Vsepr Chart Worksheet Page 2
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1
2Valence Bond Theory: How bonds form
sigma bond (p. 453)
pi bond (p. 454)
Bond Polarity p. 460-462.: Copy from Page 5 of your packet
Type of Bond
Non Polar covalent
Polar covalent
Ionic
Sharing of electrons?
Charge Distribution?
electronegativity
difference?
Types of atoms
Picture, δ+, δ-
atoms?
Example, math?
Molecular Polarity : Is the Molecule (not just the bond) Polar or Non-polar? p. 462-463
Polar
A
molecule has “different” ends. One “end” is slightly plus (δ+) the other is slightly minus (δ−).
A Non-polar molecule is “all alike.” No plus & minus ends.
Follow this Flow chart step by step to determine Molecular Polarity
1. If the bonds are non-polar, the molecule is non-polar ( All alike, no + and – ends)
!
F–F !O=O!
δ− F
different atoms
2. If there are
around the central atom, the molecule is polar.
|
F – C– Cl
!
(has a + end and a - end) (because the bonds are polar but not alike)
|
Cl δ+
same atom
3. If the
is all around the central atom (the bonds are polar and all alike) the Polarity of the
molecule depends on the shape around the central atom.
F
Cl
|
|
If a
! 3 atom linear!
\!
No Non-bonding electrons
Symmetrical
O=C=O
B
Cl –C– Cl
shape :!
trigonal planar!
} ! Charges cancel out!! ! !
!
/ \
|
F
F
Cl
Molecule is non-polar!!
Non-Polar!
tetrahedral!
/!
δ −
δ –
N
O
If a Non !
2 atom linear ! \!
Has Non-bonding electrons
δ+ δ-
/ | \
/ \
symmetrical ! bent!
}!
Charges don’t cancel out.
H – Cl
H H H
H
H
δ+ δ+ δ+
δ +
δ +
Polar
shape: !
pyramidal!
/!
Molecule is
Polar
!
!
!
(has a + end and a – end)
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