Write a Lewis structure for the phosphorus trifluoride molecule, PF3. Is the octet rule satisfied for all the atoms in your structure? (b) Determine the oxidation numbers of the P and F atoms. (c) Determine the formal charges of the P and F atoms. (d) Is the oxidation number for the P atom the same as its formal charge? Explain why or why not.
A valid Lewis structure of ________ cannot be drawn without
violating the octet rule.
a)
NI3
b)
SO2
c) ICl5
d) SiF4
Please show the Lewis structure for each so I can try to better
understand.
Draw a Lewis structure for PSF3 in
which the octet rule is satisfied on all atoms and show all
NONZERO formal charges on all atoms.
Do not include the overall ion charge in your answer.
Based on formal charge, what is the best Lewis structure for the
molecule?
Draw a Lewis structure that obeys the octet rule for
each of the following ions. Assign formal charges to each atom.Draw
a Lewis structure that obeys the octet rule for each of
the following ions. Assign formal charges to each atom.
ClO3−
NO3−
Draw a Lewis structure for SO2 in which all atoms obey the octet rule. Show formal charges. Do not consider ringed structures.
Draw a Lewis structure for SO2 in which all atoms have a formal charge of zero. Explicitly showing the zero charges is optional. Do not consider ringed structures.
What is the "octet rule" and what role does it play in Lewis
structures. Use the octet rule to predict Lewis structures for a
few simple molecules such as ammonia (NH3), carbon
dioxide (CO2), ozone (O3), ethane
(C2H6), ethylene (C2H4)
or acetylene (C2H2).
Please add references
In the compound (CH3)3N=CH2, how is the lewis structure formed,
considering that the octet rule must be maintained, but only one of
the three CH3's actually become a CH2? Also, is the reason why
(CH3)3N(+) - (-C:)H2 not permissible because the Carbon atom on CH2
has too many electrons, and the cation should be on Nitrogen
instead? This is in regards to Organic Chemistry (10th Ed) Problem
19P in chapter 1.
1.Draw a Lewis structure for each of them. Remember that some
molecules violate the Octet Rule in different ways. Some of these
use multiple bonds and some don't. You need to figure out which do.
Use the rules we had in class for writing Lewis structures and
compare with these with the molecules we did write Lewis structures
for. None of these have resonance structures.
SF6 CH4 I3-
N2 XeF4 NH3
OH- CO C2H4 (in this molecule
there is...