| Intermolecular Force |
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DESCRIPTION AND STRENGTH These are fundamentally Electrostatic interactions (ionic interactions, hydrogen bond, dipole-dipole interactions) or Electrodynamic interactions (van der Waals/London forces). Electrostatic interactions are Classically described by Coulomb's Law ; the basic difference between them is the strength of their charge. Ionic interactions are the strongest with integer level charges, hydrogen bonds have partial charges that are about an order of magnitude weaker, and dipole-dipole interactions also come from partial charges another order of magnitude weaker. Ionic interactions These are interactions that occur between charged species ( Ion s). Like charges repel, while opposite charges attract. These bonds form when the Electronegativities between two atoms are large enough that one steals an electron from the other. The now oppositely charged ions are attracted. Ionic compounds have high melting and boiling points due to the large amount of heat required to break the forces between the charged ions. When molten they are also good conductors of heat and electricity, due to free or delocalised electrons. Hydrogen bonding ) and can interact with another highly electronegative atom in an adjacent molecule (again N, O, or F). This results in a stabilizing interaction that binds the two molecules together. An important example is Water : δ+ δ- δ+ H O - H \ / |
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