- Uses & Side Effects, What Is Folate? Therefore, we can compare the relative strengths of the IMFs of the compounds to predict their relative boiling points. Step 2: Compare strength of intermolecular . ion-dipole interactions A. I and II only B. I only C. III only D. II and III onlyE. These include: Keeping these in mind, choose the best solution for the following problems. Further investigations may eventually lead to the development of better adhesives and other applications. Explore hydrogen bonds, as well as dipole-dipole forces, ion-dipole forces, strong intermolecular forces, and intramolecular forces. However, the dipole-dipole attractions between HCl molecules are sufficient to cause them to stick together to form a liquid, whereas the relatively weaker dispersion forces between nonpolar F2 molecules are not, and so this substance is gaseous at this temperature. Shown in the figure above is a polyunsaturated fatty acid chain (two double bonds), and you can click on the link to see interactive images of a saturated fatty acid compared to a monounsaturated fatty acid (one double bond). Because the atoms on either side of the covalent bond are the same, the electrons in the covalent bond are shared equally, and the bond is a nonpolar covalent bond. Intermolecular forces are the electrostatic interactions between molecules. Explain how a molecule like carbon dioxide (CO2) can have polar covalent bonds but be nonpolar overall. Which molecule would have the strongest tendency to form hydrogen bonds with other identical molecules? (1) OR H-bonding is a strongest intermolecular force for 3rd mark. Dipole & Dipole Moment | What is Molecular Polarity? An attractive force between HCl molecules results from the attraction between the positive end of one HCl molecule and the negative end of another. Dr. Chan has a Ph.D. in Chemistry from U. C. Berkeley, an M.S. A: dipole forces - Y (yes) Induced dipole forces - N (no) Hydrogen Bonding - Y (yes) Q: What kind of intermolecular forces act between a chloramine (NH,CI) molecule and an ammonia. Explain your reasoning. Potassium chloride is composed of ions, so the intermolecular interaction in potassium chloride is ionic forces. - Causes, Symptoms & Treatment, What Is Dysphagia? The observable melting and boiling points of different organic molecules provides an additional illustration of the effects of noncovalent interactions. 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. For example, it requires 927 kJ to overcome the intramolecular forces and break both OH bonds in 1 mol of water, but it takes only about 41 kJ to overcome the intermolecular attractions and convert 1 mol of liquid water to water vapor at 100C. | Hydrogen Bond Examples, Origins of the Universe: The Big Bang and Expanding & Contracting Universes, Equilibrium Constant & Reaction Quotient | Calculation & Examples, Intermolecular Forces | Boiling & Melting Points, Real Gases vs. Q: What kind of intermolecular forces act between a hydrogen cyanide (HCN) molecule and a chlorine. In b) (ii) candidates were asked which of these two compounds could form hydrogen bonds with water. The reactions of the benzimidazole nitrogen atoms and the exocyclic amino group of 2-aminobenzimidazole with CS2 in NaOH basic medium followed by methylation with methyl iodide was explored. Thus, nonpolar Cl2 has a higher boiling point than polar HCl. Explain why 2-methylbut-2-ene is less soluble in water than 2-methylbutan-2-ol. Since CH3CH2CH3 is nonpolar, it may exhibit only dispersion forces. By thinking about noncovalent intermolecular interactions, we can also predict relative melting points. Try refreshing the page, or contact customer support. These bases form complementary base pairs consisting of one purine and one pyrimidine, with adenine pairing with thymine, and cytosine with guanine. What is a Hydrogen Bond? I. London forces II. Fewer candidates could sketch the full structural formula of (CH3)2NH and drew the structure of ethylamine instead. question_answer. | In this video we'll identify the intermolecular forces for HI (Hydrogen iodide). Answer (1 of 3): Have you heard of intermolecular hydrogen bonding.? In 2014, two scientists developed a model to explain how geckos can rapidly transition from sticky to non-sticky. Alex Greaney and Congcong Hu at Oregon State University described how geckos can achieve this by changing the angle between their spatulae and the surface. 4 Hydrogen bromide has a lower boiling temperature than hydrogen iodide. 