2.1.3 Metallic bonding in metals

• What are positive metal ions called?

  Positive metal ions
• What are the key features of metallic bonding structure?

  • Regular array of metal ions
  • Surrounded by an electron sea
  • Delocalized electrons flow freely
  • Ions arranged in sliding layers
• How does metallic bonding differ from ionic bonding?

  Electrons are shared in metallic bonding
• If you wanted to calculate the area of a circle with radius $r =$$5\text{ cm}$, what formula would you use?


  $A =$$\pi r^2 =$$25\pi \text{ cm}^2$
• What type of particles are indicated by "-" symbols in the image?

  Electrons
• What type of particles are indicated by "+" symbols in the image?

  Positive ions
• How do the delocalized electrons in the Electron Sea Model contribute to the properties of metals?

  • The delocalized electrons allow for electrical conductivity in metals
  • The free movement of electrons also contributes to the high thermal and electrical conductivity of metals
  • The delocalized electrons help hold the metal ions together, giving metals their characteristic strength and malleability
• What are the three main types of bonding?

  Metallic, ionic, and covalent
• How are metal ions arranged in metallic bonding?

  In layers that can slide over each other
• What is the characteristic of the metallic structure?

  Strong metallic structure
• How do delocalised electrons contribute to the properties of metals?

  • High electrical conductivity
  • High thermal conductivity
  • Malleability
  • Ductility
• What are the positively charged particles shown in the Electron Sea Model?

  Metal ions
• What are the characteristics of covalent bonding?

  • Involves non-metal + non-metal atoms
  • Electrons are shared between atoms
• According to the image, how are the positive ions arranged initially?

  In a lattice structure
• What surrounds the metal ions in metallic bonding?

  Electron sea of delocalized electrons
• What properties are affected by the type of bonding?

  • Electrical conductivity
  • Melting points
  • Overall strength
• How does the ability to conduct electricity and heat differ between metallic, ionic, and covalent bonding?

  Metallic bonding can conduct electricity and heat, ionic bonding may conduct depending on the state, and covalent bonding may conduct depending on the atoms.
• What is metallic bonding?

  A type of bonding in metals
• What is one characteristic of copper?

  Excellent conductivity
• What are the key characteristics of metallic bonding?

  • Delocalized electrons
  • Sea of electrons surrounding metal ions
  • Electrons are shared and mobile
  • Allows conduction of electricity and heat
• What are the key differences in melting and boiling points between metallic, ionic, and covalent bonding?

  • Metallic bonding has high melting and boiling points
  • Ionic bonding also has high melting and boiling points
  • Covalent bonding has low melting and boiling points
• What are the key differences in how the atoms interact in metallic, ionic, and covalent bonding?

  In metallic bonding, atoms release their electrons to become cations, in ionic bonding atoms give off or accept electrons, and in covalent bonding atoms share electrons.
• What holds the ions together in metals?

  Strong metallic bonds
• How does the Electron Sea Model differ from other models of metallic bonding?

  The Electron Sea Model shows delocalized electrons surrounding metal ions, unlike other models that depict localized bonds between atoms
• What is the structure of metals described as?

  Sea of electrons
• What does it mean for electrons to be delocalized in metallic bonding?

  Electrons are free to move between metal atoms
• What are the characteristics of ionic bonding?

  • Involves metal + non-metal atoms
  • Electrons are transferred between atoms
• 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 the three bond types differ?

  Based on how electrons are shared between atoms
• What can the layers of positive metal ions do?

  The layers can slide over each other
• Why do copper and iron have similar properties?

  They share a common electron sea
• Why do atoms seek stability in all three types of bonding?

  Atoms seek stability by attaining a full valence electron shell through bonding.
• What is the name of the model shown in the image?

  Electron Sea Model
• What does it mean for iron to be malleable?

  It can be shaped into different products
• What are the key properties of metals due to metallic bonding?

  • Conduct electricity well
  • Conduct heat effectively
  • Be malleable and ductile
  • Have a strong metallic structure
• How does the strength of the bond differ between metallic, ionic, and covalent bonding?

  • Metallic bonding can be bent without breaking
  • Ionic bonding easily breaks
  • Covalent bonding's strength depends on the atoms involved
• Why can metals conduct electricity and heat easily?

  Because electrons are shared and mobile
• What kind of structure is depicted in the image?

  Metallic structure:

  • Positive ions arranged in a lattice
  • Surrounded by a "sea" of delocalised electrons
• What are two characteristics of iron?

  Malleable and ductile
• What property allows metals to be malleable and ductile?

  Layers can slide past each other