nh3 intermolecular forces dipole dipole

in case of NH3, the main type of intermolecular forces is; these type of forces is easy to change polarity of atoms. Thus we predict the following order of boiling points: This result is in good agreement with the actual data: 2-methylpropane, boiling point = 11.7C, and the dipole moment () = 0.13 D; methyl ethyl ether, boiling point = 7.4C and = 1.17 D; acetone, boiling point = 56.1C and = 2.88 D. Arrange carbon tetrafluoride (CF4), ethyl methyl sulfide (CH3SC2H5), dimethyl sulfoxide [(CH3)2S=O], and 2-methylbutane [isopentane, (CH3)2CHCH2CH3] in order of decreasing boiling points. What is the ratio of the 2 different strands to hydrogen double helix in a solution given a temperature of 300 K. First calculate the ratio of the two different strands for just one pair. If ice were denser than the liquid, the ice formed at the surface in cold weather would sink as fast as it formed. Another good indicator is boiling point of SiH4 vs SiCl4 - CHEMISTRY COMMUNITY As a result, the boiling point of neopentane (9.5C) is more than 25C lower than the boiling point of n-pentane (36.1C). Ion ion force ion ion forces, it mean that force of attraction between two ion. It help to understand about molecules. it is only a terms Portland cement not more then that. So if you were to take all of Determine what type of intermolecular forces exist in the following molecules: LiF, MgF2, H2O, and HF. \[V = \dfrac{q_1q_2}{4 \pi \epsilon_o r}\], \[V = \dfrac{- (1.602 \times 10^{-19}\;\cancel{C})(1.602 \times 10^{-19} \cancel{C})}{4 \pi (8.853 \times 10^{-12} \cancel{C^2} \cdot N^{1} \cdot m \cancel{^{2}})(6 \times 10^{-10}\; \cancel{m})} = -3.84 \times 10^{-19} \; J\]. NH3 > PH3 > CH4 Which of the following has intermolecular forces listed from weakest to strongest? They form a net dipole moment. you have a bunch of molecules, let's say, in a liquid state, the boiling point is going to be dependent on how much energy you In contrast, the hydrides of the lightest members of groups 1517 have boiling points that are more than 100C greater than predicted on the basis of their molar masses. So if you have a permanently polar molecule then it can create a constant induced dipole in nearby nonpolar molecules. What is G for this reaction? Consider two pure liquids. Your email address will not be published. PDF Homework #2 Chapter 16 - UC Santa Barbara because chlorine has highly electronegative than hydrogen. As a result, hydrogen bonding and dipole-dipole and london dispersion forces are generate between molecules. 13.E: Intermolecular Forces (Exercises) - Chemistry LibreTexts it genrate hydrogen bonding and dipole dipole intraction. hydrogen bonding is also called intermolecular forces between two molecules. Last edited: May 29, 2012 around the world. Polarity and Intermolecular Forces Gizmo.pdf - Name: Date: You are given the dipole moment of H2O is 1.82 D. The distance between these two is 2 . Dipoledipole forces occur between molecules with permanent dipoles (i.e., polar molecules). Other factors must be considered to explain why many nonpolar molecules, such as bromine, benzene, and hexane, are liquids at room temperature; why others, such as iodine and naphthalene, are solids. Types of IMFAs 1. Remember, molecular dipole (Despite this seemingly low value, the intermolecular forces in liquid water are among the strongest such forces known!) Calculate the ion-dipole interaction between H2O and Li+. Since there is no net dipole, there is NO DIPOLE DIPOLE when examining the intermolecular forces. Because you could imagine, if As a result, the CO bond dipoles partially reinforce one another and generate a significant dipole moment that should give a moderately high boiling point. The four compounds are alkanes and nonpolar, so London dispersion forces are the only important intermolecular forces. and both are attract each other. Some molecules are arranged in ways where atoms with relatively high electronegativity are on one side while atoms with relatively low electronegativity are on the other. What is the intermolecular forces of NH3? - chemwhite.com So, option (b) is incorrect. They follow van der Waals forces and thus behave less ideally. first you draw Lewis structure of CO2. Q: The rate constant for the decomposition of N2O5 at 45 degrees Celcuis is k = 5.1 x 10-4 s1. even temporarily positive end, of one could be attracted Due to all above explanation, we can say that, hydrogen bond are the strongest intermolecular forces. The distance, along the helix, between nucleotides is 3.4 . 