lewis base => electron pair donar species are called as
lewis base
a) CO = Carbon monoxide here the oxygen has two lone pairs and then it can donate electron pair and acts as lewis base
b) O2- => here the oxygen has three lone pairs and then it can donate electron pair and acts as lewis base
c) Ag+ => the ion is cation and then it accepts the electron pair rather than donating and then acts as lewis acid not base
d) NH3 => here the nitrogen has one lone pair and then it can donate electron pair and acts as lewis base
e) CN- => here the nitrogen has one lone pair and then it can donate electron pair and acts as lewis base
answer => C
which of these substances cannot behave as a lewis base in an aq solution a- Co...
which of the combination of substances below constitute a Lewis acid-base reaction? a) PH3+ H+ b) Ag+ + NH3 c) BF3 + NH3 d) CH3CH2OCH2CH3 +AlCl3 I'm stuck between a and b, but I am very confused because both seem to be lewis acids and bases to me
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Identify the Lewis acid and Lewis base in the reactant of the reaction: HCl (aq) + NH3 (aq) = NH4+ (aq) + Cl(aq)
17 5 points Which of the following cannot act as a Lewis base? O C₂O4²- OCH OCH4 O NH3 O H20 Previous
1. Which of the followi ch of the following reactions is not readily explained by the Arrhenius concept of acids and bases? a. A. HCl(aq) + NaOH(aq) - NaCl(aq) + H20() b. H30(aq) + OH-(aq) + 2H20(1) c. HCI(g) + NH3(g) - NH4Cl(s) d. HC2H302(aq) + H2O(l) H30*(aq) + C2H302-(ag) e. H30 (aq) + OH-(aq) + 2H2O(aq) 2. Classify each of the following species as Brønsted acid or base or both: a) H20, b) OH", c) H30, d) NH3, e)...
1. Which of the followi ch of the following reactions is not readily explained by the Arrhenius concept of acids and bases? a. A. HCl(aq) + NaOH(aq) - NaCl(aq) + H20() b. H30(aq) + OH-(aq) + 2H20(1) c. HCI(g) + NH3(g) - NH4Cl(s) d. HC2H302(aq) + H2O(l) H30*(aq) + C2H302-(ag) e. H30 (aq) + OH-(aq) + 2H2O(aq) 2. Classify each of the following species as Brønsted acid or base or both: a) H20, b) OH", c) H30, d) NH3, e)...