Brainscape's Knowledge GenomeTM

Browse over 1 million classes created by top students, professors, publishers, and experts.


See full index

chemistry > Redox 1 > Flashcards

Redox 1 Flashcards

1
Q

What is an oxidation number?

A

The number of electrons an atom uses to bond with any other atom

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

What is the oxidation number of an uncombined element such as C, H, O2?

A

0

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

What is the oxidation number of combined oxygen such as in H2O?

A

-2

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

Oxidation number of oxygen in peroxides

A

-1

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

What is the oxidation number of combined hydrogen such as in NH3, H2S

A

+1

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

What is the oxidation number of combined hydrogen such as in metal hydrides, LiH

A

-1

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

Oxidation number of a simple ion

A

Charge on the ion.
Na=+1
Cl=-1

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

What is the oxidation numberNof combined fluorine such as in NaF, CaF2

A

-1

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

When an element has more than one stable oxidation number how is it indicated?

A

Written as a roman numeral

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

What is the oxidation number of Fe in iron (Ill) chloride?

A

+3

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

What are oxyanions

A

Negative ions that have an element along with oxygen

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

Oxidation number of S in SO4 2-

A

+6
Because, combined oxygen has an oxidation number of -2.
4 X-2 =-8.
The charge on the compound is -2. Sum of oxidation numbers must
equal -2
SO, -2-(-8) = +6

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

Define oxidation in terms of electron transfer and oxidation number

A

Oxidation is
- loss of electrons
- increase in oxidation number

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

Define reduction in terms of electron transfer and oxidation number

A

Reduction is
-gain of electrons
- decreased oxidation number

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

What is a redox reaction

A

A reaction where both oxidation and reduction take place

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

Oxidation number of a metal

A

0 because it is an element

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

What is an oxidising agent

A

Species that gains electrons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

What is a reducing agent

A

Species that loses electrons

19
Q

Oxidation state of chlorine in NaClO

A

+1

20
Q

Define disproportionation

A

same species undergoes oxidation and reduction simultaneously

21
Q

Ocidation state of P in PCl5

A

+5

22
Q

Oxidation state of nitrogen in ammonia

A

+3

23
Q

Oxidation state of arsenic in AsO4 3-

A

+5

24
Q

Oxidation state of iron in K4Fe(Cn)6

A

2+

25
Q

6 type of ionic equations

A

Dissociation into ions
Displacement reactions
Redox
Metal reacts with acid
Neutralisation
Precipitation

26
Q

What is dissociation

A

Particles in a substance spread out when heated or dissolved

27
Q

Ionic compounds are always ….. but ……. In water

A

Solid
Dissolve

28
Q

Ionic equation for barium chloride dissociation into ions

A

BaCl2(aq)+aq—> Ba2+(aq) + 2Cl-(aq)

29
Q

Ionic equation of magnesium and copper sulfate displacement reaction

A

Mg(s) + CuSO4(aq)—> MgSO4 (aq) + Cu(s)
Mg(s) + Cu2+(aq)—> Mg2+ + Cu(s)

30
Q

Ionic equation of sodium chloride and silver nitrite redox reaction

A

NaCl(aq) + AgNO3(aq)—> NaNO3 (aq) + AgCl(s)
Cl- + Ag+ —> AgCl(s)

31
Q

Ionic equation of magnesium and sulfuric acid metal reacts with acid

A

Mg(s) + 2H+ —> Mg2+(aq) + H2(g)

32
Q

Ionic equation sodium hydroxide and sulfuric acid neutralisation

A

2OH-(aq) + 2H+ —> 2H2O(l)

33
Q

Ionic equation of lead nitrate and potassium iodide precipitation reaction

A

Pb2+(aq) + 2I- —> PbI2(s)

34
Q

Oxidation agent

A

Species that accepts electrons, undergoes reduction

35
Q

Reducing agent

A

Gives away electrons, undergoes oxidation

36
Q

Oxidation number rules

A

Uncombined elements=0
Ions made of just one atom = charge on the ion
Sum of all oxidation states in a compound= 0
Sum of oxidation states of a complex ion = charge on ion

37
Q

Acids we must know

A

HCl hydrochloric acid
H2SO4 sulfuric acid
HNO3 nitric acid

38
Q

Alkalis we must know

A

NaOH
KOH
Ca(OH)2

39
Q

What is disproportionation reaction

A

Same species is oxidised and reduced at the same time

40
Q

Oxidation state of iron in Fe2O3

A

+3

41
Q

Oxidation state of chromium in Cr2O7 2-

A

+6

42
Q

Balance this redox reaction
H2SO4–>H2S

A

H2SO4 + 8e- + 8H+ —>H2S + 4H20

43
Q

Balance this redox reaction
NO3 - —> NO2

A

NO3- + 2H+ +e- —> NO2 + H2O

chemistry (7 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2024 Bold Learning Solutions. Terms and Conditions