سلام
امروز وبلاگم رو با یک فایل power point به روز میکنم
عنوان این مطلب The liquid-liquid phase separation and crystallization of vanillin in 1-propanol/water solutionهستش ، یعنی جداسازی مایع-مایع و تبلور وانیلین از محلول آب و 1-پروپانول که البته به زبان انگلیسی هستش.
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سلام
امروز میخوام یک ترفند برای محدود کردن تعداد افرادی که میتونن به وایفای منزل شما وصل بشن بهتون آموزش بدم ، شاید واستون پیش اومده باشه که رمز وایفاتون رو در اختیار کسی قرار داده باشین و دوس نداشته باشین که کسی بجز اون شخص از حجم اینترنت شما استفاده کنه، برای اینکه بتونید تعداد افرادی که میتونن به اینترنت شما دسترسی داشته باشن رو محدود کنید کافیه که از mac filter استفاده کنید.
وارد تنظیمات مودم خودتون بشید(معمولا در اکثر مودم ها با وارد کردن 192.168.1.1 در address bar مرورگر،میشه وارد تنظیمات مودم شد)
وارد قسمتadsl setup یا wireless setup بشید و به دنبال wireless mac filter بگردید،اگر پیداش نکردید واردadvance بشید چون به احتمال زیاد اونجا پیداش میکنید:
حالا مک آدرس دستگاه های مورد نظر (کامپیوتر، تبلت، تلفن همراه و...) رو در بخشهای مشخص شده وارد کنید و گزینه actiated رو انتخاب و apply setting رو بزنید.
دقت کنید که اگر بخش action روی allow associated باشد یعنی فقط دستگاه هایی که شما مک ادرس شان را وارد کردید مجاز به مصرف اینترنت شما هستند ؛ همچنین اگر بخش action روی deny باشد یعنی فقط دستگاه هایی که شما مک آدرس آنها را وارد کردید مجاز نیستند از اینترنت استفاده کنند و سایر افرادی که رمز را داشته باشند مجاز به اتصال هستند.
حالا mac address چیست؟
اگر بخواهید مک آدرس یک گوشی یا تبلت را پیدا کنید کافیست وقتی که گوشی به وایفا وصل است وارد تنظیمات شوید و در قسمتی که مشخصات سخت افزاری و نرم افزاری گوشیتان نوشته شده (بخش about phone) مک آدرس را پیدا نمایید.
اگر میخواهید مک آدرس کامپیوتری را که به اینترنت شما وصل است پیدا کنید فقط کافیست وارد start شوید و سپس عبارت cmd را بنویسید و کلید enter بفشارید، پنجره ای باز میشود که میبایست در آن عبارت getmac تایپ شود تا مک آدرس را نشان دهد:
حالا اگه کسی بجز افرادی که مک آدرس اونها رو وارد کردید حتی رمز وایفای شمارو هم داشته باشه،نمیتونه به اینترنت وصل بشه.
امیدوارم که توضیحاتم به دردتون خورده باشه.
Name: Actinium
Symbol: Ac
Atomic Number: 89
Atomic Mass: (227.0) amu
Melting Point: 1050.0 °C (1323.15 K, 1922.0 °F)
Boiling Point: 3200.0 °C (3473.15 K, 5792.0 °F)
Number of Protons/Electrons: 89
Number of Neutrons: 138
Classification: Rare Earth
Crystal Structure: Cubic
Density @ 293 K: 10.07 g/cm3
Color: Silvery
![[Bohr Model of Actinium]](http://www.chemicalelements.com/bohr/b0089.gif) |
|
| Isotope | Half Life |
| Ac-225 | 10.0 days |
| Ac-226 | 1.2 days |
| Ac-227 | 21.8 years |
| Ac-228 | 6.16 hours |
Date of Discovery: 1899
Discoverer: Andre Debierne
Name Origin: From the Greek word aktinos (ray)
Uses: No uses known
Obtained From: extremely rare
Name: Lanthanum
Symbol: La
Atomic Number: 57
Atomic Mass: 138.9055 amu
Melting Point: 920.0 °C (1193.15 K, 1688.0 °F)
Boiling Point: 3469.0 °C (3742.15 K, 6276.2 °F)
Number of Protons/Electrons: 57
Number of Neutrons: 82
Classification: Rare Earth
Crystal Structure: Hexagonal
Density @ 293 K: 6.7 g/cm3
Color: white
![[Bohr Model of Lanthanum]](http://www.chemicalelements.com/bohr/b0057.gif) |
|
| Isotope | Half Life |
