Draw Lewis structures and assign formal charges for the following compounds and ions. Note any resonance forms and explain which resonance form is the most important. Make a note of any other unusual features (such as "this one doesn't work" and why- what are the shortcomings of the model.) CO3²- CO NO₂ CNO (include isomers) Al₂Cl6 B₂H6 O2 (paramagnetic) H3O+ LiF IF7

Draw Lewis structures and assign formal charges for the following compounds and ions. Note any resonance forms and explain which resonance form is the most important. Make a note of any other unusual features (such as "this one doesn't work" and why- what are the shortcomings of the model.) CO3²- CO NO₂ CNO (include isomers) Al₂Cl6 B₂H6 O2 (paramagnetic) H3O+ LiF IF7

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 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.
Draw the correc (best) Lewis structure (LS) for the ionic compound K2SeO3 (on looose leaf paper--NOT TO BE SUBMITTED) and then answer the following questions.(NOTE: Use the cardinal numbers 0, 1, 2, 3, and so on for any quantity required)a) What charge does the K ion have in this compound? (give size & sign of charge: e.g., 1+, 2-, etc.) b) What charge does the SeO3 ion have in this compound? (give size & sign of charge: e.g., 1+, 2-, etc.) c) How many lines, if any, attach each K ion to the SeO3 ion? d) How many valence electrons does the SeO3 ion (alone) have? e) How many single bonds does the LS of the SeO3 ion have? f) What is the number of lone electron pairs in the LS of the SeO3 ion?
5. There are three possible ways to linearly connect the atoms for an anion whose chemical formula is [CNO]. They are [CNO], [NOC], and [NCO]. Draw a Lewis structure (showing all bonds, lone pairs, and formal charges) for each of the three possible ions. Which is the most stable arrangement? (Hint: the most stable structure will be the one with the most octets, fewest and lowest formal charges, etc., as we discussed in class.)
a. Write a Lewis structure that obeys the octet rule for the following species. Assign the formal charge for the central atom of XeO4. If multiple resonance structures exist, use one that does not involve an expanded valence. Formal charge: b. Write a Lewis structure that obeys the octet rule for the following species. Assign the formal charge for the central atom of clO3¯. If multiple resonance structures exist, use one that does not involve an expanded valence. Formal charge:
a. Write a Lewis structure that obeys the octet rule for the following species. Assign the formal charge for the central atom of Cl04~. If multiple resonance structures exist, use one that does not involve an expanded valence. Formal charge: b. Write a Lewis structure that obeys the octet rule for the following species. Assign the formal charge for the central atom of ClO3-. If multiple resonance structures exist, use one that does not involve an expanded valence. Formal charge:
One of the Lewis structures that can be drawn for the N₂O molecule is: :N=N-O: What are the formal charges on the N (end), N (center), and O atoms in this structure? 0, -1, +1 0, +1, -1 O 0, 0, 0 +1, +1, -2 +1, 0, -1
The value of Ka1 of hypophosphorous acid, H3PO2, is nearly the same as the Ka1 of phosphoric acid, H3PO4. Draw a Lewis structure for phosphoric acid that is consistent with this behavior. Draw the Lewis structure with the formal charges minimized. Do not include formal charges in your structure. Include hydrogen atoms and nonbonding electrons in the structure.
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 thiocyanate ion , SCN" . 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. :S- C=N: S =C=N :S= C-N: А В Formal Charge C N 2. The structure that contributes most significantly to the overall electronic structure of SCN¯ is
For each of the following, draw resonance structures, assign formal charges to the atoms in each structure, and determine relative contributions of each structure to the overall electronic structure. a) CIO2 b) CI3PO
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 Use the References to access important values if needed for this question. 02 03 S KNENEN :0: B A I 2- 2. The best Lewis structure for SO3²- is A :0: C Previous Next
Draw Lewis structure(s) for the acetate ion (CH2CO0). If there are equivalent resonance structures, draw all of them. • Draw one structure per sketcher box, and separate added sketcher boxes with the 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. symbol. CH3COO":