogen bond between two hydrogen fluoride molecules
A chemist is studying small organic compounds to evaluate their potential for use as an antifreeze. When 0.243 g of a compound is dissolved in 25.0 mL of water, the freezing point of the solution is −0.201°C.(a) Calculate the molar mass of the compound (d of water = 1.00 g/mL).(b) Analysis shows that the compound is 53.31 mass % C and 11.18 mass % H, the remainder being O. Determine the empirical and molecular formulas of the compound.(c) Draw a Lewis structure for a compound with this formula that forms H bonds and another for one that does not.
For pairs of molecules in the gas phase, average H-bond dissociation energies are 17 kJ/mol for NH3, 22 kJ/mol for H2O, and 29 kJ/mol for HF. Explain this increase in H-bond strength.
Furfural, which is prepared from corncobs, is an important solvent in synthetic rubber manufacturing, and it is reduced to furfuryl alcohol, which is used to make polymer resins. Furfural can also be oxidized to 2-furoic acid.Which of these compounds can form H bonds? Draw structures in each case.
Furfural, which is prepared from corncobs, is an important solvent in synthetic rubber manufacturing, and it is reduced to furfuryl alcohol, which is used to make polymer resins. Furfural can also be oxidized to 2-furoic acid.The molecules of some substances can form an “internal” H bond, that is, an H bond  within a molecule. This takes the form of a polygon with atoms as corners and bonds as sides and an H bond as one of the sides. Which of these molecules is (are) likely to form a stable internal H bond? Draw the structure. (Hint: Structures with 5 or 6 atoms as corners are most stable.)
The ball-and-stick models below represent three compounds with the same molecular formula, C4H8O2:(a) Which compound(s) can form intermolecular H bonds?
Define the following and give an example of each:(c) hydrogen bond
What major type of attractive interaction must be overcome for water to evaporate?
You may want to reference (Pages 439 - 445) Section 11.2 while completing this problem.Which of the following molecules can form hydrogen bonds with other molecules of the same kind: CH3F, CH3NH2, CH3OH, CH3Br?
What is/are the strongest intermolecular force(s) in methanol?a. H-bondingb. dipole-dipolec. dispersion
Rank these compounds by their expected solubility in hexane, C6H14.
Rank these compounds by their expected solubility in hexane C6H14. C2H5OH, H2O, C2H6
What is/are the strongest intermolecular force(s) in 2-propanol?a. H-bondingb. dipole-dipolec. dispersion
What is/are the strongest intermolecular force(s) in water?a. H-bondingb. dipole-dipolec. dispersion
Describe the intermolecular forces that must be overcome to convert each of the following from a liquid or solid to a gas.SO2
Describe the intermolecular forces that must be overcome to convert each of the following from a liquid or solid to a gas.CH3CH2OH
Describe the intermolecular forces that must be overcome to convert each of the following from a liquid or solid to a gas.H2Se
In the molecule below, how many atoms could make hydrogen bonds with water? a. 5 b. 7 c. 9 d. 10 e. 12
Identify the most important type of interparticle forces present in solid Ar.
Identify the most important type of interparticle forces present in solid HCl.
Identify the most important type of interparticle forces present in solid HF.
Identify the most important type of interparticle forces present in solid CaCl 2.
Identify the most important type of interparticle forces present in solid CH 4.
Identify the most important type of interparticle forces present in solid CO.
What is the strongest interparticle force in each substance?(a) CH3OH
Spontaneous dissolving under standard-state conditions at 25oC occurs with a mix of a. CH2Cl2 & H2O b. KNO3 & CH2Cl2 c. acetone & H2O d. CH2Cl2 & NaCl
What is the strongest interparticle force in each substance?(b) CCl4
Identify the most important type of interparticle forces present in solid NaNO 3.
Identify the most important type of interparticle forces present in solid BaSO 4.
Identify the most important type of interparticle forces present in solid H 2S.
List the intermolecular forces that occur for CCl3F.
Identify the most important type of interparticle forces present in solid Xe.
What is the strongest interparticle force in each substance?(a) H3PO4
You may want to reference (Pages 450 - 453) Section 11.4 while completing this problem.The critical temperatures (K) and pressures (atm) of a series of halogenated methanes are as follows:CompoundCCl3FCCl2F2CClF3CF4Critical Temperature (K)471385302227Critical Pressure (atm)43.540.638.237.0Predict the order of decreasing intermolecular attraction, from least to most, for this series of compounds.
