Hydrazine

N2H4 is an inorganic chemical compound. It is a colorless flammable liquid that is derived from the same manufacture as ammonia.

Above is a three dimensional model of the molecule N2H4. The arrows depict the the natural flow of polarity from the lower energy level to the higher energy level. The white represents the Hydrogen atoms while the blue represents the nitrogen atoms

Polarity Energies:

H	N
2.2	3.0

As shown in the model above, the arrow goes from the lower electronegativity level, the Hydrogen, to the higer level, the Nitrogen.

N	N
3.0	3.0

In the model above there is no arrow between the Nitrogen because the bond between them is absolutely covalent, meaning the energy can not go from the lower to the higher, so it is balanced.

Polarity

Polarity

Every molecule is depicted as either polar or nonpolar. These terms just mean whether or not a molecule has an even distribution of electrons throughout. Polar means that there is an uneven distribution of electrons throughout the molecule. For example the molecule H2O is a polar molecule due to the excess electrons that are not being used by the Hydrogen. Nonpolar means that there is an even distribution of electrons throughout the molecule. This means that the hydrogen have a more positive charge while the Oxygen has a more negative charge. ClF4 is an example of a molecule that has an even distribution of electrons as although they have unused electrons, every single Fluorine has six unused electrons. This means that no atom is more negative than any other.

Hydrazine, N2H4, is a polar molecule. This is because it has an uneven distribution of electrons in the molecule.

The dash model above shows that although each of the four hydrogen have an even distribution, the two nitrogens do not. The Nitrogens originally contained five electrons, and the Hydrogen only one electron. So, pairing off the single hydrogen electron to one of the single nitrogen electron, a single pair of nitrogen electrons is left over. Each has a pair of electrons that are not being used, causing the uneven distribution. This causes the Hydrogen to be slightly positive where as the Nitrogen has a slightly negative charge.

Intermolecular Forces of Attraction

Intermolecular Forces of Attraction

Intermolecular forces of attraction are the forces of attraction that exist between molecules. Every molecule has some force of attraction when attached to another molecule. The three forces of attraction are: London Dispersion forces, Dipole-Dipole forces and Hydrogen Bonding.

London Dispersion Forces:
The force of attraction between any two molecules created by temporary dipoles which are caused by the movement of electrons both atoms.


Dipole Dipole Forces:
Electrostatic attraction caused by the positive end of one dipole being attracted to the negative end of another dipole.


Hydrogen Bonding:
Special case of dipole dipole attraction where a temporary covalent bond forms between hydrogen of one molecule and the oxygen, nitrogen or fluorine of an adjacent molecule.

All molecules attracted to another molecule have London Dispersion forces whether they be polar or nonpolar. However, the polarity of a molecule decides whether they have Dipole Dipole and/ or Hydrogen Bonding. If a pair of molecules are polar than they will have Dipole Dipole and possibly Hydrogen Bonding if there is an hydrogen on one molecule and an oxygen, nitrogen or fluorine on another molecule. But, if one molecule is nonpolar and the other is polar they will only have London Dispersion.

Hydrazine's Forces of Attraction:

N2H4 happens to have all three forces of attraction, London Dispersion, Dipole-Dipole, Hydrogen bonding:

Above is dash structure with the forces shown as well as some of the charges. As shown the slightly positive hydrogen is attracted to the slightly negative nitrogen. Both Hydrogen Bonding and Dipole Dipole forces occur between these two elements. The top bond shows the temporary covalent bond that forms and then breaks between the nitrogen and hydrogen. The bottom shows the attraction of a positive to a negative which just happens to also be the nitrogen and hydrogen. The London Dispersion forces, although there, can not be shown by any sort of symbol, they just occur randomly around the molecules.

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HYDRAZINE

A small undistinguished chemical that can do more than you would have ever thought

Do you like safety? Do you like the moon? Then get some Hydrazine!

This very inorganic chemical compound may have a colorless liquid appearance, but it can do a lot. It is used in things like rocket fuel, so without this little guy we wouldn’t be on the moon, and it is used as a fuel for the ejection of air bags. With this chemical you could save a life or maybe go to the moon! It also is the major power source for several planes like the F-16 Fighting Falcon.

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The production of spandex fibers!

 

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**However, be warned this chemical is a bit hazardous and quite toxic, so use it with care!