In the VSEPR model, the geometry of the regions defined by the electron pairs in the valence shell of an atom is called the electron-pair geometry. A. The Lewis diagram for CS2 is: S=c=S Recall that for predicting geometry, double and triple bonds count as only one electron pair region. The electron-pair geometry around the C atom in CS, is There are unshared pair(s) around the central atom, so the geometry of the CS, molecule is B. The Lewis diagram for NO, is: 0-N=ö: Recall that for predicting geometry, double and triple bonds count as only one electron pair region. The electron-pair geometry around the N atom in NO2" is There are unshared pair(s) around the central atom, so the geometry of the NO," molecule is

In the VSEPR model, the geometry of the regions defined by the electron pairs in the valence shell of an atom is called the electron-pair geometry. A. The Lewis diagram for CS2 is: S=c=S Recall that for predicting geometry, double and triple bonds count as only one electron pair region. The electron-pair geometry around the C atom in CS, is There are unshared pair(s) around the central atom, so the geometry of the CS, molecule is B. The Lewis diagram for NO, is: 0-N=ö: Recall that for predicting geometry, double and triple bonds count as only one electron pair region. The electron-pair geometry around the N atom in NO2" is There are unshared pair(s) around the central atom, so the geometry of the NO," molecule is

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 94AP: The molecular ion S3N3 has the cyclic structure All SN bonds are equivalent. (a) Give six...

See similar textbooks

Similar questions

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.
The molecular ion S3N3 has the cyclic structure All SN bonds are equivalent. (a) Give six equivalent resonance hybrid Lewis diagrams for this molecular ion. (b) Compute the formal charges on all atoms in the molecular ion in each of the six Lewis diagrams. (c) Determine the charge on each atom in the polyatomic ion, assuming that the true distribution of electrons is the average of the six Lewis diagrams arrived at in parts (a) and (b). (d) An advanced calculation suggests that the actual charge resident on each N atom is 0.375 and on each S atom is +0.041 . Show that this result is consistent with the overall +1 charge on the molecular ion.
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?
White phosphorus (P4) consists of four phosphorus atoms arranged at the corners of a tetrahedron. Draw the valence electrons on this structure to give a Lewis diagram that satisfies the octet rule.
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.
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+
Given the bonds C N, C H, C Br, and S O, (a) which atom in each is the more electronegative? (b) which of these bonds is the most polar?
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.
Which of the following statements is false concerning bonding? Elements with extremely different electronegativities tend to form ionic bonds with each other. In an N—O bond. electron density is greater near the O atom. An N—O bond is an example of a polar covalent band. In general, chemical bonds form to minimize energy. The bond in KBr is formed by sharing electrons.
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?
Atoms form ions so as to achieve electron configurations similar to those of the noble gases. For the following pairs of noble gas configurations, give the formulas of two simple ionic compounds that would have comparable electron configurations. msp;a.[He]and[Ne]c.[He]and[Ar]b.[Ne]and[Ne]d.[Ne]and[Ar]