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.
Want to see the full answer?
Check out a sample textbook solutionChapter 2 Solutions
EP ORGANIC CHEMISTRY -MOD.MASTERING 18W
- You will not find “hydroxide” in the stockroom, but you will find sodium hydroxide (NaOH) andpotassium hydroxide (KOH). Lithium hydroxide (LiOH) is expensive and used in spacecraft airfilters since hydroxide reacts with carbon dioxide, and lithium is lighter than sodium or potassium.Cesium and francium hydroxides are very expensive and little used. Is this information consistentwith your answer to the previous question?arrow_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_forward● 8. Draw all the possible resonance structures for (a) and (b) and predict which has the greatest contribution. Briefly justify your answer(s). 10 a) b) O ΟΞΗarrow_forward
- Consider the reaction 2H₂ + O₂ --> 2H₂O. One way to imagine this reaction (this is NOT how it really happens) is by breaking all the bonds in H₂ and O2, and then forming new bonds in the H₂O. In the three boxes below, draw out: 2H₂ + O2 (Showing all the bonds) What it would look like if all the bonds in 2H₂ + O2 broke 2H₂O (showing all the bonds)arrow_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_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_forward
- The bond energy of C2 is 599 kJ/mol, the bond distance is 110 pm. Take a rough estimate of the Coulomb repulsion in doubly ionized C2 (i.e., C22+). How far would the C-C bond have to stretch for the Coulomb repulsion to be less than the bond energy in neutral C2? Do you think that the C22+ molecule will still be stable?arrow_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.) CO3²- CO NO₂ CNO (include isomers) Al₂Cl6 B₂H6 O2 (paramagnetic) H3O+ LiF IF7arrow_forwardTwo useful organic compounds that contain Cl atoms are vinyl chloride (CH2 = CHCI) and chloroethane (CH;CH;CI). Vinyl chloride is the starting material used to prepare poly (vinyl chloride), a plastic used in insulation, pipes, and bottles. Chloroethane (ethyl chloride) is a local anesthetic. Why is the C – Cl bond of | vinyl chloride stronger than the C – Cl bond in chloroethane.arrow_forward
- 3. Resonance can be used to explain the relative stabilities of the two "phenoxide" ions shown below. Draw the resonance structures of each ion and based on those structures, explain why one is more stable than the other. 90 more stable a. Draw the resonance structures: 00 oe less stable b. Explain the observation. Why is one more stable than the other?arrow_forward23. Given AH+ [(NF3(g)] = -132 kJ mol-¹ and the bond enthalpy (D) data, D(N₂) = 946 kJ mol-¹ and D(F2) = 159 kJ mol-, which of the following statements is/are FALSE? The average N-F bond enthalpy in NF3 is 281 kJ mol-¹. AH+ [(NF3(g)] > AH+ [(NF3(1)] AH+ [(F(8)] = 159 kJ mol-¹ CEEarrow_forward5.) a.) F-S-F bond angles in OSF4 are 115° and 164° while F-S-F bond angles in SF4 are 101° and 173°. Draw the structure you would expect for OSF4 and SF4, and suggest a reasonable explanation for the observed F-S-F bond angles. b.) predict the shapes of the molecule (Me3P) SBCI3 and indicate approximate bond angles (ex. >180 or <180, etc.) around the central atom. Explain your reasoning.arrow_forward
- Organic Chemistry: A Guided InquiryChemistryISBN:9780618974122Author:Andrei StraumanisPublisher:Cengage Learning