draw a resonance structure Draw a second resonance form for the structure shown below.H2C=N=N:• Include all valence lone pairs in your answer.• In cases where there is more than one answer, just draw one.• Should you want to restart the exercise, the drop-down menu labeled == starting points == can be used to redraw the startingmolecule on the sketcher.• In your structure, all second row elements should have a complete octet when possible.opyasteノ/H;C=N=N° Draw a second resonance form for the structure shown below.Include all valence lone pairs in your answer.• In cases where there is more than one answer, just draw one.Should you want to restart the exercise, the drop-down menu labeled == starting points == can be used to redraw the startingmolecule on the sketcher.• In your structure, all second row elements should have a complete octet when possible.opyasteH.

Answered: Image /qna-images/answer/2977e5d6-1c43-43a9-b3b8-d634cd682c5b.jpg

Answered: Draw a second resonance form for the…

Science

Chemistry

Draw a second resonance form for the structure shown below. H2C=N=N:

Chemical Principles in the Laboratory

11th Edition

ISBN:9781305264434

Author:Emil Slowinski, Wayne C. Wolsey, Robert Rossi

Publisher:Emil Slowinski, Wayne C. Wolsey, Robert Rossi

Chapter13: The Geometrical Structure Of Molecules-an Experiment Using Molecular Models

Section: Chapter Questions

Problem 4ASA: a. How many sticks did you need to make the skeleton structure?____________ b. How many sticks are...

See similar textbooks

Similar questions

Propose a correct Lewis structure for the following species H6C2NO1+. All the steps of the procedure that allowed you to obtain the structure should appear. To do this, write what is indicated in each of the boxes. Draw 10 boxes on a sheet and in each of them indicate the following corresponding to its number. 1) Number of external electrons 2) Core atom 3) Initial structure (skeleton or order of atoms) 4) Spent electrons (used or bonding) 5) Missing electrons to put (remaining or surplus) 6) Numbers of electrons to complete octets. Show them in the structure. 7) Number of extra links (multiple links) 8) Proposed structure 9) Formal charges. 10) Final structure.
PLEASE NOTE: This question has been answered, but DID NOT INCLUDE THE “DOTS” for the Lewis-dot structure. I'm needing someone to ADD THE “DOTS” and hand-draw, please. I am completely and totally lost with how to do these!!!! For the following molecules, provide ALL possible resonance structures. Calculate the formal charge for each atom in the molecule. Determine which structure is the major contributing structure for the resonance hybrid. Explain WHY it is preferred over the others. Remember your rules for setting up Lewis-dot structures. a) HCO2- b) SO3 c) Cl2CO d) OCN-
a. How many sticks did you need to make the skeleton structure?____________ b. How many sticks are left over? ____________ If your model is to obey the octet rule, each ball must have four sticks in it except for hydrogen atom balls, which need and can only have one. Each atom in an octet rule species is surrounded by four pairs of electrons. c. How many holes remain to be filled? ____________ Fill them with the remaining sticks, which represent nonbonding electron pairs. Draw the complete Lewis structure for NH2Cl using lines for bonds and pairs of dots for nonbonding electrons.
A complete Lewis structure must show all nonzero formal charges. Complete each of thefollowing Lewis structures by adding any missing formal charges.
a.)Draw a Lewis diagram for IO4- in which the central I atom has a formal charge of zero and show all NONZERO formal charges on all atoms. note overall charge of ion is -1 b.)Draw a Lewis structure for IO4- in which the octet rule is satisfied on all atoms and show all NONZERO formal charges on all atoms. C.Based on formal charge, what is the best Lewis structure for the ion? smallest formal charge or octet rule satisfied for all atoms
Draw a Lewis structure of your choice that has at least three equally reasonable resonance structures. You must show your work as to how the structure was drawn including showing valence electrons, any structures you draw that don’t work and require you to show a multiple bond, and formal charges on each atom that has a formal charge. For example, Nitrate ion has three structures (but you can’t draw this one). All three structures have formal charges and no one structure is preferred based on formal charge. Carbon dioxide would not be a valid choice. While it does have three structures, the structure that has two double bonds is the preferred structure while the structures with triple bonds are not equivalent to the double bonded version as they have multiple formal charges present.
Draw the Lewis structure of BH4- and use your Lewis structure to help fill in the missing numbers. Hint: you must put a number in each box. If the answer is zero, you must enter "0". The Lewis structure has: lone pairs = single bonds = double bonds = triple bonds = atoms with a positive formal charge = atoms with a negative formal charge = Is this structure stabilised by resonance? (Enter either yes or no below - no other words).
1) What do you predict the average bond length and average bond energy values for the F-F bond based on the chart below? WIll it be higher than, lower than, or the same as the other bonds shown in the chart. Justify your answer. Bond Average Bond Length (PM) Average Bond Energy (KJ/MOLE) CL-CL 199 243 Br-Br 228 193 I-I 267 151 2) Explain how a stable covalent bond is formed in terms of attractive and repulsive forces. Note: Please briefly explain, Thank you.
Question 4 options: Draw the Lewis structure of CS2 and use your Lewis structure to help fill in the missing numbers. Hint: you must put a number in each box. If the answer is zero, you must enter "0". The Lewis structure has: lone pairs, single bonds, double bonds, triple bonds, atoms with a positive formal charge, and atoms with a negative formal charge. Is this structure stabilised by resonance? (Enter either yes or no below - no other words).
ClO2F2+(a) Draw all of the possible Lewis structures (including reasonance structures) of the following compounds.(b) Label the formal charge for each atom.(c) Determine which resonance structure(s) is(are) the better/best and briefly explain. Question 5. Finish the questions regarding the molecule/ion in Question 4 above. (a) Draw the best Lewis structure with a three-dimensional fashion by using dash and solid wedges.(b) Name the electron geometry and molecular geometry of the molecules. Identify the bond angles. Note: For the non-standard bond angels, use “<” or “>” to suggest the deviation of the bond angles from the standard bond angel. (c) Determine wether the molecule is molecule is polar or non-polar. Briefly explain.
Draw two valid Lewis structures for POCl. Structure A should have Phosphorus as the central atom (O-P- Cl) and Structure B should have Oxygen as the central atom (P-O-Cl). In both structures, the Cl atom should be singly bonded to the central atom What is the formal charge of EACH atom is Structure A? What is the formal charge of EACH atom is Structure B? On the basis of formal charge, which is the best structure for this compound? Explain why you chose that partcular structure.
Draw the complete Lewis structure for NO2-(the nitrite ion) showing the steps used to get the correct answers (not just the correct answer). Be sure to include formal charges and both resonance structures a. Draw the Lewis Structure and show work