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Which of the options below provides a reason why the covalent radius of hafnium (1.44 Å) is less than that of zirconium (1.45 Å), even though the element above it in the periodic table? A. Between Zr and Hf lies the 4d10 configuration due to the transition metals. This leads to much greater Z* because the d electrons are so poor at shielding. Thus Hf is smaller than expected for an element in a higher shell than Zr, called the Scandide contraction. B. Hf being below Zr suggests that it will have a smaller atomic radius because the trend shows a decrease going down a group. C. Hf is below Zr and has a smaller ionisation energy, electron affinity and electronegativity compared to Zr. This reduces its atomic radius, thus leading to it having a smaller atomic radius compared to that of Zr. D. Between Zr and Hf lies the 4f14 configuration due to the Lanthanides. This leads to much greater Z* because the f electrons are so poor at shielding. Thus Hf is smaller than expected for an element in a higher shell than Zr, called the Lanthanide contraction.

Which of the options below provides a reason why the covalent radius of hafnium (1.44 Å) is less than that of zirconium (1.45 Å), even though the element above it in the periodic table? A. Between Zr and Hf lies the 4d10 configuration due to the transition metals. This leads to much greater Z* because the d electrons are so poor at shielding. Thus Hf is smaller than expected for an element in a higher shell than Zr, called the Scandide contraction. B. Hf being below Zr suggests that it will have a smaller atomic radius because the trend shows a decrease going down a group. C. Hf is below Zr and has a smaller ionisation energy, electron affinity and electronegativity compared to Zr. This reduces its atomic radius, thus leading to it having a smaller atomic radius compared to that of Zr. D. Between Zr and Hf lies the 4f14 configuration due to the Lanthanides. This leads to much greater Z* because the f electrons are so poor at shielding. Thus Hf is smaller than expected for an element in a higher shell than Zr, called the Lanthanide contraction.

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Which of the options below provides a reason why the covalent radius of hafnium (1.44 Å) is less than that of zirconium (1.45 Å), even though the element above it in the periodic table? A. Between Zr and Hf lies the 4d10 configuration due to the transition metals. This leads to much greater Z* because the d electrons are so poor at shielding. Thus Hf is smaller than expected for an element in a higher shell than Zr, called the Scandide contraction. B. Hf being below Zr suggests that it will have a smaller atomic radius because the trend shows a decrease going down a group. C. Hf is below Zr and has a smaller ionisation energy, electron affinity and electronegativity compared to Zr. This reduces its atomic radius, thus leading to it having a smaller atomic radius compared to that of Zr. D. Between Zr and Hf lies the 4f14 configuration due to the Lanthanides. This leads to much greater Z* because the f electrons are so poor at shielding. Thus Hf is smaller than expected for an element in a higher shell than Zr, called the Lanthanide contraction.
Transcribed Image Text:Which of the options below provides a reason why the covalent radius of hafnium (1.44 Å) is less than that of zirconium (1.45 Å), even though the element above it in the periodic table? A. Between Zr and Hf lies the 4d10 configuration due to the transition metals. This leads to much greater Z* because the d electrons are so poor at shielding. Thus Hf is smaller than expected for an element in a higher shell than Zr, called the Scandide contraction. B. Hf being below Zr suggests that it will have a smaller atomic radius because the trend shows a decrease going down a group. C. Hf is below Zr and has a smaller ionisation energy, electron affinity and electronegativity compared to Zr. This reduces its atomic radius, thus leading to it having a smaller atomic radius compared to that of Zr. D. Between Zr and Hf lies the 4f14 configuration due to the Lanthanides. This leads to much greater Z* because the f electrons are so poor at shielding. Thus Hf is smaller than expected for an element in a higher shell than Zr, called the Lanthanide contraction.
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