Ionization Energy Trends Practice

What is ionization energy?

• Energy required to remove an electron
• Energy needed to split an electron
• Energy required to add an electron

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NGSS.HS-PS1-1

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Ionization energy __________ as you go down a group.

• stays the same

• decreases

• increases

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NGSS.HS-PS1-1

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Ionization energy __________ as you go across a period

• stays the same

• decreases

• increases

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NGSS.HS-PS1-1

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Select ALL that explain the ionization energy trend within periods going left to right

• electrons are closer to the nucleus

• their is a weak pull between electrons from the nucleus, making them easily moveable

• feel more of a pull from nucleus, making them harder to move

• electrons are further from the nucleus

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NGSS.HS-PS1-1

NGSS.HS-PS1-2

Select ALL that explain the ionization energy trend within groups going top to bottom.

• electrons are closer to the nucleus

• their is a weak pull between electrons from the nucleus, making them easily moveable

• feel more of a pull from nucleus, making them harder to move

• electrons are further from the nucleus

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NGSS.HS-PS1-1

NGSS.HS-PS1-2

Which element has the greater ionization energy?

• Magnesium (Mg)

• Phosphorus (P)

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NGSS.HS-PS1-1

Which element has the greater ionization energy?

• Iodine (I)

• Chlorine (Cl)

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NGSS.HS-PS1-1

NGSS.HS-PS1-2

 After the atom is ionized, it then requires more energy to remove a second electron because the second electron is nearer the nucleus.

• False
• True

Why is there a large jump in ionization energy 1 and 2 for Lithium?

• the valence electrons are harder to lose than core electrons

• the valence electrons are easier to lose than core electrons

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NGSS.HS-PS1-1

NGSS.HS-PS1-2

Which element has the greater ionization energy?

• Strontium
• Boron

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NGSS.HS-PS1-1

NGSS.HS-PS1-2