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RUBIDIUM - Rb
Properties Rubidium Rb:
An alkali metal. White, soft, very low melting. The vapor of rubidium is painted in a greenish-blue color. Chemically dissolves in liquid NH3 (dark-blue solution), in the melt RbOH. Extremely reactive, strong reducing agent. Vigorously reacts with oxigen of air, water (there is inflammation of the metal and released hydrogen), dilute acids, non-metals, ammonia, hydrogen sulfide. Does not react with nitrogen. It is well preserved only under a layer of paraffin oil or vaseline. With the mercury forms an amalgam. Colors the flame of a gas burner in a purple color.
Obtaining rubidium Rb:
2RbH = 2Rb + H2 (t > 200° С).
2Rb2O = Rb2O2 + 2 Rb (400-550° С).
RbOH (liquid) → Electrolysis → 4Rb (cathode) + O2↑(anode) + 2 H2O.
2RbCl (liquid) → Electrolysis → 2Rb (cathode) + Cl2↑(anode).
2RbCl + 2 H2O → Electrolysis → H2↑ (cathode) + Cl2↑(anode) + 2 RbOH,
2RbCl(melt)(on Hg-cathode) → Electrolysis → 2Rb (cathode) + Cl2↑ (anode).
Сhemical reactions with rubidium Rb:
2Rb + 2H2O = 2 RbOH + H2↑.
2Rb + 2HCl (diluted) = 2RbCl + H2↑.
8Rb + 6H2SO4 (diluted, cold) = 4 Rb2SO4 + SO2 + S↓ + 6 H2O (impurity H2S).
21Rb + 26HNO3 (diluted, cold) = 21 RbNO3 + NO↑ + N2O↑ + N2↑ + 13 H2O.
2Rb + 2RbOH = 2 Rb2O + H2 (400° С).
2Rb + H2 = 2 RbH (300-350° С, pressure).
Rb + O2 (air) = RbO2 (burning).
4Rb + O2 = 2Rb2O (in the cold),
Rb → + O2 → Rb2O2 → + O2 → time → RbO2↓(-50° С, in the liquid NH3).
4Rb + O2 + 2 H2O = 4 RbOH (normal temp.).
2Rb + E2 = 2RbE (normal temp.; E = F, Cl, Br, I).
2Rb + S = Rb2S (100-130° С).
2Rb + 2 H2S (saturated) = 2 RbHS ↓ + H2↑ (in benzene).
2Rb + 2 NH3 (gas) = 2 RbNH2 + H2 (40-60° С).
Rb + 6 NH3 (liquid) = [Rb(NH3)6] (-40° С),
[Rb(NH3)6] + nNH3 (liquid) ↔ [Rb(NH3)6]+ + e-·nNH3.
4Rb + 3SiO2 = Rb2SiO3 + Si (t > 300° C).
RUBIDIUM SULFIDE Rb2S
Properties Rubidium sulfide Rb2S:
White, melts without decomposition. Thermally stable. Anhydrous powdered Rb2S pyrophoric in dry air. It is readily soluble in water (the strong hydrolysis of anion). Reactive, oxidized in moist air. Decomposed by strong acids. Typical reductant.
Obtaining rubidium sulfide Rb2S:
2 Rb + S = Rb2S (100—130° С).
RbH + Cl2 = RbCl + HCl (400° С),
2 RbH + 2 S = Rb2S + H2S (300—350° С).
Сhemical reactions with rubidium sulfide Rb2S:
Rb2S·4H2O = Rb2S + 4 H2O (200° С, vacuum).
Rb2S (diluted) + 12 H2O = 2 [Rb(H2O)6]+ + S2-, S2- + H2O ↔ HS- + OH-; рКo = 1,09.
Rb2S + 2 HCl = 2 RbCl + H2S ↑.
Rb2S + 3 H2SO4 (conc.) = 2RbHSO4 + SO2 ↑ + S ↓ + 2 H2O.
