Show how these elements combine into octet-rule ionic compounds, as in the first example.First, draw atomic Lewis structures for the atoms and their O.R. ions. Show their charges, anduse them to find the unit formula, and the name. Then draw atomic Lewis structures for allatoms in the formula unit together, show with arrows how all e s are transferred to make theions, and draw the Lewis structure of the ionic compound.Unit formulaAtomsO.R. ionsNameTransfer e s with arrowsLewis StructureLizNle1e30LithiumLi. + •N•Li.•N• Li.Li30Li Li Li :N:nitride)leLi.PbandKandH

Answered: Show how these elements combine into…

Pushing Electrons

4th Edition

ISBN:9781133951889

Author:Weeks, Daniel P.

Publisher:Weeks, Daniel P.

Chapter1: Lewis Structures

Section: Chapter Questions

Problem 52EQ

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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.
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.
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]
rite the Lewis structure for each of the following atoms. msp;a.He(Z=2)d.Ne(Z=10)b.Br(Z=35)e.I(Z=53)c.Sr(Z=38)f.Ra(Z=88)
7.97 Consider the structure shown below for as well as any other important resonance structures. (a) What is the expected O—N—O bond angle in this structure? (b) The molecule contains N—O bonds of two different lengths. How many sborter N—O bonds would be present?
Which statement(s) is/are true about bond enthalpy? (a) The bond energy for a triple bond between A and B is three times that of a single bond between A and B. (b) H for the breaking of a bond is always a negative number. (c) Energy is required to make a bond. (d) Bond enthalpy is defined only for bonds broken or formed in the gaseous state. (e) The presence of bonds does not influence the geometry of a molecule. However, the presence of bonds affects the value of the bond enthalpy between two atoms.
These are NOTlegitimate Lewisstructures (and aremissing formalcharges). Show (as inthe example) how apair of electrons canbe moved to make theLewis structurelegitimate.
The molecules BH3 and SF6 and the ion SO42 exist and are stable. Draw a Lewis structure of each,and comment on whether they are exceptions to Lewis’ octet rule.
Represent the following reaction using Lewis structures: I+II2
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.
Show how these elements combine into octet-rule ionic compounds, as in the first example. First, draw atomic Lewis structures for the atoms and their O.R. ions. Show their charges, and use them to find the unit formula, and the name. Then draw atomic Lewis structures for all atoms in the formula unit together, show with arrows how all e¯s are transferred to make the ions, and draw the Lewis structure of the ionic compound. Atoms O.R. ions Unit formula Lewis Structure Name Transfer e¯s with arrows Mg + Br Magnesium bromide Li + C Lithium carbide Ge + S

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