Answer :
It appears we have a snippet of a table and some scrambled words that need context. However, to answer any question derived from this, I will provide a proper example for ordering atoms based on ionization energy as might be expected from the hint present in the provided input.
### Example Question:
Which set correctly orders the elements from lowest to highest ionization energy?
### Solution:
To determine the correct order of elements by their ionization energy, you need to understand the concept of ionization energy:
Ionization Energy is the amount of energy required to remove an electron from a gaseous atom or ion. This property generally increases across a period (from left to right) and decreases down a group (from top to bottom) in the periodic table.
Given the hint “O < S < Se < Te,” it means:
- Oxygen (O) has the lowest ionization energy among the four elements.
- Sulfur (S) has a higher ionization energy than Oxygen but lower than Selenium (Se).
- Selenium (Se) comes next.
- Tellurium (Te) has the highest ionization energy amongst these four elements.
### Correct Order from Lowest to Highest Ionization Energy:
[tex]\[ \text{O} < \text{S} < \text{Se} < \text{Te} \][/tex]
If we were to extend this example to other common elements or groups of elements mentioned in the table based on their periodic trends:
Let's consider another set:
For Alkali Metals (Group 1 elements):
- Rubidium (Rb), Cesium (Cs), and Francium (Fr):
- Francium (Fr) has the lowest ionization energy as it is the largest atom in this group.
- Cesium (Cs) has a higher ionization energy than Francium.
- Rubidium (Rb) has the highest ionization energy among the three.
So, from lowest to highest ionization energy:
[tex]\[ \text{Fr} < \text{Cs} < \text{Rb} \][/tex]
### Conclusion:
Given any group of elements, to find the order from lowest to highest ionization energy, you need to refer to their respective positions in the periodic table and follow the trend mentioned:
[tex]\[ \text{Ionization Energy increases across a period and decreases down a group}. \][/tex]
By applying this principle, you can correctly order any set of elements based on their ionization energies.
### Example Question:
Which set correctly orders the elements from lowest to highest ionization energy?
### Solution:
To determine the correct order of elements by their ionization energy, you need to understand the concept of ionization energy:
Ionization Energy is the amount of energy required to remove an electron from a gaseous atom or ion. This property generally increases across a period (from left to right) and decreases down a group (from top to bottom) in the periodic table.
Given the hint “O < S < Se < Te,” it means:
- Oxygen (O) has the lowest ionization energy among the four elements.
- Sulfur (S) has a higher ionization energy than Oxygen but lower than Selenium (Se).
- Selenium (Se) comes next.
- Tellurium (Te) has the highest ionization energy amongst these four elements.
### Correct Order from Lowest to Highest Ionization Energy:
[tex]\[ \text{O} < \text{S} < \text{Se} < \text{Te} \][/tex]
If we were to extend this example to other common elements or groups of elements mentioned in the table based on their periodic trends:
Let's consider another set:
For Alkali Metals (Group 1 elements):
- Rubidium (Rb), Cesium (Cs), and Francium (Fr):
- Francium (Fr) has the lowest ionization energy as it is the largest atom in this group.
- Cesium (Cs) has a higher ionization energy than Francium.
- Rubidium (Rb) has the highest ionization energy among the three.
So, from lowest to highest ionization energy:
[tex]\[ \text{Fr} < \text{Cs} < \text{Rb} \][/tex]
### Conclusion:
Given any group of elements, to find the order from lowest to highest ionization energy, you need to refer to their respective positions in the periodic table and follow the trend mentioned:
[tex]\[ \text{Ionization Energy increases across a period and decreases down a group}. \][/tex]
By applying this principle, you can correctly order any set of elements based on their ionization energies.
