-2 9. CO32 Total # of Valence Electrons: Lewis Structure (show all resonance structures if applicable) Ö: (-1) :O: Ö: (-1) Ô=c–o (-1) O—C = 0 <-> (-1) <-> Any polar bonds in the molecule? Yes No 10. CS₂ Total # of Valence Electrons: Lewis Structure (show all resonance structures if applicable) Any polar bonds in the molecule? Yes No 3-D Model Sketch Molecular Shape: Molecular Polarity: 3-D Model Sketch Molecular Shape: Molecular Polarity: Polar Polar Bond Angles Non-Polar Bond Angles Non-Polar

-2 9. CO32 Total # of Valence Electrons: Lewis Structure (show all resonance structures if applicable) Ö: (-1) :O: Ö: (-1) Ô=c–o (-1) O—C = 0 <-> (-1) <-> Any polar bonds in the molecule? Yes No 10. CS₂ Total # of Valence Electrons: Lewis Structure (show all resonance structures if applicable) Any polar bonds in the molecule? Yes No 3-D Model Sketch Molecular Shape: Molecular Polarity: 3-D Model Sketch Molecular Shape: Molecular Polarity: Polar Polar Bond Angles Non-Polar Bond Angles Non-Polar

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter3: Atomic Shells And Classical Models Of Chemical Bonding

Section: Chapter Questions

Problem 37P: The percent ionic character of a bond can be approximated by the formula 16+3.52 , where is the...

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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?
A stable triatomic molecule can be formed that contains one atom each of nitrogen, sulfur, and fluorine. Three bonding structures are possible, depending on which is the central atom: NSF, SNF, and SFN. (a) Write a Lewis diagram for each of these molecules, indicating the formal charge on each atom. (b) Often, the structure with the least separation of formal charge is the most stable. Is this statement consistent with the observed structure for this molecule—namely, NSF, which has a central sulfur atom? (c) Does consideration of the electronegativities of N, S, and F from Figure 3.18 help rationalize this observed structure? Explain.
The percent ionic character of a bond can be approximated by the formula 16+3.52 , where is the magnitude of the difference in the electronegativities of the atoms (see Fig. 3.18). Calculate the percent ionic character of HF, HCl, HBr, HI, and CsF, and compare the results with those in Table 3.7.
The partial Lewis structure that follows is for a hydrocarbonmolecule. In the full Lewis structure, each carbon atomsatisfies the octet rule, and there are no unshared electronpairs in the molecule. The carbon—carbon bondsare labeled 1, 2, and 3. (a) How many hydrogen atomsare in the molecule? (b) Rank the carbon–carbonbonds in order of increasing bond length. (c) Whichcarbon—carbon bond is the strongest one?
A classmate of yours is convinced that he knows everythingabout electronegativity. (a) In the case of atoms X and Y havingdifferent electronegativities, he says, the diatomic moleculeX¬Y must be polar. Is your classmate correct? (b) Yourclassmate says that the farther the two atoms are apart in abond, the larger the dipole moment will be. Is your classmatecorrect?
A. What is the electron-pair geometry for I in IF4-? ________There are _______ lone pair(s) around the central atom, so the geometry of IF4- is __________.B. What is the electron-pair geometry for As in AsF6-? ________There are _______ lone pair(s) around the central atom, so the geometry of AsF6- is _________.
Despite the larger electronegativity difference between the bond atoms, BeCl2(a) has no dipole moment whereas SCl2(g) does possess one. Account for this difference in polarity. The answer should labelling of: Lewis structure, AXE notation, molecular and electron geometry, partial charge, dipole moment, and explanation.
Use Lewis symbols and Lewis structures to diagram the formationof PF3 from P and F atoms, showing valence-shellelectrons. (a) How many valence electrons does P have initially?(b) How many valence electrons does each F haveinitially? (c) How many valence electrons surround the P inthe PF3 molecule? (d) How many valence electrons surroundeach F in the PF3 molecule? (e) How many bonding pairs ofelectrons are in the PF3 molecule?
TRUE OR FALSEa. It requires more energy to break N-N bond (N2O4) than to break the N-N bond in N2 b. The ∆Srxn for C6H14(l) is +ve, while the ∆Srxn for C4H10(g) is -ve.
ClO- ,does it have linear (180o bond angle) or tetrahedral (o ?) VSEPR shape.
Draw the Lewis structures for the following species: (a)CN-; (b) [N3]-; (c) [SCN]- For (b) and (c), there are more than one canonical structure that satisfy the Octet rule, and resonance is likely applied. Which canonical structures do you think would be the major contributor to the overall structure (i.e., resonance hybrid)?
Between, CH3(CH2)nH2COLi, CH3(CH2)nH2CO2H, CH3(CHBr)nCH3, CH3(CH2)nCH3, CH3(CH2)nC=O which is has the highest melting point, most volatile, most soluble in water, most densest if the have thesame amount of mythelene. and finally rank the compounds from least to most polar.