Rb2S (solution, RbOH) → O2 (air), (time) S (colloid), Rb2(Sn), Rb2SO3S.
Rb2S (solid) + 2 O2 = Rb2SO4 (t>500° C),
Rb2S (solution) + (n - 1)S = Rb2(Sn) (boiling, n = 2, 3, 5).
Rb2S + H2S (saturated) = 2RbHS.
RUBIDIUM CHLORIDE RbCl
Properties Rubidium chloride RbCl:
White, melts and boils without decomposition. Readily soluble in water (without hydrolysis) and concentrated hydrochloric acid. Does not form crystalline hydrates. A weak reducing agent. Participates in exchange reactions.
Obtaining rubidium chloride RbCl:
2Rb + 2HCl(diluted) = 2RbCl + H2↑.
2Rb + E2 = 2RbE(normal temp.; E = F, Cl, Br, I).
RbOH + HCl(diluted) = RbCl + H2O,
Rb2CO3 + 2HCl (diluted) = 2RbCl + CO2 ↑ + H2O.
Rb2SO4 + BaCl2 = BaSO4↓ + 2RbCl
Сhemical reactions with rubidium chloride RbCl:
RbCl(diluted) + 6H2O = [Rb(H2O)6]+ + Cl- (pH 7).
2RbCl(solid) + H2SO4 (conc.) = Rb2SO4 + 2HCl↑ (boiling).
RbCl + RbHSO4 = Rb2SO4 + HCl (500-600°C).
10RbCl (solid) + 8H2SO4 (conc., hot) + 2KMnO4 (solid) = 5Cl2↑ + 2MnSO4 + 5Rb2SO4 + K2SO4 + 8H2O.
2RbCl + H2[SnCl6] = Rb2[SnCl6]↓ + 2HCl (in ethanol).
2RbCl + H2[PtCl6] = Rb2[PtCl6]↓ + 2HCl (in the diluted HCl).
2RbC(liquid) → Electrolysis → 2Rb (cathode) + Cl2↑(on anode).
2RbCl + 2H2O → Electrolysis → H2↑ (cathode) + Cl2↑(on anode) + 2RbOH,
2RbCl(melt, on Hg-cathode) → Electrolysis → 2Rb (on cathode) + Cl2↑(on anode).
RUBIDIUM SULFATE Rb2SO4
Properties Rubidium sulfate Rb2SO4:
White, flying, melts and boils without decomposition. Readily soluble in water (without hydrolysis). Does not form crystalline hydrates. Participates in exchange reactions.
Obtaining rubidium sulfate Rb2SO4:
8 Rb + 6 H2SO4 (diluted, cold) = 4 Rb2SO4 + SO2 + S↓ + 6H2O (impurity H2S).
2 RbCl (solid) + H2SO4(conc.) = Rb2SO4 + 2HCl↑ (boiling).
RbCl + RbHSO4 = Rb2SO4 + HCl (500—600° C).
Rb2S (solid) + 2 O2 = Rb2SO4 (t> 500° С).
Сhemical reactions with rubidium sulfate Rb2SO4:
Rb2SO4 (diluted) + 12 H2O = 2 [Rb(H2O)6]+ + SO42- (pH 7).
Rb2SO4 + H2SO4(conc.) = 2 RbHSO4.
Rb2SO4 + BaE2 = BaSO4↓ + 2 RbE (E = Cl-, OH-).
Rb2SO4 + Al2(SO4)3 + 24 H2O = 2 {RbAl(SO4)2·12H2O}↓ (alum).
RUBIDIUM NITRATE RbNO3
Properties Rubidium nitrate RbNO3:
White, melts without decomposition, decomposes on further heating. Readily soluble in water with high endo-effect (without hydrolysis). Does not form crystalline hydrates. Strong oxidizing agent at sintering. In solution recovered only by atomic hydrogen.
| Molar mass | g/mol | 147.47 |
| Density | g/cm3 | 3.11 |
| Melting point | °C | 313 |
Obtaining rubidium nitrate RbNO3:
21 Rb + 26 HNO3 (diluted, cold) = 21 RbNO3 + NO↑ + N2O↑ + N2↑ + 13 H2O.
RbOH + HNO3 (diluted) = RbNO3 + H2O.
