Nomenclature Review Worksheet

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 IB CHEMISTRY – CHAP. 7 FORMULA-NOMENCLATURE REVIEW WORKSHEET

General Rules for naming an ionic compound [metal ion or polyatomic ion bonded to a
nonmetal ion or a different polyatomic ion]. Take the name of the ion off the ion list. It the
metal ion has more than one charge listed on the ion list, use Roman numerals to indicate
the charge.

General Rules for naming a molecular compound [nonmetal bonded to nonmetal]. The
first name is the name of the first atom. If there is a subscript, use a prefix to indicate how
many atoms. The second name is the name of the second atom, but change the name so it
ends in –ide ex. Oxygen  oxide. Use a prefix to indicate how many.



DIRECTIONS: Part 1. Write the name for each of the compounds listed.
CaO    ________________________ KBr                ________________________

NaCl       ________________________            Al(OH)3         ________________________

CaCl2      ________________________            PbSO4           ________________________

NH4NO3 _________________________               MgO             ________________________

Ca(OH)2 ________________________               LiF             ________________________

K2 S       ________________________            Al2O3           ________________________

Fe2(SO4)3 ________________________             Na3PO4          ________________________

SiO2       ________________________            SO2             ________________________

SO3        ________________________            CF4             ________________________

PBr5       ________________________            P2 O5           ________________________

N2 O4      ________________________            PCl3            ________________________

N2 O5      ________________________            N2 O3           ________________________

CO         ________________________            PBr3            ________________________




Mrs. HajIbrahim IB Chemistry Chapter 7 Formula-Nomenclature Review Worksheet                      1
General Rules for writing the chemical formula of an ionic compound [metal ion or
polyatomic ion bonded to a nonmetal ion or a different polyatomic ion]. Take the formula
of the ion off the ion list. If the charges on the ions don’t cancel, use the cross rule: the
number on the charge becomes the subscript for the other ion.


General Rules for writing the chemical formula of a molecular compound [nonmetal
bonded to nonmetal]. Look up the first name and the second name of the formula on the
periodic table and copy the corresponding symbol. The prefix tells you what the subscript
should be. If a molecule has Roman numerals after the first name, treat the Roman
numerals as a charge. The use the Rules for an ionic compound.

PART 2. DIRECTIONS: Write the chemical formula for each of the following chemicals.


magnesium nitride_____________________             sodium hydrogen carbonate _______________

aluminum chloride ____________________             potassium phosphate _____________________

sodium carbonate _____________________             iron (II) nitrate__________________________

potassium sulfate _____________________            ammonium phosphate ____________________

copper (II) nitrate _____________________          calcium hydroxide_______________________

diphosphorus trioxide __________________           carbon monoxide ________________________

dinitrogen tetroxide ____________________          phosphorus trichloride ___________________

carbon tetrafluoride ____________________          silicon dioxide _________________________

sulfur dioxide     _____________________           phosphorus (III) bromide _________________

dinitrogen pentoxide ___________________           carbon tetrachloride _____________________

sulfur trioxide    _____________________           bromine (III) fluoride ____________________




Mrs. HajIbrahim IB Chemistry Chapter 7 Formula-Nomenclature Review Worksheet                     2
                      NAME:
               CRYSTALLINE STRUCTURES REVIEW SHEET

There are four different types of crystal structures: ionic, covalent; metallic;
covalent network. Consider the characteristics of each crystalline structure when
answer the following questions. Your answers should be a paragraph consisting of
logical, concise sentences. 4pts. each question.

   1. Explain why water does not conduct electricity, but salt water will conduct
      electricity.
   2. Compare the melting point of diamond to dry ice (frozen CO2).
   3. Explain why water is a liquid at room temperature while both oxygen and
      hydrogen are gases at room temperature.
   4. Explain why glass (SiO2) shatters when struck with a hammer but copper will
      flatten when struck.
                                                                       NAME:

                        EQUATION REVIEW WORKSHEET

DIRECTIONS: Answer each question completely.

