The dot structure for phosgene starts with the C atom in the center. Video Discussing London/Dispersion Intermolecular Forces. Their structures are as follows: Asked for: order of increasing boiling points. Electrostatic interactions are strongest for an ionic compound, so we expect NaCl to have the highest boiling point. Examples range from simple molecules like CH3NH2 (methylamine) to large molecules like proteins and DNA. Low concentrations may be . Step 5: Before we can confirm our Lewis Structure diagram to be the correct one, we have to check two concepts first. Identify the most significant intermolecular force in each substance. Like covalent and ionic bonds, intermolecular interactions are the sum of both attractive and repulsive components. New York: Mcgraw Hill, 2003. The hydrogen is attached directly to a highly electronegative atoms, causing the hydrogen to acquire a highly positive charge. Inter molecular forces are the attractions between molecules, which determine many of the physical properties of a substance. This prevents the hydrogen atom from acquiring the partial positive charge needed to hydrogen bond with the lone electron pair in another molecule. 3rd ed. At zero degrees, there is an double bonded oxygen. Considering CH3OH, C2H6, Xe, and (CH3)3N, which can form hydrogen bonds with themselves? Since the hydrogen donor (N, O, or F) is strongly electronegative, it pulls the covalently bonded electron pair closer to its nucleus, and away from the hydrogen atom. When the radii of two atoms differ greatly or are large, their nuclei cannot achieve close proximity when they interact, resulting in a weak interaction. NH3 - nh3 intermolecular forces has dipole dipole intraction and hydrogen bonding and London dispersion forces, hydrogen bonding is more strongest then van der wale forces, the parial positive end of one molecules to the partial negative end of another molecules. The hydrogen bonding is limited by the fact that there is only one hydrogen in each ethanol molecule with sufficient + charge. E represents the unbonded or lone pair on the central atom. However complicated the negative ion, there will always be lone pairs that the hydrogen atoms from the water molecules can hydrogen bond to. Imagine the implications for life on Earth if water boiled at 130C rather than 100C. The properties of liquids are intermediate between those of gases and solids, but are more similar to solids. Intermolecular forces are electrostatic in nature and include van der Waals forces and hydrogen bonds. Intramolecular hydrogen bonds are those which occur within one single molecule. Petrucci, et al. of around 8.3 0C. The below reaction shows the process of formation of COCl2 from CO and Cl2: What are the intermoleular forces in Cl2CO? The four compounds are alkanes and nonpolar, so London dispersion forces are the only important intermolecular forces. In contrast, the energy of the interaction of two dipoles is proportional to 1/r3, so doubling the distance between the dipoles decreases the strength of the interaction by 23, or 8-fold. The one compound that can act as a hydrogen bond donor, methanol (CH3OH), contains both a hydrogen atom attached to O (making it a hydrogen bond donor) and two lone pairs of electrons on O (making it a hydrogen bond acceptor); methanol can thus form hydrogen bonds by acting as either a hydrogen bond donor or a hydrogen bond acceptor. The electronic configuration of the central atom, here C is 1s2 2s2 2p2 (atomic number of C is 6), that of Chlorine is 1s2 2s2 2p6 3s2 3p5 ( atomic no = 17), The electronic configuration of O: 1s2 2s2 2p4 ( atomic no = 8). dimethyl sulfoxide (boiling point = 189.9C) > ethyl methyl sulfide (boiling point = 67C) > 2-methylbutane (boiling point = 27.8C) > carbon tetrafluoride (boiling point = 128C). It is important to realize that hydrogen bonding exists in addition to van der Waals attractions. 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 \(\PageIndex{2}\)). Legal. Accessibility StatementFor more information contact us atinfo@libretexts.org. Phosgene can also be used to separate ores. As a result, it is relatively easy to temporarily deform the electron distribution to generate an instantaneous or induced dipole. 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. 