Molecule Name : Pentachlorophenol Formula :C6HCl5O
What is C6HCl5O?
C6HCl5O Is a chemical compound known as Pentachlorophenol or PCP and is used as a disinfectant. The molecule is made up of Chlorine, Hydrogen, Oxygen and Carbon. Below are diagrams showing what the molecule looks like in 3d, Lewis Structure and the Dash Structure. Also it shows its polarity, covalent bonds and forces of attraction.
3D Model of C6HCl5O :
The black lines outlining the carbon molecule represent the 6 carbons.
Key:
Lewis Structure of C6HCl5O
Dash Structure of C6HCl5O
and angle degree between molecules :
- When you find the difference between the two molecules if it is between 0-1.7 it is covalent. If it is from 1.7- it is ionic. The closer to 0 the bond becomes more covalent anything above 1.7 makes the bond ionic.
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| This demonstrates the bond between chlorine and Carbon. The difference between the two is .9 making it moderately covalent |
This demonstrates the bond between Oxygen and hydrogen. The difference is 1.3 making it somewhat covalent.
This demonstrates the bond between Oxygen and Chlorine. The difference was .3 making it very covalent.
Polarity refers to a separation of Electric charge between two molecules . In this molecule Chlorine and Oxygen both have negative charges. Hydrogen however has a positive charge. Therefore because not al of the charges in the molecule are the same C6HCl5O is polar.
Cl- Cl-
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Cl- - C -Cl-
/ |
Cl- O- -H+
Intermolecular Forces
In a sitchuation where two molecules of C6HCl5O ( PCP) became attracted to each other what Intermolecular forces would be diplayed?
The arrows point the dots which represent dipole-dipole and the line that represents hydrogen bonding.
In this molecule the Intermolecular forces represented are London Dispersion, Dipole-Dipole and Hydrogen bonding.
- London Dispersion is found at all molecule attractions. Dispersion forces occur because a temporary pole is formed through motion and an uneven amount of electrons distributed.
- Dipole - Dipole forces occur because a positive end of one polar molecule and the negative end of another polar molecule attract. ( this is demonstrated though the dots between O and H . O is negative and H is positive.)
- Hydrogen bonding is a type of hydrogen bonding. Here it is the bond between the hydrogen atom and the oxygen atom. ( In other cases it can also be between N or F. It is represented as a straight line. )
The blog looks very nice. I really like the background and the way the words are white with black behind it. The ad is very appealing. I do no think the molecule is accurately drawn. C6HCl5O should have 6 carbon atoms, but the pictures only have 1 atom of carbon. CHCl5O is accurately drawn and described by correctly describing its polarity and forces.
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ReplyDeleteThe background of this blog looks chemistry-related and the colors make it very aesthetically appealing. The bold black background with white letting really makes the text stand out. Only one carbon is shown in the drawings (six should be shown for C6HCl5O). Despite this, the "C" (representing carbon) is often larger than the other atoms in the above images and could be representing the ring of carbons present in this molecule (this ring would be difficult to type out on a computer). The arrows showing electronegativity seem to be drawn correctly and the bond angles (shown in the second image) look great. It is correct that C6HCl5O is a polar molecule. It is also correct that london, dipole dipole (because of polarity), and hydrogen bonding (because of the hydrogen and oxygen atoms) would occur in between two pentachlorophenol molecules. I like the ad (posted on anther page) because it is convincing and includes a picture incorporating the molecule's practical use.
ReplyDeleteThankss Guys ! :) I just realized my mistake with the carbon and fixed it by making the carbon six sided as represented in the image above it
ReplyDeleteThe background is great, it ties in with the uses of your molecule. I like the many different models that you have drawn for the molecule, especially the that clearly shows the bond angles. I also like the many different pictures used to gradually go over the nature of the bonds, it makes it a lot easier on the eyes than if it were all jumbled together. I also like the picture that clearly proves the different intermolecular forces in your molecule. (Also, not to sound annoying but I wanted to let you know there is a typo in the forth sentence under polarity.)
ReplyDeleteThanks dan your the man !
ReplyDeleteThe blog's appearence is very nice. The black background with contrasting white text makes the text easy to read. The multiple pictures help the viewer to easily understand what is being described. Your descriptions clearly state what is happening in each picture, and all information seemed to be acurate.
ReplyDeletethank you so much
ReplyDeleteit is very useful