Atomic and Molecular Physics: Diatomic Orbitals Lecture 16 Quiz

Which force primarily contributes to hydrogen bonding?

What percentage of the strength of a covalent bond can a hydrogen bond have?

Which type of molecules can form hydrogen bonds?

What does the Born-Oppenheimer Approximation describe?

What is the nature of the dipole-dipole interaction in hydrogen bonding?

In natural systems, what tendency do molecules exhibit in terms of energy?

What does the Born-Oppenheimer approximation assume about the motions of the nuclei in a molecule?

In the context of forming a molecule, what does the Schrödinger equation describe?

What is a key factor in forming a molecule of H2 rather than having multiple H atoms floating around?

What does the Hamiltonian represent in finding the total energy of a molecule system using the Born-Oppenheimer approximation?

What is described by the Schrödinger equation for a molecule?

What is assumed about solving the Schrödinger equation for molecules with more than one electron?

What is the key assumption made when using the Born-Oppenheimer approximation?

What is a characteristic of the Schrödinger equation for hydrogen molecule ion?

What is involved in finding the total energy of a molecule system using the Born-Oppenheimer approximation?

What does an approximate wavefunction describing electronic motions assume about nuclei in a molecule?

What is assumed about solving the Schrödinger equation for atoms or molecules larger than the hydrogen atom?

Hydrogen Bonding

The electrostatic force primarily contributes to hydrogen bonding.
Hydrogen bonds can have a strength of up to 5-10% of a covalent bond.
Hydrogen bonds can form between molecules that have a hydrogen atom bonded to a highly electronegative atom (e.g., oxygen, nitrogen, or fluorine).

Born-Oppenheimer Approximation

The Born-Oppenheimer approximation describes the separation of nuclear and electronic motions in a molecule.
The approximation assumes that the motion of the nuclei is slow compared to the motion of the electrons.
The Hamiltonian represents the total energy of a molecule system using the Born-Oppenheimer approximation.

Molecule Formation

The Schrödinger equation describes the behavior of electrons in a molecule.
The key factor in forming a molecule of H2 is the overlap of atomic orbitals, which leads to a lower energy state.
The Schrödinger equation for a molecule describes the total energy of the system, including the kinetic energy of the electrons and the potential energy of the electrons and nuclei.

Assumptions and Characteristics

When solving the Schrödinger equation for molecules with more than one electron, it is assumed that the electrons do not interact with each other.
The key assumption made when using the Born-Oppenheimer approximation is that the motion of the nuclei is slow compared to the motion of the electrons.
The Schrödinger equation for the hydrogen molecule ion is characterized by a simple and exact solution.
An approximate wavefunction describing electronic motions assumes that the nuclei are stationary and do not move during the motion of the electrons.
For atoms or molecules larger than the hydrogen atom, it is assumed that the Schrödinger equation cannot be solved exactly, and approximations must be made.

Natural Systems

In natural systems, molecules tend to exhibit a minimum energy state, which is a stable state.

Test your knowledge on topics covered in Lecture 16 of SIF3002 (Atomic and Molecular Physics) with a focus on diatomic orbitals, hydrogen molecule ion, Born-Oppenheimer Approximation, molecular orbitals, and bonding/anti-bonding orbitals.