The highest occupied molecular orbital of a molecule is abbreviated as the HOMO. The lowest unoccupied molecular orbital in a molecule is called the LUMO. Experimentally, one can measure the difference in energy between the HOMO and LUMO by taking the electronic absorption (UV-visible) spectrum of the molecule. Peaks in the electronic absorption spectrum can be labeled as π_2p-π_2p, σ_s-σ_2s, and so on, corresponding to electrons being promoted from one orbital to another. The HOMO-LUMO transition corresponds to molecules going from their ground state to their first excited state. (c) The electronic absorption spectrum of the N₂ molecule has the lowest energy peak at 170 nm. To what orbital transition does this correspond?

Verified step by step guidance

Identify the type of electronic transition that occurs in the N2 molecule when it absorbs light at 170 nm.

Understand that the lowest energy peak in the electronic absorption spectrum corresponds to the HOMO-LUMO transition.

Recall that the HOMO (Highest Occupied Molecular Orbital) and LUMO (Lowest Unoccupied Molecular Orbital) are involved in the transition from the ground state to the first excited state.

Determine the nature of the orbitals involved in the HOMO-LUMO transition for the N2 molecule, which typically involves \(\pi\) \, \(\text{to}\) \, \(\pi\)^* \, \(\text{or}\) \, \(\sigma\) \, \(\text{to}\) \, \(\sigma\)^* \, \(\text{transitions}\).

Conclude that the transition at 170 nm corresponds to the HOMO-LUMO transition, likely involving a \(\pi\) \, \(\text{to}\) \, \(\pi\)^* \, \(\text{transition}\) \, \(\text{in}\) \, \(\text{the}\) \, \(\text{N}\)_2 \, \(\text{molecule}\).

Verified video answer for a similar problem:

This video solution was recommended by our tutors as helpful for the problem above.

Video duration:

Was this helpful?

Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

HOMO and LUMO

The Highest Occupied Molecular Orbital (HOMO) is the highest energy orbital that contains electrons in a molecule, while the Lowest Unoccupied Molecular Orbital (LUMO) is the lowest energy orbital that is empty. The energy difference between these two orbitals is crucial for understanding electronic transitions, as it determines the energy required for an electron to be excited from the HOMO to the LUMO.

Electronic Absorption Spectrum

An electronic absorption spectrum is a graphical representation of the wavelengths of light absorbed by a molecule as electrons transition between energy levels. Peaks in this spectrum indicate specific electronic transitions, such as from the HOMO to the LUMO, and the position of these peaks can provide information about the energy levels of the molecular orbitals involved.

Orbital Transitions

Orbital transitions refer to the movement of electrons between different molecular orbitals, typically from a lower energy orbital to a higher energy one. In the context of the question, the transition from the HOMO to the LUMO corresponds to the absorption of a photon, which promotes an electron to a higher energy state, and is fundamental in understanding the electronic properties of molecules.

Recommended video:

Guided course

03:12

Transition Metals

Related Practice

Textbook Question

One of the molecular orbitals of the H2- ion is sketched below:

(a) Is the molecular orbital a s or p MO? Is it bonding or antibonding?

Textbook Question

One of the molecular orbitals of the H2- ion is sketched below: (d) Compared to the H¬H bond in H2, the H¬H bond in H2- is expected to be which of the following: (i) Shorter and stronger, (ii) longer and stronger, (iii) shorter and weaker, (iv) longer and weaker, or (v) the same length and strength?

Textbook Question

Place the following molecules and ions in order from smallest to largest bond order: N22+, He2+, Cl2 H2-, O22-.

Textbook Question

The structure of borazine, B₃N₃H₆, is a six-membered ring of alternating B and N atoms. There is one H atom bonded to each B and to each N atom. The molecule is planar. (e) What are the hybridizations at the B and N atoms in the Lewis structures from parts (a) and (b)? Would you expect the molecule to be planar for both Lewis structures? Would you expect the molecule to be planar for both Lewis structures?

Textbook Question

The structure of borazine, B₃N₃H₆, is a six-membered ring of alternating B and N atoms. There is one H atom bonded to each B and to each N atom. The molecule is planar. (c) What are the formal charges on the atoms in the Lewis structure from part (b)? Given the electronegativities of B and N, do the formal charges seem favorable or unfavorable? What are the formal charges on the atoms in the Lewis structure from part (b)?