Metals are good conductors because they have many free electrons. How are these free electrons obtained?

Sodium $Na_11^23$ is so reactive that if sodium metal is placed in water it will react vigorously to produce Hydrogen gas and heat often causing an explosion. All of...

And the hydroxides of metals are usually bases... And a few oxo-acids are $(HO)_2S(=O)_2$, $(HO)_3P=O$, $HOstackrel+N(=O)O^(-)$, and $(O=)_3ClOH$...what are the conventional names of these acids? On the other hand, when...

A metalloid is an element whose properties are "in between" those of . For example, metals are excellent electothermal conductors, and nonmetals are non-conductors. Metalloids are described as semiconductors....

Metals are excellent conductors because the atoms in a metal form a matrix through which their outer electrons can move freely. Instead of orbiting their respective metal atoms, they form...

However, the classic representation of metals is of $"positive ions in a sea of electrons"$. Metals are thus conceived to be whose are somewhat delocalized, with each metal contributing 1...

Metals lose electrons to become positive ions. The elemental metals bond using which uses a sea of electrons to bond unlimited numbers of atoms together. Most are metals. magnesium, iron,...

Electrical conductivity in metals is a result of the movement of electrically charged particles. The atoms of metal are characterized by the presence of - electrons in the outer shell...

for discussion on atomic radii of the transition metals.

In terms of actual , there is literally only one example. You can consider that their oxidation states have never gotten higher than $+8$, except for Iridium: In terms...

$"Metallic bonding"$ 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...