How do London dispersion forces arise in a nonpolar molecule? Because if you have high We don't see any bonds between hydrogen and an oxygen, a nitrogen, or a fluorine. are in the gaseous state, every now and then they're Does isopropyl alcohol have a dipole moment? 0000001613 00000 n
The greater the intermolecular the force, the greater the energy 0000006246 00000 n
Of the compounds that can act as hydrogen bond donors, identify those that also contain lone pairs of electrons, which allow them to be hydrogen bond acceptors. And I put one of these, a sample of one of these A crystalline solid can be represented by its unit cell, which is the smallest identical unit that when stacked together produces the characteristic three-dimensional structure. Vaporization occurs when a liquid changes to a gas, which makes it an endothermic reaction. And so that's going to keep happening. Now, you might notice, With solid's particles being closely packed and having little motion relative to each other, and gas particles being greatly disperse from each other. To log in and use all the features of Khan Academy, please enable JavaScript in your browser. highest intermolecular forces when they're in a liquid state? WebMethyl Ethyl Ketone CAS: 78-93-3 Methyl Ethyl Ketone also known as MEK, butanone, 2-butanone, butan-2-one, oxobutane, or methyl acetone is a clear volatile liquid that is soluble in water and has a mild, acetone odour and has the molecular formula C 4 H 8 O, CAS: 78-93-3. The test liquid is isopropyl alcohol (Sigma-Aldrich 99.5%), with a surface tension of 20.8 mN/m, a density of 0.785 g/ml, a viscosity of 1.66 mPas, a conductivity of K 6 S/m, and a relative permittivity of 18.6. WebThis allows the water molecules to have enough kinetic energy to continue evaporation. 0000001016 00000 n
Considering CH3OH, C2H6, Xe, and (CH3)3N, which can form hydrogen bonds with themselves? Solids are characterized by an extended three-dimensional arrangement of atoms, ions, or molecules in which the components are generally locked into their positions. And if we look at the actual data, it's consistent with what https://www.khanacademy.org/science/ap-chemistry-beta/x2eef969c74e0d802:intermolecular-forces-and-properties/x2eef969c74e0d802:intermolecular-forces/v/dipole-dipole-forces. Because alcohols form hydrogen bonds with water, they tend to be relatively soluble in water. , 4 stanza poem about chemical bonds and its importance to humans, 7. The amount of energy we need to add to make this physical change must overcome all the intermolecular forces Would like to know which video tells us about Dipole-Dipole forces, Thanks. Draw the hydrogen-bonded structures. But then when that vapor gets high enough or when you could say the vapor Figure 1 MATERIALS Water has strong intermolecular forces called hydrogen bonds. Water, alcohol, ether, acetone, tetrahydrofuran, chloroform and benzene are widely used as solvents. Im? Most of the common alcohols are colourless liquids at room temperature. Does isopropyl alcohol evaporate faster than ethyl alcohol? Map: Chemistry - The Central Science (Brown et al. A Of the species listed, xenon (Xe), ethane (C2H6), and trimethylamine [(CH3)3N] do not contain a hydrogen atom attached to O, N, or F; hence they cannot act as hydrogen bond donors. which of the following will have the highest boiling point? are going to break away, and so you're going to by the intermolecular forces and enter a liquid state. So what are we talking about, why, about vapor pressure, and why Thanks to its -OH group, isopropyl alcohol molecules can form weak bonds, called hydrogen bonds, that help hold the molecules together. Consequently, it has a much higher boiling and melting point than propane, which also contains three carbons and eight hydrogens. What is the strongest attractive force in isopropyl alcohol? WebHowever, the study of intermolecular forces formed by 1,2-propanediamine with mono-alcohols has not been reported; therefore, the present work investigates the intermolecular forces between 1,2-propanediamine and n-propanol/isopropanol. intermolecular forces, it would take a lot of energy 0000003644 00000 n
