Sunday, February 27, 2011
Forces of Attraction
With this molecule, CH2CCl2, if it came across another CH2CCl2, there would be a dipole-dipole attraction and london dispersion forces.
Dipole-Dipole- An electrostatic attraction between the poitive end of a dipole and the negative end of another dipole. This could occur with the Cl (negative) of one molecule and the H (positive) of the other molecule.
London Dispersion Forces- A weak force of attraction between two molecules created by temporary dipoles caused by elections moving around two atoms. This happens among all molecules that come across each other because the electrons are constantly moving.
If CH2CCl2 were to come across another molecule such as HF, there would be hydrogen bonding.
Hydrogen Bonding- A special case of dipole-dipole where a temporary covalent bond occurs between a hydrogen of one molecule and a Oxygen, Nitrogen or Fluorine of another molecule. One Hydrogen from CH2CCl2 would be attracted to the Fluorine of the HF. The F would switch constantly between the H of CH2CCl2 and the H of HF.
Dipole-Dipole- An electrostatic attraction between the poitive end of a dipole and the negative end of another dipole. This could occur with the Cl (negative) of one molecule and the H (positive) of the other molecule.
London Dispersion Forces- A weak force of attraction between two molecules created by temporary dipoles caused by elections moving around two atoms. This happens among all molecules that come across each other because the electrons are constantly moving.
If CH2CCl2 were to come across another molecule such as HF, there would be hydrogen bonding.
Hydrogen Bonding- A special case of dipole-dipole where a temporary covalent bond occurs between a hydrogen of one molecule and a Oxygen, Nitrogen or Fluorine of another molecule. One Hydrogen from CH2CCl2 would be attracted to the Fluorine of the HF. The F would switch constantly between the H of CH2CCl2 and the H of HF.
Electronegativity
C-----H
2.5 - 2.2 = .3
Very Covalent
C-----C
2.5 - 2.5 = 0.0
Absolutely Covalent
Cl-----C
3.2 - 2.5 = .7
Moderately Covalent
2.5 - 2.2 = .3
Very Covalent
C-----C
2.5 - 2.5 = 0.0
Absolutely Covalent
Cl-----C
3.2 - 2.5 = .7
Moderately Covalent
Model
CH2CCl2
Here, you can see there is no central atom. Therefore, this is a linear structure and the bond angles are 180°.
There is a double bond between the two Carbon atoms, a single bond between the Carbon and Hydrogen, and a single bond between the Carbon and Chlorine. Since the Hydrogen side of the molecule is positively charged and the Chlorine side is negatively charged, the molecule is POLAR.
There is a double bond between the two Carbon atoms, a single bond between the Carbon and Hydrogen, and a single bond between the Carbon and Chlorine. Since the Hydrogen side of the molecule is positively charged and the Chlorine side is negatively charged, the molecule is POLAR.
You need some Vinylidene chloride (VDC)!
Great for use by doctors!
-VDC will help you create X-ray films, even photograph films as well!
Great for taking down your enemy!
-It is colorless but an extremely strong odor! They will never see it coming!
-It could cause eye, skin, and even throat irritation.
-Let the enemy inhale it. This molecule will cause kidney and liver problems!
-If all of this fails, set it on fire! It is extremely flammable when in liquid form!
It is always nice to have some VDC available. You never know when it could be handy.
Pick up your container of VDC at a lab. You will not find this at your local drug store.
-VDC will help you create X-ray films, even photograph films as well!
Great for taking down your enemy!
-It is colorless but an extremely strong odor! They will never see it coming!
-It could cause eye, skin, and even throat irritation.
-Let the enemy inhale it. This molecule will cause kidney and liver problems!
-If all of this fails, set it on fire! It is extremely flammable when in liquid form!
It is always nice to have some VDC available. You never know when it could be handy.
Pick up your container of VDC at a lab. You will not find this at your local drug store.
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