Decide whether the Lewis structure proposed for each molecule is reasonable or not. molecule OCI₂ Be H₂ CIF₂ proposed Lewis structure : CI- I Cl: H- Be H :F: Is this a reasonable structure? If not, why not? O Yes, it's a reasonable structure. O No, the total number of valence electrons is wrong. The correct number is: O No, some atoms have the wrong number of electrons around them. The symbols of the problem atoms are: 0 O Yes, it's a reasonable structure. O No, the total number of valence electrons is wrong. The correct number is: O No, some atoms have the wrong number of electrons around them. The symbols of the problem atoms are: O Yes, it's a reasonable structure. O No, the total number of valence electrons is wrong. The correct number is: O No, some atoms have the wrong number of electrons around them. The symbols of the problem atoms are: * If two or more atoms have the wrong number of valence electrons around them, just enter the chemical symbol for the atom as many times as necessary. For example, if two oxygen atoms have the wrong number of electrons around them, enter the symbol O twice. 9 Or 0.0 G

Decide whether the Lewis structure proposed for each molecule is reasonable or not. molecule OCI₂ Be H₂ CIF₂ proposed Lewis structure : CI- I Cl: H- Be H :F: Is this a reasonable structure? If not, why not? O Yes, it's a reasonable structure. O No, the total number of valence electrons is wrong. The correct number is: O No, some atoms have the wrong number of electrons around them. The symbols of the problem atoms are: 0 O Yes, it's a reasonable structure. O No, the total number of valence electrons is wrong. The correct number is: O No, some atoms have the wrong number of electrons around them. The symbols of the problem atoms are: O Yes, it's a reasonable structure. O No, the total number of valence electrons is wrong. The correct number is: O No, some atoms have the wrong number of electrons around them. The symbols of the problem atoms are: * If two or more atoms have the wrong number of valence electrons around them, just enter the chemical symbol for the atom as many times as necessary. For example, if two oxygen atoms have the wrong number of electrons around them, enter the symbol O twice. 9 Or 0.0 G

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 99AP: A stable triatomic molecule can be formed that contains one atom each of nitrogen, sulfur, and...

See similar textbooks

Similar questions

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?
Fill in the blanks in each line of the following table that involves characteristics of various bonds between nonmetals. The first line is already completed as an example.
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?
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
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.
According to the VSEPR model, what are the arrangements of two, three, four, five, and six valence-shell electron pairs about an atom?
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.
These are NOTlegitimate Lewisstructures (and aremissing formalcharges). Show (as inthe example) how apair of electrons canbe moved to make theLewis structurelegitimate.
Acrolein is the starting material for certain plastics. (a) Which bonds in the molecule are polar and which are nonpolar? (b) Which is the most polar bond in the molecule? Which atom is the partial negative end of this bond?
rite a Lewis structure for each of the following simple molecules. Show all bonding valence electron pairs as lines and all nonbonding valence electron pairs as dots. For those molecules that exhibit resonance, draw the various possible resonance forms. msp;a.SO2b.N2O(Nincenter)c.O3