Periodic Trends Quiz

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

• Due to increased nuclear charge and decreased atomic radius

• Due to decreased nuclear charge and increased atomic radius

• Due to increased electron shielding

• Due to decreased electron shielding

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What is the trend in atomic radius as you move down a group in the periodic table?

• It decreases

• It remains constant

• It increases

• It first increases then decreases

Predict the element that would have a higher electron affinity: Oxygen (O) or Sulfur (S), and justify your answer.

• Oxygen, because it is smaller in size

• Sulfur, because it is larger in size

• Oxygen, because it has a higher nuclear charge

• Sulfur, because it has more electron shielding

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Which of the following elements has the highest electronegativity?

• Sodium (Na)

• Chlorine (Cl)

• Aluminum (Al)

• Sulfur (S)

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Which of the following elements has the smallest ionization energy?

• Helium (He)

• Lithium (Li)

• Fluorine (F)

• Neon (Ne)

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Analyze the trend in metallic character as you move from left to right across a period and provide a reason for this trend.

• It increases due to increased nuclear charge

• It decreases due to increased nuclear charge

• It remains constant due to electron shielding

• It decreases due to decreased atomic radius

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Compare and contrast the trends in ionization energy and electron affinity across a period. How do these trends relate to each other?

• Both increase; related to increased nuclear charge

• Both decrease; related to increased atomic radius

• Ionization energy increases, electron affinity decreases; unrelated

• Ionization energy decreases, electron affinity increases; unrelated

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Design an experiment to investigate the trend in reactivity of alkali metals with water. What observations would you expect?

• Reactivity decreases down the group; expect less vigorous reactions

• Reactivity increases down the group; expect more vigorous reactions

• Reactivity remains constant; expect similar reactions

• Reactivity is unpredictable; expect varied reactions

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Synthesize information about periodic trends to predict which element in the third period would have the highest melting point and explain why.

• Sodium (Na), due to its metallic bonding

• Silicon (Si), due to its covalent network structure

• Chlorine (Cl), due to its molecular structure

• Argon (Ar), due to its noble gas configuration

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Evaluate the effect of electron shielding on the atomic radius as you move down a group in the periodic table.

• Electron shielding decreases, causing a smaller atomic radius

• Electron shielding increases, causing a larger atomic radius

• Electron shielding remains constant, causing no change in atomic radius

• Electron shielding decreases, causing a larger atomic radius