Draw the Lewis structure, including all lone pairs and non-zero formal charges, for the molecule below.ClF5

Step 1: Calculate the total valence electronsAtomValence Electrons# of AtomsCl71F75Total7(1) + 7(5)…

Answered: Draw the Lewis structure, including all…

Chemistry & Chemical Reactivity

9th Edition

ISBN:9781133949640

Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Chapter8: Bonding And Molecular Structure

Section8.5: Exceptions To The Octet Rule

Problem 1Q

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Consider the pyrosulfate ion, S2O72-. It has no sulfurâ€“sulfur nor oxygenâ€“oxygen bonds. (a) Write a Lewis structure for the pyrosulfate ion using only single bonds. (b) What is the formal charge on the sulfur atoms for the Lewis structure you drew in part (a)? (c) Write another Lewis structure using six bonds and two Oâ€”S bonds. (d) What is the formal charge on each atom for the structure you drew in part (c)?
Write Lewis structures for these ions. Show all valence electrons and all formal charges. (a) Amide ion, NH2 (b) Bicarbonate ion, HCO3 (c) Carbonate ion, CO32 (d) Nitrate ion, NO3 (e) Formate ion, HCOO (f) Acetate ion, CH3COO
Draw Lewis structures for the following species. (The skeleton is indicated by the way the molecule is written.) (a) Cl2CO (b) H3Câ€”CN (c) H2Câ€”CH2
Experimental evidence indicates the existence of HC3N molecules in interstellar clouds. Write a plausible Lewis structure for this molecule.
A complete Lewis structure must show all nonzero formal charges. Complete each of thefollowing Lewis structures by adding any missing formal charges.
Carbon monoxide (CO) is an example of an overall neutral molecule (netcharge=0) that hasnon-zero formal charges. Draw a Lewis structure of carbon monoxide (CO).
Draw Lewis structures showing all valence electrons for these molecules. (a) C2H6 (b) CS2 (c) HCN
Draw Lewis structures for the following species. (The skeleton is indicated by the way the molecule is written.) (a) Cl2CO (b) H3CCN
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.
Write the Lewis structure and chemical formula of the compound with a molar mass of about 70 g/mol that contains 19.7% nitrogen and 80.3% fluorine by mass, and determine the formal charge of the atoms in this compound.
Successive substitution of F atoms for H atoms in the molecule NH3 produces the molecules NH2F, NHF2, and NF3. a. Draw Lewis structures for each of the four molecules. b. Using VSEPR theory, predict the geometry of each of the four molecules. c. Specify the polarity (polar or nonpolar) for each of the four molecules.
Carbon and sulfur form compounds with each other with the formulas CS2 and C3S2. Draw a Lewis structure for each compound that has a formal charge of zero for all atoms in the structure.

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Draw the Lewis structure, including all lone pairs and non-zero formal charges, for the molecule below. ClF 5