کل واکنشهای عنصر لیتیم
LITHIUM - Li
An alkali metal. A silvery-white. The easiest of the metals, soft, low melting. Reactive, air-oxide-nitride coated film. Ignited at a moderate heat, stains flame of a gas burner in a dark-red color. A strong reducing agent, reacts with water, acids, non-metals, ammonia.
| Molar mass | g/mol | 6.941 |
| Density | g/cm3 | 0.534 |
| Melting point | °C | 180.5 |
| Boiling point | °C | 1336.6 |
Obtaining Lithium:
2LiH = 2Li + H2 (450°C).
2LiH (liquid) → Electrolysis → 2Li(on cathode) + H2↑(on anode).
2Li2O + Si = 4Li + SiO2 (1000°C).
Li2O + Mg = 2Li + MgO (t> 800°C).
3Li2O + 2Al = 6Li + Al2O3 (t> 1000°C).
2LiCl(liquid) → Electrolysis 2Li(on cathode) + Cl2↑(on anode).
2LiCl(melt) (on Hg-cathode) → Electrolysis → 2Li(on cathode) + Cl2↑(on anode).
2Li3N = 6Li + N2 (300-500°C, vacuum).
Reactions with Lithium:
2Li + 2H2O = 2LiOH + H2↑.
2Li + 2HCl(conc.) = 2LiCl + H2↑.
2Li + 3H2SO4(conc.) = 2LiHSO4 + SO2↑ + 2H2O.
3Li + 4HNO3(dilute) = 3LiNO3 + NO↑ + 2H2O.
2Li + H2 = 2LiH (500-700°C).
2Li + E2 = 2LiE (normal temp., E = F, Cl, Br; t>200°C, E = I).
4Li + O2 = 2Li2O (t>200°C, impurity Li2O2)
2Li + S = Li2S (t>130° C)
6Li + N2(moist) = 2Li3N (normal temp.)
6Li + N2 = 2Li3N (200-250°C, pressure)
2Li + 2C = Li2C2 (t>200°C, vacuum)
4Li + Si = Li4Si (600-700°C, impurity Li2Si)
2Li + 2NH3 = 2LiNH2 + H2 (220°C)
2Li + NH3 = Li2NH + H2 (400°C)
Li + 4NH3 (liquid) = [Li(NH3)4]0 (blue) [-40°C]
[Li(NH3)4]0 + nNH3(liquid) ↔ [Li(NH3)4]+ + e- + nNH3.
LITHIUM OXIDE Li2O
White, hygroscopic, refractory, when heated, does not decompose. Behaves as a typical oxide, reacts vigorously with water (formed alkaline solution), acids, metals, acid oxides, absorbs CO2 from the air.
Obtaining Lithium oxide Li2O:
4Li + O2 = 2Li2O (t> 200°C, impurity Li2O2)
2LiOH = Li2O + H2O (800-1000°C, in the atm. of H2).
Li2CO3 = Li2O + CO2 (730-1270°C).
Li2CO3 + C(coke) = Li2O + 2CO (800°C).
4LiNO3 = 2Li2O + 4NO2 + O2 (475-650°C).
Reactions with Lithium oxide Li2O:
Li2O + H2O = 2LiOH.
Li2O + 2HCl (delute) = 2LiCl + H2O.
Li2O + H2S = Li2S + H2O (900-1000°C).
2Li2O + Si = 4Li + SiO2 (1000°C).
Li2O + Mg = 2Li + MgO (t>800°C).
3Li2O + 2Al = 6Li + Al2O3 (t>1000°C).
Li2O + CO2 = Li2CO3 (500-600°C).
2Li2O + SiO2 = Li4Si04 (1000°C),
Li2O + SiO2 = Li2SiO3 (1200-1300°C).
LITHIUM PEROXIDE Li2O2
White, when heated decomposes without melting. Fully hydrolyzed by water, reacts with acids. Vigorously absorbs CO2 from the air.
Obtaining Lithium peroxide Li2O2:
2 LiOH + H2O + 2 H2O2 (hot) = Li2O2-H2O2-3H2O↓ (in ethanol),
Li2O2-H2O2-3H2O = Li2O2 + H2O2 + 3 H2O (over P4O10, vacuum).
