کل واکنشهای عنصر سزیم
CESIUM - Cs
Properties of metallic cesium Cs:
An alkali metal. White (on the cut - light yellow), soft, very low melting. The vapor of cesium is painted in a greenish-blue color. Chemically dissolves in liquid ammonia (dark blue solution), the melt of CsOH. It is extremely reactive, the strongest reducing agent, reacts with oxygen in the air, water (there is inflammation of the metal and hydrogen is released), 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 the blue.
Obtaining metallic cesium Cs:
2 Cs2O = Cs2O2 + 2 Cs (300—500° C).
4 CsOH (liquid) → Electrolysis 4 Cs (cathode) + O2↑ (anode) + 2 H2O.
2 CsCl + 2H2O → Electrolysis H2↑ (cathode) + Cl2↑ (anode) + 2 CsOH,
2 CsCl (melt) (on Hg-cathode)→ Electrolysis 2 Cs (cathode) + Cl2↑(anode).
Сhemical reactions with metallic cesium Cs:
2 Cs + 2 H2O = 2CsOH + H2↑.
2 Cs + 2 HCl (diluted) = 2 CsCl + H2↑.
8 Cs + 6 H2SO4 (diluted, cold) = 4 Cs2SO4 + SO2 + S↓ + 6H2O (impurity H2S),
21 Cs + 26 HNO3 (diluted, cold) = 21 CsNO3 + NO↑ + N2O↑ + N2↑ + 13H2O.
2 Cs + 2 CsOH = 2 Cs2O + H2↑ (300—350° C).
2 Cs + H2 = 2 CsH (300—350° C, pressure).
Cs + O2(air) = CsO2 (combustion),
4 Cs + O2 = 2 Cs2O (in the cold), Cs →(O2) Cs2O2↓ →(O2), (time) CsO2↓ (-50° C, in the liquid NH3).
4 Cs + O2 + 2 H2O = 4 CsOH.
2 Cs + E2 = 2 CsE (normal temp.; E = F, Cl, Br, I).
2 Cs + S = Cs2S (100—130° C).
2 Cs + 2 H2S (saturated) = 2 CsHS ↓ + H2 ↑ (in benzene).
2 Cs + 2 NH3 (gas) = 2 CsNH2 + H2 (30—45° C).
Cs + 6 NH3 (liquid) = [Cs(NH3)6](time, blue) [-40° C],
[Cs(NH3)6] + nNH3 (liquid) ↔ [Cs(NH3)6]+ + e-·nNH3.
4 Cs + 3 SiO2 = 2 Cs2SiO3 + Si (t>300° C).
CESIUM POLYSULFIDES Cs2S(n)
Properties of cesium polysulfides Cs2S(n):
A mixture of Cs2S(n) (n = 2, 3, 5, 6) has a yellow-brown color. All Cs2S(n) - a very solid, melt without decomposition, melts - is a dark brown mobile liquid. Thermal stability decreases with increasing n. Well soluble in water, to a lesser degree (compared to Cs2S), are hydrolyzed by the anion, the solution is colored in dark yellow. Oxidized in air, decomposed by acids. Possess oxidative properties.
Obtaining metallic cesium polysulfides Cs2S(n):
Cs2S (solution) (- CsOH)→O2 (air), (time) S(colloid), Cs2(Sn), Cs2SO3S.
Cs2S +(n - 1)S = Cs2(Sn) [boiling].
Сhemical reactions with cesium polysulfides Cs2S(n):
Cs2S(n) = Cs2S + (n - 1)S (t>600° C).
Cs2S(n)[diluted] + 12H2O = 2[Cs(H2O)6]+ + Sn2-,
Sn2- + H2O ↔ HSn- + OH-; pKo = 8,30 (n = 5).
Cs2S(n) + 2HCl(diluted) = 2 CsCl + H2S↑ + (n - 1)S↓ (normal temp.),
Cs2S(n) + 2HCl(conc.) = 2 CsCl + H2Sn (-15° C).
