ELEMENTS FROM THE SEA

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104 Terms

1
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What is the charge of a group 5 ion?

-3

2
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What does NaCl (aqueous) mean?

The Na+ and Cl- are completely separate. The ions are surround by water molecules held by ion-dipole forces.

3
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Formula for hydrogen sulfate ion

HSO4-

4
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Formula for hydrogen carbonate ion

HCO3-

5
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Formula for nitrate ion

NO3-

6
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Formula for nitrite ion

NO2-

7
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Formula for sulfate ion

SO4 2-

8
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Formula for sulfite ion

SO3 2-

9
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Formula for ammonium ion

NH4+

10
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Formula for chromate ion

CrO4 2-

11
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Formula for dichromate ion

Cr2O7 2-

12
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Formula for peroxide ion

O2 2-

13
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Formula for cyanide ion

CN-

14
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Formula for phosphate ion

PO4 3-

15
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Formula for permanganate ion

MnO4-

16
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What is the name of ions that do not take part in a reaction?

Spectator ions

17
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Name the 4 common spectator ion

NO3- / SO4 2- / Na+ / K+

18
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What is a spectator ion?

Ions that do not take part in a reaction

19
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What is a precipitate?

A solid held suspended in a liquid. Formed when 2 ionic solutions are mixed and a double displacement reaction occurs

20
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What is a positively charged ion?

A cation

21
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What is a negatively charged ion?

An anion

22
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Flame colour of Li+

Crimson

23
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Flame colour of Na+

Orange-yellow

24
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Flame colour of K+

Lilac

25
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Flame colour of Ca2+

Brick-red

26
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Flame colour of Ba2+

Green

27
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Flame colour of Cu2+

Blue-green

28
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Describe the test for halides

Add dilute nitric acid, then silver nitrate solution.

29
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How to distinguish between silver halide precipitates?

Add dilute ammonia (NH3) / AgCl dissolves / AgBr partially dissolves / AgI dont dissolve.

30
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Precipitate test for Fe2+ ion (include test result)

Add NaOH, green precipitate forms

31
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Precipitate test for Fe3+ ion (include test result)

Add NaOH, brown precipitate forms

32
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Precipitate test for Cu2+ ion (include test result)

Add NaOH, blue precipitate forms

33
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Test for sulphates (include test results)

Add dilute HCl and barium chloride, white precipitate forms

34
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Test for hydroxide ions (include test results)

Dip red litmus paper into solution, if hydroxide ion is present then the paper will turn blue.

35
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Test for ammonia gas (NH3)

Expose ammonia gas to a piece of damp red litmus paper. If ammonia is present, paper will turn blue.

36
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Test for ammonium ion (NH4+)

NH4+ + OH- —> NH3 + H2O. Then test for ammonia gas

37
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Test for iodide ion (without AgNO3)

Add Pb(NO3)2, bright yellow precipitate forms

38
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What happens to O.S during oxidation

O.S becomes more positive

39
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What happens to O.S during reduction

O.S becomes more negative

40
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What happens to the electrons / oxygen / hydrogen during oxidation?

Electrons are lost / oxygen is gained / hydrogen is lost

41
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What happens to the electrons / oxygen / hydrogen during reduction

Electrons are gained / oxygen is lost / hydrogen is gained

42
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O.S of fluorine is always…

-1

43
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O.S of elements are always…

0

44
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Cl in covalent compounds are usually…

-1

45
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What is the colour of Br2 in water?

Orange

46
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What is the colour of Cl2 in water?

V.pale green / colourless

47
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What is the colour of I2 (iodine) in water?

Orange-brown

48
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What is the colour of F2 (fluorine) in water?

N/A

49
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What is the colour of Br2 in organic solvent?

Orange

50
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What is the colour of Cl2 in organic solvent?

Colourless

51
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What is the colour of I2 (iodine) in organic solvent?

Purple

52
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What is the colour / state of Br2 at RTP?

Liquid / red-brown

53
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What is the colour / state of Cl2 at RTP?

Gas / v.pale green

54
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What is the colour / state of I2 (iodine) at RTP?

