Draw Lewis structures and assign formal charges for the following compounds and ions. Note anyresonance forms and explain which resonance form is the most important. Make a note of any otherunusual features (such as "this one doesn't work" and why-what are the shortcomings of the model.)2-CO3²-B₂H6COO₂ (paramagnetic)H₂O*LiFIF,NO₂CNO (include isomers)Al₂Cl6

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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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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.
Using average bond enthalpies (linked above), estimate the enthalpy change for the following reaction: CH4(g) + Cl₂(g)-CH3CI(g) + HCl(g) kj
Column I: Draw the best Lewis structure. Label any atoms with nonzero formal charge. Column II: List the total number of major resonance contributors and draw at least two (if they exist). Column III: How many electron groups are around the central atom? Column IV: What is the electron geometry? Column V: What is the molecular geometry? Possible answers: linear, trigonal planar, tetrahedral, trigonal bipyramidal, octahedral, bent, trigonal pyramidal, see-saw, T-shaped, square pyramidal, square planar). Column VI: Give values of the bond angles around the central atom. (for example, 109.5°, less than 109.5°, 120°, less than 120°, etc.). Column VII: Give the hybridization of the central atom. Column VIII: State how many sigma bonds and pi bonds are present in the molecule or ion. Column IX: Is the molecule polar or non-polar?
Based on the bond energies for the reaction below, what is the enthalpy of the reaction? HC≡CH (g) + 5/2 O₂ (g) → 2 CO₂ (g) + H₂O (g)
One of the Lewis structures that can be drawn for the N₂O molecule is: What are the formal charges on the N (end), N (center), and O atoms in this structure? 0, 0, 0 -1, 0, +1 +1, 0, -1 -1, +1, 0 +1, -1, 0
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The azide ion, N3, is a symmetrical ion, all of whose contributing structures have formal charges. Draw three important contributing Lewis structures for this ion. Draw the molecule by placing atoms on the grid and connecting them with bonds. Include all nonbonding electrons. Show the formal charges of all atoms in the correct structure. Q Q Q ? ⒸNNNITY [] + F g i с H N S P Br CI | X Press [TAB] to move to the next option. Press (ALT+A) to get to the bonds and More
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

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