Ionization Energy Trends

Explain the trend in ionization energy across periods in the periodic table.

• Ionization energy decreases across periods in the periodic table.

• Ionization energy increases across periods in the periodic table.

• Ionization energy remains constant across periods in the periodic table.

• Ionization energy is not affected by the position in the periodic table.

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

• Ionization energy remains constant

• Ionization energy increases

• Ionization energy fluctuates

• Ionization energy decreases

Why does ionization energy generally increase across a period?

• Shielding effect increases across a period.

• Effective nuclear charge increases across a period.

• Electron affinity decreases across a period.

• Atomic radius decreases across a period.

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Explain the concept of electron shielding and its effect on ionization energy.

• Electron shielding increases the ionization energy by attracting more electrons.

• Electron shielding reduces the effective nuclear charge felt by outer electrons, leading to a decrease in ionization energy.

• Electron shielding increases the effective nuclear charge felt by outer electrons, leading to a decrease in ionization energy.

• Electron shielding has no effect on the effective nuclear charge felt by outer electrons.

Explain why ionization energy generally increases across a period from left to right.

• Due to increased electron shielding

• Due to increased nuclear charge

• Due to decreased atomic radius

• Due to increased atomic mass

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Discuss why ionization energy generally increases across a period from left to right.

• Due to increased nuclear charge and constant shielding effect

• Due to decreased nuclear charge and increased shielding effect

• Due to increased atomic radius

• Due to decreased electron affinity

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As you move from left to right across a period in the periodic table, what generally happens to the ionization energy?

• It decreases

• It increases

• It remains constant

• It first increases, then decreases

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Explain why the ionization energy decreases as you move down a group in the periodic table.

• Due to increased atomic radius and increased shielding effect

• Due to decreased atomic radius and decreased shielding effect

• Due to increased nuclear charge

• Due to decreased electron affinity

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Why does fluorine have a higher ionization energy than iodine?

• Fluorine has a higher electronegativity

• Fluorine has a higher atomic mass

• Fluorine has a smaller atomic radius

• Fluorine has more protons in its nucleus

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Which element has the highest ionization energy?

• Sodium (Na)

• Magnesium (Mg)

• Aluminum (Al)

• Neon (Ne)

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