Difference between revisions of "Sulfur"

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[[File:Native_sulfur.jpg|thumb|220px|A native sulfur chunk of low purity]]
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{{Infobox element
'''Sulfur''' (or '''sulphur''') is a chemical element with the atomic number 16. It is a brittle, yellow nonmetal with a faint yet distinct odor. Sulfur is found commonly on Earth in elemental form and also in the form of [[sulfide]] and [[sulfate]] minerals.<ref>http://en.wikipedia.org/wiki/Sulfur</ref>
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<!-- top -->
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|image name=Native_sulfur_zts16.jpg
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|image alt=
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|image size=
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|image name comment=A native sulfur chunk of low purity
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|image name 2=
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|image alt 2=
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|image size 2=
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|image name 2 comment=
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<!-- General properties -->
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|name=Sulfur
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|symbol=S
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|pronounce=
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|pronounce ref=
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|pronounce comment=
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|pronounce 2=
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|alt name=Sulphur
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|alt names=
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|allotropes=More than 30
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|appearance=Yellow solid
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<!-- Periodic table -->
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|above=[[Oxygen|O]]
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|below=[[Selenium|Se]]
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|left=[[Phosphorus]]
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|right=[[Chlorine]]
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|number=16
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|atomic mass=32.065
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|atomic mass 2=
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|atomic mass ref=
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|atomic mass comment=
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|series=
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|series ref=
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|series comment=
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|series color=
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|group=16
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|group ref=
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|group comment=
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|period=3
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|period ref=
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|period comment=
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|block=p
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|block ref=
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|block comment=
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|electron configuration=[Ne] 3s<sup>2</sup> 3p<sup>4</sup>
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|electron configuration ref=
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|electron configuration comment=
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|electrons per shell=2, 8, 6
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|electrons per shell ref=
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|electrons per shell comment=
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<!-- Physical properties -->
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|physical properties comment=
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|color=Yellow
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|phase=Solid
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|phase ref=
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|phase comment=
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|melting point K=388.36
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|melting point C=115.21
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|melting point F=​239.38
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|melting point ref=
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|melting point comment=
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|boiling point K=717.8
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|boiling point C=444.6
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|boiling point F=832.3
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|boiling point ref=
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|boiling point comment=
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|sublimation point K=
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|sublimation point C=
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|sublimation point F=
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|sublimation point ref=
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|sublimation point comment=
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|density gplstp=
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|density gplstp ref=
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|density gplstp comment=
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|density gpcm3nrt=2.07
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|density gpcm3nrt ref=
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|density gpcm3nrt comment=(alpha)
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|density gpcm3nrt 2=1.96
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|density gpcm3nrt 2 ref=
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|density gpcm3nrt 2 comment=(beta)
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|density gpcm3nrt 3=1.92
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|density gpcm3nrt 3 ref=
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|density gpcm3nrt 3 comment=(gamma)
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|density gpcm3mp=1.819
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|density gpcm3mp ref=
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|density gpcm3mp comment=
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|density gpcm3bp=
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|density gpcm3bp ref=
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|density gpcm3bp comment=
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|molar volume=
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|molar volume unit =
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|molar volume ref=
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|molar volume comment=
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|triple point K=
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|triple point kPa=
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|triple point ref=
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|triple point comment=
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|triple point K 2=
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|triple point kPa 2=
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|triple point 2 ref=
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|triple point 2 comment=
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|critical point K=1314
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|critical point MPa=20.7
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|critical point ref=
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|critical point comment=
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|heat fusion=1.727
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|heat fusion ref=
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|heat fusion comment=(mono)
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|heat fusion 2=
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|heat fusion 2 ref=
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|heat fusion 2 comment=
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|heat vaporization=45
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|heat vaporization ref=
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|heat vaporization comment=(mono)
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|heat capacity=22.75
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|heat capacity ref=
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|heat capacity comment=
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|heat capacity 2=
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|heat capacity 2 ref=
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|heat capacity 2 comment=
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|vapor pressure 1=375
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|vapor pressure 10=408
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|vapor pressure 100=449
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|vapor pressure 1 k=508
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|vapor pressure 10 k=591
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|vapor pressure 100 k=717
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|vapor pressure ref=
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|vapor pressure comment=
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|vapor pressure 1 2=
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|vapor pressure 10 2=
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|vapor pressure 100 2=
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|vapor pressure 1 k 2=
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|vapor pressure 10 k 2=
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|vapor pressure 100 k 2=
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|vapor pressure 2 ref=
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|vapor pressure 2 comment=
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<!-- Atomic properties -->
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|atomic properties comment=
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|oxidation states='''6''', 5, '''4''', 3, '''2''', 1, -1, '''-2'''
