State the kind of intermolecular forces that would occur between the solute and solvent in barium nitrate (ionic).

Check all that apply.

ion-dipole
hydrogen bonding
dispersion
dipole-dipole

ion-dipole and dispersion

dispersion

In order to determine the type of intermolecular forces that occur between the solute (barium nitrate) and the solvent, it is important to consider the nature of the compounds involved. Barium nitrate is an ionic compound, meaning it is composed of positively charged ions (cations) and negatively charged ions (anions).

When barium nitrate dissolves in a solvent, such as water, the solvent molecules (in this case, water molecules) interact with the ions of the solute. The type of intermolecular forces that occur between the solute and the solvent depend on the charges and partial charges present.

Based on this information, the intermolecular forces that can occur between the solute (barium nitrate) and the solvent include:

1. Ion-dipole forces: Since barium nitrate contains ions (Ba2+ and NO3-) and the solvent is a polar molecule (such as water), ion-dipole forces can occur. The positive end of the polar water molecule (dipole) is attracted to the negatively charged nitrate ions, while the negative end of the water molecule is attracted to the positively charged barium ions.

2. Dipole-dipole forces: If the solvent is also a polar molecule, dipole-dipole forces can occur. In this case, the dipoles of the solvent molecules can interact with one another and with the ions of the solute.

3. Dispersion forces: Dispersion forces, also known as London forces or Van der Waals forces, can occur between any type of molecules, including ionic compounds like barium nitrate. However, dispersion forces are generally weaker compared to ion-dipole and dipole-dipole forces. These forces arise from temporary fluctuations in electron distributions, creating temporary dipoles in molecules or ions.

Hydrogen bonding, however, is not a likely intermolecular force between barium nitrate (ionic) and a solvent, as hydrogen bonding tends to occur between molecules that contain hydrogen bonded directly to highly electronegative elements such as oxygen, nitrogen, or fluorine. Barium nitrate does not fulfill this condition.

In summary, the intermolecular forces that would occur between barium nitrate and a solvent include ion-dipole forces, dipole-dipole forces, and dispersion forces. Hydrogen bonding is not applicable in this case.

I would look at a, c(slight with anything almost), and d.