SNC 2D0 Nomenclature - polyatomic ions and multivalent metals by nuhman10

VIEWS: 164 PAGES: 5

									SNC 2D0 Nomenclature: Multivalent Metals & Polyatomic Ions                      Name:

    PART II - IONIC COMPOUNDS (Continued)
    B. Ionic compounds with multivalent metals.
    Some of the transition metals have more than one possible valence. When naming
    compounds containing a multivalent metal (also called variable valence) metal,
    you must indicate the valence of the metal in the name of the compound.

    Naming
      ► look at the formula of the compound, and identify whether or not the metal
         is a transition metal, and whether or not it is multivalent – use your periodic
         table
      ► use the „reverse criss-cross‟ method to determine the valence of the metal
      ► write the name of the metal element
      ► write the valence of the metal in roman numerals in brackets
      ► write the name of the non-metal, and change the ending to “ide”


    example:        3 1 -the valence of Cl is 1, so the valence of Fe must be 3


                    FeCl3 = iron (III) chloride

    a) SnCl4        _______________________       g) CrP          _______________________


    b) PbO2         _______________________       h) Hg2O         _______________________


    c) SnF2         _______________________       i) HgO          _______________________

    d) SnF4         _______________________       j) NiCl2        _______________________


    e) PbO          _______________________       k) SbCl5        _______________________

    f) PbO2         _______________________       l) SbCl3        _______________________


    Writing formulas
       ►      write the symbol for the metal element first, the non-metal element second.
       ►      mentally mark in the valence numbers above each element: for the metal,
              use the valence indicated in the name (in Roman numerals)
       ►      bring the valence numbers into the subscripts after crisscrossing
       ►      eliminate any signs (+ or - ) and omit any 1's.
       ►      reduce the subscripts to lowest terms if possible

    a) chromium (III) phosphide___________                 f) nickel (II) chloride ___________

    b) antimony (V) chloride      ___________              g) lead (IV) oxide    ___________

    c) antimony (III) chloride    ___________              h) lead (II) oxide    ___________
d) mercury (II) oxide       ___________      i) tin (IV) fluoride      ___________

e) mercury (I) oxide        ___________      j) tin (II) fluoride      ___________

                        VARIABLE VALENCE ELEMENTS EXERCISE

A. Name the compounds below:                 B. Write the formula for:

1. Au2O       _________________________      1. manganese (II) oxide         ____

2. FeO        _________________________      2. nickel (III) nitride         ____

3. FeCl3      _________________________      3. tin (IV) oxide               ____

4. Sb2S3      _________________________      4. iron (II) oxide              ____

5. Sb2S5      _________________________      5. copper (I) chloride          ____

6. CuBr2      _________________________      6. chromium (III) oxide         ____

7. Hg2O       _________________________      7. lead (II) bromide            ____

8. HgCl       _________________________      8. chromium (III) nitride       ____

9. PbBr3      _________________________      9. mercury (II) chloride        ____

10. Au2S      _________________________      10. mercury (I) chloride        ____

11. SbI5      _________________________      11. cobalt (III) oxide          ____

12. SnF2      _________________________      12. manganese (IV) oxide ____

13. SnCl4     _________________________      13. tin (IV) chloride           ____

14. MnO2      _________________________      14. tin (II) fluoride           ____

15. Co2O3     _________________________      15. antimony (V) iodide         ____

16. HgCl      _________________________      16. gold (I) sulfide             ____

17. HgCl2     ________________________       17. lead (II) bromide           ____

18. CrN       _________________________      18. mercury (I) chloride        ____

19. PbBr2     _________________________      19. mercury (I) oxide           ____

20. Cr2O3     _________________________      20. copper (II) bromide         ____

21. CuCl      _________________________      21. antimony (V) sulfide        ____

22. FeO       _________________________      22. antimony (III) sulfide      ____

23. SnO2      _________________________      23. iron (III) chloride         ____
24. NiN         _________________________         24. iron (II) oxide          ____

