Which one of these statements is false?Lewis structures are resonance structures if they have the same fixed nuclear arrangement, but a differentdistribution of the electrons.O Molecules with resonance exhibit extra stability.A molecule has resonance if more than one correct Lewis structure can be drawn for the molecule.O Individual resonance structures exist as separate molecules and oscillate between the resonant structures.

Interpretation : We have to choose the incorrect options.

Answered: Which one of these statements is false?…

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter6: Covalent Bonding

Section: Chapter Questions

Problem 117QRT

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Similar questions

Two Lewis structures can be written for nitrosyl fluoride, which contains one nitrogen, one oxygen, and one fluorine atom per molecule. Write the two Lewis structures land assign a formal charge to each atom.
Three resonance forms can be drawn for the molecule N2O. Which resonance form is likely to more closely resemble the structure of this molecule? (a) (b) (c)
Chloromethane has the Lewis structure _______________________________ The carbon atom is sharing 4 electron pairs. In each shared pair the carbon atom “owns” 1 electron. The number of electrons that “belong” to carbon is ___. Carbon, being a Group ___ element would have 4 , outer shell electrons in the unbonded, neutral state. Therefore, the carbon atom in chloromethane has a formal charge of zero.
The “Chemistry in Focus" segment Hiding Carbon Dioxide- discusses attempts at sequestering (storing) underground CO2produced at power plants so as to diminish the: greenhouse effect. Draw all resonance structures of the CO2molecule.
What aspect of the following Lewis structure indicates that the concept of coordinate covalency is needed to explain the bonding in the molecule?
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 study of carbon-containing compounds and their properties is called organic chemistry. Besides carbon atoms, organic compounds also can contain hydrogen, oxygen, and nitrogen atoms (as well as other types of atoms). A common trait of simple organic compounds is to have Lewis structures where all atoms have a formal charge of zero. Consider the following incomplete Lewis structure for an organic compound called histidine (an amino acid), which is one of the building blocks of proteins found in our bodies: Draw a complete Lewis structure for histidine in which all atoms have a formal charge of zero.
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?
Write reasonable Lewis structures for the following species, none of which follow the octet rule. (a) BeCl2 (b) SeO2- (c) ClO3 (d) CH3
Consider the following compounds: CO2, SO2, KrF2, SO3, NF3, IF3, CF4, SF4, XeF4, PF5, TF5, and SCl6. These 12 compounds are all examples of different molecular structures. Draw the Lewis structures for each and predict the molecular structures. Predict the bond angles and the polarity of each. (A polar molecule has a net dipole moment, while a nonpolar molecule does not.) See Exercises 25 and 26 for the molecular structures based on the trigonal bipyramid and the octahedral geometries.
Draw resonance structures for each of these ions: NSO− and SNO−. (The atoms are bonded in the order given in each case, that is, S is the central atom in NSO−.) Use formal charges to determine which ion is likely to be more stable. Explain why the two ions cannot be considered resonance structures of each other.

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