Aqueous sodium chloride reacted with aqueous silver nitrate to produce a white
precipitate.
    • Write a balanced equation for the reaction. Use the following symbols where
        appropriate: (s) (l)  (g)       (aq)    (ppt.)
    • Write an ionic equation for the reaction.
    • What are the spectator ions?
    • Write the net ionic equation




Aqueous sodium hydroxide was titrated against hydrochloric acid producing water and a
soluble salt.
    • Write a balanced equation for the reaction. Use the following symbols where
       appropriate: (s) (l)   (g)       (aq)    (ppt.)
    • Write an ionic equation for the reaction.
    • What are the spectator ions?
    • Write the net ionic equation
Use the activity series (your textbook, p286) to predict the products for the following
single replacement reaction.

A nail is placed in an aqueous solution of copper (II) sulfate..
   • Write a balanced equation for the reaction. Use the following symbols where
        appropriate: (s) (l)    (g)      (aq)     (ppt.)
   • Write an ionic equation for the reaction.
   • What are the spectator ion(s)?
   • Write the net ionic equation




Use the activity series (your textbook, p286) to predict the products for the following
single replacement reaction.

Zinc wire is placed in an aqueous solution of iron (II) nitrate.
   • Write a balanced equation for the reaction. Use the following symbols where
       appropriate: (s) (l)    (g)       (aq)     (ppt.)
   • Write an ionic equation for the reaction.
   • What are the spectator ion(s)?
   • Write the net ionic equation
Zinc displaces the copper ions from a copper (II) sulfate solution. Metallic copper
precipitates.
    • What color is copper (II) sulfate solution?
    • What color is copper metal?
    • What color is zinc metal?
    • Write a balanced equation for the reaction. Use the following symbols where
        appropriate: (s) (l)    (g)     (aq)      (ppt.)
    • Write an ionic equation for the reaction.
    • What are the spectator ions?
    • Write the net ionic equation
           Names, Formulas, and Charges of Some Common Ions
Positive Ions, Cations           Negative Ions, Anions
                      3+
Aluminum           Al            Acetate                     CH3COO-
                                                             or
                                                             C2H3O2-
Ammonium           NH4+          Bromide                     Br-
Barium             Ba2+          Carbonate                   CO32-
Cadmium            Cd2+          Hydrogen carbonate,         HCO3-
                                 bicarbonate
                      2+
Calcium            Ca            Chlorate                    ClO3-
Chromium (II)      Cr2+          Chloride                    Ci-
Chromium (III) Cr3+              Chlorite                    ClO2-
Cobalt (II)        Co2+          Chromate                    CrO42-
Cobalt (III)       Co3+          Dichromate                  Cr2O72-
Copper (I)         Cu+           Fluoride                    F-
Copper (II)        Cu2+          Hydride                     H-
Hydrogen           H+            Hydroxide                   OH-
Hydronium          H3O+          Hypochlorite                ClO-
Iron (II)          Fe2+          Iodide                      I-
Iron (III)         Fe3+          Nitrate                     NO3-
Lead (II)          Pb2+          Nitride                     N3-
Lead (IV)          Pb4+          Nitrite                     NO2-
Lithium            Li+           Oxalate                     C2O42-
Magnesium          Mg2+          Oxide                       O2-
Manganese (II)     Mn2+          Perchlorate                 ClO4-
Mercury (I)        Hg22+         Permanganate                MnO42-
Mercury (II)       Hg2+          Phosphate                   PO43-
Nickel (II)        Ni2+          Monohydrogen phosphate      HPO42-
Potassium          K+            Dihydrogen phosphate        H2PO4-
Scandium           Sc3+          Sulfate                     SO42-
Silver             Ag+           Hydrogen sulfate, bisulfate HSO4-
Sodium             Na+           Sulfide                     S2-
Strontium          Sr2+          Hydrogen sulfide, bisulfide HS-
Tin (II)           Sn2+          Sulfite                     SO32-
Tin (IV)           Sn4+          Hydrogen sulfite, bisulfite HSO3-
Zinc               Zn2+
Draw Lewis structures for each of the following species?

F2    C Cl4    H2 O      NH3        NH4+    NH2-    AlCl3

				
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