Draw the Lewis Structures and name all the isomers of
C4H9Cl.
Name
Lewis Structure
Draw the Lewis Structures and name all the isomers
of C2H2Cl2.
Name
Lewis Structure
Cycloalkanes
Would you predict that cyclopropane and cyclobutane are
highly stable molecules?
1. N2O2 is an unstable compound. Draw
Lewis structure and show all resonance structures.
b) Rank of the following ions in order of increasing
nitrogen-oxygen bond energy:
NO2-,NO+,and
NO3-
C)Rank the following bonds from nonpolar to most
polar: H--H, H--F, H--Cl, H--Br, H--I.
1) draw the most appropriate Lewis structure, 2) all resonance
structures, and 3) formal charges for all atoms having any. Then,
determine the electron and molecular geometries for each
structure.
?????
VAL:
STAB:
BOND:
LONE:
BP:
LP:
Lewis
Structure:
VESPR:
steric
number (# e-‐ pairs): electron pair geometry:
# lone pairs: molecular geometry:
Lewis Structure Drawn with Molecular Geometry:
Be STAB:
Rule Exception: Formal Charges
. a) Draw the Lewis structure of SO3 2- . b)- Identify the
electronic and molecular geometries of the molecule, and the
hybridization of the central atom. c) Is this molecule polar?
Justify your answer by drawing the VSEPR molecular geometry and
labeling the molecular dipole moment.
Draw the lewis dot structure and all resonance structures for
the dithiorcarbonate molecule (S2CO -2).
Which lewis structure is the best for this structure?(formal
charge)
Draw the Lewis structure (including resonance structures) for
methyl azide (CH3N3). Draw the molecule by placing atoms on the
canvas and connecting them with bonds. Do not identify the charge
on each of these species. Include all lone pairs of electrons.
Draw the Lewis structure for AsF3
Draw the Lewis dot structure. To change the symbol of an atom,
double-click on the atom and enter the letter of the new atom.
Draw the Lewis structure for CH3+. Be sure to show the formal
charge on any atom that has a non-zero formal charge.
Draw the Lewis dot structure.
Draw the Lewis structure for BrF3
Draw the Lewis dot structure.
Complete the Lewis structures of SO2 and
SO3. Be sure to draw only the resonance form with the
lowest formal charges (zero) on all atoms. Do not add the formal
charges to the structures. Then predict the solubility of the
structures.