List the intermolecular forces that occur for CCl2F2.
Identify the most important type of interparticle forces present in solid C 2H6.
What is the strongest interparticle force in each substance?(c) MgCl2
List the intermolecular forces that occur for CClF3.
Identify the most important type of interparticle forces present in solid CsI.
List the intermolecular forces that occur for CF4.
Identify the most important type of interparticle forces present in solid P 4.
What is the strongest interparticle force in each substance?(a) CH3Cl
What is the strongest interparticle force in each substance?b) CH3CH3
Identify the most important type of interparticle forces present in solid NH 3.
What is the strongest interparticle force in each substance?(c) NH3
Predict which substance between CO2 or OCS would have the greater intermolecular force.
What is the strongest interparticle force in each substance?(a) Kr
Predict which substance between SeO 2 or SO 2 would have the greater intermolecular force.
What is the strongest interparticle force in each substance?(b) BrF
Predict which substance between CH 3CH2CH2NH2 or H2NCH2CH2NH2 would have the greater intermolecular force.
What is the strongest interparticle force in each substance?(c) H2SO4
Predict which substance between CH 3CH3 or H2CO would have the greater intermolecular force.
Predict which substance between CH 3OH or H2CO would have the greater intermolecular force.
Which of the following compound(s) exhibit only London dispersion intermolecular forces? Which compound(s) exhibit hydrogen-bonding forces? Considering only the compounds without hydrogen-bonding interactions, which compounds have dipole–dipole intermolecular forces?a. SF4                   d. HFb. CO2                 e. ICl  5c. CH3CH2OH    f. XeF4
Which of the following statements about intermolecular forces is(are) true?a. London dispersion forces are the only type of intermolecular force that nonpolar molecules exhibit.b. Molecules that have only London dispersion forces will always be gases at room temperature (25 ˚C).c. The hydrogen-bonding forces in NH 3 are stronger than those in H 2O.d. The molecules in SO 2 (g) exhibit dipole–dipole intermolecular interactions.e. CH3CH2CH3 has stronger London dispersion forces than does CH 4.
Which forces oppose vaporization of each substance?(a) Hexane
Which forces oppose vaporization of each substance?(b) Water
Which forces oppose vaporization of each substance?(c) SiCl4
Which forces oppose vaporization of each substance?(a) Br2
Which forces oppose vaporization of each substance?(b) SbH3
Which forces oppose vaporization of each substance?(c) CH3NH2
Spontaneous dissolving under standard-state conditions at 25oC occurs with a mix of: a. KNO3 & n-butanol b. I2 & CH2Cl2 c. CaCO3 & hexane d. acetone & KNO3  
One of these substances is a liquid at room temperature. Which one?a) CH3OHb) CF4c) SiH4d) CO2
Under certain conditions, molecules of acetic acid, CH3COOH, form “dimers,” pairs of acetic acid molecules held together by strong intermolecular attractions:Draw a dimer of acetic acid, showing how two CH3COOH molecules are held together, and stating the type of IMF that is responsible.
Proteins are chains of amino acids that can form in a variety of arrangements, one of which is a helix. Whatkind of IMF is responsible for holding the protein strand in this shape? On the protein image, show the locations of the IMFs that hold the protein together:
At room temperature, Si is a solid, CCl4 is a liquid, and Ar is a gas.List these substances in order of decreasing intermolecular energy of attraction.
Which is generally stronger, intermolecular interactions or intramolecular interactions?
You may want to reference (Pages 439 - 445) Section 11.2 while completing this problem.Which of these kinds of interactions, intermolecular interactions or intramolecular interactions, are broken when a liquid is converted to a gas?
Identify the intermolecular forces present in the following solids:(a) CH3CH2OH
A number of salts containing the tetrahedral polyatomic anion, BF4–, are ionic liquids, whereas salts containing the somewhat larger tetrahedral ion SO42– do not form ionic liquids. Explain this observation.
Identify the intermolecular forces present in the following solids:(b) CH3CH2CH3
Based on their composition and structure, list CH2Cl2, CH3CH2CH3, and CH3CH2OH in order of decreasing intermolecular forces.