2 Cs2S(n) + 2H2O(cold) + O2 = 2nS(colloid) + 4CsOH (In the light).
CESIUM SULFIDE Cs2S
Properties of cesium sulfide Cs2S:
White, heat-resistant. Anhydrous powdered Cs2S is pyrophoric in dry air. Readily soluble in water (strong hydrolysis of the anion). Reactive, in humid state oxidation by O2 of air, appends Decomposes sulfur acids. Typical reductant.
Obtaining metallic cesium sulfides Cs2S:
2 Cs + S = Cs2S (100—130° C).
CsH + Cl2 = CsCl + HCl (400° C),
2 CsH + 2S = Cs2S + H2S (300—350° C).
Сhemical reactions with cesium sulfide Cs2S:
Cs2S·4H2O = Cs2S + 4H2O (150° C, vacuum).
Cs2S (diluted)+ 12 H2O = 2[Cs(H2O)6]+ + S2-, S2- + H2O ↔ HS- + OH-; pK0 = 1,09.
Cs2S + 2 HCl (diluted) = 2CsCl + H2S↑.
Cs2S + 3 H2SO4 (conc.) = 2CsHSO4 + S↓ + SO2↑ + 2H2O.
Cs2S (solution) (-CsOH)→(O2, air), (time) S(colloid), Cs2S(n), Cs2SO3S.
Cs2S + 2 O2 = Cs2SO4 (t>500° C).
Cs2S + H2S (saturated) = 2CsHS.
CESIUM CHLORIDE CsCl
Properties of cesium chloride CsCl:
White, melts and boils without decomposition. Readily soluble in water (without hydrolysis). Does not form crystalline hydrates. Dissolved in concentrated hydrochloric acid. A weak reducing agent. Participates in exchange reactions.
Obtaining cesium chloride CsCl:
2 Cs + 2HCl (diluted) = 2 CsCl + H2↑.
2 Cs + E2 = 2 CsE (normal temp.; E = F, Cl, Br, I).
CsOH + HCl (diluted) = CsCl + H2O,
2 CsOH + H2SO4 (diluted) = Cs2SO4 + 2 H2O,
CsOH + HNO3 (diluted) = CsNO3 + H2O.
Cs2CO3 + 2 HCl (diluted) = 2 CsCl + CO2↑ + H2O.
Cs2SO4 + BаE2 = BaSO4↓ + 2 CsE (E = Cl-, OH-).
Сhemical reactions with cesium chloride CsCl:
CsCl (diluted) + 6H2O = [Cs(H2O)6]+ + Cl- (pH 7).
2 CsCl (solid) + H2SO4 (conc.) = Cs2SO4 + 2HCl↑ (кип.).
CsCl + CsHSO4 = Cs2SO4 + HCl (550—700° C).
10 CsCl (solid) + 8H2SO4 (conc., hot) + 2KMnO4(solid) = 5 Cl2↑ + 2 MnSO4 + K2SO4 + 5 Cs2SO4 + 8 H2O.
2 CsCl + H2[SnCl6] = Cs2[SnCl6]↓ + 2 HCl (in the conc. HCl).
3 CsCl + 2H[SbCl4] = Cs3[Sb2Cl9]↓ + 2 HCl (in the conc. HCl).
2 CsCl + H2[PtCl6] = Cs2[PtCl6]↓ + 2 HCl (in the diluted HCl).
2 CsCl (liquid) →Electrolysis 2Cs(cathode) + Cl2↑ (anode).
2 CsCl + 2 H2O →Electrolysis H2↑ (cathode) + Cl2↑ (anode) + 2 CsOH,
2 CsCl (melt) (on Hg-cathode)→Electrolysis 2 Cs (cathode) + Cl2↑ (anode)./p>
CESIUM SULFATE Cs2SO4
Properties of cesium sulfate Cs2SO4:
White, volatile, melts without decomposition. Readily soluble in water (without hydrolysis). Does not form crystalline hydrates. Participates in exchange reactions.
