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Ch. 12 Worksheet 1 _12.1 _ 12.2_ How are ionic bonds and covalent

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Ch. 12 Worksheet 1 _12.1 _ 12.2_ How are ionic bonds and covalent Powered By Docstoc
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Ch. 12 Worksheet 1 (12.1 & 12.2)
 1.  How are ionic bonds and covalent bonds different? Ionic – electrons not shared. Cation (metal) has
    completely lost at least 1 electron. Anion (nonmetal) has gained at least 1 electron. Covalent –
    electrons are shared (equally or not). Nonmetal & metal.
 2. How does a polar covalent bond differ from a nonpolar covalent bond? polar – electrons are shared
    unequally. Bonding atoms have different electronegativities.


 3. If a very electronegative atom is bonded to a very non-electronegative atom, what type of bond is likely
    to form? an ionic bond. The very electronegative atom pulls all of the electron to it.




 4.    If a non-electronegative atom is bonded to a slightly electronegative atom, what type of bond is likely to
      form?           polar covalent bond (electrons are shared, but unequally so there is a slight dipole.)




 5.    If 2 atoms with the same electronegativity form a bond, what type of bond will it be?
      pure covalent (nonpolar covalent). equal sharing of electrons


 6. For each of the following binary molecules, write the type of bond expected to form between them.
    (ionic, polar covalent, covalent) Tell which atom is the most negative.

      a. H – H       nonpolar covalent             f. C – C    nonpolar covalent


      b. H – F       polar covalent                g. NaBr     ionic (metal/nonmetal)
         + -                                           + -

      c. F – F    nonpolar covalent                h. CO       polar covalent
                                                      + -

      d.   KF    ionic                             i. OH polar covalent
           + -                                        - +

      e. NaF ionic                                 j. NO polar covalent
         + -                                          + -
                                                                                                                   2

       12.3 & 12.4 Predicting Formulas for Ionic Compounds Using Electron Configurations

   1. a. Why do metals lose electrons to form ions? So that their electron configuration is the same as the
      previous noble gas. (More energetically favorable)

       b. When does a metal stop losing electrons? When it has the same electron configuration as the previous
       noble gas.

   2. Use its electron configuration to show why Oxygen forms an O2- ion and not an O3- ion.
      O (8 e)         1s22s22p4      O2- (10 e) 1s22s22p6- same as Neon. If it gained 3 electrons, the electron
      configuration would be 1s22s22p63s1. (Not favorable)


   3. Write the electron configurations for the pairs of atoms given below. Use them to predict the formula
      for an ionic compound formed from these elements.
      a. Mg          Mg2+                                   S      [Ne]3s23p4    6 valence      MgS
              2                                               2-         2  6
      [Ne] 3s        [Ne]                                   S      [Ne]3s 3p = [Ar]
      2 valence electrons

       b. K [Ar]4s1             1 valence                    Cl      [Ne]3s23p5     7 valence e    KCl
          K+ [Ar]                                                    [Ne]3s23p6 or [Ar]


       c. Cs           [Xe]6s1         1 valence             F       [He]2s22p5     7 valence e    CsF
          Cs+          [Xe]                                  F-      [Ne]


       d. Ba           [Xe]6s2    2 valence          Br      [Ar]4s23d104p5 7 valence (only s & p)         BaBr2
          Ba2+         [Xe]                          Br-     [Ar]4s23d104p6 = [Kr]


       e. Li           1s22s1          1 valence             F        [He]2s22p5    7 valence e    LiF
          Li+          1s2                                   F-      [Ne]


       f. Al           [Ne]3s23p1      3 valence             O       1s22s22p4      6 valence      Al2O3
          Al3+         [Ne]                                  O2-     1s22s22p6

(Thinking Question) Why are cations smaller than their parent atoms? Why are anions larger?
Cations have lost electrons in the outer (larger) shell so are smaller after they have lost their electrons.
Anions have gained electrons and, even though the electrons do not go into a larger shell (they generally just fill
up a shell), more negative charge with the same amount of positive to attract and hold the negative charge,
makes for a larger particle.

				
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