The content discusses the concept of formal charge in chemistry, emphasizing its role in understanding bonding in molecules or ions. Specifically, it addresses the formal charge as the hypothetical charge an element would have if bonding electrons were shared equally.### Explanation:We are considering the sulfite ion, \( \text{SO}_3^{2-} \). The discussion focuses on using formal charge and electronegativity to determine the most accurate Lewis structure representation.**Task: Assign Formal Charges**1. **Objective:** Assign formal charges to the elements in the given Lewis structures.2. **Instructions:** Count oxygen atoms starting from the left for each structure.### Diagram Description:There are three structures labeled A, B, and C.- **Structure A:** - Central sulfur (S) atom is bonded to three oxygen (O) atoms. Double bonds and lone pairs are depicted.- **Structure B and C:** - Similar layout with variation in double bonds and lone pairs, affecting formal charge distribution.**Table for Formal Charges:**This section provides a systematic way to specify formal charges for sulfur (S) and each oxygen atom (\( O_1, O_2, O_3 \)) in structures A, B, and C.### Selection:2. **Result:** Determination of the best Lewis structure for \( \text{SO}_3^{2-} \) which is indicated by selecting one of the options (A, B, or C).This educational content helps students practice calculating formal charges and applying theoretical principles to practical scenarios in molecular chemistry.

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The formal charge is the "charge" an element would have in a molecule or ion if all of the bonding electrons were shared equally between atoms. We can draw three inequivalent Lewis structures for the sulfite ion, SO32. The concepts of formal charge and electronegativity can help us choose the structure that is the best representation. 1. Assign formal charges to the elements in each of the structures below. Note: Count oxygen atoms starting from the left for each structure. Formal Charge S 0₁ 0₂ 03 A :0: 2. The best Lewis structure for SO3²- is A . B –8: • Previous Next

The formal charge is the "charge" an element would have in a molecule or ion if all of the bonding electrons were shared equally between atoms. We can draw three inequivalent Lewis structures for the sulfite ion, SO32. The concepts of formal charge and electronegativity can help us choose the structure that is the best representation. 1. Assign formal charges to the elements in each of the structures below. Note: Count oxygen atoms starting from the left for each structure. Formal Charge S 0₁ 0₂ 03 A :0: 2. The best Lewis structure for SO3²- is A . B –8: • Previous Next

