London Dispersion Force- a very temporary, uneven distribution of electrons, creating a temporary dipole. It forms a week bond between two molecules.
Dipole-Dipole- an electrostatic attraction between the negative side of one molecule and the positive end of the other molecule. In the Methanol molecule there is a dipole-dipole force between the oxygen of one molecule and hydrogen of another. It is represented by a doted line.
Hydrogen Force-a special type of dipole-dipole that forms a temporary covalent bond. A hydrogen bond forms between hydrogen and oxygen, hydrogen and nitrogen, or hydrogen and fluorine. In Methane it forms between the hydrogen of one molecule and the oxygen of another molecule. It is represented by a solid line.
Methanol has all three types of forces.
Great job explaining exactly what each force is and where it is seen with Methane.
ReplyDeleteThis blog is a very helpful blog to learn about methanol. Great job drawing the molecule's picture. The arrows are all pointing from teh atom with the lower electronegativity value to the atom with the higher value, with the picture even showing the valence electrons. The statement that the molecule is polar is also correct. The forces are described in good detail. The ad was very convincing and very direct in what methanol can be used for.
ReplyDeleteKatie, you explained the intermolecular forces very well. You stated what each force was and how methanol had it. The descriptions are very detailed.
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