Physical Properties of Metals

Eight question-and-answer flashcards covering metallic properties, bonding, and structure for exam revision.

What are the key physical properties common to most metals?

High melting and boiling points, good electrical conductivity, good thermal conductivity, malleability, ductility, lustrous appearance, and high density.

Why do metals have high melting and boiling points?

Strong metallic bonds—electrostatic attraction between positive metal ions and delocalised electrons—require a large amount of energy to break.

Why are metals good conductors of electricity?

They contain delocalised electrons that are free to move through the metallic lattice, allowing electric current to flow.

Why do metals conduct heat efficiently?

Delocalised electrons transfer kinetic energy quickly, and closely packed metal ions vibrate and pass heat energy through the lattice.

What structural feature of metals makes them malleable and ductile?

Layers of metal ions can slide over one another without breaking the metallic bond because delocalised electrons maintain electrostatic attraction during movement.

Why do metals exhibit a lustrous (shiny) appearance?

Delocalised electrons absorb and re-emit light, producing a reflective, shiny surface.

Why do metals generally have high density?

Metal ions are closely packed in a regular lattice, resulting in a high mass per unit volume.

How does the number of delocalised electrons influence metallic properties?

More delocalised electrons strengthen metallic bonding, raising melting point, hardness, and electrical conductivity.