rebel molecules. most of the time the octet rule is followed, ome molecules disobey octet rule c, n,...
TRANSCRIPT
Rebel Molecules
Rule Breakers
MOST OF THE TIME THE OCTET RULE IS FOLLOWED, ome molecules disobey octet rule
C, N, O, and F are mostly rule keepers
1) Odd Number of Valence Electrons2) Incomplete Octets3) Expanded Valence Shells
Molecular Exceptions to the Octet Rule
Not every electron is in a pairAll atoms in the molecule cannot have their
octet satisfiedThese molecules are generally NOT stable CHECK electron number before assuming
odd number of electrons
Ex. NO, NO2
1) Odd Number of Valence Electrons
Molecules with odd valence electron #, not stable
Very reactive
Intermediate compounds in a chemical reaction, short-living
Free Radicals
Not enough valence electrons to go around ! Not every atom can achieve the octet rule as a result
Reactive
1st share single electron pair and then if necessary, it is possible to satisfy the octet rule for ALL atoms by sharing 2-3 electron pairs
Atoms with strong double/triple bonds are C, N, O, P, and S.
2) Incomplete Octets (cont.)
Example: ozone (O3)
GENERALLY,
A) All Lewis Structures are not necessarily equal for resonance hybrid
B) Some resonance structures contribute more to the structure of the resonance hybrid than others.
2) Incomplete Octets (cont.)
Applies only to elements in 3+ periods of periodic table
Central atom’s valence shell expands to account for extra electrons
3) Expanded Valence Shells
**Applies only to elements in 3+ periods of periodic table **
** Applied when not possible to draw Lewis structure without expanding the shells **
Valence shell incorporates “d subshell region” (up to 18 electrons) More than 8 electrons shared
Add valence shells if more than 8 valence electrons are around the central atom
3) Expanded Valence Shells
Example: sulfur tetrafluoride (SF4)
1) Common Exceptions---H, HeOnly one electron pair needed to fill valence shell
2) Elements located AT or GREATER than 3rd period.Exceed octet, EXPAND VALENCE SHELL, not electron
deficient
3) Elements located WITHIN 2nd Period. No surpassing octet, can be electron deficient
**Octet rule applies to C, N, and O so applies to many molecules!!!
In Summary---
There is an error in each of these structures. What is it?
Example 2:
Only one Lewis Structure is correct. Identify it and state the problem (s) with the other structures.
Example 3:
Read pp. 361-366
Problems pp. 381-382 #53-54, 59-60
Homework