Intermolecular forces 4.8 (11 reviews) Term 1 / 24 O2 (oxygen) Click the card to flip Definition 1 / 24 Dispersion Click the card to flip Flashcards Learn Test Match Created by Joel_Varner6 Terms in this set (24) O2 (oxygen) Dispersion CH2O (Formaldehyde) dispersion, dipole Water Dispersion, dipole, hydrogen-bonding CH3Cl (chloromethane) An alcohol is an organic molecule containing an -OH group. 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. Both molecules have about the same shape and ONF is the heavier and larger molecule. This book uses the Because molecules in a liquid move freely and continuously, molecules always experience both attractive and repulsive dipoledipole interactions simultaneously, as shown in Figure \(\PageIndex{2}\). Consider a polar molecule such as hydrogen chloride, HCl. We also acknowledge previous National Science Foundation support under grant numbers 1246120, 1525057, and 1413739. It is a type of chemical bond that generates two oppositely charged ions. When gaseous water is cooled sufficiently, the attractions between H2O molecules will be capable of holding them together when they come into contact with each other; the gas condenses, forming liquid H2O. Compare ionic bonding with covalent bonding.Ionic is metal/nonmetal; covalent is 2 nonmetals 5. The hydrogen bonding is limited by the fact that there is only one hydrogen in each ethanol molecule with sufficient + charge. This effect, illustrated for two H2 molecules in part (b) in Figure \(\PageIndex{3}\), tends to become more pronounced as atomic and molecular masses increase (Table \(\PageIndex{2}\)). An intermolecular force is an attractive force that arises between the positive components (or protons) of one molecule and the negative components (or electrons) of another molecule. Both HCl and F2 consist of the same number of atoms and have approximately the same molecular mass. c) Phosphorus trichloride reacts with hydrogen gas to form phosphorus trihydride and hydrogen chloride. The nitrogen dioxide is a covalent compound where one nitrogen is the central atom which is bonded to two oxygen atoms, where one oxygen atom is bonded by a single bond and other oxygen atom by a double bond. Hydrogen bond formation requires both a hydrogen bond donor and a hydrogen bond acceptor. . This problem has been solved! The answer lies in the highly polar nature of the bonds between hydrogen and very electronegative elements such as O, N, and F. The large difference in electronegativity results in a large partial positive charge on hydrogen and a correspondingly large partial negative charge on the O, N, or F atom. If there are no dipoles, what would make the nitrogen atoms stick together to form a liquid? The polarizability of a substance also determines how it interacts with ions and species that possess permanent dipoles. This question was answered by Fritz London (19001954), a German physicist who later worked in the United States. These result in much higher boiling points than are observed for substances in which London dispersion forces dominate, as illustrated for the covalent hydrides of elements of groups 1417 in Figure \(\PageIndex{5}\). Boiling Points For general purposes it is useful to consider temperature to be a measure of the kinetic energy of all the atoms and molecules in a given system. 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. The investigation of PT reaction in group of compounds known as bipirydine-diols lead to the description of the mechanism of double intra-molecular PT reaction in compounds with hydrogen bond in OHN bridge. c. Although this molecule does not experience hydrogen bonding, the Lewis electron dot diagram and VSEPR indicate that it is bent, so it has a permanent dipole. Since the hydrogen donor is strongly electronegative, it pulls the covalently bonded electron pair closer to its nucleus, and away from the hydrogen atom. If we use this trend to predict the boiling points for the lightest hydride for each group, we would expect NH3 to boil at about 120 C, H2O to boil at about 80 C, and HF to boil at about 110 C. Using a flowchart to guide us, we find that N2 only . The overall order is thus as follows, with actual boiling points in parentheses: propane (42.1C) < 2-methylpropane (11.7C) < n-butane (0.5C) < n-pentane (36.1C). In this section, we explicitly consider three kinds of intermolecular interactions: There are two additional types of electrostatic interaction that you are already familiar with: the ionion interactions that are responsible for ionic bonding and the iondipole interactions that occur when ionic substances dissolve in a polar substance such as water. This can account for the relatively low ability of Cl to form hydrogen bonds. They were both injured in another NCl3 explosion shortly thereafter. It has a peculiar odor and belongs to the organic halogen compound family. In contrast, each oxygen atom is bonded to two H atoms at the