Chapter 7 Ionic Bonding 83A

• Covalent bond is formed by shared electrons
• Metals are said to have noble electrons
• Double bond consists of 2 pairs of shared electrons
• Charged particle is formed when an atom gains or loses one or more valence electrons
• Valence electrons diagram shows how electrons are transferred
• Nonpolar covalent bond: electrons are shared equally between atoms
• Ionic compounds will react to end up with a set of valence electrons, similar to noble gases
• Polar molecule has one pole that is partly negatively charged and one pole that is partly positively charged, acting like a little magnet with large intermolecular forces
• Molecule is also known as a molecular compound
• Symmetrical molecule has identical parts on each side of each axis
• Metal atoms allow their valence electrons to freely move throughout the structure
• Metals are good conductors of charged particles
• Chapter 7 - Ionic Bonding
• Covalent bond is a bond between two atoms that is formed by shared electrons
• Substances conduct electricity when charged particles move freely through them
• Asymmetrical molecule lacks symmetry about at least one axis
• Covalent compound formation


  Formed when the atoms of a molecule share electrons in order to bond together
• Polar (covalent) bond: electrons are shared unequally between two atoms due to different electronegativities
• Octet (8 valence) electrons make atoms "happy or stable"
• Electronegativity is the attraction of an atom for shared electrons in a bond
• Triple bond consists of 3 pairs of shared electrons
• Dipole


  A molecule that is polar
• Hydrogen bonding is not an actual bond
• Water exhibits hydrogen bonding between molecules
• Hydrogen bonding


  A very strong intermolecular force between very polar molecules
• Intermolecular force


  An attractive force between molecules
• VSEPR theory

  A theory that helps us to determine the shape of molecules by saying that electron pairs repel each other and want to be as far apart as possible, thus determining the molecular shape
• Examples of elements that exhibit hydrogen bonding

  • Hydrogen
  • Fluorine
  • Oxygen
  • Nitrogen
• Structural formula


  A formula that represents covalent bonds with dashes and shows the arrangement of covalently bonded atoms