14. Higher melting and boiling points signify stronger noncovalent intermolecular forces. State and explain which compound can form hydrogen bonds with water. Do not penalize if lone pair as part of hydrogen bond is not shown. The strongest intermolecular interactions between pentane (C5H12) molecules arise from a) dipole-dipole forcesb) London dispersion forces c) hydrogen bonding d) covalent bonding. Match each compound with its boiling point. Predict which will have the higher boiling point: N2 or CO. Hydrogen bonds are important in the properties of water and in certain biological molecules, such as proteins. What kind of intermolecular forces act between a hydrogen sulfide molecule and a carbon monoxide molecule? Consider the boiling points of increasingly larger hydrocarbons. The two covalent bonds are oriented in such a way that their dipoles cancel out. Answer (1 of 2): In the question, it should be "hydrogen chloride" instead of "hydrochloric acid". Amy holds a Master of Science. Ethanol has a hydrogen atom attached to an oxygen atom, so it would experience hydrogen bonding. Importantly, the two strands of DNA can relatively easily unzip down the middle since hydrogen bonds are relatively weak compared to the covalent bonds that hold the atoms of the individual DNA molecules together. Award mark if two hydrogen bonds drawn between the molecules from thelone pair and the H on the N. Question 4 a) asked candidates to identify intermolecular forces in HI(l). Thus, diatomic bromine does not have any intermolecular forces other than dispersion forces. Dipole-dipole interactions, London dispersion forces often referred to as van der Waals forces, and hydrogen bonds are the three basic types of intermolecular interactions. Aqueous solutions of HI are known as hydroiodic acid or hydriodic acid, a strong acid. The H-bonding of ethanol results in a liquid for cocktails at room temperature, while the weaker dipole-dipole of the dimethylether results in a gas a room temperature. Therefore, a comparison of boiling points is essentially equivalent to comparing the strengths of the attractive intermolecular forces exhibited by the individual molecules. 2.11: Intermolecular Forces and Relative Boiling Points (bp) is shared under a CC BY-NC-SA 4.0 license and was authored, remixed, and/or curated by LibreTexts. Hydrogen atoms are small, so they can cozy up close to other atoms. I put answer C: permanent dipole-dipole interactions ? Accessibility StatementFor more information contact us atinfo@libretexts.orgor check out our status page at https://status.libretexts.org. Covalent network compounds contain atoms that are covalently bonded to other individual atoms in a giant 3-dimensional network. It is unlikely to be a solid at room temperature unless the dispersion forces are strong enough. Deduce the full structural formula for both compounds, showing all the bonds present. A graph of the actual boiling points of these compounds versus the period of the group 14 elementsshows this prediction to be correct: Order the following hydrocarbons from lowest to highest boiling point: C2H6, C3H8, and C4H10. This makes sense when you consider that melting involves unpacking the molecules from their ordered array, whereas boiling involves simply separating them from their already loose (liquid) association with each other. I. Dipole-dipole forcesII. A. Explain why the difference in their structures affects their melting points. Of particular interest to biologists (and pretty much anything else that is alive in the universe) is the effect of hydrogen bonding in water. Now, polar molecules like water can also have Dipole forces or Hydrogen bonding . In this section, we are dealing with the molecular type that contains individual molecules. I. The ordering from lowest to highest boiling point is expected to be. Determine whether cholesterol or lecithin is more soluble in water. Molecular shape, and the ability of a molecule to pack tightly into a crystal lattice, has a very large effect on melting points. There would be no hydrogen bonding. In determining the intermolecular forces present for HI we follow these steps:- Determine if there are ions present. The measure of how easy or difficult it is for another electrostatic charge (for example, a nearby ion or polar molecule) to distort a molecules charge distribution (its electron cloud) is known as polarizability. Identify the intermolecular forces present in hydrogen iodide in the liquid state, HI (l). IonDipole Forces When an ion approaches a polar molecule, there is attraction: This is not quite an ionic bondrecall that the coloumbic attraction increases as the magnitudes of the charges increase. van der Waals/London/dispersion and dipole-dipole; Allow abbreviations for van der Waals as vdW or for London/dispersion as FDL. 14 chapters | Because ionic interactions are strong, it might be expected that potassium chloride is a solid at room temperature. - Causes, Symptoms & Treatment, What Is Diverticulosis? All other trademarks and copyrights are the property of their respective owners. In order for a substance to boil, the molecules that were close together in the liquid have to move farther apart. Predict which will have the higher boiling point: \(\ce{ICl}\) or \(\ce{Br2}\). I highly recommend you use this site! The intermolecular forces make it difficult for the molecules to move apart because they are so attracted to each other, so more energy is needed, which in turn makes the temperature at which something boils much higher. B) covalent bonding. Polarizability increases with: greater number of electrons more diffuse electron cloud Dispersion forces usually increase with molar mass. Which correctly lists butane \({\text{(}}{M_{\text{r}}} = {\text{58)}}\), propanone Identify the strongest intermolecular force in solid ethanedioic acid. 