CHEM 120 Lecture Notes - Lecture 1: Lewis Structure, Ionic Compound, Lone Pair

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16 Aug 2016
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Types of Bonds
Covalent Bonds
Even sharing the electrons relative to the other types of bonding
The difference between their electro negativities should be with 0-0.2
oH and F are both diatomic but have completely different electronegativity's
oBoth in bond have 0 difference, so all diatomic molecules are perfectly covalent
o*Fluorine combined with any other non-metal is not covalent*
Polar Covalent Bonds
"Shared" electrons that spend more time on one element than another
One's going to be more negative (where the electron hangs out), the other more
positive (the loner)
The range for the difference of electronegativities is 0.3 to 1.4
oPolar bond /dipole bond (same thing
e.g. HCl
3.0 - 2.1 = 0.9 Polar covalent bond
(more positive) H -------- Cl (more negative)
Ionic Bonds
Anything that has an electronegativity difference greater than 1.5 is ionic
They do not share electrons
oElectrons have moved from the less electronegative to the more electronegative
oThey break into 2 ions
The bond is due to the attraction of more positive nucleus of the ion to
the extra electrons on the outer valence shell of the more electronegative
element which is an electrostatic attraction
In other words, ionic bonds are bonds because of the electrostatic attraction between
the produced ions, or it simply is an electrostatic attraction
There is no place where the electron should be since they aren’t being shared, which
explains the crystal lattice structure of a solid ionic compound
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