Ethandl Heptane 10 20 30 40 70 80 90 100 110 50 60 Temperature (C) The vapor pressure of propanol is 400 mm Hg at 82.0 C. The intermolecular forces in CHCOH are an especially strong type of dipole-dipole force given its own special name hydrogen bonding. Discussion - See all questions in Intermolecular Forces of Attraction. CHBr3 CHCl3 CHI3 Question Which of the following molecules has the weakest intermolecular force? Also, It melts at -140 C. apply. Clearly,in this case; the increase in mass outweighs the change in polarity when it comes to affecting boiling point. The major intermolecular forces would be dipole-dipole forces and London dispersion forces. How positive invironments support the development of young children learning outcome? %%EOF H-F bonds it can interact with itself and with other choh molecules. What is the strongest intermolecular force in CHCl3? How do intermolecular forces affect surface tension and viscosity? How do intermolecular forces affect evaporation rate? Submit Answer Retry Entire Group 9 more group attempts remaining What is the most significant Like water, acetic acid has strong hydrogen bonds. (b) Which of the two would you expect to have the highest viscosity at 25 C? Acetic acid melts at 16 C. 0.50 m Zn(NO3)2 has the LOWEST The only intermolecular forces in methane are London dispersion forces. Butane, CH, has almost the same molar mass. 0000001214 00000 n In that instance, the dominant intermolecular force will be dipole-dipole interactions. How do intermolecular forces of attraction affect the evaporation of liquids? Legal. The only intermolecular forces in this long hydrocarbon will be (2) Which liquid would be expected to have the highest vapor pressure at 51.7 C? Submit Answer Retry Entire Group 9 more group attempts remaining 0.25 m Na2SO4 has the LOWEST We reviewed their content and use your feedback to keep the quality high. Identify type of the intermolecular forces in the following compound. Both CHCl3 and NH3 are polar molecules . In a nonpolar molecule, electrons are always moving. We reviewed their content and use your feedback to keep the quality high. WebWhich intermolecular forces do you expect to be present in chloroform (CHCl3) in its liquid form? CH3OH in CCl4 CH3OH is not very soluble in CCl4, but some molecules of CH3OH can manage to get into the CCl4. C than the intermolecular forces in carbon disulfide. Choose the molecule or compound that exhibits dipole-dipole forces as its strongest intermolecular force. SO2 and CHCl3 experience dipole-dipole intermolecular forces. A hydrogen atom between two small, electronegative atoms (such as \(\ce{F}\), \(\ce{O}\), \(\ce{N}\)) causes a strong intermolecular interaction known as the hydrogen bond. WebIn an another study of a similar mixture (CH3 OH/CH2 Cl2 ) with 0.4 mole fraction of methanol, intermolecular electron transfer rate is found to be slowest and solvent reorganization energy is highest, which is associated with slower solute diusion in the mixture. WebIdentify type of the intermolecular forces in the following compound. because there are more unproductive collisions between 0000006096 00000 n Its strongest intermolecular forces are London dispersion forces. FOIA. WebAnswer and Explanation: Hydrogen bonding will be another intermolecular force of attraction for the two molecules since both hydrogen peroxide and methanol has a hydrogen atom that is bonded to an Oxygen atom. Solid CO2 sublimesChoose one or more: A.Dispersion forces B.Dipoledipole interactions C.Hydrogen bonding CHCl3 boilsChoose one or more: A.Dispersion forces B.Dipoledipole interactions C.Hydrogen bonding Ice meltsChoose one or more: Why does CH3Cl have a high boiling point? Use. The hydrogen bonds cause this enormous difference in melting point. The positive charge attracts the electrons in an adjacent molecule. being in the center. apply. it is polar. Two inter molecular forces that are active between two molecules of CHCl3 are Dipole Dipole, Some answers can be found in the Confidence Building Questions. the covalent bonds which binds all of the atoms with the carbon 0000001343 00000 n Answer: HF has the higher boiling point because HF molecules are more polar. (a) In which of the two are the intermolecular forces the weakest? The stronger these forces, the lower the rate of evaporation and the lower the vapor pressure. How is melting point related to the intermolecular forces of attraction? How do London dispersion forces come about? Which has the higher boiling point, \(\ce{Br2}\) or \(\ce{ICl}\)? 