H2 H. +::HThe Lewis representation above depicts a reaction between hydrogen (blue) and a main-group element from groupв (red).In this representation, each Y atom needsbond(s) with atoms of H.electron(s) to complete its octet, and gains these electrons by formingThere areunshared electron pair(s) andbonding electron pair(s) in the product molecule.The bonds in the product areSubmit AnswerRetry Entire Group

There are two types of bond formation - 1- ionic bond (donation of electron) 2- covalent bond…

H 2 H. + H:Y: The Lewis representation above depicts a reaction between hydrogen (blue) and a main-group element from group e (red). In this representation, each Y atom needs electron(s) to complete its octet, and gains these electrons by forming bond(s) with atoms of H. There are unshared electron pair(s) and bonding electron pair(s) in the product molecule. The bonds in the product are

H 2 H. + H:Y: The Lewis representation above depicts a reaction between hydrogen (blue) and a main-group element from group e (red). In this representation, each Y atom needs electron(s) to complete its octet, and gains these electrons by forming bond(s) with atoms of H. There are unshared electron pair(s) and bonding electron pair(s) in the product molecule. The bonds in the product are

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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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 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 which is the more polar bond in each of the following pairs. msp;a.HForHClc.HBrorHClb.HClorHId.HIorHBr
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.
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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.
7.47 Which of the species listed has a Lewis structure with only one lone pair of electrons? F2 , CO32 , CH4 , PH3
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.
Based on the concept of formal charge, what is the central atom in (a) HCN (do not include H as a possibility)? b) NOCI (Cl is always a terminal atom)?
These are NOTlegitimate Lewisstructures (and aremissing formalcharges). Show (as inthe example) how apair of electrons canbe moved to make theLewis structurelegitimate.
Explain the terms resonance and delocalized electrons. When a substance exhibits resonance, we say that none of the individual Lewis structures accurately portrays the bonding in the substance. Why do we draw resonance structures?