Question

Classify each of the following as a Lewis acid or a Lewis base. Drag the appropriate...

Classify each of the following as a Lewis acid or a Lewis base. Drag the appropriate items to their respective bins.

1.OH-

2.(CH3)2NH

3.SiCl4

4.I-

5.Ag+

6.NO2

7.CH3OH

Lewis acids

Lewis bases

Part C In the following pair, which species would you expect to be the stronger Lewis acid? Hints In the following pair, which species would you expect to be the stronger Lewis acid? Cu+ Cu2+

Pls add explanation i am still not clear what lewis acids and bases are. Thank you !

Homework Answers

Answer #2

answered by: anonymous
Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
Identify the Lewis acid and Lewis base from among the reactants in each of the following...
Identify the Lewis acid and Lewis base from among the reactants in each of the following equations. Part A Ag+(aq)+2NH3(aq)⇌Ag(NH3)2+(aq) a. Ag+ is the Lewis acid and NH3 is the Lewis base. b. Ag+ is the Lewis base and NH3 is the Lewis acid. Part B AlBr3+NH3⇌H3NAlBr3 a. AlBr3 is the Lewis base and NH3 is the Lewis acid. b. AlBr3 is the Lewis acid and NH3 is the Lewis base. Part C Cl−(aq)+AlCl3(aq)⇌AlCl4−(aq) a. AlCl3 is the Lewis acid...
Part A Classify the following reactions as precipitation reactions, oxidation-reduction reactions, or acid-base reactions. Drag each...
Part A Classify the following reactions as precipitation reactions, oxidation-reduction reactions, or acid-base reactions. Drag each item to the appropriate bin. Zn(s)+Ni2(aq)=Zn2+(aq)+Ni(s) Mg(OH)2(aq)+H2SO4(aq)=@H2O(1)+MgSO4(aq)
Classify each of the following reactants and products as an acid or base according to the...
Classify each of the following reactants and products as an acid or base according to the Brønsted theory:         CH3CH2O- + HC (triple bond) CH ......> HC (triple bond) C- (with lone pair) + CH3CH2OH
Which of the following is the softest Lewis acid? a. Ag+ b. Ac3+ c. Au+ d....
Which of the following is the softest Lewis acid? a. Ag+ b. Ac3+ c. Au+ d. As3+ So far from what i've found "soft" lewis acids have electronegativies around 2.2, they have a low or no charge, and they have a large cationic radius. Because Arsenic and Actinum have 3+ charges i've ruled them out so now I just have to determine which is the softer acid between Gold and Silver. The electronegativities of Gold and Silver are 2.54 and...
Write Bronsted acid-base equilibrium equations for the following: b) Show the acid-base conjugated species, labeling all...
Write Bronsted acid-base equilibrium equations for the following: b) Show the acid-base conjugated species, labeling all species c) Indicate if the species on the right or left of the reaction are favored/which way does the equilibrium lie?. Also can you explain why it shifts towards to the right or left? That's mostly the part I am having trouble understanding. HSO4-   + HSO3-  < - > HF + NO2- H2CO3  + NH3
For each of the following acid-base reactions, ~rewrite the reaction using complete Lewis structures for all...
For each of the following acid-base reactions, ~rewrite the reaction using complete Lewis structures for all reactants and products ~identify the Bronsted acid, the Bronsted base, the conjugate acid, and the conjugate base ~illustrate the movement of electrons in the reaction using "arrow-pushing" a.) HI(aq) + OH-(aq)------H2O(l) + I-(aq) b.) CO3-2(aq) + HCl(aq)--------HCO3-(aq) + Cl-(aq) (Note: for CO3-2, the carbon atom is the central atom.)
For the following equation label the conjugate acid-base pairs. HC2H3O2 + NH3 <===> NH4+ + C2H3O2-...
For the following equation label the conjugate acid-base pairs. HC2H3O2 + NH3 <===> NH4+ + C2H3O2- 2. The formation of products is strongly favored in this acid-base system: HX + B- <===> HB + X- a) Identify the bases competing for protons. b) Which is the weaker acid in the above equation? Explain. c) Which base is the stronger? Explain. d) How would the equilibrium be affected by the addition of the soluble salt, NaB? e) Would the Keq for...
Acid-Base Behavior In addition to following the general safety rules, chemicals need to be handled properly....
Acid-Base Behavior In addition to following the general safety rules, chemicals need to be handled properly. In particular, two very important classes of compounds called acids and bases require special attention. These compounds are commonly used reagents in the laboratory; therefore, understanding their proper disposal is beneficial. Physical differences between acids and bases can be detected by the some of the five senses, including taste and touch. Acids have a sour or tart taste and can produce a stinging sensation...
1.) You will work with 0.10 M acetic acid and 17 M acetic acid in this...
1.) You will work with 0.10 M acetic acid and 17 M acetic acid in this experiment. What is the relationship between concentration and ionization? Explain the reason for this relationship 2.) Explain hydrolysis, i.e, what types of molecules undergo hydrolysis (be specific) and show equations for reactions of acid, base, and salt hydrolysis not used as examples in the introduction to this experiment 3.) In Part C: Hydrolysis of Salts, you will calibrate the pH probe prior to testing...
Acid/Base Chemistry Portland Community College Staff* Version 42-0137-00-01 Lab Report Assistant                          &n
Acid/Base Chemistry Portland Community College Staff* Version 42-0137-00-01 Lab Report Assistant                                                                                             This document is not meant to be a substitute for a formal laboratory report. The Lab Report Assistant is simply a summary of the experiment’s questions, diagrams if needed, and data tables that should be addressed in a formal lab report. The intent is to facilitate students’ writing of lab reports by providing this information in an editable file which can be sent to an instructor. Observations                                                                                                            In columns...