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5.E: Homework Chapter 5

  • Page ID
    208525
  • GENERAL QUESTIONS

    1.      Metals lose or gain electrons to form what type of ions?

    2.      Non-metals lose or gain electrons to form what type of ions?

    3.      Hydrogen is unusual because it can form both positive and negative ions.  Write the chemical symbol and name for each of these ions.

    CHEMICAL FORMULAS

    4.      How many Oxygen atoms are in each chemical formula?

    a.       H3PO4

    b.      Ca(HCO3)2

    c.       Ba(C2H3O2)2

    d.      Sr(OH)2

    e.       Mg3(PO4)2

     

    5.      Determine the total number of each type of atom in each formula.

    a.       NH4Cl

    b.      NaCN

    c.       Ba(HCO3)2

    d.      Ca(NO2)2

    e.       MgCl2

     

    6.      Give the formula of each molecule.

    a.       A molecule with a single phosphorus atom and three fluorine atoms.

    b.      A compound with one carbon atom and one oxygen atom.

    c.       A molecule with two selenium atoms and two bromine atoms.

     

    7.      Which of these formulas represent molecules? State how many atoms are in each molecule.

    a.       Fe

    b.      PCl3

    c.       P4

    d.      Ar

     

    8.      Write the formula for each compound

    a.       magnesium sulfate, which has 1 magnesium atom, 4 oxygen atoms, and 1 sulfur atom

    b.      ethylene glycol (antifreeze), which has 6 hydrogen atoms, 2 carbon atoms, and 2 oxygen atoms

    c.       acetic acid, which has 2 oxygen atoms, 2 carbon atoms, and 4 hydrogen atoms

    d.      potassium chlorate, which has 1 chlorine atom, 1 potassium atom, and 3 oxygen atoms

    e.       sodium hypochlorite pentahydrate, which has 1 chlorine atom, 1 sodium atom, 6 oxygen atoms, and 10 hydrogen atoms

     

    9.      Complete the table.

    Formula

    Number of SO42- Units

    Number of Sulfur Atoms

    Number of Oxygen atoms

    Number of metal atoms

    CaSO4

     

     

     

     

    Al2(SO4)3

     

     

     

     

    K2SO4

     

     

     

     

     

    10.  Write the chemical formula of the compound containing one magnesium atom for every two chlorine atoms.

    11.      The white light in fireworks displays is produced by burning magnesium in air, which contains oxygen. What compound is formed?

    12.      How many Hydrogen atoms are in each of the formulas in Question 4?

    MOLECULAR VIEW OF ELEMENTS AND COMPOUNDS

    13.      Determine whether each compound is ionic or molecular.

    a.       P2O5

    b.      MgCl2

    c.       NaC2H3O2

    d.      NH3

    e.       CCl4

    14.      For each of the following compounds, state whether it is ionic or covalent. If it is ionic, write the symbols for the ions involved:

    a.        NF3

    b.       BaO,

    c.       (NH4)2CO3

    d.       Sr(H2PO4)2

    e.        IBr

    15.      Classify each compound as ionic or molecular.

    a.       PtO2

    b.      FeN2

    c.       SiH4

    d.      BaSO4

     16.      Identify each compound as ionic or covalent.

    a.       Na2O

    b.      PCl3

    c.       NH4Cl

    d.      OF2

    17.      Which elements have molecules as their basic units?

    a.       Iron

    b.      Bromine

    c.       Oxygen

    d.      Helium

    18.      Classify each compound as ionic or molecular.

    a.       K3PO4

    b.      SiI4

    c.       CrPO4

    d.      N2O4

    19.      Classify each element as atomic or molecular.

    a.       Bromine

    b.      Fluorine

    c.       Neon

    d.      Cobalt

    20.  Provide the classification (i.e. atomic element, molecular element, molecular compound, or ionic compound) of each substance.

    a.       PCl3

    b.      LiBr

    c.       P4

    d.      oxygen gas

    21.  Provide the classification (i.e. atomic element, molecular element, molecular compound, or ionic compound) of each substance.

