Ionic Bonds

  1. Chemical Bond
    Force that holds two atoms together
  2. Ionization Energy
    How easy an atom loses it's electron
  3. Electron Affinity
    How much attraction the atom has for it's electron
  4. Chemical reactivity is directly related to ________
    Valence electrons
  5. Why do elements react with each other?
    So they can acquire a stable 8 electron structure in their outermost layer
  6. Which group of elements don't react much? Why?
    • Noble Gases
    • Because they are already chemically stable because they have a full outermost shell
  7. Cation
    A positively charged ion
  8. Anion
    A negatively charge ion
  9. What suffix is added to an anion when writing the formula?
  10. Ionic Bond
    Force that holds oppositely charged particles together in an ionic compound
  11. Ionic Compounds
    Compounds that contain ionic bonds
  12. Most ionic bonds are _______
    • Binary
    • Meaning they contain only two different elements
  13. What are binary ionic compounds made of?
    A metallic cation and a nonmetallic anion
  14. Ionic Crystal
    • Structure of alternating cations and anions
    • Large numbers of ions together in ratio according to how many electrons needed to be transfered
    • Vary in shape according to the size and relative numbers of the ions bonded
  15. Crystal Lattice
    • 3-D geometric arrangement of particles
    • Each anion is surrounded by cations and visa versa
  16. Name 7 properties of ionic compounds
    • High melting and boiling point
    • Hard
    • Rigid
    • Brittle
    • Bad conductors of electricity in solid state
    • Conductors of electricity in aqueous state
  17. Endothermic
    When energy is absorbed during a chemical reaction
  18. Exothermic
    • When energy is released during a chemical reaction
    • Formation of ionic compounds from positive and negative ions
  19. Which has more energy: individual ions or oppositely charged ions that are bonded?
    Individual ions have more energy because ions that are bonded are more stable
  20. How much energy is needed to break an ionic compound?
    If the amount of energy released during bond formation is added to the ionic compound, the bond breaks
  21. Lattice Energy
    The energy required to separate one mole of the ions of an ionic compound
  22. What are two factors that lattice energy is related to?
    • Size: smaller ions have higher lattice energy
    • Charge of the ion: ionic bond formed by ions with a larger positive or negative charges have higher lattice energy
  23. Formula Unit
    The simplest ratio of the ions represented in an ionic compound
  24. Monatomic ion
    A one-atom ion
  25. Oxidation number (state)
    Is the charge of a monatomic ion
  26. Polyatomic ions
    Ions made up of more than one atom
Card Set
Ionic Bonds
Chapter 8