What is the density (g/cm 3 ) of aluminum? Surfactants are molecules that reduce the surface tension of polar liquids like water. or a higher boiling point to really overcome those In a solution of water and ethanol, hydrogen bonding The intermolecular forces between molecules of isopropyl alcohol are in the form of hydrogen bonds, where a partially positive hydrogen atom of one molecule experiences a strong attractive force to a partially negative oxygen atom of another molecule. thing called vapor pressure. because water has stronger hydrogen bonding (intermolecular forces) it has a higher heat capacity and boiling point at 100 The more water that evaporates from your skin, the cooler your skin feels. is Methanol the same thing as Breaking bad? to get to an ethanol. 10.3: Intermolecular Forces in Liquids is shared under a CC BY-NC-SA 4.0 license and was authored, remixed, and/or curated by LibreTexts. Why is the Lewis structure of isopropyl alcohol polar? 0000042173 00000 n
Web[1 mark C] Surface tension is the elastic property of a liquids surface, determined by its intermolecular forces, that allows it to resist an external force. Stronger intermolecular forces will produce greater surface tension The intermolecular forces present in a sample of water are hydrogen bonds The high surface tension of water allows a paper clip to float on the surface of the water. Enter a Melbet promo code and get a generous bonus, An Insight into Coupons and a Secret Bonus, Organic Hacks to Tweak Audio Recording for Videos Production, Bring Back Life to Your Graphic Images- Used Best Graphic Design Software, New Google Update and Future of Interstitial Ads. You will examine the molecular structure of alkanes and alcohols for the presence and relative strength of two intermolecular forceshydrogen bonding and dispersion forces. So London dispersion forces. Pause this video, and (See chemical bonding: Intermolecular forces for a discussion of hydrogen bonding. 0000010376 00000 n
Water has the strongest intermolecular force among thus option because the molecules of water are been tied by Hydrogen bond. Many molecules are polar and can form bipole-bipole bonds without forming hydrogen bonds or even having hydrogen in their molecule. At the beginning of the video, when Sal was figuring out the boiling points, he was looking at the O-H bonds. The physical states differ in how close the particles of matter are to each other essentially. i%+gY`eM^GrzTx*=JOSTx*nJ7)MdM:a~&#&ks1yL3~0)_-
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2 Does isopropyl alcohol have strong intermolecular forces? )%2FUnit_3%253A_The_States_of_Matter%2F10%253A_Solids_Liquids_and_Phase_Transitions%2F10.3%253A_Intermolecular_Forces_in_Liquids, \( \newcommand{\vecs}[1]{\overset { \scriptstyle \rightharpoonup} {\mathbf{#1}}}\) \( \newcommand{\vecd}[1]{\overset{-\!-\!\rightharpoonup}{\vphantom{a}\smash{#1}}} \)\(\newcommand{\id}{\mathrm{id}}\) \( \newcommand{\Span}{\mathrm{span}}\) \( \newcommand{\kernel}{\mathrm{null}\,}\) \( \newcommand{\range}{\mathrm{range}\,}\) \( \newcommand{\RealPart}{\mathrm{Re}}\) \( \newcommand{\ImaginaryPart}{\mathrm{Im}}\) \( \newcommand{\Argument}{\mathrm{Arg}}\) \( \newcommand{\norm}[1]{\| #1 \|}\) \( \newcommand{\inner}[2]{\langle #1, #2 \rangle}\) \( \newcommand{\Span}{\mathrm{span}}\) \(\newcommand{\id}{\mathrm{id}}\) \( \newcommand{\Span}{\mathrm{span}}\) \( \newcommand{\kernel}{\mathrm{null}\,}\) \( \newcommand{\range}{\mathrm{range}\,}\) \( \newcommand{\RealPart}{\mathrm{Re}}\) \( \newcommand{\ImaginaryPart}{\mathrm{Im}}\) \( \newcommand{\Argument}{\mathrm{Arg}}\) \( \newcommand{\norm}[1]{\| #1 \|}\) \( \newcommand{\inner}[2]{\langle #1, #2 \rangle}\) \( \newcommand{\Span}{\mathrm{span}}\)\(\newcommand{\AA}{\unicode[.8,0]{x212B}}\), 10.2: Intermolecular Forces - Origins in Molecular Structure. Please explain in detail so I can follow 0000003732 00000 n
bonding, copy the molecule below and highlight or circle the, which liquid has stronger intermolecular forces water or isopropyl alcohol 2021, which liquid has stronger intermolecular forces water or isopropyl alcohol, Costco Breaded Tilapia Cooking Instructions, The Untamed Special Edition Ending Explained. 5 Does isopropyl alcohol evaporate faster than ethyl alcohol? If you continue to use this site we will assume that you are happy with it. Accessibility StatementFor more information contact us atinfo@libretexts.org. Which has the weakest? But we can think about So London dispersion Consequently, HO, HN, and HF bonds have very large bond dipoles that can interact strongly with one another. Ionic solids consist of positively and negatively charged ions held together by electrostatic forces; the strength of the bonding is reflected in the lattice energy. How do ionic and molecular compounds compare in terms of boiling points? The effect is most dramatic for water: if we extend the straight line connecting the points for H2Te and H2Se to the line for period 2, we obtain an estimated boiling point of 130C for water! and the right kinetic energy to escape and get into the vapor state, into a gaseous state. WebWater had the strongest intermolecular forces and evaporated most slowly. Explanation: Short chain alcohols have intermolecular forces that are dominated by H-bonds and dipole/dipole, so they dissolve in water readily (infinitely for trailer
