Chapter 6 Chemistry Vocabulary

  1. Mutual electrical attraction between the nuclei and valence electrons of different atoms that binds the atoms together
    Chemical Bond
  2. Chemical bonding that results from the electrical attraction between cations and anions
    Ionic Bonding
  3. Results from the sharing of electron pairs between two atoms
    Covalent Bonding
  4. A covalent bond in which the bonding electrons are shared equally by the bonded atoms, resulting in a balanced distribution of electrical charge
    Non-Polar Covalent Bond
  5. Have uneven distribution of charge
  6. A covalent bond in which the bonded atoms have an unequal attraction for the shared electrons
    Polar Covalent Bond
  7. A Neutral group of atoms that are held together by covalent bonds
  8. A chemical compound whose simplest units are molecules
    Molecular Compound
  9. Indicates the relative numbers of atoms of each kind in a chemical compound by using atomic symbols and numerical subscripts
    Chemical Formula
  10. Shows the types and numbers of atoms combined in a single molecule of a molecular compound
    Molecular Formula
  11. The energy required to break a chemical bond and form neutral isolated atoms
    Bond energy
  12. An electron-configuration notation in which only the valence electrons of an atom of a particular element are shown, indicated by dots placed around the element’s symbol
    Electron-Dot Notation
  13. 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 electrons
    Lewis Structures
  14. Indicates the kind, number, arrangement, and bonds but not the unshared pairs of the atoms in a molecule
    Structural Formula
  15. A covalent bond in which one pair of electrons is shared between two atoms
    Single Bond
  16. Double and triple bonds
    Multiple Bonds
  17. Refers to bonding in molecules or ions that cannot be correctly represented by a single Lewis structure
  18. Composed of positive and negative ions that are combined so that the numbers of positive and negative charges are equal
    Ionic Compound
  19. The simplest collection of atoms from which an ionic compound’s formula can be established
    Formula Unit
  20. The energy released when one mole of an ionic crystalline compound is formed from gaseous ions
    Lattice Energy
  21. A charged group of covalently bonded atoms
    Polyatomic Ion
  22. The chemical bonding that results from the attraction between metal atoms and the surrounding sea of electrons
    Metallic Bonding
  23. Ability of a substance to be hammered or beaten into thin sheets
  24. Ability of a substance to be drawn, pulled, or extruded through a small opening to produce a wire
  25. States that repulsion between the sets of valence-level electrons surrounding an atom causes these sets to be oriented as far apart as possible
    VSEPR theory
  26. The mixing of two or more atomic orbitals of similar energies on the same atom to produce new hybrid atomic orbitals of equal energies
  27. Orbitals of equal energy produced by the combination of two or more orbitals on the same atom
    Hybrid Orbitals
  28. Created by equal but opposite charges that are separated by a short distance
  29. The intermolecular force in which a hydrogen atom that is bonded to a highly electronegative atom is attracted to an unshared pair of electrons of an electronegative atom in a nearby molecule
    Hydrogen Bonding
  30. The intermolecular attractions resulting from the constant motion of electrons and the creation of instantaneous dipoles
    London Dispersion Forces
Card Set
Chapter 6 Chemistry Vocabulary
Chapter 6 Chemistry Vocabulary