Identify the intermolecular forces present in the following solids:(c) CH3CH2Cl
Which forces are intramolecular and which intermolecular?(a) Those preventing oil from evaporating at room temperature(b) Those preventing butter from melting in a refrigerator(c) Those allowing silver to tarnish(d) Those preventing O2 in air from forming O atoms
What is the evidence that all neutral atoms and molecules exert attractive forces on each other?
Which forces are intramolecular and which intermolecular?(a) Those allowing fog to form on a cool, humid evening(b) Those allowing water to form when H2 is sparked(c) Those allowing liquid benzene to crystallize when cooled(d) Those responsible for the low boiling point of hexane
Use the figure below to answer the following: What is the principal intermolecular force in CH4 and Hg?
Determine the kinds of intermolecular forces that are present in each element or compound.Kr
Determine the kinds of intermolecular forces that are present in each element or compound.NCl3
Determine the kinds of intermolecular forces that are present in each element or compound.SiH4
Determine the kinds of intermolecular forces that are present in each element or compound.HF
Consider the formation of the three solutions shown in the table.a. Rank the solutions A, B, and C from the most exothermic to the most endothermic.b. Rank the enthalpy of solution from most exothermic to most endothermic. To rank items as equivalent, overlap them.
Water and toluene are not miscible. Which of the following is most likely the formula of toluene?a. C6H5CH3b. C6H12O6c. CH3OHd. CH3COOH
Which of the following will be the most soluble in water?a. CH3CH2CH2CH2CH2CH2OH b. CH3CH2CH2OHc. CH3CH2CH2CH2OHd.  CH3CH2CH2CH2CH2OH
List the substances Ar, Cl2, CH4, and CH3COOH, in order of increasing strength of intermolecular attractions.
You may want to reference (Pages 439 - 445) Section 11.2 while completing this problem.Which of the following statements are true?(a) For molecules with similar molecular weights, the dispersion forces become stronger as the molecules become more polarizable.(b) For the noble gases the dispersion forces decrease while the boiling points increase as you go down the column in the periodic table.(c) In terms of the total attractive forces for a given substance, dipole–dipole interactions, when present, are always greater than dispersion forces.(d) All other factors being the same, dispersion forces between linear molecules are greater than those between molecules whose shapes are nearly spherical.(e) The larger the atom, the more polarizable it is.
List the three states of matter in order of increasing intermolecular attractions.
Identify the kinds of intermolecular forces that are present in each element or compound.N2
Identify the kinds of intermolecular forces that are present in each element or compound.NH3
Identify the kinds of intermolecular forces that are present in each element or compound.CO
Identify the kinds of intermolecular forces that are present in each element or compound.CCl4
Identify the kinds of intermolecular forces that are present in each element or compound.H2S
What atoms must a molecule contain to participate in hydrogen bonding with other molecules of the same kind?
Identify the kinds of intermolecular forces that are present in each element or compound.HBr
Identify the kinds of intermolecular forces that are present in each element or compound.CH3OH
Identify the kinds of intermolecular forces that are present in each element or compound.I2
Identify which of the following molecules can exhibit hydrogen bonding as a pure liquid.
The following image is an electrostatic potential map for ethylene oxide, (CH2)2O, a polar molecule.Use the electrostatic potential map to predict the geometry for how one ethylene oxide molecule interacts with another.
An electrostatic potential map for acetonitrile (CH3CN), which is polar, is shown below.From this map, determine the geometry for how two acetonitrile molecules would interact with each other.
Which substance experiences dipole-dipole forces?a) CCl4b) NF3c) CS2d) SO3
Define the following and give an example of each:(b) dipole-dipole attraction
Electronegativities of the ElementsElementElectronegativityH2.1C2.5O3.5F4.0Si1.8Cl3.0Br2.8I2.5Which molecules have dipole-dipole forces?(a) CI4(b) CH3Cl(c) HCl
Which member of the following pairs has the larger London dispersion forces?SiH4 or GeH4?
Ball-and-stick models and Lewis structures for two hydrated hydronium ions.Which type of intermolecular force do the dotted lines in this figure represent?
Classify the species given below by the intermolecular forces present in a pure sample of each:Ar H2 HCN HF BrCl5 NH3 CH3OH H2S PF5 CH2Cl2Are they dispersion, dipole-dipole, or H-bond?
