Essay On Intermolecular Forces
Intramolecular and intermolecular forces are arising from electrostatic attraction between opposite charges. Bonding forces are due to the attraction between cations and anions (ionic bonding), nuclei and electron pairs (covalent bonding), or metal cations and delocalized valence electrons (metallic bonding). Intermolecular forces, on the other hand, are due to attraction between molecules as a result of partial charges, or the attraction between ions and molecules. The two types of forces differ in magnitude, and coulomb’s law explains why:
• Bonding forces are relatively strong because they involve larger charges that are closer together.
• Intermolecular forces are relatively weak because they typically involve small charges that are farther apart.
How far apart are the charges between molecules that give rise to intermolecular forces? Consider Cl2 as an example. When we measure the distance between two Cl nuclei in a sample of solid Cl2, we obtain two different values. The shorter distance is between two bonded Cl atoms in the same molecule. It is, as you know, called the bond
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The most important atoms are Nitrogen, Oxygen and Fluorine. The H-N, H-O, and H-F bonds are very polar, so electron density is withdrawn from H. As a result, the partially positive H of one molecule is attracted to the partially negative lone pair on the Nitrogen, Oxygen or Fluorine of another molecule, and a hydrogen bond (H bond) forms. Hydrogen bonding is especially important in aqueous solution. It is a primary factor in the solubility in water and thus cell fluid of many oxygen and nitrogen containing organic and biological compounds, such as alcohols, sugars, amines and amino acids. Oxygen and Nitrogen are small and electronegative, so their bound H atoms are partially positive and can get very close to the Oxygen of water
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