Periodic Families and Trends

Analyze the trend in electronegativity across a period from left to right. Which of the following best describes this trend?

• Electronegativity decreases because atomic radius increases.

• Electronegativity increases because atomic radius decreases.

• Electronegativity remains constant because the number of valence electrons is the same.

• Electronegativity decreases because ionization energy decreases.

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Using the periodic table, predict which element in the halogen family is most likely to gain an electron easily.

• Fluorine

• Chlorine

• Bromine

• Iodine

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Interpret the trend in atomic radius as you move down a group in the periodic table. Which statement is correct?

• Atomic radius decreases because the number of electron shells decreases.

• Atomic radius increases because the number of electron shells increases.

• Atomic radius remains constant because the number of valence electrons is the same.

• Atomic radius decreases because the nuclear charge increases.

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Predict the properties of noble gases based on their valence electron configuration. Which statement is correct?

• Noble gases are highly reactive because they have one valence electron.

• Noble gases are inert because they have a full valence shell.

• Noble gases are highly reactive because they have seven valence electrons.

• Noble gases are inert because they have an empty valence shell.

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Analyze the trend in ionization energy across a period from left to right. Which of the following best describes this trend?

• Ionization energy decreases because atomic radius increases.

• Ionization energy increases because atomic radius decreases.

• Ionization energy remains constant because the number of valence electrons is the same.

• Ionization energy decreases because electronegativity decreases.

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Interpret the trend in reactivity of halogens as you move down the group. Which statement is correct?

• Reactivity increases because atomic radius decreases.

• Reactivity decreases because atomic radius increases.

• Reactivity remains constant because the number of valence electrons is the same.

• Reactivity increases because ionization energy increases.

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NGSS.HS-PS1-2

Analyze the trend in atomic mass as you move across a period from left to right. Which of the following best describes this trend?

• Atomic mass decreases because the number of protons decreases.

• Atomic mass increases because the number of protons increases.

• Atomic mass remains constant because the number of valence electrons is the same.

• Atomic mass decreases because the number of neutrons decreases.

Interpret the trend in electronegativity as you move down a group in the periodic table. Which statement is correct?

• Electronegativity increases because atomic radius decreases.

• Electronegativity decreases because atomic radius increases.

• Electronegativity remains constant because the number of valence electrons is the same.

• Electronegativity increases because ionization energy increases.

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NGSS.HS-PS1-2

Analyze the trend in reactivity of alkaline earth metals as you move down the group. Which statement is correct?

• Reactivity increases because atomic radius increases.

• Reactivity decreases because atomic radius decreases.

• Reactivity remains constant because the number of valence electrons is the same.

• Reactivity decreases because ionization energy increases.

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NGSS.HS-PS1-1

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Predict which element in the alkaline earth metals is most likely to lose two electrons easily.

• Beryllium

• Magnesium

• Calcium

• Barium

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