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A.liquids B.gases C.solids D.both, The radius of an indium atom is 0.163 nm. Web[1 mark C] Surface tension is the elastic property of a liquids surface, determined by its intermolecular forces, that allows it to resist an external force. During the winter when lakes begin to freeze, the surface of the water freezes and then moves down toward deeper water; this explains why people can ice skate on or fall through a frozen lake. The states of matter exhibited by a substance under different temperatures and pressures can be summarized graphically in a phase diagram, which is a plot of pressure versus temperature. The hydrogen-bonded structure of methanol is as follows: Considering \(\ce{CH3CO2H}\), \(\ce{(CH3)3N}\), \(\ce{NH3}\), and \(\ce{CH3F}\), which can form hydrogen bonds with themselves? 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). intermolecular forces that we have studied. Web2. It's the same mechanism, it's just that hydrogen bonding only generally applies to molecules where hydrogen is directly bonded to fluorine, oxygen, or nitrogen. CHEM 114. Expert Help. We also acknowledge previous National Science Foundation support under grant numbers 1246120, 1525057, and 1413739. 6 Why is isopropyl alcohol like all alcohols? Changes from a more-ordered state to a less-ordered state (such as a liquid to a gas) are endothermic. Stronger intermolecular forces will produce greater surface tension The intermolecular forces present in a sample of water are hydrogen bonds The high surface tension of water allows a paper clip to float on the surface of the water. Hydrogen bonding is an intermolecular force, so it acts between molecules. 'kN9rt[hP">!R">EL(bB02 GL8bp#&1EoaZFJ. So just looking at this, I know that water's going to The bridging hydrogen atoms are not equidistant from the two oxygen atoms they connect, however. WebIn this portion of the lab, you will determine which liquid has the highest surface tension: water, soapy water, or rubbing alcohol. Most of this difference results from the ability of ethanol and other alcohols to form intermolecular hydrogen bonds. 0000001409 00000 n
WebWater had the strongest intermolecular forces and evaporated most slowly. Hydrogen bonds are especially strong dipoledipole interactions between molecules that have hydrogen bonded to a highly electronegative atom, such as O, N, or F. The resulting partially positively charged H atom on one molecule (the hydrogen bond donor) can interact strongly with a lone pair of electrons of a partially negatively charged O, N, or F atom on adjacent molecules (the hydrogen bond acceptor). 0000004997 00000 n
The normal boiling point (760 mm Hg) of diethyl ether is 35o C. What pressure does diethyl ether boil at 25o C? Using Grignard and organolithium reagents, Acidity of alcohols: formation of alkoxides. And you might have also noticed Hydrogen bond formation requires both a hydrogen bond donor and a hydrogen bond acceptor. What is a functional group in organic chemistry? %PDF-1.6
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Helium is nonpolar and by far the lightest, so it should have the lowest boiling point. The strength of the intermolecular forces in isopropyl alcohol are in between water and acetone, but probably closer to acetone because the water took much longer to evaporate. Asked for: order of increasing boiling points. Water's heat of vaporization is 41 kJ/mol. uc>fX1vYUx6K+*q%s\pI.K2eEeEeEdvdo;z9r= + 0000010401 00000 n
Did Billy Graham speak to Marilyn Monroe about Jesus? And you can literally take atoms away from that to get to a water. See all questions in Definition of 'Chemistry' and 'Organic'. If you're seeing this message, it means we're having trouble loading external resources on our website. WebAn atom or molecule can be temporarily polarized by a nearby species. Rubbing alcohol consists mainly of ethanol or isopropanol. Thanks to its -OH group, isopropyl alcohol molecules can form weak bonds, called hydrogen bonds, that help hold the molecules together. The strength of the intermolecular forces in isopropyl alcohol are in between water and acetone, but 1 What intermolecular forces does isopropyl alcohol have? I would put would be water, followed by, since ethanol at 20 degrees Celsius, it's lower than the boiling point of all of these characters. (i) is probably the most significant contributor, and it reduced by comparison with say, water, because there is only the one #""^(delta-)O-H^(delta+)# dipole in isopropanol. degrees Celsius while isopropyl has a lower boiling point. It's important to remember, however, that not all of the particles have the same velocities. Acetone and isopropyl alcohol have similar molar masses and both are polar compounds. London dispersion forces. Also to know, what kind of intermolecular forces are present in isopropyl alcohol? 