Explain why metals are malleable

• What is the definition of malleability?

  Malleability is a metal's ability to change shape.
• What happens when you hit a piece of copper?

  It can be flattened to make it wider.
• What are the key differences between positive metal ions and negative ions?

  • Positive metal ions have a sea of delocalized electrons that can conduct electricity
  • Negative ions do not have this sea of delocalized electrons
• How are positive metal ions arranged in a metallic bond?

  They are arranged regularly
• What is the sea of delocalized electrons in positive metal ions?

  • A sea of electrons that can move freely between the positive metal ions
• How do delocalized electrons contribute to metallic bonding?

  They attract positive metal ions from all sides
• What is the effect of delocalized electrons on the flexibility of metals?

  They allow adjustment as metal ions rearrange
• What is the role of the electron sea in metallic structures?

  • Delocalized electrons move freely
  • Create strong bonding with metal ions
  • Allow for flexibility in the metal lattice
• How does the arrangement of positive metal ions and delocalised electrons in the image explain the electrical conductivity of metals?

  • The positive metal ions provide a regular lattice structure
  • The delocalised electrons can move freely through this lattice
  • This allows for the conduction of electricity in metals
• What is the significance of delocalized electrons in metallic bonding?

  They move freely between positive ions
• What is the relationship between the positive metal ions and the delocalised electrons in the image?

  • The positive metal ions are surrounded by the delocalised electrons
  • The delocalised electrons are able to move freely between the positive metal ions
  • This arrangement allows for the conduction of electricity in metals
• How are the atoms arranged in a pure metal compared to a metal alloy?

  • Pure metal: Atoms are arranged in a regular, repeating pattern
  • Metal alloy: Atoms are arranged in a more irregular, random pattern
• What can metal ions do when forces are applied?

  Slide past each other
• What is meant by delocalized electrons in metals?

  They move freely through the metal lattice.
• How does the delocalization of electrons affect their movement in metals?

  It allows electrons to flow easily between ions.
• Why can metal ions move without breaking bonds?

  Because of delocalized electrons
• If the positive metal ions were to be removed, how would this affect the delocalised electrons?

  The delocalised electrons would no longer be able to move freely and conduct electricity
• What allows the metal lattice to change shape?

  Delocalized electrons maintaining attraction
• What property of metals allows them to be shaped easily?

  Malleability
• How do individual layers of metal behave when hammered?

  They maintain their structure while sliding
• How does the presence of delocalized electrons contribute to the malleability of metals?

  They allow ions to move without breaking bonds
• What happens to a block of pure metal when hammered?

  It can be hammered into a sheet
• What is the significance of delocalized electrons in a molecule?

  • Delocalized electrons are not confined to a single bond or atom
  • They can move freely throughout the molecule
  • This allows for increased stability and reactivity
• What allows metal ions to slide past each other?

  Delocalized electrons
• What do delocalized electrons do when metal ions slide?

  Adjust instantly to maintain attraction
• How do metal ions slide past each other?

  Like cards in a deck
• What happens to the outer electrons in a metal atom?

  They become delocalized
• How can aluminum be shaped into foil?

  By rolling it, allowing ions to slide
• What happens to metal ions when you hammer a metal?

  They slip and align
• What is the difference between a pure metal and a metal alloy?

  • Pure metal: Consists of only one type of metal atom
  • Metal alloy: Consists of two or more types of metal atoms
• What is the process that allows metals to be malleable?

  • Atoms in metals can slide past each other
  • This sliding allows deformation without breaking
  • Results in the ability to form different shapes
• What is the result of metal ions slipping and aligning?

  The metal's shape changes without tearing
• What do scientists call the arrangement of delocalized electrons in metals?

  Electron sea.
• How does malleability allow metals to be shaped?

  Atoms can slide past each other easily.
• How does the movement of delocalized electrons affect the strength of the metal lattice?

  It provides flexibility and enhances strength
• How do the arrangements of atoms differ between the pure metal and metal alloy shown in the image?

  Pure metal has a regular, repeating pattern, while metal alloy has a more irregular, random pattern
• How do the properties of a pure metal differ from a metal alloy?

  • Pure metal: Higher electrical and thermal conductivity, lower strength
  • Metal alloy: Lower electrical and thermal conductivity, higher strength
• What can the layers of positive metal ions do?

  The layers can slide over each other
• What type of structure does a metal form?

  Lattice structure
• What is the process of metal ions sliding past each other under force?

  • Metal ions in layers slide past each other
  • Delocalized electrons adjust to maintain attraction
  • Metal lattice changes shape without breaking