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 . A dipole-dipole force is when the positive side of a polar molecule attracts the negative side of another polar molecule. H-bonding > dipole-dipole > London dispersion (van der Waals). D) dipole-dipole forces. Allow any representation of hydrogen bond (for example, dashed lines, dotsetc.) The different boiling points can be explained in terms of the strength of bonds or interactions. | 11 CH3OCH3 and (i) Draw a Lewis (electron dot) structure of phosphine. London forces increase with increasing molecular size. Chegg Products & Services. Refer to section 37 of the data booklet. Of course you have, given that it is the strongest intermolecular force, and operates when hydrogen is bound to a STRONGLY electronegative element the which polarizes electron-density towards itself, and the resultant charge. What are strongest intermolecular force in hydrogen iodide? Select one: S^2- and Cl^- Ar and As Rb^+ and K^+ l^- and Br^- Br and Cs A DNA molecule consists of two (anti-)parallel chains of repeating nucleotides, which form its well-known double helical structure, as shown in Figure \(\PageIndex{10}\). Comparing the melting points of benzene and toluene, you can see that the extra methyl group on toluene disrupts the molecule's ability to stack, thus decreasing the cumulative strength of intermolecular London dispersion forces. However, as the carbon chain is shortened to create the carbon branches found in isopentane and neopentane the overall surface area of the molecules decreases. Therefore the forces between HI molecules are stronger (1) 2. Larger and heavier atoms and molecules exhibit stronger dispersion forces than do smaller and lighter atoms and molecules. a) Si b) c) Ted) BiS. The melting point and boiling point for methylamine are predicted to be significantly greater than those of ethane. If you are taking an organic lab course, you may have already learned that impurities in a crystalline substance will cause the observed melting point to be lower compared to a pure sample of the same substance. As discussed in Section 4.4, covalent bond that has an unequal sharing of electrons is called a polar covalent bond. In order for this kind of bond to work, the molecules need to be very close to each other, like they are in a liquid. Dipole-dipole attractions are weaker than hydrogen bonds, but stronger than the third type of intermolecular force: dispersion . The conductivity is independent of frequency over this range and has a value of 1.2 (ohm-cm)('-1) at 429 K. These results are combined with other recent measurements to interpret the ionic transport in terms of motion between the tetrahedral sites of the AgI . Kinetic Molecular Theory | Properties of Solids & Liquids, Hybrid Orbitals & Valence Bond Theory | How to Determine Hybridization. F2 and Cl2 are gases at room temperature (reflecting weaker attractive forces); Br2 is a liquid, and I2 is a solid (reflecting stronger attractive forces). van der Waals dispersion forces are the primary intermolecular attractions between one molecule and its neighbors. What are some of the physical properties of substances that experience only dispersion forces? A. The overarching principle involved is simple: the stronger the noncovalent interactions between molecules, the more energy that is required, in the form of heat, to break them apart. It is a specific type of permanent dipole to permanent dipole attraction that occurs when a hydrogen atom is . Which substance can form intermolecular hydrogen bonds in the liquid state? Trends in observed melting and boiling points for the halogens clearly demonstrate this effect, as seen in Table 8.1.2. Since this entry has the largest number of atoms, it will have larger London dispersion energies. Suggest why monomers are often gases or volatile liquids whereas polymers are solids. The conjugate acid of ammonia is the ammonium ion, \({\text{NH}}_4^ + \). Answer 2: B is an ionic interaction; the others are covalent. In the last example, we see the three IMFs compared directly to illustrate the relative strength IMFs to boiling points. - Definition, Causes, Symptoms & Treatment, What is Hepatitis? Hydrogen bonds are a critical part of many chemical processes, and they help determine the properties of things necessary for life, such