Which of the following is an electron pair donor? a. Arrhenius acid b. Arrhenius base c....
Question:
Which of the following is an electron pair donor?
a. Arrhenius acid
b. Arrhenius base
c. Bronsted-Lowry acid
d. Bronsted-Lowry base
e. Lewis acid
f. Lewis base
Acids and Bases:
Many scientists have given different definitions for defining acids and bases. The basic definition of an acid and a base is that an acid is a substance that releases {eq}H^+ {/eq} ions in the aqueous solution whereas a base is a substance that releases {eq}OH^- {/eq} ions in its aqueous solution.
Answer and Explanation: 1
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View this answerThe correct option is (f.) Lewis base.
According to Lewis's concept, an acid is a substance that can accept a pair of electrons, whereas a base is a...
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The Bronsted-Lowry and Lewis Definition of Acids and Bases
from
Chapter 10 / Lesson 4
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Chemist Johannes Bronsted and scientist Thomas Lowry proposed that an acid should be defined as a substance that can donate a proton, while a base is any substance that can accept protons. American chemist G.N. Lewis proposed a different theory. Learn about three popular scientific definitions of acids and bases.
Related to this Question
- Which of the following is a proton donor? a. Arrhenius acid b. Arrhenius base c. Bronsted-Lowry acid d. Bronsted-Lowry base e. Lewis acid f. Lewis base
- Which of the following is an electron pair acceptor? a. Arrhenius acid b. Arrhenius base c. Bronsted-Lowry acid d. Bronsted-Lowry base e. Lewis acid f. Lewis base
- Which of the following is a proton acceptor? a. Arrhenius acid b. Arrhenius base c. Bronsted-Lowry acid d. Bronsted-Lowry base e. Lewis acid f. Lewis base
- Which of the following produces protons in an aqueous solution? a. Arrhenius acid b. Arrhenius base c. Bronsted-Lowry acid d. Bronsted-Lowry base e. Lewis acid f. Lewis base
- Which of the following produces hydroxide ions in an aqueous solution? a. Arrhenius acid b. Arrhenius base c. Bronsted-Lowry acid d. Bronsted-Lowry base e. Lewis acid f. Lewis base
- Which of the following is both an Arrhenius and Bronsted-Lowry base? a. HCOOH(aq) b. NH4OH(aq) c. HCl(g) d. NH3(g)
- Which of the following is a Bronsted-Lowry base but not a Lewis base? a) H_2O b) CO_3^{-2} c) CN^- d) NH_3 e) all choices are both a B/L and Lewis base.
- Which acts as a Lewis acid but neither Arrhenius nor Bronsted-Lowry? a. H2CO3 b. HCO3- c. BF3 d. HClO3
- What is a compound that can donate a proton called? a. Bronsted-Lowry acid b. Bronsted-Lowry base c. Lewis acid d. Lewis base
- Which act as a Lewis acid but neither Arrhenius nor Bronsted- Lowry? (a) H_2SO_4 (b) HSO_4^- (c) CH_3CH_2COOH (d) Ni^{2+}
- Which pair below cannot have a Bronsted-Lowry acid base reaction between them? a. OH- and NH b. PO43- and ClO- c. HCO3- and SO32- d. HClO4 and HNO2 e. HSO4- and HCl
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- In the reaction A l C l 3 + C l A l C l 4 , the C l functions as a(n) (a) Bronsted-Lowry acid. (b) Bronsted-Lowry base. (c) Arrhenius base. (d) Lewis acid. (e) Lewis base.
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- What is the difference between an Arrhenius acid/base, a Bronstead Lowry acid/base and a Lewis acid/base?