Reactions with lithium peroxide Li2O2:
2 Li2O2 = 2Li2O + O2 (200—400° C).
Li2O2-H2O = Li2O2 + H2O (t> 0° C).
Li2O2 + 2 H2O (cold) = 2 LiOH + H2O2
2 Li2O2 + 2 H2O (hot) = 4 LiOH + O2↑.
Li2O2 + 2 HCl (dilute, cold) = 2 LiCl + H2O2,
2 Li2O2 + 2 H2SO4 (dilute,hot.) = 2Li2SO4 + 2H2O + O2↑.
2 Li2O2 + 2 CO2 = 2 Li2CO3 + O2 (t>200° C),
Li2O2 + CO = Li2CO3 (40—70° C).
LITHIUM HYDROXIDE LiOH
White, melts without decomposition, further heating is decomposed in an atmosphere of H2. It is readily soluble in water. Exhibits the properties of the basic hydroxide (alkali), reacts with acids, acid oxides, absorbs CO2 from the air.
| Molar mass | g/mol | 23.95 |
| Density | g/cm3 | 1.46 |
| Melting point | °C | 471 |
Obtaining lithium hydroxide LiOH:
2 Li + 2 H2O = 2 LiOH + H2↑.
LiH + H2O = LiOH + H2↑.
2 LiH + O2 = 2 LiOH (t> 500°C).
Li2O + H2O = 2 LiOH.
Li2CO3 + Ca(OH)2 = 2 LiOH + CaCO3 (to 600°C).
Li2SO4 + Ba(OH)2 = BaSO4 ↓ + 2LiOH.
2 LiCl + 2 H2O → Electrolysis 2 LiOH + H2↑ (cathode) + Cl2 (anode).
Reactions with lithium hydroxide LiOH:
2 LiOH = Li2O + H2O (800-1000°C, in the atm. H2).
LiOH-H2O = LiOH + H2O (500°C, in the atm. H2).
LiOH (dilute) + 4 H2O = [Li(H2O)4]+ + OH-.
LiOH + HCl (dilute.) = LiCl + H2O.
2 LiOH (conc.) + CO2 = Li2CO3 ↓ + H2O (norm. temp).
4 LiOH (dilute) + SiO2 (solid) ↔ Li4SiO4 (solution) + 2H2O (norm. temp).
2 LiOH (saturated) + SO2 = Li2SO3 + H2O.
2 LiOH + H2O + 2H2O2 (hot) = Li2O2-H2O2-3H2O↓ (in ethanol),
Li2O2-H2O2-3H2O = Li2O2 + H2O2 + 3H2O (over P4O10, vacuum).
2 LiOH (cold) + Cl2 = LiClO + LiCl + H2O,
6 LiOH (cold) + 3 Cl2 = LiClO3 + 5 LiCl + 3H2O.
LITHIUM CARBONATE Li2CO3
Properties of lithium carbonate:
White, calcination decomposes above the melting point. Moderately soluble in cold water, less in hot water. Crystalline hydrates are not. Reacts with acids, metals and non-metals, their oxides.
| Molar mass | g/mol | 73.89 |
| Density | g/cm3 | 2.11 |
| Melting point | °C | 618 |
Obtaining Lithium carbonate Li2CO3:
Li2O + CO2 = Li2CO3 (500-600°C).
2LiOH (conc.) + CO2 = Li2CO3↓ + H2O (normal temp.).
Li2SO4 (conc.) + Na2CO3 = Li2CO3↓ + Na2SO4 (boiling).
Reactions with Lithium carbonate Li2CO3:
Li2CO3 = Li2O + CO2 (730-1270°C).
Li2CO3 + 2 HCl (dilute)= 2LiCl+CO2↑ +H2O.
Li2CO3 + C(coke)= Li2O + 2CO (800°C).
Li2CO3 + Mg = 2Li + MgO + CO2 (500°C).
Li2CO3 (solid) + H2O + CO2 → 2LiHCO3 (solution)
2Li2CO3 +SiO2 = Li4SiO4 + 2CO2 (800-1000°C).
Li2CO3 + 4 B(OH)3 = Li2B4O7 + CO2 + 6H2O (600°C).
Li2CO3 + Al2O3 = 2LiAlO2 + CO2 (800-900°C).