    a.       I2

    b.      H2O

    c.       Al

    d.      CuCl

    22.  Classify each compound as ionic or molecular.

    a.       CF2Cl2

    b.      CO

    c.        SO3

    d.      Al(NO3)2

    23.   Predict whether the compound formed in each case is an ionic or a covalent compound.

    a.       Carbon Dioxide

    b.      Potassium Oxide

    c.       Nitrogen Chloride

    d.      Dinitrogen Tetroxide

    24.  Classify each substance as an atomic element, molecular element, or ionic compound.

    a.       Krypton

    b.      Nitrogen gas

    c.       Potassium Nitrate

    d.      Gold

    WRITING FORMULA FOR IONIC COMPOUNDS: NAMING IONIC COMPOUNDS

    25.  Briefly describe the process for naming an ionic compound.

    26.  In what order do the names of ions appear in the names of ionic compounds?

    27.  Which ionic compounds can be named using two different systems? Give an example.

    28.  Name the ionic compound formed by each pair of ions.

    a.       Na+ and Br

    b.      Mg2+ and Br

    c.       Mg2+ and S2−

    29.  Name the ionic compound formed by each pair of ions. Use both the Stock and common systems, where appropriate.

    a.       Fe3+ and Br

    b.      Fe2+ and Br

    c.       Au3+ and S2−

    d.      Au+ and S2−

    30.  Name the ionic compound formed by each pair of ions. Use both the Stock and common systems, where appropriate.

    a.       Cr3+ and NO3

    b.      Fe2+ and PO43−

    c.       Ca2+ and CrO42−

    d.      Al3+ and OH

     31.   Provide the formula for each ionic compound named below.

    a.       Sodium hypochlorite

    b.      Potassium hydroxide

    c.       Ammonium nitrate

    d.      ​Aluminum sulfite

    e.       Iron(III) cyanide

    32.   Complete the table below

    Cations

    Anions

    Formula Unit

    Zn2+

    Br-

     

    K+

    CO32-

     

    Al3+

    HCO3-

     

    Fe2+

    OH-

     

    Cu+

    NO3-

     

     

    33.  Provide the name of the individual ions that make up each of the following ionic compounds and indicate how many of each ion there are.

    a.       Al(OH)3

    b.      ​Li3PO4

    c.       KCl

    d.      ZnF2

    e.       ​Na2O

    34.  Combine the following pairs of elements (or ions) to express them as an ionic compound.

    a.       Sodium and Sulfur

    b.      Barium and Iodine

    c.       Iron(III) and Oxygen

    d.      Aluminum and Bromine

    e.       Lithium and Nitrogen

    35.   Name each ionic compound AND give the names of the individual ions that make up the formula.

    a.       Hg2S

    b.      Cr2O3

    c.       K2SO4

    d.      Fe2(CO3)3

    e.       Zn(ClO)2

    36.  Transition metals tend to have varying charges. Determine the charges on each transition metal in the following ionic compounds.

    a.       AuN

    b.      SnO2

    c.       Cu2S

    d.      PbBr4

    e.       FeI2

    37.  The following chemical formulas are INCORRECT.  Rewrite the formulas with the proper number of cations and anions to balance the formulas then name the ionic compounds

    a.       BaC2H3O2

    b.      NH4SO4

    c.       ZnClO

    d.      AlOH

    e.       NaCO3

    38.  Determine if the following ionic compounds are correctly balanced.  If they are not correctly balanced, then rewrite the chemical formula correctly.

    a.       Ca2O

    b.      Na(OH)2

    c.       AlBr2

    d.      Zn3(PO4)2

    e.       Sr2N

    39.   Mercury forms two possible cations—Hg2+Hg2+ and Hg2+2Hg22+, the second of which is actually a two-atom cation with a 2+ charge.  What are the chemical formulas of the ionic compounds these ions make with the oxide ion, O2−O2−?

    40.  Which compounds would you predict to be ionic?

    a.       Li2O

    b.      (NH4)2O

    c.       CO2

    d.      FeSO3

    e.       C6H6

    f.        C2H6O

    41.  The following ionic compounds are found in common household products. Write the formulas for each compound:

    a.        potassium phosphate

    b.      copper(II) sulfate

    c.        calcium chloride

    d.       titanium dioxide

    e.        ammonium nitrate

    f.         sodium bisulfate (the common name for sodium hydrogen sulfate)

