Sure, let's analyze the ionization energy trends for the Group 2 elements: beryllium (Be), calcium (Ca), and strontium (Sr).
Ionization Energy and Periodic Trends:
1. Ionization Energy Definition: Ionization energy is the energy required to remove an electron from an atom in its gaseous state.
2. General Trend in the Periodic Table: For elements in the same group (column) of the periodic table, ionization energy generally decreases as you move down the group. This is because the atomic size increases down the group, and the outer electrons are further from the nucleus and are more easily removed.
Given that Be, Ca, and Sr are all in Group 2 of the periodic table, we can predict their ionization energies based on their positions:
- Beryllium (Be): It is at the top of Group 2.
- Calcium (Ca): It is below Beryllium in Group 2.
- Strontium (Sr): It is below Calcium in Group 2.
Since ionization energy decreases down the group:
- Beryllium (Be) will have the highest ionization energy among the three.
- Calcium (Ca) will have a lower ionization energy than Beryllium but higher than Strontium.
- Strontium (Sr) will have the lowest ionization energy among the three.
Building the Correct Relationship:
- Beryllium (Be) > Calcium (Ca) > Strontium (Sr)
This indicates that the correct relationship in terms of increasing ionization energy is:
[tex]\[ \text{Sr} < \text{Ca} < \text{Be} \][/tex]
Reviewing the Possible Choices:
A. [tex]\( \text{Ca} < \text{Be} < \text{Sr} \)[/tex] (Incorrect)
B. [tex]\( \text{Sr} < \text{Be} < \text{Ca} \)[/tex] (Incorrect)
C. [tex]\( \text{Be} < \text{Ca} < \text{Sr} \)[/tex] (Incorrect)
D. [tex]\( \text{Sr} < \text{Ca} < \text{Be} \)[/tex] (Correct)
E. [tex]\( \text{Ca} < \text{Sr} < \text{Be} \)[/tex] (Incorrect)
Thus, the correct answer is:
[tex]\[ \boxed{D. \ \text{Sr} < \text{Ca} < \text{Be}} \][/tex]
