Metallic bonding

• What is metallic bonding?

  Sharing of outermost electrons by metal atoms
• How do delocalized electrons contribute to metallic bonding?

  They create a sea of electrons around positive ions
• What forces hold metal atoms together in metallic bonding?

  Strong electrostatic forces between positive ions and electrons
• What are the properties of metals regarding melting and boiling points?

  High melting and boiling points
• Why are metals good conductors of electricity and heat?

  Delocalized electrons facilitate energy transfer
• What does malleability in metals allow them to do?

  Be shaped without breaking
• What is the difference between pure metals and alloys?

  Alloys are mixtures of two or more elements
• How do different sized atoms in alloys affect their structure?

  They disrupt the regular structure of metals
• How does the hardness of alloys compare to pure metals?

  Alloys are generally harder than pure metals
• What are the key properties of metals?

  • High melting and boiling points
  • Excellent conductors of electricity and heat
  • Malleable and can be shaped without breaking
• What are the advantages of using alloys over pure metals?

  • Enhanced hardness and strength
  • Improved resistance to corrosion
  • Tailored properties for specific applications