molecular structure
DESCRIPTION
Molecular Structure. Both atoms and molecules are quantum systems We need a method of describing molecules in a quantum mechanical way so that we can predict structure and properties The method we use is the Linear Combination of Atomic Orbitals - PowerPoint PPT PresentationTRANSCRIPT
Chemistry 120
Molecular Structure
Both atoms and molecules are quantum systems
We need a method of describing molecules in a quantum mechanical way so that we can predict structure and properties
The method we use is the
Linear Combination of Atomic Orbitals
where we can use the properties of atoms to predict the properties of molecules.
Chemistry 120
Molecular Structure
We combine atoms to form molecules by considering the phase of the atomic orbitals we are using
We represent the phase via the shading we give the orbital.
The phase represents the sign of the wavefunction
Chemistry 120
Molecular Structure
We combine atoms to form molecules by considering the phase of the atomic orbitals we are using
The phase represents the sign of the wavefunction
We represent the phase via the shading we give the orbital.
Chemistry 120
Molecular Structure
For an s orbital, the orbital has the same phase everywhere:
For a p orbital, there is a
change in the sign of the
wavefunction across the
nodal plane:2p orbital, n = 2, l = 1, ml = -1
1s orbital, n = 1, l = 0
Chemistry 120
Molecular Structure
Consider two H atoms (1s1) coming together from infinite separation.
There are two possibilities:
1 The wavefunctions are in phase
2 The wavefunctions are not in phase
Chemistry 120
Molecular Structure
Case 1: The wavefunctions are in phase
The atoms move together and the electron waves overlap with the same phase, producing constructive interference and a build up of electron density between the nuclei
The energy of the system drops and we form a bond
Chemistry 120
r = 8 Å
r = 7 Å
r = 6 Å
r = 5 År = 0.75 Å
r = 1 Å
r = 2 Å
r = 3 Å
Chemistry 120
Molecular Structure
Case 2: The wavefunctions are out of phase
The atoms move together and the electron waves have opposite phase.
The electron waves overlap producing destructive interference and electron density between the nuclei is reduced.
The energy of the system rises and we have an antibonding situation
Chemistry 120
r = 8 Å
r = 7 Å
r = 5 Å
r = 4 Å r = 0.75 Å
r = 1 Å
r = 2 Å
r = 3 Å
Chemistry 120
Bonding Antibonding
Two atoms with wavefunctions in phase overlap with constructive interference. Electron density increases between the nuclei and the overall energy decreases.
When the wavefunctions are of opposite phase, the electron density between the nuclei decreases due to destructive interference. The energy of the system rises and we have an antibonding situation
Chemistry 120
Bonding
Antibonding
Here we see 2 2s orbitals in the bonding and antibonding regimes
In the antibonding regime, there is no build-up of density between the nuclei at any separation.
How do we represent this energetically?
Chemistry 120
Bond length at the minimum energy
Bonding
Antibonding
Energies and phase
Chemistry 120
Bond length at the minimum energy
Bonding
Antibonding
Energies and phase
For the antibonding interaction, there is no minimum in energy at any distance
For the bonding interaction, there is a minimum. The distance is the bond length and the energy is the bond energy
Chemistry 120
Organic Structure and Bonding
bonds and bonds
bonds are in general stronger than bonds and can be formed from either s or p orbitals:
Chemistry 120
Organic Structure and Bonding
bonds and bonds
bonds have no nodal plane that contains the two nuclei.
The * antibonding orbital has a nodal plane between the two nuclei
Chemistry 120
Organic Structure and Bonding
bonds and bonds
bonds have a nodal plane that contains both nuclei,
The * antibonding orbital also has a plane between the nuclei
Chemistry 120
Organic Structure and Bonding
bonds and bonds
These , bonding orbitals and *, * antibonding orbitals are the orbitals that are used to bind all simple organic molecules together.
We can also describe the bonding in diatomic molecules
important models for larger organic systems
Chemistry 120
Organic Structure and Bonding
bonds and bonds
To describe the bonding in the diatomic molecules such as O2, N2 and X2 (X = F, Cl, Br and I), we use both the s orbitals and the p orbitals on the two atoms as a basis set - the palette of atomic orbitals from which we will build the molecular orbitals.
The energies of the two different l states, s and p, are slightly different in polyelectronic atoms.
Chemistry 120
Organic Structure and Bonding
bonds and bonds
The s orbitals and the p orbitals appear as follows
Chemistry 120
Organic Structure and Bonding bonds and bonds
We arrange the atoms along one of the axes for convenience and so the first pair of orbitals we construct are the s and s* orbitals from the s orbitals on the atoms.
Chemistry 120
Organic Structure and Bonding bonds and bonds
We now us the higher energy p orbitals to construct p and porbitals
Chemistry 120
Organic Structure and Bonding bonds and bonds
The complete molecular orbital diagram for all the diatomic molecules from Li2 to N2
Chemistry 120
Organic Structure and Bonding bonds and bonds
The complete molecular orbital diagram for all the diatomic molecules from Li2 to N2
As each molecule has a different number of electrons,
Li2 2 Be2 4 B2 6 C2 8
N2 10 O2 12 F2 14 Ne2 16
Chemistry 120
Organic Structure and Bonding bonds and bonds
Li2 2 Be2 4 B2 6 C2 8
N2 10 O2 12 F2 14 Ne2 16
We can write the electronic structure of each molecule by placing electron pairs into the orbitals.
Chemistry 120
Organic Structure and Bonding bonds and bonds
Li2 2 Be2 4 B2 6 C2 8
N2 10 O2 12 F2 14 Ne2 16
Something peculiar happens after N2
Recall that as the charge on the nucleus increases, the orbitals become more stabilized and the electrons become more strongly bound.
Chemistry 120
Organic Structure and Bonding bonds and bonds
Li2 2 Be2 4 B2 6 C2 8
N2 10 O2 12 F2 14 Ne2 16
This happens by different amounts, depending on the orbital.
After N2 (10 e-), the ordering of the orbitals derived from p change their order in the molecule
Chemistry 120
Organic Structure and Bonding bonds and bonds
For N2 (10 e-), the ordering is this
For O2 (12 e-), the ordering is this
Chemistry 120
Organic Structure and Bonding bonds and bonds
This is an example of configurational interaction
Each electron moves in the field of the other electrons. If the energies of the two molecular orbitals are sufficiently close and the nodal properties are correct, molecular orbitals will interact and shuffle their energies in the molecule.
This causes the orbitals to change their energetic ordering but only when the nuclear charge is high enough to force the electrons close in energy.
Chemistry 120
Organic Structure and Bonding bonds and bonds
Configurational interaction
Each electron moves in the field of the other electrons. If the energies of the two molecular orbitals are sufficiently close and the nodal properties are correct, molecular orbitals will interact and shuffle their energies in the molecule.
This causes the orbitals to change their energetic ordering but only when the nuclear charge is high enough to force the electrons close in energy.
Chemistry 120
Chemistry 120
Chemistry 120
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