Discovery of:

Bond cleavage refers to the breaking of chemical bonds between atoms in a molecule. This process is crucial in many chemical reactions, including those involved in organic synthesis, biochemistry, and various industrial processes. Bond cleavage can occur in several ways, primarily categorized as either homolytic or heterolytic cleavage: 1. **Homolytic Cleavage**: In this type of cleavage, the bond breaks symmetrically, resulting in the formation of two radical species.

Early electron diffraction experiment from 1927 that drastically confirmed the matter wave hypothesis.

The Bond Valence Method (BVM) is a semi-empirical approach used in solid-state chemistry and crystallography to analyze and predict the bonding characteristics of atoms in a crystal or molecular structure. It is particularly useful for understanding the distribution and strengths of bonds in complex materials, such as minerals and coordination compounds.

Inverted ligand field theory (ILFT) is a theoretical framework used to understand the electronic structure and behavior of transition metal complexes, particularly in the context of their crystal field environments. It is a modification of traditional ligand field theory (LFT), which focuses on the effects of the surrounding ligands on the energy levels of metal d-orbitals.

A carbon-carbon (C-C) bond is a chemical bond between two carbon atoms. These bonds can be found in various types of organic molecules and are fundamental to the structure of many compounds. There are three main types of carbon-carbon bonds: 1. **Single bonds (C-C)**: This is formed when two carbon atoms share one pair of electrons. This is the most common bond in organic compounds, such as in alkanes.

Thérèse Delpech was a prominent French intellectual and expert in international relations, particularly known for her work on nuclear policy and disarmament. Born in 1948 and passing away in 2012, she had a significant influence on discussions around French and global security issues. Delpech served as a director at the French Institute of International Relations (IFRI) and contributed to various scholarly publications on topics related to strategic studies and geopolitics.

The carbon-fluorine (C-F) bond is a chemical bond between carbon and fluorine atoms. It is characterized by several important features: 1. **Polarity**: The C-F bond is highly polar due to the significant difference in electronegativity between carbon (2.5) and fluorine (3.98). This polarity means that the bond has a partial negative charge on the fluorine atom and a partial positive charge on the carbon atom.

A charge-shift bond is a type of chemical bond that involves a transient shift of electron density between two atoms or groups, typically in a covalent bonding scenario. Unlike traditional covalent bonds, where electron sharing is more stable and constant, charge-shift bonds exhibit a dynamic feature where the electronic charge fluctuates between the bonding partners. This can occur due to external influences, such as electrical fields, changes in temperature, or the presence of reactive species.

Server run on the current machine. That's how all websites are developed and born!

Local symmetries appear to be a synonym to internal symmetry, see description at: Section "Internal and spacetime symmetries".

As mentioned at Quote , local symmetries map to forces in the Standard Model.

Appears to be a synonym for: gauge symmetry.

A local symmetry is a transformation that you apply a different transformation for each point, instead of a single transformation for every point.

TODO what's the point of a local symmetry?

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A carbon–hydrogen (C–H) bond is a covalent bond between a carbon atom and a hydrogen atom. This bond is fundamental in organic chemistry, as it is a key component of many organic molecules. ### Characteristics of C–H Bonds: 1. **Bonding**: The bond forms when carbon, which has four valence electrons, shares one of its electrons with hydrogen, which has one valence electron.

A carbon-nitrogen bond is a type of chemical bond that occurs between carbon (C) and nitrogen (N) atoms. This bond can be found in various organic and inorganic compounds, typically in the form of a single bond, double bond, or even triple bond, depending on the specific structure and context of the compound. **Characteristics of Carbon-Nitrogen Bonds:** 1.

A carbon–oxygen bond is a chemical bond between a carbon atom and an oxygen atom. This type of bond is fundamental in organic chemistry and biochemistry, as both carbon and oxygen are key elements in many biological molecules and organic compounds. There are two primary types of carbon–oxygen bonds: 1. **Single Bond (C–O)**: In this bond, one pair of electrons is shared between the carbon atom and the oxygen atom. This type of bond is seen in alcohols (e.

Cation–π interaction is a type of non-covalent interaction that occurs between a positively charged ion (cation) and the electron-rich π system of an aromatic ring or other π-conjugated systems. This interaction is significant in various fields, including chemistry, biochemistry, and molecular biology, as it plays a role in stabilizing molecular structures and contributing to the specificity of molecular recognition processes.

Cyclodipeptide synthases (CDPSs) are enzymes that catalyze the formation of cyclodipeptides, which are cyclic dipeptides. These compounds consist of two amino acids linked by a peptide bond, forming a cyclic structure. Cyclodipeptides can exhibit a variety of biological activities, including antimicrobial, antifungal, and anticancer properties, and are of interest for their potential pharmaceutical applications.

D-block contraction refers to a phenomenon observed in the periodic table, particularly in the transition metals, where the d-orbitals are involved in bonding and chemical behavior. More specifically, it often describes the decrease in the size of the atoms of transition metals as you move from left to right across a period, despite an increase in the number of protons in the nucleus. This contraction is primarily due to the poor shielding effect of the d-electrons.

A lone pair refers to a pair of valence electrons that are not shared with another atom and remain localized on a single atom. These electrons are often found in the outermost shell of an atom and can influence the atom's chemical behavior, including bond angles and molecular geometry. Lone pairs are important in the formation of molecular shapes, as they can repel other electron pairs (both bonding and lone pairs) according to the principles of VSEPR (Valence Shell Electron Pair Repulsion) theory.