The Lewis structure for the chlorate ion is :0: Calculate the formal charge on the chlorine (Cl ) atom. Express your answer as an integer. , View Available Hint(s) formal charge on Cl = Submit Part B Calculate the formal charge on each of the oxygen (0) atoms labeled a, b, and c in the following Lewis structure. :0: Express your answers as integers separated by commas. • View Available Hint(s) formal charge on Oa, Ob, Oc = Submit prmal charges to predict the most stable structure he interactive activity shows how to calculate the formal charge of atoms in a structure. These formal charges can be used to predict the resonance structure that contributes most to the stability of a molecule or ion. The struc enerally the most stable. Part C What are the formal charges on the sulfur (S), carbon (C), and nitrogen (N) atoms, respectively, in the resonance structure that contributes most to the stability of the thiocyanate ion, SCN ? The possible resonance structures for the thiocyanate ion, SCN , are S=c=N 5-c=N]" [:s=c-N]" Structure A Structure B Structure C Express your answers as integers separated by commas. • View Available Hint(s) formal charge on sulfur (S), carbon (C) and nitrogen (N ) atoms =

The Lewis structure for the chlorate ion is :0: Calculate the formal charge on the chlorine (Cl ) atom. Express your answer as an integer. , View Available Hint(s) formal charge on Cl = Submit Part B Calculate the formal charge on each of the oxygen (0) atoms labeled a, b, and c in the following Lewis structure. :0: Express your answers as integers separated by commas. • View Available Hint(s) formal charge on Oa, Ob, Oc = Submit prmal charges to predict the most stable structure he interactive activity shows how to calculate the formal charge of atoms in a structure. These formal charges can be used to predict the resonance structure that contributes most to the stability of a molecule or ion. The struc enerally the most stable. Part C What are the formal charges on the sulfur (S), carbon (C), and nitrogen (N) atoms, respectively, in the resonance structure that contributes most to the stability of the thiocyanate ion, SCN ? The possible resonance structures for the thiocyanate ion, SCN , are S=c=N 5-c=N]" [:s=c-N]" Structure A Structure B Structure C Express your answers as integers separated by commas. • View Available Hint(s) formal charge on sulfur (S), carbon (C) and nitrogen (N ) atoms =

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

The Lewis structure of acetone is Circling the carbonyl carbon, i.e., the carbon atom attached to oxygen, and its octet gives Circling the oxygen atom and its octet gives Thus, atoms share electrons in making bonds, and a pair of electrons may be included in the octet of two different atoms. When computing the formal charge on an atom, the number of electrons that belong to that atom is compared with the number of electrons the atom would have in the unbonded and neutral state. If the two numbers are the same, the formal charge on the atom is zero. In a Lewis structure both electrons in an unshared pair belong to the atom, and one of every pair of shared (bonding) electrons belongs to the atom.
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.
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)?
Two possible Lewis diagrams for sulfine (H2CSO) are (a) Compute the formal charges on all atoms. (b) Draw a Lewis diagram for which all the atoms in sulfine have formal charges of zero.
How many resonance structures can be drawn for the hydrogen tellurate ion (HTeO4–) in which the central tellurium atom bears a –1 formal charge and the oxygens bear formal charges of either zero or –1? Enter your answer as a whole number.
Consider the incomplete structure shown. Determine the formal charge on the bromine atom in the structure. If the atom is formally neutral, indicate a charge of zero.
In the BEST Lewis structure for hydrogen cyanide, HCN, the formal charge charge on H is __________, the formal charge on C is___________ , and the formal charge on N is _________. Indicate formal charge with a sign followed by a numerical charge (e.g. -2, +1) unless the charge is 0, then enter 0.
which one is favored and why. Predict formal charges for each atom in both resonance forms and use them to support the argument and justification.
For the carbonate ion (CO32-), there are 3 resonance structures. For any given structure what would the formal charge be for an oxygen that has a single bond to the central carbon atom?
What is the formal charge on the iodine atom in the iodate ion, IO3–? give the correct answer and solve it
Calculate formal charges for the nonhydrogen atoms in the following molecules:
Draw the Lewis structure for one of the possible resonance structure for the chlorate ion (ClO3−). Minimize the formal charge assigned to each atom. Include all nonzero formal charges.