Please tell me if I\'m wrong. 1) CH3COONa = dipole dipole 2) NH3 = London disper
ID: 762079 • Letter: P
Question
Please tell me if I'm wrong. 1) CH3COONa = dipole dipole 2) NH3 = London dispersion force 3) Ch3ch2ch2ch2ch3 = london dispersion force 4) h20 = hydrogen bonding 5) CH3OH = HYDROGEN bonding ( dipole dipole ) 6) (CH3)2 CO - LONDON DISPERSIONExplanation / Answer
1The CH3COONa catalyst was finally recovered through the reaction ..... employed, a3 can be stabilized by the dipole–dipole interactions between solvent 2Both have highly electropositive H and electronegative N and F elements. Polarity of these elements gives rise to London-Dispersion, and a dipole-dipole interaction. and obviously coz of H hydrogen bonding it there. viscosity and surface tension are both related to intermolecular forces (IMFs) 3pentane is nonpolar and cannot H-bond, so only LDF is possible (London Dispersion Force) pentanal is polar, but cannot H-bond => (Dipole-Dipole) pentanol has an OH group, so it can H-bond => (Hydrogen Bonding) With higher IMFs, you get greater surface tension and greater viscosity (since the liquid molecules are more attracted to each other) In order of decreasing IMF: (and thus decreasing viscosity/surface tension) pentanol pentanal pentane 4Yes, H20 is an example of Hydrogen bonding. Hydrogen bonds are weak bonds that connect hydrogen atoms to nitrogen, oxygen, or fluorine atoms. The oxygen atom in water has two hydrogen bonds, one to each of the two hydrogen atoms. 5 I2 - dispersion forces only CH3OH - H-bonding, dipole-dipole and dispersion I2 to CH3OH - dispersion only I2 has no dipole so it cannot form dipole-dipole interactions. It has no small electronegative atom (i.e. F,O,N) so it cannot form hydrogen bonds. It does however, form fairly srong dispersion forces as the electron density in iodine is easily polarised by neighbouring molecules, especially if they have a dipole (like CH3OH) 6When you say: "dipole-dipole,London dispersion, ionic, hydrogen bonding", these terms represent the intermolecular forces, not intramolecular forces. That is, the forces which holds the species together in the condensed form (liquid or solid state). As you know in gaseous state particles are free to move and there is no attractive forces between them according to the kinetic molecular theory.