| La-134 | 6.5 minutes |
| La-137 | 6000.0 years |
| La-138 | 1.05E10 years |
| La-139 | Stable |
| La-140 | 1.67 days |
| La-141 | 3.9 hours |
| La-142 | 1.54 minutes |
Date of Discovery: 1839
Discoverer: Carl Mosander
Name Origin: From the Greek word lanthaneis (to lie hidden)
Uses: expensive camera lenses
Obtained From: monazite, bastnasite
Name: Hydrogen
Symbol: H
Atomic Number: 1
Atomic Mass: 1.00794 amu
Melting Point: -259.14 °C (14.009985 K, -434.45203 °F)
Boiling Point: -252.87 °C (20.280005 K, -423.166 °F)
Number of Protons/Electrons: 1
Number of Neutrons: 0
Classification: Non-metal
Crystal Structure: Hexagonal
Density @ 293 K: 0.08988 g/cm3
Color: colorless
![[Bohr Model of Hydrogen]](http://www.chemicalelements.com/bohr/b0001.gif) |
|
| Isotope | Half Life |
| H-1 | Stable |
| H-2 | Stable |
| H-3 | 12.3 years |
Date of Discovery: 1766
Discoverer: Henry Cavendish
Name Origin: From the Greek words hudôr (water) and gennan (generate)
Uses: Balloons, metal refining
Obtained From: mines, oil, gas wells
Name: Beryllium
Symbol: Be
Atomic Number: 4
Atomic Mass: 9.012182 amu
Melting Point: 1278.0 °C (1551.15 K, 2332.4 °F)
Boiling Point: 2970.0 °C (3243.15 K, 5378.0 °F)
Number of Protons/Electrons: 4
Number of Neutrons: 5
Classification: Alkaline Earth
Crystal Structure: Hexagonal
Density @ 293 K: 1.8477 g/cm3
Color: gray
![[Bohr Model of Beryllium]](http://www.chemicalelements.com/bohr/b0004.gif) |
|
| Isotope | Half Life |
| Be-7 | 53.3 days |
| Be-9 | Stable |
| Be-10 | 2600000.0 years |
Date of Discovery: 1798
Discoverer: Fredrich Wohler
Name Origin: From the mineral beryl
Uses: spacecraft, missiles, aircraft
Obtained From: beryl, chrysoberyl
Name: Boron
Symbol: B
Atomic Number: 5
Atomic Mass: 10.811 amu
Melting Point: 2300.0 °C (2573.15 K, 4172.0 °F)
Boiling Point: 2550.0 °C (2823.15 K, 4622.0 °F)
Number of Protons/Electrons: 5
Number of Neutrons: 6
Classification: Metalloid
Crystal Structure: Rhombohedral
Density @ 293 K: 2.34 g/cm3
Color: brownish
![[Bohr Model of Boron]](http://www.chemicalelements.com/bohr/b0005.gif) |
|
| Isotope | Half Life |
| B-10 | Stable |
| B-11 | Stable |
Date of Discovery: 1808
Discoverer: Sir Humphry Davy, J.L Gay-Lussac
Name Origin: From borax and carbon
Uses: heat resistant alloys
Obtained From: kernite
Name: Carbon
Symbol: C
Atomic Number: 6
Atomic Mass: 12.0107 amu
Melting Point: 3500.0 °C (3773.15 K, 6332.0 °F)
Boiling Point: 4827.0 °C (5100.15 K, 8720.6 °F)
Number of Protons/Electrons: 6
Number of Neutrons: 6
Classification: Non-metal
Crystal Structure: Hexagonal
Density @ 293 K: 2.62 g/cm3
Color: May be black
![[Bohr Model of Carbon]](http://www.chemicalelements.com/bohr/b0006.gif) |
|
| Isotope | Half Life |
| C-11 | 20.3 minutes |
| C-12 | Stable |
| C-13 | Stable |
| C-14 | 5730.0 years |
| C-15 | 2.5 seconds |
Date of Discovery: Known to the ancients
Discoverer: Unknown
Name Origin: From the Latin carbo (coal)
Uses: steel, filters
Obtained From: burning with insufficient oxygen
Name: Nitrogen
Symbol: N
Atomic Number: 7
Atomic Mass: 14.00674 amu
Melting Point: -209.9 °C (63.250008 K, -345.81998 °F)
Boiling Point: -195.8 °C (77.35 K, -320.44 °F)
Number of Protons/Electrons: 7
