Are hydrophobic interactions weak or strongSolutionHydrophobi.pdf

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Are hydrophobic interactions weak or strong? Solution Hydrophobic interactions describe the relations between water and hydrophobes (Low-water soluble molecule). Hydrophobes are non-polar molecules and usually have a long chain of carbon that do not interact with water molecules. Strength of hydrophobic bonds are relatively stronger than other weak intermolecular forces (i.e., Vander Waals forces and hydrogen bonds). The strength of hydrophobic interactions depends on several factors like: 1. Temperature: As the temperature increases, the strength of hydrophobic interaction also increases also. However, at extreme temperatures, hydrophobic interactions denature. 2. Number of carbons on hydrophobes: Molecules with greatest number of carbon atoms will have the strongest hydrophobic interactions. 3. The shape of hydrophobes: Aliphatic organic molecules will have stronger interactions than aromatic organic molecules..

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Intermolecular Forces are foces actingwithin a molecule. You should first note whehter the molecule is metallic, ionicor covalent. There are three different types of Intermolecular Forces thatapplies for covalent molecules: Dispersion force,Dipole-dipole interactions and hydrogen bonds. The relative strength of these forces are: dispersion forces< dipole-dipole interactions < hydrogen bonds Hence, dispersion forces are the weakest and hydrogen bondsare the strongest. Dispersion forces (aka. van der Waals Forceor London Force) are for non-polarmolecules.Non- polar molecules have no dipoles, or the dipoledoesn\'t extend throughout the molecule, and only dispersion forces.They are generally don\'t mix with water, and are usually anyelement and carbon compounds. For example:Cl2,CO2,N2O4,CH4 Dipole-Dipole forces occur between moleculesthat have permanent net dipoles, (hencepolar molecules) Polar molecules usually have a dipole and may contain a highlyelectronegative element bonded to hydrogen, allowing hydrogenbonding. They are also usually soluble in water. For example: SCl2 , PCl3,CH3Cl Hydrogen Bonds occur between molecules thathave permanent net dipole resulting from hydrogen beingcovalently bonded to either fluorine, oxygen ornitrogen. For example: HF, H2O, H2O2 ,CH3OH, CH3COOH,CH3NH2 These forces operate between covalentmolecules. As for your answer, Na+: Dispersion H3C-CH3: Dispersion K2O : Ionic Bond H2O: Hydrogen bonding, the hydrogen has a verylow electronegativety resulting in the oxygen atoms having greateraffinity to the covalently shared electrons. NH3 : polar, hence dipole-dipole and hydrogenbonding, since the hydrogen is slightly +ve and the nitrogenslightly -ve. There more electronegative nitrogen pulls thehydrogen electron towards it, giving a dipole moment . Ne: non polar, hence dispersion forces only(randomness of electron clouds instantaneously causes oppositecharges at the ends of the molecule which induces the same effectin another) If you want to learn more, this site might help: http://science.uwaterloo.ca/~cchieh/cact/c123/intermol.html Solution Intermolecular Forces are foces actingwithin a molecule. You should first note whehter the molecule is metallic, ionicor covalent. There are three different types of Intermolecular Forces thatapplies for covalent molecules: Dispersion force,Dipole-dipole interactions and hydrogen bonds. The relative strength of these forces are: dispersion forces< dipole-dipole interactions < hydrogen bonds Hence, dispersion forces are the weakest and hydrogen bondsare the strongest. Dispersion forces (aka. van der Waals Forceor London Force) are for non-polarmolecules.Non- polar molecules have no dipoles, or the dipoledoesn\'t extend throughout the molecule, and only dispersion forces.They are generally don\'t mix with water, and are usually anyelement and carbon compounds. For example:Cl2,CO2,N2O4,CH4 Dipole-Dipole forces occur between moleculesthat have permanent net dipoles, (hencepolar molecu.

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