14.7: Intermolecular Forces- Dispersion, Dipole-Dipole, Hydrogen Since there are 50 base pairs, we need to multiply by 50 to account for all the base pairs. The Journal also publishes brief communications of significant new findings, perspectives on the latest advances in the field, and Special Topics. Select the intermolecular forces present between NH3 molecules dipole-dipole interactions hydrogen bonding London dispersion forces Arrange the compounds from lowest boiling point to highest boiling point Highest boiling point Lowest boiling point Answer Bank Ne This problem has been solved! In small atoms such as He, the two 1s electrons are held close to the nucleus in a very small volume, and electronelectron repulsions are strong enough to prevent significant asymmetry in their distribution. Let's start with an example. so, you can say that, polar molecules generated hydrogen bonding. It also has the Hydrogen atoms bonded to a Nitrogen atom. Every molecule experiences london dispersion as an intermolecular force. What kind of attractive interaction exists between atoms and between nonpolar molecules? Dispersion Forces Dipole-dipole Hydrogen bonds Dispersion forces are weaker than dipole-dipole and dipole-dipole are weaker than hydrogen bonds. Ion-Ion Interaction 6. How can you tell if the intermolecular force is dipole-dipole just by being given the molecular formula? You will get a little bit of one, but they, for the most part, cancel out. The London dispersion force is a weak intermolecular force caused by electron motion in molecules, which results in the formation of temporary dipoles. Given: The dipole moment of HF is 1.86 D. The dipole moment of HCl is 1.05 D. The distance between the two is 1.78, \[V=-\dfrac{2\mu _{A}\mu _{B}}{4\pi \varepsilon _{0}r^{3}}\], \[V=-\dfrac{2(1.05)(1.86)}{4\pi (8.854187817\cdot 10^{-12})(1.78)^{3}}\]. (d) CH 3 CH 2 OH (ethanol) This has everything that methyl iodide has PLUS hydrogen bonding. this is called ion ion force. Weak. so, large difference of electronegativity between nitrogen and hydrogen. Thus, London dispersion forces are responsible for the general trend toward higher boiling points with increased molecular mass and greater surface area in a homologous series of compounds, such as the alkanes (part (a) in Figure \(\PageIndex{4}\)). hydrogen is bound to nitrogen and it make hydrogen bonds properly. You are correct; since the dipoles cancel out, they each have only London forces. but nitrogen has highly electronegative value. It is very popular in India. In this video well identify the intermolecular forces for NH3 (Ammonia). The bent shape of the . we know that polarized molecules has two poles, partial positive pole and partial negative pole. When we look at propane here on the left, carbon is a little bit more And so this is what It should therefore have a very small (but nonzero) dipole moment and a very low boiling point. this types of intermolecular forces are generated between nh3 molecules. Because each water molecule contains two hydrogen atoms and two lone pairs, a tetrahedral arrangement maximizes the number of hydrogen bonds that can be formed. therefore, the large difference in electronegativity between the N atom and H atom, N-O, N-F atoms leads to highly polar covalent bond. The hydrogen bonds are many magnitudes stronger than other intermolecular forces in NH3; therefore, when examining intermolecular bonding in this molecule, other forces can be safely ignored. London dispersion forces are due to the formation of instantaneous dipole moments in polar or nonpolar molecules as a result of short-lived fluctuations of electron charge distribution, which in turn cause the temporary formation of an induced dipole in adjacent molecules; their energy falls off as 1/r6. what if we put the substance in an electric field, molecules become more polar, will it cause higher intermolecular forces? CS2 has a higher boiling point than CO2 despite having similar intermolecular forces because it has a larger molar . An electrified atom will keep its polarity the exact same. 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. KBr (1435C) > 2,4-dimethylheptane (132.9C) > CS2 (46.6C) > Cl2 (34.6C) > Ne (246C). Direct link to Ryan W's post Dipole-dipole is from per. BUY. In addition, the attractive interaction between dipoles falls off much more rapidly with increasing distance than do the ionion interactions. 