Сhemical reactions with rubidium nitrate RbNO3:
2 RbNO3 = 2 RbNO2 + O2 (540—880° C).
RbNO3 (diluted) + 6 H2O = [Rb(H2O)6]+ + NO3- (pH 7).
RbNO3 (saturated) + (1 - 2) HNO3 (conc.) = RbNO3·(1 - 2)HNO3↓ (normal. temp).
RbNO3 + 2H0(Zn, diluted HCl) = RbNO2 + H2O (boiling),
RbNO3 + 8H0(Zn, conc. NaOH) = NH3 ↑ + 2 H2O + RbOH (boiling).
2 RbNO3 + (NH4)2SO4 = Rb2SO4 + 2N2O + 4 H2O (300-350° C).
RbNO3 + Pb = RbNO2 + PbO (400° C)
RUBIDIUM CARBONATE Rb2CO3
Properties Rubidium carbonate Rb2CO3:
White, during calcination decomposes, melts only pressurized CO2. Sensitive to moisture and CO2 of air. Very soluble in water (strong hydrolysis of the anion), creates a highly alkaline environment. Decomposes by acids. Participates in exchange reactions.
| Molar mass | g/mol | 230.94 |
| Melting point | °C | 873 |
Obtaining rubidium carbonate Rb2CO3:
4 RbO2 + 2CO2(humid) = 2Rb2CO3 + 3O2 (normal temp.),
2 RbO2 + CO = Rb2CO3 + O2 (30-40° C).
2 RbOH (conc.) + CO2 = Rb2CO3 + H2O.
Сhemical reactions with rubidium carbonate Rb2CO3:
Rb2CO3 = Rb2O + CO2 (t>900° C, vacuum).
Rb2CO3·1,5H2O = Rb2CO3 + 1,5H2O (t>190° C).
Rb2CO3(diluted) + 12H2O = 2[Rb(H2O)6]+ + CO32-,
CO32- + H2O ↔ HCO3 - + OH -.
Rb2CO3 + 2HCl (diluted) = 2RbCl + CO2↑ + H2O.
Rb2CO3 + 2HClO4 (conc., cold) = 2RbClO4↓ + CO2↑ + H2O.
Rb2CO3 + H2O + CO2 (170-180° C) ↔ 2RbHCO3.
Rb2CO3 + Ca(OH)2 (saturated) = 2RbOH + CaCO3↓.
RUBIDIUM HYDROXIDE RbOH
Properties Rubidium hydroxide RbOH:
White, thermally stable, melting without decomposition, volatile at a strong heat. Readily soluble in water with a high exo-effect, creates a highly alkaline environment. Exhibits the properties basic hydroxides (refers to alkali), is neutralized by acid, reacts with acidic oxides, oxygen and ozone.
Obtaining rubidium hydroxide RbOH:
2Rb + 2H2O = 2RbOH + H2↑.
4Rb + O2 + 2H2O = 4RbOH (normal temp.).
2RbO2 + H2O = RbOH + RbHO2 (solution) + O2↑ (0° C),
2RbHO2 → (time) → 2RbOH + O2↑ (normal temp.).
4RbO2 + 2 H2O (hot) = 4RbOH + 3O2↑.
Rb2CO3 + Cа(OH)2 (saturated) = 2RbOH + CаCO3↓.
Rb2SO4 + BaE2 = BaSO4↓ + 2RbE (E = Cl-, OH-).
Сhemical reactions with rubidium hydroxide RbOH:
RbOH·2H2O = RbOH·H2O + H2O (47—54° C, vacuum),
RbOH·H2O = RbOH + H2O (300° C,in the stream H2).