shorter distance and two at the longer distance, corresponding to two OH covalent bonds and two OH hydrogen bonds from adjacent water molecules, respectively. These attractive interactions are weak and fall off rapidly with increasing distance. This greatly increases its IMFs, and therefore its melting and boiling points. The same effect that is seen on boiling point as a result of hydrogen bonding can also be observed in the viscosity of certain substances. There are a total of 7 lone pairs in the Lewis structure of HNO3. These interactions become important for gases only at very high pressures, where they are responsible for the observed deviations from the ideal gas law at high pressures. Hydrogen bonds are much weaker than covalent bonds, only about 5 to 10% as strong, but are generally much stronger than other dipole-dipole attractions and dispersion forces. Thus we predict the following order of boiling points: 2-methylpropane < ethyl methyl ether < acetone. Recall from the chapter on chemical bonding and molecular geometry that polar molecules have a partial positive charge on one side and a partial negative charge on the other side of the moleculea separation of charge called a dipole. A DNA molecule consists of two (anti-)parallel chains of repeating nucleotides, which form its well-known double helical structure, as shown in Figure 10.13. A graph of the actual boiling points of these compounds versus the period of the group 14 element shows this prediction to be correct: C2H6 < C3H8 < C4H10. For example, liquid water forms on the outside of a cold glass as the water vapor in the air is cooled by the cold glass, as seen in Figure 10.3. This force is often referred to as simply the dispersion force. Because the electrons of an atom or molecule are in constant motion (or, alternatively, the electrons location is subject to quantum-mechanical variability), at any moment in time, an atom or molecule can develop a temporary, instantaneous dipole if its electrons are distributed asymmetrically. Nitrogen trichloride, also known as trichloramine, is the chemical compound with the formula NCl3. Even the noble gases can be liquefied or solidified at low temperatures, high pressures, or both (Table \(\PageIndex{2}\)). Although dispersion forces are very weak, the total attraction over millions of spatulae is large enough to support many times the geckos weight. N2 intermolecular forces - N2 has a linear molecular structure and is a nonpolar molecule. A molecule that has a charge cloud that is easily distorted is said to be very polarizable and will have large dispersion forces; one with a charge cloud that is difficult to distort is not very polarizable and will have small dispersion forces. The van, attractions (both dispersion forces and dipole-dipole attractions) in each will be much the same. Larger and heavier atoms and molecules exhibit stronger dispersion forces than do smaller and lighter atoms and molecules. Thus far we have considered only interactions between polar molecules, but other factors must be considered to explain why many nonpolar molecules, such as bromine, benzene, and hexane, are liquids at room temperature, and others, such as iodine and naphthalene, are solids. This reaction is inhibited for dilute gases. Additionally, we cannot attribute this difference in boiling points to differences in the dipole moments of the molecules. Intramolecular hydrogen bonds are those which occur within one single molecule. These two rapidly fluctuating, temporary dipoles thus result in a relatively weak electrostatic attraction between the speciesa so-called dispersion force like that illustrated in Figure 10.6. what are the intermolecular forces present in nitrogen trichloride This problem has been solved! Within a vessel, water molecules hydrogen bond not only to each other, but also to the cellulose chain which comprises the wall of plant cells. This review collects some of the most recent advancements in photocatalytic R generation a These forces are generally stronger with increasing molecular mass, so propane should have the lowest boiling point and n-pentane should have the highest, with the two butane isomers falling in between. Although CH bonds are polar, they are only minimally polar. For the group 15, 16, and 17 hydrides, the boiling points for each class of compounds increase with increasing molecular mass for elements in periods 3, 4, and 5. Intermolecular forces determine bulk properties such as the melting points of solids and the boiling points of liquids. Those substances which are capable of forming hydrogen bonds tend to have a higher viscosity than those that do not. An attractive force between HCl molecules results from the attraction between the positive end of one HCl molecule and the negative end of another. Now, polar molecules like water can also have Dipole forces or Hydrogen bonding . Interactions between these temporary dipoles cause atoms