Number of Neutrons: 7
Classification: Non-metal
Crystal Structure: Hexagonal
Density @ 293 K: 1.2506 g/cm3
Color: colorless
![[Bohr Model of Nitrogen]](http://www.chemicalelements.com/bohr/b0007.gif) |
|
| Isotope | Half Life |
| N-13 | 9.97 minutes |
| N-14 | Stable |
| N-15 | Stable |
| N-16 | 7.13 seconds |
Date of Discovery: 1772
Discoverer: Daniel Rutherford
Name Origin: Greek
Uses: forms most of atmosphere
Obtained From: from liquid air
Name: Oxygen
Symbol: O
Atomic Number: 8
Atomic Mass: 15.9994 amu
Melting Point: -218.4 °C (54.750008 K, -361.12 °F)
Boiling Point: -183.0 °C (90.15 K, -297.4 °F)
Number of Protons/Electrons: 8
Number of Neutrons: 8
Classification: Non-metal
Crystal Structure: Cubic
Density @ 293 K: 1.429 g/cm3
Color: colorless
![[Bohr Model of Oxygen]](http://www.chemicalelements.com/bohr/b0008.gif) |
|
| Isotope | Half Life |
| O-15 | 122.2 seconds |
| O-16 | Stable |
| O-17 | Stable |
| O-18 | Stable |
Date of Discovery: 1774
Discoverer: Joseph Priestly
Name Origin: From the Greek words oxus (acid) and gennan (generate)
Uses: supports life
Obtained From: from liquid air
Name: Fluorine
Symbol: F
Atomic Number: 9
Atomic Mass: 18.998404 amu
Melting Point: -219.62 °C (53.530006 K, -363.31598 °F)
Boiling Point: -188.14 °C (85.01 K, -306.652 °F)
Number of Protons/Electrons: 9
Number of Neutrons: 10
Classification: Halogen
Crystal Structure: Cubic
Density @ 293 K: 1.696 g/cm3
Color: Greenish
![[Bohr Model of Fluorine]](http://www.chemicalelements.com/bohr/b0009.gif) |
|
| Isotope | Half Life |
| F-18 | 1.8 hours |
| F-19 | Stable |
Date of Discovery: 1886
Discoverer: Joseph Henri Moissan
Name Origin: From the Latin word fluo (flow)
Uses: Refrigerants
Obtained From: mineral fluorite
Name: Helium
Symbol: He
Atomic Number: 2
Atomic Mass: 4.002602 amu
Melting Point: -272.0 °C (1.15 K, -457.6 °F)
Boiling Point: -268.6 °C (4.549994 K, -451.48 °F)
Number of Protons/Electrons: 2
Number of Neutrons: 2
Classification: Noble Gas
Crystal Structure: Hexagonal
Density @ 293 K: 0.1785 g/cm3
Color: colorless
![[Bohr Model of Helium]](http://www.chemicalelements.com/bohr/b0002.gif) |
|
| Isotope | Half Life |
| He-3 | Stable |
| He-4 | Stable |
Date of Discovery: 1895
Discoverer: Sir William Ramsay
Name Origin: From the Greek word hêlios (sun)
Uses: balloons, deep sea diving
Obtained From: natural gas deposit, air
Properties of Carbon:
Nonmetal. A steady form of existence of an element of carbon (alpha-C). Are known also thermodynamic metastable forms: beta-C - diamond, (C2)n - carbyne, C60 and C70 - fullerens. Graphite - gray-black, with metal gloss, fat to the touch, soft, possesses conductivity. Chemically active (in difference from diamond and a carbyne). Reacts with hydrogen, oxygen, fluorine, sulfur, metals. Typical reducer. Reacts with water vapor, the concentrated nitric acid, oxides of metals. Receiving in the industry - pyrolysis of coal or hydrocarbons.
| Molar mass | g/mol | 12.011 |
| Density | g/cm3 | 2.27 |
| Melting point | °C | 3800 |
| Boiling point | °C | 4000 |
Сhemical reactions with Carbon:
C + H2O(steam) = CO + H2 (800-1000°C).
C + 2H2SO4(conc., hot) = CO2↑ + 2SO2↑ + 2H2O.
