Question: What is the ionization energy trend in the periodic table?
Options:
Increases down a group
Decreases across a period
Increases across a period
Decreases down a group
Correct Answer: Increases across a period
Solution:
Ionization energy generally increases across a period due to increasing nuclear charge.
What is the ionization energy trend in the periodic table?
Practice Questions
Q1
What is the ionization energy trend in the periodic table?
Increases down a group
Decreases across a period
Increases across a period
Decreases down a group
Questions & Step-by-Step Solutions
What is the ionization energy trend in the periodic table?
Step 1: Understand what ionization energy is. It is the energy required to remove an electron from an atom.
Step 2: Look at the periodic table. It is organized in rows (periods) and columns (groups).
Step 3: Notice that as you move from left to right across a period, the number of protons in the nucleus increases. This is called increasing nuclear charge.
Step 4: Realize that with more protons, the attraction between the nucleus and the electrons becomes stronger.
Step 5: Because of this stronger attraction, it takes more energy to remove an electron, which means ionization energy increases.
Step 6: Also, remember that as you move down a group, ionization energy generally decreases because the outer electrons are farther from the nucleus and are less tightly held.
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