Obtaining cesium sulfate Cs2SO4:
8 Cs + 6H2SO4 (diluted, cold) = 4 Cs2SO4 + SO2 + S↓ + 6 H2O (impurity H2S).
2 CsOH + H2SO4 (diluted) = Cs2SO4 + 2H2O.
Cs2S (solid) + 2O2 = Cs2SO4 (t> 500° C).
Сhemical reactions with cesium sulfate Cs2SO4:
Cs2SO4 (diluted) + 12 H2O = 2[Cs(H2O)6]+ + SO42- (pH 7).
Cs2SO4 (solid) + H2SO4 (conc.) = 2 CsHSO4.
Cs2SO4 + ВаE2 = BaSO4↓ + 2 CsE (E = Cl-, OH-).
Cs2SO4 + Al2(SO4)3 + 24 H2O = 2{CsAl(SO4)2·12H2O}↓ (alum).
CESIUM NITRATE CsNO3
Properties of cesium nitrate CsNO3:
White, melts without decomposition, decomposes on further heating. Readily soluble in water with an endo-effect (without hydrolysis). Does not form crystalline hydrates. Strong oxidizing agent during sintering. In solution recovered only by atomic hydrogen.
Obtaining cesium nitrate CsNO3:
21 Cs + 26 HNO3 (diluted, cold) = 21 CsNO3 + NO↑ + N2O↑ + N2↑ + 13 H2O.
CsOH + HNO3 (diluted) = CsNO3 + H2O.
Сhemical reactions with cesium nitrate CsNO3:
2 CsNO3 = 2 CsNO2 + O2 (585-850° C).
CsNO3 (diluted) + 6 H2O = [Cs(H2O)6]+ + NO3- (pH 7).
CsNO3 (saturated) + (1 - 2)HNO3(conc.) = CsNO3·(1 - 2)HNO3 ↓ (normal temp.).
CsNO3 + 2 H0 (Zn, dilutedHCl) = CsNO2 + H2O (normal temp.),
CsNOs + 8H0(Zn, conc. NaOH) = NH3 ↑ + 2H2O + CsOH (boiling).
2 CsNO3 + (NH4)2SO4 = Cs2SO4 + 2 N2O + 4 H2O (350° C).
CsNO3 + Pb = CsNO2 + PbO (400° C).
CESIUM CARBONATE Cs2CO3
Properties of cesium carbonate Cs2CO3:
White, at calcination decomposes, melts under pressurized CO2. Sensitive to moisture and CO2 of air. Very soluble in water (strong hydrolysis of the anion), creates a highly alkaline environment. Decomposed by acids. Participates in exchange reactions.
Obtaining cesium carbonate Cs2CO3:
Cs2O + CO2(humid) = Cs2CO3 (normal temp.),
Cs2O + H20 + 2 CO2 = 2 CsHCO3 (normal temp.).
CsOH (conc.) + CO2 = Cs2CO3 + H2O.
Сhemical reactions with cesium carbonate Cs2CO3:
Cs2CO3 = Cs2O + CO2 (620 - 1000°C, vacuum).
Cs2CO3x3.5H2O = Cs2CO3 + 3.5 H2O, (150-160°C).
Cs2CO3 (diluted) + 12 H2O = 2[Cs(H2O)6]+ + (CO3)2-,
(CO3)2- + H2O = HCO3- + OH-, pK0 = 3.67
Cs2CO3 + 2HCl(diluted) = 2CsCl + CO2↑+ H2O.
Cs2CO3 (saturated) + 2 HClO4(conc. cold) = 2CsClO4↓ + CO2↑ + H2O.
Cs2CO3 + H2O + CO2 -> 2 CsHCO3 (20°C),
2 CsHCO3 -> Cs2CO3 + H2O + CO2 (170-180°C).
Cs2CO3 + Ca(OH)2 (saturated) = 2CsOH + CaCO3↓.