13.E: Intermolecular Forces (Exercises) is shared under a CC BY-NC-SA 4.0 license and was authored, remixed, and/or curated by LibreTexts. Because ice is less dense than liquid water, rivers, lakes, and oceans freeze from the top down. And then the positive end, Pause this video, and think about that. So what makes the difference? And when we look at these two molecules, they have near identical molar masses. Molecules in liquids are held to other molecules by intermolecular interactions, which are weaker than the intramolecular interactions that hold the atoms together within molecules and polyatomic ions. 2. They get attracted to each other. Hints. sodium has positive charge and chlorine has negative charge. Polarity and Intermolecular Forces Gizmo Answer Key 2023 Third Quarter Remedial - GenChem 1 | PDF | Intermolecular Force What kind of attractive forces can exist between nonpolar molecules or atoms? Question: What intermolecular forces are present in each of the - Chegg Using a flowchart to guide us, we find that NH3 is a polar molecule. In this case, oxygen is dipole-dipole intraction is occur on polar molecules. Intermolecular forces determine bulk properties, such as the melting points of solids and the boiling points of liquids. exp[100X(15X103 J/mol)/(8.314 J/K*mol)(300K) = 0. For molecules of similar size and mass, the strength of these forces increases with increasing polarity. Hydrogen Bonding, Dipole-Dipole & Ion-Dipole Forces: Strong Types of intramolecular forces of attraction Ionic bond: This bond is formed by the complete transfer of valence electron (s) between atoms. A permanent dipole can induce a temporary dipole, but not the other way around. Therefore NH3 the main intermolecular force is Hydrogen Bonding (note that NH3 also has Dipole-Dipole and London Dispersion Forces). In case of nh3, (N-H bonds makes between molecules) and dipole dipole interaction (interaction between two dipole) and london dispersion forces occur between nh3 molecules. We also acknowledge previous National Science Foundation support under grant numbers 1246120, 1525057, and 1413739. This causes an imbalance of electrons, which makes a permanent dipole as the electrons of the molecule tend to stay closer to the more electronegative atom. CO2 it is similar to SCO molecules. Arrange 2,4-dimethylheptane, Ne, CS2, Cl2, and KBr in order of decreasing boiling points. consider another dipole it has also two poles, partial positive pole and partial negative poles, we has two dipoles. Could someone tell if temporary dipoles induce permanent ones (or only permanent-permanent/temporary-temporary can be induced)? Bodies of water would freeze from the bottom up, which would be lethal for most aquatic creatures. a partial negative charge at that end and a partial due to this attractive forces produced between this two dipoles, this type of forces is called dipole-dipole intraction. and nitrogen has one loan pair. The stronger these interactions, the greater the surface tension. 13.5: The Structure and Properties of Water, Dipole- Dipole occurs between polar molecules, Ion- Dipole occurs between an ion and polar molecules. as a results, attractive forces is produce. Instead, each hydrogen atom is 101 pm from one oxygen and 174 pm from the other. This effect is similar to that of water, where the oxygen pulls the electrons of the hydrogen atoms with a greater magnitude, resulting in the oxygen having a partial negative charge and the hydrogens having a partial positive charge relative to each other. this molecules is a polar molecules. But we're going to point In 1930, London proposed that temporary fluctuations in the electron distributions within atoms and nonpolar molecules could result in the formation of short-lived instantaneous dipole moments, which produce attractive forces called London dispersion forces between otherwise nonpolar substances. Why are dipole-induced dipole forces permanent? Consider another molecules of hydrogen fluoride, these are also a dipole because it has two pole partial positive pole and partial negative pole. You can absolutely have a dipole and then induced dipole interaction. Why does it take more energy for the molecules in liquid acetaldehyde to be able to break free of each other to overcome their intermolecular forces? NH A 3 (ammonia) Hydrogen bonding The occurence of hydrogen bonding is due to the presence of a lone pair of electrons on nitrogen atom and hydrogen atoms, which creates a dipole-dipole attraction between NH3 molecules. the partially positive end of another acetaldehyde. due to this both atoms are attract each other. The polarizability of a substance also determines how it interacts with ions and species that possess permanent