How would you answer part III of this FRQ? this is a non graded practice. (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 pyramidalWhat is the molecular geometry (shape) of the XeF4 molecule?AB4E2Square planarBoth IFs and XeF4 contain polar bonds, but only one is a polar molecule. Which of the substances is apolar 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 onintermolecular forces.(v)Both IFs and XeF4 are gases at room conditions. Which of the two compounds would you expect tobehave more ideally (like an ideal gas)? Justify your decision.004 0001 COST 003

(iii) Polar and Non-Polar Molecules: Iodine Monofluoride (IF₅):Iodine monofluoride has a trigonal…

Answered: (b) The Lewis structures for IFs and…

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter7: Chemical Bonding And Molecular Structure

Section: Chapter Questions

Problem 7.43PAE

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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.
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.
7.47 Which of the species listed has a Lewis structure with only one lone pair of electrons? F2 , CO32 , CH4 , PH3
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?
What aspect of the following Lewis structure indicates that the concept of coordinate covalency is needed to explain the bonding in the molecule?
The percent ionic character of a bond can be approximated by the formula 16+3.52 , where is the magnitude of the difference in the electronegativities of the atoms (see Fig. 3.18). Calculate the percent ionic character of HF, HCl, HBr, HI, and CsF, and compare the results with those in Table 3.7.
7.50 Chemical species are said to be isoelectronic if they have the same Lewis structure (regardless of charge). Consider these ions and write a Lewis structure for a neutral molecule that is isoelectronic with each of them, (a) CN , (b) NH4+ . (c) CO32

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