CESIUM HYDROXIDE CsOH
Properties of cesium hydroxide CsOH:
White, melts without decomposition, volatile. Readily soluble in water with a strong exo effect, creates a highly alkaline environment. Exhibits the properties of basic hydroxides (refers to alkali), neutralized by acid, reacts with acidic oxides, oxygen and ozone.
Obtaining cesium hydroxide CsOH:
2 Cs + 2 H2O = 2 CsOH + H2↑.
4 Cs + O2 + 2 H2O = 4 CsOH.
Cs2O + H2O = 2 CsOH.
Cs2CO3 + Ca(OH)2 (saturated) = 2 CsOH + CaCO3↓.
Cs2SO4 + BaE2 = BaSO4↓ + 2CsE, (E = Cl-, OH-).
2 CsCl + 2 H2O → (Electrolysis) H2↑(cathode) + Cl2↑(anode) + 2 CsOH.
Сhemical reactions with cesium hydroxide CsOH:
CsOH x H2O = CsOH + H2O (300°C, in flow of H2).
CsOH (diluted) + 6H2O = [Cs(H2O)6]+ + OH-.
CsOH + HCl (diluted) = CsCl + H2O.
2 CsOH + H2SO4 (diluted) = Cs2SO4 + 2 H2O.
CsOH + HNO3 (diluted) = CsNO3 + H2O.
4 CsOH(liquid) + 3O2 = 4 CsO2 + 2 H2O (400°C).
4 CsOH + 4O3 = 4 CsO3 + O2 + 2H2O (20°C).
2 CsOH(conc.) + CO2 = Cs2CO3 + H2O.
4 CsOH(liquid) → (Electrolysis) 4Cs(cathode) + O2↑(anode) + 2H2O.
CESIUM OZONIDE CsO3
Properties of cesium ozonide CsO3:
Orange-red. More resistant than KO3 and RbO3, decomposes at moderate heat. Structure has ion (Cs+)(O3(-)). Reacts vigorously with water, acids, sulfur. Very strong oxidant.
Obtaining cesium ozonide CsO3:
CsO2 + O3 = CsO3 + O2 (norm. temp.).
4 CsOH + 4O3 = 4 CsO3 + O2 + 2H2O (20°C).
Сhemical reactions with cesium ozonide CsO3:
2 CsO3 = 2 CsO2 + O2 (70-100°C).
4 CsO3 + 2H2O = 4 CsOH + 5 O2↑ (possible traces of radicals OH(0)).
4 CsO3 + 4 HCl (diluted, cold) = 4 CsCl + 5 O2↑ +2 H2O.
4 CsO3 + 4 HCl (diluted, hot) = 2 CsCl + Cl2↑ + 2O2 + 2H2O.
4 CsO3 + H2O(moisture) + 3 CO2 = Cs2CO3 + 2 CsHCO3 + 5O2 (norm. temp.).
6 CsO3 + 5 S = Cs2SO4 + 2 Cs2S2O7 (30-40°C).
CsO3 + 2 NH3(liquid) = NH4O3 + CsNH2 (-50°C).
CESIUM SUPEROXIDE CsO2
Properties of cesium superoxide CsO2:
The orange-yellow, decomposes on heating without melting, melted by pressurized of O2. Structure has ion (Cs+)(O2(-)). Reacts vigorously with water, acids, ozone, mono- and dioxide carbon, ammonia. Very strong oxidant.
Obtaining cesium superoxide CsO2:
Cs → (O2) Cs2O2↓ → (O2, time) CsO2↓ (-50°C, in liquid NH3).
4 CsOH(liquid) + 3O2 = 4 CsO2 + 2 H2O (400°C).
Сhemical reactions with cesium superoxide CsO2:
CsO2 → (400-600°C, -O2) Cs2O2 → (640-980°C, -O2) Cs2O.
4 CsO2 + 2 H2O = 4 CsOH + 3 O2↑. (0°C)
2 CsO2 + 2 HCl(diluted, cold) = 2 CsCl + H2O2 + O2↑.
2 CsO2 + 2 H2SO4(anhydrous) = 2 CsHSO4 + O3↑ + H2O (norm. temp.).
CsO2 + O3 = CsO3 + O2 (norm. temp.).
