Multiple Choice
Which of the following species will have the highest ionization energy?
10. Periodic Properties of the Elements
Periodic Trend: Ionization Energy
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Which of the following lists the atoms in order of increasing ionization energy (smallest to largest)?
A
N < P < Si < Al
B
Si < P < N < F
C
Be < Li < Mg < Na
D
I < Te < Sb < Sn
Verified step by step guidance1
Understand the concept of ionization energy: Ionization energy is the energy required to remove an electron from an atom in the gaseous state. It generally increases across a period (left to right) and decreases down a group (top to bottom) in the periodic table.
Identify the position of each element in the periodic table: Locate each element in the given options on the periodic table to understand their relative positions.
Apply periodic trends: Use the trend that ionization energy increases across a period and decreases down a group to compare the elements. For example, within the same period, elements to the right have higher ionization energies.
Compare elements within the same group: For elements in the same group, the one higher up will have a higher ionization energy due to less electron shielding.
Arrange the elements based on the trends: Using the periodic trends, arrange the elements in each option from smallest to largest ionization energy and identify the correct sequence.
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Periodic Trend: Ionization Energy practice set
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