C + 4HNO3(conc., hot) = CO2↑ + 4NO2↑ + 2H2O.
C + 2H2 = CH4 (600°C, pressure, catalyst - Pt).
2C + H2 = C2H2 (1500-2000°C).
C + O2 = CO2 (600-700°C, burning on air).
2C + O2 = 2CO (over 1000°C).
C+ 2F2 = CF4 (over 900°C).
C + 2S = CS2 (700-800°C).
2C + N2 = C2N2 (on electric discharge).
2C + H2 + N2 = 2HCN (over 1800°C).
C + Si = SiC (1200-1300°C).
2C + Ca = CaC2 (550°C).
C + 2PbO = 2Pb + CO2 (600°C).
2C + Na2SO4 = Na2S + 2CO2 (600°C).
2C + Na2CO3 = 2Na + 3CO (900-1000°C).
3C + 8H2SO4(conc.) + 2K2Cr2O7(conc.) = 3CO2↑ + 2Cr2(SO4)3 + 2K2SO4 + 8H2O.
C → (HNO3 + H2SO4 + KClO3(KMnO4)) → CnO(graphite oxide) n=2-2.75.
2C + nF2 = 2CFn(graphite fluoride) n <1.12, 450°C.
8C + F2 = 2(C4+)(F-) (in the atm. HF).
(8+x)C + M = MC(8+x) (M = K, Rb, Cs; until 150°C).
C(diamond) → Time → C(graphite) (over 1200°C).
(C2)n(carbyne) → Time → 2nC(graphite) (2300°C).
Properties of Silicon:
Nonmetal. Large crystals - dark gray, with metal gloss, very firm, very fragile, opaque, the semiconductor at the room temperature. Amorphous in the form of very small crystals - white (without impurity) or brown (with impurity). Melts with reduction of volume. It is steady on air (formation of a protective oxidic film). In a crystal form - small reactionary ability. Doesn't react with water, acids (including also fluoric acid), hydrogen.
In an amorphous form - more active. Reacts with the concentrated fluoric acid, alkalis (it is partially transferred to solution even in the alkalescent environment), absorbs significant amounts of various gases (including hydrogen). Is oxidized by oxygen and halogens. Reacts with hydrogen halides, ammonia, hydrogen sulfide, metals sulfides by heating. It is extremely active in the melted state, reacts with alkalis, alkaline earth metals and other metals. Alloyed (but doesn't react) with beryllium, aluminum, gallium, indium, tin, antimony, zinc, silver, gold. An alloy with iron - ferrosilicium (12-90% of Si) is industrially important. The second for prevalence (after oxygen) an element in Earth lithosphere.
| Molar mass | g/mol | 28.086 |
| Density | g/cm3 | 2.33 |
| Melting point | °C | 1415 |
| Boiling point | °C | 3250 |
Methods for the preparation of Silicon:
SiH4 = Si + 2H2 (400-1000°C).
SiO2 + 2Mg = 2MgO + Si (800-900°C, in atm. of argon).
SiO2 →(air, Mg, -MgO, -Mg3N2) → Si, Mg2Si (700-900°C).
SiO2 + 5C(coke) + CaO = Si + CaC2 + 3CO (800-1000°C).
SiCl4 + 2H2 = Si + 4HCl (800°C).
SiCl4 + Li[AlH4] = Si + LiCl + AlCl3 + 2H2 (over 450°C).
SiCl4 + 4M = Si(amorphous) + 4MCl (M = Na, K; 600-700°C).
3Na2[SiF6] + 4Al = 3Si + 2Na3[AlF6] + 2AlF3 (700°C).
Na2[SiF6] → Electrolysis → Si↓(on cathode) + 2F2↑(on anode) + 2NaF (in the liquid NaF).
Сhemical reactions with Silicon:
Si(amorphous) + 2H2O(steam) = SiO2 + 2H2 (400-500°C).
Si(amorphous) + 4NaOH(conc.) = Na4SiO4 + 2H2↑.
Si(amorphous) + 6HF(conc.) = H2[SiF6] + 2H2↑.
Si + 4HF(gas) = SiF4 + 2H2 (40-100°C).
3Si + 18HF(conc.) + 4HNO3(conc.) = 3H2[SiF6] + 4NO↑ + 8H2O.
3Si + 18HF(conc.) + 2KClO3 = 3H2[SiF6] + 2KCl + 6H2O.
