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The video explains the unique properties of metals, focusing on their strong and flexible nature due to metallic bonding. Metal atoms form a lattice structure, losing electrons to become positive ions. These delocalized electrons create a sea of negative charge, allowing metals to conduct electricity and heat efficiently. The video also highlights metals' malleability and shiny appearance, making them both useful and attractive.

What makes metals both strong and flexible?

• Their unique bonding properties

• Their high melting point

• Their ability to conduct electricity

• Their shiny appearance

How do metal atoms form a lattice structure?

• By losing electrons to become positive ions

• By gaining electrons to become negative ions

• By sharing electrons with non-metals

• By forming covalent bonds

What is the role of delocalized electrons in metals?

• They give metals a dull appearance

• They make metals brittle

• They allow metals to conduct electricity

• They prevent metals from conducting heat

Why are metals good conductors of heat?

• Due to their shiny surface

• Because of their high density

• Due to the presence of free electrons

• Because they are malleable

What property allows metals to be shaped without breaking?

• Density

• Luster

• Conductivity

• Malleability