How many atoms in the pictured molecule can form hydrogen bonds with water molecules? a. 5 b. 3 c. 2 d. 8 e. 7 
In the molecule below, how many atoms could make hydrogen bonds with water? a. 5 b. 7 c. 9 d. 10 e. 12
Which term represents an intermolecular force in a sample of pure water? A) hydrogen bonding B) covalent bonding C) metallic bonding D) ionic bonding
What type(s) of intermolecular forces are expected between GeH4 molecules? Choose all that apply.a. dispersionb. dipole-dipolec. ion-iond. hydrogen bonding
What type(s) of intermolecular forces are expected between  SeOF2 molecules? Choose all that apply.a. dispersionb. dipole-dipolec. ion-iond. hydrogen bonding
Identify which of the following molecules can exhibit hydrogen bonding as a pure liquid.
Which of the following molecules can form hydrogen bonds with other molecules of the same kind?a. CH3Fb. CH3NH2c. H2Od. HIe. CH3-O-CH3f. CHCl3g. HCOOH 
Does HCl contain a hydrogen bond?
Does HF have hydrogen bonding?
What types of intermolecular forces exist between hydrogen iodide molecules?I. London forcesII. dipole-dipole interactionsIII. hydrogen bondingIV. ion-dipole interactionsA. I and II only      B. I only      C. III only      D. II and III only      E. I, II, and III only
Identify the intermolecular forces present in each of these substances.NH3COCO2CH3Cl
For the homogeneous solution, consisting of KCl and H2O, indicate the type of forces that are involved.
Sort the intermolecular forces shown below by increasing strength of interaction.
Weak noncovalent interactions ____________.(a) combine to form covalent interactions. (b) always involve water.(c) can have a large cumulative effect.(d) do not include ionic interactions.
Which statement about hydrogen bonds is false? (A) They have an optimal geometry.(B) They are weak compared with covalent bonds. (C) They cause acid-base reactions in aqueous solutions to be very rapid.(D) They only occur between water molecules.
Sort the following events by the dominant type of force overcome or formed.i. the rubber in tire is covalently crosslinked through vulcanizationii. H2 and O2 as combined in a fuel cell to form wateriii. ice meltsiv. sugar dissolves in waterv. water moves up a narrow tube due to capillary action
Rank the following types of intermolecular forces in general order of decreasing strength (strongest to weakest).London dispersion, ion-dipole, hydrogen bonding, dipole-dipole
Determine the kinds of intermolecular forces that is/are present in Kr.a) dispersion forcesb) dipole-dopole forces  c) hydrogen bonding  d) dispersion forces & dipole-dipole forces
The table below shows the normal boiling points of benzene and benzene derivatives.Which of these compounds exhibit dispersion interactions?
Which one of the following exhibits dipole-dipole attraction between molecules?Cl2BCl3XeF4CO2AsH3
Rank the following compounds in order of increasing strength of intermolecular force. HCO2H, CH4, SF2 
Rank the following compounds in order of increasing boiling point (1 = lowest, 4 = highest) RbF CH3Cl CH3OH CO2
What kind of forces must be overcome in order to vaporize the liquid, CCI 4? Select all that apply. (a) dispersion forces (b) dipole-dipole forces (c) hydrogen bonds
What kind of nonbonding interaction occurs in liquids of the molecule CH3Br? (i) hydrogen bond(ii) permanent dipole (iii) induced dipole  
What kind of nonbonding interaction occurs in liquids of the molecule CH4? (i) induced dipole (ii) permanent dipole (iii) hydrogen bond 
Arrange these compounds by their expected bolling point.
What kind(s) of intermolecular forces must be overcome during the following phase changes? Solid CO2 sublimes A. Dispersion forces B. Dipole-dipole interactions C. Hydrogen bonding
What type(s) of intermolecular forces are expected between GeH4 molecules? Indicate with a Y (yes) or an N (no) which apply.(i) dipole forces (ii) induced dipole forces (iii) hydrogen bonding
Which of the following compounds exhibits hydrogen bonding? a. HCl b. CH3OH c. CH3Br d. CH3SCH3
What is the strongest type of intermolecular force present in NH2CH3? hydrogen bonding dipole-dipole ion-dipole dispersion None of the above
What is/are the strongest intermolecular force(s) in hexane?a. H-bondingb. dipole-dipolec. dispersion
Rank these compounds by their expected solubility in hexane, C6H14.
Identify which of the following molecules can exhibit hydrogen bonding as a pure liquid.
