(b) The Lewis structures for IFs and XeF4 are shown below. :F.:F: F: (i) What is the molecular geometry (shape) of the IFs molecule? (ii) (iii) ABSE square pyramidal What is the molecular geometry (shape) of the XeF4 molecule? AB4E2 Square planar Both IFs and XeF4 contain polar bonds, but only one is a polar molecule. Which of the substances is a polar molecule, and which of the substances is a non-polar molecule? Justify your decision. Filter (pa) Honkbas (po) od (iv) voled svaro orb no word? Which of the substances would more likely be soluble in water? Justify your decision based on intermolecular forces. (v) Both IFs and XeF4 are gases at room conditions. Which of the two compounds would you expect to behave more ideally (like an ideal gas)? Justify your decision. 004 0001 COST 003

(b) The Lewis structures for IFs and XeF4 are shown below. :F.:F: F: (i) What is the molecular geometry (shape) of the IFs molecule? (ii) (iii) ABSE square pyramidal What is the molecular geometry (shape) of the XeF4 molecule? AB4E2 Square planar Both IFs and XeF4 contain polar bonds, but only one is a polar molecule. Which of the substances is a polar molecule, and which of the substances is a non-polar molecule? Justify your decision. Filter (pa) Honkbas (po) od (iv) voled svaro orb no word? Which of the substances would more likely be soluble in water? Justify your decision based on intermolecular forces. (v) Both IFs and XeF4 are gases at room conditions. Which of the two compounds would you expect to behave more ideally (like an ideal gas)? Justify your decision. 004 0001 COST 003

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter10: Molecular Structure And Bonding Theories

Section: Chapter Questions

Problem 10.123QE

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For each of the following molecules or molecular ions, give the steric number, sketch and name the approximate molecular geometry, and describe the direction of any distortions from the approximate geometry due to lone pairs. In each case, the central atom is listed first and the other atoms are all bonded directly to it. (a) TeH2 (b) AsF3 (c) PCl4+ (d) XeF5+
7.30 The bond in HF is said to be polar, with the hydrogen carrying a partial positive charge. For this to be true, the hydrogen atom must have less than one electron around it. Yet the Lewis dot structure of HF attributes two electrons to hydrogen. Draw a picture of the electron density distribution for HF and use it to describe how the hydrogen atom can carry a partial positive charge. How can these two models of the HF bond (the electron density and the Lewis structure) seem so different and yet describe the same thing?
How many and bonds are present in the molecule HCN?
(a) Use the VSEPR theory to predict the structure of the NNO molecule. (b) The substance NNO has a small dipole moment. Which end of the molecule is more likely to be the positive end, based only on electronegativity?
For each of the following molecules, complete the Lewis structure and use the VSEPR model to determine the bond angles around each central atom. Note that the drawings are only skeleton structures and may depict the angles incorrectly.
Define formal charge and explain how to calculate it. What is the purpose of the formal charge? Organic compounds are composed mostly of carbon and hydrogen but also may have oxygen, nitrogen, and/or halogens in the formula. Formal charge arguments work very well for organic compounds when drawing the best Lewis structure. How do C, H, N, O, and Cl satisfy the octet rule in organic compounds so as to have a formula charge of zero?
A stable triatomic molecule can be formed that contains one atom each of nitrogen, sulfur, and fluorine. Three bonding structures are possible, depending on which is the central atom: NSF, SNF, and SFN. (a) Write a Lewis diagram for each of these molecules, indicating the formal charge on each atom. (b) Often, the structure with the least separation of formal charge is the most stable. Is this statement consistent with the observed structure for this molecule—namely, NSF, which has a central sulfur atom? (c) Does consideration of the electronegativities of N, S, and F from Figure 3.18 help rationalize this observed structure? Explain.
Consider the following flat drawing of methane (CH4) . a. What is HCH bond angle implied by this drawing if you assume it is flat? b. Are the electron domains of this flat CH4 spread out as much as possible? c. Use model materials to make a model of CH4 (methane). If you assembled it correctly, thefour bonds (bonding electron domains) of your model will be 109.5° apart. d. In which representation, the drawing above or the model in your hand (circle one) are theH’s of CH4 more spread out around the central carbon? e. Confirm that your model looks like the following drawing. The wedgebond represents a bond coming out of the page, and the dash bondrepresents a bond going into the page f. You will often see methane drawn as if it were flat (like on the previous page). Why is thismisleading, and what is left to the viewer’s imagination when looking at such a drawing?
7.47 Which of the species listed has a Lewis structure with only one lone pair of electrons? F2 , CO32 , CH4 , PH3
What is meant by a chemical bond? Why do atoms form bonds with each other? Why do some elements exist as molecules in nature instead of as free atoms?
The compound whose molecles contain one atom of C and one of O is named carbon monoxide rather than oxygen monocarbide. Why is this the case?
9.77 When a reaction is exothermic, is the sum of bond energies of products or of reactants greater?