RbOH (diluted) + 6 H2O = [Rb(H2O)6]+ + OH-.
RbOH + HCl(diluted) = RbCl + H2O,
2RbOH + H2SO4(diluted) = Rb2SO4 + H2O,
RbOH + HNO3(diluted) = RbNO3 + H2O.
4RbOH (liquid) + 3O2 = 4RbO2 + 2H2O (450° C),
4RbOH + 4O3 = 4RbO3 + O2 + 2H2O (20° C).
2RbOH( conc.) + CO2 = Rb2CO3 + H2O.
RbOH(liquid) → Electrolysis → 4Rb (on cathode) + O2↑(on anode) + 2H2O.
RUBIDIUM OZONIDE RbO3
Properties Rubidium ozonide RbO3:
The orange-red. More stable than the KO3, decomposes when heated. Ion has the structure of (Rb+) (O3-). Reacts vigorously with water, acids, sulfur. It is a strong oxidizing agent.
Obtaining rubidium ozonide RbO3:
RbO2 + O3 = RbO3 + O2 (normal temp.).
4 RbOH + 4O3 = 4 RbO3 + O2 + 2H2O (20° C)
Сhemical reactions with rubidium ozonide RbO3:
2 RbO3 = 2 RbO2 + O2 (60—90° C).
4 RbO3 + 2 H2O = 4RbOH + 5 O2↑ (admixture of radicals OH).
4 RbO3 + 4HCl (diluted, cold) = 4 RbCl + 5O2↑ + 2H2O,
2 RbO3 + 4HCl (diluted, hot) = 2 RbCl + Cl2↑ + 2O2↑ + 2H2O.
4 RbO3 + H2O (moisture) + 3 CO2 = Rb2CO3 + 2 RbHCO3 + 5O2 (normal temp.).
6 RbO3 + 5 S = Rb2SO4 + 2 Rb2S2O7 (40—50° C).
RbO3 + NH3 (liquid) ↔ NH4O3 + RbNH2 (-50° C).
RUBIDIUM SUPEROXIDE RbO2
Properties Rubidium superoxide RbO2:
The orange-yellow. Decomposes when heated, melts under excess pressure of O2. Ion has the structure of (Rb +) (O2-). Reacts vigorously with water, acids, ozone, mono and carbon dioxide, ammonia. It is a strong oxidizing agent.
Obtaining rubidium superoxide RbO2:
Rb + O2 (air) = RbO2 (combustion).
4 Rb + O2 = 2 Rb2O (in the cold), Rb → (O2) Rb2O2 →(O2) , (time) RbO2↓ (-50° C, in the liquid NH3).
4 RbOH (liquid) + 3 O2 = 4 RbO2 + 2 H2O (450° C),
Сhemical reactions with rubidium superoxide RbO2:
RbO2 (-O2)→ (400—800° C) Rb2O2 (-O2)→(t> 1010° C) Rb2O,
2 RbO2 = Rb2O2 + O2 (290° C, vacuum).
2 RbO2 + H2O = RbOH + RbHO2 (solution) + O2↑ (0° C),
2 RbHO2 (solution) →(time) 2 RbOH + O2↑ (normal temp.).
4 RbO2 + 2 H2O (combustion) = 4 RbOH + 3O2↑.
2 RbO2 + 2 HCl (diluted, cold) = 2 RbCl + H2O2 + O2↑.
2 RbO2 + 2 H2SO4 (anhydrous) = 2 RbHSO4 + O3↑ + H2O (normal temp.).
4 RbO2 + 2 CO2 (humid) = 2 Rb2CO3 + 3O2 (normal temp.),
2 RbO2 + CO = Rb2CO3 + O2 (30—40° C).
RbO2 + O3 = RbO3 + O2 (normal temp.).