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|oxidation states ref=
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|oxidation states comment=​(a strongly acidic oxide)
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|electronegativity=2.58
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|electronegativity ref=
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|electronegativity comment=
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|ionization energy 1=999.6
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|ionization energy 1 ref=
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|ionization energy 1 comment=
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|ionization energy 2=2252
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|ionization energy 2 ref=
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|ionization energy 2 comment=
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|ionization energy 3=3357
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|ionization energy 3 ref=
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|ionization energy 3 comment=
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|number of ionization energies=
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|ionization energy ref=
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|ionization energy comment=
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|atomic radius=
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|atomic radius ref=
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|atomic radius comment=
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|atomic radius calculated=
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|atomic radius calculated ref=
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|atomic radius calculated comment=
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|covalent radius=105±3
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|covalent radius ref=
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|covalent radius comment=
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|Van der Waals radius=180
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|Van der Waals radius ref=
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|Van der Waals radius comment=
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<!-- Miscellanea -->
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|crystal structure=
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|crystal structure prefix=
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|crystal structure ref=
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|crystal structure comment= Orthorhombic
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|crystal structure 2=
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|crystal structure 2 prefix=
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|crystal structure 2 ref=
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|crystal structure 2 comment=
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|speed of sound=
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|speed of sound ref=
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|speed of sound comment=
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|speed of sound rod at 20=
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|speed of sound rod at 20 ref=
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|speed of sound rod at 20 comment=
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|speed of sound rod at r.t.=
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|speed of sound rod at r.t. ref=
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|speed of sound rod at r.t. comment=
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|thermal expansion=
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|thermal expansion ref=
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|thermal expansion comment=
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|thermal expansion at 25=
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|thermal expansion at 25 ref=
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|thermal expansion at 25 comment=
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|thermal conductivity=0.205
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|thermal conductivity ref=
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|thermal conductivity comment=(amorphous)
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|thermal conductivity 2=
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|thermal conductivity 2 ref=
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|thermal conductivity 2 comment=
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|thermal diffusivity=
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|thermal diffusivity ref=
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|thermal diffusivity comment=
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|electrical resistivity=
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|electrical resistivity unit prefix=
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|electrical resistivity ref=
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|electrical resistivity comment=
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|electrical resistivity at 0=
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|electrical resistivity at 0 ref=
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|electrical resistivity at 0 comment=
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|electrical resistivity at 20=2×10<sup>15</sup>
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|electrical resistivity at 20 ref=
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|electrical resistivity at 20 comment=(amorphous)
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|band gap=
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|band gap ref=
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|band gap comment=
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|Curie point K=
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|Curie point ref=
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|Curie point comment=
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|magnetic ordering=Diamagnetic
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|magnetic ordering ref=
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|magnetic ordering comment=
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|tensile strength=
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|tensile strength ref=
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|tensile strength comment=
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|Young's modulus=
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|Young's modulus ref=
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|Young's modulus comment=
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|Shear modulus=
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|Shear modulus ref=
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|Shear modulus comment=
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|Bulk modulus=7.7
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|Bulk modulus ref=
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|Bulk modulus comment=
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|Poisson ratio=
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|Poisson ratio ref=
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|Poisson ratio comment=
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|Mohs hardness=2.0
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|Mohs hardness ref=
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|Mohs hardness comment=
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|Mohs hardness 2=
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|Mohs hardness 2 ref=
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|Mohs hardness 2 comment=
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|Vickers hardness=
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|Vickers hardness ref=
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|Vickers hardness comment=
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|Brinell hardness=
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|Brinell hardness ref=
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|Brinell hardness comment=
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|CAS number= 7704-34-9
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|CAS number ref=
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|CAS number comment=
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<!-- History -->
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|naming=
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|predicted by=
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|prediction date ref=
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|prediction date=
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|discovered by=China
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|discovery date ref=
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|discovery date=before 2000 BCE
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|first isolation by=
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|first isolation date ref=
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|first isolation date=
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|discovery and first isolation by=
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|named by=
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|named date ref=
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|named date=
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|history comment label=
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|history comment=
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<!-- Isotopes -->
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|isotopes=
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|isotopes comment=
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|engvar=
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}}
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'''Sulfur''' (or '''sulphur''') is a chemical element with the atomic number 16 and the symbol '''S'''. It is a brittle, yellow nonmetal with a very faint yet distinct odor. Sulfur is found commonly on Earth in elemental form and also in the form of [[sulfide]] and [[sulfate]] minerals. Pure sulfur is produced from volcanic emmisions.<ref>http://en.wikipedia.org/wiki/Sulfur</ref>
  
