Chemistry: Atoms First - Chapter 7 Molecular Geometry, Intermolecular Forces, and Bonding Theories

These flashcards cover essential concepts in molecular geometry, intermolecular forces, and bonding theories as outlined in Chapter 7 of the provided notes.

What is hybridization in the context of bonding?

The mixing of atomic orbitals to form new hybrid orbitals that can explain bond angles.

What is the electron-domain geometry for a molecule with 5 electron domains?

Trigonal bipyramidal.

What type of interactions do molecules like CCl4 exhibit?

Dispersion forces only, as they are nonpolar.

What type of molecular geometry does NH3 exhibit?

Trigonal pyramidal due to the presence of a lone pair.

Why does carbon dioxide (CO2) exhibit nonpolar characteristics despite having polar bonds?

The linear geometry causes the dipoles to cancel each other.

What are molecular orbitals and how do they arise?

Molecular orbitals result from the combination of atomic orbitals that have specific shapes and energies.

What type of bond is formed during the overlap of p orbitals?

Pi (π) bond.

What occurs in the case of a molecule being paramagnetic?

It contains unpaired electrons and is attracted to a magnetic field.

What characteristic describes molecules with delocalized bonding such as benzene?

Delocalized π bonds spread out over the entire molecule.

What is the significance of hybridization in molecular chemistry?

It explains the bond angles and geometries that cannot be described by simple overlapping of atomic orbitals.

What type of force links the molecules in a solid?

Intermolecular forces such as hydrogen bonding or dipole-dipole interactions.