What is the strongest type of intermolecular force between solute and solvent in

Question

What is the strongest type of intermolecular force between solute and solvent in each of the following solutions? Explain.

a. C6H14(l) in C8H18 (l)

b. H2C=O in CH3OH (l)

c. Br2 (l) in CCl4 (l)

Please explain.

Explanation / Answer

a. is london forces b. is hydrogen bonding c. is london forces INTRAmolecular, INTER is at end of this. ionic>hydrogen>dipole-dipole>london dispersion forces. an ionic bond is easy to spot, involved a metal and a nonmetal ex: NaCl hydrogen bonding occurs between hydrogen and nitrogen, oxygen, and fluorine only. ex: H2O, HF, etc. Dipole dipole bonding is a bit harder, you have to create a lewis-dot diagram for the substance. If there are any extra electrons on one of the atoms in the diagram, then this is it. This is because when molecules of these compounds are near each other, the electrons will repel each other, and one side will become a bit more positive/negative than the other, creating an attraction with the opposite side of other nearby molecules. London dispersion forces (LDF) are caused by instantaneously induced dipoles. when it is not any of the aforementioned causes, this is it. The reasoning behind this is that the molecule will at some time completely randomly while moving will have its electrons shifted over to one side, creating a negative charge on that side, and a positive charge on the other side. this makes a weaker dipole-dipole like attraction. Or if you were looking for bond numbers, the higher the bond number, the stronger the bond because there is more attraction (this is intermolecular) Bond number is simply how many bonds are between 2 atoms in a molecule

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