Consider the A2X4 molecule depicted here, where A and Xare elements. The A¬A bond length in this molecule is d1,and the four A¬X bond lengths are each d2. (a) In terms ofd1 and d2, how could you define the bonding atomic radii ofatoms A and X? (b) In terms of d1 and d2, what would you predictfor the X¬X bond length of an X2 molecule? [Section 7.3]

Consider the A2X4 molecule depicted here, where A and Xare elements. The A¬A bond length in this molecule is d1,and the four A¬X bond lengths are each d2. (a) In terms ofd1 and d2, how could you define the bonding atomic radii ofatoms A and X? (b) In terms of d1 and d2, what would you predictfor the X¬X bond length of an X2 molecule? [Section 7.3]

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter3: Atomic Shells And Classical Models Of Chemical Bonding

Section: Chapter Questions

Problem 30P

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Concept explainers

Quantum Mechanical Treatment of the Valence Bond Theory

Quantum mechanical treatment of valence bond theory refers to the relationship established between the quantum mechanical theory and the valence bond theory to describe the chemical bonding in a particular molecule.

Question

Consider the A2X4 molecule depicted here, where A and X
are elements. The A¬A bond length in this molecule is d1,
and the four A¬X bond lengths are each d2. (a) In terms of
d1 and d2, how could you define the bonding atomic radii of
atoms A and X? (b) In terms of d1 and d2, what would you predict
for the X¬X bond length of an X2 molecule? [Section 7.3]

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Consider the A2X4 molecule depicted here, where A and Xare elements. The A¬A bond length in this molecule is d1,and the four A¬X bond lengths are each d2. (a) In terms ofd1 and d2, how could you define the bonding atomic radii ofatoms A and X? (b) In terms of d1 and d2, what would you predictfor the X¬X bond length of an X2 molecule?
Consider the A2X4 molecule depicted here, where A and X are elements. The A – A bond length in this molecule is d1, and the four A – X bond lengths are each d2 (a) In terms od d1 and d2, how could you define the bonding atomic radii of atoms A and X? (b) In terms of d1 and d2, what would you predict for the X-X bond length of an X2 molecule?
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A resident expert on electronegativity comes up to visit with you. He makes two claims (seen below) about electronegativity with relation to covalent bonding. Is the expert correct or can you refute him with your knowledge of electronegativity? (a) If a diatomic molecule is made up of atoms X and Y, which have different electronegativities, the molecule must be polar. (b) The farther two atoms are apart in a bond, the larger the dipole moment will be.
(c) Draw the orbital diagrams and Lewis symbols to depict the formation of Na* and CI ions from the atoms. Give the formula of the compound formed. (d) The predicted bond length for HF is 109 pm (the sum of the covalent radii of H, 37 pm and F. 72 pm), however the actual bond length for HF is shorter (92 pm). It was observed that the difference between predicted and actual bond lengths becomes smalleor going down the halogen group from HF to HI Describe these observations
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For many years after they were discovered, it was believed that the noble gases could not form compounds. Now we know that belief to be incorrect. A mixture of xenon and fluorine gases, confined in a quartz bulb and placed on a windowsill, is found to slowly produce a white solid. Analysis of the compound indicates that it contains 77.55% Xe and 22.45% F by mass.(a) What is the formula of the compound?(b) Write a Lewis structure for the compound.(c) Predict the shape of the molecules of the compound.(d) What hybridization is consistent with the shape you predicted?
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