Li2CO3 + Ca(OH)2 = 2LiOH + CaCO3 (to 600°C).
4Li2CO3 + 2Cr2O3 + 3O2 = 4 Li2CrO4 + 4 CO2 (600-700°C).
LITHIUM NITRATE LiNO3
Properties of lithium nitrate:
White, very hygroscopic, melts without decomposition, decomposes on further heating. It is readily soluble in water (without hydrolysis). Oxidizing agent during sintering. In solution recovered only by atomic hydrogen.
Obtaining Lithium nitrate LiNO3:
3 Li + 4 HNO3 (dilute) = 3 LiNO3 + NO ↑ + 2H2O.
LiF + HNO3 (conc.) = LiNO3 + HF ↑.
Li2S + 4 HNO3 (conc.) = 2 LiNO3 + 2NO2 ↑ + S ↓ + 2H2O
Reactions with Lithium nitrate LiNO3:
4 LiNO3 = 2 Li2O + 4 NO2 + O2 (475—650° C).
LiNO3-3H2O = LiNO3 + 3 H2O (200° C, vacuum).
LiNO3 (dilute.) + 4H2O = [Li(H2O)4]+ + NO3- ↑ (pH 7).
LiNO3 + 2 H0 (Zn, conc. HCl) = LiNO2 + H2O.
LiNO3 + Pb = LiNO2 + PbO (400° C)
LITHIUM ORTHOPHOSPHATE Li3PO4
Properties of lithium orthophosphate:
White, melts without decomposition. Poorly soluble in water, the solubility increases in the presence of ammonia hydrate. Decomposes by acids.
Obtaining lithium orthophosphate:
3 LiCl (conc.) + K3PO4 = Li3PO4 ↓ + 3 KCl.
3 LiCl (conc.) + Na2HPO4 + NaOH = Li3PO4 ↓ + H2O + 3 NaCl
Reactions with lithium orthophosphate:
Li3PO4-12 H2O = Li3PO4 + 12H2O (120° C, vacuum).
Li3PO4 + 2 HCl (conc.) = LiH2PO4 + 2LiCl.
Li3PO4 + H2SO4 (dilute) = 2 Li2HPO4 + Li2SO4
Li3PO4 + 3 H2SO4 (conc.) =3 LiHSO4 + H3PO4.
Li3PO4 + 3 CaCl2 (conc.) = 6 LiCl + Ca3(PO4)2 ↓
LITHIUM SULFATE Li2SO4
Properties of lithium sulfate:
White, melts without decomposition. It is readily soluble in water (hydrolysis does not). Participates in exchange reactions.
Obtaining lithium sulfate:
2 LiH + 2 SO2 = Li2SO4 + H2S (200° C).
Li2S + 2 O2 = Li2SO4 (t> 300° C)
Reactions with lithium sulfate:
Li2SO4-H2O = Li2SO4 + H2O (130—500° C).
Li2SO4 (dilute) + 8H2O = 2[Li(H2O)4]+ + SO42- (pH7).
Li2SO4 + H2SO4 (conc.) = 2 LiHSO4.
Li2SO4 (conc.) + Na2CO3 = Li2CO3 ↓ +Na2SO4.
Li2SO4 + BaCl2 = BaSO4 ↓ + 2LiCl.
Li2SO4 + Ba(OH)2 = BaSO4 ↓ + 2 LiOH.
Li2SO4 + Ba(N3)2 = 2 LiN3 + BaSO4 ↓.
Li2SO4 + 4 C (coke) = Li2S + 4 CO (800—900° C).
Li2SO4 + 4 H2 = Li2S + 4 H2O (600—700° C).
LITHIUM FLUORIDE LiF
Properties of lithium fluoride:
White, melts without decomposition. It is readily soluble in water (hydrolysis does not). Participates in exchange reactions.
| Molar mass | g/mol | 25.94 |
| Density | g/cm3 | 2.635 |
| Melting point | °C | 845.1 |
| Boiling point | °C | 1676 |
Obtaining lithium fluoride:
2 Li + E2 = 2LiE (normal temp., E = F, Cl, Br; t> 200° C, E = I).
LiCl (conc.) + NH4F (conc.) = LiF↓ + NH4Cl.
Reactions with lithium fluoride:
LiF (solid) + HF (conc.) = Li(HF2) (solution).
