What intermolecular force exists between the CH3CH2CH3 , CH4 , or the "CH3CH2"
end of the ethanol molecule and the water molecules?
A. dipole-dipole forces
B. hydrogen bonding
C. London Dispersion forces
D. no intermolecular interaction exists
its C....because these molecule are nonpolar so the are LDF exist here
I would go with C.
The alkanes mostly have dispersion forces acting among them,,so CH4 is dispersion forces as well as for c3h8 and c2h5 is ethyl which likean alkane..
To determine the intermolecular force between the given molecules, we need to consider their molecular structures and the types of attractive forces that could be present.
In the case of CH3CH2CH3, also known as propane, its structure consists of only carbon and hydrogen atoms. It does not have an electronegative atom (such as oxygen or nitrogen) that can create a permanent dipole moment. As a result, there are no significant dipole-dipole interactions or hydrogen bonding interactions between propane and water molecules. However, London Dispersion forces can still occur. These forces are the result of temporary fluctuations in electron distribution that induce temporary dipoles, causing neighboring molecules to be attracted to each other.
For CH4, also known as methane, it has a tetrahedral structure with four hydrogen atoms surrounding a central carbon atom. The carbon-hydrogen bonds in methane are non-polar, so there are no permanent dipole moments in the molecule. Hence, there are no dipole-dipole interactions or hydrogen bonding between methane and water molecules. However, like propane, methane can still exhibit London Dispersion forces.
Now, for the "CH3CH2" end of the ethanol molecule, ethanol (C2H5OH) has an -OH functional group, which gives rise to a polar covalent bond between the oxygen and hydrogen atoms. This polar bond results in a permanent dipole moment in the molecule, allowing it to form both dipole-dipole interactions and hydrogen bonding with water molecules.
In summary, the intermolecular force that exists between water molecules and the CH3CH2 end of the ethanol molecule is hydrogen bonding (choice B). The intermolecular forces between water molecules and CH3CH2CH3 or CH4 are London Dispersion forces (choice C).