vespr theory. vsepr theory vsepr theory (valence shell electron pair repulsion theory) a model for...
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VESPR Theory
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VSEPR Theory
VSEPR Theory (Valence Shell Electron Pair Repulsion Theory)
A model for describing the shapes of molecules whose main postulate is that the structure around a given atom is determined by minimizing the electron pair repulsion
Therefore, the electrons and elements bonded to the central atom want to be as far apart as possible
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VSEPR Steps
1. Draw the Lewis structure for the molecule
2. Count the total number of things that are around the central atom to determine the electron pair geometry
3. Imagine that the lone pairs of electrons are invisible and describe the molecular shape
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Summary VSEPR and Hybridization Table
Electron Domains
Electron Domain
Geometry
PredictedBond Angle(s)
Hybridization of Central
Atom
Molecular Geometry
0 Lone Pair
1 Lone Pair 2 Lone Pair
2 Linear 180º sp Linear
3 Trigonal Planar 120º sp2 Trigonal Plan
ar
Bent
4 Tetrahedral 109.5º sp3 Tetrahedral
Trigonal Pyramidal
Bent
5 Trigonal Bipyrami
dal
90º, 120º sp3d Trigonal Bipyramidal
Seesaw T-shaped
6 Octahedral 90º sp3d2 Octahedral Square Pyramidal Square Planar
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2 Electron Pairs
If there are 2 things attached to the central atom, the shape is linear
Bond angle = 180° Hybridization = sp
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3 Electron Pairs
If there are 3 electron pairs the shape will be trigonal planar
Bond angle = 120°Hybridization =sp2
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3 electron pairs
Now imagine that you have 3 electron pairs, but one is just a lone pair (invisible) what would it look like then?
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4 electron pairs
If there are 4 electron pairs, the shape will be tetrahedral
Bond angle = 109.5°Hybridization = sp3
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4 electron pairs
What if 1 of the electron pairs is a lone pair (invisible)? What would it look like then?
Trigonal Pyramidal
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4 electron pairs
What if there are 2 lone pairs (invisible)? What would it look like then?
bent
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5 electron pairs
If there are 5 electron pairs the shape will be Trigonal Bipyramidal
Bond angles = 90º & 120º Hybridization = sp3d
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5 electron pairs
What is there is 1 lone pair (invisible)
Seesaw
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5 electron pairs
What is there are 2 lone pairs (invisible)
T-shaped
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6 electron pairs
If there are 6 electron pairs the shape will be octahedral
Bond angle = 90°Hybridization = sp3d2
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6 electron pairs
What if there is 1 lone pair (invisible)?
Square pyramidal
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6 electron pairs
What if there are 2 lone pairs (invisible)
Square planar
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Formal Charge
Formal charges can be used in 1 of 2 ways…
1. Suggest where the charges are
2. Help select the most plausible structure from a set of resonance structures
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1 - Suggest where the charges are
Formal charge =
e bonding of #21e bondingnon of #- veof #
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Example
Calculate the formal charge on each element in the carbonate ion
CO3 2-
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Example
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Example
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Example
The sum of the formal charges of the individual charges equals the formal charge on the molecule or ion
The formal charge for carbonate =0 + 0 + -1 + -1 = -2
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2 - Help select the most plausible structure from a set of resonance structures
When choosing the most likely resonance structure
Most likely – All formal charges are zero Next likely – All formal charges add up to zero Next likely – Formal charges add up to the
lowest possible charge Next likely – Negative charge is on most
electronegative atom
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Example
Which of the following resonance structures is most likely for CH2O and why?
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Example
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Another Example
Which is the most likely structure for N2O?
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Another example
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Polar bonds & polar molecules(Dipole or non dipole)
In order for a substance to be polar, the bonds within the molecule must carry different charges and cannot cancel out due to symmetry
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Polar or non polar
CHF3
CO2
BCl3CH4
H2O
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Polar or non polar
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Polar or non polar
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Rule for solubility
Like dissolves likePolar will dissolve in polarNon polar will dissolve in non polar
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Bonding
Intramolecular forces – bonding within molecule (ionic or covalent)
Intermolecular forces – bonding between molecules
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Intermolecular Bonding
2 factors determine if a substance is a solid, liquid, or a gas:
1. Kinetic energy
2. Intermolecular forces holding the particles together
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Intermolecular Bonding
Interactions between molecules
Hydrogen bonding(H attached to N, O,
or F)
Van der Waals forces(attractions between
Dipoles – permanent or Induced)
Dipole – Dipole(polar molecules)
Permanent dipoles
London Dispersion Forces(non polar molecules)
Induced dipoles
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Hydrogen bonding
H is special when it bonds with another element.
The electron is on one side leaving an exposed nucleus
An approaching charged group can get very close the H nucleus creating a lrge electrostatic attraction
These attractions are especially large when H is bonded to a highly electronegative atom like F, O, or N
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Hydrogen bonding
These bonds are called Hydrogen bonds
They are VERY strong leading to 1. High boiling points
2. Viscous
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Van der Waals Forces
Dipole – Dipole Remember, dipoles mean that the molecule has a
partial positive & a partial negative charges at one end
This has a significant effect only when the molecules are close together
The partial positive and partial negative will attract These attractions are called dipole dipole
attractions These come from polar molecules ONLY!!!
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London Dispersion forces
Small electrostatic forces caused by the movement of the electron in molecules that n=have no permanent dipole
In all molecules – polar & non polarHeavier atoms stronger LDF because
valence electrons are further apart in larger molecules & held less tightly so they can more easily form temporary dipoles
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What type of intermolecular forces are present?
Ar HCl HF CaCl2 CH4
CO NaNO3
LDF DD, LDF HB, LDF Ionic LDF DD, LDF Ionic
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Which will have the …
Highest boiling point… HBr, Kr, Cl2 HBr (DD, LDF) Highest freezing point…H2O, NaCl, HF NaCl (ionic) Lowest freezing point…N2, CO, CO2
N2 (smallest non polar present LDF only) Lowest boiling point…CH4, CH3CH3, CH3CH2CH3
CH4 (smallest nonpolar, LDF only) Highest boiling point…HF, HCl, HBr HF (Hydrogen bonding)
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More examples
At 25C ONF is a gas where H2O is a liquid. Why?
H2O forms H bonds which are stronger than the dipole dipole forces in ONF
At 25C Br2 is a liquid when Cl2 is a liquid. Why?
Both have only LDF, but since Br2 is heavier, the LDF are greater