25. MnO         _________________________         25. gold (I) oxide           ____

C. Compounds containing polyatomic ions
Compounds containing more than two types of atoms are called polyatomic
compounds. They are formed by the combination of a single element ion and a
polyatomic ion (an ion with two or more different elements in it).
example:        NH4Cl - contains more than two types of atoms (nitrogen, hydrogen
                and chlorine); it contains the NH4+ polyatomic ion

Naming compounds with polyatomic ions:
   ►   the same rules apply as discussed for binary ionic compounds
   ►   the trick is to recognize that a polyatomic ion is present in the
       compound: Refer to the chart on the back of your periodic table for a list of
       polyatomic ions
   ►   DO NOT CHANGE THE ENDING OF THE POLYATOMIC ION

H2SO4 _________________________             NaMnO4 _________________________

AlPO4 _________________________             (NH4)2CO3 _________________________

Ge(OH)4 _________________________                 Fe(C2H3O2)3 _________________________


Writing the formula of compounds with polyatomic ions
   ►   recognize that any compound name ending in "ate" contains a polyatomic
             ion; the only polyatomic ions that don‟t end in “ate” are the hydroxide
             and cyanide ions
   ►      place the ions as you would in writing a binary formula, imagining the
          valence above the ions
   ►         before you criss-cross, place the polyatomic ion in brackets
   ►         place the crossed over number outside of the bracket as a subscript
   ►         note that the polyatomic ion is NOT changed from its original form
   ►         if the subscript is "1" remove the bracket (and remove the “1”)

   example:           sodium chlorate       magnesium chlorate
                         +1    -1                        +2              -1
                          Na   ClO3                    Mg               ClO3

       NaClO3                     Mg(ClO3)2


Write formulas for the following compounds :

sodium sulfate        _________             aluminum fluorate            _________

magnesium nitrate _________                 barium permanganate          _________

potassium chlorate _________                silver carbonate             _________
ammonium phosphate         _________    zinc acetate                 _________

calcium hydroxide _________             strontium bromide            _________

beryllium oxide      _________          lithium nitride              _________

                        POLYATOMIC COMPOUNDS EXERCISE

A. Name the compounds below:                   B. Write the formula for:

1. HNO3       _____________________________    1. barium hydroxide         ______

2. KClO3      _____________________________    2. potassium permanganate_______

3. Mg(OH)2 _____________________________       3. silver nitrate           ______

4. Al(NO3)3    ____________________________    4. lithium phosphate        ______

5. Li2SO4     _____________________________    5. ammonium carbonate       ______

6. Na2CO3     _____________________________    6. boron nitrate            ______

7. AlPO4      _____________________________    7. calcium carbonate        ______

8. Ca(C2H3O2)2 _____________________________   8. sodium sulfate           ______

9. (NH4)SO4 _____________________________      9. ammonium chlorate        ______

10. ZnCO3     _____________________________    10. magnesium nitrate       ______

11. NH4OH     _____________________________    11. aluminum sulfate        ______

12. Ge3(PO4)4_____________________________     12. sodium hydroxide        ______

13. HClO3     _____________________________    13. hydrogen chlorate       ______

14. NaOH      _____________________________    14. germanium phosphate ______

15. Al2(SO4)3 _____________________________    15. ammonium hydroxide ______

16. Mg(NO3)2 _____________________________     16. zinc carbonate          ______

17. NH4ClO3 _____________________________      17. ammonium sulfate        ______

18. Na2SO4    _____________________________    18. calcium acetate         ______

19. CaCO3     _____________________________    19. aluminum phosphate ______

20. B(NO3)3   _____________________________    20. sodium carbonate        ______

21. (NH4)2CO3_____________________________     21. lithium sulfate         ______

22. Li3PO4    _____________________________    22. aluminum nitrate        ______
23. AgNO3     _____________________________   23. magnesium hydroxide ______

24. KMnO4     _____________________________   24. potassium chlorate   ______

25. Ba(OH)2   _____________________________   25. hydrogen nitrate     ______

								
To top