Periodic Trends 2

Which of these statements is an accurate description of the ionization energies of elements in the periodic table?

• The ionization energy of lithium is greater than that of potassium.

• The ionization energy of iodine is greater than that of fluorine.

• The ionization energy of magnesium is greater than that of sulfur.

• The ionization energy of krypton is greater than that of neon.

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The atomic radius of magnesium is 150 pm. The atomic radius of strontium is 200 pm. What is the atomic radius of calcium?

• smaller than 150 pm

• greater than 200 pm

• between 150 and 200 pm

• not enough information

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Li has an ionization energy of 520 kJ/mol. F has an ionization energy of 1680 kJ/mol. Which of the following is a possible explanation for the trend?

• Fluorine has strong attractive forces between the nucleus and the electrons. It takes more energy to remove an electron from fluorine than lithium.

• Each electron on an atom has a set amount of energy. Since fluorine has more electrons, then it will have more ionization energy than lithium.

• Lithium has a smaller atomic radius than fluorine. It takes less energy for an electron to be added to the outer energy level on lithium than the outer energy level on fluorine.

• Ionization energy increases down the periodic table and decreases across the periodic table.

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Which element has the largest atomic radius?

• a

• b

• c

• d

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Which of these elements is the most electronegative?

• argon

• chlorine

• phosphorus

• sulfur

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Argon, chlorine, aluminum and sulfur are found in Period 3 of the periodic table.

– Order the elements argon, chlorine, aluminum, and sulfur from least electronegative to

most electronegative.

• Al, Ar, Cl, S

• Al, S, Cl, Ar

• Ar, Cl, S, Al

• Ar, Al, S, Cl

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Which element is most likely to ionize by losing two electrons?

• beryllium

• helium

• lithium

• oxygen

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Which statement best describes the name and location on the Periodic Table of the elements with the highest and lowest electronegativity, respectively?

• Helium, on the upper right, has the highest electronegativity, and Francium, on the lower left, has the lowest electronegativity.

• Fluorine, on the upper right, has the highest electronegativity, and Francium, on the lower left, has the lowest electronegativity.

• Neon, on the upper right, has the highest electronegativity, and Francium, on the lower left, has the lowest electronegativity.

• Hydrogen, on the upper left, has the highest electronegativity, and Radon, on the lower right, has the lowest electronegativity.

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Which of the following elements has the largest atomic radius?

• Calcium

• Sodium

• Potassium

• Magnesium

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Which statement below accurately describes the elements in Group 16 of the Periodic Table as considered from top to bottom?

• The atomic radii decrease and the ionization energies increase.

• The atomic radii increase and the ionization energies decrease.

• The atomic radii decrease and the ionization energies decrease.

• The atomic radii increase and the ionization energies increase.

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