Multiple Choice
Which of the following atoms will be expected to have the smallest second ionization energy?
26
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
Which of the following elements has the highest second ionization energy (IE\(_2\))?
A
K
B
Al
C
Na
D
Mg
Verified step by step guidance1
Understand that the second ionization energy (IE\(_2\)) refers to the energy required to remove the second electron from a singly charged ion (M\(^+\) → M\(^{2+}\) + e\(^-\)).
Recall the electron configurations of the elements and their ions after the first ionization: \\ For example, Na (atomic number 11) loses one electron to form Na\(^+\) with a noble gas configuration (Ne), which is very stable.
Recognize that removing a second electron from a stable, noble gas-like configuration requires significantly more energy, so elements that achieve a noble gas configuration after the first ionization tend to have very high second ionization energies.
Compare the elements: K, Al, Na, and Mg. Identify which element's ion after the first ionization has a noble gas configuration, indicating a high IE\(_2\).
Conclude that the element whose singly charged ion has a noble gas configuration will have the highest second ionization energy.
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