When we think of in molecules, we assume the (valence) electrons are shared between the two bonded atoms (only). This electrons, which "belong" to the bonded atoms are said to...
The reason as to why metallic posses these properties is because the electrons do not stay in their assigned orbitals, they become delocalised and move all over the place....
Most metals have melting points that are accessible in a laboratory or at least in a forge or metal foundry. A few metals are even liquid at room temperature. Caesium...
And the prevailing of metals does tend to account for the these properties. Metals are often described as $"positive ions in a sea of electrons"$. Each metal ATOM...
But caesium and mercury are certainly room temperature LIQUIDS. That metals exist in condensed phases under standard conditions is a consequence of , which is a non-molecular force of interaction,...
$"Metallic bonding"$ consists of an array of close-packed metal atoms, which each contribute one or two or more electrons to the overall metallic lattice. And the result is the familiar...
are usually made of a metal cation and a nonmetal anion. Anions can be negatively charged ions made from , such as the oxide ion ($"O"^(2-)$), or chloride ion...
Metals generally have a valence electron that isn't strongly attracted to the nucleus allowing it to "flow" around the compound. This is the reason metals are so good at...
Metal are typically , in which a metal cation is ionically bonded to an anion. The anion can be from a single element, such as chlorine, or it can be...
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