Oxidation-reduction Flashcards

1
Q

Reduces other species by losing electrons

A

reducing agent

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2
Q

Oxidizes other species by gaining electrons

A

oxidizing agent

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3
Q

Common oxidizing agents are __, __, __ and _____, which favor gaining an electron to have a full octet

A

O2, O3, H2SO4, halogens

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4
Q

Common reducing agents are __, __, __ and ___ __ which favor losing an electron to have a full octet

A

H2, Fe, Zn, alkali metals

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5
Q

the total number of electrons that an atoms gains or loses electrons when a bond is formed

A

oxidation states

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6
Q

atoms in their ___ ___ have an oxidation number of zero. Oxidation numbers for atoms in ____ ___ are equal to their charge. __ is always assigned an oxidation number of -1, oxygen is often ___, and hydrogen is usually ___

A

elemental state, monoatomic ions, fluorine, +2, +1

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7
Q

__ ___ often have an oxidation number of +1, and ___ __ ____ often have an oxidation number of +2

A

alkali metals, alkaline earth metals

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8
Q

Exceptions are, if oxygen is in a ___, (___), it’s oxidation number is -1. If oxygen is bonded to fluorine the oxidation number of oxygen is ____. If hydrogen is part of a __ ___, the oxidation number is ____

A

peroxide, H2O2, +1, metal hydride, -1

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9
Q

To balance the redox reaction under acidic conditions, each ___ reaction must be written and firstly all atoms must be balanced other than __ and ___. Then balance the number of oxygen atoms by adding the same number of __ molecules to the opposite side. Balance the hydrogen atoms by adding __ to the opposite side. Balance the charges by adding ____. Multiply the equations to make sure each half reaction has the same number of ___, then add them together and cancel common terms

A

half, oxygen hydrogen, H2O, H+, electrons, electrons

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10
Q

In basic reactions the H+ must be balanced with ___ and then combined to create ____.

A

OH-, H2O

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11
Q

Electrochemical cells convert ___ energy to ___ energy or vice versa using __ __ and the movement of ___

A

chemical energy, electrical, redox reactions, electrons

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12
Q

Electrons always flow from the ___ to the ___

A

anode, cathode

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13
Q

energy produced from chemical reactions from energy stored in the bonds of atoms and molecules

A

chemical energy

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14
Q

energy produced from the flow of electrons

A

electrical energy

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15
Q

a cell that is spontaneous like a battery

A

galvanic (voltaic) cell

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16
Q

a non spontaneous cell like a rechargeable battery

A

electrolytic cell

17
Q

In a galvanic cell, due to a chemical reaction in the battery ____, the __ builds up an excess of ___. Then electrons flow from the __ to the ___ spontaneously through the wire to produce ___. This process converts __ energy to ___ energy

A

electrolyte, anode, electrons, anode, cathode, electricity, chemical, electrical

18
Q

Galvanic cells have a delta G ___ 0, the electrons move from the anode (__) to the cathode (__), they turn __ energy to ___ energy, do not require an external __ ___, have oxidation at the __ and reduction at the ___, and have a Ecell __ 0

A

< -, +, chemical, electrical, power source, anode, cathode, >

19
Q

The salt bridge is a tube filled with __ ____. The anions from it flow towards the ____, which balances the increasing cations in the solution, and the ____ from the salt bridge flow to the ____ which balances the decreasing cations in the solution. As the reaction progresses the size of the ____ electrode increases, and the __ electrode decreases

A

nonreactive electrolytes, anode, cations, cathode, copper, zinc

20
Q

Spontaneous redox reactions ___ electrons released by the anode, causing the battery to __ __ and not produce electricity

A

deplete, lose power

21
Q

Electrolytic cells use a __ __ to force electrons to flow ___ in order to ensure the battery can be fully charged

A

power source, non spontaneously

22
Q

In electrolytic cells, the delta g is __ 0, the electrons flow from the anode (__) to the cathode (__). ____ energy is converted to ____ energy, it requires an external __ __, oxidation is at the __, and reduction is at the ____, and the Ecell is __ 0

A

> , +, =, electrical, chemical, power source, anode, cathode, <

23
Q

a porous barrier is a barrier that allows for the flow of __ and ___ charges like a salt bridge. The use of one is dependent on the design and not always ___

A

ions, neutralizes, necessary

24
Q

When a power source forces the nonspontaneous movement of electrons to the cathode

A

molten electrolysis

25
Q

In ____ one metal is plated with another to cover it in a thin layer. The metal being plated is made into the ___ and is the site of____

A

electroplating, cathode, reduction

26
Q

The sum of the oxidation potential and reduction potential measured in voltage

A

Ecell

27
Q

If Ecell __ 0, the cell is spontaneous. if Ecell is ___ 0 the cell is non spontaneous

A

> , <

28
Q

Reduction potentials that are greater and more negative are stronger __ ___, weaker __ __, and want to __ electrons

A

reducing agents, oxidizing agents, lose

29
Q

The moles of the product formed in electroplating is given by ____

A

I (current) (time)/number of moles of electrons transferred (F)

30
Q

To find the change in free energy and cell potential, the following equation is used ___

A

delta G = -nFE