Chemistry Chapter 17

An acid donates a proton to form its conjugate ____________ which therefore has one less _____________ atom and one more _________ charge than its acid.

base; hydrogen; negative

Match each species to the correct Lewis acid-base definition

Lewis base ---> electron pair donor Lewis acid ---> electron pair acceptor

Which of the following types of substances are classified as acids only under the Lewis definition? Select all that apply.

Molecules that contain a polar multiple bond Molecules with electron deficient central atoms

Arrange the following compounds in order of increasing acid strength (weakest at the top to strongest at the bottom of the list).

1. H2O 2. HF 3. HBr

A Bronsted-Lowry acid is a proton _____ and must therefore contain at least one ionizable _____ atom in its formula.

donor; hydrogen

An acid-base reaction occurs when one species loses a(n) ______ and another species simultaneously _________ a proton. An acid-base reaction can therefore be viewed as a proton-___________ process.

proton; gains; transfer

The two factors that influence the extent of ionization of an acid are the ________ and __________ of the HX bond, where HX is the general formula of an acid

strength; polarity

In the reaction illustrated here, a proton is transferred from _____, which is the Bronsted _____, to _____, which acts as the Bronsted _____.

water, acid, ammonia, base

How does a conjugate acid differ from its conjugate base? Select all that apply.

A conjugate base may be positively charged, neutral, or negatively charged. The conjugate acid has one more H than its conjugate base. The conjugate acid of a neutral base will have a charge of +1.

Which statement best explains the trend in acid strength: H2SO4 > H2SO3 > H2SeO3?

H2SO4 is stronger than H2SO3 because it has more O atoms.

Water is an amphoteric species. Match the product formed from water acting as an acid or a base.

H3O+ Water acting as a base. . OH- Water acting as an acid.

Which of the following formulas can be used to represent a hydrogen ion in aqueous solution?

H+ H3O+

Predict which of the following species would act as an amphoteric compound, that is, as both a Bronsted acid and a Bronsted base? Select all that apply.

H2PO4- HCO3- H2O

Which of the following statements accurately describe Bronsted-Lowry acid-base reactions? Select all that apply.

Some species can act as either an acid or a base depending on the other species present. The reactants and products contain an acid and a base.

Oxoacids have the general formula illustrated, where the number of bonds to the central element E can vary. For the same element E, acid strength will _____ as the number of O atoms increases. For the same number of O atoms, acid strength increases as the _____ of element E increases.

increase; electronegativity

The product of a Lewis acid-base reaction is (CH3)2OBF3. Select all the statements that correctly describe this reaction.

An empty 2p orbital on B accepts an electron pair from O. BF3 accepts an electron pair in this reaction.

Which of the protons depicted in the structure of acetic acid is considered acidic or ionizable?

D Reason: In carboxylic acids, the ionizable proton is the one bonded to oxygen. Hydrogen atoms bonded to carbon do not ionize.

Select all the reactions in which the Lewis acid is a cation and the Lewis base is a molecule with one or more lone pairs of electrons.

Fe3+ + 6H2O ⇌ Fe(H2O)63+ Ni2+ + 6NH3 ⇌ Ni(NH3)62+

Which of the following is NOT a conjugate acid-base pair?

H2PO4-/PO43- Reason: Conjugate acid-base pairs differ by a single proton (H+). The conjugate acid of PO43- is HPO42-, not H2PO4-.

Which of the following statements correctly describes the relative strength of binary acids?

H2S is a stronger acid than H2O.

Which of the following statements correctly describe the relationship between the species in the reaction shown? Select all that apply.

HSO3- is the conjugate acid of SO32-. The base in the forward reaction is CH3NH2. B and D are a conjugate acid-base pair.

What is the conjugate base of HNO2 if it reacts as a Bronsted acid in H2O?

NO2- Reason: NO2- is the conjugate base of the Bronsted acid HNO2; a conjugate acid-base pair differ by one proton (H+).

Which of the following species are Lewis acids? Select all that apply.

SO3 Cu2+ BF3

Which of the hydrogens in chloroacetic acid is(are) considered acidic or ionizable?

The hydrogen bonded to oxygen

A Bronsted-Lowry base is a __________ proton . A Bronsted-Lowry base must contain an available ___________ pair of in its formula in order to form a _____________ bond to H+.

acceptor; lone; electrons; covalent

A Lewis acid is any species that _____ an electron pair, whereas a Lewis base is a species that _____ an electron pair.

accepts; donates

In a Bronsted-Lowry acid-base reaction, the acid reacts to form its _____ and the base will form its _____.

conjugate base conjugate acid

An acid can be defined as a substance that loses one or more H+ ions when dissolved in water. An H+ ion is a hydrogen atom that has lost a(n) ___________ and is therefore just a(n) ____________. The H+ ion is not an isolated ion, but interacts strongly with H2O to produce the ______________ ion, which has the formula H3O+.

electron; proton; hydronium

The strength of an acid is measured by its tendency to __________ and produce _____________ ions in aqueous solution.

ionize; hydrogen

Which of the following statements correctly explain the relative strengths of the oxoacids shown: HBrO < HClO < HClO2 < HClO3? Select all that apply.

HBrO is weaker than HClO because Br is less electronegative than Cl. HClO3 is stronger than HClO2 because HClO3 has more O atoms.

The hydrogen phosphate ion, HPO42-, can act as both a Bronsted acid and Bronsted base in water. Select all the options that correctly describe the reaction that occurs when HPO42- acts as a Bronsted base in water.

OH- is one of the products. H2PO4- is one of the products. H2O acts as the Bronsted acid.

Which of the following factors will affect the relative strength of oxoacids? Select all that apply.

The electronegativity of the central nonmetal atom The number of O atoms attached to the central nonmetal atom

The product of a Lewis acid-base reaction contains a new bond called a __________ covalent bond

coordinate

A Lewis acid-base reaction results in the donation of a pair of electrons from the base to the acid in the formation of a(n) _____ bond.

coordinate covalent