Si + 6HF(conc.) + KNO3 = H2[SiF6] + 2KNO2 + 2H2O.
Si + O2 = SiO2 (1200-1300°C).
Si + 2F2 = SiF4 (normal temp., burning in the fluorine).
Si + 2Cl2 = SiCl4 (340-420°C, under argon).
Si + 2Br2 = SiBr4 (620-700°C, under argon).
Si + 2I2 = SiI4 (750-810°C, under argon).
Si + 4HI = SiI4 + 2H2 (400-500°C).
Si + S = SiS (650-700°C, pressure).
Si + 2S = SiS2 (250-600°C).
Si + 2E = SiE2(800°C, E = Se, Te; under argon).
3Si + 2N2 = Si3N4 (1200-1500°C).
Si + C(graphite) = SiC (1200-1300°C).
Si + M = MSi (by alloying, M = Na, K, Rb, Cs).
Si + 2M = M2Si (by alloying, M = Mg, Ca).
Si + M = MSi, MSi2 (by alloying, M = Ca, Sr, Ba).
2Si + M = MSi2 (by alloying, M = La, Th, Ti, Cr, Mo, Mn, Fe).
3Si + 4NH3 = Si3N4 + 6H2 (1300-1500°C).
Si + 2H2S = SiS2 + 2H2 (1200-1300°C).
Light gray, fragile, solid metal. In damp air becomes covered by an oxidic film. Possesses small reactionary ability. Doesn't react with water, diluted acids, alkalis, hydrate of ammonia. Reacts with concentrated sulfuric and nitric acids. Brought into solution by hydrogen peroxide in the presence of alkalis. Reacts with oxygen, halogens, chalcogens, ammonia, hydrogen fluoride and hydrogen sulfide.
| Molar mass | g/mol | 72.610 |
| Density | g/cm3 | 5.350 |
| Melting point | °C | 937 |
| Boiling point | °C | 2850 |
Methods for the preparation of Germanium:
GeH4 = Ge + 2H2 (220-350°C).
GeO2 + 2H2 = Ge + 2H2O (600-650°C).
GeO2 + C(coke) = Ge + CO2 (500-600°C, in the atm. of hydrogen).
GeCl4 + 2H2 = Ge + 4HCl (700°C).
Сhemical reactions with Germanium:
Ge + 4H2SO4(conc.) = Ge(SO4)2 + 2SO2↑ + 4H2O.
Ge + 4HNO3(conc.) = GeO2↓ + 4NO2↑ + 2H2O (time).
3Ge + 4HNO3(conc.) + 12HCl(conc.) = 3GeCl4↓(liquid) + 4NO↑ + 8H2O.
Ge + 2NaOH(diluted) + 2H2O2 = Na2GeO3 + 3H2O.
Ge + 2NaOH(conc.) + 2H2O2 = Na2[Ge(OH)6].
Ge + 4H0(Mg, diluted H2SO4) = GeH4↑ (impurities of GenH2n+2, n>1).
Ge + O2 = GeO2 (over 700°C).
Ge + 2F2 = GeF4 (100°C, burning in the fluorine).
Ge + 2E2 = GeE4 (150-200°C, E = Cl; 350°C, E = Br; 560°C, E = I).
Ge + 2S = GeS (600-860°C).
Ge + S = GeS (over 1000°C).
Ge + E = GeE (600-700°C, E = Se, Te).
Ge + 2HF(liquid) = GeF2 + H2↑ (200°C, pressure).
Ge + H2S = GeS + H2 (600-800°C).
3Ge + 4NH3 = Ge3N4 + 6H2 (650-700°C).
Ge + CO2 = GeO + CO (700-900°C).
3Ge + 2SO2 = 2GeO2 + GeS2 (over 500°C).
Silver-white, very soft metal, viscous at the room temperature (beta modification). At a temperature below + 13,2°C it is scattered in gray powder (an alpha modification). Low-melting, high-boiling. Doesn't react with water, hydrate of ammonia. Shows amphoteric properties. Reacts with acids and concentrated alkalis. Is oxidized by halogens, oxygen, chalcogens.
| Molar mass | g/mol | 118.710 |
| Density | g/cm3 | 5.75(alpha),7.31(beta) |
| Melting point | °C | 231.9681 |
| Boiling point | °C | 2620 |
Methods for the preparation of Tin:
2SnO = SnO2 + Sn(liquid) (400°C).
