Exploring Periodic Table Trends

What is ionization energy?

• The energy needed to add an electron

• The energy needed to remove an electron

• The energy needed to split an atom

• The energy needed to form a bond

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Which element has more electron shells, lithium or potassium?

• Neither has electron shells

• Potassium

• Both have the same number of shells

• Lithium

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What effect does electron shielding have on potassium's valence electron?

• It has no effect on the electron

• It holds the electron more tightly to the nucleus

• It attracts the electron closer to the nucleus

• It makes the electron more likely to leave

As you go down a group, what happens to ionization energy?

• It fluctuates randomly

• It remains the same

• It decreases

• It increases

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Why does ionization energy increase as you go across a period?

• Because the number of electron shells increases

• Because the number of protons decreases

• Because the effective nuclear charge increases

• Because the atomic radius increases

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What happens to atomic radius as you go down a group?

• It fluctuates randomly

• It increases

• It decreases

• It remains the same

Why does atomic radius decrease as you go across a period?

• Because the number of electron shells decreases

• Because the effective nuclear charge decreases

• Because the effective nuclear charge increases

• Because the number of protons decreases

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What is electronegativity?

• The energy needed to remove an electron

• The size of an atom

• The ability of an atom to attract electrons

• The number of electron shells in an atom

As you go down a group, what happens to electronegativity?

• It increases

• It remains the same

• It decreases

• It fluctuates randomly

Why does electronegativity increase as you go across a period?

• Because the number of electron shells increases

• Because the number of protons decreases

• Because the number of protons increases

• Because the effective nuclear charge decreases

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NGSS.HS-PS1-1

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