11 0 obj<>stream What intermolecular forces are present in #CO_2#? WebThe polar water molecules interact better with the polar CHCl3 molecules than with the non-polar CCl4 molecules so CHCl3 is more soluble. Discussion - Part B: CHBr3 molecules possess stronger intermolecular interaction due to higher molar mass than CHCl3 Explanation: Fluorine is more electronegative than chlorine. therefore, dipole-dipole and dispersion forces (always present) What is the intermolecular forces of What is the intermolecular force of CHCL3. Two inter molecular forces that are active between two molecules of CHCl3 are Dipole Dipole, because it is a polar molecule, and London dispersion, because all molecules use them. What are the definitions of rogelia folk dance? Chloromethane is a carbon with three hydrogens and a chlorine attached to it. for \(\ce{H2O}\) is 100 deg C, and that of \(\ce{H2S}\) is -70 deg C. Very strong hydrogen bonding is present in liquid \(\ce{H2O}\), but no hydrogen bonding is present in liquid \(\ce{H2S}\). The predominant intermolecular force of CH3Cl, chloromethane, is See, Animal Cage Market Growth, Trends, Size, Share, Demand Forecast to 2023 to 2032, Fish Protein Hydrolysates Market Overview Analysis, Trends, Share, Size, Type & Future Forecast 2032, Powered Prosthetics Market Size, Global Trends, Latest Techniques, And Forecasts Till 2032, Golden opportunity for 200-hour teacher training in India, Cash App Account Has Been Closed Due To Suspicious Activity. WebIntermolecular forces (IMFs) can be used to predict relative boiling points. WebSubstance 3: CHCl3 The three substances above each have one of the following vapor pressures: 2.1 kPa, 15.3 kPa, and 26 kPa. Use the References to access important values if needed for this question. The intermolecular forces in CHCOH are an especially strong type of dipole-dipole force given its own special name hydrogen bonding. 8.43 Identify the kinds of intermolecular forces (London dispersion, dipoledipole, or hydrogen bonding) that are the most important in each of the following substances. In CH3Cl, the C-Cl bond is polar. The energy required to break a bond is called the bond-energy. solutions: 1.00 m LiBr has the LOWEST freezing point. Water has strong hydrogen bonds. 0000005022 00000 n 20794 views Department of Health and Human Services. WebHow can you determine the intermolecular forces of CHCl3? startxref Use the following vapor pressure data to answer the questions: Liquid Vapor Pressure, torr Temperature, C A CHyNha 400 31.5 B CC14 400 57.8 (1) In which liquid are the intermolecular attractive forces the strongest ? (a) In which of the two are the intermolecular forces the weakest? 0000003034 00000 n The b.p. Share Save Helvetica Comment Bholu Friend 3 years ago Follow Chloroform has a distinct dipole moment. <<756da9636b8db4449f174ff241673d55>]>> There are no bond dipoles and no dipole-dipole interactions. What kind of intermolecular forces are present in CHCl3? Induced dipoles are responsible for the London dispersion forces. Ethandl Heptane 10 30 20 40 90 80 100 110 50 60 70 Temperature (C) The vapor pressure of chloroform is 400 mm Hg at 42.0 C. Few things to consider, in order: Do they contain hydrogen bonds? If there is a bond between hydrogen and either oxygen, nitrogen, or fluorine? The Submit Answer Retry Entire Group 9 more group attempts remaining. Therefore, we can compare the relative strengths of the IMFs of the compounds to predict their relative boiling points. Web2 a. water (H2O) and chloroform (CHCl3) b. benzene (C6H6) and chloroform (CHCl3) c. water (H2O) and vinegar (CH3COOH) d. acetone (C3H6O) and toluene (C6H5CH3) e. carbon tetrachloride (CCl4) and water (H2O) Strong intermolecular forces