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octet rule
being like noble gas
Lewis structure for covalent bonds (not ionic)
yupp
ionic bonds
covalent bonds
nonpolar and polar
nonpolar
equal or most equal sharing of electrons
X - Y
polar
unequal sharing of electrons with slight separation of charge
Electronegativity (EN)
ability of an atom to attract shared electrons in a bond
Trend L to R ↑
Bottom to Top ↑
Polar bonds have...
Dipole moment
Dipole Moment
(μ)
shift in electron density
H -- Cl
------>
+ -
arrow where more electronegative
Which atom is usually the central atom?
usually least electronegative BUT hydrogen is NEVER the centre
notes about lewis structures
distribute remaining electrons on OUTSIDE first to give an octet then work way inside
and if central doesn't have octet... make that shit work somehow with double and triple and quad bonds
Formal Charge
NOT actual charge, just a way to track electrons
For lewis structure electrons
1. All nonbinding electrons
2. Half of bonding electrons
basically bonds count as one and each free electron also counts as one
if more than one possible structure...
1. choose structure when sum of charge = charge on molecule
2. choose struture with small formal charges (0, +/- 1) not +/- 2, +/- 3 etc
3. choose structures when most EN atom has a negative formal charge
Resonance Stuctures
More than one way to draw a lewis structure that is correct
don't for get to add <---> thingy
Exceptions to the Octet Rule
Incomplete Octet
exception: H needs 2; B needs 6; Be needs 4
Odd number of Valence
ie Nitrogen
Expanded Octet
ie SF6
Author
misol
ID
298199
Card Set
Chemistry Chapter 6
Description
chemistry chapter 6 exam
Updated
3/11/2015, 11:04:48 PM
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