Metals are good conducter of heat
Answers
Answer:
true because they allows heat to pass through them
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Answer:
Metallic bonds are made from a lattice of ions in a 'cloud' of free electrons. These free electrons are responsible for the ability of metals to
→conduct electricity
→conduct heat especially well.
Thermal conducivity
Metals are good conductors of heat. There are two reasons for this:
→the close packing of the metal ions in the lattice
→the delocalised electrons can carry kinetic energy through the lattice.
Explanation:
Ionic vibrations:
The positive metal ions in a metal structure are packed closely together in a symmetrical geometric arrangement. They don’t move from their position in the lattice but they are constantly vibrating. If a metal is heated, the positive metal ions vibrate more vigorously. These ions collide with neighbouring ions and make them vibrate more vigorously too. In this way, the energy is passed, or conducted, through the metal.
However, metals are particularly good conductors of heat. In general, they are better than ionic compounds which also have strong bonds. So we need another mechanism to explain their especially good conductivity. It is their free electrons.
Free electrons :
The ions in the lattice are vibrating . The ions at the hot end of a piece of metal vibrate more.
The electrons at the hot end will speed up – they gain kinetic energy from the vigorously vibrating ions.
Some of them will move down to the cooler end and collide with ions that are vibrating less vigorously than those at the hot end.
In these collisions, the electrons will lose kinetic energy and make the ions vibrate more vigorously.
In effect, the electrons have carried the vibrational energy from the hot end to the cold end. And, because they are free to move through the lattice, they are able to do this more quickly than the bonds between the ions in the lattice.