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. an Ion and (B.) The He-, Ne-, and Ar-Phosgene Intermolecular Potential Energy Surfaces The J. Phys. Arrange 2,4-dimethylheptane, Ne, CS2, Cl2, and KBr in order of decreasing boiling points. Although hydrogen bonds are significantly weaker than covalent bonds, with typical dissociation energies of only 1525 kJ/mol, they have a significant influence on the physical properties of a compound. Hydrogen bonding cannot occur without significant electronegativity differences between hydrogen and the atom it is bonded to. Your email address will not be published. The values indicate that all the elements are having the least possible formal charges within the phosgene molecular structure that we have drawn. His research entails the study of intermolecular forces and dynamics, intramolecular energy flow, high-field effects in molecular spectroscopy, and the vibrational spectroscopy of free radicals. COCl2 has carbon as the central atom It has three surrounding atoms: one of oxygen and two of chlorine and no lone pair. Because the boiling points of nonpolar substances increase rapidly with molecular mass, C60 should boil at a higher temperature than the other nonionic substances. Severe respiratory effects, including pulmonary edema, pulmonary emphysema, and death have been reported in humans. Dipole-dipole interactions Since the vessel is relatively small, the attraction of the water to the cellulose wall creates a sort of capillary tube that allows for capillary action. Draw the hydrogen-bonded structures. Comparing the two alcohols (containing -OH groups), both boiling points are high because of the additional hydrogen bonding; however, the values are not the same. If a double bond is there, there will be both and pairs. Exposure to phosgene may cause irritation to the eyes, dry burning throat, vomiting, cough, foamy sputum, breathing difficulty, and chest pain; and when liquid: frostbite. at 90 and 270 degrees there are singly bonded Cl atoms. Phosgene 75-44-5 Hazard Summary Phosgene is used as a chemical intermediate; in the past, it was used as a chemical warfare agent. The major intermolecular forces include dipole-dipole interaction, hydrogen . This is the expected trend in nonpolar molecules, for which London dispersion forces are the exclusive intermolecular forces. 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. Step 1: The initial step is to calculate the valence or outermost shell electrons in a molecule of COCl2. The electron geometry for the Phosgene is also provided.The ideal bond angle for the Phosgene is 120 since it has a Trigonal planer molecular geometry. The intermolecular forces are ionic for CoCl2 cobalt chloride. It doesn't go that far, but the attraction is significantly stronger than an ordinary dipole-dipole interaction. AOs are arranged in order of their increasing energies following the Aufbau principle and the Madelung rule. 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. Source: Dipole Intermolecular Force, YouTube(opens in new window) [youtu.be]. 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. Intermolecular forces (IMFs) occur between molecules. The electric dipoles do not get canceled out. Phosgene is acyl chloride. Compare the molar masses and the polarities of the compounds. Xe is liquid at atmospheric pressure and 120 K, whereas Ar is a gas. The substance with the weakest forces will have the lowest boiling point. This, without taking hydrogen bonds into account, is due to greater dispersion forces (see Interactions Between Nonpolar Molecules). 1. Check all that apply. We have included topics like Lewis Structure, VSEPR theory from which we can predict Molecular Geometry, Orbital Hybridization, and Polarity. Explosive release results in formation of a white cloud. Techiescientist is a Science Blog for students, parents, and teachers. Save my name, email, and website in this browser for the next time I comment. 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. 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. On average, however, the attractive interactions dominate. Compounds such as HF can form only two hydrogen bonds at a time as can, on average, pure liquid NH3. Compounds with higher molar masses and that are polar will have the highest boiling points. Furthermore, hydrogen bonding can create a long chain of water molecules, which can overcome the force of gravity and travel up to the high altitudes of leaves. Constituent atoms are distanced far away from each other in a molecule in order to minimize these repulsive forces. COCl2 (Phosgene) Molecular Geometry, Bond Angles (and Electron Geometry) Wayne Breslyn 632K subscribers 10K views 1 year ago An explanation of the molecular geometry for the COCl2 (Phosgene). Check all that Identify the types of intermolecular forces present in sulfur dioxide SO2. Formal charge for O atom = 6 *4 4 = 0. Hydrogen