2 RbO2 + 2 NH3 →(time) 2RbOH + N2 + 2H2O (normal temp.).
RUBIDIUM PEROXIDE Rb2O2
Properties Rubidium peroxide Rb2O2:
White (with a admixture of RbO2 - yellow). Thermally stable, melting without decomposition. Extremely sensitive to O2 and CO2 of air. Ion has the structure of (Rb +) 2 (O22-). Completely decomposed by water, acids. Exhibits redox properties.
Obtaining rubidium oxide Rb2O2:
4 Rb + O2 = 2 Rb2O (in the cold), Rb →(O2) Rb2O2 →(O2), (time) RbO2↓ (-50° C, in the liquid NH3).
RbO2 (-O2)→(400-800° C) Rb2O2 (-O2)→(t>1010°) C Rb2O,
2 RbO2 = Rb2O2 + O2 (290° C, vacuum).
Сhemical reactions with rubidium oxide Rb2O2:
2 Rb2O2 = 2 Rb2O + O2 (t>1010° C).
Rb2O2 + 2 H2O = 2 RbOH + H2O2 (0° C),
2 Rb2O2 + 2 H2O (hot) = 4 RbOH + O2↑.
Rb2O2 + 2 HCl (diluted, cold) = 2 RbCl + H2O2,
2 Rb2O2 + 2 H2SO4 (diluted, hot) = 2 Rb2SO4 + 2 H2O + O2↑.
Rb2O2 + O2(air) = 2 RbO2 (normal temp.).
2 Rb2O2 + 2CO2 = 2 Rb2CO3 + O2, Rb2O2 + CO = Rb2CO3 (normal temp.).
5 Rb2O2 + 8 H2SO4 (diluted) + 2 RbMnO4 = 5 O2↑ + 2 MnSO4 + 6 Rb2SO4 + 8 H2O.
RUBIDIUM OXIDE Rb2O
Properties Rubidium oxide Rb2O:
Yellowish-white, when heated turns bright yellow. Volatile in a vacuum. Sensitive to light (darkens and decomposes). Stable in a clean, dry air. Shows the basic properties, reacts vigorously with water (is formed strongly alkaline solution), acids, acid oxides, liquid ammonia.
Obtaining rubidium oxide Rb2O:
2Rb + 2RbOH = 2Rb2O + H2 (400°C).
4Rb + O2 = 2Rb2O (cold).
Rb → (O2) Rb2O2 → (O2, time) → RbO2↓ (-50°C, in the liquid NH3),
RbO2 → (-O2)(400-800°C) → Rb2O2 → (-O2)(t>1010°C) → Rb2O,
2RbO2 = Rb2O2 + O2 (290°C, vacuum).
Rb2CO3 = Rb2O + CO2 (t>900°C, vacuum).
Сhemical reactions with rubidium oxide Rb2O:
2Rb2O = Rb2O2 + 2Rb (400-550°C).
Rb2O + H2O = 2RbOH.
Rb2O + 2HCl(diluted) = 2RbCl + H2O.
Rb2O + CO2(moisture) = Rb2CO3,
Rb2O + H2O + 2CO2 = 2RbHCO3 (normal temp.).
Rb2O + NH3 (liquid) → (time) → RbNH2↓ + RbOH (-50°C).
RUBIDIUM HYDRIDE RbH
Properties Rubidium hydride RbH:
White. Decomposes when heated, pressurized H2 melts without decomposition. A strong reducing agent, reacts with water, acids, ammonia, oxygen, chlorine.
Obtaining rubidium hydride RbH:
2 Rb + H2 = 2 RbH (300—350° C, pressure).
Сhemical reactions with rubidium hydride RbH:
2 RbH = 2 Rb + H2 (t>200° C).
RbH + H2O = RbOH + H2↑.
RbH + HCl (diluted) = RbCl + H2↑.
2 RbH + O2 = 2 RbOH (t>200° C).
RbH + Cl2 = RbCl + HCl (400° C),
2 RbH + 2 S = Rb2S + H2S (300—350° C).
RbH + NH3 (gas) = RbNH2 + H2 (300° C).
