Please see the attachment for a better formatting of these questions.
1) Draw a structural formula for each of the following molecules. Which bonds are polar? Indicate the polarity by proper placement of the symbols d+ and d-.
2) Draw structural formulas for all possible isomers having the following molecular formulas:
3) Write electron-dot formulas for the following ionic species. Show the formal charges on individual atoms in each ion.
bisulfite ion, HSO3¯
ammonium ion, NH4+
carbonate ion, CO32¯
carbon dioxide, CO2
chlorate ion, ClO3¯
chlorite ion, ClO2¯
4) Fill in any electron pairs that are missing from the following formulas:
(double bond) between the O and C
5) Use lines, dashed wedges, and solid wedges to show the geometry of CH4, CH2Cl2, and CF3OH.
6) Write a structural formula that corresponds to the molecular formula C6H12O and is:
1 a) CH3Cl The C-Cl bond is polar due to the difference in electronegativity between the C and the Cl. I have shown the polarity on this using the dipole moment convention.
b) H2 Since both H's have exactly the same electronegativity there is no polar bond.
2) The only 2 possibilities are a ketone and an aldehyde.
3) Remember that formal charge is the number of electrons an atom wants to have relative to the number that is assigned to it. Lone pairs are completely controlled by an atom and so are assigned to that atom. Bonding pairs are shared so that only ½ of the bonding ...
This response provides assistance on drawing structural formulas for molecular formulas and determines whether these formulas are polar.