Structure and bonding in metals

• What is the main characteristic of metals that allows them to conduct electricity?

  They have delocalised electrons.
• How does the structure of metals contribute to their high melting and boiling points?

  The strong metallic bonding requires large amounts of energy to overcome.
• What is the definition of metallic bonding?

  Bonding in metal elements consisting of a giant structure of metal atoms and their delocalised electrons.
• Why are metals good conductors of thermal energy?

  Because their delocalised electrons transfer energy through the metal.
• What are the physical properties of metals mentioned in the study material?

  They are electrical conductors, good conductors of thermal energy, and have high melting and boiling points.
• What is the role of delocalised electrons in metallic bonding?

  They are free to move through the whole structure, resulting in strong metallic bonding.
• What are the properties of metals that result from their structure and bonding?

  • Electrical conductors due to delocalised electrons
  • Good conductors of thermal energy
  • High melting points
  • High boiling points
• What is the smallest part of an element that can exist?

  An atom.
• How does the arrangement of atoms in metals contribute to their properties?

  Atoms are arranged in a regular pattern, contributing to their strength and conductivity.
• What is the definition of a conductor in the context of metals?

  A material which allows charge to move easily through it.
• Why do metals have a shiny appearance?

  Because of their ability to reflect light due to their electron structure.
• How does the presence of delocalised electrons affect the conductivity of metals?

  Delocalised electrons allow for the easy movement of electrical charge through the metal.
• What is the significance of the term "giant structure" in relation to metals?

  It refers to the large arrangement of atoms in a metal that contributes to its properties.
• What happens to the outer electrons of metal atoms in metallic bonding?

  They become delocalised and are free to move through the structure.
• How does the strong metallic bonding in metals affect their physical properties?

  It results in high melting and boiling points due to the energy required to break the bonds.