Why are all the transition elements metallic?

Answer 1

this may not be what you were looking for but all of the elements on the periodic tables are metals instead of a special area called the nonmetals which are between the transitions and the noble gases. They make a stair like shape from like Boron and down

Answer 2

Wow, this question is almost philosophical in nature. (Praying to God it's someone with actual scientific curiosity instead of copying some essay question out of your exam, but in any case....)

What are the things that make people think of metals: shiny colors, high mp/bp, usually pretty tough, and conduct electricity. All of those things result from one aspect of all the transition elements: the fact that the d (and f) electrons are not held nearly as tightly as s and p electrons. Because of this the elements in their natural form instead of forming distinct bonds end up sharing all their valence electrons across the entire bulk of the solid (that means if you have a yard long piece of pure metal, you actually have electrons that are "a yard long"--the wavefunction describing their orbital is a yard long, meaning they are localized across the entire size of the piece of metal).

The delocalized nature of the electrons (they essentially act like a glue) accounts for all the properties we associate with metals; the high mp/bp, high tensile strength, the fact that they conduct electricity (and temperature) really well, etc. If you've taken inorganic chemistry it's all a result of the shielding of the d and f electrons by the s and p electrons which are more tightly held.