Metallic Bonding Research Paper

865 Words4 Pages
Shadi Salem
Bonding in Metals

Bonding in metals, also known as, metallic bonding is a chemical bond between a metallic element’s atoms, which forms when its valence electrons move freely through the material. It is the sharing of positively charged ions. This chemical bond is what holds the metal’s atoms together and in place.
Along the creation of quantum mechanics, metallic bonds were given more formal interpretation through the free electron model and its extension, the nearly free electron model. Hume-Rothery attempted to explain why intermetallic alloys with certain compositions and others would not. With the beginning of x-ray diffraction, construction of phase diagrams, and thermal analysis, it is possible to study the composition,
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Metallic radii decrease across the period due to the increase in nuclear charges, and increase down the group due to the increase in quantum number.

When it comes to comparing metallic bonds and ionic bonds, they are generally similar in strength. Bond strength is measured for energy that is needed to break it. Ionic bonds’ trends are having higher melting points and chemical inertness; therefore, ionic bonds are stronger. In metallic bonds, the valence electrons from s and p orbitals delocalize. So they form a “sea” where they can move freely around the nuclei instead of orbiting their atoms.

Metallic bonding in complicated compounds does not necessarily mean that part of the elements are equal. It is possible to have an element or more to not join in. It is also possible to see which of the elements join by looking at the core levels in an x-ray photoelectron spectroscopy spectrum. If an element joins, its peaks
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When metal clusters are formed, it is seen as a way for the metal do localize its electron bonding. Hydrogen is an example of this localization, because it becomes metal at high pressures. At lower pressures it becomes localized into a covalent bond. Another related phenomenon are the charge density

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