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Which of the following pairs of elements would you expect to have lower first ionization energy? Explain.(i) Cl or F(ii) Cl or S(iii) K or Ar(iv) Kr or Xe |
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Answer» The ionization energy. (a) Decreases in going from top to bottom in a group. (b) Increases in going from left to right in a period. Thus (i) Cl is below F in the group (or Cl is bigger than F), hence Cl has lower ionization energy than F. (ii) Cl is in the group 17th, while S belongs to 16th group (of the same period, Period 3). Thus, S should have lower ionization due to lower nuclear charge. (iii) K appears immediately after Ar in the periodic table. K belongs to group 1 of the periodic table; hence K should have lower ionization energy. (iv) Xe occurs below Kr in group 18 of the periodic table, hence Xe should have lower ionization energy due to its larger size. |
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