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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