Related Experiment Video
Updated: Apr 18, 2026
09:45
A Protocol for Safe Lithiation Reactions Using Organolithium Reagents
Published on: November 12, 2016
32.4K
One lithium atom binding with P-nitroaniline: lithium salts or lithium electrides?
Ying Gao1, Heng-Qing Wu, Shi-Ling Sun
1Institute of Functional Material Chemistry, Faculty of Chemistry, Northeast Normal University, Changchun, 130024, Jilin, People's Republic of China.
Journal of Molecular Modeling
|January 27, 2015
Summary
Researchers explored lithium (Li) configurations with p-nitroaniline (PNA). They found one configuration, 3-Li-PNA, exhibits properties of both Li salts and Li electrides, and possesses exceptionally high hyperpolarizability.
Area of Science:
- Computational Chemistry
- Materials Science
- Quantum Chemistry
Background:
- Lithium (Li) salts and Li electrides are actively researched materials.
- Distinguishing between Li salts and Li electrides in specific configurations remains an open question.
Purpose of the Study:
- To investigate the nature of Li atom interactions with p-nitroaniline (PNA).
- To explore whether specific Li-PNA configurations represent Li salts, Li electrides, or a hybrid.
Main Methods:
- Computational modeling of four Li-PNA configurations (n-Li-PNA, n=1-4).
- Analysis using the ROMP2 method to determine electronic properties and stability.
- Calculation of vertical ionization potential (VIP) and interaction energy (E int).
Main Results:
- 1-Li-PNA and 2-Li-PNA were identified as typical Li salts.
- 4-Li-PNA was classified as a typical Li electride.
- 3-Li-PNA demonstrated characteristics of both Li salts and Li electrides, exhibiting the largest first hyperpolarizability (2.9 × 10^6 au).
- 3-Li-PNA's hyperpolarizability is approximately 2600 times greater than that of PNA.
Conclusions:
- The study successfully differentiates Li salt and Li electride characteristics in Li-PNA systems.
- The 3-Li-PNA configuration presents a unique hybrid material with significant nonlinear optical potential.
- Stability analysis indicates 3-Li-PNA is less stable than typical Li salts but more stable than typical Li electrides.
Related Concept Videos
00:55Nitriles to Amines: LiAlH4 Reduction
5.2K
Nitriles are reduced to amines in the presence of strong reducing agents like lithium aluminum hydride through a typical nucleophilic acyl substitution. The reaction requires two equivalents of the reducing agent. The reducing agent acts as a source of hydride ions.
As shown below, the mechanism involves three steps. Firstly, the hydride ion acting as a nucleophile attacks the nitrile carbon to form an anion. In the second step, a second equivalent of the hydride ion attacks the anion to...
As shown below, the mechanism involves three steps. Firstly, the hydride ion acting as a nucleophile attacks the nitrile carbon to form an anion. In the second step, a second equivalent of the hydride ion attacks the anion to...
5.2K
01:10α-Alkylation of Ketones via Enolate Ions
4.2K
Ketones with α protons are deprotonated by strong bases like lithium diisopropylamide (LDA) to form enolate ions. The anion is stabilized by resonance, and its hybrid structure exhibits negative charges on the carbonyl oxygen and the α carbon. This ambident nucleophile can attack an electrophile via two possible sites: the carbonyl oxygen, known as O-attack, or the α carbon, known as C-attack. The nucleophilic attack via the carbanionic site is preferred. This is due to the...
4.2K
01:20Amides to Amines: LiAlH4 Reduction
6.8K
Amide reduction with strong reducing agents like lithium aluminum hydride proceeds through a nucleophilic acyl substitution to form amines. Primary, secondary, and tertiary amides yield primary, secondary, and tertiary amines, respectively.
Amide reduction requires two equivalents of the reducing agent, acting as a source of hydride ions. As shown in the figure, the reaction is initiated with a nucleophilic attack by the hydride ion at the carbonyl carbon to form a tetrahedral intermediate.
Amide reduction requires two equivalents of the reducing agent, acting as a source of hydride ions. As shown in the figure, the reaction is initiated with a nucleophilic attack by the hydride ion at the carbonyl carbon to form a tetrahedral intermediate.
6.8K
01:13Preparation of Amines: Reduction of Amides and Nitriles
3.3K
Nitriles can be reduced to primary amines using reducing agents like lithium aluminum hydride or catalytic hydrogenation. The reduction introduces an amino group with an extra carbon in the skeleton. Nitriles are formed from the reaction between alkyl halides and sodium cyanide through the SN2 mechanism. Primary alkyl halides are the preferred substrates to prepare nitriles.
Amides can be reduced to primary, secondary, and tertiary amines using catalytic hydrogenation, active metals like Fe,...
Amides can be reduced to primary, secondary, and tertiary amines using catalytic hydrogenation, active metals like Fe,...
3.3K
02:48Ionic Bonding and Electron Transfer
56.2K
Ions are atoms or molecules bearing an electrical charge. A cation (a positive ion) forms when a neutral atom loses one or more electrons from its valence shell, and an anion (a negative ion) forms when a neutral atom gains one or more electrons in its valence shell. Compounds composed of ions are called ionic compounds (or salts), and their constituent ions are held together by ionic bonds: electrostatic forces of attraction between oppositely charged cations and anions.
56.2K
02:51Metal-Ligand Bonds
25.9K
The hemoglobin in the blood, the chlorophyll in green plants, vitamin B-12, and the catalyst used in the manufacture of polyethylene all contain coordination compounds. Ions of the metals, especially the transition metals, are likely to form complexes.
In these complexes, transition metals form coordinate covalent bonds, a kind of Lewis acid-base interaction in which both of the electrons in the bond are contributed by a donor (Lewis base) to an electron acceptor (Lewis acid). The Lewis acid in...
In these complexes, transition metals form coordinate covalent bonds, a kind of Lewis acid-base interaction in which both of the electrons in the bond are contributed by a donor (Lewis base) to an electron acceptor (Lewis acid). The Lewis acid in...
25.9K