A metallic bond is the bond formed between atoms of metals in the matrix of their structure. It could be atoms of the same metal, or atoms of different metals in a mixture called an alloy. The heart of the metallic bond is the sharing of electrons by different atomic nuclei. It works sorta like this. A couple of atoms of one metal snuggles up to another atom of that metal when the atoms are molten and being cooled. As they cool and solidify, an electron or two (depending on the metal) of one atom are "pulled over" near the other two atoms and they all share the electron(s). The electron(s) involved are said to be delocalized. This sharing of delocalized electrons "ties the atoms together" and gives the solid metal strength and contributes to a number of its physical properties. It may be beneficial to visualize the metal matrix as a bunch of positive ions (the metal atoms) set up in a metallic crystal structure with electrons being "hung onto" by the positive ions and giving the whole structure its "stick togetherness" and strength. A link to the Wikipedia article on the metallic bond is provided. At least slide over and read the first paragraph of the article. It will provide some clarity and help lock in the concept.
Electron pairs
VSEPR theory stands for Valence Shell Electron Pair Repulsion theory. It is a model used to predict the geometry of molecules based on minimizing the repulsion between electron pairs in the valence shell of an atom. By considering the repulsions between electron pairs, VSEPR theory helps determine the shape of molecules.
Dalton's theory proposed that atoms are indivisible and have no subatomic particles, which was not supported by Thomson's discovery of the electron. Thomson's findings showed that atoms contain subatomic particles, challenging the notion of indivisible atoms in Dalton's theory.
1.Electron do not contribute to d repulsion force around d central atom
VeSPER theory, which stands for Valence Shell Electron Pair Repulsion theory, is a model used to predict the molecular geometry of molecules based on the repulsion of electron pairs in the valence shell of an atom. It helps to determine the shape of a molecule by considering the arrangement of bonding and nonbonding electron pairs around the central atom. It is a useful tool in understanding the properties and behavior of molecules in chemistry.
Electron pool theory was proposed by Gilbert Lewis. He suggested that in certain chemical reactions, electrons are shared and not tied to specific atoms, forming a "pool" of electrons that can be used by multiple atoms. This theory played a significant role in the development of our understanding of chemical bonding.
write note on free electron theory
Electronic theory is the theory of the behavior of the electron under various conditions including a free electron, a bound electron in either an outer or inner orbit of the atom.
the same way an insulator and a conductor will work with out the electron theory!
There is no single unified theory that explains all correlated electron systems.
Classical free electron theory could not explain many physical properties. In 1928, Sommerfeld developed a new theory applying quantum mechanical concepts and Fermi-Dirac statistics to the free electrons in the metal. This theory is called quantum free electron theory.
an atom
Rutherford.
Electron pairs
free electron model not take into account the potential neither the electron interaction. nearly free electron take into account the potential.J.C. Aguiar
VSEPR theory stands for Valence Shell Electron Pair Repulsion theory. It is a model used to predict the geometry of molecules based on minimizing the repulsion between electron pairs in the valence shell of an atom. By considering the repulsions between electron pairs, VSEPR theory helps determine the shape of molecules.
acid: electron pair acceptor Base: electron pair donor