 
==Properties==
 
==Properties==
 
===Chemical===
 
===Chemical===
When burned in air, sulfur burns with a blue flame and [[sulfur dioxide]] gas is formed. Sulfur will also react readily with the air to form sulfur dioxide when it is molten. Sulfur reacts with [[chlorine]] gas to form sulfur chlorides, namely [[disulfur dichloride]] and [[sulfur dichloride]], and similarly reacts with [[bromine]] to form [[disulfur dibromide]].<ref>http://www.sciencemadness.org/talk/viewthread.php?tid=2467</ref>Sulfur can be digested in a strong solution of [[sodium hydroxide]] to form [[sodium sulfide]], a useful precursor to other sulfides.
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When burned in air, sulfur burns with a blue flame and [[sulfur dioxide]] gas is formed. Sulfur will also react readily with the air to form sulfur dioxide when it is molten. Sulfur reacts with [[chlorine]] gas to form sulfur chlorides, namely [[disulfur dichloride]] and [[sulfur dichloride]], and similarly reacts with [[bromine]] to form [[disulfur dibromide]].<ref>http://www.sciencemadness.org/talk/viewthread.php?tid=2467</ref>
[[File:Burning_sulfur.JPG|thumb|256px|Blue flames created by burning molten sulfur.]]
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===Physical===
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Sulfur can be digested in a strong solution of [[sodium hydroxide]] to form [[sodium sulfide]], a useful precursor to other sulfides.
Sulfur is a yellow solid under standard conditions. It is brittle; chunks of it can easily be broken by hand. Sulfur will melt at about 115°C, and is a viscous, blood red liquid when molten. Sulfur is insoluble in most common solvents, but is soluble in [[carbon disulfude]], benzene and toluene. There are over 30 [[Allotrope|allotropes]] of sulfur, more than any other element. The most common of these is α-octasulfur (S<sub>8</sub>), which is the form it is almost always seen in. When sulfur is melted and quickly cooled, amorphous polymeric sulfur is formed, which is light brown and has a rubbery consistency. It will only remain as this allotrope for a certain amount of time, varying from a few minutes to a few hours, eventually reverting back to octasulfur.<ref>Shakhashiri, ''Chemical Demonstrations, Vol. 1''</ref>
+
  
