Concept explainers
Interpretation:
The bond-line representation of the given molecule should be drawn in the box by considering only valence electrons.
Concept Introduction:
The distribution of electrons in atom into orbitals is said to be electronic configuration. The electronic configuration for every element present in the periodic table is unique or different.
The representation in which the bonds present between atoms are represented by lines is known as bond line representation.
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Organic Chemistry: A Guided Inquiry
- Consider the Lewis structure shown for thionitromethane. Draw the major resonance structure for the compound shown; include lone pairs of electrons, formal charges, and condensed hydrogen atoms (located in the More menu). Then draw curved arrows to show how this can be converted to the Lewis structure given.arrow_forwardThe resonance form that results from the curved arrows drawn in the figure isarrow_forwardConsider this Lewis structure in the curved arrows joke. Draw the resident structure obtained by moving electrons as indicated by the curved arrows.arrow_forward
- Focus on the C atom on the left as the central atom. How many other atoms are directly bonded to this C atom? How many bonding domains are there on the C atom on the left? How many lone pairs of electrons are there on the C atom on the left? How many nonbonding domains are there on the C atom on the left?arrow_forwardIV. Write the resonance structure that would result from moving the electrons in the way indicated by the curved arrows. Submit your answer as assignment. H2Narrow_forwardDraw the simplest set of curved arrows that shows how the structure on the left could be turned into the structure on the right. Show all lone pairs. If you need to expand part of the structure to show some lone pairs, expand it by drawing in all atoms and bond lines. CT 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_forwardIndicate if the bond is polar or nonpolar (in box). If non-polar write non-polar, If polar, show direction of dipole.arrow_forwardButane is an unbranched alkane with the molecular formula C4H10C4H10. a) Draw the complete structure of butane. (Show all hydrogen atoms.) b) Draw the structure of butane in line-bond or skeleton mode. (Do not show the hydrogen atoms.)arrow_forward
- Follow the curved arrows and draw a Lewis structure for the resulting resonance contributor of 1,3-butadiene, adding charges and lone electron pairs to the appropriate atoms. CH2arrow_forwarda) Draw the formal charges to the molecule below. Label atleast two functional groups found in this molecule. Identify and circle the π bonds. b) Draw a curly arrow notation to show how the electrons are redistributed to show a new resonance structure in which the formal charge has moved to a different heteroatom.arrow_forwardBased on the 3D structure, does the bond-line drawing match the given 3D representation? And if not draw the correct bond line structure based on the 3D representation.arrow_forward
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