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10.E: Chapter 10 Homework

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    202194
  • General Questions

    1.      What type(s) of elements make up a covalent compound? What type(s) of elements make up an ionic compound?

    2.      How do electrons behave differently in ionic and covalent bonds?

    3.      In bonding theory, what is an octet and why do atoms try to get them?

    4.      Why don’t Hydrogen atoms need to form octets? What is this called instead of an octet?
    5.      What is the difference between a molecule and a formula unit?
    6.      How can you tell if a molecule might have a double or triple bond?

    Electron Configurations and Single Atom Lewis Structures

    7.  Write the full electron configuration and the number of valence electrons for each atom.

    a)     Ar:

    b)     Na:

    c)      B:

    d)     H:

    e)     F:

    8. Write the full electron configuration for each atom.

    a)     Zr:       

    b)     Se:       

    c)      Pb:      

    d)     Cr:       

    9. Write the electron configuration for the following atoms and ions using their noble gas cores.

    a)     K+     

    b)     Pb:      

    c)     P3-:      

    d)     Ce:       

     10. Draw the Lewis structure for the following elements.

    a)     C:

    b) Cl:

    c) Li:

    d) Kr:

    11. Draw the Lewis structure for the following ions.

    a)    S2-:

    b)   P3-:  

    c) Na+:

    12. Name the element with the same electron configuration as the given ion (write out the electron configuration if you are having trouble solving them).

    a)     Cl-:

    b)     I-

    c)      Ca2+:

    d)     O2-:     

    Lewis Structures for Ionic Compounds

    13. Identify whether the following compounds are Ionic or Not-Ionic.

    a)     NaCl:

    b)     CaI2:

    c)      SO2:

    d)     HCl:

    14. Identify whether the following compounds are Ionic or Not-Ionic.

    a)     H2O:

    b)     NaOH:

    c)      AgF:

    d)      MgO:

    15. Draw the Lewis structure for NaCl.

    16. Draw the Lewis structure for Potassium Iodide.

    17. Draw the Lewis structure for CaCl2.

    18. For the following pairs of elements, determine how many of each element you would need to pair them together and how many valence electrons the Ionic compound would have.

    a)     Al / O:

    b)     Li / F:

    c)      Ca / N:

    d)     Na / P:

    19. Draw the Lewis structures for the following Ionic compounds.

    a)     KCl:

    b)     MgS:

    c)      CaF2:

    d)     LiI:

    20. Draw the Lewis structures for the following Ionic compounds.

    a)     CaBr2:

    b)     Rb2S:

    c)      SrCl2:

    d)     Na2O:

    21. Draw the Lewis structure for the following Ionic compounds.

    a)     Li2S:

    b)     BaO:

    c)      K2O:

    d)     RbI:

    Covalent Lewis Structures

     22.  Draw the Covalent Lewis structures for the following molecules.

    a)     H2O:

    b)     NH3:

    c)      CCl4:

    d)     NF3:

    23. Draw the Covalent Lewis structures for the following molecules.

    a)     O2:

    b)     CH3COOH (Both Carbons are central atoms):

     c)      CO2:

    d)     PCl3:

     24. Draw the Covalent Lewis structures for the following molecules.

    a)     Cl2O:

    b)     C2H4 (Carbons are central atoms):

    c)      CH3Cl

    d)     CH4:

     25. Draw the Covalent Lewis structure and their resonance structures, if applicable.

    a)     CH2O:

    b)     O3

    c)      NO3-:

    d)     NO2-:

    26. For each ion, draw the Covalent Lewis structure and their resonance structures, if applicable.

    a)     OH-:

    b)     CH3COO-:

    c)      ClO-:

    27. For each ion, draw the Covalent Lewis structure and their resonance structures, if applicable.

    a)     CHO2-:

    b)     PO43-:

    c)      CO32-:

    Molecular and Electron Geometry

    28. In the given molecules, draw the Lewis structure and  determine how many electron groups are around each central atom.

    a)     CH3-:

    b)     CH4:

    c)      BeCl2:

    d)     CH2O:

    29. Determine the electron and molecular geometries for each of the molecules from the previous problem.

    a)     CH3-:

    b)     CH4:

    c)      BeCl2:

    d)     CH2O:

    30. What are the bond angles for each molecule in the previous two problems?

    a)     CH3-:

    b)     CH4:

    c)      BeCl2:

    d)     CH2O:

    31. In the given molecules, draw the Lewis structure and  determine how many electron groups are around each central atom.

    a)     CO2:

    b)     SCl2:

    c)      NF3:

    d)     CH2O;

    32. Determine the electron and molecular geometries for each of the molecules from the previous problem:

    a)     CO2:

    b)     SCl2:

    c)      NF3:

    d)     CH2O;

    33. What are the bond angles for each molecule from in the previous two problems?

    a)     CO2:

    b)     SCl2:

    c)      NF3:

    d) CH2O;

    34. In the given molecules, draw the Lewis structure and determine how many electron groups are around each central atom.

