; Unit 4 Homework Packet-Honors - Properties of Ionic Compounds
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Unit 4 Homework Packet-Honors - Properties of Ionic Compounds

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									                                          Name _____________________________
                                          Period________ Date Assigned _______
                                          Date Turned In ______

Unit 2 Homework Packet-Honors
          Properties of Ionic Compounds Worksheet
1) Explain why ionic compounds do not conduct electricity in their crystalline form.




2) Why do metals and nonmetals usually form ionic compounds, whereas two bonded
   nonmetals are never ionic? Explain.




3) Why is the formation of ionic compounds exothermic?




4) Why do ionic compounds tend to be hard?




5) Describe whether the following compounds are likely to be ionic or not ionic based
   on the properties given. Explain your reasoning.
    Compound 1 has a melting point of 545 degrees Celsius and dissolves well in
      water.



      Compound 2 is is a brittle material that is used to melt road ice during storms.



      Compound 3 melts at 85 degrees Celsius and catches fire when heated to 570
       degrees Celsius.
Naming Ionic Compounds and Writing Formulas

Naming Compounds

Naming ionic compounds:

    1. Name the monatomic cation using the element name and simply use the name of the positive
       polyatomic ion.
    2. Name the monatomic anion using the root of the element name with the suffix –ide and us the
       name for the negative polyatomic ion.


***You must include Roman numerals in parenthesis only if the formula includes an ion that may have
more than one charge (it is a transition element or Pb or Sn) associated with it.



Writing ionic formulas:

    1. Assign charges to each of the ions present.
    2. Arrange the ions so that the cation is on the left and the anion is on the right.
    3. Cross the charges and drop the sign.
                          Al2(SO4)3
                                                              Al3+                    SO42-
Examples:


        NaCl                      MgBr2                      Fe2(SO4)3                     (NH4)2CO3




Sodium chloride           Magnesium bromide          Iron(III) sulfate          Ammonium carbonate
                            Compound Names and Formulas
For the list on the left, name the compound. For the list on the right, give the chemical formula that
corresponds to the name

1)      NaF                                       13)     potassium fluoride


2)      K2CO3                                     14)     ammonium sulfate



3)      MgCl2                                     15)     magnesium iodide



4)      Be(OH)2                                    16)    copper (II) sulfite



5)      SrS                                       17)     aluminum phosphate



6)      Cu2S                                      18)     lead (II) nitrite



7)      ZnI2                                      19)     cobalt (II) selenide



8)      Ca3(PO4)2                                 20)     silver cyanide



9)      NH4I                                      21)     copper (II) bicarbonate



10)     Mn(NO3)3                                  22)     iron (II) oxide



11)     FePO4                                     23)     lithium cyanide



12)     CoCO3                             24)    lead (IV) sulfite
More Ionic Practice:




Naming molecular (covalent) compounds:

    1. A prefix is used with the name of the first element (less electronegative) only if more than one
       atom is present.
    2. The second element is named by combining (a) a prefix if more than one compound can be
       formed by the two elements, (b) the root of the name of the second element, and (c) the ending
       –ide.


Dinitrogen monoxide     Carbon tetrafluoride      Dinitrogen tetroxide      Phosphorus trichloride

N2O                     CF4                       N2O4                      PCl3
Writing molecular formulas:

    1. Write the symbol of the element followed by a subscript that represents the number of atoms
       of that element present in the molecule.




Practice:




Naming binary acids:

    1. Start with the prefix hydro-, then the root of the element name, and end with the suffix –ic.
    2. Add the word acid.


  Hydrochloric acid         Hydrobromic acid            Hydroiodic acid           Hydrosulfuric acid

            HCl                    HBr                        HI                          H2S



Naming oxyacids(those that contain a polyatomic ion):

    1. Name the polyatomic ion and change the suffixes –ate to –ic and –ite to –ous…leave the
       prefixes alone.
    2. Add the word acid.


     Chloric acid           Hypoiodous acid         Nitric acid         Sulfuric acid

         HClO3                   HIO                  HNO3                 H2SO4



Practice:

Write the name for the following acids in the space given.



1. HCl                                 ______________________________________



2. H2SO4                               ______________________________________



3. H3PO4                               ______________________________________



4. HNO3                                ______________________________________



5. HI                                  ______________________________________



Write the formula for the following acids in the space given.

