5.9 Bonding Quiz Review Notes

5.9 Bonding Quiz Review

Part 1: Vocabulary Review

  • Valence Electrons:
    • Definition: C. Outer shell electrons involved in bonding.
  • Oxidation State:
    • Definition: I. A number assigned to an ion, representing the number of electrons lost or gained; the charge.
  • Covalent Bond:
    • Definition: A. Bond formed by sharing electrons between nonmetals.
  • Ion:
    • Definition: B. Charged particle formed by losing or gaining electrons.
  • Electronegativity:
    • Definition: E. The ability of an atom to attract electrons in a bond.
  • Polyatomic Ion:
    • Definition: F. A charged group of covalently bonded atoms, used in ionic bonding.
  • Subscript:
    • Definition: G. Number written below and to the right in a formula, shows # of atoms.
  • Prefix:
    • Definition: H. Word part used to indicate number of atoms in covalent compounds.
  • Ionic Bond:
    • Definition: D. Bond formed by transferring electrons from metal to nonmetal.
  • Ions Formation:
    • Atoms have a neutral charge.
    • When forming ionic bonds, atoms turn into ions, which do have a charge.
    • Cations are positively charged.
    • Anions are negatively charged.

Part 2: Ionic Bonding Practice

  • A. Naming Ionic Compounds
    • NaBr → Sodium Bromide
    • CaO → Calcium Oxide
    • Li₂S → Lithium Sulfide
    • MgCl₂ → Magnesium Chloride
    • FeCl₂ → Iron (II) Chloride (Iron is a polyvalent ion, so Roman numerals are used to indicate its charge)
  • B. Writing Ionic Formulas
    • Potassium chloride → KCl
    • Beryllium sulfide → BeS
    • Aluminum oxide → Al₂O₃
    • Calcium nitrate → Ca(NO₃)₂
    • Copper (II) Fluoride → CuF₂

Part 3: Covalent Bonding Practice

  • A. Naming Covalent Compounds
    • CO₂ → Carbon Dioxide
    • P₂O₅ → Diphosphorus Pentoxide
    • SF₆ → Sulfur Hexafluoride
    • N₂O₄ → Dinitrogen Tetroxide
  • B. Writing Covalent Formulas
    • Dinitrogen trioxide → N₂O₃
    • Carbon tetrachloride → CCl₄
    • Phosphorus pentabromide → PBr₅
    • Iodine heptafluoride → IF₇

Part 4: Drawing Bonds of Compounds

  • BeF₂
  • H₂O
  • SO₂
  • AlCl₃
  • NH₃
  • PF₅

Ionic Bonding Rules and Guidelines

  1. Non-metals at the end of a compound end in -ide.
  2. Polyatomic ions keep their names.
  3. Transition metals have Roman Numerals indicating their charges.

Covalent Bonding Rules and Guidelines

  1. Draw a skeletal structure
    • Make it as symmetrical as possible.
    • H and He are always terminal atoms.
    • Halogens and O are often terminal atoms.
    • Central atom is usually first and/or single.
  2. Count total number of valence electrons
  3. Place pairs of electrons between all atoms
  4. Place remaining electrons to fulfill octet rule.
  5. Unshared pairs of electrons go on the same side of the central atom
  6. If too few electrons, use a double or triple bond
  7. If too many electrons, “extra” go on central atom
Exceptions to Octet Rule
  • H, He only want 2 electrons
  • Be may take only 4
  • B, Al, Ga may take only 6
  • Families 13 to 18 (Periods 3-6) may take more than 8
Naming Rules
  1. The prefix mono is never used with the first element in the compound.
  2. The prefixes mono, tetra, penta, hexa, etc… LOSE their final “o” or “a” when placed in front of oxygen.
  3. The ending of the second element is again changed to –ide.

Additional Information for Quiz

  • You will be given:
    • Periodic table
    • Polyatomic ion chart
    • Prefixes used when naming covalent compounds
    • Exceptions to the octet rule
  • You are responsible for knowing the steps and rules of ionic and covalent bonding and naming.