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- In the following reaction, identify any Arrhenius, Bronsted-Lowry, and Lewis acids and bases. HNO3 + KOH arrow H2O + KNO3
- Classify the following substances as a Bronsted-Lowry acid, Bronsted-Lowry base, Lewis acid, and/or Lewis base. HCl, BF_3, CCl_3, -H CH_2O, CH_3Cl -OCH_3 , NH_3
- Which of the following represents a Bronsted-Lowry conjugate acid-base pair? a) SO3{(2-) and SO2 b) CO3(2-) and CO c) H3O and H2 d) NH4+ and NH3
- In the following reaction, does NH3 act as a Bronsted-Lowry acid, Bronsted-Lowry base, Lewis acid, and/or Lewis base? HBr(aq) + NH3(aq) arrow Br-(aq) + NH4+(aq)
- In the following reaction, does BH3 act as a Bronsted-Lowry acid, Bronsted-Lowry base, Lewis acid, and/or Lewis base? BH3(aq) + NH3(aq) arrow BH3NH3(aq)
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- Which of the following is a Bronsted Lowry base? (a)Cl^{ -} (b)HNO_3 (c)NH_4^{+} (d)HNO_3
- CH_3CH_2OCH_2CH_3 is best classified as a ______. A) Bronsted-Lowry acid. B) Lewis acid. C) Bronsted-Lowry base. D) Lewis base. E) Both C & D.
- Identify the Bronsted Lowry acid, bace, and conjugates in the following reaction HNO2 H2SO4 HSO4- NO2- Options 1) bronzed lowry acid 2) Bronsted lowry base 3) conjugated base bronsted lowry ac
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- For the following chemical reaction, decide whether the NH3 reactant is a Bronsted-Lowry acid, a Bronsted-Lowry base, or neither. HNO3 (aq) + NH3 (aq) rightarrow NO3^(-) (aq) + NH4^(+) (aq)
- For the following chemical reaction, decide whether the NO3^(-) reactant is a Bronsted-Lowry acid, a Bronsted-Lowry base, or neither. NO3^(-) (aq) + NH4^(+) (aq) rightarrow HNO3 (aq) + NH3 (aq)
- Which of the following is NOT true? A) The Arrhenius Model of acids and bases applies toward substances that are nonaqueous. B) The Arrhenius Model of acids and bases was developed before the Bronsted-Lowry Model. C) The Bronsted-Lowry Model can apply to
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- Is C a ( O H ) 2 an Arrhenius base, a Bronsted-Lowry base, or both?
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- What are the two Bronsted-Lowry acids in the following: H2S+H2O <----> HS-+H3O+
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- Which of the following reactions are Bronsted-Lowry acid base reactions?
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- Rank the acid-base definitions from most specific (exclusive) to most general (inclusive): a. Arrhenius, Bronsted-Lowry, Lewis b. Arrhenius, Lewis, Bronsted-Lowry c. Bronsted-Lowry, Lewis, Arrhenius d. Lewis, Arrhenius, Bronsted-Lowry
- What is the role of methylchloride in the following reaction? a. Lewis acid b. Lewis base c. Bronsted-Lowry acid d. Bronsted-Lowry base
- A Bronsted-Lowry base is defined as: a. a hydroxide ion b. a proton donor c. a hydronium ion d. a proton acceptor e. an electron pair acceptor
- Classify the given compound as a Lewis base, a Bronsted-Lowry base, both, or neither.
- Are all Arrhenius acids and bases also Bronsted-Lowry acids and bases? Explain.
- HNO3 (aq) + H2O (l) \rightarrow H3O+ (aq) + NO3- (aq) Identify the reactant that is a Bronsted- Lowry Acid and the reactant that is a Bronsted- Lowry Base in the reaction.
- Tell if the given compound acts as a Lewis base, a Bronsted-Lowry base, both, or neither.
- Which are the Bronsted-Lowry bases? (a) PO_{43} and HPO_{42} (b) PO_{43} and OH (c) PO_{43} and H_2O (d) H_2O and OH (e) H_2O and HPO_{42}
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- According to the Bronsted-Lowry model, an acid is a "proton donor" and a base is a "proton acceptor". Explain.
- Which of the following is a Bronsted-Lowry acid? a. HCl b. AlCl3 c. BCl3
- Which of the following statements about Lewis acids and bases is true? a. A Lewis base always accepts an electron pair from a Lewis acid. b. The interaction between a Lewis acid and a Lewis base creates a covalent bond. c. Lewis acids are also commonly ca
- Which of the following cannot act as a Bronsted-Lowry acid? (a) NH4+ (b) NO3- (c) HCl (d) HC2H3O2 (e) H3PO4
- For the following, identify the Bronsted-Lowry acid, the Bronsted-Lowry base, the conjugate acid, and the conjugate base. HBr (aq) + H_2O (l) to H_3O^+ + Br^- (aq)
- For the following, identify the Bronsted-Lowry acid, the Bronsted-Lowry base, the conjugate acid, and the conjugate base. HI(aq) + H_2O to H_3O^+(aq)+I^-(aq)
- How is a species that can accept electrons classified? a. Lewis base b. Lewis acid c. Bronsted-Lowry acid d. Bronsted-Lowry base
- Classify each of the compounds NaH, BeH_2, BH_3, CH_4, NH_3, H_2O, and HF as a Bronsted-Lowry base, a Bronsted- Lowry acid, or neither.