6. hydrobromic acid                    ______________________________________

7. cyanic acid                         ______________________________________

8. perchloric acid                     ______________________________________

9. hydrofluoric acid                   ______________________________________

10. sulfurous acid                     ______________________________________
Mixed Practice:
Name: __________________________ Section: ________ Date: ________________



EXERCISES:



1.    Classify the following substances, using the procedure outlined by the flowchart in
      Figure 1. For example, HCl is a covalent binary compound; NaI is an ionic binary
      compound with only one likely charge on the cation.

      (a)    SO2     _____________________________________________________
      (b)    I2 _____________________________________________________
      (c)    H2SO4 _____________________________________________________
      (d)    K2SO4 _____________________________________________________
      (e)    CuCrO4_____________________________________________________
      (f)    Co2(CrO4)4__________________________________________________
      (g)    CCl4   _____________________________________________________
      (h)    Ca3N2 _____________________________________________________
      (i)    N2O4 _____________________________________________________


2.    Name the substances you classified above:


      (a)    ___________________________________________________________
      (b)    ___________________________________________________________
      (c)    ___________________________________________________________
      (d)    ___________________________________________________________
      (e)    ___________________________________________________________
      (f)    ___________________________________________________________
      (g)    ___________________________________________________________
      (h)    ___________________________________________________________
      (i)    ___________________________________________________________
3.   Classify and name the following substances:

 Chemical Formula            Classification        Name


        P4



       LiBr



      SnCl2



      K2SO3



     Fe(ClO3)2



       CS2



     Sr(OH)2



       P2S4



     Al(NO3)3



       NO



      NaIO3



      HBrO3
KMnO4



Ti(CO3)2
4.        Classify and write the formula for the following substances:



      Chemical Name                Classification                        Formula


     Hypobromous Acid



       Phosphorous

       pentachloride


      Sodium oxalate



      Calcium iodide



     Hydrobromic Acid



         Dinitrogen

        pentaoxide


       Silver sulfide



        Iodous Acid



     Iron(III) phosphate



           Cobalt



     Titanium(II) nitrate



        Magnesium
   carbonate


   Manganese

   perchlorate


Tetraphosphorous

    trisulfide


Potassium sulfite
5.     The chemical name given to each of the compounds below is incorrect. Write the correct name for each compound and briefly
       explain the basis of your correction.


 Compound       Incorrect Name            Correct Name                  Explanation


     SnCl4        Tin chloride



                  Monosulfur
     SF6
                  hexafluoride


                 Aluminum(III)
     AlF3
                    fluoride


     HIO4          Iodic Acid



      F2           Difluoride



                   Tricalcium
     Ca3P2
                diphosphorous
6.      The chemical formula given to each of the compounds below is incorrect. Write the correct formula for each compound and briefly
        explain the basis of your correction.

                              Incorrect
          Name                               Correct Formula              Explanation
                              Formula

 Copper(II) carbonate          Cu2CO3



 Potassium periodate            KIO3



 Carbon tetrachloride           CCl3



     Strontium sulfate         SrSO3



      Barium nitrate           BaNO2



     Hydronitric Acid           HNO3
             Practice These Lewis Structure

Draw Lewis structures for the following. Include the geometry for the structure. And
Whether it is polar or nonpolar. Honors only, Include any resonance structures. If more
than one Lewis structure can be drawn, use formal charges to decide on the most
preferred Lewis structure. Also include what type of hybridized orbitals the structure has


                                                                                           2–
1. CH4                                11. C2H2                               21. C2O4
                                               –
2. BF3                                12. N3                                 22. H2PO4          –

3. HCN                                13. NOF                                23.   XeO4
                                                   +                                   –
4. NH3                                14. ClF2         (Cl = Chlorine)       24. PO3

5. H2O                                15. FNO2                               25.   NO
         –                                         +

6. ClO3      (Cl = Chlorine)          16. XeF5
7. H3O+    17. BrF5
       –         –
8. NH2     18. IF4
       +
9. NH4     19. SF6
10. C2H4   20. N2O4
Formula   Lewis Structure (with Resonance- Molecular   Polarity   Hybridized orbitals
          Honors)                          Geometry               (HONORS)


CH4




BF3




HCN
NH3




H2O




      –
ClO3
Cl=Chlorine
      +
H3O




   –
NH2




   +
NH4




C2H4
C2H2




 –
N3




NOF
       +
ClF2
Cl=Chlorine




FNO2




       +
XeF5
BrF5




  –
IF4




SF6
N2O4




     2–
C2 O 4
        –
H2PO4




XeO4




   –
PO3
NO
      –
IF4




SF6
N2O4




         2–
C 2O 4
          –
H2PO 4




XeO 4




      –
PO3
NO

								
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