Quizlet Chemistry Ch 6

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  1. Bond Energy: then energy required to break a chemical bond and form neutral isolated atoms
  2. Bond Length: the distance between two bonded atoms at their minimum potential energy
  3. Chemical Bond: a mutual electrical attraction between the nuclei and valence electrons of different atoms that binds the atoms together
  4. Chemical formula: indicates the relative numbers of atoms of each kind in a chemical compound by using atomic symbols and numerical subscrpts
  5. Covalent Bonding: the sharing of electron pairs between two atoms
  6. Diatomic Molecule: a molecule with only two atoms
  7. Dipole: created by equal but opposite charges that are seperated by a shore distance
  8. Dipole-Dipole: the forces of attraction between polar molecules
  9. Electron dot nNotation: an electron-configuration notation in which only the valence electrons of an atom of a particular element are shown, indicated by the dots placed around the elements
  10. Formula Unit: the simplest collection of atoms from which an ionic compound's formula can be established
  11. Hybridization: the mixing of two or more atomic orbitals of similar energies on the same atom to produce new orbitals of equal energies
  12. Hydrogen Bonding: the intermolecular force in which a hydrogen atom that is bonded to a highly electronegative atom is attracted to an unshared pair of electrons and electronegative atom in a nearby molecule
  13. Ionic Bonding: chemical bonding that results from the electrical attraction between large numbers of cations and anions
  14. Ionic Compound: composed of postivite and negative ions that are combined so that the numbers of positive or negative charges are equal
  15. Lattice Energy: the energy relased when one mole of an ionic crystalline compound is formed from gaseous ions
  16. Lewis Structures: formulas in which atomic symbols represent nuclei and inner-shell electrons, dot-pairs or dashes between two atomic symbols represent electron pairs in covalent bonds and dots adjacent to only one atomic symbol represent unshared electron
  17. London Dispersion Forces: the intermolecular attractions resulting fromt he constant motion of electrons and the creation of instantaneous dipoles
  18. Molecular compound: a chemical compound whose simplest units are molecules
  19. Molecular Formula: types and numbers of atoms combined in a single molecule of a molecular compound
  20. Molecular Polarity: the uneven distribution of molecular charge
  21. Molecule: a neutral group of atoms that are held together by covalent bonds
  22. Non-polar covalent bond: a covalent bond in which the bonding electrons are shared equally by the bonded atoms, resulting in a balanced distribution
  23. Octed Rule: Chemical compounds tend to form so that each atom by gaining losing sharing electrons has an octet of electrons in its highest occupied energy level
  24. Polar: having uneven distribution of charge
  25. Polar-covalent Bond: a covalent bond in which the bonded atoms have an unequal attraction for the shared electrons
  26. Single Bond: a covalent bond produced by the sharing of one pair of electrons between two atoms
  27. Structural Formula: indicates the kind number arrangement bonds but not the unshared pairs of the atoms in a molecul
  28. Unshared Pair: a pair of electrons that is not involved in bonding and that belongs exclusively to one atom; une pair
  29. VSEPR theory: repulsion between the sets of valence level electrons surrounding an atom causes thses sets to be oriented as far apart as possible