Unit 5 - Lesson 3 - Ionization Energy

Which of the following elements has the highest first ionization energy?

• Sodium (Na)

• Magnesium (Mg)

• Aluminum (Al)

• Neon (Ne)

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NGSS.HS-PS1-1

What is the general trend in ionization energy as you move across a period from left to right in the periodic table?

• It decreases

• It increases

• It remains constant

• It fluctuates

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NGSS.HS-PS1-1

NGSS.HS-PS1-2

Explain why ionization energy generally increases across a period.

• Due to increased nuclear charge and constant shielding

• Due to decreased atomic radius and increased electron shielding

• Due to increased atomic radius and decreased nuclear charge

• Due to decreased nuclear charge and increased atomic radius

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NGSS.HS-PS1-1

NGSS.HS-PS1-2

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

• Atomic radius

• Nuclear charge

• Electron shielding

• Melting point

How does the ionization energy change as you move down a group in the periodic table?

• It increases

• It decreases

• It remains constant

• It fluctuates

Compare the ionization energy of lithium (Li) and fluorine (F). Which one is higher and why?

• Lithium, because it has a larger atomic radius

• Fluorine, because it has a higher nuclear charge

• Lithium, because it has a lower nuclear charge

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MI.PE.SCI.9-12.HS-PS1-1

Which of the following elements has the lowest first ionization energy?

• Helium (He)

• Potassium (K)

• Calcium (Ca)

• Argon (Ar)

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NGSS.HS-PS1-1

NGSS.HS-PS1-2

Why does ionization energy decrease as atomic radius increases?

• Because electrons are closer to the nucleus

• Because electrons are further from the nucleus

• Because nuclear charge decreases

• Because electron shielding decreases

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NGSS.HS-PS1-1

NGSS.HS-PS1-2

Which of the following statements is true about the relationship between ionization energy and atomic radius going down the periodic table?

• As atomic radius increases, ionization energy increases

• As atomic radius decreases, ionization energy decreases

• As atomic radius increases, ionization energy decreases

• There is no relationship between atomic radius and ionization energy

What is the primary reason for the increase in ionization energy across a period?

• Increase in atomic radius

• Increase in nuclear charge

• Decrease in electron shielding

• Decrease in atomic mass