    42.  Name each ionic compound.

    a.       CaCl2

    b.      AlF3

    c.       Co2O3

    d.      Sc2O3

    e.       AgCl

    43.  Name the following ionic compounds:

    a.        CsCl

    b.      BaO

    c.        K2S

    d.      BeCl2

    e.        HBr

    f.        AlF3

    NAMING MOLECULAR COMPOUNDS

    44.  Write the formulas of the following molecular and ionic compounds:

    a.        chlorine dioxide

    b.       dinitrogen tetroxide

    c.       potassium phosphide

    d.       silver(I) sulfide

    e.        aluminum nitride

    45.  Give the names of the following covalent compounds.

    a.       N2O4

    b.      SCl6

    c.       CBr4

    d.      P2O5

    e.       ClF7

    46.   Write the formula for each molecular compound.

    a.       dinitrogen monoxide

    b.      silicon tetrafluoride

    c.       boron trichloride

    d.      nitrogen trifluoride

    e.       phosphorus tribromide

    47.  Determine whether the name shown for each molecular compound is correct. If not, provide the compound’s correct name.

    a.       NCl3             Nitrogen Chloride

    b.      CI4                 Carbon(IV)iodide

    c.       CO           Carbon Oxide

    d.      SCl4              Sulfur tetrachloride

    48.  Give the formula for each molecule.

    a.       carbon tetrachloride

    b.      silicon dioxide

    c.       trisilicon tetranitride

    d.      disulfur difluoride

    e.       iodine pentabromide

    49.   Give a systematic name for each of the following molecular compounds:

    a.       CF4 

    b.       Cl2O3

    c.       I4O9

    d.       SF6

    50.  Provide the formula for each of the following molecular compounds:

    a.       dinitrogen pentoxide

    b.       iodine monobromide

    c.       sulfur tetrafluoride

    d.       chlorine dioxide

    51.  Name the following molecular compounds.

    a.       NBr3

    b.      O2

    c.       NH3

    d.      CH4

    52.  Write a formula for each molecular compound.

    a.       Hydrogen iodide

    b.      Sulfur tetrachloride

    c.       Chlorine Dioxide

    d.      Selenium hexafluoride

    53.  What is the formula mass for each compound?

    a.       FeBr3

    b.      FeBr2

    c.       Au2S3

    d.      Au2S

    54.  What is the formula mass for each compound?

    a.       Cr(NO3)3

    b.      Fe3(PO4)2

    c.       CaCrO4

    d.      Al(OH)3.

    55.  Calculate the formula mass for each compound.

    a.       KMnO4

    b.      H2CO3

    c.       Ba(ClO3)2

    d.      Mg3(PO4)2

    Cumulative

    56.  Complete the table below.

    Element

    Number of valence

    electrons

    Symbol of ion formed by this element

    Report the number of electrons lost or gained

    K

     

     

     

    Br

     

     

     

    Ca

     

     

     

    O

     

     

     

    Al

     

     

     

    57.  Complete the table below.

    Ionic compound

    Cation symbol and name

    Anion symbol and name

    NaC2H3O2

     

     

    Cr(NO3)3

     

     

    PbCl2

     

     

    Hg3(PO4)2

     

     

    Ca(HCO3)2

     

     

    58.  Write the empirical formula for the binary compound formed by the most common monatomic ions formed by each pair of elements.

    a.       lithium and nitrogen

    b.      cesium and chlorine

    c.       gallium and oxygen

    d.      rubidium and sulfur

    e.       arsenic and sodium

    59.  Complete the table below.

    Formula Unit

    Chemical Name

    MgS

     

     

    Aluminum Oxide

    Fe(OH)3

     

     

    Copper(II) chloride

    Pb(CO3)2

     

     

    Zinc bicarbonate

    CaSO4

     

     

    Sodium acetate

    BaBr2

     

     

    Ammonium nitrate

     

    60.  Each of the following compounds contains a metal that can exhibit more than one ionic charge. Name these compounds:

    a.        Cr2O3

    b.       FeCl2

    c.       CrO3

    d.       TiCl4

    e.        CoO

     

    61.  Complete the following table by filling in the formula for the ionic compound formed by each cation-anion pair.

    Ion

    K+

    Fe3+

    NH4+

    Ba2+

    Cl-

     

     

     

     

    SO42-

     

     

     

     

    PO43-

     

     

     

     

    NO3-

     

     

     

     

    OH-

     

     

     

     

    62.  Write the formulas of the following compounds and calculate its formula mass.

    a.        rubidium bromide

    b.      magnesium selenide

    c.       calcium chloride

    d.      hydrogen fluoride

    e.       sodium oxide

    63.  Determine whether the name shown for each molecular compound is correct. If not, provide the compound’s correct name.

    a.       SF4                 monosulfur hexafluoride

    b.      K2O                dipotassium monoxide

    c.       CaI2               Calcium diiodide

    d.      PBr5              Phosphorus (v) pentabromide