tend to yield solids and liquids while weak intermolecular forces favor formation of gases. The steric number in the case of CH3Cl is 4. The stronger the IMFs, the lower the vapor pressure of the substance and the higher the boiling point. If only London dispersion forces are present, which should have a lower boiling point, \(\ce{H2O}\) or \(\ce{H2S}\)? Webch_10_practice_test_liquids_solids-and-answers-combo - Read online for free. .For CHCl3, the molecule is tetrahedral but the atoms around the C are not all the same (3 Cl atom. (Select all that apply.) The greater the intermolecular forces, the greater the CH3 lot I d -CH3 c) e) a a) b) OH I+ H3C f) A: Chiral center :- The center or carbon atom in molecule which is connected with four different Q: Which is more polar:hexane or water?How will the difference in polarity be exploited in the What is the strongest intermolecular force in CHCl3? WebThe compound is: JIPMER - 1998 Alcohols Chemistry The alcohol having molecular formula C_4H_9OH C 4H 9OH, when shaken with a mixture of anhydrous ZnCl_2 Z nC l2 and conc. These are polar forces, intermolecular forces of attraction If you are looking for specific information, your study will be efficient. Above 4 deg C, the thermal expansion is more prominent than the effect of hydrogen bonds. Hint: Ethanol has a higher boiling point. The equation consist of: (1) ( P + n 2 a V 2) ( V n b) = n R T The V in the formula refers to the volume of gas, in moles n. The intermolecular forces of attraction is incorporated into the equation with the n 2 a V 2 term where a is a the molecule hcl is Atomic weights for \(\ce{Br}\) and \(\ce{I}\) are 80 and 127 respectively. Select all that apply. dipole - dipole Use the following vapor pressure data to answer the questions: Liquid Vapor Pressure, torr Temperature, C A CHyNha 400 31.5 B CC14 400 57.8 (1) In which liquid are the intermolecular attractive forces the strongest ? WebHere, we have synthesized four series of polyamide-conductive polymers and used them to modify Fe3O4 NPs/ITO electrodes. \(\ce{R-OH}\) group is both proton donor and acceptor for hydrogen bonding. 0000000776 00000 n Their boiling points are 332 K and 370 K respectively. initial rate experiment shown for the reaction: 2 A + 3 B -> So, there are permanent Which has a higher boiling point, \(\ce{I2}\) or \(\ce{Br2}\)? CHCl3 - Chemistry | Shaalaa.com. Hydrogen bonds form when you have a negative O, N, or F atom in one molecule and a positive H atom attached to an O, N, or F atom in another molecule. 0000002374 00000 n Use the following vapor pressure data to answer the questions: Vapor Pressure, torr Temperature, C Liquid CHI A 400 25.3 B C7H16 400 78.0 (1) In which liquid are the intermolecular attractive forces the strongest ? Both London forces and permanent dipole - permanent dipole interactions are the intermolecular forces that holds up these molecules. London forces The intermolecular forces operating in NO would be dipole Routing number of commercial bank of Ethiopia? CH2Cl2 has a tetrahedral shape. How to Make a Disposable Vape Last Longer. WebIntermolecular Forces are the forces between the two molecules, and can be classified under dipole-dipole (Hydrogen bonds falls under this), ion-dipole, or London Dispersion 0 Why? How do functional groups affect intermolecular attractions? CH3Cl intermolecular forces has dipole-dipole forces and London dispersion forces.the chemical name of CH3Cl is chloromethane. Hello, reders today we will discuss about what is the intermolecular forces of ch3cl and polarity . I have made this guide to help you out. So, hold your seat and be with the end of guide. WebCHCl3 molecules are polar. Question: 1. 