Concept explainers
(a)
To determine: The amount of charge separation in the given
Interpretation: The amount of charge separation in the given
Concept introduction: The polarity of an individual bond is measured as its bond dipole moment. A quantity that describes two opposite charges separated by a distance is the dipole moment. The dipole moment is calculated by the formula,
(b)
To determine: The relative importance of the given two resonance contributors.
Interpretation: The relative importance of the given two resonance contributors is to be evaluated.
Concept introduction: The delocalization of electrons due to the presence of lone pair of electrons and double bond is called resonance. The resonance structure is more stable if there are more resonating structures. In resonance forms of any compound, the connectivity of atoms is same but the distribution of electrons is different. Resonance helps to explain the structure and reactivity of organic molecules.
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Organic Chemistry (9th Edition)
- 4. Determine the enthalpy of reaction for the below (you will need to use a bond dissociation energy (BDE) table from book/internet): a. (CH3)2CH2 + Brz > (CH3)2CHBr + HBr b. (CH3)3CH + Br₂ → (CH3)3CBr + HBrarrow_forwardD. Calculate the enthalpy of dissociation (or bond energy) of the X-X bond. Treat multiplication as consecutive addition for the purpose of sig. figs. Reaction AH value Reaction/Process Enthalpy of sublimation of M i. AHsub = 137 kJ/mol First ionization energy of M i. AHIE1 = 765 kJ/mol -> AHIE2 = 1221 kJ/mol Second ionization iii. energy of M AHIE3 = 7453 kJ/mol Third ionization iv. energy of M Enthalpy of dissociation of X2 (g) AHD = ?? V. AHEA1 = -366 kJ/mol First electron affinity of X %3! vi. AHlattice = -5230. kJ/mol vii. Lattice energy of MX3 Enthalpy of formation vii. M (s) + X2 (g) MX3 (s) AH: = 3882 kJ/mol of MX3arrow_forwardI need part C, please explain how to do the problem, it would help a lot!!arrow_forward
- a) Rank the following bonds in order of decreasing strength (decreasing bond dissociation energies: BDE), from strongest to weakest, and briefly explain your answer. O-H, O-C, C=O, O=O b) Rank the following bonds in order of decreasing strength (decreasing bond dissociation energies: BDE), from strongest to weakest, and briefly explain your answer. N-H, N=N, N=C, N≡Narrow_forward9a.) Let's put some pieces together. We can also apply energy diagrams to resonance structures. Explain what is happening in the following energy diagram AND draw curved arrows to show the "movement" of electrons from A, to A2.arrow_forward22.) Estimate the enthalpy of reaction of the given reaction using the following data: C3H6 (g) + Hz (g) → C3H8 (g) Bond С-Н H-H С-С C=C Bond Energy (kJ/mol) 614 413 432 347 a.) -220 kJ/mol b.) -286 kJ/mol c.) -127 kJ/mol d.) 286 kJ/mol 23.) Calculate the standard enthalpy of combustion of aniline from the following standard enthalpies of formations. C6H5NH2 (1) + 31/4 02 (g) –→ 6 CO2 (g) + ½ N2 (g) + 7/2 H2O (1) H20 (1) CO2 (g) -393.51 C6H5NH2 (1) -285.83 A:H° (kJ/mol) +31.1 c.) -3123 kJ/mol d.) -4107 kJ/mol a.) -3393 kJ/mol b.) -3330 kJ/molarrow_forward
- 1. Mark the following statements (A-E) as true or false A. The halogen bond dissociation energy decreases in the row Cl2 Br2 I2 because of repulsion between the electrons in the lower shells. B. The melting points of the dihalogens increase down the group because the interactions between the dihalogen molecules get stronger C. The electronegativity of the halogens decreases down the group because of the decrease of the electron affinity and the increase of the ionization energy. D. The unusually low bond dissociation energy of the F2 molecule is a direct result of the high electronegativity of fluorine E. The high reactivity of fluorine is in part due to the low bond dissociation energy of the F2 moleculearrow_forwardDraw Lewis structures and assign formal charges for the following compounds and ions. Note any resonance forms and explain which resonance form is the most important. Make a note of any other unusual features (such as "this one doesn't work" and why-what are the shortcomings of the model.) 2- CO3²- B₂H6 CO O₂ (paramagnetic) H₂O* LiF IF, NO₂ CNO (include isomers) Al₂Cl6arrow_forwardQuestions 6a, b, c, d is linked to one another and focus on the molecule shown below. H ба) Before we can start assigning hybridization, we need to correctly assign our VSEPR electron-pair geometries to each central atom. For each of the chosen central atom, match it with it's corresponding electron-pair geometry. Drag and drop options on the right-hand side and submit. For keyboard navigation. SHOW MORE V C1 trigonal planar c C2 linear O N1 tetrahedral C trigonal pyramidal N 01 tetrahedral N trigonal planar o Bent O tetrahedral O :0: :0= II II I-0 - -I I-z: Iarrow_forward
- The purple pathway: the oxygen - flow to the C-O bond, then from the C=C bond to the carbon atom, then the water molecule. I do not understand why cant the electrons flow from the oxygen - to the water directly AND why cant electrons flow from C=c to the water molecule , but have to land on a carbon atom first before flowing to water.arrow_forwardWhich of the following item(s) explain the differences between the Ka values.Choose one or more: A. The negative charge is on the more electronegative fluorine atom in trifluoroacetate. B. The oxidation state for oxygen in trifluoroacetate is more negative than the oxidation state for oxygen in acetate. C. The trifluoroacetate molecule has more resonance structures than the acetate molecule. D. The electron-withdrawing fluorine atoms pull electron density from the oxygen in trifluoroacetate. The negative charge is more stabilized in trifluoroacetate by this effect.arrow_forwardWhat is the molecular electronic structure (energy levels diagram) of the sulfur molecule (S2), (S2-) and (S2+)? Arrange the three cases in ascending order according to the following: 1- Electrical properties 2- Magnetic properties 3- Bonding strength (B.O) 4 Length of the bond 5- Stability 6-lonization susceptibility (IE) 7- Irritability (effects) 8- Polarity of the bond معدلة 6:53 مarrow_forward
- Principles of Modern ChemistryChemistryISBN:9781305079113Author:David W. Oxtoby, H. Pat Gillis, Laurie J. ButlerPublisher:Cengage Learning