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AEC > Redox I > Flashcards

Redox I Flashcards

1
Q

Oxidation

A

When a species loses one or more electron

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2
Q

Reduction

A

When a species gains one or more electrons

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3
Q

Oxidation number

A

Charge that the element would have if the compounds were fully ionic

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4
Q

Disproportionation

A

Redox reaction in which an element in a single species is simultaneously oxidised and reduced.

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5
Q

A redox reaction involves

A

both reduction and oxidations

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6
Q

Give everyday examples of oxidation

A

burning of fuels
Rusting of ions
Bleaching of dyes

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7
Q

Give everyday example of reduction

A

extraction of metals

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8
Q

In a redox reaction, the oxidising agents

A

a species that oxidises another species by removing one or more electrons but itself is reduced

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9
Q

In a redox reaction, the reducing agents

A

a species that reduces another species by giving it one or more electrons but itself is oxidised

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10
Q

For the oxidising agent Cl 2, what is produced when reduced.

A

Cl -

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11
Q

For the oxidising agent Br2, what is produced when reduced.

A

Br -

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12
Q

For the oxidising agent MnO 4-, what is produced when reduced.

A

Mn 2+

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13
Q

For the oxidising agent Cr2O7 2-, what is produced when reduced.

A

Cr 3+

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14
Q

For the oxidising agent H2O2, what is produced when reduced.

A

H2O

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15
Q

For the oxidising agent Fe 3+, what is produced when reduced.

A

Fe 2+

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16
Q

For the oxidising agent H2SO4, what is produced when reduced.

A

SO 2

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17
Q

For the oxidising agent HNO3, what is produced when reduced.

A

NO 2

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18
Q

For the oxidising agent H+ in dilute acids , what is produced when reduced.

A

H 2

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19
Q

For the reducing agent. I- / HI, what is the product when oxidised?

A

I 2

20
Q

For the reducing agent H2S, what is the product when oxidised?

A

S

21
Q

For the reducing agent SO2, what is the product when oxidised?

A

SO4. 2-

22
Q

For the reducing agent Fe 2+, what is the product when oxidised?

A

Fe 3+

23
Q

For the reducing agent H2O2, what is the product when oxidised?

A

0

24
Q

For the reducing agent Sn 2+Tin, what is the product when oxidised?

A

Sn 4+

25
Q

For the reducing agent Carbon , what is the product when oxidised?

A

carbon monoxide or carbon dioxide

26
Q

How does an ionic equation show chemical change?

A

by showing only the reacting ions and any other reacting atoms or molecules whilst leaving out the spectator ions

27
Q

What is a half equation?

A

An ionic equations used to describe either the gain or loss of electrons during a relic reaction

28
Q

What are oxidation numbers calculated on the basis of?

A

that bonding electrons are assigned to the more electronegative atom in covalent bond

29
Q

The ionic half equations can be combined to give

A

full ionic equations

30
Q

When writing a half equation for oxidation…

A

the electrons are seen on the RHS

31
Q

When writing a half equation for reduction…

A

the electrons are seen on the LHS

32
Q

When writing a half equation for complex compounds… what are some rules

A

“If reaction takes place in acid solution add H+ ions (LHS) + H20 (RHS)
Balance atoms followed by charge to become neutral”

33
Q

What is the oxidation number of uncombined elements ?

A

ZERO

34
Q

What is the oxidation number for monatomic ions?

A

charge on the ion

35
Q

What is the oxidation number for group 1 metals?

A

1+

36
Q

What is the oxidation number for group 2 metals?

A

2+

37
Q

What is the oxidation number for Fluorine?

A

1-

38
Q

What is the oxidation number for Hydrogen?

A

1+

39
Q

What is the oxidation number for Hydrogen combined with a metal ?

A

1-

40
Q

What is the oxidation number for oxygen ?

A

2-

41
Q

What is the oxidation number for oxygen in peroxide or superoxides?

A

depends

42
Q

What is the sum of oxidation numbers in a neutral compound?

A

zero

43
Q

What is the sum of oxidation numbers in a polyatomic ion?

A

1-

44
Q

Do all elements have fixed oxidation numbers?

A

no only some

45
Q

How do metal elements form positive ions?

A

when their atoms react by loss of electrons with an increase in oxidation number

46
Q

How do non-metal elements form negative ions ? The

A

when their atoms or molecules react by gain of electrons with a decrease in oxidation numbers

47
Q

How are compounds of an element classified?

A

Into oxidation states

AEC (19 decks)

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