169558 views WebA liquid with weak intermolecular forces evaporates more easily and has a high vapor pressure. See Chloroform (data page) - Wikipedia. What is the intermolecular forces of CHCl3? xref 0000002221 00000 n Its boiling point is 61.2 degrees C. That is a 22% difference in molecular mass,and a 21% increase in boiling point. On average, 463 kJ is required to break 6.023x1023 \(\ce{O-H}\) bonds, or 926 kJ to convert 1.0 mole of water into 1.0 mol of \(\ce{O}\) and 2.0 mol of \(\ce{H}\) atoms. Which intermolecular forces do you expect to be present in WebIdentify all possible types of intermolecular forces that can form between particles of each substance below. This link gives an excellent introduction to the interactions between molecules. (a) CO2 dipole-dipole interactions hydrogen bonding interactions ion-dipole interactions London dispersion forces (b) CHCl3 dipole-dipole interactions hydrogen bonding interactions ion-dipole interactions London 0000000959 00000 n There are no bond dipoles and no dipole-dipole interactions. Octane is non-polar organic compound. That eliminates hydrogen bonding and dipole-dipole interactions. What you have left is induced dipole to indu energies are lower. (a) Reactions are faster at a higher temperature because activation Submit Answer Retry Entire Group more group attempts remaining Vapor pressure (mm Hg) 8 8 8 8 8 900 800 700 600 500 400 300 200 100 wwwfus Carbon disulfide, Methanol Chloroform has a distinct dipole moment. chloroform (CHCl3) in its liquid form? The two covalent bonds from the single oxygen to the two hydrogens are forced from positions at opposite sides by the presence of two lone pairs of 0000006682 00000 n The strength of a hydrogen bond depends upon the electronegativities and sizes of the two atoms. The predominant intermolecular force of CH3Cl, chloromethane, is the covalent bonds which binds all of the atoms with the carbon being in the center. 4Hm_&+LsknEv&SsqExT 2H3KZI`Q9vy'i67%ZYfE2cuU:r. Accessibility StatementFor more information contact us atinfo@libretexts.orgor check out our status page at https://status.libretexts.org. The LibreTexts libraries arePowered by NICE CXone Expertand are supported by the Department of Education Open Textbook Pilot Project, the UC Davis Office of the Provost, the UC Davis Library, the California State University Affordable Learning Solutions Program, and Merlot. In a smaller molecule, there is less hindrance around the polar bonds, making intermolecular bonding stronger. Discussion - dipole - induced dipole induced dipole - induced dipole Experts are tested by Chegg as specialists in their subject area. Solution : The N2 and CO2 molecules are nonpolar , so only dispersion forces are present . The forces holding molecules together are generally called intermolecular forces. Check out a sample Q&A here See Solution star_border Students whove seen this question also like: World of Chemistry, 3rd edition 0000004613 00000 n I think youve got it backward. A molecules geometry helps to determine its dipole moment. The molecules dipole moment is the vector sum of its i WebWhat kind (s) of intermolecular forces must be overcome during the following phase changes? Because methane is a non-polar molecule it is not capable of hydrogen bonding or dipole-dipole intermolecular forces. For example, the average bond-energy for \(\ce{O-H}\) bonds in water is 463 kJ/mol. In solid acetic acid, the molecules form cyclic pairs connected by hydrogen bonds. Intermolecular forces: the forces of attraction present in between the molecules or atoms or compounds is termed as intermolecular forces. od [Review Topics Use the References to access important values if needed for this question. What parameters cause an increase of the London dispersion forces? The heat of vaporization of chloroform would be expected to be than the heat of vaporization of carbon disulfide. slideshare.net There is some degree of hydrogen-bonding, but given the graph, it is clear that dispersion forces tend to dominate as the major intermolecular force in the lower hydrogen halides. What chemical groups are hydrogen acceptors for hydrogen bonds? Experts are tested by Chegg as specialists in their subject area. WebThe intermolecular forces in propanol are Submit Answer Retry Entire Group Vapor pressure (mm Hg) 900 800 700 600 500 400 300- 200 100- 0 Carbon disulfide Methano more group attempts remaining Use the References to access important values if needed for this question. HlSK0W~FX+ A$CwaugM]4kPu-A@/NPiNCZp89\o:[xxT\pyM3HoQKHDunQwH: 0lAE$8lnRTFDb 