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(Green) redox Flashcards

(Green) redox

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1
Q

CuO + H2 —-> H2O + Cu

Which substance is being oxidised
Which substance is being reduced
Explain why

A

Which substance is being oxidised? H

Which substance is being reduced? CuO

Explain why gained an O atom

Explain why lost an O atom

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2
Q

give the definitions of oxidation and reduction

A

OXIDATION is when a species LOSES one or more ELECTRONS

REDUCTION is when a species GAINS one or more ELECTRONS

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3
Q

describe what oxidation involves

A

increase in oxidation number
loss of electrons
gain of oxygen or loss of hydrogen

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4
Q

describe what reduction involves

A

decrease in oxidation number
gain of electrons
loss of oxygen or gain of hydrogen

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5
Q

what is the definition of redox

A

A chemical reaction that takes place between an oxidizing substance and a reducing substance. The oxidizing substance loses electrons in the reaction, and the reducing substance gains electrons.

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6
Q

is glucose a reducing agent or oxidising agent

A

reducing agent , remember there reducing sugers

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7
Q

what is the definition of oxidation number

A

Oxidation Number is the charge the species in a molecule or ion would have if the bonding was 100% ionic.

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8
Q

info card (read and recite)

A

1) Elements in their uncombined state have an oxidation number of zero.

2) The sum of all the oxidation numbers in an uncharged molecule is zero.

3) The sum of all the oxidation numbers in an ion is the charge on the ion.

4) The oxidation number of hydrogen is +1 except in metal hydrides when it is -1.

5) Being the most electronegative element, fluorine (unlike the other halogens) always has the oxidation number -1, and can bring out the highest oxidation number in any element it reacts with.

6) The oxidation number of oxygen is -2 apart from in compounds with fluorine or in peroxides (-1).

7) The oxidation number of chlorine is -1 apart from in compounds with fluorine or oxygen

8).The oxidation number of all the group one and two metals is +1 and +2 respectively.

9) In any combination of two elements, the more electronegative one has the negative oxidation number.

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9
Q

what is the oxidation number of :
Ba in BaCl2

A

+2

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10
Q

what is the oxidation number of :
Li in Li2O

A

+1

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11
Q

what is the oxidation number of :
P in P2O5

A

+5

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12
Q

what is the oxidation number of :
P in P2O3

A

+3

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13
Q

what is the oxidation number of :
C in CO

A

+2

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14
Q

what is the oxidation number of :
I in I2

A

0

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15
Q

what is the oxidation number of :
C in CCl4

A

+4

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16
Q

what is the oxidation number of :
I in I-

A

-1

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17
Q

what is the oxidation number of :
Cr in CrO4-2

A

+6

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18
Q

what is the oxidation number of :
P in PO43-

A

+5

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19
Q

what is the oxidation number of :
Cr in Cr2O72-

A

+6

20
Q

what is the oxidation number of :
O in H2O2

A

-1

21
Q

what is the oxidation number of :
Mn in MnO2

A

+4

22
Q

what is the oxidation number of :
Xe in XeF4

A

+4

23
Q

what is the oxidation number of :
N in NH3

A

-3

24
Q

what is the oxidation number of :
N in N2O4

A

+4

25
Q

what is the oxidation number of :
H in LiH

A

-1

26
Q

what is the oxidation number of :
S in Na2S4O6

A

+2.5

27
Q

What is the problem with the oxidation number of sulfur in Na2S4O6?

A

S has an oxidation number of +2.5, cannot have ½ electron! But this method works for electron counting purposes

28
Q

what is the definition of Disproportionation

A

Disproportionation is the simultaneous oxidation and reduction of atoms of the same element

29
Q

what is the oxi state and colour of MnO4-

A

purple
+7

30
Q

what is the oxi state and colour of MnO4 2-

A

green
+6

31
Q

what is the oxi state and colour of MnO2

A

brown
+4

32
Q

what is the oxi state and colour of Mn2+

A

very pale pink
+2

33
Q

what is the colour of Cu 2+

A

pale blue

34
Q

what are the observations of adding CuSO4
to Chloride ions and starch

A

solution remained pale blue

35
Q

what are the observations of adding CuSO4
to Bromide ions and starch

A

solution remained pale blue

36
Q

what are the observations of adding CuSO4
to Iodide ions and starch

A

solution turned brown. When starch added it turned blue/black

37
Q

what observations do you see when adding Fe2+
to hydroxide ions

A

pale green ppt. starts to turn brown with time Fe(OH)2(s)

38
Q

what observations do you see when adding Fe2+
to Thiocyanate (SCN-)

A

No change (turned slightly pink with time)

39
Q

what observations do you see when adding Fe2+
to Iodide (I-)

A

No change

40
Q

what observations do you see when adding Fe2+
to Manganate (MnO4-)

A

pale pink/slight brown ppt REDOX

41
Q

what observations do you see when adding Fe2+
to Silver Ag+

A

sparkly particles appeared Ag(s) REDOX

42
Q

what observations do you see when adding Fe3+
to OH-

A

Red/brown ppt. Fe(OH)3(s)

43
Q

what observations do you see when adding Fe3+
to Thiocyanate SCN-

A

Blood red solution Fe(SCN)3(s)

44
Q

what observations do you see when adding Fe3+
to Iodide I-

A

orange solution I2 turned black with starch REDOX

45
Q

what observations do you see when adding Fe3+
to Manganate MnO4-

A

No change

46
Q

what observations do you see when adding Fe3+
to Silver (Ag+)

A

No change

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