molecular orbital theory? my teacher was like "im not teaching it, but its going to be on your test" can you please summarize what it is,
i read the online sites,tehy don't make sense...
What text do you have, please?
Molecular orbitals are orbitals for shared electron pairs (also called covalent bonds). They are based on Quantum Mechanics and they have been developed fully for only for diatomic molecules through the second row of the periodic table.
There are two kinds of orbitals: Bonding, and anti-bonding (marked by a star).
Starting with sigma1s^2 you place the total number of electrons for the two atoms into those orbitals until you run out of electrons. I am using the word "sigma" for the Greek (Symbol) lower case letter sigma:
sigma(1s)^2, sigma(1s)*^2, sigma(2s)^2, sigma(2s)*^2, sigma(2p)^2, π(2p)^2, π(2p)^2, π(2p)*^2, π(2p)*^2, sigma(2p)*^2.
For examples of how this orbital energy sequence is used with specific diatomic molecules of ions, go to:
http://www.mpcfaculty.net/mark_bishop/molecular_orbital_theory.htm
To find the the "bonding order", use:
[#bonding electrons - #anti-bonding] / 2
The bonding order tells you if you have a single, double, or triple covalent bond.
Of course! Molecular orbital theory is a fundamental concept within chemistry that helps us understand the behavior of molecules and their electronic structure. It provides a more detailed understanding of chemical bonding than other theories, such as Lewis structures or hybridization.
In molecular orbital theory, we consider the combination of atomic orbitals (AOs) from individual atoms to form molecular orbitals (MOs) that describe the behavior of the electrons in a molecule. These MOs are distributed over the entire molecule, rather than being localized on specific atoms.
The process of forming MOs involves the combination and interaction of atomic orbitals, resulting in the formation of bonding and antibonding molecular orbitals. Bonding orbitals help to stabilize the molecule by lowering its energy, while antibonding orbitals have higher energy and contribute to destabilization.
The number of molecular orbitals formed is equal to the number of atomic orbitals combined. These molecular orbitals can then be populated with electrons according to the Aufbau principle, Pauli exclusion principle, and Hund's rule.
By determining the energy levels and electron occupancy of molecular orbitals, we can predict properties like bond order, molecular stability, and the presence of unpaired electrons or radical species.
To fully understand molecular orbital theory, it is important to have a solid foundation in basic atomic structure, atomic orbitals, and electron configuration. It can be a complex topic, so it may require some time and effort to grasp the concepts fully.
I recommend reviewing your textbook or studying resources that provide detailed explanations and examples of molecular orbital theory. Additionally, seeking assistance from your teacher or classmates for clarification can be beneficial.