2-7. A Lewis electron-dot diagram of the oxalate ion, C₂0₂², is shown.(a) Identify the hybridization of the valence orbitals of either carbon atom in the oxalate ion.(b) Silver oxalate, Ag₂C₂O4(s), is slightly soluble in water. The value of Köp for Ag₂C₂04 is 5,40 × 10-¹².(i) Write the expression for the solubility-product constant, Kp, for Ag₂C₂04.(ii) Calculate the molar solubility of Ag₂C₂O4 in neutral distilled water.

a). Hybridization is calculated with the help of steric number. Steric number = Number of sigma…

7. A Lewis electron-dot diagram of the oxalate ion, C₂042, is shown. (a) Identify the hybridization of the valence orbitals of either carbon atom in the oxalate ion. (b) Silver oxalate, Ag, C₂O4(s), is slightly soluble in water. The value of Kp for Ag₂C₂O4 is 5.40 × 10-¹². (i) Write the expression for the solubility-product constant, Kp, for Ag₂C₂O4. (ii) Calculate the molar solubility of Ag₂C₂O4 in neutral distilled water.

7. A Lewis electron-dot diagram of the oxalate ion, C₂042, is shown. (a) Identify the hybridization of the valence orbitals of either carbon atom in the oxalate ion. (b) Silver oxalate, Ag, C₂O4(s), is slightly soluble in water. The value of Kp for Ag₂C₂O4 is 5.40 × 10-¹². (i) Write the expression for the solubility-product constant, Kp, for Ag₂C₂O4. (ii) Calculate the molar solubility of Ag₂C₂O4 in neutral distilled water.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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The sulfate ion can be represented with four S-O bonds or with two S-O and two So=O bonds.(a) Which representation is better from the standpoint of formal charges?(b) What is the shape of the sulfate ion, and what hybrid orbitals of S are postulated for the σ bonding?(c) In view of the answer to part (b), what orbitals of S must be used for the π bonds? What orbitals of O?(d) Draw a diagram to show how one atomic orbital from S and one from O overlap to form a π bond.
(a) What are trihalomethanes (THMs)? (b) Draw the Lewisstructures of two example THMs.
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The sulfate ion can be represented with four S—O bonds orwith two S—O and two S=O bonds. (a) Which representation is better from the stand point of formal charges? (b) What is theshape of the sulfate ion, and what hybrid orbitals of S are postu-lated for the σ bonding? (c) In view of the answer to part (b),what orbitals of S must be used for the π bonds? What orbitalsof O? (d) Draw a diagram to show how one atomic orbital fromS and one from O overlap to form a π bond.
The strength of a covalent bond depends upon the size of the atoms and the bond order. In general short bonds are strong bonds. For each pair of covalently bonded atoms, choose the one expected to have the higher bond energy.(A) N≡N(B) N-N ...... (A,B) fill in the blank 1(C) C=O(D) C≡O ...... (C,D) fill in the blank 2