Sulfur is not soluble in water, but a few organic solvents like [[Xylene|xylene]] and [[Toluene|toluene]].
+
===Physical===
 +
Sulfur is a yellow solid under standard conditions. It is brittle; chunks of it can easily be broken by hand. Sulfur will melt at about 115 °C, and is a viscous, blood red liquid when molten. Sulfur is insoluble in most common solvents and water, but is soluble in [[carbon disulfide]], [[benzene]], [[toluene]] and [[xylene]]. There are over 30 [[allotrope]]s of sulfur, more than any other element. The most common of these is α-octasulfur (S<sub>8</sub>), which is the form it is almost always seen in. When sulfur is melted and quickly cooled, amorphous polymeric sulfur is formed, which is light brown and has a rubbery consistency. It will only remain as this allotrope for a certain amount of time, varying from a few minutes to a few hours, eventually reverting back to octasulfur.<ref>Shakhashiri, ''Chemical Demonstrations, Vol. 1''</ref>
  
 
==Availability==
 
==Availability==
[[File:Recrystallized_sulfur.jpg|thumb|300px|Sulfur recrystallized from hot xylene.]]Sulfur is the 10th most abundant element in the universe. Sulfur can be acquired at some garden stores as an insect repellant or fungicidal powder, although it is not usually very pure in these products, generally containing about 10% bentonite, a common clay. It can be extracted from the mixture by dissolving it in hot [[Toluene|toluene]] or [[Xylene|xylene]], in which sulfur is very soluble. Once the mixture cools, elemental sulfur will begin to precipitate, as while it's very soluble in hot solvent, it's not very soluble when cold. Because the melting point of sulfur (115.21 °C) is slightly higher than the boiling point of toluene (111°C) and slightly below xylene's boiling point (138-144°C), it is best to avoid heating the precipitated sulfur too much as it will melt. Vacuum drying the sulfur is recommended, especially if there's a large quantity of it. Melting also works, but requires grinding afterwards.
+
Sulfur is the 10th most abundant element in the universe. Sulfur can be acquired at some garden stores as an insect repellent or fungicidal powder, although it is not usually very pure in these products, generally containing about 10% bentonite, a common clay. It can be extracted from the mixture by dissolving it in hot [[toluene]] or [[xylene]], in which sulfur is very soluble. Once the mixture cools, elemental sulfur will begin to precipitate, as while it's very soluble in hot solvent, it's not very soluble when cold. Because the melting point of sulfur (115.21 °C) is slightly higher than the boiling point of toluene (111°C) and slightly below xylene's boiling point (138-144°C), it is best to avoid heating the precipitated sulfur too much as it will melt. Vacuum drying the sulfur is recommended, especially if there's a large quantity of it. Melting also works, but requires grinding afterwards.
  
 
Sulfur can be purchased in fairly pure form on the internet from chemical and industrial companies that are willing to sell to individuals.<ref>http://www.dudadiesel.com/search.php?query=sulfur</ref>
 
Sulfur can be purchased in fairly pure form on the internet from chemical and industrial companies that are willing to sell to individuals.<ref>http://www.dudadiesel.com/search.php?query=sulfur</ref>
  
Sulfur can also be obtained by the decomposition (through heat) of Cinnabar ([[Mercury(II) Sulfide]]), which forms [[Mercury|mercury]] and sulfur. This method is rather dangerous for any amateur, as it produces mercury vapor, which is highly toxic.
+
Sulfur can also be obtained by the decomposition (through heat) of cinnabar ([[mercury sulfide]]), which forms [[mercury]] and sulfur. This method is rather dangerous and complicated for any amateur, as it produces mercury vapor, which is highly toxic as well as an environmental hazard.
  
 
==Preparation==
 
==Preparation==
Sulfur can be prepared by reducing sulfur dioxide with hydrogen sulfide, process known as "Claus process", used in industry to remove hydrogen sulfide. This is a very useful way to neutralize hydrogen sulfide, as opposed to burning it, as it produces elemental sulfur and water and does not generate dangerous gases.
+
Sulfur can be prepared by reducing [[sulfur dioxide]] with [[hydrogen sulfide]], process known as "Claus process", used in industry to remove hydrogen sulfide. This is a very useful way to neutralize hydrogen sulfide, as opposed to burning it, as it produces elemental sulfur and water and does not generate dangerous gases.
  
