5. NO₂ Total # of Valence Electrons: Lewis Structure (show all resonance structures if applicable) 3-D Model Sketch Any polar bonds in the molecule? Yes No Molecular Shape: Molecular Polarity: Any polar bonds in the molecule? Yes No +1 6. H30¹¹ - use a yellow ball for oxygen (not red) when constructing this model Total # of Valence Electrons: 3-D Model Sketch Lewis Structure (show all resonance structures if applicable) Molecular Shape: Molecular Polarity: Polar Polar Bond Angles Non-Polar Bond Angles Non-Polar

5. NO₂ Total # of Valence Electrons: Lewis Structure (show all resonance structures if applicable) 3-D Model Sketch Any polar bonds in the molecule? Yes No Molecular Shape: Molecular Polarity: Any polar bonds in the molecule? Yes No +1 6. H30¹¹ - use a yellow ball for oxygen (not red) when constructing this model Total # of Valence Electrons: 3-D Model Sketch Lewis Structure (show all resonance structures if applicable) Molecular Shape: Molecular Polarity: Polar Polar Bond Angles Non-Polar Bond Angles Non-Polar

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 5.88EP: Successive substitution of F atoms for H atoms in the molecule NH3 produces the molecules NH2F,...

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Similar questions

The valence shell of an atom in a legitimate Lewis structure (see Figure 2.3) has what in commonwith the valence shell of a noble gas? (Noble gases are stable elements found in the last column ofthe periodic table, e.g., He, Ne, Ar, etc.)
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.
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.
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.
Acrylonitrile is the building block of the synthetic fiber Orlon. Acrylonitrile Which carbon-carbon bond is shorter? Which carbon-carbon bond is stronger? Which bond is the most polar? What is the partial negative end of that bond?
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?
complete #13 & #14, use #15 as an example!
Examples: Example: H▬N▬H HIN: Examples: :F Н lone pair : -bond pair (2 e-) single bond :F: Non-Polar 8+. H :F: H:Cl: HCl:o is better represented as closer to Cl due to its greater electronegativity. Thus, HCl contains a polar covalent bond. H :0: Polar lone pair 8- :S H -S= :0: 2 bond pairs (4 e-) double bond because the bond electrons are pulled F: Pola
3. Sil – use a black ball for silicon when constructing this model Total # of Valence Electrons: 3-D Model Sketch Lewis Structure (show all resonance structures if applicable) Any polar bonds in the molecule? Yes No 4. HCN Total # of Valence Electrons: Lewis Structure (show all resonance structures if applicable) Any polar bonds in the molecule? Yes No Molecular Shape: Molecular Polarity: 3-D Model Sketch Molecular Shape: Molecular Polarity: Polar Polar Bond Angles Non-Polar Bond Angles Non-Polar
5. Molecule: XeFs* indicate the number of available electrons that are ae = in the molecule. Trial Structure: in the space to the right connect all of the atoms to the central atom and then make each atom follow the octet rule (duet rule for hydrogen). How many electrons are necessary in the trial structure? ne = Circle the correct ne = ae ne ae relationship between ne and ae. Draw the corrected Lewis Structure to the right. Add Later: e- geometry: molecular geom: Hybridization:
In the BEST Lewis structure for the molecule XeF2, how many unshared pairs are there on the central atom? Enter a number.
= Deciding whether a Lewis structure satisfies the octet rule Decide whether these proposed Lewis structures are reasonable. proposed Lewis structure :5: I :Z: H- :0: | U: -C-C-H Is the proposed Lewis structure reasonable? Yes. No, it has the wrong number of valence electrons. The correct number is: 0 No, it has the right number of valence electrons but doesn't satisfy the octet rule. The symbols of the problem atoms are:* 0 Yes. No, it has the wrong number of valence electrons. The correct number is: 0 No, it has the right number of valence electrons but doesn't satisfy the octet rule. The symbols of the problem atoms are:* Yes. No, it has the wrong number of valence electrons. The correct number is: No, it has the right number of valence electrons but doesn't satisfy the octet rule. The symbols of the problem atoms are:* * If two or more atoms of the same element don't satisfy the octet rule, just enter the chemical symbol as many 1/5