Chapter 7 Chemistry Nomenclature

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Author:
anmott
ID:
268684
Filename:
Chapter 7 Chemistry Nomenclature
Updated:
2014-04-20 12:57:20
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Chem Chemistry
Folders:
Chem
Description:
Chapter 7 Notes and Other Random Things I Find Important
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  1. Binary Compounds
    Binary Compounds are composed of two elements.
  2. Binary Ionic Compounds Named...
    Binary Ionic Compounds are named by combining the names of the positive and negative ions.
  3. Monoatomic Ion
    Ions formed from a single atom.
  4. Nomenclature
    Naming system
  5. Salt
    An ionic compound composed of a cation and the anion from an acid is often referred to as a salt.
  6. Oxyanion
    Polyatomic ions that contain oxygen.
  7. Ionic Compound (transfer e-)
    Metal/Nonmetal; Example- MgClMagnesium Chloride
  8. Hydrocarbons
    Are molecular compounds composed solely of carbon and hydrogen.
  9. Ionic Compound
    Consists of a lattice of positive and negative ions held together by mutual attraction.
  10. Stock System
    • This system uses Roman numerals to indicate an ion's charge. The numeral is enclosed in parentheses and placed immediately after the metal name.
    • CuCl2  copper(ll) chloride.
  11. Naming Binary Molecular Compounds
    • The old system of naming molecular compounds is based on the use of prefixes.
    • CCL4 -Carbon Tetrachloride
  12. Covalent Network Compounds
    • Similar to naming molecular compounds.
    • SiC- Silicon Carbide
    • SiO2- Silicon Dioxide
  13. Binary Acid
    Are acids that consists of two elements, usually hydrogen and one of the halogens.
  14. Oxyacids
    Are acids that contain hydrogen, oxygen, and a third element (usually a nonmetal).
  15. Oxidation Numbers/Oxidation States
    • Hydrogen: +1
    • Oxygen: -2
    • Halogens: -1
  16. Salts
    • Metal/Nonmetal; a neutral exchange of e
    • Example: FeO Iron(ll) Oxide
    • Example: Sr(OH)Strontium Hydroixide
  17. Hydrates
    • Salt w/water molecules; name= salt x #Hydrate
    • Example:PbO Lead(lV) Oxide Hexahydrate
  18. Molecular Compounds
    • Nonmetal/Nometal; covalent bonds share e
    • Name= #element #-ide
    • Example:P2ODiphoshorous Pentaoxide
  19. Organic Compounds
    • Single bonds between C: ane
    • Double bonds between C: ene
    • Alcohol- OH

    • 1-methyl (MeEatPeanutButter)
    • 2-ethyl
    • 3.propal
    • 4.butly 

    • Methane
    • Meth- One Carbon Ane- Single Bonds (Carbon has four bonding sites so four single bonds)
  20. Acids
    • H+       -ide    = Hydro__ic Acid (NO O!!!)
    • H+       -ate   = ____ic Acid
    • H     -ite    = ____ous Acid

    • Example: Phosphoric Acid H3PO4
    • Example: HNONitrous Acid
    • Example: H2S Hydrosulfuric Acid
  21. Mass of water . .  .. .
    Can be refered to as a moleular mass.
  22. Formula Mass
    Of any molecule, formula unit, or ion is the sum of the average atomic masses of all atoms represented in its formula.
  23. Molar Mass & Formula Mass
    Molar mass and formula mass are both numerically equal.
  24. Empirical Formula
    Consists of the symbols for the elements combined in a compound, with subscripts showing the smallest whole number ratio of different atoms in the compound.

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