2Na[Sn(OH)3](solution) = Sn↓ + Na2[Sn(OH)6] (normal temp.) .
2SnSO4 + 2H2O → Electrolysis → 2Sn↓(on cathode) + O2↑(on anode) + 2H2SO4.
SnCl2 + M = MCl2 + Sn (200-300°C, M = Mg, Zn).
3SnCl2 + 2Al = 2AlCl3 + 3Sn (250-300°C).
SnCl2(melt) → Electrolysis → Sn↓(on cathode) + Cl2↑(on anode).
Сhemical reactions with Tin:
Sn + 3HCl(conc.) = H[SnCl3] + H2↑ (time).
Sn + 2HCl(gas) = SnCl2 + H2 (150-250°C).
Sn + 2H2SO4(conc.) = SnSO4 + SO2↑ + 2H2O (time, impurity Sn(SO4)2).
Sn + 4HNO3(conc.) = SnO2↓ + 4NO2↑ + 2H2O (boiling).
5Sn + 12HNO3(diluted) = 5Sn(NO3)2 + N2↑ + 6H2O (time, impurity NO).
Sn + 10HNO3(high diluted) = 4Sn(NO3)2 + NH4NO3 + 3H2O (time).
Sn + NaOH(conc. cold) + 2H2O = Na[Sn(OH)3] + H2↑ (time).
Sn + 2NaOH(conc.) + 4H2O = Na2[Sn(OH)6] + 2H2↑ (boiling).
3Sn + 4HNO3(conc.) + 18HCl(conc.) = 3H2[SnCl6] + 4NO↑ + 8H2O.
Sn + O2 = SnO2 (200°C, burning on air).
Sn + 2E2 = SnE4 (until 100°C, E = F; normal temp., E = Cl, Br).
Sn + I2 = SnI2 (boiling in the diluted HCl).
Sn + 2I2 = SnI4 (boiling in the liquid CCl4).
Sn + E = SnE (900°C, E = S, Se, Te).
Sn + 2S = SnS2 (430-440°C, in the presence of NH4Cl).
Sn(powder) + CuSO4(solution) = SnSO4 + Cu↓ (in the diluted H2SO4).
Gray with a bluish shade, heavy, very soft, malleable, plastic metal. Low-melting, on air becomes covered by a steady oxidic film. Possesses small reactionary ability. It is passivated in water, hydrochloric acid, the diluted sulfuric acid, the concentrated nitric acid. Doesn't react with hydrate of ammonia. Weak reducer. Transferred to solution by the concentrated sulfuric acid, diluted nitric acid. Is oxidized by oxygen, halogens, chalcogens.
| Molar mass | g/mol | 207.2 |
| Density | g/cm3 | 11.337 |
| Melting point | °C | 327.502 |
| Boiling point | °C | 1745 |
Methods for the preparation of Lead:
Pb(NO3)2 + Zn = Pb↓ + Zn(NO3)2.
Pb(NO3)2 + 2H2O → Electrolysis → Pb↓(on cathode) + O2↑(on anode) + 2HNO3.
PbSO4(damp) + Zn(plate) = Pb↓(sponge) + ZnSO4.
PbCl2 + H2 = Pb + 2HCl (300-350°C).
PbS + H2 = Pb + H2S (400-600°C).
PbS + 2PbO = 3Pb + SO2 (800-900°C).
Сhemical reactions with Lead:
Pb + 3H2SO4(conc.>80%) = Pb(HSO4)2 + SO2↑ + 2H2O (30-50°C).
Pb + 2H2SO4(conc.) = PbSO4↓ + SO2↑ + 2H2O (boiling).
3Pb + 8HNO3(diluted, hot) = 3Pb(NO3)2 + 2NO↑ + 4H2O.
Pb + 2NaOH(conc.) + 2H2O = Na2[Pb(OH)4] + H2↑.
2Pb + O2 = 2PbO (over 600°C).
3Pb + 2O2 = (Pb2IIPbIV)O4 (400-500°C).
Pb + E2 = PbE2 (200-300°C, E = F, Cl, Br, I).
Pb + 2F2 = PbF4 (400-500°C).
Pb + 2HF = PbF2 + H2 (160°C).
Pb + E = PbE (800-1200°C, E = S, Se, Te).
2Pb(powder) + 2H2O + O2 = 2Pb(OH)2↓ (time).
2Pb + H2O + O2 + CO2 = Pb2CO3(OH)2↓ (time).
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