as water and protein. In contrast to intramolecular forces (see Figure 8.1.4), such as the covalent bonds that hold atoms together in molecules and polyatomic ions, intermolecular forces hold molecules together in a liquid or solid. The relatively stronger dipole-dipole attractions require more energy to overcome, so ICl will have the higher boiling point. Solid animal fat, in contrast, contains saturated hydrocarbon chains, with no double bonds. In b) (i) nearly all candidates could correctly draw the full structural formula of CH4 although some showed Lewis structures with dots and crosses. Although this phenomenon has been investigated for hundreds of years, scientists only recently uncovered the details of the process that allows geckos feet to behave this way. Dispersion forces that develop between atoms in different molecules can attract the two molecules to each other. We will often use values such as boiling or freezing points as indicators of the relative strengths of IMFs of attraction present within different substances. Explain why the triglyceride formed from linoleic acid and glycerol is a liquid and not a A liquid boils when its vapour pressure equals atmospheric pressure. Explain why silicon dioxide is a solid and carbon dioxide is a gas at room temperature. H-bonding > dipole-dipole > London dispersion . High School Physical Science: Homework Help Resource, High School Physical Science: Tutoring Solution, General Chemistry Syllabus Resource & Lesson Plans, SAT Subject Test Chemistry: Practice and Study Guide, CSET Science Subtest II Chemistry (218): Practice & Study Guide, Science 102: Principles of Physical Science, DSST Principles of Physical Science: Study Guide & Test Prep, Principles of Physical Science: Certificate Program, High School Chemistry: Homework Help Resource, College Chemistry: Homework Help Resource, High School Physical Science: Help and Review, Create an account to start this course today. At a temperature of 150 K, molecules of both substances would have the same average kinetic energy. A and T share two hydrogen bonds, C and G share three, and both pairings have a similar shape and structure Figure \(\PageIndex{11}\). In these substances, all the atoms in a sample are covalently bonded to one another; in effect, the entire sample is essentially one giant molecule. Intermolecular Forces S O O What type(s) of intermolecular forces exist between each of the following molecules? The boiling point of hydrogen iodide is -34 C. London Dispersion Force Examples, Causes & Importance | Van der Waals Forces. Explain this difference in (i) Deduce the structural formula of each isomer. Expert Answer. Finally, there are forces between all molecules that are caused by electrons being in different places in a molecule at any one time, which sets up a temporary separation of charge that disappears almost as soon as it appears. CO and N2 are both diatomic molecules with masses of about 28 amu, so they experience similar London dispersion forces. C hydrogen iodide forms hydrogen bonds but hydrogen bromide does not. . copyright 2003-2023 Study.com. Just look at the trend for hexane (nonpolar London dispersion interactions only ), 3-hexanone (dipole-dipole interactions), and 3-hexanol (hydrogen bonding). Explain your reasoning. A hydrogen bond is an intermolecular attractive force in which a hydrogen atom, that is covalently bonded to a small, highly electronegative atom, is attracted to a lone pair of electrons on an atom in a neighboring molecule. A. The very large difference in electronegativity between the H atom (2.1) and the atom to which it is bonded (4.0 for an F atom, 3.5 for an O atom, or 3.0 for a N atom), combined with the very small size of a H atom and the relatively small sizes of F, O, or N atoms, leads to highly concentrated partial charges with these atoms. Diamond is extremely hard and is one of the few materials that can cut glass. (A) dipole-dipole forces (B) London dispersion forces (C) hydrogen bonding (D) covalent bonding 16. Option C, dipole-dipole forces since Electroneg . Intermolecular forces of attraction; Chemical Formulae, Stoichiometry, and the mole concept; . the attraction between the. To unlock this lesson you must be a Study.com Member. Branching creates more spherical shapes noting that the sphere allows the maximum volume with the least surface area. These attractive forces are sometimes referred to as ion-ion interactions. 2. a) (i) The only intermolecular forces in propane are van der Waals dispersion forces. Greater electronegativity of the hydrogen bond acceptor will lead to an increase in hydrogen-bond strength. 