Concept explainers
(a)
Interpretation:
The number of electron groups that surround the triple bonded C in Figure 2-1a is to be determined.
Concept introduction:
A group of electrons around an atom is a lone pair or a bond with another atom. The bond, whether a
(b)
Interpretation:
The number of electron groups that surround the central C in Figure 2-1b is to be determined.
Concept introduction:
A group of electrons around an atom is a lone pair or a bond with another atom. The bond, whether a
(c)
Interpretation:
The number of electron groups that surround each C in Figure 2-1c is to be determined.
Concept introduction:
A group of electrons around an atom is a lone pair or a bond with another atom. The bond, whether a
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Organic Chemistry: Principles and Mechanisms (Second Edition)
- d) Rank by number of localized electron pairs. Use a "1" for the highest number, followed by a "2", then a "3" for the lowest number. HN N'arrow_forwardIn the following Lewis structure of [(CH3)2OH]+, every atom, bond and lone pair is positioned. To complete the structure, drag the formal charge tags to the appropriate atom(s). Each marker may be used more than once, or not at all. If an atom has a formal charge of zero, do not drag a tag to it. When you drag the marker in, place the little crosshairs in the upper left corner of the marker directly over the atom(s) in question (not above them). H H-C-O-C-H HHH - H I Η Η Η 0 0 + 2+ 2-arrow_forwardDiazomethane has the formula H2CN2. Draw all valid resonance contributors for diazomethane and, using Table 1-3, propose which one contributes more to the resonance hybrid. Hint: There are no structures that avoid charged atoms.arrow_forward
- In the following Lewis structure of [(CH3)2OH]*, every atom, bond and lone pair is positioned. To complete the structure, drag the formal charge tags to the appropriate atom(s). Each marker may be used more than once, or not at all. If an atom has a formal charge of zero, do not drag a tag to it. When you drag the marker in, place the little crosshairs in the upper left corner of the marker directly over the atom(s) in question (not above them). H. H-C Н-С-О-С-Н C-H H HH 2- II 2-arrow_forwardGive 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_forwardIn the following Lewis structure of [BrO3]", every atom, bond and lone pair is positioned. To complete the structure, drag the formal charge tags to the appropriate atom(s). Each marker may be used more than once, or not at all. If an atom has a formal charge of zero, do not drag a tag to it. When you drag the marker in, place the little crosshairs in the upper left corner of the marker directly over the atom(s) in question (not above them). Ö: Br: 2+ 2-arrow_forward
- Which of the highlighted chemical bonds in the molecules below is longest? Shortest? In between? Which highlighted bond requires the highest energy to break? Lowest? In between? Answer these questions by completing the second and third columns in the table. compound H HICIO | H :C=0: :0: || H-C-H H length of highlighted bond choose one choose one - V choose one - ✓ energy of highlighted bond choose one choose one choose one X Śarrow_forwardIn the following compound, identify all carbon atoms that you expect will be different in electron density. Drag the appropriate partial charges to these carbon atoms. S+ ..arrow_forwardComplete the Lewis structure for each of the following molecules using the information proVided in lable 1-4. You may assume that all formal charges are zero. All H atoms are shown; add only bonding pairs and lone pairs of electrons. (a) (b) нн H (c) N- H-C-Ć-C-N-0 н н H. N.arrow_forward
- Make a continuous model for C4H10 by using 4 black 4 hole carbon atoms, 10 white one hole hydrogen atoms, and 13 pink bonds. Then write in wedge dash notation C4H10 and add in missing hydrogen atoms.arrow_forward(a) Draw all resonance contributors of the following ion. In drawing each additional resonance structure, use curved arrows to indicate which pairs of electrons are being shifted. (b) Draw the resonance hybrid. (c) Which c–C bond is the longest?arrow_forwardWhich of the highlighted chemical bonds in the molecules below is longest? Shortest? In between? Which highlighted bond requires the highest energy to break? Lowest? In between? Answer these questions by completing the second and third columns in the table. compound H H | | H-C=C -0- - H H-C=C-O-H H H | | H-C-C-0-H I I H H length of highlighted bond choose one - choose one - v choose one energy of highlighted bond choose one - choose one choose onearrow_forward
- Organic Chemistry: A Guided InquiryChemistryISBN:9780618974122Author:Andrei StraumanisPublisher:Cengage Learning