Paper Example on Intermolecular Force

Introduction

Molecules are classified into polar and non-polar molecules based on their general appearance and structure. In some instances, molecules may appear to be in between the two classifications, but this only occurs on rare occasions. Additionally, molecules may undergo chemical bonding whenever they share some of their electrons within the atom to form an orbit. Some orbits and shells enable atoms to have an equal distribution of electrons. A polar molecule, therefore, can be described as one which has an even distribution of electrons which produce positive charges one side and negative charges on the other side. On the other hand, a non-polar molecule is described as one which has a systematic flow of electron distribution and does not have any excess charges produced on either of the sides. However, these intermolecular forces have different effects on melting and boiling points, energy and evaporation, and sweating as discussed below.

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The polar and non-polar molecules affect melting and boiling points in various ways. For instance, an element with non-polar molecules causes a substance to have a high boiling and melting point. It is also critical to consider the strength and stability of an element's intermolecular force before making conclusions based on their effect on the melting and boiling points of a substance. An example is that ionic and metallic bonds display high melting and boiling points because they have non-polar molecules which exhibit a strong intermolecular force. This is because the bonds found with such substances are strong and robust and therefore they tend to affect a substance by raising its boiling and melting point since it is more bonded. This means that a substance whose bond is weak is likely to have a lower boiling and melting point because its intermolecular forces are not strong enough to hold the molecules together.

A higher intensity of intermolecular forces signifies a slower generation of energy and evaporation rate. The positive and negative charges found in polar and non-polar molecules align together to form an attraction which enables the holding of polar liquid more. It, therefore, signifies that the more polar liquids are held together, the slower their rate of evaporation. Additionally, molecules which are held together tightly by the intermolecular forces means that they will have enough energy (kinetic) to separate from each other and therefore they will lead to slow evaporation. On the contrary, polar and non-polar molecules which are loosely held together will have a faster separation rate because they require only little kinetic energy to separate themselves.

A higher intermolecular force of non-polar and polar molecules portrays a higher rate of sweating. This is because the charges present in the molecules generate a lot of heat which enables sweating to occur at a faster rate. Also, intermolecular forces that are strong within molecules allow a quicker rate of sweating because molecules generate a lot of heat as they struggle to separate from each other. On the other side, weak intermolecular forces allow molecules to separate easily as they use minimal energy and therefore this causes slower sweating.

Conclusion

In conclusion, the intermolecular forces between polar and non-polar molecules affect evaporation and energy, melting and boiling point and sweating in different ways. All this depends on the amount of kinetic energy that is required to break the forces and loosen the molecules. Hence, a stronger intermolecular force causes a high melting and boiling point, slower evaporation and higher sweating rates of a substance.