3-D image of Acetone

CH3COCH3

Legend:

Red- Oxygen

Black- Carbon

Silver- Hydrogen

Note: The arrows signify the different electronegativity values of each element in the molecule and point to the atom which has a greater electronegativity value. An electronegativty value is the tendency for an atom to attract other electrons towards itself. For example, Oxygen, which has a negativity value of 3.6, is more negative than Carbon, which has a negativity value of 2.6, so the arrow points towards the Oxygen atom.

Electronegativity Values:

Oxygen- 3.6

Carbon- 2.6

Hydrogen- 2.2

Is Acetone a Polar or Non-Polar Molecule?

First off, the definition of a Polar Molecule is, the molecule has a difference in the negativity between the atoms and the definition of a Non-Polar Molecule is, the molecule has an equal negativity between the atoms. According to the negativity values stated above, there is a difference with both the Oxygen to Carbon bond and the Carbon to Hydrogen bonds. This difference leads to the conclusion that Acetone is indeed a Polar Molecule!



Math:



Oxygen (3.6)-Carbon (2.6)= Difference (1.0)



Carbon (2.6)-Hydrogen(2.2)= Difference (0.4)



Another way to discover if this molecule is Polar or Non-Polar is by seeing if there is an imbalance in electron distribution. Oxygen naturally has 2 unshared pairs of electrons because of the 6 valence electrons. Because Carbon and Hydrogen do not have any unshared pairs of electrons due to the 4 valence and 1 valence electron, there is an imbalance in the electron distribution. Therefore, Acetone is a Polar Molecule!

What Forces Would Keep 2 Acetone Molecules Together?

Forces:


London Dispersion Force: The weakest intermolecular force which is a temporary attraction that happens when the electrons of 2 adjacent atoms form temporary dipoles due to the movement of electrons around the 2 atoms. This force is present in both Polar and Non-Polar molecules.


Dipole Dipole: An attraction between the postive dipole of one atom with the negative dipole of the other atom. In other words, the dipoles are attracted like the negative side of a magnet is attracted to the positive side of another magnet. Unlike London Dispersion Forces, this type of attraction is only present in Polar molecules.


Hydrogen Bond: A special type of Dipole Dipole where temporary covalent bonds are established between a Hydrogen atom of one molecule and a Fluorine, Oxygen, or Nitrogen atom of the other same molecule.


The Forces Acting on Acetone


The forces that are acting on Acetone are all three; London Dispersion Forces, Dipole Dipole, and Hydrogen Bonding. London Dispersion Forces are acting on this molecule because they act on every molecule, Dipole Dipole is acting on this molecule because the molecule is Polar and finally Hydrogen Bonding is acting on the molecule because a Hydrogen atom of one molecule can bond with the Oxygen atom of the second molecule. This is shown below:

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