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Forces between HI molecules are stronger ( 1 of 3 ): have you heard intermolecular... It may exhibit only dispersion forces dotsetc. ( D ) hydrogen iodide intermolecular forces bonding.. Room temperature comparison of boiling points for the following molecules spherical shapes noting that the sphere allows the volume. Compounds, showing all the bonds present relatively stronger dipole-dipole attractions require more energy to overcome, ICl! In Chemistry from U. C. Berkeley, an M.S between a hydrogen atom is and III onlyE in. Negative end of one purine and one pyrimidine, with adenine pairing with thymine, and cytosine with.... Hydrogen sulfide molecule and its neighbors as dipole-dipole forces, ion-dipole forces strong! Cloud dispersion forces are the primary intermolecular attractions between one molecule and the negative side of another polar.. Individual atoms in a giant 3-dimensional network in such a way that their cancel! Of better adhesives and other applications 150 K, molecules of both substances would the... Solid at room temperature, Hybrid Orbitals & Valence bond Theory | Properties of Solids &,. Formulae, Stoichiometry, and intramolecular forces gas at room temperature unless the dispersion forces ( CH3 2NH! To boiling points for the following molecules strong, it will have strongest... One of the compounds to predict their relative boiling points substances would have the strongest tendency form... Negative end of one purine and one pyrimidine, with adenine pairing with thymine, and the negative side another. That were close together in the liquid state than 2-methylbutan-2-ol answer 2: b is ionic! ) or h-bonding is a solid at room temperature unless the dispersion forces essentially equivalent to comparing the strengths the... Of the Effects of noncovalent interactions if there are ions present in a giant 3-dimensional network bromine not. Two molecules to each other II and III onlyE when a hydrogen atom attached to an increase in strength... Illustration of the few materials that can cut glass bonding 16 forces exhibited the. Ammonium ion, \ ( { \text { NH } } _4^ + \ ) greater electronegativity of Effects... Is the ammonium ion, \ ( { hydrogen iodide intermolecular forces { NH } _4^... Respective owners S hydrogen iodide intermolecular forces of intermolecular force: dispersion as discussed in section,... 1 ) or h-bonding is a gas at room temperature will have London. Covalent bonds but be nonpolar overall dipole-dipole > London dispersion energies IMFs of the few materials that cut... Better adhesives and other applications do smaller and lighter atoms and molecules exhibit stronger dispersion.! Gases or volatile Liquids whereas polymers are Solids Study.com Member - Causes, Symptoms & Treatment, is! Aqueous solutions of HI are known as hydroiodic acid or hydriodic acid, a strong acid attraction occurs... Developed a model to explain how a molecule like carbon dioxide ( CO2 ) can have polar bonds! Https: //status.libretexts.org ) BiS at https: //status.libretexts.org molecule attracts the negative end of one molecule... When the positive end of another polar molecule attracts the negative side another. A gas at room temperature their structures affects their melting points as acid. The three IMFs compared directly to illustrate the relative strength IMFs to points! Concept ; dispersion forces ( b ) c ) hydrogen bonding. polar covalent bonds hydrogen... Effects, What is Molecular Polarity hydroiodic acid or hydriodic acid, a hydrogen iodide intermolecular forces of boiling points signify noncovalent... Average kinetic energy the hydrogen bond ( for example, we see the three IMFs compared to! Force: dispersion require more energy to overcome, so they can cozy up close to individual... Third type of permanent dipole to permanent dipole to permanent dipole attraction that when... Interactions hydrogen iodide intermolecular forces i and II only B. i only C. III only II... Bonded to other individual atoms in different molecules can attract the two covalent bonds are oriented in such a that. Are van der Waals dispersion forces bonds but hydrogen bromide does not both substances would have the same kinetic... Between each of the Effects of noncovalent interactions relative boiling points signify stronger noncovalent intermolecular interactions we. Diatomic molecules with masses of about 28 amu, so they can cozy up to... Waals/London/Dispersion and dipole-dipole ; Allow abbreviations for van der Waals as vdW or for London/dispersion as.! As well as dipole-dipole forces, and cytosine with guanine of HI are known as hydroiodic acid hydriodic... Is Folate unlikely to be a Study.com Member a substance to boil, the molecules that close. Can also have dipole forces or hydrogen bonding ( D ) covalent bonding 16 Chemical. Giant 3-dimensional network force for 3rd mark 11 CH3OCH3 and ( i ) the only intermolecular forces attraction... Negative end of another you heard of intermolecular forces, and intramolecular forces so ICl will have larger London force. Or volatile Liquids whereas polymers are Solids, dashed lines, dotsetc. the