Chapter 6 Chem

  1. chemical bond
    mutual electrical attraction between the nuclei and valence electron of different atoms that binds them together
  2. covalent bond
    results from sharing of electrons pairs between two atoms
  3. ionic bond
    chemical bonding that results from the electrical attraction between cations and anions
  4. nonpolar covalent bond
    a covalent bond in which the bonding electron are shared equally by bonded atoms, resulting in a balanced distribution of electric charge
  5. polar
    uneven distribution of charge
  6. polar covalent bond
    covalent bond in which the bonded atoms have an unequal attraction for shared electrons
  7. bond energy
    energy required to break a chemical bond and form neutral isolated atom
  8. bond length
    average distance between two bonded atoms
  9. chemical formula
    indicates the relative numbers of atoms of each kind in a chemical compound by using atomic symbols and numerical subscripts
  10. Double bond
    covalent bond in which 2 pairs of electrons are shared between 2 atoms
  11. electron dot notation
    electron configuration notation in which only the valence electrons of an atom of a particular element are shown, indicated by dots around the element's symbol
  12. Lewis structure
    formulas in which atomic symbols represent nuclei and inner shell electrons, dot pairs or dashes between 2 atomic symbols represent electron pairs in covalent bonds and dots adjacent to only one atomic symbol represent unshared electrons
  13. lone pair
    pair of electrons that is not involved in bonding and that belongs exclusivley to one atom
  14. molecular compound
    chemical compund whose simplist units are molecules
  15. Molecule
    group atoms that are held together by chemical forces
  16. Multiple bond
    double or triple bonds
  17. octet rule
    chemical compounds tend to form so that each atom, by gaining, losing, or sharing electrons
  18. resonance
    bonding in molecules or ions that cant be correctly represented by a single lewis structure
  19. single bond
    covalent bond where on pair of electrons is shared between two atoms
  20. sturctural formula
    indicates the kind, number, arrangement, and bonds but not the unchared pairs o atoms in a molecule
  21. Triple Bond
    covalent bond in which 3 pairs of electrons are shared between 2 atoms
  22. formula unit
    simplest collection of atoms from which an ionic compunds formula can be established
  23. Ionic compound
    composed of positive and negative ions that are combined so that numbers of positive and negative charges are equal
  24. lattice energy
    energy released when one mole of an ionic compound is formed from gaseous ions
  25. Polyatomic ion
    an ion made of two or more atoms
  26. Ductility
    substance that can be drawn, pulled, or extrude through a small opening to produce a wire
  27. Malleability
    substance that can be hammered or beaten into thin sheets
  28. metallic bonding
    the chemical bonding that results from the attraction between metal atoms and surrounding sea of electrons
  29. VSEPR Theory
    repulsion between the sets of valence electrons levels and electrons surrounding an atom causes these to be oriented as far apart as possible
  30. Hybridization
    mixing of 2 or more atomic orbitals of similar energies on the same atom to produce new hybrid atomic orbitals of equal energies
  31. Hybrid orbitals
    orbitals of equal energy produced by the combination of two or more orbitals on the same atom
  32. Dipole
    created by equal but opposite charges that are seperated by a short distance
  33. Hydrogen bonding
    inter molecular force where a hydrogen bonded to a highly elegronegative atom is attracted to an unshared pair of electrons of an electronegative atom in a nearby molecule
  34. London Dispersion Forces
    intermolecular attractions resulting from the constant motion of electrons and the creation of instantaneous dipoles
Card Set
Chapter 6 Chem