LiF + H2SO4 (conc.) = LiHSO4 + HF ↑.
LiF + HNO3 (conc.) = LiNO3 + HF ↑.
2 LiF + CaO = Li2O + CaF2 (600—700° C).
2 LiF + Ca(OH)2 (saturated solution, hot) = 2 LiOH + CaF2 ↓
LITHIUM CHLORIDE LiCl
Properties of lithium chloride LiCl:
White, deliquescent. Melts and boils without decomposition. Readily soluble in water (hydrolysis does not). Decomposed by concentrated acids. Participates in exchange reactions.
| Molar mass | g/mol | 42.39 |
| Density | g/cm3 | 2.068 |
| Melting point | °C | 610 |
| Boiling point | °C | 1380 |
| Solubility in water at 25°C | g/100g water | 84.5 |
Obtaining lithium chloride LiCl:
2Li + 2 HCl (dilute) = 2LiCl + H2↑.
2Li + E2 = 2LiE (normal temp., E = F, Cl, Br; t> °C C, E = I).
LiH + HCl (dilute) = LiCl + H2↑ (normal temp.).
LiH + Cl2 = LiCl + HCl (400-450°C).
Li2O + 2HCl (dilute) = 2LiCl + H2O.
LiOH + HCl (dilute) = LiCl + H2O.
Li2CO3 + 2HCl (dilute) = 2LiCl + CO2↑ + H2O.
Li2SO4 + BaCl2 = BaSO4↓ + 2LiCl.
Reactions with lithium chloride LiCl:
LiCl-H2O = LiCl + H2O (t> 98°C).
LiCl (dilute) + 4 H2O = [Li(H2O)4]+ + Cl-.
2LiCl (solid) + H2SO4 (conc.) = Li2SO4 + 2 HCl↑ (boiling).
LiCl + LiHSO4 = Li2SO4 + HCl (450-500°C).
LiCl (conc.) + NH4F(conc.) = LiF↓ + NH4Cl.
LiCl (cold) + AgNO2(saturated) = LiNO2 + AgCl↓.
3LiCl (conc.) + K3PO4 = Li3PO4↓ + 3 KCl.
3LiCl (conc.) + Na2HPO4 + NaOH = Li3PO4↓ + H2O + 3 NaCl.
LiCl (conc.) + 4(NH3-H2O) (conc.) = [Li(NH3)4]Cl + 4 H2O.
2 LiCl (liquid) → Electrolysis → 2Li (on cathode) + Cl2↑(on anode).
2 LiCl + 2H2O → Electrolysis → 2LiOH + H2↑(on cathode + Cl2 (on anode).
2 LiCl (melt)(on Hg-cathode) → Electrolysis → 2Li(on cathode) + Cl2↑(on anode)
LITHIUM SULFIDE Li2S
Properties of lithium sulfide:
Light yellow, melts without decomposition. Readily soluble in water (hydrolysis of the strong anion). Crystalline hydrates are not. Reductant, in the moist state oxidized by atmospheric oxygen. Reacts with acids, non-metals.
Obtaining lithium sulfide Li2S:
2Li + S = Li2S (t>130° C)
2LiH + 2S = Li2S + H2S (300-50°C).
Li2O + H2S = Li2S + H2O (900-1000°C).
Li2SO4 + 4C (coke) = Li2S + 4CO (800-900°C).
Li2SO4 + 4H2 = Li2S + 4H2O (600-700°C).
Reactions with lithium sulfide Li2S:
Li2S (dilute) + 8H2O = 2[Li(H2O)4]+ + S2-
S2- + H2O ↔ HS- + OH-.
Li2S + 2HCl(dilute) = 2LiCl + H2S↑.
Li2S + 3H2SO4(conc.) = 2LiHSO4 + SO2↑ + S↓ + 2H2O.
Li2S + 4HNO3(conc.) = 2LiNO3 + 2NO2↑ + S↓ + 2H2O.
Li2S(cold) + H2S (saturated) = 2LiHS.
Li2S + 2 O2 = Li2SO4 (t>300°C).
2Li2S + 2 H2O (cold) + O2 = S↓ + 4LiOH.
