U have to show the partial charges and bond dipoles on my ;lewis structure of CH3Cl
For the partial charges would I just have a negetive sign as the superscript of Cl and a positive sign and the superscript of C ?
What exactly must I do to show bond dipoles?
I didn't know that such things were included on a lewis structure.
Often they are not included. If you can envision CH3Cl as something like this:
H3C--Cl, then place a small Greek letter, delta (small, not a capital delta which is a triangle) together with a - sign. Then on the H3C end place a delta + sign.
what does the delta mean?
It means a partial negative charge or a partial positive charge. Placing a - sign or a + sign (with no small delta in front of either) means you are assigning a full -1 charge (or a -2 or -3 or any other number yu place there) to that atom or end of the molecule. The partial means part of a negative or positive charge but doesn't designate the quantity; thus, the quantity for a partial + or - charge can be anywhere from just over 0 up to but just under -1 (or +1).
Thank you :)
Scroll down to the delta (you will see the cap and the small letter).
http://www.mathacademy.com/pr/prime/articles/greek/index.asp
To show the partial charges on a Lewis structure of CH3Cl, you need to consider the electronegativity difference between the atoms. Electronegativity is a measure of an atom's ability to attract electrons towards itself in a chemical bond. Higher electronegativity values indicate a stronger attraction for electrons.
In the case of CH3Cl, carbon (C) has a lower electronegativity than chlorine (Cl). Therefore, chlorine will have a partial negative charge (δ-) while carbon will have a partial positive charge (δ+) in order to indicate the unequal sharing of electrons in the bond. However, it is important to note that the magnitude of these partial charges can vary depending on the specific electronegativity values of the atoms involved and the molecular environment.
Regarding the bond dipoles, they are represented by arrows in the Lewis structure and indicate the direction of electron density shift. To show bond dipoles, you need to determine the difference in electronegativity between the atoms involved in each bond. If the electronegativity difference is significant, the bond is said to be polar, meaning there is an uneven distribution of electron density.
In CH3Cl, the C-Cl bond is polar because chlorine is more electronegative than carbon. Therefore, you can show the bond dipole by drawing an arrow from the less electronegative atom (carbon) towards the more electronegative atom (chlorine). The arrow represents the direction of the electron density shift, indicating the partially negative (δ-) and partially positive (δ+) ends of the bond.
Keep in mind that Lewis structures mainly depict the arrangement of atoms and electrons in a molecule. The representation of partial charges and bond dipoles is a simplified way to show the unequal sharing of electrons. For a more accurate depiction, consider using other molecular modeling techniques such as molecular orbital theory or computational methods.