Chapter 16: Introduction to Electrochemistry Flashcards

1
Q

sometimes called redox reactions

A

oxidation/ reduction reactions

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

is an electron donor

A

reducing agent

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

is an electron acceptor

A

oxidizing agents

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

A substance that has a strong affinity for electrons

A

oxidizing agent

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

donates electrons to another species

A

reducing agent

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

Oxidation/reduction reactions can be viewed in a way that is analogous to the

A

Bronsted Lowry concept

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

TRUE or FALSE
When an acid donates a proton, it becomes a conjugate base that is capable of accepting a proton

A

TRUE

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

TRUE or FALSE
when a reducing agent donates an electron, it becomes an oxidizing agent
that can then accept an electron.

A

TRUE

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

unique aspect of oxidation/reduction reactions is that the transfer of electrons— and thus an identical net reaction—can often be brought about in an ______ in which the oxidizing agent and the reducing agent are physically separated from one another

A

electrochemical cell

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

isolates the reactants but maintains electrical contact between the two halves of the cell.

A

salt bridge

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

When a voltmeter of high internal resistance is connected as shown or the electrodes
are not connected externally, the cell is said to be at _______ and delivers the full cell potential

A

open circuit

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

When the circuit is open, no net reaction occurs in the cell, although we shall show that the cell has the ________ for doing work

A

potential

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

voltmeter measures what

A

potential difference or voltage, between two electrodes ar any instant

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

is a measure of the tendency of the cell reaction to proceed toward equilibrium.

A

voltage

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

TRUE or FALSE
A cell with zero voltage does not
perform work, as anyone who has found a “dead” battery in a flashlight or in a laptop
computer can attest.

A

TRUE

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

The electrodes in some cells share a
common electrolyte; these are known
as

A

cells without liquid junction

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

is an electrode where
reduction occurs

A

cathode

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

electrode where oxidation occurs

A

anode

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q

An electrochemical cell consists of two conductors called

A

electrodes

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
20
Q

TRUE or FALSE
The most common way of avoiding mixing is to insert a salt bridge, between solutions

21
Q

stores electrical energy or also known as voltaic cells

A

galvanic cells

22
Q

consume electricity

A

electrolytic cells

23
Q

are usually made from several such cells connected in series to produce higher voltages than a single cell can produce.

24
Q

TRUE or FALSE
There is a liquid junction potential at each interface of cell notation

25
Galvanic cells operate spontaneously, and the net reaction during discharge is called the
spontaneous cell reaction
26
In this cell, reversing the current reverses the cell reaction when the direction of flo is changed
reversible cell
27
In this cell, reversing the current causes a different half-reaction to occur at one or both of the electrodes.
irreversible cell
28
was one of the earliest galvanic cells to find widespread practical application
Daneill gravity cell
29
The phase boundary between an electrode and its solution is called an
interface
30
If the reactants and products are in their standard states, the resulting cell potential is called the
standard cell potential
31
is a reference state that allows to obtain relative values of such thermodynamic quantities as free energy, activity, enthalpy, and entropy. All substances
standard state
32
formula of delta G
delta G= -nFEcell =-RTln Keq
33
requires an external source of electrical energy for operation
electrolytic cell
34
meets specifications such as an electrode must be easy to construct, reversible, and highly reproducible in its behavior, which has been used throughout the world for many years as a universal reference electrode and is a typical gas electrode
standard hydrogen electrode
35
The standard hydrogen electrode is sometimes called the
normal hydrogen electrode
36
is a layer of finely divided platinum that is formed on the surface of a smooth platinum electrode by electrolytic deposition of the metal from a solution of chloroplatinic acid,
platinum black
37
TRUE or FALSE By convention, the potential of the standard hydrogen electrode is assigned a value of 0.000 V at all temperatures
TRUE
38
is defined as the potential of a cell in which the electrode in question is the right-hand electrode and the standard hydrogen electrode is the left-hand electrode.
electrode potential
39
is defined as its electrode potential when the activities of the reactants and products are all unity
standard electrode potential
40
A metal ion/metal half-cell is sometimes called a
couple
41
is by definition a reduction potential
electrode potential
42
is the potential for the half-reaction written in the opposite way. The sign of an oxidation potential is, therefore, opposite that for a reduction potential, but the magnitude is the same.
oxidation potential
43
TRUE or FALSE The standard electrode potential for a half-reaction is temperature dependent
TRUE
44
The following further complicate application of standard electrode potential data to many systems of interest in analytical chemistry:
association dissociation complex formation solvolysis equilibria
45
are empirical potentials that compensate for the types of activity and competing equilibria effects that we have just described.
formal potential
46
is the electrode potential when the ratio of analytical concentrations of reactants and products of a half-reaction is exactly 1.00 and the molar concentrations of any other solutes are specified
formal potential
47
is the potential of the half-cell with respect to the standard hydrogen electrode measured under conditions such that the ratio of analytical concentrations of reactants and products as they appear in the Nernst equation is exactly unity and the concentrations of other species in the system are all carefully specified
formal potential
48
this rule implies that one should always measure the cell potential by connecting the positive lead of the voltmeter to the right-hand electrode in the schematic or cell drawing and the common, or ground, lead of the voltmeter to the left-hand electrode
plus right rule
49
potential of hydrogen electrode depends on
temperature activities of hydrogen ion molecular hydorgen in the solution