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Related Concept Videos

Ionic Bonds00:42

Ionic Bonds

132.2K
Overview
When atoms gain or lose electrons to achieve a more stable electron configuration they form ions. Ionic bonds are electrostatic attractions between ions with opposite charges. Ionic compounds are rigid and brittle when solid and may dissociate into their constituent ions in water. Covalent compounds, by contrast, remain intact unless a chemical reaction breaks them.
Opposing Charges Hold Ions Together in Ionic Compounds
Ionic bonds are reversible electrostatic interactions between ions...
132.2K
Bonding in Metals02:32

Bonding in Metals

52.9K
Metallic bonds are formed between two metal atoms. A simplified model to describe metallic bonding has been developed by Paul Drüde called the “Electron Sea Model”. 
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Metal-Ligand Bonds02:51

Metal-Ligand Bonds

24.5K
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...
24.5K
Ionic Bonding and Electron Transfer02:48

Ionic Bonding and Electron Transfer

49.8K
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. 
49.8K
Types of Chemical Bonds02:37

Types of Chemical Bonds

94.6K
Chemical bonding theories were pioneered by American chemist Gilbert N. Lewis. He developed a model called the Lewis model to explain the type and formation of different bonds. Chemical bonding is central to chemistry; it explains how atoms or ions bond together to form molecules. It explains why some bonds are strong and others are weak, or why one carbon bonds with two oxygens and not three; why water is H2O and not H4O. 
94.6K
Bond Energies and Bond Lengths02:49

Bond Energies and Bond Lengths

31.6K
Stable molecules exist because covalent bonds hold the atoms together. The strength of a covalent bond is measured by the energy required to break it, that is, the energy necessary to separate the bonded atoms. Separating any pair of bonded atoms requires energy — the stronger a bond, the greater the energy required to break it.
31.6K

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Photoelectron Imaging of Anions Illustrated by 310 Nm Detachment of F&#8722;
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Photoelectron Imaging of Anions Illustrated by 310 Nm Detachment of F−

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Titanium Insertion into CO Bonds in Anionic Ti-CO2 Complexes.

Leah G Dodson, Michael C Thompson, J Mathias Weber

    The Journal of Physical Chemistry. A
    |March 8, 2018
    PubMed
    Summary
    This summary is machine-generated.

    Titanium cluster anions exhibit metal carbonyl CO stretching modes, indicating titanium atom insertion into C-O bonds. Oxalato ligands promote this C-O bond insertion, revealing titanium

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    Area of Science:

    • Inorganic Chemistry
    • Materials Science
    • Physical Chemistry

    Background:

    • Titanium cluster anions are of interest for their unique bonding and reactivity.
    • Understanding the formation pathways of these clusters is crucial for materials design.

    Purpose of the Study:

    • To elucidate the structures of titanium cluster anions, specifically [Ti(CO2)y]-.
    • To investigate the role of titanium in C-O bond insertion reactions during cluster formation.

    Main Methods:

    • Infrared photodissociation spectroscopy to probe vibrational modes.
    • Quantum chemistry calculations to determine stable structures and reaction mechanisms.

    Main Results:

    • Observed spectral signatures of metal carbonyl CO stretching modes, confirming titanium-carbon-oxygen bonding.
    • Identified oxalato, carbonato, and oxo ligands coordinated to the titanium center.
    • Demonstrated that metal oxalato ligands promote C-O bond insertion in these titanium systems.

    Conclusions:

    • Titanium readily inserts into C-O bonds, forming metal carbonyl species within cluster anions.
    • The presence of oxalato ligands is a key factor facilitating C-O bond insertion.
    • These findings underscore titanium's strong affinity for C-O bond activation and insertion reactions.