LITHIUM NITRIDE Li3N
Properties of lithium nitride:
Dark-red, melts under pressure, decomposed under heating. Fully hydrolyzed in water, decomposes by acids.
Obtaining lithium nitride:
6 Li + N2 (moist) = 2 Li3N (normal temp.)
6 Li + N2 = 2 Li3N (200—250° C, р)
3 LiH + N2 = Li3N +NH3 (500—600° C)
Reactions with lithium nitride:
2 Li3N = 6 Li + N2 (300—500° C, vacuum).
Li3N + 4 H2O (cold) = 3 LiOH + NH3-H2O.
Li3N + 4 HCl (dilute) = 3 LiCl + NH4Cl.
Li3N + 3 H2 = 3 LiH + NH3 (300° C, impurity Li2NH)
LITHIUM AMIDE LiNH2
Properties of lithium amide:
White, melts without decomposition, decomposes on further heating. Completely hydrolysed by water. Reacts with acids.
Obtaining lithium amide:
2 Li + 2 NH3 = 2 LiNH2 + H2 (220° C)
LiH + NH3 = LiNH2 + H2 (350° C).
LiH + NH3 (liquid) = LiNH2 ↓ + H2 ↑ (- 40° C).
Reactions with lithium amide:
2 LiNH2 = Li2NH + NH3 (400—500° C).
LiNH2 + 2 H2O (cold) = LiOH + NH3-H2O.
LiNH2 + 2 HCl (dilute) = LiCl + NH4Cl
LITHIUM IMIDE Li2NH
Properties of lithium imide Li2NH:
White, decomposes when heated. Completely hydrolyzed in water. Reacts with acids and hydrogen.
Obtaining lithium imide Li2NH:
2 Li + NH3 = Li2NH + H2 (400° С)
2 LiNH2 = Li2NH + NH3 (400—500° C)
Reactions with lithium imide LI2NH:
3 Li2NH = 2Li3N + NH3 (t>500° С).
Li2NH + ЗН2О (cold) = 2LiOH + NH3-Н2О.
Li2NH + НСl (dilute) = LiCl + NH4Cl.
Li2NH + H2 = LiNH2 + LiH (250—350° C).
LITHIUM HYDRIDE LiH
White, light and melts without decomposition, decomposes on further heating. A strong reducing agent, reacts with water, acids, non-metals, oxides of nonmetals.
Obtaining lithium hydride LiH:
2 Li + H2 = 2 LiH (500-700° C).
Li3N + 3H2 = 3 LiH + NH3 (300° C, impurity Li2NH).
Reactions lithium hydride LiH:
2 Li + H2 = 2 LiH (500-700° C).
Li3N + 3 H2 = 3 LiH + NH3 (300° C, impurity Li2NH).
2 LiH = 2Li + H2 (450° C).
LiH + H2O = LiOH + H2↑.
LiH + HCl (dilute) = LiCl + H2↑ (normal temp.).
2 LiH + O2 = 2 LiOH (t> 500° C).
LiH + Cl2 = LiCl + HCl (400-450° C).
2 LiH + 2S = Li2S + H2S (300—350° C).
3 LiH + N2 = Li3N +NH3 (500—600° C).
2 LiH + 4C (graphite) = Li2C2 + C2H2 (400° C).
2 LiH + 2SO2 = Li2SO4 + H2S (200° C).
LiH + CO2 = Li(HCOO) [250° C, р].
4 LiH + 3SiO2 = 2Li2SiO3 + Si + 2H2 (500° C).
LiH + NH3 = LiNH2 + H2 (350° C).
LiH + NH3(liquid) = LiNH2↓ + H2↑ (- 40° C).
4 LiH + AlCl3 = Li[AlH4] + 3LiCl↓ (in ether).
2 LiH (liquid) → Electrolysis → 2Li(on cathode) + H2↑(on anode).
بعضی ها ما را سرزنش می کنند که چرا دم از کربلا می زنید و از عاشورا ؛
آنها نمیدانند که برای ما کربلا بیش از آنکه یک شهر باشد، یک افق است! که آن را به تعداد شهدایمان فتح کرده ایم ، نه یک بار نه دو بار ... به تعداد شهدایمان(شهیدسیدمرتضی آوینی)
لایک= اللهم ارزقنا توفیق الشهادة فی سبیلک...