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

Solution

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.

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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