TReview Topics)(ReferencesUse the References to access important vahues if needed for this question.For each bond, show the direction of polarity by selecting the correct partial charges.Ge-SevGe-BrY Br-SeThe most polar bond is9 more group attempts remainingRetry Entire GroupSubmit Answerhuluacer96

The polarity in a bond is due to the difference in electronegativity of the bonding atoms.…

Answered: TReview Topics) (References Use the…

Living by Chemistry

2nd Edition

ISBN:9781464142314

Author:Angelica M. Stacy

Publisher:Angelica M. Stacy

ChapterU2: Smells: Molecular Structure And Properties

Section: Chapter Questions

Problem 15STP

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A compound is being tested for use as a rocket propellant. Analysis shows that it contains 18.54% F, 34.61% Cl, and 46.85% O. (a) Determine the empirical formula for this compound. (b) Assuming that the molecular formula is the same as the empirical formula, draw a Lewis diagram for this molecule. Review examples elsewhere in this chapter to decide which atom is most likely to lie at the center. (c) Use the VSEPR theory to predict the structure of the molecule from part (b).
Mixing SbCl3 and GaCl3 in a 1:1 molar ratio (using liquid sulfur dioxide as a solvent) gives a solid ionic compound of empirical formula GaSbCl6 . A controversy arises over whether this compound is (SbCl2+)(GaCl4) or (GaCl2+)(SbCl4) . (a) Predict the molecular structures of the two anions. (b) It is learned that the cation in the compound has a bent structure. Based on this fact, which formulation is more likely to be correct?
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.
On the basis of the electronegativity values given in Fig. 12.3, indicate whether each of the following bonds would be expected to be covalent, polar covalent, or ionic. msp;a.SSb.SHc.SK
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.
Complete the rest of the table for N, O or X by drawing the number of Lewis structures specified.
Under certain conditions, the stable form of sulfur consists of rings of eight sulfur atoms. Draw the Lewis diagram for such a ring.
Give the Lewis structure of the followingcompound by indicating all bonds and lone pairelectrons as dots.
The total number of σ bonds in H-C≡C-C≡C-C≡C-H is???
Give the approximate values for the indicated bond angles inthe following molecules:
Ignoring tables of electronegativity values and guided onlyby the periodic table, arrange these atoms in order ofincreasing electronegativity: O, F, S, Si, K. Briefly explainyour reasoning
Describe the difference between a full Lewis structure and bond-line notation. What changes? Why is it easier to write?Dont

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