Draw the resonance hybrid structure for ClF3. Indicate the formal
charge for each atom and the bond order for each bond (two Cl-F
bonds are 170 pm and one Cl-F bond is 160 pm). Thanks!
Write the Lewis structure. Calculate the formal charge on the
center atom. Show resonance if it exists.
a.) chlorate ion
b.) XeF3 +
c.) NO2 +
d.) nitrous oxide (remember H bonds to Oxygen. Calculate the
formal charge on nitrogen.)
A.) Draw a Lewis diagram for SO42- in
which the central S atom has a formal charge of zero and show all
NONZERO formal charges on all atoms.
B.)Draw a Lewis structure for SO42- in
which the octet rule is satisfied on all atoms and show all NONZERO
formal charges on all atoms.
C.)Based on formal charge, what is the best Lewis structure for
the ion? Octet rule or smallest formal charge
1. Draw the possible resonance
structures for [S2CN(CH3)2]- and assign formal charges. Indicate
which resonance structure provides the best description for the ion
and why?
2. Predict and draw the Lewis dot
structures for the following compounds. Include a description of
distortion from ideal geometry and why.
a) [IF3]2-
b) XeO2F2
3. Predict the order of solubility in
water for the following series, and explain the factors
involved.
PbCl2 PbBr2 PbBI2 PbS
4. Draw all isomers for the compound
[Cr(H2O)3Br(Cl)(I)]...
Write two resonance structures of
C3H3− ion. Mention the
formal charge of each atom.
A covalent bond has 3.15% ionic character. If the experimental
value of the dipole moment were found to be 0.22 D, what would be
the length of the covalent bond in picometer?
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