Question 3: (12 marks)Complete the following chart by drawing the Lewis Diagram (1 mark each), the 3D VSEPR Shape (1 markeach) and providing information regarding the shape, angle(s) and molecular polarity (0.5 marks each).Species Lewis Structure3D VSEPR SketchShape InformationCH4Electronic shape:Molecular shape:Bond Angle(s):Polar/Non-Polar?:Electronic shape:_CO₂Molecular shape:Bond Angle(s):Polar/Non-Polar?:Electronic shape:Molecular shape:_ICIABond Angle(s):Polar/Non-Polar?:_Page 5 of 8

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Answered: Question 3: (12 marks) Complete the…

General, Organic, and Biological Chemistry

7th Edition

ISBN:9781285853918

Author:H. Stephen Stoker

Publisher:H. Stephen Stoker

Chapter5: Chemical Bonding: The Covalent Bond Model

Section: Chapter Questions

Problem 5.63EP

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Similar questions

For each of the following molecular models, write an appropriate Lewis formula.
Given the bonds C N, C H, C Br, and S O, (a) which atom in each is the more electronegative? (b) which of these bonds is the most polar?
3-106 Consider the structure of Penicillin G shown below, an antibiotic used to treat bacterial infections caused by gram-positive organisms, derived from Penicillium fungi: (a) Identify the various types of geometries present in each central atom using VSEPR theory. (b) Determine the various relative bond angles associated with each central atom using VSEPR theory (c) Which is the most poiar bond in Penicillin G? (d) Would you predict Penicillin G to be polar or nonpolar?
Use the Molecule Shape simulator (http://openstaxcollege.org/I/6MolecShape) to build a molecule. Starting with the central atom, click on the double bond to add one double bond. Then add one single bond and one lone pair. Rotate the molecule to observe the complete geometry. Name the electron group geometry and molecular structure and predict the bond angle. Then click the check boxes at the bottom and right of the simulator to check your answers.
7.30 The bond in HF is said to be polar, with the hydrogen carrying a partial positive charge. For this to be true, the hydrogen atom must have less than one electron around it. Yet the Lewis dot structure of HF attributes two electrons to hydrogen. Draw a picture of the electron density distribution for HF and use it to describe how the hydrogen atom can carry a partial positive charge. How can these two models of the HF bond (the electron density and the Lewis structure) seem so different and yet describe the same thing?
hat does it mean to say that a bond is polar? Give two examples of molecules with polar bonds. Indicate in your examples the direction of the polarity.
Fill in the blanks in each line of the following table that involves characteristics of various bonds between nonmetals. The first line is already completed as an example.
The connectivity of HNO could be either HNO or HON. Draw a Lewis structure for each and predict which connectivity is the more favorable arrangement.
Successive substitution of F atoms for H atoms in the molecule NH3 produces the molecules NH2F, NHF2, and NF3. a. Draw Lewis structures for each of the four molecules. b. Using VSEPR theory, predict the geometry of each of the four molecules. c. Specify the polarity (polar or nonpolar) for each of the four molecules.
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.
3-105 Consider the structure of Vitamin E shown below, which is found most abundantly in wheat germ oil, sunflower, and safflower oils: (a) Identify the various types of geometries present in each central atom using VSEPR theory. (b) Determine the various relative bond angles as sociated with each central atom using VSEPR theory. (c) Which is the most polar bond in Vitamin E? (d) Would you predict Vitamin E to be polar or nonpolar?
Successive substitution of F atoms for H atoms in the molecule CH4 produces the molecules CH3F, CH2F2, CHF3, and CF4. a. Draw Lewis structures for each of the five molecules. b. Using VSEPR theory, predict the geometry of each of the five molecules. c. Specify the polarity (polar or nonpolar) for each of the five molecules.

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