chapter 9 covalent bonding: orbitals hybridization the mixing of atomic orbitals to form special...
TRANSCRIPT
Chapter 9Covalent Bonding: Orbitals
Hybridization
• The mixing of atomic orbitals to form special orbitals for bonding.
• The atoms are responding as needed to give the minimum energy for the molecule.
The Valence Orbitals on a Free Carbon Atom: 2s, 2px, 2py, and 2pz
The Formation of sp3 Hybrid Orbitals
An Energy-Level Diagram Showing the Formation of Four sp3 Orbitals
Tetrahedral Set of Four sp3 Orbitals
The Nitrogen Atom in Ammonia is sp3 Hybridized
sp3 HybridizationThe experimentally known structure of CH4 molecule can be explained if we assume that the carbon atom adopts a special set of atomic orbitals. These new orbital are obtained by combining the 2s and the three 2p orbitals of the carbon atom to produce four identically shaped orbital that are oriented toward the corners of a tetrahedron and are used to bond to the hydrogen atoms.
Whenever a set of equivalent tetrahedral atomic orbitals is required by an atom, this model assumes that the atom adopts a set of sp3 orbitals; the atom becomes sp3 hybridized.
The Hybridization of the s, px, and py Atomic Orbitals
An Orbital Energy-Level Diagram for sp2 Hybridization
• A sigma () bond centers along the internuclear axis.
• A pi () bond occupies the space above and below the internuclear axis.
CCH H
HH
An sp2 Hybridized C Atom
The Bonds in Ethylene
Sigma and Pi Bonding
The Orbitals for C2H4
When One s Orbital and One p Orbital are Hybridized, a Set of Two sp Orbitals Oriented at 180 Degrees Results
The Hybrid Orbitals in the CO2 Molecule
The Orbital Energy-Level Diagram for the Formation of sp Hybrid Orbitals on Carbon
The Orbitals of an sp Hybridized Carbon Atom
The Orbital Arrangement for an sp2 Hybridized Oxygen Atom
The Orbitals for CO2
The Orbitals for N2
A Set of dsp3 Hybrid Orbitals on a Phosphorus Atom
An Octahedral Set of d2sp3 Orbitals on a Sulfur Atom
The Relationship of the Number of Effective Pairs, Their Spatial Arrangement, and the Hybrid Orbital Set Required
The Localized Electron Model
Three Steps: Draw the Lewis structure(s)
Determine the arrangement of electron pairs (VSEPR model).
Specify the necessary hybrid orbitals.
Molecular Orbitals (MO)
• Analagous to atomic orbitals for atoms, MOs are the quantum mechanical solutions to the organization of valence electrons in molecules.
• Molecular orbitals have many of the same characteristics as atomic orbitals, such as they can hold two electrons with opposite spins and the square of the molecular orbital wave function indicates electron probability.
The Combination of Hydrogen 1s Atomic Orbitals to Form Molecular Orbitals
The Molecular Orbitals for H2
Types of MOs
• bonding: lower in energy than the atomic orbitals from which it is composed. Electrons in this type of orbital will favor the molecule.
• antibonding: higher in energy than the atomic orbitals from which it is composed. Electrons in this type of orbital will favor the separated atoms.
Bonding and Antibonding Molecular Orbitals (MOs)
The Molecular Orbital Energy-Level Diagram for the H2 Molecule
The Molecular Orbital Energy-Level Diagram for the H2- Ion
Bond Order (BO)
• Difference between the number of bonding electrons and number of antibonding electrons divided by two.
• Bonds order is an indication of bond strength. Large bond order means greater bond strength.
B O = # b o n d in g e lec tro n s # an tib o n d in g e lec to n s
2
The Molecular Orbital Energy-Level Diagram for the He2 Molecule
Bonding in Homonuclear Diatomic Molecules
In order to participate in MOs, atomic orbitals must overlap in space. (Therefore, only valence orbitals of atoms contribute significantly to MOs.)
The Relative Sizes of the Lithium 1s and 2s Atomic Orbitals
The Molecular Orbital Energy-Level Diagram for the Li2 Molecule
The Molecular Orbitals from p Atomic Orbitals
The Expected Molecular Orbital Energy-Level Diagram Resulting from the Combination of the 2p Orbitals on Two Boron Atoms
The Expected Molecular Orbital Energy-Level Diagram for the B2 Molecule
Paramagnetism
unpaired electrons
attracted to induced magnetic field
much stronger than diamagnetism
Diamagnetism
paired electrons
repelled from induced magnetic field
much weaker than paramagnetism
Diagram of the Kind of Apparatus Used to Measure the Paramagnetism of a Sample
The Correct Molecular Orbital Energy-Level Diagram for the B2 Molecule
Molecular Orbital Summary of Second Row Diatomics
Outcomes of MO Model
1. As bond order increases, bond energy increases and bond length decreases.
2. Bond order is not absolutely associated with
a particular bond energy.
3. N2 has a triple bond, and a correspondingly
high bond energy.
4. O2 is paramagnetic. This is predicted by the MO model, not by the LE model, which predicts diamagnetism.
Combining LE and MO Models
bonds can be described as being localized.
bonding must be treated as being delocalized.
The Resonance Structures for O3 and NO3-
A Benzene Ring
The Sigma System for Benzene
The Pi System for Benzene
The NO3- Ion