bonds are are generally stronger than ordinary dipole-dipole and dispersion forces, but weaker than true covalent and ionic bonds. Previous problem problem 2:59m Watch next 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. Here, activated porous carbon acts as the catalyst. valenbraca Answer: Phosgene has a higher boiling point. Required fields are marked *. Intermolecular forces are electrostatic in nature; that is, they arise from the interaction between positively and negatively charged species. London was able to show with quantum mechanics that the attractive energy between molecules due to temporary dipoleinduced dipole interactions falls off as 1/r6. In order for a hydrogen bond to occur there must be both a hydrogen donor and an acceptor present. As shown in part (a) in Figure \(\PageIndex{3}\), the instantaneous dipole moment on one atom can interact with the electrons in an adjacent atom, pulling them toward the positive end of the instantaneous dipole or repelling them from the negative end. The bond angle of C-Cl bonds is around 111.8 degrees ( less than 120 degrees due to C=O electron density that reduces the bond angle). Substances capable of forming hydrogen bonds tend to have a higher viscosity than those that do not form hydrogen bonds. The substance with the weakest forces will have the lowest boiling point. It is the 3-dimensional atomic arrangement that gives us the orientation of atomic elements inside a molecular structural composition. For example, Xe boils at 108.1C, whereas He boils at 269C. We will arrange them according to the bond formation and keeping in mind the total count. 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. Types of intramolecular forces of attraction Ionic bond: This bond is formed by the complete transfer of valence electron (s) between atoms. For example, intermolecular hydrogen bonds can occur between NH3 molecules alone, between H2O molecules alone, or between NH3 and H2O molecules. Master Intermolecular Forces & Physical Properties Concept 1 with a bite sized video explanation from Jules Bruno. Determine the intermolecular forces in the compounds, and then arrange the compounds according to the strength of those forces. Expert Answer 100% (4 ratings) The intermolecular forces present in propane C3H8 are London dispersion forces. Like covalent and ionic bonds, intermolecular interactions are the sum of both attractive and repulsive components. It only has six electrons surrounding its atom. Answer: a) n-butane has a higher boiling point b) 1-butanol has a higher boiling Explanation: Given the molecules, propane (C3H8) and n-butane (C4H10), n-butane has a higher boiling point mainly due to greater molar mass and longer chain (more interactions between each molecule). It has a boiling point (b.p.) However, ethanol has a hydrogen atom attached directly to an oxygen; here the oxygen still has two lone pairs like a water molecule. Thus far, we have considered only interactions between polar molecules. It is used to manufacture precursors for herbicide production and used to manufacture pharmaceuticals and pesticides. Neopentane is almost spherical, with a small surface area for intermolecular interactions, whereas n-pentane has an extended conformation that enables it to come into close contact with other n-pentane molecules. If you plot the boiling points of the compounds of the group 14 elements with hydrogen, you find that the boiling points increase as you go down the group. What kind of attractive forces can exist between nonpolar molecules or atoms? b. Dipole-dipole bonding. 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. If you are interested in the bonding in hydrated positive ions, you could follow this link to co-ordinate (dative covalent) bonding. It, therefore, has 4 valence electrons. Video Discussing Dipole Intermolecular Forces. Arrange n-butane, propane, 2-methylpropane [isobutene, (CH3)2CHCH3], and n-pentane in order of increasing boiling points. The higher boiling point of the butan-1-ol is due to the additional hydrogen bonding. In tertiary protein structure, interactions are primarily between functional R groups of a polypeptide chain; one such interaction is called a hydrophobic interaction. Molecules with hydrogen bonds will always have higher boiling points than similarly sized molecules which don't have an -O-H or an -N-H group. Source: Hydrogen Bonding Intermolecular Force, YouTube(opens in new window) [youtu.be]. Intermolecular forces. Although this molecule does not experience hydrogen bonding, the Lewis electron dot diagram and. Electrons are subatomic particles that make up a negatively charged cloud atmosphere around the nuclei. However, the double bond seems to act much like a nonbonding pair of electrons, reducing the ClCCl bond angle from 120 to 111. Similarly, solids melt when the molecules acquire enough thermal energy to overcome the intermolecular forces that lock them into place in the solid. 