Laboratory Experimental Procedure Intramolecular forces are the forces that resu

Question

Laboratory Experimental Procedure Intramolecular forces are the forces that result from chemical bonds within an individual molecule. We've learned that these bonds can be covalent, ionic or metallic Intermolecular forces are forces that exist between molecules and are much weaker than intramolecular forces. The properties of matter result from the properties of the individual molecule (chemical bonding) but how the molecules act macroscopically result, in part, from intermolecular forces. Below is a summary of the forces we've learned this far in kilojoules of energy per mole. London dispersion forces are also called induced dipole-induced dipole forces. Model Attraction (kj/mol) Example Force Bonding Ionic Cation-anion 400-4000 NaCl Nuclei-shared Covalent 150-1100 H-H e pair Metallic Cations-delocalized 75-1000 Fee electrons Nonbonding (Intermolecular) Ion charge- lon-dipole 40-600 Na .....o dipole charge Polar bond to H 0-40 H bond -A-H "T dipole charge Chigh EN of N, O, F) Dipole-dipole Dipole charges 5-25 HCI I-Cl lon charge- 3-15 Fe? ....0, Ion-induced dipole polarizable e cloud Dipole-induced Dipole charge- H CI CI CI 2-10 dipole polarizable e cloud Polarizable e Dispersion 0.05-40 F-F....F-F (London) clouds

Explanation / Answer

Hexane is a non polar molecule and hence the type of interation with water is dispersion (London) interaction (the last one in the above table). These interactions are far weaker as compared with isoproponol (which also interacts by H-bonding). So the number of drops held by the penny will be very less, in fact even the first drop may fall off the penny.

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