- #1
carle
- 13
- 0
Hello. I have a question about ionization energy:
Two hypothetical elements in the 2nd or 3rd period have the following ionization energies:
Element X
First: 800 kJ/mol
Second: 2500 kJ/mol
Third: 3900 kJ/mol
Fourth: 23000 kJ/mol
Element Y
First: 700 kJ/mol
Second: 2200 kJ/mol
Third: 3500 kJ/mol
Fourth: 19000 kJ/mol
To what group in the periodic table should element X be in, and what charge should the ion in element X have?
The answer is group 13 and charge +3. How could you possibly know this? I can see that the fourth energy level is far more than the third, so it should be somewhere between group 13-17, but how do you know which one?
Two hypothetical elements in the 2nd or 3rd period have the following ionization energies:
Element X
First: 800 kJ/mol
Second: 2500 kJ/mol
Third: 3900 kJ/mol
Fourth: 23000 kJ/mol
Element Y
First: 700 kJ/mol
Second: 2200 kJ/mol
Third: 3500 kJ/mol
Fourth: 19000 kJ/mol
To what group in the periodic table should element X be in, and what charge should the ion in element X have?
The answer is group 13 and charge +3. How could you possibly know this? I can see that the fourth energy level is far more than the third, so it should be somewhere between group 13-17, but how do you know which one?