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. In phosgene, the overall dipole moment of the molecule is weakened. 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. { "Dipole-Dipole_Interactions" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", Dipole_Moment : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", Dipole_moments : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", Hydrogen_Bonding : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "Ion_-_Dipole_Interactions" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "Ion_-_Induced_Dipole_Interactions" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "Ion_-_Ion_Interactions" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "Lennard-Jones_Potential" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", Polarizability : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", Van_Der_Waals_Interactions : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()" }, { Hydrogen_Bonding : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", Hydrophobic_Interactions : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", Multipole_Expansion : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", Overview_of_Intermolecular_Forces : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", Specific_Interactions : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", Van_der_Waals_Forces : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()" }, [ "article:topic", "hydrogen bonding", "showtoc:no", "license:ccbyncsa", "licenseversion:40", "author@Jim Clark", "author@Jose Pietri" ], https://chem.libretexts.org/@app/auth/3/login?returnto=https%3A%2F%2Fchem.libretexts.org%2FBookshelves%2FPhysical_and_Theoretical_Chemistry_Textbook_Maps%2FSupplemental_Modules_(Physical_and_Theoretical_Chemistry)%2FPhysical_Properties_of_Matter%2FAtomic_and_Molecular_Properties%2FIntermolecular_Forces%2FSpecific_Interactions%2FHydrogen_Bonding, \( \newcommand{\vecs}[1]{\overset { \scriptstyle \rightharpoonup} {\mathbf{#1}}}\) \( \newcommand{\vecd}[1]{\overset{-\!-\!\rightharpoonup}{\vphantom{a}\smash{#1}}} \)\(\newcommand{\id}{\mathrm{id}}\) \( \newcommand{\Span}{\mathrm{span}}\) \( \newcommand{\kernel}{\mathrm{null}\,}\) \( \newcommand{\range}{\mathrm{range}\,}\) \( \newcommand{\RealPart}{\mathrm{Re}}\) \( \newcommand{\ImaginaryPart}{\mathrm{Im}}\) \( \newcommand{\Argument}{\mathrm{Arg}}\) \( \newcommand{\norm}[1]{\| #1 \|}\) \( \newcommand{\inner}[2]{\langle #1, #2 \rangle}\) \( \newcommand{\Span}{\mathrm{span}}\) \(\newcommand{\id}{\mathrm{id}}\) \( \newcommand{\Span}{\mathrm{span}}\) \( \newcommand{\kernel}{\mathrm{null}\,}\) \( \newcommand{\range}{\mathrm{range}\,}\) \( \newcommand{\RealPart}{\mathrm{Re}}\) \( \newcommand{\ImaginaryPart}{\mathrm{Im}}\) \( \newcommand{\Argument}{\mathrm{Arg}}\) \( \newcommand{\norm}[1]{\| #1 \|}\) \( \newcommand{\inner}[2]{\langle #1, #2 \rangle}\) \( \newcommand{\Span}{\mathrm{span}}\)\(\newcommand{\AA}{\unicode[.8,0]{x212B}}\), More complex examples of hydrogen bonding, Hydrogen bonding in organic molecules containing nitrogen, methoxymethane (without hydrogen bonding). Larger molecules have more space for electron distribution and thus more possibilities for an instantaneous dipole moment. 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. Argon and N2O have very similar molar masses (40 and 44 g/mol, respectively), but N2O is polar while Ar is not. Intermolecular forces are forces that exist between molecules. 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. In water, two hydrogen bonds and two lone pairs allow formation of hydrogen bond interactions in a lattice of water molecules. In addition, the attractive interaction between dipoles falls off much more rapidly with increasing distance than do the ionion interactions. 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 \(\PageIndex{6}\). Water is an ideal example of hydrogen bonding. So, in this reason we can say that, NH3 has both forces such as, dipole dipole interaction, and hydrogen bonding, and also . Because a hydrogen atom is so small, these dipoles can also approach one another more closely than most other dipoles. 