Chemical bonding

• Compound


  Substance made up of 2 or more elements chemically combined
• Compound


  • Stability
  • Full energy level
  • Valence outermost 2 filled sublevel
• Ionic Bonding


  Chemical bonding where electrons are completely transferred from one atom onto another, forming ions
• Covalent Bonding


  Chemical bonding where electrons are shared between atoms
• Atoms will tend to lose, gain or share electrons in order to get a full outer shell</b>
• Intermolecular Bonding


  Bonding between molecules, including van der Waals, dipole-dipole, and hydrogen bonding
• Hydrogen bonding occurs when hydrogen is bonded to highly electronegative elements like N, O, or F
• Crystal Lattice


  Ions arranged in a regular repeating structure
• Electronegativity Difference


  Measure of an atom's ability to attract shared electrons in a covalent bond
• Types of Bonding


  • Pure covalent (electronegativity difference < 0.3)
  • Polar covalent (electronegativity difference 0.3-1.5)
  • Ionic (electronegativity difference > 1.5)
• Covalent Bonds


  • Sigma orbitals overlap head-on
  • Pi orbitals overlap in parallel
• Covalent Bond Types


  • Single
  • Double
  • Triple
• Polar Bond


  One end slightly negative, one end slightly positive
• VSEPR Theory


  Pairs of electrons arrange themselves as far away from each other as possible
• Molecular Shapes


  • Linear
  • Trigonal planar
  • Tetrahedral
  • Trigonal bipyramidal
  • Octahedral
• Ion: a charged atom or group of atoms.
• Transition metal: one that forms at least one ion with a partially filled d sublevel.
• Molecule: a group of atoms joined together. The smallest particle of an element or compound that can exist independently.
• Law of conservation of mass


  States that the total mass of the products of a chemical reaction is the same as the total mass of the reactants.
• Law of conservation of matter


  States that in any chemical reaction, matter is neither created or destroyed but merely changes from one form into another.