6) Why will 3. Among the option, water has the The strength of the Ethanol has one oxygen-hydrogen bond. Fusion, vaporization, and sublimation are endothermic processes, whereas freezing, condensation, and deposition are exothermic processes. Because ice is less dense than liquid water, rivers, lakes, and oceans freeze from the top down. WebThe stronger the intermolecular force the greater the surface tension. deep into vapor pressure. 10: Solids, Liquids, and Phase Transitions, { "00:_Front_Matter" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "10.1:_Bulk_Properties_of_Liquids_-_Molecular_Interpretation" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "10.2:_Intermolecular_Forces_-_Origins_in_Molecular_Structure" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "10.3:_Intermolecular_Forces_in_Liquids" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "10.4:_Phase_Equilibrium" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "10.5:_Phase_Transitions" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "10.6:_Phase_Diagrams" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "10.E:_Solids_Liquids_and_Phase_Transitions_(Exercises)" : "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]()" }, { "09:_The_Gaseous_State" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "10:_Solids_Liquids_and_Phase_Transitions" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "11:_Solutions" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()" }, [ "article:topic", "intermolecular forces", "hydrogen bond", "showtoc:no", "license:ccbyncsa", "licenseversion:40" ], https://chem.libretexts.org/@app/auth/3/login?returnto=https%3A%2F%2Fchem.libretexts.org%2FBookshelves%2FGeneral_Chemistry%2FMap%253A_Principles_of_Modern_Chemistry_(Oxtoby_et_al. Methanol, ethanol, n-propyl alcohol, isopropyl alcohol, and t-butyl alcohol are all miscible with water. So we know that this is 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. Identify the intermolecular forces in each compound and then arrange the compounds according to the strength of those forces. If indium crystallizes in a face-centered unit cell, what is the length of an edge of the unit cell? The intermolecular forces that operates between isopropanol molecules are (i) hydrogen bonding, and (ii) dispersion forces between the alkyl residues. Imagine the implications for life on Earth if water boiled at 130C rather than 100C. ethanol as a tie for second. Log in Join. We know this because the Lewis Structure of the molecule only has one line of symmetry , and a molecule is polar if it has one or less line of symmetry. could view as a measure of the average kinetic We also acknowledge previous National Science Foundation support under grant numbers 1246120, 1525057, and 1413739. Isopropyl alcohol (IUPAC name propan-2-ol and also called isopropanol or 2-propanol) is a colorless, flammable chemical compound (chemical formula CH3CHOHCH3) with a strong odor. Over time all of the isopropyl alcohol boils away, half of the water boils, and none of the oil boils. Which of these has the strongest intermolecular forces? +x I would put methanol and All phase changes are accompanied by changes in the energy of a system. We use cookies to ensure that we give you the best experience on our website. (The amount of energy per mole that is required to break a given bond is called its bond energy.). 48366 views 0000004617 00000 n