0000000016 00000 n solubility. A molecule with polar bonds unsymmetrically arranged will possess a permanent dipole. dispersion forces. Polarization separates centers of charge giving. Intermolecular forces also play important roles in solutions, a discussion of which is given in Hydration, solvation in water. is/are correct regarding the following strong electrolyte How to Make a Disposable Vape Last Longer. der Waal's forces(London forces). The intermolecular forces in propanol are Submit Answer Retry Entire Group Vapor pressure (mm Hg) 900 800 700 600 500 400 300- 200 100- 0 Carbon disulfide Methano more group attempts remaining 0000004070 00000 n Arrange the following substances in order of 13.1: Intermolecular Interactions is shared under a CC BY-NC-SA 4.0 license and was authored, remixed, and/or curated by LibreTexts. An atom or molecule can be temporarily polarized by a nearby species. the chemical name of CH3Cl is chloromethane. 2003-2023 Chegg Inc. All rights reserved. Thus, London dispersion forces are strong for heavy molecules. chloroform (CHCl3) in its liquid form? The only intermolecular forces in methane are London dispersion forces. Ammonia contains hydrogen bonds as well as dispersion forces. Chloroform has a distinct dipole moment. c) CH3OH Hydrogen bonding CH3SH Dipole-dipole interaction Hydrogen bonding is the strongest intermolecular force, so CH3OH will have the higher boiling point. Ideal" is not just a word, it is a game of assumptions. It had a monopoly in the 17th century when Boyle introduced his law which was a stepping s The major intermolecular forces would be dipole-dipole forces and London dispersion forces. Dipole forces and London forces are present as intermolecular Of course all types can be present simultaneously for many substances. At any instant, they might be at one end of the molecule. See Chloroform endstream endobj 10 0 obj<> endobj 12 0 obj<> endobj 13 0 obj<>/ProcSet[/PDF/Text]/ExtGState<>>> endobj 14 0 obj<> endobj 15 0 obj<> endobj 16 0 obj<> endobj 17 0 obj<> endobj 18 0 obj<> endobj 19 0 obj<> endobj 20 0 obj<> endobj 21 0 obj<> endobj 22 0 obj<> endobj 23 0 obj<> endobj 24 0 obj<>stream Submit Answer Retry Entire Group 9 more group attempts remaining let's not forget that like all other molecules, there are also Van Contrary to most other substances, the density of water decreases as temperature decreases between 4 and 0 deg C. This is due to, increasing number of hydrogen bonds formed. Consider carefully the purpose of each question, and figure out what there is to be learned in it. 8600 Rockville Pike, Bethesda, MD, 20894 USA. xb```PV,``X llLH B1dsoK'0\$U?KE,@ - r around the world. The forces holding molecules together are generally called intermolecular forces. Few things to consider, in order: Do they contain hydrogen bonds? If there is a bond between hydrogen and either oxygen, nitrogen, or fluorine? The Expert Solution Want to see the full answer? A summary of the interactions is illustrated in the following diagram: See if you can answer the following questions. How do intermolecular forces affect freezing point? The four prominent types are: The division into types is for convenience in their discussion. WebBoth CHCl3 and NH3 are polar molecules. intermolecular forces forces that exist between molecules 11.1: A Molecular Comparison of Gases, Liquids, and Solids The state of a substance depends on the balance Chung (Peter) Chieh (Professor Emeritus, Chemistry @University of Waterloo). A liquid with stronger intermolecular forces does not evaporate easily and thus has a lower vapor pressure. Discussion - Assuming ideal behavior, which of the following statements (2) The vapor pressure of C3H-NH at 57.8 C would be [ than 400 torr. what type of intermolecular force does chbr3 have? Contact. Which intermolecular forces do you expect to be present in Which of the following statements are incorrect? dipole - induced dipole C. Which of the following statements are correct with respect to From the plot of vapor pressures vs temperature above, estimate the temperature at which the vapor pressure of carbon disulfide is 400 mm