Sulfur can be made from thioethers, which take the form R-S-R':
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Sulfur can also be made from thioethers, which take the form R-S-R':
 
:R-S-R + 2 H<sub>2</sub> → 2 RH + H<sub>2</sub>S
 
:R-S-R + 2 H<sub>2</sub> → 2 RH + H<sub>2</sub>S
 +
:2 H<sub>2</sub>S + SO<sub>2</sub> → 3 S + 2 H<sub>2</sub>O
  
 
==Projects==
 
==Projects==
*Making polymeric sulfur
+
*Make polymeric sulfur
*Making gunpowder
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*Make gunpowder
*Making sulfides
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*Make sulfides
*Making sulfuric acid
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*Make sulfuric acid
 
*Make aluminium sulfide
 
*Make aluminium sulfide
 
*Make hydrogen sulfide
 
*Make hydrogen sulfide
 
*Make [[thermate]]
 
*Make [[thermate]]
* Neutralize mercury and other toxic heavy metal spills
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*Neutralize mercury and other toxic heavy metal spills
 +
*Make sulfur chlorides and sulfur bromides
  
==Safety==
+
==Handling==
 +
===Safety===
 
Elemental sulfur is not toxic, but when burned or melted it produces highly toxic sulfur dioxide gas. Care must be taken to perform any experiments involving sulfur dioxide in a fume hood or an otherwise well-ventilated area.
 
Elemental sulfur is not toxic, but when burned or melted it produces highly toxic sulfur dioxide gas. Care must be taken to perform any experiments involving sulfur dioxide in a fume hood or an otherwise well-ventilated area.
  
 
Sulfides react with many acids to produce extremely toxic hydrogen sulfide, which smells like rotten eggs.
 
Sulfides react with many acids to produce extremely toxic hydrogen sulfide, which smells like rotten eggs.
 +
 +
===Storage===
 +
Sulfur should be kept in closed bottles away from any flame source or acidic vapors.
 +
 +
===Disposal===
 +
Burning sulfur is not recommended as it releases the toxic and corrosive sulfur dioxide. Although it may be dumped in the soil, large quantities will be oxidized by the microorganisms to sulfuric acid, which increases the acidity of the soil. Sulfur wastes are best disposed by mixing it with lime.<ref>http://environment.gov.ab.ca/info/library/7417.pdf</ref>
 +
 +
==Gallery==
 +
<gallery widths="200" position="center" columns="4" orientation="none">
 +
Recrystallized_sulfur_xylene.jpg|Sulfur recrystallized from hot xylene
 +
Burning_sulfur.jpg|Blue flames created by burning molten sulfur
 +
</gallery>
  
 
==References==
 
==References==
 
<references />
 
<references />
 
===Relevant Sciencemadness threads===
 
===Relevant Sciencemadness threads===
 +
*[http://www.sciencemadness.org/talk/viewthread.php?tid=65817 Sulfur purity]
 +
*[http://www.sciencemadness.org/talk/viewthread.php?tid=7260 What can I do with Sulfur?]
 +
 +
[[Category:Elements]]
 +
[[Category:Nonmetals]]
 +
[[Category:Chalcogens]]
 +
[[Category:P-block]]

Latest revision as of 18:25, 13 February 2021

Sulfur,  16S
Native sulfur zts16.jpg
A native sulfur chunk of low purity
General properties
Name, symbol Sulfur, S
Alternative name Sulphur
Allotropes More than 30
Appearance Yellow solid
Sulfur in the periodic table
O