to be attracted to one another. Because the electrons are in constant motion, however, their distribution in one atom is likely to be asymmetrical at any given instant, resulting in an instantaneous dipole moment. The hydrogen atom is then left with a partial positive charge, creating a dipole-dipole attraction between the hydrogen atom bonded to the donor, and the lone electron pair on the, hydrogen bonding occurs in ethylene glycol (C, The same effect that is seen on boiling point as a result of hydrogen bonding can also be observed in the, Hydrogen bonding plays a crucial role in many biological processes and can account for many natural phenomena such as the, The cohesion-adhesion theory of transport in vascular plants uses hydrogen bonding to explain many key components of water movement through the plant's xylem and other vessels. Indeed, there are enough electrons in the I2 molecule to make the temporary dipoles, which create dispersion forces. (there is also some dispersion force associated with. The structure of liquid water is very similar, but in the liquid, the hydrogen bonds are continually broken and formed because of rapid molecular motion. A and T share two hydrogen bonds, C and G share three, and both pairings have a similar shape and structure Figure 10.14. Types of intramolecular forces of attraction Ionic bond: This bond is formed by the complete transfer of valence electron (s) between atoms. Phosphorus trichloride molecule is made up of 3 chlorine and 1 phosphorus atom. Boron trifluoride (BF3) Dispersion forces. In methoxymethane, lone pairs on the oxygen are still there, but the hydrogens are not sufficiently + for hydrogen bonds to form. Question: What kind of intermolecular forces act between a nitrogen trichloride molecule and a chloroform (CHCI) 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. Chang, Raymond. The N-Cl distances are 1.76, and the Cl-N-Cl angles are 107.[2]. The hydrogen bonding is limited by the fact that there is only one hydrogen in each ethanol molecule with sufficient, lone pairs on the oxygen are still there, but the. The strength of the dispersion forces increases with the contact area between molecules, as demonstrated by the boiling points of these pentane isomers. The first two are often described collectively as van der Waals forces. In the following description, the term particle will be used to refer to an atom, molecule, or ion. Such molecules will always have higher boiling points than similarly sized molecules which don't have an -O-H or an -N-H group. They are certainly strong enough to hold the iodine together as a solid. [5][6] The pure substance (rarely encountered) is a dangerous explosive, being sensitive to light, heat, even moderate shock, and organic compounds. this type of forces are called intermolecular forces. This process is called hydration. Hydrogen bonding can occur between ethanol molecules, although not as effectively as in water. Furthermore, \(H_2O\) has a smaller molar mass than HF but partakes in more hydrogen bonds per molecule, so its boiling point is consequently higher. (credit: modification of work by Sam-Cat/Flickr). The presence of this dipole can, in turn, distort the electrons of a neighboring atom or molecule, producing an induced dipole. Carbon Monoxide (CO) london forces. The shapes of molecules also affect the magnitudes of the dispersion forces between them. Because a hydrogen atom is so small, these dipoles can also approach one another more closely than most other dipoles. It is a very explosive substance. The predicted order is thus as follows, with actual boiling points in parentheses: He (269C) < Ar (185.7C) < N2O (88.5C) < C60 (>280C) < NaCl (1465C). Recall that the attractive energy between two ions is proportional to 1/r, where r is the distance between the ions. Identify the compounds with a hydrogen atom attached to O, N, or F. These are likely to be able to act as hydrogen bond donors. NCl3 explodes to give N2 and chlorine gas. This simulation is useful for visualizing concepts introduced throughout this chapter. The ordering from lowest to highest boiling point is therefore C2H6 < C3H8 < C4H10. However, when we measure the boiling points for these compounds, we find that they are dramatically higher than the trends would predict, as shown in Figure 10.12. It has a melting point of 40C and a boiling point of 71C. The forces are relatively weak, however, and become significant only when the molecules are very close. CH3CH3 and CH3NH2 are similar in size and mass, but methylamine possesses an NH group and therefore may exhibit hydrogen bonding. In addition, the attractive interaction between dipoles falls off much more rapidly with increasing distance than do the ionion interactions. Identify the most significant intermolecular force in each substance. Due to London dispersion forces, nitrogen atoms stick together to form a liquid. Alongside monochloramine and dichloramine, trichloramine is responsible for the distinctive 'chlorine smell' associated with swimming pools, where the compound is readily formed as a product from hypochlorous acid reacting with ammonia and other nitrogenous substances in the water, such as urea from urine.