What is the trend in ionization energy for alkali metals down the group?

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Question: What is the trend in ionization energy for alkali metals down the group?

Options:

Correct Answer: Decreases

Solution:

Ionization energy decreases down the group for alkali metals.

What is the trend in ionization energy for alkali metals down the group?

What is the trend in ionization energy for alkali metals down the group?

Step 1: Understand what ionization energy is. It is the energy required to remove an electron from an atom.
Step 2: Identify the group we are talking about. Alkali metals are in Group 1 of the periodic table.
Step 3: Recognize that alkali metals include lithium (Li), sodium (Na), potassium (K), rubidium (Rb), cesium (Cs), and francium (Fr).
Step 4: Note that as you move down the group from lithium to francium, the size of the atoms increases.
Step 5: Understand that larger atoms have their outer electrons further from the nucleus, making them easier to remove.
Step 6: Conclude that because the outer electrons are easier to remove in larger atoms, the ionization energy decreases as you go down the group.

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