Periodic Table Trends and Electronegativity Insights

What is atomic radius?

• The energy required to remove an electron

• The distance between the outermost electrons and the nucleus

• The size of an atom, measured as half the distance between two nuclei of identical atoms

• The number of protons in the nucleus

How does atomic radius change as you move down a group in the periodic table?

• It fluctuates

• It decreases

• It remains the same

• It increases

What is the shielding effect?

• The attraction between the nucleus and the outermost electrons

• The repulsion between electrons in the same shell

• The increase in nuclear charge

• The decrease in attraction between the nucleus and an electron in atoms with multiple electron shells

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Why does atomic radius decrease across a period?

• Because the number of electron shells increases

• Because the shielding effect increases

• Because the effective nuclear charge increases

• Because the atomic number decreases

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What is first ionization energy?

• The energy released when an electron is added to an atom

• The energy required to remove the most loosely held electron from an atom

• The energy required to remove a proton from the nucleus

• The energy required to add an electron to an atom

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How does first ionization energy change as you move down a group?

• It increases

• It remains the same

• It decreases

• It fluctuates

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What is electronegativity?

• The number of protons in the nucleus

• The energy required to remove an electron

• The measure of how strongly an atom attracts shared electrons to itself

• The size of an atom

Which element is the most electronegative?

• Helium

• Neon

• Fluorine

• Oxygen

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How does electronegativity change across a period?

• It remains the same

• It fluctuates

• It decreases

• It increases

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Where on the periodic table would you find elements with the lowest first ionization energy?

• Upper right

• Lower left

• Upper left

• Lower right