State the kind of intermolecular forces that would occur between the solute and solvent in isopentyl alcohol (polar, contains an OH group). Check all that apply.(i) dipole-dipole (ii) dispersion (iii) hydrogen bonding (iv) ion-dipole
What kind of nonbonding interaction occurs in liquids of the molecule NH3?(i) hydrogen bond(ii) permanent dipole(iii) induced dipole
Table salt and sugar dissolve in water for different reasons. Select the two forces responsible. (a) ion-dipole forces (b) London forces (c) electrostatic forces (d) dipole-dipole forces (e) hydrogen bonding
What type(s) of intermolecular forces are expected between SeOBr2 molecules? Indicate with a Y (yes) or an N (no) which apply.(i) dipole forces (ii) induced dipole forces (iii) hydrogen bonding
Which of the following substances have polar interactions (dipole-dipole forces) between molecules? F2, Cl2, ClF, NF3
What kind(s) of intermolecular forces must be overcome during the following phase changes? CHCl3 boilsA. Dispersion forces B. Dipole-dipole interactions C. Hydrogen bonding
Rank these compounds by their expected solubility in Hexane C 6H14. Rank from most soluble to lease soluble.i) C3H8ii) CH3OHiii) H2O
What kind(s) of intermolecular forces must be overcome during the following phase changes? Ice meltsA. Dispersion forces B. Dipole-dipole interactions C. Hydrogen bonding
Decide which intermolecular forces act between the molecules of each compound in the table below.
Select the single best answer. What is the strongest interparticle force in a sample of SO 2? (A) ionic bonding forces (B) dipole-dipole forces (C) dispersion forces (D) ion-induced dipole forces (E) dipole-induced dipole forces (F) hydrogen bonding forces (G) ion-dipole forces
What kind of intermolecular forces act between a hydrogen cyanide (HCN) molecule and a dichloroethylene (CH2CCl2) molecule? Note: If there is more than one type of intermolecular force that acts, be sure to list them all, with a comma between the name of each force. 
Which of the following molecules can hydrogen bond? 
Which diagram CORRECTLY represent a hydrogen bond? 
What type of interaction occurs between atoms in a nonbonding atomic solid.a. covalent bondingb. weak dispersion forcesc. polar bondingd. ionic bonding  
Organic compounds are always polar and dissolve in water a. True b. False
Which of the following substances has the highest boiling point?a. He b. I2c. O2d. H 
The strongest interaction between C3H8 and CH3OH isa. dispersion forces b. dipole-dipole forcesc. dipole-induced dipole forcesd. hydrogen bonds 
Select the single best answer. What is the strongest type of intermolecular force between solute and solvent in Cu(s) in Ag(s)? (a) dipole-dipole (b) metallic bonding (c) hydrogen bonding (d) dipole-induced dipole
Select the molecule with the strongest dispersion force with itself.a. N2b. O2c. Br2d. F2 
For each pair below, which of the two has the higher boiling point and state your reason why? (a) helium or argon? (b) ethanol or acetone?(c) pentane or heptane?
Which molecule or molecules can form hydrogen bonds with water? Select all that apply.a) C2H6b) CH3(CH2)4COOHc) CH3CH2OHd) CH3CH2CHO
What intermolecular force(s) is/are present in solid SO 3 ?1. London dispersion2. dipole-dipole3. hydrogen bondinga. 1 onlyb. 2 onlyc. 3 onlyd. 1 and 2e. 1 and 3 
The DNA double helix (Figure25.40) at the atomic level looks like a twisted ladder, where the "rungs" of the ladder consist of molecules that are hydrogen-bonded together. Sugar and phosphate groups make up the sides of the ladder. Shown are the structures of the adenine-thymine (AT) "base pair" and the guanine-cytosine (GC) base pair.You can see that AT base pairs are held together by two hydrogen bonds, and the GC base pairs are held together by three hydrogen bonds.Which base pair is more stable to heating?
What is the strongest type of intermolecular force present in CHF 3?a. dispersionb. dipole-dipolec. hydrogen bondingd. ion-dipolee. none of the above
What is the strongest type of intermolecular force between solute and solvent in the following solution?CH3OCH3(g) in H2O(l)a) ion-dipoleb) H bondc) dipole-dipoled) ion-induced dipolee) dipole-induced dipolef) dispersion
What is the strongest interparticle force in each substance?(c) Cl2
Which of the following exhibit only London (dispersion) forces?a) Heb) H2Oc) Cl2d) HCl