2 CsO2 + 2 NH3 →(time) 2CsOH + N2 + 2 H2O (norm. temp.).
4 CsO2 +2 CO2(humid) = 2 Cs2CO3 + 3O2 (norm. temp.).
2 CsO2 + CO = Cs2CO3 + O2 (30-40°C).
CESIUM PEROXIDE Cs2O2
Properties of cesium peroxide Cs2O2:
White (with a impurity of CsO2 - yellow). Thermally stable, with a strong heated melts and decomposes. Extremely sensitive to O2 of air, absorb moisture and CO2. Completely decomposed by water, acids. Shows redox properties.
Obtaining cesium peroxide Cs2O2:
Cs → (O2) Cs2O2↓ → (O2, time) CsO2↓ (-50°C, in liquid NH3).
CsO2 → (400-600°C, -O2) Cs2O2 → (640-980°C, -O2) Cs2O.
Сhemical reactions with cesium peroxide Cs2O2:
2 Cs2O2 = 2 Cs2O + O2 (640–980° C).
Cs2O2 + 2H2O = 2 CsOH + H2O2 (0° C).
2 Cs2O2 + 2 H2O(hot)= 4 CsOH + O2↑.
Cs2O2 + 2 HCl(dilute, cold)= 2 CsCl + H2O2.
2 Cs2O2 + 2 H2SO4(dilute, hot)= 2 Cs2SO4 + 2H2O+O2↑.
Cs2O2 + O2(air)= 2 CsO2 (normal temp.).
2 Cs2O2 + 2 CO2 = 2 Cs2CO3 + O2.
Cs2O2 + CO = Cs2CO3 (normal temp.).
5 Cs2O2 + 8 H2SO4(dilute) + 2 CsMnO4 = 5 O2↑ +2 MnSO4 + 6 Cs2SO4 + 8 H2O.
CESIUM OXIDE Cs2O
Properties of cesium oxide Cs2O:
Orange-red, when heated becomes first dark red, and then black. Volatiles in vacuo. Sensitive to light (darkens and decomposes).Stable in a clean, dry air. Shows basic properties, vigorously reacts with water (is formed strongly alkaline solution), acids, acidic oxides, liquid ammonia.
Obtaining cesium oxide Cs2O:
Cs + O2(air) = CsO2 (combustion),
4 Cs + O2 = 2 Cs2O (in the cold),
Cs →(O2) Cs2O2↓ →(O2), (time) CsO2↓ (-50° C, in the liquid NH3).
Сhemical reactions with cesium oxide Cs2O:
2 Cs2O = Cs2O2 + 2 Cs (300–500°C).
Cs2O + H2O = 2 CsOH.
Cs2O + 2 HCl(diluted) = 2 CsCl + H2O.
Cs2O + CO2(humid) = Cs2CO3,
Cs2O + H2O + CO2 = 2 CsHCO3 (normal temp.).
Cs2O + NH3(liquid) → (time) CsNH2↓ + CsOH (−50°C).
CESIUM HYDRIDE CsH
Properties of cesium hydride CsH:
White. Decomposes when heated, pressurized by H2 melts without decomposition. A strong reducing agent, reacts with water, acids, ammonia, oxygen, and chlorine.
Obtaining cesium hydride CsH:
2 Cs + H2 = 2 CsH (300–350°C, pressure).
Сhemical reactions with cesium hydride CsH:
2 CsH = 2Cs + H2 (above 200°C).
Cs+ H + H2O = CsOH + H2↑.
CsH + HCl(diluted)= CsCl+H2↑.
2 CsH + O2 = 2 CsOH (above 200°C).
CsH + Cl2 = CsCl + HCl (400°C).
2 CsH + 2 S = Cs2S + H2S (300–350°C).
CsH + NH3(gas) = CsNH2 +H2 (350°C).
