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Ionic and Metallic Bonds Review

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Terms in this set (20)

  • What is an ionic bond?
    An ionic bond is a chemical bond formed by the transfer of electrons from a metal to a nonmetal, resulting in oppositely charged ions that attract each other.
  • How do ionic bonds form?
    Ionic bonds form when one atom loses electrons to become a cation and another atom gains electrons to become an anion, creating electrostatic attraction.
  • What types of elements typically form ionic bonds?
    Ionic bonds usually form between metals (which lose electrons) and nonmetals (which gain electrons).
  • Describe the electron transfer in ionic bonding.
    In ionic bonding, electrons are transferred from the metal atom to the nonmetal atom, resulting in charged ions.
  • What is a metallic bond?
    A metallic bond is the attraction between metal atoms and the delocalized sea of electrons that move freely around them.
  • How do metallic bonds differ from ionic bonds?
    Metallic bonds involve a sea of delocalized electrons shared among metal atoms, while ionic bonds involve electron transfer and attraction between ions.
  • What properties result from metallic bonding?
    Metallic bonding gives metals properties like conductivity, malleability, ductility, and luster.
  • Why are ionic compounds generally solid at room temperature?
    Ionic compounds have strong electrostatic forces between ions, requiring high energy to break, so they are usually solid.
  • What is the role of electrostatic forces in ionic bonds?
    Electrostatic forces are the attractive forces between positively and negatively charged ions that hold ionic compounds together.
  • Explain the concept of a 'sea of electrons' in metallic bonding.
    The 'sea of electrons' refers to the delocalized electrons that move freely around metal cations, allowing conductivity and bonding.
  • How does electron configuration change in ionic bonding?
    Atoms achieve a stable electron configuration (often a full octet) by losing or gaining electrons in ionic bonding.
  • What is the typical charge on metal ions in ionic compounds?
    Metal ions typically have a positive charge (cations) because they lose electrons.
  • What is the typical charge on nonmetal ions in ionic compounds?
    Nonmetal ions typically have a negative charge (anions) because they gain electrons.
  • Why do metals conduct electricity in the solid state?
    Metals conduct electricity because their delocalized electrons can move freely through the metal lattice.
  • What is the difference between ionic and covalent bonds?
    Ionic bonds involve electron transfer and attraction between ions, while covalent bonds involve electron sharing between atoms.
  • How does the strength of ionic bonds compare to metallic bonds?
    Ionic bonds are generally stronger due to electrostatic attraction, while metallic bonds vary but allow flexibility.
  • What happens to the melting point of ionic compounds?
    Ionic compounds have high melting points because strong ionic bonds require much energy to break.
  • Can ionic compounds conduct electricity?
    Ionic compounds conduct electricity only when molten or dissolved because ions are free to move.
  • What is the lattice structure in ionic compounds?
    Ionic compounds form a crystal lattice where ions are arranged in a repeating 3D pattern to maximize attraction.
  • Why are metals malleable and ductile?
    Metals are malleable and ductile because the sea of electrons allows metal atoms to slide past each other without breaking bonds.