Molecular Atomic Orbital

What is the basic principle behind molecular atomic orbitals?

• Formation of ionic bonds between atoms

• Interaction of electrons with the nucleus

• Creation of covalent bonds within a single atom

• Combination of atomic orbitals from different atoms

How do sigma and pi bonds differ in molecular atomic orbitals?

• Sigma bonds allow free rotation, while pi bonds restrict rotation.

• Sigma bonds form between s orbitals, while pi bonds form between p orbitals.

• Pi bonds are more flexible than sigma bonds.

• Sigma bonds are stronger than pi bonds.

Explain the concept of hybridization in molecular atomic orbitals.

• Hybridization involves the separation of atomic orbitals into distinct energy levels

• Hybridization results in the formation of identical atomic orbitals

• Hybridization in molecular atomic orbitals involves the mixing of atomic orbitals to form new hybrid orbitals with unique properties.

• Hybridization is the process of converting a molecule into a hybrid species

What is the significance of the overlap of atomic orbitals in molecular orbital theory?

• It has no impact on molecular structure

• It leads to the formation of new molecular orbitals through constructive or destructive interference.

• It results in the formation of ionic bonds

• It causes the atoms to repel each other

Describe the shape of a sp3 hybridized orbital.

• Linear

• Square

• Octahedral

• Tetrahedral

What is the difference between bonding and antibonding molecular orbitals?

• Bonding orbitals have higher energy than antibonding orbitals.

• Antibonding orbitals are more stable than bonding orbitals.

• Bonding orbitals repel electrons while antibonding orbitals attract electrons.

• Bonding molecular orbitals are lower in energy and higher in stability compared to antibonding molecular orbitals.

How does the number of atomic orbitals involved in hybridization affect the geometry of molecules?

• The number of atomic orbitals involved in hybridization determines the hybridization type and subsequently the molecular geometry.

• The number of atomic orbitals involved in hybridization influences the boiling point of molecules

• The number of atomic orbitals involved in hybridization determines the color of molecules

• The number of atomic orbitals involved in hybridization has no effect on the geometry of molecules

What is the role of symmetry in molecular atomic orbitals?

• Symmetry is only relevant for inorganic molecules, not organic molecules

• Symmetry causes molecular atomic orbitals to have different electron configurations

• Symmetry helps determine the shape, energy levels, bonding behavior, and molecular geometry of molecular atomic orbitals.

• Symmetry has no impact on molecular atomic orbitals

Explain the concept of delocalization in molecular orbital theory.

• Delocalization only occurs in ionic compounds, not covalent molecules.

• Delocalization in molecular orbital theory involves the spread of electrons over multiple atoms or regions in a molecule, leading to the formation of molecular orbitals.

• Delocalization leads to the formation of localized molecular orbitals.

• Delocalization refers to the confinement of electrons within a single atom in a molecule.

What are the key assumptions of the molecular orbital theory?

• The number of molecular orbitals formed is always equal to the number of atomic orbitals combined

• Molecular orbitals are always lower in energy than atomic orbitals

• Linear combination of atomic orbitals, conservation of total number of orbitals, filling of molecular orbitals with electrons following Pauli exclusion principle and Hund's rule.

• Electrons in molecular orbitals are not subject to the Pauli exclusion principle