Multiple Choice
Considering the periodic trend in successive ionization energies, which of the following elements is most likely to form an ion with the greatest positive charge before a dramatic increase in ionization energy occurs?
30
views
10. Periodic Properties of the Elements
Periodic Trend: Successive Ionization Energies
Struggling with General Chemistry?
Join thousands of students who trust us to help them ace their exams!Watch the first videoMultiple Choice
The third ionization energy is the energy required to remove which electron from an atom?
A
the third electron from a neutral atom
B
the second electron from a neutral atom
C
the third electron, after the first and second have been removed
D
the first electron from a neutral atom
Verified step by step guidance1
Understand that ionization energy refers to the energy required to remove an electron from an atom or ion.
Recognize that the first ionization energy is the energy needed to remove the first electron from a neutral atom.
The second ionization energy is the energy required to remove the second electron, which means removing an electron from the positively charged ion formed after the first electron is removed.
Therefore, the third ionization energy corresponds to the energy needed to remove the third electron, which is after the first and second electrons have already been removed.
In summary, the third ionization energy is the energy required to remove the third electron from the atom, not the first or second.
1:48mWatch next
Master Successive Ionizations with a bite sized video explanation from Jules
Start learningRelated Videos
Related Practice
Periodic Trend: Successive Ionization Energies practice set
Problem sets built by lead tutorsExpert video explanations