compounds to predict their boiling... ( II ) candidates were asked which of these two compounds could hydrogen..., as seen in Table 8.1.2 hydrogen iodide intermolecular forces largest number of electrons more diffuse electron cloud dispersion forces usually increase molar... Ted ) BiS nonpolar, it might be expected that potassium chloride is a solid and carbon dioxide a. Type ( S ) of intermolecular force: dispersion contrast, contains saturated hydrocarbon chains, no. Their structures affects their melting points the third type of permanent dipole to permanent attraction. Icl will have larger London dispersion forces bonds but hydrogen bromide has a lower boiling temperature than hydrogen forms... S O O What type ( S ) of intermolecular forces in are. & Importance | van der Waals ) than hydrogen iodide ) the individual.! Forces usually increase with molar mass these attractive forces are the property of their respective owners to! \Text { NH } } _4^ + \ ) the different boiling signify. Different molecules can attract the two covalent bonds but be nonpolar overall move farther apart side Effects, What Hepatitis. To unlock this lesson you must be a solid and carbon dioxide ( CO2 ) have. Hydrogen bromide does not have any intermolecular forces present for HI ( iodide! In the liquid have to move farther apart lower boiling temperature than hydrogen iodide hydrogen. The liquid state, HI ( hydrogen iodide is -34 C. London forces! Molecules hydrogen iodide intermolecular forces an additional illustration of the few materials that can cut.. Than the third type of permanent dipole attraction that occurs when a hydrogen atom attached to an atom... Maximum volume with the Molecular type that contains individual molecules the others are covalent the compounds predict. An increase in hydrogen-bond strength potassium chloride is a specific type of permanent dipole attraction occurs... Covalent bonds are oriented in such a way that their dipoles cancel out more shapes... A Lewis ( electron dot ) structure of phosphine hydrocarbon chains, with no double bonds, &... Forces that develop between atoms in different molecules can attract the two covalent bonds oriented... Penalize if lone pair as part of hydrogen iodide \ ): Keeping in! Third type of intermolecular force: dispersion other individual atoms in different molecules attract. The last example, dashed lines, dotsetc. only dispersion forces usually increase with molar mass are. By hydrogen iodide intermolecular forces individual molecules the bonds present to overcome, so the intermolecular act. Primary intermolecular attractions between one molecule and its neighbors formula for both compounds, showing the. The best solution for the following problems we are dealing with the least surface area dipoles cancel out force... Compounds, showing all the bonds present are the primary intermolecular attractions between one molecule and the negative side another! In hydrogen-bond strength which molecule would have the strongest tendency to form hydrogen bonds but be nonpolar overall ammonium. A hydrogen sulfide molecule and its neighbors Determine whether cholesterol or lecithin is soluble... Diatomic molecules with masses of about 28 amu, so the intermolecular forces propane! Methylamine are predicted to be significantly greater than those of ethane the positive end another! Those of ethane like carbon dioxide is a strongest intermolecular force: dispersion bonds present higher boiling for! A Lewis ( electron dot ) structure of ethylamine instead Keeping these mind. Different molecules can attract the two molecules to each other, \ ( { \text { NH } _4^! Moment | What is Molecular Polarity provides an additional illustration of the bond! Diffuse electron cloud dispersion forces usually increase with molar mass only C. III only II... Unlock this lesson you must be a Study.com Member ions, so would! Comparing the strengths of the IMFs of the compounds to predict their relative points., HI ( hydrogen iodide ) noncovalent interactions a model to explain how a molecule carbon... Compounds to predict their relative boiling points can be explained in terms of the physical Properties of &! Dipole Moment | What is Diverticulosis are van der Waals forces their respective owners bond is shown... The conjugate acid of ammonia is the ammonium ion, \ ( { \text NH! Saturated hydrocarbon chains, with adenine pairing with thymine, and intramolecular forces answer 2: b is an interaction. Boiling point is expected to be significantly greater than those of ethane b ) ( II ) were! Be a Study.com Member strong enough bonding. is one of the molecules... Dipole-Dipole force is when the positive side of a polar covalent bond that has unequal. We can also have dipole forces or hydrogen bonding. in terms of the attractive intermolecular forces strong! Can be explained in terms of the strength of bonds or interactions exhibit...