Lewis structures and VSEPR. CO 2 NH 3 H2OH2O CH 4 Lewis structures Please draw the valence shell...
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Transcript of Lewis structures and VSEPR. CO 2 NH 3 H2OH2O CH 4 Lewis structures Please draw the valence shell...
Lewis structures and VSEPR
CO2
NH3
H2OCH4CH4
Lewis structures
Please draw the valence shell picture for NH3 and CO2.
NH3
N needs three covalent bonds to fill its valence shell.
NH H
H
CO2
C needs four covalent bonds to fill its valence shell.
O requires two covalent bonds to fill its valence shell
C OO
maximum number of pairs of electrons two main group atoms can share is 3 pairs.
Lewis structures show the bonding.
Lewis structures do not show the molecular shape.
Valence Shell Electron PairRepulsion or VSEPR
VSEPR model gives molecular shape.
Bonds formation, not electron pair repulsion,is responsible for molecular geometries.
L. S. Bartell J. Chem. Educ., 1968, 45 (12), p 754
VSEPR:
(1) Determine steric number (SN)
(2) Use SN to predict molecular shape
SN
2
3
4
SN
5
6
axial site
equitorial site
more electronegatve atomalways chooses axial site.
two methods to determine SN for VSEPR
1) central atom method
2) Lewis structure method
Central atom method of determining SN(easiest method when there is one atomin the center of the molecule/ion bondedto all the other atoms)
Central atom method is based on the periodic table.
N takes 1 e- awayfrom central atom count.
H contributes 1 e-to central atomelectron count.
Br contributes 1 e-.
O contributes 0 e-.
Z = Zentralatom
Use central atom method to determine SN and shape of:
Determine SN and shape of:
General rule: (99+% true in stable molecules/ions) The least electronegative main groupatom (excluding H) is at the center.
Determine SN and shape of:
XeF5+ XeO3 IOF4
-
SOCl2
c(F) > c(O) > c(N) = c(Cl)
The remarkable molecule OFCl
two methods to determine SN for VSEPR
1) central atom method
2) Lewis structure method
As the molecules get less central-atom-likeit is easiest to use the Lewis-structure methodfor determining the steric number, SN
sulfuricacid
pyro-sulfuricacid
Use the Lewis-structuremethod to determinea plausible molecularshape for pyro-sulfuricacid.*
*method requires one to determineLewis structure before determining molecular shape
or
compound XnYm
Is XnYm a molecule or extended solid?
Ionic metal atoms often 6 coordinate
the shape of XnYm
Locate X and Y onthe periodic table.
Have you seen XnYm before?
Are X and Y fromopposite sides ofthe periodic table?
Is Dc small or are Xor Y 1st and 2nd rowelements?
Are X and Y both p-blockelements?
Use ionic bonding model
Use covalent bonding model
central atommethod
determineLewis structure
determineLewis structure
applyVSEPR
Determine a plausible molecular/extended solid shape. If a portion of the compound might be covalent use covalent model for that portion.
Is XnYm a molecule or extended solid?
yes
no yes
no
yes
Are X and Yboth metals
Use metallic bonding
yes
no
atoms have 10-16bonds each, oftenin closest packing
yes no no
Determine shapes of:
I3- CO2
NH3 TeF6
formal charge
Two standard methods for electron counting
a) formal charge method: Divide equally the shared electrons in bonds between the bondedatoms. Lone pairs ( ) are assigned to host atom.
b) oxidation state method
oxygen startswith six outer shell electrons
carbon startswith four outer shell electrons
O
C
Two standard methods for electron counting
a) formal charge method: Divide equally the shared electrons in bonds between the bondedatoms. Lone pairs ( ) are assigned to host atom.
oxygen startsand ends with six outer shell electrons. O formalcharge is zero.
O
carbon startsand ends with four outer shell electrons. C formalcharge is zero.
C
Please draw a Lewis structure for each of the the above three species. Where ever an atom has non-zero formal chargeplease note the non-zero charge next to the atom.
Please draw a Lewis structure for each of the the above three species. Where ever an atom has non-zero formal chargeplease note the non-zero charge next to the atom.
Correct Lewis structures require placement of all non-zero formal charges on the Lewis diagram.
octet rule
If formal charge is zero :
If formal charge is +1 then atom behaves as if it is an atom one column to the left.
If formal charge is -1 then atom behaves as if it is an atom one column to the right.
and so forth.
assuming atom has eight valence shell electrons.
assuming atom has eight outer shell electrons.
modern and traditional Lewis structures
deducing modern Lewis structures
1. if at all possible, all main group atoms (besides H) have an outer (valence) shell with eight electrons. Hydrogen just needs two. This is the octet rule. Outer shell electrons are called valence electrons.
2. having done step 1, make formal charges as small as possible.
3. no more than 3 bonds (multiple bonds) allowed between two main group atoms. One of the two atoms in this multiple bond istypically a second row element.
it's a puzzle and needs to be solved like a puzzle
draw Lewis structures for all the ions below:
carbonate has 3 resonancestructures
how many resonancestructures does bicarbonatehave?
draw Lewis structures for all the ions to theleft:
deducing traditional Lewis structures
1. make formal charges as small as possible.
2. second row main group elements almost always obey the octetrule.
3. other rows obey octet rule if it doesn't interfere with rules 1 and 2.
4. multiple bonds: allowed to make up to 3 bonds between a pair ofmain group atoms. One of the two atoms in multiple bond is typically a second row element.
it's a puzzle and needs to be solved like a puzzle
please deduce both modern and traditional Lewis structures for the molecules and ions belowPlease also deduce SN and geometry:
SO42-, the sulfate ion
XeO4
PF3Cl2
the modern Lewis structure of PF3Cl2
is a resonant ''detached'' diagram whereeach resonant structure looks like the molecule is separated in two. But the tworesonant structures taken together show a single cohesive whole molecule.
Detached diagrams like this always require the three atoms to be in a straight row, a syzygy. The bonding is called the 3-center 4-electron bond.
comparative studies of modern andtraditional Lewis structures show themodern method is more correct.
comparative studies of modern andtraditional Lewis structures show themodern method is more correct.