Please do not explain the theory of metallic bonding. I just need straightforward chemical names. "Eg: NaCL for ioninic bonding". I've seen similar questions asked, but answers turned out to be explaining what it is and the properties. I just need the two metal chemical names.
THanks.
2007-03-01 00:30:37 · 2 answers · asked by Anonymous in Science & Mathematics ➔ Chemistry
Just name any two metals - as they metallicly bond with themselves - similar to covalent bonding in non-metallics.
i.e. Iron (Fe), Lithium (Li), Potassium (K), Gold (Au), Silver (Ag) etc..
you could name alloys such as Brass, which is an alloy of Copper and Zinc (CuZn) or even Terfenol-D (a magnetostrictive alloy) which is TbDyFe - Terbium, Dysprosium and Iron.
Hope this helps my good man...
2007-03-01 00:49:36 · answer #1 · answered by Doctor Q 6 · 0⤊ 0⤋
The crystal lattice of metals consists of ions NOT atoms surrounded by a 'sea of electrons' forming another type of giant lattice.
The outer electrons (-) from the original metal atoms are free to move around between the positive metal ions formed (+).
These free or 'delocalised' electrons are the 'electronic glue' holding the particles together.
There is a strong electrical force of attraction between these mobile electrons (-) and the 'immobile' positive metal ions (+) and this is the metallic bond.
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The physical properties of metals:
This strong bonding generally results in dense, strong materials with high melting and boiling points.
Usually a relatively large amount of energy is needed to melt or boil metals. Energy changes for the physical changes of state of melting and boiling for a range of differently bonded substances are compared in a section of the Energetics Notes.
Metals are good conductors of electricity because these 'free' electrons carry the charge of an electric current when a potential difference (voltage!) is applied across a piece of metal.
Metals are also good conductors of heat. This is also due to the free moving electrons. Non-metallic solids conduct heat energy by hotter more strongly vibrating atoms, knocking against cooler less strongly vibrating atoms to pass the particle kinetic energy on. In metals, as well as this effect, the 'hot' high kinetic energy electrons move around freely to transfer the particle kinetic energy more efficiently to 'cooler' atoms.
Typical metals also have a silvery surface but remember this may be easily tarnished by corrosive oxidation in air and water.
Unlike ionic solids, metals are very malleable, they can be readily bent, pressed or hammered into shape. The layers of atoms can slide over each other without fracturing the structure (see below). The reason for this is the mobility of the electrons. When planes of metal atoms are 'bent' or slide the electrons can run in between the atoms and maintain a strong bonding situation. This can't happen in ionic solids.
For more on the properties and uses of metals see Transition Metals and Extra Industrial Chemistry pages and the note and diagram below.
2007-03-01 00:40:20 · answer #2 · answered by jtaylor1993 5 · 0⤊ 0⤋