Answer:
The order of relative magnitude of intermolecular forces is:
Ion-ion forces> Ion-dipole forces> Hydrogen bonds> Dipole-dipole forces> London Dispersion Forces
Explanation:
Electronegativity is defined as the ability of an element to attract the electrons that link it to another element.
The covalent bond (chemical bond between atoms where electrons are shared, forming a molecule. This bond is established between non-metallic elements) between two atoms can be polar or nonpolar.
When two atoms have different electronegativities, the one with the highest electronegativity will attract the electrons towards each other, giving rise to two opposite charges on the bond. That is, this generates that in a polar molecule there is separation between positive and negative charges. The bonds will be all the more polar the greater the difference in electronegativity between the bound atoms.
On the other hand, the non-polar covalent bond occurs between atoms of the same element or between atoms with very little electronegativity difference. It is thus characterized to molecules or bonds that do not exhibit any polarity.
Intermolecular forces or junctions are those interactions that hold the molecules together. They are electrostatic forces.
Van der Waals forces are weak attractions that hold electrically neutral molecules together. At some point these molecules have an induced dipole, that is, the molecule acquires a partially positive and a partially negative charge momentarily, causing them to attract each other. They are Van de Waals forces: Dipolo - Dipolo forces, London forces, Ion forces - Dipolo.
- London Dispersion Forces: occurs between non-polar molecules due to the movement of electrons. At some point there are more electrons to one side, which, being close to another atom or molecule, the electrons of the second are repelled, originating two instantaneous dipoles, which give rise to a force of attraction. In summary, this type of force occurs because when two molecules approach, a distortion of the electronic clouds of both originates, generating in them, transient induced dipoles, due to the movement of the electrons, so that they allow them to interact with each other. They are very weak forces.
- Ion-ion forces: It is the attraction between two ions of different charge: cations (ion with positive charge) and anions (ion with negative charge). That is, it occurs between different charged molecules that will tend to form an electrostatic junction between the ends of opposite charges due to the attraction between them.
- Ion-dipole forces: they are attractive forces between an ion (an atom that has lost or gained an electron, then it has a charge) and a polar molecule. A molecule is a dipole when there is an asymmetric distribution of electrons because the molecule is made up of atoms of different electronegativity. Then, the ion binds to the part of the molecule that has its opposite charge: the positive end of the polar molecule is oriented towards the anion (ion with negative charge) and the negative end of the polar molecule is oriented towards the cation ( ion with positive charge).
- Dipole-dipole forces: the dipole-dipole forces are forces of attraction between polar molecules. These molecules attract when the positive end of one of them is close to the negative of the other.
- Hydrogen bonds: they are a type of dipole-dipole force. In this interaction a molecule that has hydrogen interacts, with another that has an atom with a high electronegativity, such as oxygen, fluorine or nitrogen (O, F, N). In this way, between the hydrogen, which has a low electronegativity and the electronegative atom, an interaction is established, due to its opposite charges.
<u><em>The order of relative magnitude of intermolecular forces is:
</em></u>
<u><em>Ion-ion forces> Ion-dipole forces> Hydrogen bonds> Dipole-dipole forces> London Dispersion Forces</em></u>
