1. (a) Lewis diagrams may look different but represent the same bonding between atoms.Pair the Lewis diagrams A through D to each other. Explain your choice.Structure AStructure BStructure CHHHStructure DHHH-C-HH-C-HO-HH--C-HO-H"HHHH-HH-O:-HH-##H-C-H HHH D:H-C-H 1. (b) A Lewis diagram can be related to one or more 3D VSEPR diagrams. Connect each ofthe VSEPR diagrams below to all of Structures A through D, in Question 1(a), that apply.Check your answers by building models based on the Lewis diagrams. You may need tomanipulate any models you build for the Lewis diagrams in 1(a) to match the VSEPRperspectives given below.H-HHHHHC--HH-H-H-HH-HH-HLewis structures Athrough D that relateto the VSEPR above.Lewis structures Athrough D that relateto the VSEPR above.Lewis structures Athrough D that relateto the VSEPR above.Lewis structures Athrough D that relateto the VSEPR above.

Step 1:Lewis diagrams (or Lewis structures) represent the bonding between atoms in a molecule and…

Answered: 1. (a) Lewis diagrams may look…

Chemistry

9th Edition

ISBN:9781133611097

Author:Steven S. Zumdahl

Publisher:Steven S. Zumdahl

Chapter8: Bonding: General Concepts

Section: Chapter Questions

Problem 7RQ: Define formal charge and explain how to calculate it. What is the purpose of the formal charge?...

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On the basis of the electronegativity values given in Fig. 12.3, indicate whether each of the following bonds would be expected to be covalent, polar covalent, or ionic. msp;a.SSb.SHc.SK
Write Lewis structures for: (a) PO43 (b) ICl4 (c) SO32 (d) HONO
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.
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.
Please don't provide handwritten solution .....
Decide whether these proposed Lewis structures are reasonable. proposed Lewis structure H : 0: - C. | : 0: : 0: H H O H-CEN: H Is the proposed Lewis structure reasonable? Yes. No, it has the wrong number of valence electrons. The correct number is: No, it has the right number of valence electrons but doesn't satisfy the octet rule. The symbols of the problem atoms are:* Yes. No, it has the wrong number of valence electrons. The correct number is: No, it has the right number of valence electrons but doesn't satisfy the octet rule. The symbols of the problem atoms are:* 0 Yes. No, it has the wrong number of valence electrons. The correct number is: No, it has the right number of valence electrons but doesn't satisfy the octet rule. The symbols of the problem atoms are:* * If two or more atoms of the same element don't satisfy the octet rule, just enter the chemical symbol as many times as necessary. For example, if two oxygen atoms don't satisfy the octet rule, enter "O,O". X 5
Nn.130. Subject:- Chemistry
A molecule is connected H₂CC (O) CH₂ where the oxygen is connected to the middle carbon and the outside carbons are also connected to the middle carbon. The hydrogens are connected to the outside carbons. Which of the following represents the Lewis Dot Structure for this compound? A) B) H-C-C-C-H C) H H OB H DE OD DA DC H H H 80: H H H-C-C-C-H HC- H-C-C=C-H Both A and B are correct H o: H Both C and D are correct H 80: H D) H ●● H-C-C-C-H H E) H H H - 80: H ●● H -C-C-H 80: H
Examples: Example: H▬N▬H HIN: Examples: :F Н lone pair : -bond pair (2 e-) single bond :F: Non-Polar 8+. H :F: H:Cl: HCl:o is better represented as closer to Cl due to its greater electronegativity. Thus, HCl contains a polar covalent bond. H :0: Polar lone pair 8- :S H -S= :0: 2 bond pairs (4 e-) double bond because the bond electrons are pulled F: Pola
ed Lewis struc :: :Z: : Z: |d=8: the proposed Lewis structure reasonable? Yes. No, it has the wrong number of valence electrons. The correct number is: No, it has the right number of valence electrons but doesn't satisfy the octet rule. The symbols of the problem atoms are:* Yes. No, it has the wrong number of valence electrons. The correct number is: No, it has the right number of valence electrons but doesn't satisfy the octet rule. The symbols of the problem atoms are:* Yes. No, it has the wrong number of valence electrons. The correct number is: No, it has the right number of valence electrons but doesn't satisfy the octet rule. The symbols of the problem atoms are:*
iii. Vinyl chloride is the starting material for the production of poly(vinyl chloride), abbreviated PVC. Its recycling code is "V". The major use of PVC is for tubing in residential and commercial construction. H Cl H H Vinyl chloride (a) Complete the Lewis structure for vinyl chloride by showing all unshared pairs of electrons. (b) Predict the H-C-H, H-C-C and Cl-C-H, bond angles in this molecule. (c) Does vinyl chloride have polar bonds? (d) Is it a polar molecule? (e) Does it have a dipole? iv. Diazene (N,H,) and hydrazine (NH,NH,) are reactive nitrogen compounds. Use the hybrid orbitals theory to compare the bonding in these two molecules, and describe the differences in their molecular structures. v. Which molecules in the following figure show an increase in bond order when one electron is added to the molecule? (Hint: Use the molecular orbitals theory.) Liz Bez B3 C2 N2 O2 Nez vi. Use the molecular orbitals theory to decide whether NF would be stabilized or destabilized by…
Decide whether the Lewis structure proposed for each molecule is reasonable or not. molecule proposed Lewis structure CIF 3 PF 4 O CI₂ :: : Cl .. :F: :F: | P :F: .. : 0: F : O о оо Is this a reasonable structure? If not, why not? Yes, it's a reasonable structure. No, the total number of valence electrons is wrong. The correct number is: No, some atoms have the wrong number of electrons around them. The symbols of the problem atoms are: Yes, it's a reasonable structure. No, the total number of valence electrons is wrong. The correct number is: No, some atoms have the wrong number of electrons around them. The symbols of the problem atoms are: Yes, it's a reasonable structure. No, the total number of valence electrons is wrong. The correct number is: No, some atoms have the wrong number of electrons around them. The symbols of the problem atoms are: 0 * 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…

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