Group the following molecular formulas under their respective geometries. Use the Real Molecules mode to verify the correct geometry for select structures. Drag the appropriate items to their respective bins. > View Available Hint(s) Reset Help BeCl2 SF. CO2 CH4 PCl, HCN BF3 PF, CH20 NH4+ Linear Trigonal planar Tetrahedral Trigonal bipyramidal Octahedral

Group the following molecular formulas under their respective geometries. Use the Real Molecules mode to verify the correct geometry for select structures. Drag the appropriate items to their respective bins. > View Available Hint(s) Reset Help BeCl2 SF. CO2 CH4 PCl, HCN BF3 PF, CH20 NH4+ Linear Trigonal planar Tetrahedral Trigonal bipyramidal Octahedral

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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The compound shown below can be depicted by two different Lewis structures. The rules for valence electron octets apply for all atoms except hydrogen. a) Draw these two Lewis structures (be sure to show all bonding and non- bonding electrons as well as any formal charges). b) Explain what relationship is between these two structures. c) Explain which of these structures is most important. d) For your most important structure, predict bond angles and atom hybridization. H2C*CHO
Draw the Lewis structure of SF showing all lone pairs. Select Draw Templates More Ć sp² S F What is the hybridization of the central atom? sp sp³ sp³ d² n³ d Erase Q2 Q Identify the molecular geometry of SF 4* O trigonal planar square planar octahedral O trigonal pyramidal see-saw tetrahedral linear O T-shaped O trigonal bipyramidal square pyramidal bent What are the ideal bond angles of this geometry? 109.5° 120° 180° 90°
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Formula Total valence e- (show calc) CF4 NHBr₂ (Nis central) POCI3 CSe₂ Structure Total electron groups Geometry (Shape) Angle Polar? Y/ N if yes state why
Consider BF3, SO3, and XeO3. Which of these molecules is considered to be polar? > View Available Hint(s) O S03 O BF3 O XeO3 O All of these Submit Provide Feedback
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1. Briefly explain in your own words why the bond angle increases as the number of electron groups decrease? 2. How does electron domain geometry differ from molecular geometry? Briefly explain in your own words. 3. Write a complete list of steps you will utilize to predict the electron-domain geometry for a given species using only the Lewis structure. The only information you are provided with is the molecular formula and the net charge.
Mark the following statements as true or false. A molecule with very polar bonds can be nonpolar. blank The electrons in a polar bond are found nearer to the more electronegative element. blank Fluorine is very polarizable. blank Covalent bonds are partially ionic because of polarizability of atoms. blank Kr and Sr2- are isoelectronic.
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