Intermolecular+forces

Jona Tyrell Fox​ This page is here so i can descibe the influence of intermolecular forces on the physical properties of covalent compounds.
 * Why is this page is here. **

Intermolecular forces are the forces that hold molecules together.
 * What is an intermolecular force? **

There is Hydrogen Bonding, which is the strongest type of intermolecular force, dipole attraction which is the second strongest type of intermolecular force, and London dispersion which is the weakest type of intermolecular force. Hydrogen bonding can be thought of as a chain holding two objects together. It can be thought of this way because of the strength of the attraction. Dipole attraction can be thought of as a rope holding two objects together. It can be thought of this way because it is a strong attraction just not as strong as a hydrogen bond.London dispersion can be thought of as a man being hit in the face with a soccer ball. It can be thought of this way because the man's face and the soccer ball have no real attraction to each other but they eventually deveolp a temporary attraction and meet. After they meet they continue moving in their own direction.
 * What are the types of forces and how can i remember them? **



Since Hydrogen Bonding is such a strong intermolecular force, and the molecules of the compound are held together so strongly that it takes alot of energy to break these bonds resulting in very high melting points, very high heat of vaporation, and a high surface tension. It does not take very cold temperatures to freeze it because the molecules are already so close together that it takes alot less time to get them together and to stop moving. This has finally helped me realize how the lizard that i saw run across the water, on the discovery channel, was able to do it. Since the surface tension of water was so high it was able to move quickly on the water and not fall in.
 * How can these forces have any effect on a substance? **

Dipole attration is essentially the same as hydrogen bonding because the bond is also strong just not as strong as hydrogen bonding, so compounds with dipole attraction have high melting points, high heat of evaporation, and high surface temperature, just not as high as hydrogen bonding. It needs colder temperatures to freeze because since the molecules are farther apart it takes more to get them colser together.

The last of the intermolecular forces is almost the opposite of hydrogen bonding. Because of its almost zero attraction to other molecules they are not held together tightly at all so it takes less energy to do things to it. It has a low melting point, low heat of evaporation, and low surface tension,"Molecules" Yet it needs very cold temperatures to freeze it because its molecules are spread so far apart that it takes extreme cold to get the molecules together and to stop moving.

Many people get Intra and Intermolecular forces confused. There is a huge difference. Intermolecular forces are how the molecules themselves stick to each other, but intramolecular bonds are how the elements inside of the molecules attract each others electrons.
 * A common misunderstanding. **

The intermolecular bond that hold water molecules together is extremely important in our community. If water molecules were not held together by a hydrogen bond then the bond would be too easily broken so it would be much easier for the water on our planet to evaporated. Also it would need to be much colder for water to freeze, so ice would be hard to find. **A close connection to Physics.** Intermolecular forces is closely related to physics because physics is the study of matter and its motion through space and time, and I think that physicists probably need to know what type of bonds molecules have before they can begin to measure how certain compounds can possibly move.
 * How this effects our community? **

"Molecules." __Science of Everyday Things__. Ed. Neil Schlager. Vol. 1: //Real-Life Chemistry//. Detroit: Gale, 2002. 8 pp. 4 vols. __Gale Virtual Reference Library__. Gale. Patrick F Taylor Science & Tech Academy. 13 Nov. 2009 .
 * Work Cited **

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