Solid / grey-black

55
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Describe a test for displacement reaction between a halogen and halide ion

1cm³ of halogen + 1cm³ of halide solution, shake, + 1cm³ of cyclohexane, shake well

56
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Systematic name for SO4 2-

Sulphate (VI) ion

57
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Systematic name for N2O

Nitrogen (I) oxide

58
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Systematic name for FeCl2

Iron (II) chloride

59
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Systematic name for Mn(OH)2

Manganese (II) hydroxide

60
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Which electrode does oxidation occurs?

The anode

61
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Which electrode does reduction occur?

The cathode

62
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Whats the equation for the oxidation of H2O?

H2O —> ½ O2 + 2e- + 2H+

63
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Whats the equation for the reduction of H2O?

H2O + e- —> ½ H2 + OH-

64
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What can be oxidised at the anode during aqueous electrolysis?

Either halide ions OR H2O

65
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What can be reduced at the cathode during aqueous electrolysis?

Either group 3 / transition metal ions OR H2O

66
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What electrolyte is used during the purification of copper?

CuSO4 (aq) solution (blue)

67
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What is the anode made of? (purification of copper)

Impure copper

68
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What is the cathode made of? (purification of copper)

Pure copper

69
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What happen at the anode? (purification of copper)

Impurities fall / mass decreases

70
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What happens at the cathode? (purification of copper)

Mass of cathode increases as Cu (s) is formed

71
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Equation at the anode (purification of copper)

Cu —> Cu2+ + 2e-

72
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Equation at the cathode (purification of copper)

Cu2+ + 2e- —> Cu (s)

73
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Equation for atom economy (using Mr)

(Mr of useful products / Mr of all reactant) x 100

74
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How can you get 100% atom economy?

All products are useful / if only one product is made (addition rxns) / rearrangement rxns

75
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Equation for %yield

(Actual mass of products / max possible mass of products) x 100

76
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(Main) reasons for a low yield (2)

Transfer losses / reaction may not have gone to completion

77
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Reason for a yield over 100% (1)

Solid (usually organic) may be wet

78
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Explain, in terms of electrons, why a bromine atom is more reactive than an iodine atom

Bromine attracts electrons more (strongly) than iodide

79
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Explain which of chloromethane and bromomethane would undergo hydrolysis more rapidly

Bromomethane, the C-Br bond enthalpy is lower / weaker than the C-Cl bond

80
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What bonds do hydrogen halides have?

Covalent

81
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What does HX (g) in water make?

Acid (solution)

82
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Equation for % yield:

(Actual mass / theoretical mass) x 100

83
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What are the main 2 reasons for low yield?

Transfer losses / Reaction may not have gone to completion

84
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What are the main reasons for yield over 100%

Solid may be wet

85
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What does volatility mean (in halogens)?

How easily something becomes a gas

86
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What is the trend in volatility of the halogens? + give a short reason

Decreases down the group as IMF gets stronger

87
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What are the (2) importance of chlorine

To extract Br2 from seawater / to make bleach, to treat water as it kills bacteria

88
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Which halogen is the best oxidising agent?

F2 is the best as smallest atoms, therefore strongest force of attraction

89
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What are the 3 reactions of halogens? (bullet point it)

  1. Halogen + halide

  2. Halogen + alkene

  3. Halogen + alkane

90
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What type of reaction is halogen + alkane?

Radical substitution

91
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What type of reaction occurs when u heat hydrogen halides?

Thermal decomposition

92
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Write an balanced equation of what happens when you heat HX (hydrogen halide)

2HX → H2 + X2

93
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Which hydrogen halide is the easiest to decompose? (just state)

HI

94
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What is the trend of thermal stability of hydrogen halides?

Decreases down the group

95
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Why is H-I the weakest covalent bond in comparison to other hydrogen halides?

Iodine is the largest halogen atom / the shared e- are further from the nucleus

96
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Charge density is only valid for what type of particle?

Ions

97
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What molecule is used to test for HX (g)? (include state symbols)

NH3(g)

98
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What are the observations of heating HBr? and why?

Orange-brown gas / Br(g) produced

99
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What are the observations of heating HI? and why?

Purple gas / I2(g) produced

100
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What is the general equation for MAKING hydrogen halides? include state symbols

NaX(s) + c.H2SO4(aq) → NaHSO4(aq) + HX(g)