[1]. Science Chemistry What kind of intermolecular forces act between a formaldehyde (H,CO) molecule and a nitrogen trichloride molecule? The huge numbers of spatulae on its setae provide a gecko, shown in Figure 10.8, with a large total surface area for sticking to a surface. The relatively stronger dipole-dipole attractions require more energy to overcome, so ICl will have the higher boiling point. As a result, the boiling point of neopentane (9.5C) is more than 25C lower than the boiling point of n-pentane (36.1C). The effect of increasingly stronger dispersion forces dominates that of increasingly weaker dipole-dipole attractions, and the boiling points are observed to increase steadily. Substances which have the possibility for multiple hydrogen bonds exhibit even higher viscosities. The boiling point of the 2-methylpropan-1-ol isn't as high as the butan-1-ol because the branching in the molecule makes the van der Waals attractions less effective than in the longer butan-1-ol. These bases form complementary base pairs consisting of one purine and one pyrimidine, with adenine pairing with thymine, and cytosine with guanine. Hydrogen bonding. b__1]()", "10.02:_VSEPR_Theory_-_The_Five_Basic_Shapes" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+>c . Accessibility StatementFor more information contact us atinfo@libretexts.orgor check out our status page at https://status.libretexts.org. Under appropriate conditions, the attractions between all gas molecules will cause them to form liquids or solids. Metal with nonmetal: electron transfer and ionic bonding. In contrast to intramolecular forces, such as the covalent bonds that hold atoms together in molecules and polyatomic ions, intermolecular forces hold molecules together in a liquid or solid. Instead, each hydrogen atom is 101 pm from one oxygen and 174 pm from the other. The three compounds have essentially the same molar mass (5860 g/mol), so we must look at differences in polarity to predict the strength of the intermolecular dipoledipole interactions and thus the boiling points of the compounds. Consequently, HO, HN, and HF bonds have very large bond dipoles that can interact strongly with one another. Intermediates in this conversion include monochloramine and dichloramine, NH2Cl and NHCl2, respectively. Because the electron distribution is more easily perturbed in large, heavy species than in small, light species, we say that heavier substances tend to be much more polarizable than lighter ones. When we consider the boiling points of molecules, we usually expect molecules with larger molar masses to have higher normal boiling points than molecules with smaller molar masses. The cohesion-adhesion theory of transport in vascular plants uses hydrogen bonding to explain many key components of water movement through the plant's xylem and other vessels. 2: Structure and Properties of Organic Molecules, { "2.01:_Pearls_of_Wisdom" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "2.02:_Molecular_Orbital_(MO)_Theory_(Review)" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "2.03:_Hybridization_and_Molecular_Shapes_(Review)" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "2.04:_2.4_Conjugated_Pi_Bond_Systems" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "2.05:_Lone_Pair_Electrons_and_Bonding_Theories" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "2.06:_Bond_Rotation" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "2.07:_Isomerism_Introduction" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "2.08:_Hydrocarbons" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "2.09:_Organic_Functional_Groups" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "2.10:_Intermolecular_Forces_(IMFs)_-_Review" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "2.11:_Intermolecular_Forces" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "2.12:_Intermolecular_Forces" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "2.13:__Additional_Practice_Problems" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "2.14:_Organic_Functional_Groups:_H-bond_donors" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "2.15:__Additional_Exercises" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "2.16:_2.15_Solutions_to_Additional_Exercises" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()" }, { "00:_Front_Matter" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "01:_Introduction_and_Review" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "02:_Structure_and_Properties_of_Organic_Molecules" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "03:_Functional_Groups_and_Nomenclature" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "04:_Structure_and_Stereochemistry_of_Alkanes" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "05:_An_Introduction_to_Organic_Reactions_using_Free_Radical_Halogenation_of_Alkanes" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "06:_Stereochemistry_at_Tetrahedral_Centers" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "07:_Alkyl_Halides:_Nucleophilic_Substitution_and_Elimination" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "08:_Structure_and_Synthesis_of_Alkenes" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "09:_Reactions_of_Alkenes" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "10:_Alkynes" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "zz:_Back_Matter" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()" }, 2.10: Intermolecular Forces (IMFs) - Review, [ "article:topic", "showtoc:no", "license:ccbyncsa", "transcluded:yes", "licenseversion:40" ], https://chem.libretexts.org/@app/auth/3/login?returnto=https%3A%2F%2Fchem.libretexts.org%2FCourses%2FSacramento_City_College%2FSCC%253A_Chem_420_-_Organic_Chemistry_I%2FText%2F02%253A_Structure_and_Properties_of_Organic_Molecules%2F2.10%253A_Intermolecular_Forces_(IMFs)_-_Review, \( \newcommand{\vecs}[1]{\overset { \scriptstyle \rightharpoonup} {\mathbf{#1}}}\) \( \newcommand{\vecd}[1]{\overset{-\!-\!\rightharpoonup}{\vphantom{a}\smash{#1}}} \)\(\newcommand{\id}{\mathrm{id}}\) \( \newcommand{\Span}{\mathrm{span}}\) \( \newcommand{\kernel}{\mathrm{null}\,}\) \( \newcommand{\range}{\mathrm{range}\,}\) \( \newcommand{\RealPart}{\mathrm{Re}}\) \( \newcommand{\ImaginaryPart}{\mathrm{Im}}\) \( \newcommand{\Argument}{\mathrm{Arg}}\) \( \newcommand{\norm}[1]{\| #1 \|}\) \( \newcommand{\inner}[2]{\langle #1, #2 \rangle}\) \( \newcommand{\Span}{\mathrm{span}}\) \(\newcommand{\id}{\mathrm{id}}\) \( \newcommand{\Span}{\mathrm{span}}\) \( \newcommand{\kernel}{\mathrm{null}\,}\) \( \newcommand{\range}{\mathrm{range}\,}\) \( \newcommand{\RealPart}{\mathrm{Re}}\) \( \newcommand{\ImaginaryPart}{\mathrm{Im}}\) \( \newcommand{\Argument}{\mathrm{Arg}}\) \( \newcommand{\norm}[1]{\| #1 \|}\) \( \newcommand{\inner}[2]{\langle #1, #2 \rangle}\) \( \newcommand{\Span}{\mathrm{span}}\)\(\newcommand{\AA}{\unicode[.8,0]{x212B}}\), More complex examples of hydrogen bonding, When an ionic substance dissolves in water, water molecules cluster around the separated ions. In a larger atom, the valence electrons are, on average, farther from the nuclei than in a smaller atom. For similar substances, London dispersion forces get stronger with increasing molecular size. KBr (1435C) > 2,4-dimethylheptane (132.9C) > CS2 (46.6C) > Cl2 (34.6C) > Ne (246C). Argon and N2O have very similar molar masses (40 and 44 g/mol, respectively), but N2O is polar while Ar is not. These are polar forces, intermolecular forces of attraction between molecules. By changing how the spatulae contact the surface, geckos can turn their stickiness on and off. (credit photo: modification of work by JC*+A!/Flickr). is due to the additional hydrogen bonding. This occurs when two functional groups of a molecule can form hydrogen bonds with each other. As we progress down any of these groups, the polarities of the molecules decrease slightly, whereas the sizes of the molecules increase substantially. Since both N and O are strongly electronegative, the hydrogen atoms bonded to nitrogen in one polypeptide backbone can hydrogen bond to the oxygen atoms in another chain and visa-versa. The melting point and boiling point for methylamine are predicted to be significantly greater than those of ethane. c. Nitrogen trichloride NCl3 d. Boron trisulfideBS3 4. Examples range from simple molecules like CH. ) Creative Commons Attribution License If ice were denser than the liquid, the ice formed at the surface in cold weather would sink as fast as it formed. Here, in HNO2 molecule, nitrogen atom bonded to two oxygen atoms which means A = Nitrogen. The compound NCl3 is an ionic compound (metal and nonmetal), and therefore does not require prefixes- -so NCl3 is nitrogen trichloride. For example, Xe boils at 108.1C, whereas He boils at 269C. Intra molecular forces are those within the molecule that keep the molecule together, for example, the bonds between the atoms. Hydrogen Isotopes. The phase in which a substance exists depends on the relative extents of its intermolecular forces (IMFs) and the kinetic energies (KE) of its molecules. Comparing the two alcohols (containing -OH groups), both boiling points are high because of the additional hydrogen bonding due to the hydrogen attached directly to the oxygen - but they are not the same. The diagram shows the potential hydrogen bonds formed to a chloride ion, Cl-. The two strands of the famous double helix in DNA are held together by hydrogen bonds between hydrogen atoms attached to nitrogen on one strand, and lone pairs on another nitrogen or an oxygen on the other one.
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