Some are faster than others, which is why pressure is the average of all of the forces exerted on the surfaces by the gas particles. What is the difference between an intermolecular force and an intramolecular force? H\@w+fBzQy c)4})]0TIM~60?S?t_[h9s?$ya^)IpNcRU&)99I~8_Ii/~Mft$}moti{w}Xsi_>29jS}Q'~['FnBR;y9]X4znY-&hR~RDc?)IU^1x_=rvN5|K-UB@k!%,|I}-|I}-|I}-|I}-|ZZy//M5C)r!'kN9rt! KBr (1435C) > 2,4-dimethylheptane (132.9C) > CS2 (46.6C) > Cl2 (34.6C) > Ne (246C). Accessibility StatementFor more information contact us atinfo@libretexts.org. Excess thermodynamic and thermoacoustic parameters were discussed in terms of the difference in molecular structure and intermolecular forces between the components of the system. do we see this relationship? Im going back in a minute I need a little more help I have a lot to get to get to work but Im not sure what to say to. Are compounds that lower the surface tension between two liquids, between a gas and a. liquid, or between a liquid and a solid. WebA discussion and demonstration of intermolecular forces with examples of surface tension. 0.461 nm C. 0.029 nm D. 0.922 nm E. 0.115. ), The oxygen atom of the strongly polarized OH bond of an alcohol pulls electron density away from the hydrogen atom. won the tiebreaker, followed by ethanol, followed by methanol, and then the lowest boiling A primarily electrostatic force of attraction between a hydrogen atom which is covalently, bound to a more electronegative atom or group, and another electronegative atom, Is the tendency of liquid surfaces to shrink to the smallest possible surface area when they, are at rest. Capillary action is the phenomenon in which liquids rise up into a narrow tube called a capillary. Why does the dipole-dipole occur in isopropanol? 0000001993 00000 n
How is the strength of London dispersion forces related to the number of electrons? on boiling points, the highest boiling point The strength of the intermolecular forces in isopropyl alcohol are in between water and acetone, but probably closer to acetone because the water took much longer to evaporate. The thrice 11.2: Intermolecular Forces - Chemistry LibreTexts | Alcohol - Physical properties of alcohols 0000008329 00000 n
And I'm not going to go no you can tell by their boiling points. hydrogen bond contribution to the intermolecular forces, I would put water as number one 'cause it can form the (i) is probably 0000010720 00000 n
Isopropyl alcohol, like all alcohols, is polar. This molecule is polar. There are basically 3 - dipole/dipole, London Dispersion, and H-Bonds. WebIntermolecular Forces (IMF) and Solutions. Vapor pressure is inversely related to intermolecular forces, so those with stronger intermolecular forces have a lower vapor pressure. WebA liquids vapor pressure is directly related to the intermolecular forces present between its molecules. WebMethanol, ethanol, n-propyl alcohol, isopropyl alcohol, and t-butyl alcohol are all miscible with water. A liquids vapor pressure is directly related to the intermolecular forces present between its molecules. Solution. Direct link to Richard's post So Sal is looking at the , Posted a year ago. Dipoledipole interactions arise from the electrostatic interactions of the positive and negative ends of molecules with permanent dipole moments; their strength is proportional to the magnitude of the dipole moment and to 1/r6, where r is the distance between dipoles. Water has strong intermolecular forces (hydrogen bonds). this will keep happening where things go from liquid, Consequently, it has a much higher boiling and melting point than propane, which also contains three carbons and eight hydrogens. And it's clear that diethyl ether has the highest molar mass, followed by ethanol, followed by methanol, followed by water. What is the general formula of a carboxylic acid? Answers at Chapter 2 Practice Questions. Does the term "hydrogen bond" refer to the bond between the hydrogen and an atom in its own molecule or the attraction between the hydrogen and another molecule? have a lower vapor pressure when you get to that equilibrium. vapor pressure measures tendency of a liquid to evaporate. Isopropyl alcohol has stronger attrac-tive forces than acetone. And every now and then, they might approach the surface with the right kinetic energy, A. Isopropyl Alcohol C3H8O. on that on Khan Academy. 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. Intermolecular forces determine bulk properties such as the melting points of solids and the boiling points of liquids. intermolecular forces, more of the vapor is going to form, and so you're going to have A C60 molecule is nonpolar, but its molar mass is 720 g/mol, much greater than that of Ar or N2O. 0000004728 00000 n