12.7: Types of Crystalline Solids- Molecular, Ionic, and Atomic, 2-methylpropane < ethyl methyl ether < acetone, 1.4: The Scientific Method: How Chemists Think, Chapter 2: Measurement and Problem Solving, 2.2: Scientific Notation: Writing Large and Small Numbers, 2.3: Significant Figures: Writing Numbers to Reflect Precision, 2.6: Problem Solving and Unit Conversions, 2.7: Solving Multistep Conversion Problems, 2.10: Numerical Problem-Solving Strategies and the Solution Map, 2.E: Measurement and Problem Solving (Exercises), 3.3: Classifying Matter According to Its State: Solid, Liquid, and Gas, 3.4: Classifying Matter According to Its Composition, 3.5: Differences in Matter: Physical and Chemical Properties, 3.6: Changes in Matter: Physical and Chemical Changes, 3.7: Conservation of Mass: There is No New Matter, 3.9: Energy and Chemical and Physical Change, 3.10: Temperature: Random Motion of Molecules and Atoms, 3.12: Energy and Heat Capacity Calculations, 4.4: The Properties of Protons, Neutrons, and Electrons, 4.5: Elements: Defined by Their Numbers of Protons, 4.6: Looking for Patterns: The Periodic Law and the Periodic Table, 4.8: Isotopes: When the Number of Neutrons Varies, 4.9: Atomic Mass: The Average Mass of an Elements Atoms, 5.2: Compounds Display Constant Composition, 5.3: Chemical Formulas: How to Represent Compounds, 5.4: A Molecular View of Elements and Compounds, 5.5: Writing Formulas for Ionic Compounds, 5.11: Formula Mass: The Mass of a Molecule or Formula Unit, 6.5: Chemical Formulas as Conversion Factors, 6.6: Mass Percent Composition of Compounds, 6.7: Mass Percent Composition from a Chemical Formula, 6.8: Calculating Empirical Formulas for Compounds, 6.9: Calculating Molecular Formulas for Compounds, 7.1: Grade School Volcanoes, Automobiles, and Laundry Detergents, 7.4: How to Write Balanced Chemical Equations, 7.5: Aqueous Solutions and Solubility: Compounds Dissolved in Water, 7.6: Precipitation Reactions: Reactions in Aqueous Solution That Form a Solid, 7.7: Writing Chemical Equations for Reactions in Solution: Molecular, Complete Ionic, and Net Ionic Equations, 7.8: AcidBase and Gas Evolution Reactions, Chapter 8: Quantities in Chemical Reactions, 8.1: Climate Change: Too Much Carbon Dioxide, 8.3: Making Molecules: Mole-to-Mole Conversions, 8.4: Making Molecules: Mass-to-Mass Conversions, 8.5: Limiting Reactant, Theoretical Yield, and Percent Yield, 8.6: Limiting Reactant, Theoretical Yield, and Percent Yield from Initial Masses of Reactants, 8.7: Enthalpy: A Measure of the Heat Evolved or Absorbed in a Reaction, Chapter 9: Electrons in Atoms and the Periodic Table, 9.1: Blimps, Balloons, and Models of the Atom, 9.5: The Quantum-Mechanical Model: Atoms with Orbitals, 9.6: Quantum-Mechanical Orbitals and Electron Configurations, 9.7: Electron Configurations and the Periodic Table, 9.8: The Explanatory Power of the Quantum-Mechanical Model, 9.9: Periodic Trends: Atomic Size, Ionization Energy, and Metallic Character, 10.2: Representing Valence Electrons with Dots, 10.3: Lewis Structures of Ionic Compounds: Electrons Transferred, 10.4: Covalent Lewis Structures: Electrons Shared, 10.5: Writing Lewis Structures for Covalent Compounds, 10.6: Resonance: Equivalent Lewis Structures for the Same Molecule, 10.8: Electronegativity and Polarity: Why Oil and Water Dont Mix, 11.2: Kinetic Molecular Theory: A Model for Gases, 11.3: Pressure: The Result of Constant Molecular Collisions, 11.5: Charless Law: Volume and Temperature, 11.6: Gay-Lussac's Law: Temperature and Pressure, 11.7: The Combined Gas Law: Pressure, Volume, and Temperature, 11.9: The Ideal Gas Law: Pressure, Volume, Temperature, and Moles, 11.10: Mixtures of Gases: Why Deep-Sea Divers Breathe a Mixture of Helium and Oxygen, Chapter 12: Liquids, Solids, and Intermolecular Forces, 12.3: Intermolecular Forces in Action: Surface Tension and Viscosity, 12.6: Types of Intermolecular Forces: Dispersion, DipoleDipole, Hydrogen Bonding, and Ion-Dipole, 12.7: Types of Crystalline Solids: Molecular, Ionic, and Atomic, 13.3: Solutions of Solids Dissolved in Water: How to Make Rock Candy, 13.4: Solutions of Gases in Water: How Soda Pop Gets Its Fizz, 13.5: Solution Concentration: Mass Percent, 13.9: Freezing Point Depression and Boiling Point Elevation: Making Water Freeze Colder and Boil Hotter, 13.10: Osmosis: Why Drinking Salt Water Causes Dehydration, 14.1: Sour Patch Kids and International Spy Movies, 14.4: Molecular Definitions of Acids and Bases, 14.6: AcidBase Titration: A Way to Quantify the Amount of Acid or Base in a Solution, 14.9: The pH and pOH Scales: Ways to Express Acidity and Basicity, 14.10: Buffers: Solutions That Resist pH Change, 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).