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Answer :
Let's consider the elements beryllium (Be), calcium (Ca), and strontium (Sr), which all belong to Group 2 of the periodic table.
### Ionization Energy Trend in Group 2:
In Group 2, elements exhibit a trend in their ionization energies due to their increasing atomic size and the shielding effect as you move down the group. Here’s the trend typically observed:
1. Atomic Size: As you move down the group from beryllium to strontium, the atomic size increases. This means that the valence electrons are farther from the nucleus.
2. Shielding Effect: An increase in the number of inner electron shells results in a greater shielding effect. This further reduces the effective nuclear charge experienced by the valence electrons.
### Implication on Ionization Energy:
Due to the larger atomic size and greater shielding effect:
- Ionization Energy Decreases Down the Group: It becomes easier to remove an electron as you move down the group because the valence electron is further from the nucleus and is less tightly bound.
### Specific Elements:
1. Beryllium (Be): Being at the top of Group 2, it has the smallest atomic size and the least shielding effect, resulting in the highest ionization energy among the three.
2. Calcium (Ca): It is below beryllium and has a larger atomic size and a greater shielding effect, resulting in lower ionization energy than beryllium.
3. Strontium (Sr): It is further down the group than calcium and beryllium, with the largest atomic size and the greatest shielding effect among the three, resulting in the lowest ionization energy.
### Conclusion:
The correct relationship in terms of ionization energy from lowest to highest is:
[tex]\[ \text{Sr} < \text{Ca} < \text{Be} \][/tex]
Thus, the correct answer is:
D. [tex]\( \text{Sr} < \text{Ca} < \text{Be} \)[/tex]
### Ionization Energy Trend in Group 2:
In Group 2, elements exhibit a trend in their ionization energies due to their increasing atomic size and the shielding effect as you move down the group. Here’s the trend typically observed:
1. Atomic Size: As you move down the group from beryllium to strontium, the atomic size increases. This means that the valence electrons are farther from the nucleus.
2. Shielding Effect: An increase in the number of inner electron shells results in a greater shielding effect. This further reduces the effective nuclear charge experienced by the valence electrons.
### Implication on Ionization Energy:
Due to the larger atomic size and greater shielding effect:
- Ionization Energy Decreases Down the Group: It becomes easier to remove an electron as you move down the group because the valence electron is further from the nucleus and is less tightly bound.
### Specific Elements:
1. Beryllium (Be): Being at the top of Group 2, it has the smallest atomic size and the least shielding effect, resulting in the highest ionization energy among the three.
2. Calcium (Ca): It is below beryllium and has a larger atomic size and a greater shielding effect, resulting in lower ionization energy than beryllium.
3. Strontium (Sr): It is further down the group than calcium and beryllium, with the largest atomic size and the greatest shielding effect among the three, resulting in the lowest ionization energy.
### Conclusion:
The correct relationship in terms of ionization energy from lowest to highest is:
[tex]\[ \text{Sr} < \text{Ca} < \text{Be} \][/tex]
Thus, the correct answer is:
D. [tex]\( \text{Sr} < \text{Ca} < \text{Be} \)[/tex]
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