3D picture of H2O2

The arrows represent the electronegativity of the hydrogen; less than the oxygen. 

Polar or Nonpolar?

Hydrogen Peroxide is polar. 

A polar molecule is a molecule that has an uneven distribution of electrons, therefore its charge is unevenly distributed.

The electrons in the oxygen of the molecule are more negative. This is found through the electronegativity table in which it states that Oxygen has an electronegativity of 3.5. Hydrogen has an electronegativity of 2.2. [[The larger the number, the more negative the element is.]]  Therefore, the negatives and positives form the uneven distribution of electrons, making the molecule polar, even though the O-O bond is nonpolar because of the equal distribution of electrons. 


-*Another way to determine polarity is through drawing lines of symmetry. To be symmetrical, the line drawn must cut the molecule in "half", or in other words, you are able to see a mirror image. If 0 or only 1 line of symmetry can be drawn through the drawing (Lewis Structure) of the molecule, then it is polar. If 2 or more lines of symmetry can be drawn, then the molecule is nonpolar.

Influential Intermolecular Forces

There are 3 intermolecular forces that are keeping the molecules attracted: 

1.                  London Dispersion Forces

2.                    Dipole-Dipole 

3.                    Hydrogen Bonding 

-* How?

London Dispersion Forces- the force of attraction between all molecules (any two at one time), created by temporary dipoles, which are caused by the movement of electrons around two atoms. 

So, London Dispersion has an effect on all molecules, and these temporary dipoles are the temporary shift in electrons as they change their positions. London Dispersion Forces are very weak, easy to pull nonpolar from nonpolar.

Dipole-Dipole-  an electrostatic attraction caused by the positive end of one dipole being attracted to the negative end of another dipole. 

 Dipole-Dipole is asymmetrical, and applies to hydrogen peroxide because it is a polar molecule. Discussed in the polarity post is the requirements of being a polar molecule. The basic idea that the uneven distribution of electrons proves dipole-dipole to be true in that the positives attract the negatives and vice versa.

Hydrogen Bonding- a special case of dipole-dipole attraction where a temporary covalent bond forms between the hydrogen molecule, and the O,N,F of an adjacent molecule. 

Hydrogen Bonding is applicable to hydrogen peroxide through the simplicity of O and H being attracted to each other, forming a bond. 

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