I have to write the exact lewis electron dot structure for para xylene C8H10. I tried writing it out but it doesnt work out proerly. C is supposed to have 31 electrons and H is supposed to have 10 totaling 42. i was doing research and it says that it is aromatic and i tried to do it as a ring like structure but i have 2 H left over and nowhere to put them. I also tried putting the Cs all in a line and I have Cs sitting there with a couple electrons not paired up. I also tried rearrranging the Cs and i would still have 1 electron sitting alone in 4 spots. arent they supposed to be paired up? please help me!
I suspect you aren't adding the alternating double bonds. Here is a site that should help you.
http://chemistry.about.com/od/factsstructures/ig/Chemical-Structures---X/Xylene.-0VC.htm
To determine the Lewis electron dot structure for para-xylene (C8H10), let's first count the total number of valence electrons.
The molecular formula C8H10 tells us that carbon (C) is present in the compound and there are 8 carbon atoms. Each carbon atom contributes 4 valence electrons (it belongs to group 14).
The formula also indicates the presence of hydrogen (H) atoms, with a total of 10. Each hydrogen atom contributes 1 valence electron (it belongs to group 1).
Therefore, the total number of valence electrons is:
(8 carbon atoms × 4 electrons) + (10 hydrogen atoms × 1 electron) = 32 + 10 = 42 electrons
To distribute these electrons in the Lewis electron dot structure, follow these steps:
1. Start by connecting the carbon atoms in a chain. Since para-xylene has 8 carbon atoms, represent them in a straight line.
C-C-C-C-C-C-C-C
2. Place the remaining electrons around the carbon atoms. Begin by adding pairs of electrons around each carbon atom to fulfill the octet rule. Each carbon atom should have 4 valence electrons around it (except for the terminal carbon atoms, which will have fewer connections).
3. Distribute the remaining electrons as lone pairs to fulfill the octet rule for carbon and hydrogen atoms, ensuring that all the electrons are used.
At this point, if you have extra valence electrons, place them on the terminal carbon atoms. Each carbon atom should have enough valence electrons to fulfill the octet rule.
Remember that hydrogen atoms only require 2 valence electrons to complete their duet rule.
Please note that it's difficult to illustrate the exact Lewis electron dot structure here, but this should provide a general guide on how to construct it. It's also important to consider that the actual molecule may have resonance structures due to its aromaticity.
To draw the Lewis electron dot structure for para xylene (C8H10), we need to determine the total number of valence electrons.
Carbon (C) has 4 valence electrons, and there are 8 carbon atoms in para xylene. Hydrogen (H) has only 1 valence electron, and there are 10 hydrogen atoms. So, the total number of valence electrons is:
(4 valence electrons/C) * (8 C atoms) + (1 valence electron/H) * (10 H atoms) = 32 + 10 = 42 valence electrons.
Now, let's draw the Lewis structure for para xylene step-by-step:
1. Start with a carbon atom in the center and place the other 7 carbon atoms around it to form a ring.
C C C C C C C
\ | | | | /
C C
2. Add the hydrogen atoms to complete the structure. Each carbon atom should have 4 bonds (either to other carbon atoms or hydrogen atoms) to satisfy the octet rule.
H H H H H
| | | | |
C C C C C
\ | | /
C
Note that each carbon atom is now connected to 4 other atoms, and each hydrogen atom is connected to 1 carbon atom. All atoms in the structure have satisfied the octet rule.
Remember that in Lewis structures, it's not necessary to pair up all electrons. Unpaired electrons (often called radical electrons) are allowed in some cases, as long as all atoms have valence electrons.
Lastly, para xylene is considered aromatic because it fulfills the criteria for aromaticity, such as having a fully conjugated ring of π electrons.