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Chem 23 > Redox Titration > Flashcards

Redox Titration Flashcards

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1
Q

It is a number assigned to an element in a compound which enables us to describe oxidation-reduction reactions and balancing redox chemical reactions.

A

Oxidation state

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2
Q

most common source of error; caused by resistance to the flow of charge at a boundary

A

junction potential

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3
Q

It consumes electrical energy from an external source, using it to cause a nonspontaneous redox reaction to occur ( ΔG>0 ).

A

Electrolytic cell

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4
Q

These are shown by single vertical lines

A

Phase boundaries

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5
Q

The _______________ is the substance that loses electrons and is oxidized in the process

A

reductant

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6
Q

The reaction of gaseous hydrogen chloride and iron oxide is a __________________________

A

double replacement reaction

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7
Q

energy released by spontaneous redox reaction is converted to electrical energy

A

galvanic cell

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8
Q

It relates the potential, E, to the standard electrode potential, E⁰ by the following equation

A

Nernst equation

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9
Q

Oxidation state enables us to describe __________________ and _____________________.

A

oxidation-reduction reactions, balancing redox chemical reactions

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10
Q

The oxidation number of a monatomic (composed of one atom) ion is the same as the ________ of the ion

A

charge

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11
Q

It is considered to be any element in an uncombined state, whether monatomic or polyatomic.

A

free element

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12
Q

There is no net change in the number of electrons in a

A

redox reaction

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13
Q

In molecular compounds, the names are given which refer to the ________________ present in the compound.

A

number of molecules

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14
Q

An ________________________ is any chemical reaction in which the oxidation number of a molecule, atom, or ion changes by gaining or losing an electron.

A

oxidation-reduction reaction

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15
Q

In ionic compounds, the names are given which refer to the ___________________.

A

oxidation (ionic) state

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16
Q

It uses the energy released during a spontaneous redox reaction (ΔG<0) to generate electricity.

A

Galvanic (voltaic) cell

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17
Q

electrical energy is used to drive nonspontaneous redox reaction

A

electrolytic cell

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18
Q

ΔG < 0

A

reaction can spontaneously proceed to the right

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19
Q

reduced, accepts electrons, oxidation number decreases

A

oxidizing agent

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20
Q

In ionic and covalent molecular compounds, usually the ____________________ element is given first.

A

less electronegative

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21
Q

OIL RIG

A

“oxidation is loss” and “reduction is gain,“

22
Q

LEO says GER

A

“loss of e- = oxidation” and “gain of e- = reduced.”

23
Q

When the circuit is closed, electrons flow from the _________ to the ____________

A

anode, cathode

24
Q

____________________ have some practical significance in everyday life, including the reaction of hydrogen peroxide, H2O2 poured over a cut.

A

Disproportionation reactions

25
Q

In a neutral molecule, the sum of the oxidation numbers of all atoms is _______

A

zero

26
Q

A redox reaction can be described as ____________________, one representing the oxidation process and one the reduction process.

A

two half-reactions

27
Q

In ______________________ the names are given which refer to the oxidation (ionic) state.

A

ionic compounds

28
Q

ΔG > 0

A

reaction can spontaneously proceed to the left

29
Q

It is an apparatus that is used to generate electricity from a spontaneous redox reaction or, conversely, that uses electricity to drive a nonspontaneous redox reaction

A

Electrochemical cell

30
Q

it is where reduction half-reaction occurs

A

cathode

31
Q

it is where oxidation half-reaction occurs

A

anode

32
Q

Oxidation-Reduction Reaction comprised of two parts

A
  1. reduced half
  2. oxidized half
33
Q

There is no ___________ in the number of electrons in a redox reaction.

A

net change

34
Q

The ___________ of the cell, measured in volts, is the difference in electrical potential between the two half-reactions and is related to the energy needed to move a charged particle in an electric field.

A

potential

35
Q

“Red Cat An Ox”

A

Reduction in cathode; Oxidation in anode

36
Q

the _____________ is the species that gains electrons and is reduced in the process

A

oxidant

37
Q

The oxidation number of an atom in a neutral free element is __________.

A

zero

38
Q

It is the movement of an electron from one atom to another.

A

Electron transfer

39
Q

In ___________________, the names are given which refer to the number of molecules present in the compound.

A

molecular compounds

40
Q

Both types contain _________________, which are solid metals connected to an external circuit that provides an electrical connection between the two parts of the system.

A

two electrodes

41
Q

Phase boundaries are shown by?

A

single vertical lines

42
Q

charge an atom would possess if the bonding were ionic

A

oxidation state

43
Q

This does not need to begin with neutral molecules and can involve more than two species with differing oxidation states (but rarely).

A

Disproportionation reactions

44
Q

The identity of the electrodes and the chemical contents of the compartments are indicated by their chemical formulas, with the anode written on the far ____ and the cathode on the far _____.

A

left, right

45
Q

ΔG = 0

A

the reaction is at equilibrium

46
Q

It is a useful tool for keeping track of electron transfers especially for transition metals.

A

Oxidation state

47
Q

single substance can be both oxidized and reduced in some redox reactions. These are known as ________________________________

A

disproportionation reactions

48
Q

The associated ______________________ is determined by the potential difference between the valence electrons in atoms of different elements.

A

potential energy

49
Q

oxidized, donates electrons, oxidation number increases

A

reducing agent

50
Q

charge that results when the electrons in a covalent bond are assigned to the more electronegative atom

A

oxidation state

Chem 23 (7 decks)

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