- Which of the following is an acid according to Bronsted-Lowry Acid-Base Theory? 1) KCl 2) NaOH 3) None of these are correct 4) HC2H3O2 5) NH3
- For the following chemical reaction, decide whether the NH4^(+) reactant is a Bronsted-Lowry acid, a Bronsted-Lowry base, or neither. NO3^(-) (aq) + NH4^(+) (aq) rightarrow HNO3 (aq) + NH3 (aq)
- Which of the following is not a Bronsted-Lowry acid? a. H2CO3 b. HCO3- c. CO32- d. H2O e. H3O+
- Identify each reactant and product in the given chemical reaction as a Bronsted-Lowry acid, a Bronsted-Lowry base, or neither. Arrange the species in the given reaction as conjugate acid-base pairs. HNO2+H2O--H3O+ +NO2-
- Would the reaction of NaOH and HCl be Arrhenius, Bronsted-lowry, or lewis? What about NaOH and H_2SO_4?
- Which of the following statements about Lewis acids and bases is true? \\ A. Lewis base always accepts an electron pair from a Lewis acid B. Lewis acids are also commonly called nucleophiles. C. A Lewis base always accepts a proton (H^+) from a Lewis a
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- Identify the Bronsted-lowry acids and bases : HCN(aq) + NO_2(aq) \to CN(aq) + HNO(aq).
- Identify the Bronsted-Lowry acids and bases in these reactions and group them into conjugate acid-base pairs. a) NH3 + HBr = NH4+ + Br- b) NH4+ + HS- = NH3 + H2S c) H3O+ + PO4^3- = H2O + HPO4^2-
- Could a Bronsted-Lowry acid not be an Arrhenius acid? Explain.
- Are all Lewis bases also Bronsted-Lowry bases? Explain.
- 2Li+(aq) + 2OH(aq) + H2SO3(aq) 2Li+(aq) + SO32(aq) +2H2O(l) The acid base reaction above can be explained by A. only the Arrhenius theory. B. only the Bronsted-Lowry theory. C. only the Lewis theory. D. the Arrhenius, Bronsted-Lowry, and Lewis theories
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- Identify the Bronsted-Lowry acid and base in the given reaction and group them into conjugate acid-base pairs. NH3+ HBr-- NH4+ + Br-
- Are all Arrhenius bases also Bronsted - Lowry bases? Explain.
- CO3^2- (aq) + H2O (l) \rightarrow (HCO3)- (aq) + OH- (aq) Identify the reactant that is a Bronsted- Lowry Acid and the reactant that is a Bronsted- Lowry Base in the reaction.
- Classify each of these compounds as a Bronsted-Lowry acid, a Bronsted-Lowry base, or neither. H2SO4, HF, HNO2, (CH3)3N, C2H5NH2, NH3, KCl, CHCl3.
- Using the Bronsted-Lowry definition of acids and bases, identify the reactants in the following reaction as an acid or base. H3O+ + Cl- arrow H2O + HCl
- For the following chemical reaction, decide whether the HNO3 reactant is a Bronsted-Lowry acid, a Bronsted-Lowry base, or neither. HNO3 (aq) + NH3 (aq) rightarrow NO3^(-) (aq) + NH4^(+) (aq)
- Indicate which of the following substances can act as (i) an acid, (ii) a base, or (iii) both according to the Arrhenius (classical) theory or the Bronsted-Lowry theory. (Do not be confused by the way in which the formulas are written.) a) H_2S b) PO(OH)
- According to the Bronsted-Lowry definition, which chemical in the following reaction is the base? H 3 P O 4 + H 2 O H 3 O + + H 2 P O 4
- Identify the Bronsted-Lowry acid and base in the reaction below: K O H + H B r H 2 O + K B r
- Which of the following rows identifies the Bronsted-Lowry acids and a conjugate acid-base pair in the equation above?
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