most etakONE (1) of the following, then (a) draw two possible resonance hybrids, and (b) circle thestable hybrid.1.IL.III.C.HCHOC,H,O

Resonance structures: structure which have least separation of charges is the best contributing…

Answered: most t ONE () of the following, then…

Living By Chemistry: First Edition Textbook

1st Edition

ISBN:9781559539418

Author:Angelica Stacy

Publisher:Angelica Stacy

ChapterU2: Smells: Molecular Structure And Properties

SectionU2.4: Connect The Dots: Lewis Dot Symbols

Problem 6E

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What happens to the bond angle (column 4) as the # of lone pairs (column 2) increases? Based on your answer above, do lone pairs or bonds take up more space?
Consider the following flat drawing of methane (CH4) . a. What is HCH bond angle implied by this drawing if you assume it is flat? b. Are the electron domains of this flat CH4 spread out as much as possible? c. Use model materials to make a model of CH4 (methane). If you assembled it correctly, thefour bonds (bonding electron domains) of your model will be 109.5° apart. d. In which representation, the drawing above or the model in your hand (circle one) are theH’s of CH4 more spread out around the central carbon? e. Confirm that your model looks like the following drawing. The wedgebond represents a bond coming out of the page, and the dash bondrepresents a bond going into the page f. You will often see methane drawn as if it were flat (like on the previous page). Why is thismisleading, and what is left to the viewer’s imagination when looking at such a drawing?
Consider the incomplete orbital representation of O2 , below right. a. Identify which lobes are hybrid orbitals (identify the type) and which lobes arep orbitals. b. Use dotted lines to show any bonds. c. Use up or down arrows to show electron occupation of each hybrid orbital or bond.
On the left side of Figure 3.6, label the areas shown with a dotted line where... one bond can form. one bond can form.
A student draws the picture of ammonia (NH3) in the box below, left, and predicts it will be a flatmolecule with HNH bond angles of exactly 120°. Unfortunately, the student left something out. a. What did the student omit from his drawing? b. What is the actual HNH bond angle of ammonia (based on the draw g above, right)? c. Explain why water, ammonia, and methane (shown below) all have about the same bondangles (close to 109.5°) even though they have different numbers of bonds.
Draw the lewis structure of SO2 ( best resonance) and 2nd best resonance showing the shape and bond angles of each one, the 3D structure with polar bonds or bonds dipole of each one and the molecular polarity. Here is an example of what I want the answer to be like:
which one of the figures below has every sp3 hybridized atom circled?
draw all possible lewis/resonance sturcures for CBr2O and circle/explain the best one
Draw a second resonance structure for carbocation A, as well as the hybridof both resonance structures. Then use Rules [1]–[3] to rank the relativestability of both resonance structures and the hybrid
Explain below ? The resonance hybrid is more stable than any resonance structurebecause it delocalizes electron density over a larger volume.
- What orbital(s) are the lone pairs of electrons on the O atom placed? - What orbital is the lone pair of electrons on the N atom placed? - What type of bond(s) are formed between Ca1 – C? - What type of bond(s) are formed between C = O? - What type of bond(s) are formed between C – N? - What type of bond(s) are formed between N – Ca2? - What type of bond(s) are formed between N – H? - What is the angle between Ca1 – C = O? - What is the angle between Ca1 – C – N? - What is the angle between O = C – N? - What is the angle between C – N – Ca2?
Can someone help me this this? The question is: Determine the orbital in which the indicated non-bonding electrons reside. Candidates include atomic orbitals (s and p), hybrid orbitals (sp, sp2, and sp3), and molecular orbitals (s, s*, p, p*). Here is the picture for it

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most t ONE () of the following, then (a) draw twn possible resonance hybrids, and (b) circle the stable hybrid. 1. CH CHO C,H,O IL II.