Table of Contents
- 1 What are the limitations of molecular orbital theory?
- 2 How does molecular orbital theory explain resonance?
- 3 What are the condition for the formation of molecular orbital from atomic orbital?
- 4 Which molecular orbitals are formed when the 1s orbitals of two hydrogen atoms combine to form a hydrogen molecule?
- 5 What is the hybridization of chlorine trifluoride in ClF3?
- 6 What is boron trifluoride?
What are the limitations of molecular orbital theory?
MO theory says that the electrons are delocalized. That means that they are spread out over the entire molecule. The main drawback to our discussion of MO theory is that we are limited to talking about diatomic molecules (molecules that have only two atoms bonded together), or the theory gets very complex.
What can molecular orbital theory be applied to?
This promotion weakens the bond between the two hydrogen atoms and can lead to photodissociation—the breaking of a chemical bond due to the absorption of light. Molecular orbital theory is used to interpret ultraviolet-visible spectroscopy (UV-VIS).
How does molecular orbital theory explain bonding?
The Rules of Molecular Orbital Theory: First principle: The number of molecular orbitals produced is always equal to the number of atomic orbitals brought by the atoms that have combined. According to MO Theory, the two molecular orbitals that form are called s (sigma = bonding) and s* (sigma star = antibonding).
How does molecular orbital theory explain resonance?
Molecular Orbital theory starts by assuming that the three atomic p orbitals on the O atoms overlap to form three molecular π orbitals that extend over the whole molecule. Thus, Molecular Orbital theory explains resonance delocalization automatically as the natural state of the molecule.
Can molecular orbital theory predict stability?
We can therefore use a molecular orbital energy-level diagram and the calculated bond order to predict the relative stability of species such as H2+.
What does molecular orbital theory explain that other bonding theories do not?
Unlike valence bond theory, which uses hybrid orbitals that are assigned to one specific atom, MO theory uses the combination of atomic orbitals to yield molecular orbitals that are delocalized over the entire molecule rather than being localized on its constituent atoms.
What are the condition for the formation of molecular orbital from atomic orbital?
For the formation of the proper molecular orbital, proper energy and orientation are required. For proper energy, the two atomic orbitals should have the same energy of orbitals and for the proper orientation, the atomic orbitals should have proper overlap and the same molecular axis of symmetry.
How molecular orbitals are formed?
When multiple atoms combine chemically into a molecule, the electrons’ locations are determined by the molecule as a whole, so the atomic orbitals combine to form molecular orbitals. The electrons from the constituent atoms occupy the molecular orbitals.
How are molecular orbitals formed?
Molecular orbitals are obtained by combining the atomic orbitals on the atoms in the molecule. One of the molecular orbitals in this molecule is constructed by adding the mathematical functions for the two 1s atomic orbitals that come together to form this molecule.
Which molecular orbitals are formed when the 1s orbitals of two hydrogen atoms combine to form a hydrogen molecule?
Thus, the overlap of the 1s orbitals of two hydrogen atoms to form H2 produces two molecular orbitals (Figure 9.32). FIGURE 9.32 The combination of two H 1s atomic orbitals forms two molecular orbitals of H2.
How does molecular orbital theory explain stability?
Bonding molecular orbitals are formed by in-phase combinations of atomic wave functions, and electrons in these orbitals stabilize a molecule. Antibonding molecular orbitals result from out-of-phase combinations of atomic wave functions and electrons in these orbitals make a molecule less stable.
What makes a molecular orbital stable?
It is called a sigma ( ) molecular orbital because it looks like an s orbital when viewed along the H-H bond. Since the * antibonding molecular orbital forces the electron to spend most of its time away from the area between the nuclei, placing an electron in this orbital makes the molecule less stable.
What is the hybridization of chlorine trifluoride in ClF3?
When we talk about the hybridization of chlorine trifluoride we have to consider its central atom which is Cl. This atom contains 7 valence electrons while ClF3 should consist of 3 bond-pairs and 2 lone-pairs. If we take a closer look at the valence electronic configuration of Cl it is represented as 3s 2, 3px 2, 3py 2, 3pz 1, 3d.
How many hybrid orbitals should be present in ClF3?
Here two hybrid orbitals will contain a pair of electrons and three hybrids will contain unpaired electrons which will again overlap with the 2p orbital of F to form single bonds. The central atom Cl needs three unpaired electrons to bond with three F-atoms. ClF3 should consist of 3 bond-pairs and 2 lone-pairs.
What do you know about electron geometry of chlorine trifluoride?
The electron geometry of chlorine trifluoride is trigonal bipyramidal with a 175° F-Cl-F bond angle. Put your understanding of this concept to test by answering a few MCQs. Click ‘Start Quiz’ to begin! Congrats!
What is boron trifluoride?
Boron trifluoride is a boron fluoride. Boron trifluoride is a colorless gas with a pungent odor. It is toxic by inhalation. It is soluble in water and slowly hydrolyzed by cold water to give off hydrofluoric acid, a corrosive material. Its vapors are heavier than air.