Periodic Trends: Ionization Energy

Which trend correctly describes the change in ionization energy across a period in the periodic table?

• Ionization energy decreases from left to right.

• Ionization energy increases from left to right.

• Ionization energy remains constant across a period.

• Ionization energy first increases, then decreases across a period.

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What happens to the ionization energy as you move down a group in the periodic table?

• It increases because the atomic radius decreases.

• It decreases because the atomic radius increases.

• It remains constant because the number of protons remains the same.

• It increases because the electron shielding effect decreases.

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Which factor does NOT affect the ionization energy of an element?

• Atomic radius

• Nuclear charge

• Electron shielding

• Color of the element

How does the atomic radius of an atom relate to its ionization energy?

• Larger atomic radius means higher ionization energy.

• Smaller atomic radius means higher ionization energy.

• Atomic radius has no relation to ionization energy.

• Larger atomic radius means lower ionization energy, but only in metals.

Which element is likely to have the highest ionization energy?

• Sodium (Na)

• Magnesium (Mg)

• Aluminum (Al)

• Silicon (Si)

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Of these four elements [C, F, Ge, Br], which would you expect to have the highest ionization energy?

• C

• F

• Ge

• Br

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Which of the following statements is true regarding ionization energy and electron shielding?

• Increased electron shielding results in higher ionization energy.

• Electron shielding has no effect on ionization energy.

• Increased electron shielding results in lower ionization energy.

• Electron shielding only affects metals.

Why does helium have a higher ionization energy than hydrogen?

• Helium has a larger atomic radius.

• Helium has more electron shielding.

• Helium has a higher nuclear charge.

• Hydrogen has more protons.

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Which of the following elements would you expect to have the lowest ionization energy?

• Fluorine (F)

• Neon (Ne)

• Sodium (Na)

• Argon (Ar)

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The ionization energy of an element is affected by its:

• Color and phase at room temperature.

• Atomic radius and nuclear charge.

• State of matter and temperature.

• Name and symbol.

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