17 smartbook
Which of the following factors will affect the relative strength of oxoacids? Select all that apply.
The number of O atoms attached to the central nonmetal atom The electronegativity of the central nonmetal atom
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
Which of the following formulas can be used to represent a hydrogen ion in aqueous solution?
H+ H3O+
Which of the following statements accurately describe Bronsted-Lowry acid-base reactions? Select all that apply.
The reactants and products contain an acid and a base. Some species can act as either an acid or a base depending on the other species present.
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
An acid donates a proton to form its conjugate _____ , which therefore has one less _____ atom and one more _____ charge than its acid.
base, H, negative
A Bronsted-Lowry acid is a proton _____ and must therefore contain at least one ionizable _____ atom in its formula.
donor; hydrogen
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
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, accepts, transfer
In the reaction illustrated here, a proton is transferred from _____, which is the Bronsted _____, to _____, which acts as the Bronsted _____.
water, acid, ammonia, base
Which of the following species are Lewis acids? Select all that apply.
BF3 SO3 Cu2+
The product of a Lewis acid-base reaction is (CH3)2OBF3. Select all the statements that correctly describe this reaction.
BF3 accepts an electron pair in this reaction. An empty 2p orbital on B accepts an electron pair from O.
Which of the protons depicted in the structure of acetic acid is considered acidic or ionizable?
D
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-
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 explain the relative strengths of the oxoacids shown: HBrO < HClO < HClO2 < HClO3? Select all that apply.
HClO3 is stronger that HClO2 because HClO3 has more O atoms. HBrO is weaker than HClO because Br is less electronegative than Cl.
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-
How does a conjugate acid differ from its conjugate base? Select all that apply.
The conjugate acid of a neutral base will have a charge of +1. The conjugate acid has one more H than its conjugate base. A conjugate base may be positively charged, neutral, or negatively charged.
Click and drag on elements in order Arrange the following compounds in order of increasing acid strength (weakest at the top to strongest at the bottom of the list).
h20 hf hbr
The strength of an acid is measured by its tendency to _____ and produce _____ ions in aqueous solution.
ionize, hydrogen
Match each species to the correct Lewis acid-base definition.
lewis base- Electron pair donor lewis acid- Electron pair acceptor
Which statement best explains the trend in acid strength: H2SO4 > H2SO3 > H2SeO3?
H2SO4 is stronger than H2SO3 because it has more O atoms
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
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 H2O is one of the Bronsted acid H2PO4 is one of the products.
Which of the hydrogens in chloroacetic acid is(are) considered acidic or ionizable?
The hydrogen bonded to oxygen
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
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
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