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Draw the best Lewis Structure for SOCl2 based on overall formal charges. Answer the questions below based on that structure. How many (total) bonding electron pairs are in the molecule? How many (total) non-bonding electron pairs are in the molecule? How many non-bonding electron pairs are on the central atom?
Write a Lewis structure for each of the following polyatomic ions. Show all bonding valenceelectron pairs as lines and all nonbonding valence electron pairs as dots. For those ions thatexhibit resonance, draw the various possible resonance forms.a. phosphate ion, PO4 3-b. chlorate ion, ClO3-
An incomplete Lewis structure is shown below. The structure only shows the atoms and how they are connected. The molecule has a net charge of zero. H I H-C-C-N-O | H Complete the Lewis structure giving all atoms full octets. If there is more than one way to do this, draw resonance structures showing all possibilities. If not, just draw one Lewis structure. Be sure to write in any non-zero formal charges.
Draw Lewis structure(s) for the carbonate lon (CO₂). If there are equivalent resonance structures, draw all of them. n D co₂2: 0 . Draw one structure per sketcher box, and separate added sketcher boxes with the symbol. Do not include overall lon charges or formal charges in your drawing. Do not draw double bonds to oxygen unless they are needed in order for the central atom to obey the octet rule. ● 6 # H Ⓒ CH, CHO: 0 Y Chemic b Draw Lewis structure(s) for the acetaldehyde molecule (CH₂CHO). If there are equivalent resonance structures, draw all of the POLICE 81 MEDITE HARA (4) Y Draw one structure per sketcher box, and separate added sketcher boxes with the symbol. Do not include overall ion charges or formal charges in your drawing. Do not draw double bonds to oxygen unless they are needed in order for the central atom to obey the octet rule. ARQQA 000-ZIF www HEADING Chartlkoodn MES DE A V Ja remove 000-n [ MacBook Air
Draw three resonance structures for N3-. This species has its three atoms bonded sequentially in the following fashion: N-N-N. Draw your resonance structures so that the atoms in them are bonded together in this order. Select the most important resonance structure for this species based on the formal charges on the atoms of the three resonance structures you have drawn. Now select the statement from the multiple choices which is true about this most important resonance structure.In the most important resonance structure of N3- : a) The leftmost bond (between N and N) is a single bond.b) The rightmost bond (between N and N) is a single bond.c) The formal charge on the leftmost (N) atom is -1.d) The number of nonbonding pairs (lone pairs) of electrons on the leftmost (N) atom is 4.e) The number of nonbonding (lone) pairs of electrons on the rightmost (N) atom is 4.
Use the figure to find the electronegativity difference between each of the following pairs of elements, then use the table below to classify the bonds that occur between them as pure covalent, polar covalent, or ionic. Electronegativity Difference (ΔENΔEN) Bond Type Example zero (0−0.40−0.4) pure covalent Cl2Cl2 intermediate (0.4−2.00.4−2.0) polar covalent HFHF large (2.0+2.0+) ionic NaClNaCl Find the electronegativity difference between K and Cl. Express your answer using two significant figures.
Draw the best Lewis Structure for ClO4– based on overall formal charges. Answer the questions below based on that structure. How many (total) bonding electron pairs are in the molecule? _______ How many (total) non-bonding electron pairs are in the molecule? _______ How many non-bonding electron pairs are on the central atom? _______
9. Draw all the possible resonance structures for the iodate ion. How many resonance structures can you have in total for iodate?
Draw the Lewis structures of the neutral atom of Bromine and the ion of Bromine. Determine also the number of electrons gained or lost in forming an ion. ------------------IN SHORT------------------- Draw the Lewis Structures for: 1. Neutral Atom of Bromine 2. Ion of Bromine - Determine also the number of electrons gained or lost in forming an ion. NOTE : The Answer must be two different Lewis Structures, one for the Neutral Atom of Bromine and one for the Ion of Bromine. Both are different from each other so the answer should have 2 forms of lewis structures.
A newly discovered element Lm has 3 valence electrons. How many total valence electrons are in LmF3 molecule, a molecule that Lm forms with fluorine? Draw a valid Lewis Structure for the molecule LmF3 that Lm forms with fluorine and use your Lewis structure to determine the number of lone pairs of electrons around the central Lm atom in this molecule. What is the formal charge of Lm in LmF3? (Number and sign of formal charge) What is the hybridization of Lm according to the hybrid orbital model?
The formal charge is the "charge" an element would have in a molecule or ion if all of the bonding electrons were shared equally between atoms. Use the References to access important values if needed for this question. We can draw three inequivalent Lewis structures for dinitrogen monoxide, N₂O . The concepts of formal charge and electronegativity can help us choose the structure that is the most significant representation. 1. Assign formal charges to the elements in each of the structures below. Formal Charge N₁ N₂ :N,=N,-O: || A N=N,=Ô N-N,=O: C 2. The structure that contributes most significantly to the overall electronic structure of N₂O is ↑ Formal Charge
ng and lear X G The element in period 5 that has X C Solved The following Lewis diagr. X nt/takeCovalentActivity.do?locator-assignment-take The formal charge is the "charge" an element would have in a molecule or ion if all of the bonding electrons were shared equally between atoms. Formal Charge 01 We can draw three inequivalent Lewis structures for carbon dioxide, CO₂. The concepts of formal charge and electronegativity can help us choose the structure that is the most significant representation. 1. Assign formal charges to the elements in each of the structures below. C [Review Topics] [References] Use the References to access important values if needed for this question. 02 :0₁-C=0₂: A 0,=C=0₂ :0,=C-0₂: + B 999 C *** 2. The structure that contributes most significantly to the overall electronic structure of CO₂ is. AG ENG neme Next 11:52 AM 11/28/2022 [