18.1.3 Inductive Effects Flashcards
When a molecule acts as a Brønsted-Lowry acid, it…
donates a proton to another molecule.
The ability of a molecule to act as a Brønsted-Lowry acid depends upon several factors. Which of these factors does not influence the acidic nature of a molecule directly at the H–X bond?
Inductive effects
If X is electron-rich in the molecule, X—O–H, which bond is polarized?
X—O
A simple dissociation reaction is written for each of the following acids. The inductive effect accounts for the acidic behavior of ______________.
The hydrated aluminum(III) ion;
Al(H2O)63+ (aq) ↔ H + (aq)
+ Al(H2O)5OH 2+ (aq)
Consider the relationships among acids whose strengths are compared below.
H3PO4 < HNO3
HNO2 < HNO3
H2SeO4 < H2SO4
H2SeO3 < H2SO3
HBrO4 < HClO4
HBrO3 < HClO3
H2SO3 < H2SO4
HClO < HClO2 < HClO3 < HClO4
Which of the following conclusions cannot be made from the relationships given above?
HNO2 < H3PO3
The type of electron density pattern and bond polarity depicted in the diagram below best correlates with the acidic / basic behavior of which of the following molecules?
NaOH
Which of the following is considered a relatively concentrated solution of a weak acid?
1 M HF
Which of the following is not true with regards to the acidity of the oxoacid, H–O–X?
The polarity of the O–H bond does not depend on the electronegativity of X.
Arrange the following oxoacids from the weakest to the strongest acid:
HClO hypochlorous acid HClO2 chlorous acid HIO hypoiodous acid HBrO hypobromous acid
The electronegativity values for constituent elements are:
H 2.1 O 3.5 I 2.5 Br 2.8 Cl 3.0
hypoiodous acid < hypobromous acid < hypochlorous acid < chlorous acid
Hypochlorous acid (HOCl), hypobromous acid (HOBr), hypoiodous acid (HOI), and methanol (HOCH3 ) are all considered weak acids. What factor best explains the relationship in relative acidities among these molecules?
Relative acidity: HOCH3 < HOI < HOBr < HOCl
As the series is read from left to right, the electronegativity of element X in H–O–X is increasing.
