Identify the molecules or ions below as Lewis acids, Lewis bases, or neither.If there is more than one possible site in the molecule/ion, focus on the central or the charged atom.а)Zn+2b)FeCl3NH2c)

Answer- 1-Lewis acid are those chemical species which have tendency to accept lone pair of electron…

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Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter14: Acids And Bases

Section14.9: Lewis Acids And Bases

Problem 14.25CE: Predict whether each of these is a Lewis acid or a Lewis base. (Hint: Drawing a Lewis structure for...

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1. Which of the following can act as a Lewis acid? (Hint : In each case, draw the Lewis electron dot structure of the molecule or ion. Are there lone pairs of electrons on the central atom? If so, it can be a Lewis base. Does the central atom lack an electron pair? If so, it can behave as a Lewis acid.) PH3 BCl3 H2S HS−
Boron trifluoride, BF3, and diethyl ether, (C2H5)2O, react to produce a compound with the formula BF3 : (C2H5)2O. A coordinate covalent bond is formed between the boron atom on BF3 and the oxygen atom on (C2H5)2O. Write the equation for this reaction, using Lewis electron-dot formulas. Label the Lewis acid and the Lewis base. Determine how many grams of BF3: (C2H5)2O are formed when 9.10 g BF3 and 23.3 g (C2H5)2O are placed in a reaction vessel, assuming that the reaction goes to completion.
Predict whether each of these is a Lewis acid or a Lewis base. (Hint: Drawing a Lewis structure for a molecule or ion often helps to make such predictions.) (a) PH3 (b) BCl3 (c) H2S (d) NO2 (e) Ni2+ (f) CO
Which of the following compounds or ions has the weakest conjugate base? Briefly explain your choice. a) HCN b) HClO c) NH4+
Pure liquid ammonia ionizes in a manner similar to that of water. (a) Write the equilibrium for the autoionization of liquid ammonia. (b) Identify the conjugate acid form and the base form of the solvent. (c) Is NaNH2 an acid or a base in this solvent? (d) Is ammonium bromide an acid or a base in this solvent?
For oxyacids, how does acid strength depend on a. the strength of the bond to the acidic hydrogen atom? b. the electronegativity of the element bonded to the oxygen atom that bears the acidic hydrogen? c. the number of oxygen atoms? How does the strength of a conjugate base depend on these factors? What type of solution forms when a nonmetal oxide dissolves in water? Give an example of such an oxide. What type of solution forms when a metal oxide dissolves in water? Give an example of such an oxide.
Will 0.10 M solutions of the following salts be acidic, basic, or neutral? See Appendix 5 for Ka values. a. ammonium bicarbonate b. sodium dihydrogen phosphate c. sodium hydrogen phosphate d. ammonium dihydrogen phosphate e. ammonium formate
Two strategies are followed when solving for the pH of an acid in water. What is the strategy for calculating the pH of a strong acid in water? What major assumptions are made when solving strong acid problems? The best way to recognize strong acids is to memorize them. List the six common strong acids (the two not listed in the text are HBr and HI). Most acids, by contrast, are weak acids. When solving for the pH of a weak acid in water, you must have the Ka value. List two places in this text that provide Ka values for weak acids. You can utilize these tables to help you recognize weak acids. What is the strategy for calculating the pH of a weak acid in water? What assumptions are generally made? What is the 5% rule? If the 5% rule fails, how do you calculate the pH of a weak acid in water?
Decide whether each of the following substances should be classified as a Lewis acid or a Lewis base. (a) H2NOH in the reaction H2NOH(aq)+HCl(aq)[H3NOH]Cl(aq) (b) Fe2+ (c) CH3NH2 (Hint: Draw the electron dot structure)