General Chemistry - Bonding and Molecular Theory

These flashcards cover key concepts related to bonding theories, molecular orbital theory, and hybridization as presented in the lecture notes.

What are the two conditions for a covalent bond to form according to Valence Bond Theory?

1. Two atomic orbitals must overlap. 2. The total number of electrons in both orbitals should be less than or equal to 2.

What type of hybridization is present in CH4?

sp3 hybridization.

Describe the molecular geometry of H2O based on the VSEPR model.

The molecular geometry of H2O is bent due to four pairs of electrons around oxygen.

What are σ bonds and how do they form?

σ bonds are formed by the overlap of atomic orbitals along the bonding axis.

What is the bond order formula in molecular orbital theory?

Bond order = (number of electrons in bonding orbitals - number of electrons in antibonding orbitals) / 2.

What distinguishes paramagnetism from diamagnetism?

Paramagnetism occurs in species with unpaired electrons which are attracted to magnetic fields, while diamagnetism occurs in species with all paired electrons which are repelled by magnetic fields.

What is hybridization in the context of molecular bonding?

Hybridization is the mixing of atomic orbitals to generate new sets of orbitals that form covalent bonds.

How many types of hybrid orbitals correspond to tetrahedral geometry?

Four sp3 hybrid orbitals.

What does a molecular orbital diagram illustrate?

It illustrates the bonding and antibonding interactions between atomic orbitals in a molecule.

What is the significance of lower energy in bonding orbitals compared to atomic orbitals?

Bonding orbitals provide stability to the molecule by increasing electron density between nuclear centers.