    a)     NH3:

    b)     CFCl3:

    c)      N2O (N is the central atom):

    d)     HCN:

    35. Determine the electron and molecular geometries for each of the molecules from the previous problem.

    a)     NH3:

    b)     CFCl3:

    c)      N2O (N is the central atom):

    d)     HCN:

    36. What are the bond angles for each molecule from in the previous two problems?

    a)     NH3:

    b)     CFCl3:

    c)      N2O (N is the central atom):

    d)     HCN:

    37. The two molecules below each contain multiple central atoms. Draw the Lewis structure and  determine the electron geometry, molecular geometry and how many electron pairs are around each central atom.

    a)     C2Cl4 (Carbons are the central atoms):

    b)     C2H6 (Carbons are the central atoms):

    38. The two molecules below each contain multiple central atoms. Draw the Lewis structure and  determine the electron geometry, molecular geometry and how many electron pairs are around each central atom.

    a)     C2Cl2 (Carbons are central atoms):

    b)     S2Cl2 (Sulfurs are central atoms):

    39. The two molecules below each contain multiple central atoms. Draw the Lewis structure and  determine the electron geometry, molecular geometry and how many electron pairs are around each central atom.

    a)     CH3OH (Carbon and Oxygen are central atoms):

    b)     H3COCH3 (Carbons and Oxygen are central atoms):

    40.  For the given polyatomic ions, draw the Lewis structure and determine their molecular geometry.

    a)     NO3-:

    b)     PO43-:

    41. For the given polyatomic ions, draw the Lewis structure and determine their molecular geometry.

    a)     NH4+:

    b)     SCN-:

    c)      CO32-:

    42. For the given polyatomic ions, draw the Lewis structure and determine their molecular geometry.

    a)     NO2-:

    b)     H3O+:

    c)      C2O42-:

    Electronegativity / Polarity

    43. Between each pair of elements, determine which is more electronegative.

    a)     O / F:

    b)     S / N:

    c)      H / Cl:

    d)     Li / B:

    44. Between each pair of elements, determine which is more electronegative.

    a)     Si / C:

    b)     Br / I:

    c)      N / O:

    d)     H / C:

    45. Between each pair of elements, determine which is more electronegative.

    a)     F / C:

    b)     H / Li:

    c)      Rb / S:

    d)     P / I:

    46. Using an electronegativity chart, state the difference in electronegativity between the pairs of atoms and determine if their bonds would be Ionic, Polar and Covalent, or just Covalent (Non Polar).

    a)     C / O:

    b)     K / F:

    c)      Na / N:

    d)     Br / S:

    47. Using an electronegativity chart, state the difference in electronegativity between the pairs of atoms and if their bonds would be Ionic, Polar and Covalent, or just Covalent (Non Polar).

    a)     B / F:

    b)     Cs / Cl:

    c)      I / C:

    d)     P / P:

    48. Using an electronegativity chart, state the difference in electronegativity between the pairs of atoms and if their bonds would be Ionic, Polar and Covalent, or just Covalent (Non Polar).

    a)     Mg / S:

    b)     P / Cl:

    c)      Al / O:

    d)     B / P:

    49. Identify whether the bonded pairs of elements (diatomic molecules) are Polar or Non-Polar.

    a)     HI:

    b)     Br2:

    c)      O2:

    d)     KCl:

    50. Identify whether the bonded pairs of elements (diatomic molecules) are Polar or Non-Polar.

    a)     N2:

    b)     LiF:

    c)      MgO:

    d)     NO:

    51. Identify whether the bonded pairs of elements (diatomic molecules) are Polar or Non-Polar.

    a)     HCl:

    b)     LiI:

    c)      I2:

    d)     CaS:

    52. State whether each molecule is Polar or Non-Polar.

    a)     H2O:

    b)     N2O:

    c)      CH4:

    d)     CH3COOH:

    53. State whether each molecule is Polar or Non-Polar.

    a)     CCl4:

    b)     BF3:

    c)      C2H6:

    d)     NH3:

    54. State whether each molecule is Polar or Non-Polar:

    a)     H3COCH3:

    b)     CH3Cl:

    c)      O3:

    d)     CH2Cl2:

    Cumulative Problems

    55. For the following molecules, draw their Lewis Structures and determine if they are Polar Covalent, Covalent, or Ionic compounds.

    a)     MgCl2:

    b)     C2H4:

    c)      CO2:

    d)     NH2F:

    56. Draw the Lewis structure for C2H6O (Dimethyl Ether), which is laid out in the form H3COCH3, and include any lone pairs. Determine whether the molecule is Polar or Non-Polar.

    57. For the following molecules, draw their Lewis structures and write the electron configuration for their central atoms.

    a)     NH3:

    b)     N2O:

    c)      SF2:

    d)     PCl3:

    58.  Draw the Lewis structures for the following Ionic compounds. Note that the cation or anion may be a covalently bonded polyatomic ion so be sure to show all of its bonds.

    a)     NaNO3:

    b)     CaSO4:

    c)      K2CO3:

    d)     NH4Cl: