What intermolecular forces can occur between a CO3
ion and H2O molecules? List them

The molecule of water and carbonate has consisted of hydrogen bonding, dipole interaction, and London dispersive force.

The intermolecular force has been defined as the attractive force that has been present within the molecules in between the atoms. The interaction between the molecules has been mediated by the difference in the electronegativities and the dipole interaction.

The bonding of hydrogen atoms with more electronegative elements results in the hydrogen bond. In both the molecules hydrogen has been bonded with the oxygen atom, thus there has been the presence of hydrogen bonding.

The interactions between carbon and oxygen has resulted in the dipole, thus there has been dipole interaction with the molecule. The force of attraction between the ion and dipole has been the London dispersive force.

Thus, the molecule of water and carbonate has consisted of hydrogen bonding, dipole interaction, and London dispersive force.

For more information about the intermolecular force, refer to the link:

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The intermolecular forces between CO3^2- and H2O molecules are;

1) London dispersion forces

2) ion-dipole interaction

3) hydrogen bonding

Explanation:

Intermolecular forces are forces of attraction that exits between molecules. These forces are weaker in comparison to the intramolecular forces, such as the covalent or ionic bonds between atoms in a molecule.

Considering CO3^2- and H2O, we must remember that hydrogen bonds occur whenever hydrogen is bonded to a highly electronegative atom such as oxygen. The carbonate ion is a hydrogen bond acceptor.

Also, the London dispersion forces are present in all molecules and is the first intermolecular interaction in molecular substance. Lastly, ion-dipole interactions exists between water and the carbonate ion.

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this chemical reaction releases energy in the form of light and heat. chemical energy is the potential energy stored in the arrangement of atoms within molecules. breaking chemical bonds requires energy, while forming new chemical bonds releases energy.

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