Metals & Alloys

• What should you be able to describe by the end of the video?

  Metallic bonding and the properties of pure metals and alloys
• Why are metals important in chemistry?

  They have significant applications and properties that are essential in various fields
• What is an example of pure metal shown in the video?

  A gold bar
• What is an example of an alloy mentioned in the video?

  A guitar string
• What happens to atoms when they become stable?

  They achieve a full outer energy level
• What type of bonding occurs when a metal atom reacts with a non-metal atom?

  Ionic bonding
• What type of bonding occurs when two non-metal atoms react?

  Covalent bonding
• How are atoms arranged in metals?

  In a giant structure arranged in regular layers
• What happens to the outer electrons in metal atoms?

  They are delocalized and free to move
• How many protons do lithium atoms have?

  Three protons
• What are delocalized electrons in metals?

  Electrons that are free to move through the whole structure
• What is the term used for the positive metal ions in metallic bonding?

  Positive metal ions
• What is the nature of the attraction between delocalized electrons and positive metal ions?

  It is a strong electrostatic attraction
• What is the term for the attraction in metals that is responsible for metallic bonding?

  Metallic bond
• Why do metals have high melting and boiling points?

  Because breaking strong metallic bonds requires a great deal of energy
• Why are metals excellent conductors of heat and electricity?

  Because delocalized electrons can move and carry charge
• What allows metals to conduct heat?

  Moving electrons can carry thermal energy
• What property allows metals to be bent and shaped?

  The layers of atoms can slide over each other
• Why are some pure metals not hard enough to be useful?

  Because they can be easily deformed
• What is an alloy?

  A mixture of metals
• How do different sizes of atoms in an alloy affect its properties?

  They distort the layers, making it harder for them to slide
• Why are alloys harder than pure metals?

  Because the distortion of layers makes it difficult for them to slide over each other
• What are the properties of metals and alloys?

  • High melting and boiling points
  • Excellent conductors of heat and electricity
  • Can be bent and shaped
  • Alloys are harder than pure metals
• What is the process of metallic bonding?

  1. Metal atoms lose their outer electrons
  2. Electrons become delocalized, forming a sea of electrons
  3. Positive metal ions are formed
  4. Strong electrostatic attraction occurs between delocalized electrons and positive ions