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Intermolecular forces and solubility Why mixtures mix Consider a glass of wine. Why do alcohol, water, & pigment mix together? There must be attractive.

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Presentation on theme: "Intermolecular forces and solubility Why mixtures mix Consider a glass of wine. Why do alcohol, water, & pigment mix together? There must be attractive."— Presentation transcript:

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2 Intermolecular forces and solubility

3 Why mixtures mix Consider a glass of wine. Why do alcohol, water, & pigment mix together? There must be attractive forces. Intramolecular forces occur between atoms Intermolecular forces occur between molecules The factors that determine solubility are the strength of IMFs and speed of molecules. 4 types of intermolecular forces: ionic, dipole- dipole, hydrogen bonding, and London forces.

4 Electronegativity & IMFs EN essentially defines the type of IMF. Ionic bonds form if the EN is 1.7 or greater. Dipole-dipole (polar covalent) is around Hydrogen bonding is a type of dipole-dipole. London forces exist in all molecules, but are especially important in non-polar covalent molecules (where EN is less than 0.5). Recall that ionic are strongest. Dipole-dipole are not as strong. – + + – + – + – + – + – Hydrogen bonds are about five times stronger than regular dipole-dipole bonds. London forces are weakest.

5 Hydrogen bonding H-bonding is a special type of dipole-dipole attraction that is very strong. It occurs when N, O, or F are bonded to H. Q- Calculate the EN for HCl and H 2 O The high EN of NH, OH, and HF bonds cause these to be strong forces. Also, because of the small size of hydrogen, its positive charge can get very close to the negative dipole of another molecule. It is so strongly positive that it will sometimes exert a pull on a lone pair in a non-polar compound O H H O H H HCl: EN = = 0.9 H 2 O: = 3.5 – 2.1 = 1.4

6 London forces Non-polar molecules do not have dipoles like polar molecules. How, then, can non-polar compounds form solids or liquids? London forces result from a type of tiny dipole. These forces exist between all molecules. They are masked by stronger forces (e.g. dipole-dipole) so are sometimes insignificant, but they are important in non-polar molecules. Because electrons are moving around in atoms there will be instants when the charge around an atom is not symmetrical. The resulting tiny dipoles result in attractions between atoms and/or molecules.

7 London forces Instantaneous dipole:Induced dipole: Eventually electrons are situated so that tiny dipoles form A dipole forms in one atom or molecule, inducing a dipole in the other

8 Why oil and water dont mix + – + + – + + – + + – + + – + + – + + – + + – + + – + The non-polar substance is pushed away. If it were moving faster it might break through the attractive forces. Solubility is a balance be- tween speed and attraction. Also, the more similar the strength of their dipoles the more likely two compounds are to mix.

9 Solubility is influenced by temperature. In warmer water, more solid will dissolve. This is because a high temperature means H 2 O molecules are moving faster (keeping more solid molecules suspended). Temperature and Solubility Conversely a gas will be less soluble at a higher temperature. This is because when gas molecules are moving faster they are able to escape from the liquid surface. Think of cold soda vs. warm soda. Warm soda goes flat faster.

10 Across 1.Muriatic acid 5.London 10.Intermolecular 16.Solvent 17.Heterogeneous 18.Latin 20.Mixtures 21.Compounds 23.Lone pair 24.Polar 25.Solubility 26.Bronze Answers 2.Intramolecular 3.Alloy 4.Air 6.Opaque 7.All 8.Electrolyte 9.Solute 11.NOF 12.Solution 13.Homogeneous 14.Water 15.Dissociation 19.Nonpolar 22.Four For more lessons, visit


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