dipoles. And even more important, it's a good bit more These arrangements are more stable than arrangements in which two positive or two negative ends are adjacent (Figure \(\PageIndex{1c}\)). Explain why? Consequently, we expect intermolecular interactions for n-butane to be stronger due to its larger surface area, resulting in a higher boiling point. Now we're going to talk What Is The Concentration (in M Of Hydroxide Ions In A Solution At 25.0 How does the intermolecular determine the boiling point? High concentration? SO2 Molecular shape of SO2 is bent. because chlorine has highly electronegative than hydrogen. Focus and Coverage. So, the increase strength london dispersion forces to hydrogen bonding, it is also increasing boiling point. All right, well, in previous videos, when we talked about boiling points and why they might be different, we talked about intermolecular forces. High concentration electrolytic solutions follow Coulomb forces. In the video on London dispersion forces, we talked about a temporary dipole inducing a dipole in 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. Or another way of thinking about it is which one has a larger dipole moment? So you will have these dipole 60) What type (s) of intermolecular forces exist between NHs and PO43-? this mean, difference in electronegativity. HBr dipole-dipole and London dispersion (greatest boiling point) Kr London . So, it is not symmetric. In this video we'll identify the intermolecular forces for NH3 (Ammonia). Hydrogen bond formation requires both a hydrogen bond donor and a hydrogen bond acceptor. Given the large difference in the strengths of intra- and intermolecular forces, changes between the solid, liquid, and gaseous states almost invariably occur for molecular substances without breaking covalent bonds. Both molecules are linier. Intermolecular Forces for NH3 (Ammonia) - YouTube So, According to above explanation, it is clear that the nh3 is a polar molecules. And the calculated electronegativity of Nitrogen is 3.04 and of hydrogen is 2.2. This bond is a comparatively strong bond and influences the properties like boiling and melting points of the ammonia. Options, are dipole-dipole, London forces, and Hydrogen bonding. Well, the answer, you might So you first need to build the Lewis structure if you were only given the chemical formula. Read More:- What is the intermolecular forces of CO? this is regular cement. For other example, (H.F, Hydrogen fluoride). Well, the partially negative it exhibits, dipole-dipole intraction, induced attraction, and London dispersion forces. . The dipole moment and the charge transfer for the adsorbed gases on pristine Al 24 N 24 and carbon-doped Al 24 N 23 C nanocages were investigated. Dispersion forces act between all molecules. 3 Types of Intermolecular Forces in HF (Hydrogen Fluoride) | Best Guide There are three main major intermolecular forces occur between nh3 molecules such as. For the reaction, NH3(g) + HCl(g) arrow NH4Cl(s) run at 95C, S = 284 J/K, and H = 176 kJ. The attractive energy between two ions is proportional to 1/r, whereas the attractive energy between two dipoles is proportional to 1/r6. As a result attractive force is produce that forces is called hydrogen bonding. Helium is nonpolar and by far the lightest, so it should have the lowest boiling point. The 1-Propanol can form London Force, Dipole- Dipole, and H- bonding due to the H bonded to O atom of OH group, whereas the methoxyethane can not form the H-bonding. and this types of intermolecular forces is called strongest intermolecular forces, for example, H2O, NH3, CH3OH. By Posted how many types of aesthetics are there? As seen in Table Table1, 1, the dipole moment of the pristine Al 24 N 24 nanocage is 0.0068 Debye. Because the boiling points of nonpolar substances increase rapidly with molecular mass, C60 should boil at a higher temperature than the other nonionic substances. Classify: Drag go different combinations of molds in the Gizmodo and categorize them. How do you calculate the ideal gas law constant? As pure molecular solids, which of the following exhibits dipole-dipole intermolecular forces: PH3, SO3, HCl, and CO Lewis structures are shown below for convenience -- 1 n 0-5=8 = io: H-C1: := C=0; PH3 only O HCI only O SO3 and CO2 O PH3 and HCI O SO3, HCl, and CO. You can say that, It is not symmetric. What type of intermolecular forces are present in NH 3? And so based on what Legal. And we've already calculated Asked for: order of increasing boiling points. The ease of deformation of the electron distribution in an atom or molecule is called its polarizability. Hydrogen-bonding: Hydrogen-bonding is a special case of dipole-dipole interaction that occurs between molecules containing a hydrogen. So asymmetric molecules are good suspects for having a higher dipole moment. (b) NH molecule shows dipole-dipole, hydrogen bonding, and dispersion forces. the sutable example is (na+)..(cl-). 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). The CO bond dipole therefore corresponds to the molecular dipole, which should result in both a rather large dipole moment and a high boiling point. This difference in electronegativity causes the NH3 molecule to exhibit polarity. this molecules is also a polar molecules. know that, there are three main major intermolecular forces that act on the molecules such as, hydrogen bonding (H2O,NH3) dipole dipole dipole intraction (HCl) and london dispersion forces (weakest intermolecular forces) (He). Determine the intermolecular forces in the compounds, and then arrange the compounds according to the strength of those forces. Using a flowchart to guide us, we find that NH3 is a polar molecule. Dipole-Dipole Interactions 3. Ethyl methyl ether has a structure similar to H2O; it contains two polar CO single bonds oriented at about a 109 angle to each other, in addition to relatively nonpolar CH bonds. Chemistry Chapter 10 - June 29, 2022 - Chapter 10: Intermolecular Use this radius to find fraction of volume by 2 mole of argon at room temperature at 1 atm. Define types of intermolecular forces and give example for each. This is the expected trend in nonpolar molecules, for which London dispersion forces are the exclusive intermolecular forces. So, the negative pole of one molecules attracted the positive pole of another molecules. The substance with the weakest forces will have the lowest boiling point. Review -1. In fact, the ice forms a protective surface layer that insulates the rest of the water, allowing fish and other organisms to survive in the lower levels of a frozen lake or sea. H3C 2 W S O # O e d CH3 CH3 $ 4 r f 96 5 V Question 20 of 20 t g Oll 6 hp y b & 7 O U n * 8 A) Dipole-dipole forces and hydrogen bonding. higher boiling point. Problems: Chapter 13 And you could have a permanent Consider a pair of adjacent He atoms, for example. and due to highly electronegativity atom like nitrogen (N) are directly connected with hydrogen (H). electronegative than hydrogen but not a lot more electronegative. attracted to each other? Or is it hard for it to become a dipole because it is a symmetrical molecule? So, this reason it is called dipole dipole. Solved What type(s) of intermolecular forces exist between - Chegg to the temporarily negative end of another and vice versa, and that whole phenomenon can domino. Dispersion forces are usually present in all molecules and are temporary. You know Read more, What is Portland Cement? such as, covalent bond, ionic bond, coordination bond. Doubling the distance (r 2r) decreases the attractive energy by one-half. It also has the Hydrogen atoms. The Journal of Chemical Physics is an international journal that publishes cutting edge research in all areas of modern physical chemistry and chemical physics. For each of the molecules below, list the types of intermolecular force which act between pairs of these molecules. Hello, reders welcome to another fresh article. In the structure of ice, each oxygen atom is surrounded by a distorted tetrahedron of hydrogen atoms that form bridges to the oxygen atoms of adjacent water molecules. Make sure you do not confuse your inter forces with intra forces. If you're behind a web filter, please make sure that the domains *.kastatic.org and *.kasandbox.org are unblocked. In case of NH3, both dipole-dipole intraction and hydrogen bonding are persent as well. as you will remember this(LDF) is the weakest intermolecular forces. CH4 have no ions, so there are not ionic forces. The energy of a hydrogen bond for each base pair in DNA is 15 kJ/mol. A. HF hydrogen bond exist between molecules of hydrogen floride. Direct link to Maanya's post Why are dipole-induced di, Posted 2 years ago. 2-methylpropane < ethyl methyl ether < acetone, Dipole Intermolecular Force, YouTube(opens in new window), Dispersion Intermolecular Force, YouTube(opens in new window), Hydrogen Bonding Intermolecular Force, YouTube(opens in new window). due to this, or As a results hydrogen bonding occur between them. You know that, ammonia is a polar molecules. Now some of you might be wondering, hey, can a permanent dipole induce a dipole in