1. H₂S Total # of Valence Electrons: 8 Lewis Structure (show all resonance structures if applicable) Any polar bonds in the molecule? Yes No 2. COCI₂ Total # of Valence Electrons: 24 Lewis Structure (show all resonance structures if applicable) Any polar bonds in the molecule? Yes No 3-D Model Sketch Molecular Shape: Bent Molecular Polarity: 3-D Model Sketch Polar Molecular Shape: Trigonal Planar Molecular Polarity: Polar Bond Angles Non-Polar 109.5° Bond Angles Non-Polar 120°

1. H₂S Total # of Valence Electrons: 8 Lewis Structure (show all resonance structures if applicable) Any polar bonds in the molecule? Yes No 2. COCI₂ Total # of Valence Electrons: 24 Lewis Structure (show all resonance structures if applicable) Any polar bonds in the molecule? Yes No 3-D Model Sketch Molecular Shape: Bent Molecular Polarity: 3-D Model Sketch Polar Molecular Shape: Trigonal Planar Molecular Polarity: Polar Bond Angles Non-Polar 109.5° Bond Angles Non-Polar 120°

Living by Chemistry

2nd Edition

ISBN:9781464142314

Author:Angelica M. Stacy

Publisher:Angelica M. Stacy

ChapterU2: Smells: Molecular Structure And Properties

Section: Chapter Questions

Problem 8STP

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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?
Aspartame is an artificial sweetener marketed under the name Nutra-Sweet. A partial Lewis structure for aspartame is shown below. Aspartame can be classified as an organic compound (a compound based on carbon atoms). The majority of Lewis structures for simple organic compounds have all atoms with a formal charge of zero. Therefore, add lone pairs and multiple bonds to the structure above to give each atom a formal charge of zero when drawing the Lewis structure. Also note that the six-sided ring is shorthand notation for a benzene ring (C6H5). Benzene is discussed in Section 4-7. Complete the Lewis structure for aspartame. How many C and N atoms exhibit sp1 hybridization? How many C and O atoms exhibit sp3 hybridization? How many and bonds are in aspartame?
Nhy is resonance structure A and resonance structure B not the same structure? If you rotate the molecule like a spicket handle (l. e. clockwise with the C at the center and the R group remaining in place as you look down the C - R bond) wouldn't you get the same thing? Why are these not equivalent structures? Resonance structure A t Resonance structure B Actual structure
1. NH2Cl a. In NH2Cl there is a total of ____________ valence electrons. b. The NH2Cl model consists of how many lone pairs of electrons c. How many bonds are in the NH2Cl molecule? d . What is the shape the atoms make (excluding lone pairs) in NH2Cl?
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Draw the best Lewis Structure for NCOF based on overall formal charges. The skeleton framework for NCOF is: N—C—O—F. Answer the questions below based on your final structure. How many bonding (shared) electron pairs are on the nitrogen atom? _________ How many (total) non-bonding electron pairs are in the whole molecule? ______ How many non-bonding electron pairs are on the oxygen atom? _______
central atom underlined: NH3O ICl3 XeO3 C4H4 O.R.-Lewis structure: Remember to always: • Show charge, if present. • Draw at least one more equivalent resonance structure (with «) if present, to describe delocalized covalent bonding. count all lone pairs in LS: polar: Y/N?
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Place the following in order of decreasing X-AX bond angle, where A represents the central atom and X represents the outer atoms in each molecule: CS2, CF4, SCl2. I initially thought that SCl would have a greater bond angle than CF4. Is this not the case because the bond angle of SCl2 is approximately 109.5, while CF4 is exactly 109.5 degress?
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Using BEST Lewis structures and the VSEPR model, match each molecular formula with the molecular geometry that describes it.