Questions: 68. Refer to the periodic table and predict which element in each of the following pairs has the higher ionization energy. (a) Ga or Ge (b) Si or P (c) Br or Cl (d) As or Sb

68. Refer to the periodic table and predict which element in each of the following pairs has the higher ionization energy. (a) Ga or Ge (b) Si or P (c) Br or Cl (d) As or Sb
Transcript text: 68. Refer to the periodic table and predict which element in each of the following pairs has the higher ionization energy. (a) Ga or Ge (b) Si or P (c) Br or Cl (d) As or Sb
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Solution

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Solution Steps

Step 1: Understanding Ionization Energy

Ionization energy is the energy required to remove an electron from an atom in its gaseous state. Generally, ionization energy increases across a period (left to right) and decreases down a group (top to bottom) in the periodic table.

Step 2: Comparing Elements in Each Pair

We will compare the elements in each pair based on their positions in the periodic table.

(a) Ga or Ge
  • Gallium (Ga) is in Group 13 and Period 4.
  • Germanium (Ge) is in Group 14 and Period 4.
  • Since Ge is to the right of Ga in the same period, Ge has a higher ionization energy.
(b) Si or P
  • Silicon (Si) is in Group 14 and Period 3.
  • Phosphorus (P) is in Group 15 and Period 3.
  • Since P is to the right of Si in the same period, P has a higher ionization energy.
(c) Br or Cl
  • Bromine (Br) is in Group 17 and Period 4.
  • Chlorine (Cl) is in Group 17 and Period 3.
  • Since Cl is above Br in the same group, Cl has a higher ionization energy.
(d) As or Sb
  • Arsenic (As) is in Group 15 and Period 4.
  • Antimony (Sb) is in Group 15 and Period 5.
  • Since As is above Sb in the same group, As has a higher ionization energy.

Final Answer

\[ \begin{aligned} &\text{(a) Ge has the higher ionization energy.} \\ &\boxed{\text{Ge}} \\ &\text{(b) P has the higher ionization energy.} \\ &\boxed{\text{P}} \\ &\text{(c) Cl has the higher ionization energy.} \\ &\boxed{\text{Cl}} \\ &\text{(d) As has the higher ionization energy.} \\ &\boxed{\text{As}} \end{aligned} \]

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