Hg. What is the You'll get a detailed solution from a subject matter expert that helps you learn core concepts. Use the References to access important values if needed for this question. We also acknowledge previous National Science Foundation support under grant numbers 1246120, 1525057, and 1413739. This temporary attractive force is the London dispersion force. Thus, CCl4 is a nonpolar molecule, and its strongest intermolecular forces are London dispersion forces. Discussion - What is the intermolecular forces of CH3Cl? ances Use the References to access important values if needed for this question. Identify type of the As more hydrogen bonds form when the temperature decreases, the volume expands, causing a decrease in density. Synthesis of the target-conducting polyamides, P1a–d, P2a–d, P3a, P3b, P3d, and P4c-d, WebThe polar water molecules interact better with the polar CHCl3 molecules than with the non-polar CCl4 molecules so CHCl3 is more soluble. Use the References to access important values if needed for this question. forces in these molecules. A polar covalent bond is defined as the bond which is formed when there is a difference of electronegativities between the atoms. It is also define dipole-dipole forces both molecules have tetrahedral geometries and have both london and dipole-dipole forces. The electronegativities of C and H are so close that C-H bonds are nonpolar. The London dispersion forces are so weak that methane does not condense to a liquid until it cools to 161.5 C. (b) Rates decrease with increasing concentration of reactants between molecules. WebA liquid with weak intermolecular forces evaporates more easily and has a high vapor pressure. Liquid cyclopentane (C5H0) has a normal boiling point of 49.3 C and liquid cyclohexane (C4H2) has a normal boiling point of 80.7 C. WebWhat atom is closest to the negative side. WebWhich of the following molecules has the weakest intermolecular force? between molecules. Discussion - trailer National Library of Medicine. They have similar molecular weights: \(\mathrm{Br_2 = 160}\); \(\mathrm{ICl = 162}\). You'll get a detailed solution from a subject matter expert that helps you learn core concepts. Chloroform contains dipole forces as well as dispersion forces. Why does CCl4 have no dipole moment? This implies that HF is more polar and possess stronger hydrogen bonds than HCl molecules. Webmolecules held together by weak van der Waal forces, which means that the properties of 55 %), is slightly soluble in CH2Cl2 or CHCl3 and has been characterized by electron impact mass spectrometry (Mw = 664), 13C NMR (ppm) 140.400, 136.829, large decrease in solubility already indicates that strong intermolecular interactions exist in These are polar forces, intermolecular forces of attraction a. BCl3 b. H2O c. N2. How do intermolecular forces affect solvation? A liquid with stronger intermolecular forces does not evaporate easily and thus has a lower vapor pressure. 5 people found it helpful Brainly User Two inter molecular forces that are active between two molecules of CHCl3 are Dipole Dipole, because it is a polar molecule, The electronegativities of C and H are so close that C-H bonds are nonpolar. Okay so let me start this answer by the most common misconception which people have about CHCL3 i.e. chloroform. The basic condition to form hydrog This would instantaneously create a temporary dipole, making that end negative and the other end positive. The only intermolecular forces in this long hydrocarbon will be Policies. HHS Vulnerability Disclosure. The energy required to break molecules apart is much smaller than a typical bond-energy, but intermolecular forces play important roles in determining the properties of a substance. Webintermolecular forces is viscosity, a measure of a liquids resistance to flow. CH3Cl intermolecular forces has dipole-dipole forces and London dispersion forces. Webch_10_practice_test_liquids_solids-and-answers-combo - Read online for free. around the world. Thats because it is a stronger type of intermolecular force than the alternatives of ionic bonding (there are no ions) and hydrogen bonding (the only stronger intermolecular force) are not applicable for chloroform. Liquid decane (C10H22) has a normal boiling point of 174 C and liquid heptane (CH16) has a normal boiling point of 98.4 C. The alcohol is VITEEE - 2011 Alcohols Chemistry 1 -Propanol and 2-propanol can be distinguished by VITEEE - 2017 Alcohols Hydrogen bonds form when you have a negative O, N, or F atom in one molecule and a positive H atom attached to an O, N, or F atom in another molecule. When do intermolecular forces of attraction occur? Maharashtra State Board HSC Science (Electronics) 11th. osmotic pressure at 25 C . Discussion - Map: Physical Chemistry for the Biosciences (Chang), { "13.01:_Intermolecular_Interactions" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "13.02:_The_Ionic_Bond" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "13.03:_Types_of_Intermolecular_Forces" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "13.04:_Hydrogen_Bonding" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "13.05:_The_Structure_and_Properties_of_Water" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "13.06:_Hydrophobic_Interaction" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "13.E:_Intermolecular_Forces_(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_to_Physical_Chemistry" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "02:_Properties_of_Gases" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "03:_The_First_Law_of_Thermodynamics" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "04:_The_Second_Law_of_Thermodynamics" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "05:_Solutions" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "06:_Chemical_Equilibrium" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "07:_Electrochemistry" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "08:_Acids_and_Bases" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "09:_Chemical_Kinetics" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "10:_Enzyme_Kinetics" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "11:_Quantum_Mechanics_and_Atomic_Structure" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "12:_The_Chemical_Bond" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "13:_Intermolecular_Forces" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "14:_Spectroscopy" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "15:_Photochemistry_and_Photobiology" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "16:_Macromolecules" : "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]()" }, [ "article:topic", "showtoc:no", "license:ccbyncsa", "licenseversion:40" ], https://chem.libretexts.org/@app/auth/3/login?returnto=https%3A%2F%2Fchem.libretexts.org%2FBookshelves%2FPhysical_and_Theoretical_Chemistry_Textbook_Maps%2FMap%253A_Physical_Chemistry_for_the_Biosciences_(Chang)%2F13%253A_Intermolecular_Forces%2F13.01%253A_Intermolecular_Interactions, \( \newcommand{\vecs}[1]{\overset { \scriptstyle \rightharpoonup} {\mathbf{#1}}}\) \( \newcommand{\vecd}[1]{\overset{-\!-\!\rightharpoonup}{\vphantom{a}\smash{#1}}} \)\(\newcommand{\id}{\mathrm{id}}\) \( \newcommand{\Span}{\mathrm{span}}\) \( \newcommand{\kernel}{\mathrm{null}\,}\) \( \newcommand{\range}{\mathrm{range}\,}\) \( \newcommand{\RealPart}{\mathrm{Re}}\) \( \newcommand{\ImaginaryPart}{\mathrm{Im}}\) \( \newcommand{\Argument}{\mathrm{Arg}}\) \( \newcommand{\norm}[1]{\| #1 \|}\) \( \newcommand{\inner}[2]{\langle #1, #2 \rangle}\) \( \newcommand{\Span}{\mathrm{span}}\) \(\newcommand{\id}{\mathrm{id}}\) \( \newcommand{\Span}{\mathrm{span}}\) \( \newcommand{\kernel}{\mathrm{null}\,}\) \( \newcommand{\range}{\mathrm{range}\,}\) \( \newcommand{\RealPart}{\mathrm{Re}}\) \( \newcommand{\ImaginaryPart}{\mathrm{Im}}\) \( \newcommand{\Argument}{\mathrm{Arg}}\) \( \newcommand{\norm}[1]{\| #1 \|}\) \( \newcommand{\inner}[2]{\langle #1, #2 \rangle}\) \( \newcommand{\Span}{\mathrm{span}}\)\(\newcommand{\AA}{\unicode[.8,0]{x212B}}\), status page at https://status.libretexts.org.
How Much Space Does 1 Billion Dollars Take Up, Blue Moon Light Sky Vs Michelob Ultra, Air Assault Cadence, Juliette Lewis Sister, Articles C