Concept explainers
(a)
Interpretation:
The type of bonding electron domain should be identified for each molecule in given figure.
Concept Introduction:
The bonding electron domain is defined as the shared valence electrons (2, 4, or 6 electrons) which are localized between two core atoms.
This is classified as follows:
Single bond: two electrons or 1 pair;
Double bond: four electrons or 2 pairs;
Triple bond: six electrons or 3 pairs.
The non-bonding electron domain is defined as the pair of valence electrons which are not involved in bonding.
(b)
Interpretation:
The number of electrons present in each bonding electron domain should be reported.
Concept Introduction:
The bonding electron domain is defined as the shared valence electrons (2, 4, or 6 electrons) which are localized between two core atoms.
This is classified as:
Single bond: two electrons or 1 pair;
Double bond: four electrons or 2 pairs;
Triple bond: six electrons or 3 pairs.
The non-bonding electron domain is defined as the pair of valence electrons that are not involved in bonding.
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Organic Chemistry: A Guided Inquiry
- On the left side of Figure 3.6, label the areas shown with a dotted line where... one bond can form. one bond can form.arrow_forwardII. Problem solving. 1. Choose from each pair the one that will exhibit the given property to the greater extent a. bond polarity N-H b. net number of lone pairs NH3 c. bond length CI-F d. formal charge on N e. net number of lone pairs f. bond strength g. bond polarity h. bond length electronegativity i. j. formal charge on O NH4+ NH₂™ C-O H-CI N-N O H₂O 2. Draw the Lewis structures of the following then evaluate the formal charge a. PBr3 b. CH3OH B-F CH4 F-F NH3 NH₁+ C-N H-F N = N CI H3O+ C. NO₂¹¹arrow_forwardCheck the box next to each molecule on the right that has the shape of the model molecule on the left: molecules model (check all that apply) olo O C,H, О НОСІ You can drag the slider to rotate the model molecule. O CO, O N,H, O None of the above Note for advanced students: the length of bonds and size of atoms in the model is not necessarily realistic. The model is only meant to show you the general geometry and 3D shape of the molecule.arrow_forward
- Check the box next to each molecule on the right that has the shape of the model molecule on the left: molecules model (check all that apply) O HNO O H,0 O H,S O HOCI You can drag the slide None of the above Note for advanced students: the length of bonds and size of atoms in the model is not necessarily realistic. The model is only geometry and 3D shape of the molecule.arrow_forward7. Predict the polarity of 6 real molecules. First, draw the molecules and any bond dipoles. Then draw any molecular dipoles. Explain your reasoning before you check your predictions with the simulation.arrow_forwardCheck the box next to each molecule on the right that has the shape of the model molecule on the left: molecules model (check all that apply) O CH,Cl, O CH,CI O CF4 You can drag the O BrF4 O None of the above Note for advanced students: the length of bonds and size of atoms in the model is not necessarily realistic. The model geometry and 3D shape of the molecule. toarrow_forward
- Give typed full explanation Look at figure 3-22 that shows the electron density that occurs abound the Si-O bond. This electron density map gives the "shape" of the O and Si atoms when they are bonded together. Think about the answer in Q9 and choose the best response below: (Select answer choice) a. This figure shows that the Si and O atoms, when they bond together, do not form spheres, which is due to the fact that the Si-O bond is strongly covalent and these shared electrons affect atomic shape. This change in shape limits the applicability of Pauling's Coordination principle since that principle is based on the geometry of perfect spheres. b. This figure shows that the Si and O atoms, when they bond together are close to perfect spheres, which is due to the fact that the Si-O bond is strongly covalent. This figure shows that Pauling's Coordination principle should apply very precisely to any substance that contains Si-O bonds c. This figure shows that the Si and O atoms, form in a…arrow_forwarda) Draw the Lewis structure for the molecule on the left (labeled as Molecule A above). Draw the Lewis structure which has minimum formal charges. b) Draw the correct Lewis structure for the molecule on the right (labeled as Molecule B above). Draw the Lewis structure which has minimum formal charges. c) Select the three TRUE statements from those provided below. The molecule on the right (Molecule B) is planar (all atoms lie within the same plane). The molecule on the left (Molecule A) is planar (all atoms lie within the same plane). The molecule on the right (Molecule B) has polar bonds. The molecule on the left (Molecule A) has polar bonds. We can distinguish between the two molecules (Molecule A and Molecule B) based upon their dipole moment.arrow_forwardVC 2.12... VC Gra... VC Test... 8) Formula SiF4 G - Gr... VC Topi... Bond Polarity (AEN) Total Electrons Valence Loc... science.valenciacollege.edu a Your... V http... Rough Lewis Structure VC *We... (Include formal charges other than 0.) Molecule Polarity PHET Mol... VC Lab... V https://s... Molecular Geometry/ Electron-Group Geometry Molecular Geometry: Electron-Group Geo.: More soluble in hexane or water? b Ho... 6 Tough Low Structure Bond Polarity (EN) + SOCI... More beinarrow_forward
- 1. Molecule: CF4 indicate the number of available electrons that electrons ae = are in the molecule. in the space to the right connect all of the atoms to the central atom and then make each atom follow the octet rule Trial Structure: (duet rule for hydrogen). How many electrons are necessary in the trial ne = structure? 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:arrow_forwardWhat is delocalization energy? How is it related to resonance energy? Answer by selecting all true statements. 00 Resonance energy is a term used in VB theory. Resonance energy and delocalization energy are term that describe different conditions. Resonance energy is a term used in MO theory. Resonance energy and delocalization energy are essentially the same thing. Resonance energy and delocalization energy represent the additional stability associated with a spreading out of electron density. Delocalization energy is a term used in VB theory. Delocalization energy is a term used in MO theory. Resonance energy and delocalization energy represent the additional stability associated with concentrating electron density.arrow_forwardCheck the box next to each molecule on the right that has the shape of the model molecule on the left: molecules model (check all that apply) ? alo to O BrF O NH, You can drag the slider to rotate the model molecule. O CH,O O CF4 O None of the above Note for advanced students: the length of bonds and size of atoms in the model is not necessarily realistic. The model is only meant to show you the general geometry and 3D shape of the molecule.arrow_forward
- Organic Chemistry: A Guided InquiryChemistryISBN:9780618974122Author:Andrei StraumanisPublisher:Cengage Learning