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ANALYTICAL CHEMISTRY C3 > Chapter 16: Introduction to Electrochemistry > Flashcards

Chapter 16: Introduction to Electrochemistry Flashcards

1
Q

sometimes called redox reactions

A

oxidation/ reduction reactions

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2
Q

is an electron donor

A

reducing agent

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3
Q

is an electron acceptor

A

oxidizing agents

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4
Q

A substance that has a strong affinity for electrons

A

oxidizing agent

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5
Q

donates electrons to another species

A

reducing agent

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6
Q

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

A

Bronsted Lowry concept

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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

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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

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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

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10
Q

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

A

salt bridge

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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

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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

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13
Q

voltmeter measures what

A

potential difference or voltage, between two electrodes ar any instant

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14
Q

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

A

voltage

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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

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16
Q

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

A

cells without liquid junction

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17
Q

is an electrode where
reduction occurs

A

cathode

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18
Q

electrode where oxidation occurs

A

anode

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19
Q

An electrochemical cell consists of two conductors called

A

electrodes

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20
Q

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

A

TRUE

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.

A

batteries

24
Q

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

A

TRUE

25
Q

Galvanic cells operate spontaneously, and the net reaction during discharge is called the

A

spontaneous cell reaction

26
Q

In this cell, reversing the current reverses the cell
reaction when the direction of flo is changed

A

reversible cell

27
Q

In this cell, reversing the current causes a
different half-reaction to occur at one or both of the electrodes.

A

irreversible cell

28
Q

was one of the earliest galvanic cells to find widespread practical application

A

Daneill gravity cell

29
Q

The phase boundary between an
electrode and its solution is called an

A

interface

30
Q

If the reactants and products are in their standard states, the resulting cell potential is called the

A

standard cell potential

31
Q

is a reference state that allows
to obtain relative values of such
thermodynamic quantities as free
energy, activity, enthalpy, and
entropy. All substances

A

standard state

32
Q

formula of delta G

A

delta G= -nFEcell =-RTln Keq

33
Q

requires an external source of electrical energy for operation

A

electrolytic cell

34
Q

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

A

standard hydrogen electrode

35
Q

The standard hydrogen electrode
is sometimes called the

A

normal hydrogen electrode

36
Q

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,

A

platinum black

37
Q

TRUE or FALSE
By convention, the potential of
the standard hydrogen electrode is assigned a value of 0.000 V at all temperatures

A

TRUE

38
Q

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.

A

electrode potential

39
Q

is defined as its electrode potential when the activities of the reactants and products are all unity

A

standard electrode potential

40
Q

A metal ion/metal half-cell is
sometimes called a

A

couple

41
Q

is by
definition a reduction potential

A

electrode potential

42
Q

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.

A

oxidation potential

43
Q

TRUE or FALSE
The standard electrode potential for a half-reaction is temperature dependent

A

TRUE

44
Q

The following further complicate application of standard electrode potential data to
many systems of interest in analytical chemistry:

A

association
dissociation
complex formation
solvolysis equilibria

45
Q

are empirical potentials that compensate for the types of activity and competing equilibria effects that we have just described.

A

formal potential

46
Q

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

A

formal potential

47
Q

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

A

formal potential

48
Q

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

A

plus right rule

49
Q

potential of hydrogen electrode depends on

A

temperature
activities of hydrogen ion
molecular hydorgen in the solution

ANALYTICAL CHEMISTRY C3 (21 decks)

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