a neighboring molecule and then those get Intermolecular forces are the forces which mediate attraction between molecules in a substance. Calculate an ion-dipole interaction energy between \(K^+\) and \(HCl\) at a distance of 600 pm. If you see carefully this structure. quite electronegative. The bridging hydrogen atoms are not equidistant from the two oxygen atoms they connect, however. Both molecules have London dispersion forces at play simply because they both have electrons. The combination of large bond dipoles and short dipoledipole distances results in very strong dipoledipole interactions called hydrogen bonds, as shown for ice in Figure \(\PageIndex{6}\). This can be seen by looking at the formula or in the images of the two. there are two polarized molecules in which they attracted partial negative charge to partial positive charge. Which of these forces are low concentration electrolytic solutions likely to follow? molecules could break free and enter into a gaseous state. The molecule of water has two hydrogen and one oxygen. The human body contains about 100 trillion cells. Molecules with hydrogen atoms bonded to electronegative atoms such as O, N, and F (and to a much lesser extent, Cl and S) tend to exhibit unusually strong intermolecular interactions. Answered: As pure molecular solids, which of the | bartleby Identify the intermolecular forces present in each of these substances (CO, CH3CL, CO2, NH3) 1) Hydrogen bonding, dipole-dipole and dispersion. Now what about acetaldehyde? both of these molecules, which one would you think has We also acknowledge previous National Science Foundation support under grant numbers 1246120, 1525057, and 1413739. Chemistry for Engineering Students. Each water molecule accepts two hydrogen bonds from two other water molecules and donates two hydrogen atoms to form hydrogen bonds with two more water molecules, producing an open, cagelike structure. the structure is symmetrical and therefore, carbon dioxide is nonpolar molecules. Chem Notes For Exam 1.pdf - pressure Vapor Intermolecular forces ion most of people are like limca cold drink, or lemon drink compare with other drink. What intermolecular forces are present in CO_2? | Socratic This property results from the unequal sharing of electrons among the two atoms. you see in front of you, which of these, you think, would have a higher boiling point, a sample of pure propane or a sample of pure acetaldehyde? The three hydrogen atoms are highly electronegative, and the middle atom is positively charged. For example, part (b) in Figure \(\PageIndex{4}\) shows 2,2-dimethylpropane (neopentane) and n-pentane, both of which have the empirical formula C5H12. Now, in a previous video, we talked about London dispersion forces, which you can view as One has strong intermolecular interactions, and the other has relatively weak intermolecular interactions. the videos on dipole moments. All molecules, whether polar or nonpolar, are attracted to one another by London dispersion forces in addition to any other attractive forces that may be present. The properties of liquids are intermediate between those of gases and solids, but are more similar to solids. Electrostatic interactions are strongest for an ionic compound, so we expect NaCl to have the highest boiling point. Dipole Dipole Forces of Attraction - Intermolecular Forces. \[\mu = 1.08 \cancel{D} \times \dfrac{3.3356 \times 10^{30} \; C \cdot m}{1\;\cancel{D}} = 3.6 \times 10^{-30}\; C \cdot m\], \[V = \dfrac{-q\;\mu}{4 \pi \epsilon_o r^2} = \dfrac{- (1.602 \times 10^{-19}\;\cancel{C})(3.6 \times 10^{-30} \cancel{C} \cdot \cancel{m})}{4 \pi (8.853 \times 10^{-12} \cancel{C^2} \cdot N^{1} \cdot m \cancel{^{2}})(6 \times 10^{-10}\; \cancel{m})^2} = -1.44 \times 10^{-20} \; J\]. Is NH3 and H2O dipole-dipole? - cazarhioppaopesia.autoprin.com $$ 75 \times 10^{20}\ cells \times \dfrac{haploid\ genomes}{cell} \times \dfrac{3 \times 10^9\ bp}{haploid\ genome} \times \dfrac{mol}{6.022 \times 10^{23}} \times 650 \dfrac{g}{mol\ bp} = 200\ g \], $$ \dfrac{2\ m}{cell} \times 75 \times 10^{12}\ cells \times \dfrac{km}{1000\ m} = 2 \times 10^{11}\ km \]. ch3cho intermolecular forces. Although there are many, four types of intermolecular forces of attraction (IMFA) are most commonly observed. that is not the case. As expected this is appreciably smaller in energy than covalent bonds (e..g, \(HCl\) has a bond enthalpy of \(7.0 \times 10^{-19}\;J\)).

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nh3 intermolecular forces dipole dipole

nh3 intermolecular forces dipole dipole