CH1 Flashcards

1
Q

Definition of Redox reaction

A

A chemical reaction where oxidation and reduction occur at the same time

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2
Q

Reduction in term of Oxygen

A

Loses oxygen

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3
Q

Reduction in term of Hydrogen

A

gain hydrogen

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4
Q

Reduction in term of Oxidation number

A

Oxidation number decrease

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5
Q

Reduction in term of electron transfer

A

Gain electrons

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6
Q

Oxidation in term of Oxygen

A

Gains oxygen

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7
Q

Oxidation in term of Hydrogen

A

Loses hydrogen

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8
Q

Oxidation in term of Oxidation number

A

Oxidation number increases

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9
Q

Oxidation in term of electron transfer

A

loses electron

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10
Q

Oxidation number of Oxygen in peroxides

A

-1

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11
Q

Oxidation number of hydrogen in hydrides

A

-1

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12
Q

Electrochemical series

A

K Ca Na Mg Al Zn Fe Sn Pb H Cu Ag Au

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13
Q

5 Oxidising Agent

A

Acidified Potassium Manganate (VII)
Acidified Potassium Dichromate (VI)
Acidified Hydrogen Peroxide
Chlorine Water
Bromine Water

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14
Q

1 Famous Reducing agent

A

Reactive metals

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15
Q

Color of aqueous Chlorine

A

Pale Yellow

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16
Q

Color of aqueous Bromine

A

Brown

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17
Q

Color of aqueous Iodine

A

Brown

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18
Q

Color of in Chlorine 1,1,1-trichloroethane layer

A

Colourless

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19
Q

Color of in bromine 1,1,1-trichloroethane layer

A

brown

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20
Q

Color of in iodine 1,1,1-trichloroethane layer

A

Purple

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21
Q

Describe a chemical test to identify halogens

A

add 2cm3 of 1,1,1-trichloroethane to the test tube and shake gently.

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22
Q

Definition of electrode potential

A

Potential difference produced when an equilibrium is established between metal M and the aqueous solution containing metal Mn+ ions in a half cell.

23
Q

Ion concentration at standard condition

A

1.0 mol dm-3

24
Q

Gas pressure at standard condition

A

1 atm / 101kPa

25
Q

temperature at standard condition

A

25c

26
Q

Non metal inert electrode at standard condition

A

Platinum

27
Q

Comparison between a larger and smaller standard electrode potential value

A

Element with larger E value is a stronger oxidising agent than with smaller E value
Ion of Element with larger E value has a greater tendency to receive electron to form atom
Ion of Element with larger E value undergoes reduction

28
Q

Definition of electrolytes

A

Substances that can conduct electricity in either molten state or aqueous solution and undergoes chemical changes

29
Q

Definition of Non-electrolytes

A

Substances that cannot conduct electricity in any state

30
Q

An example of Non-electrolytes

A

Covalent compounds

31
Q

2 examples of electrolytes

A

Ionic compounds in molten state
Acid & Alkali in presence of water

32
Q

Particle that conduct electricity in an electrolyte

A

Ions

33
Q

Subatomic particles that conduct electricity in a conductor

A

Electrons

34
Q

Definition of electrolysis

A

A process whereby compounds in the molten state or aqueous solution decompose into their constituent elements by passing electricity trough them.

35
Q

Change of energy on electrolytic cells

A

Electrical energy -> chemical energy

36
Q

Change of energy in voltaic cells

A

Chemical energy -> electrical energy

37
Q

Flow of cation in an electrolytic cells when electric current is passed trough

A

To cathode

38
Q

Flow of antion in an electrolytic cells when electric current is passed trough

A

To Anode

39
Q

Effect of more negative or less positive E0 value on electrolysis at anode

A

Anions easier to release electrons and be oxidised

40
Q

Effect of less negative or more positive E0 value on electrolysis at cathode

A

Cations easier to receive electrons and be reduced

41
Q

Effect of higher halide ions concentration on electrolysis at anode

A

Halide ions easier to release electrons and be oxidised

42
Q

Effect of active electrodes on electrolysis at anode

A

No anions are discharged
Metal atoms at the anode releases electrons to form metal ions

43
Q

Explain electroplating of metals through electrolysis

A

Electroplated object-cathode
Electroplating metal-anode
Electroplating metal ions-Electrolytes aqueous solution

44
Q

Extraction method for metals more reactive than carbon

A

Electrolysis

45
Q

Extraction method for metals less reactive than carbon

A

Reduction by carbon

46
Q

Extraction method for non reactive metals

A

No method. Exists as metal elements

47
Q

Explain extraction of Aluminium

A

Extracted through electrolysis
Aluminium ore or Bauxite is purified into Aluminium oxide
Aluminium Oxide is melted down with cryolite to lower its melting point
Oxide ion oxidised at Anode
Aluminium Ion reduced at Cathode

48
Q

Redox at Anode

A

Oxidation

48
Q

Redox at cathode

A

Reduction

49
Q

Explain extraction of Iron

A

Extracted through reduction by carbon
Iron ore (hematite), limestone and coke is heated up in a blast furnace

C + O2 -> CO2
C + CO2 -> 2CO

Coke, C and Carbon Monoxide reduce Iron (iii) Oxide to Molten iron ( and produces carbon dioxide)

50
Q

Explain extraction using more reactive metal

A

When heated together, more reactive metal reduces less reactive metal from its metal oxide
Metals are produced in molten state due to large amounts of heat released

51
Q

Definition of metal corrosion

A

Redox reaction when metal is oxidised spontaneuosly when metal atoms release electrons to form metal ions

52
Q

Relation between electropositivity of metal and tendency to corrode

A

More electropositive, more easier to corrode//rust

53
Q
A