Hydrogen bonds, with a strength of about 5 kilocalories (21 kilojoules) per mole, are much weaker than normal covalent bonds, with bond energies of about 70 to 110 kilocalories per mole. pressure gets high enough, remember, that pressure's just from the vapor molecules bouncing around, then you will get to some Acetone and isopropyl alcohol are both polar, so both have dipole-dipole interactions, which are stronger than dispersion forces. Water's high surface tension is due to the hydrogen bonding in water molecules. )%2F11%253A_Liquids_and_Intermolecular_Forces%2F11.S%253A_Liquids_and_Intermolecular_Forces_(Summary), \( \newcommand{\vecs}[1]{\overset { \scriptstyle \rightharpoonup} {\mathbf{#1}}}\) \( \newcommand{\vecd}[1]{\overset{-\!-\!\rightharpoonup}{\vphantom{a}\smash{#1}}} \)\(\newcommand{\id}{\mathrm{id}}\) \( \newcommand{\Span}{\mathrm{span}}\) \( \newcommand{\kernel}{\mathrm{null}\,}\) \( \newcommand{\range}{\mathrm{range}\,}\) \( \newcommand{\RealPart}{\mathrm{Re}}\) \( \newcommand{\ImaginaryPart}{\mathrm{Im}}\) \( \newcommand{\Argument}{\mathrm{Arg}}\) \( \newcommand{\norm}[1]{\| #1 \|}\) \( \newcommand{\inner}[2]{\langle #1, #2 \rangle}\) \( \newcommand{\Span}{\mathrm{span}}\) \(\newcommand{\id}{\mathrm{id}}\) \( \newcommand{\Span}{\mathrm{span}}\) \( \newcommand{\kernel}{\mathrm{null}\,}\) \( \newcommand{\range}{\mathrm{range}\,}\) \( \newcommand{\RealPart}{\mathrm{Re}}\) \( \newcommand{\ImaginaryPart}{\mathrm{Im}}\) \( \newcommand{\Argument}{\mathrm{Arg}}\) \( \newcommand{\norm}[1]{\| #1 \|}\) \( \newcommand{\inner}[2]{\langle #1, #2 \rangle}\) \( \newcommand{\Span}{\mathrm{span}}\)\(\newcommand{\AA}{\unicode[.8,0]{x212B}}\), 11.E: Liquids and Intermolecular Forces (Exercises), 11.1: A Molecular Comparison of Gases, Liquids, and Solids, 11.4.1 Energy Changes Accompanying Phase Changes, 11.5.1 Explaining Vapor Pressure on the Molecular Level, 11.5.2 Volatility, Vapor Pressure, and Temperature, 11.7.2 The Crystal structure of Sodium Chloride, assumes both the volume and shape of container is compressible diffusion within a gas occurs rapidly flows readily, Assumes the shape of the portion of the container it occupies Does not expand to fill container Is virtually incompressible Diffusion within a liquid occurs slowly Flows readily, Retains its own shape and volume Is virtually incompressible Diffusion within a solid occurs extremely slowly Does not flow, London dispersion, dipole-dipole forces, hydrogen bonds, Fairly soft, low to moderately high melting point, poor thermal and electrical conduction, Atoms connected in a network of covalent bonds, Very hard, very high melting point, often poor thermal and electrical conduction, Hard and brittle, high melting point, poor thermal and electrical conduction, Soft to very hard, low to very high melting point, excellent thermal and electrical conduction, malleable and ductile, average kinetic energy of the molecules is larger than average energy of attractions between molecules, lack of strong attractive forces allows gases to expand, attractive forces not strong enough to keep molecules from moving allowing liquids to hold shape of container, intermolecular forces hold molecules together and keep them from moving, crystalline solids with highly ordered structures, state of substance depends on balance between the kinetic energies of the particles and interparticle energies of attraction, kinetic energies depends on temperature and tend to keep particles apart and moving, interparticle attractions draw particles together, condensed phases liquids and solids because particles are close together compared to gases, increase temperature forces molecules to be closer together, intermolecular forces weaker than ionic or covalent bonds, many properties of liquids reflect strengths of intermolecular forces, three types of intermolecular forces: dipole-dipole forces, London dispersion forces, and hydrogen-bonding forces, less than 15% as strong as covalent or ionic bonds, electrostatic in nature, involves attractions between positive and negative species, Ion-Dipole Force exists between an ion and partial charge at one end of a polar molecule, magnitude of attraction increases as either the charge of ion or magnitude of dipole moment increases, dipole-dipole force exists between neutral polar molecules, effective only when polar molecules are very close together, for molecules of approximately equal mass and size, the strengths of intermolecular attractions increase with increasing polarity, interparticle forces that exist between nonpolar atoms or molecules, motion of electrons can create an instantaneous dipole moment, polarizability ease in which the charge distribution in a molecule can be distorted, larger molecules have greater polarizability, London dispersion forces increase with increasing molecular size, Dispersion forces increase in strength with increasing molecular weight, Molecular shape affects intermolecular attractions, dispersion forces operate between all molecules.
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