S

Se
PhosphorusSulfurChlorine
Atomic number 16
Standard atomic weight (Ar) 32.065
Group, block , p-block
Period period 3
Electron configuration [Ne] 3s2 3p4
per shell
2, 8, 6
Physical properties
Yellow
Phase Solid
Melting point 388.36 K ​(115.21 °C, ​​239.38 °F)
Boiling point 717.8 K ​(444.6 °C, ​832.3 °F)
Density near r.t. 2.07 g/cm3 (alpha)
1.96 g/cm3 (beta)
1.92 g/cm3 (gamma)
when liquid, at  1.819 g/cm3
Critical point 1314 K, 20.7 MPa
Heat of fusion 1.727 kJ/mol (mono)
Heat of 45 kJ/mol (mono)
Molar heat capacity 22.75 J/(mol·K)
 pressure
Atomic properties
Oxidation states 6, 5, 4, 3, 2, 1, -1, -2 ​​(a strongly acidic oxide)
Electronegativity Pauling scale: 2.58
energies 1st: 999.6 kJ/mol
2nd: 2252 kJ/mol
3rd: 3357 kJ/mol
Covalent radius 105±3 pm
Van der Waals radius 180 pm
Miscellanea
Crystal structure ​Orthorhombic
Thermal conductivity 0.205 W/(m·K) (amorphous)
Electrical resistivity 2×1015 Ω·m (at 20 °C) (amorphous)
Magnetic ordering Diamagnetic
Bulk modulus 7.7 GPa
Mohs hardness 2.0
CAS Registry Number 7704-34-9
History
Discovery China (before 2000 BCE)
· references

Sulfur (or sulphur) is a chemical element with the atomic number 16 and the symbol S. It is a brittle, yellow nonmetal with a very faint yet distinct odor. Sulfur is found commonly on Earth in elemental form and also in the form of sulfide and sulfate minerals. Pure sulfur is produced from volcanic emmisions.[1]

Properties

Chemical

When burned in air, sulfur burns with a blue flame and sulfur dioxide gas is formed. Sulfur will also react readily with the air to form sulfur dioxide when it is molten. Sulfur reacts with chlorine gas to form sulfur chlorides, namely disulfur dichloride and sulfur dichloride, and similarly reacts with bromine to form disulfur dibromide.[2]

Sulfur can be digested in a strong solution of sodium hydroxide to form sodium sulfide, a useful precursor to other sulfides.

Physical

Sulfur is a yellow solid under standard conditions. It is brittle; chunks of it can easily be broken by hand. Sulfur will melt at about 115 °C, and is a viscous, blood red liquid when molten. Sulfur is insoluble in most common solvents and water, but is soluble in carbon disulfide, benzene, toluene and xylene. There are over 30 allotropes of sulfur, more than any other element. The most common of these is α-octasulfur (S8), which is the form it is almost always seen in. When sulfur is melted and quickly cooled, amorphous polymeric sulfur is formed, which is light brown and has a rubbery consistency. It will only remain as this allotrope for a certain amount of time, varying from a few minutes to a few hours, eventually reverting back to octasulfur.[3]

Availability

Sulfur is the 10th most abundant element in the universe. Sulfur can be acquired at some garden stores as an insect repellent or fungicidal powder, although it is not usually very pure in these products, generally containing about 10% bentonite, a common clay. It can be extracted from the mixture by dissolving it in hot toluene or xylene, in which sulfur is very soluble. Once the mixture cools, elemental sulfur will begin to precipitate, as while it's very soluble in hot solvent, it's not very soluble when cold. Because the melting point of sulfur (115.21 °C) is slightly higher than the boiling point of toluene (111°C) and slightly below xylene's boiling point (138-144°C), it is best to avoid heating the precipitated sulfur too much as it will melt. Vacuum drying the sulfur is recommended, especially if there's a large quantity of it. Melting also works, but requires grinding afterwards.

Sulfur can be purchased in fairly pure form on the internet from chemical and industrial companies that are willing to sell to individuals.[4]

Sulfur can also be obtained by the decomposition (through heat) of cinnabar (mercury sulfide), which forms mercury and sulfur. This method is rather dangerous and complicated for any amateur, as it produces mercury vapor, which is highly toxic as well as an environmental hazard.

Preparation

Sulfur can be prepared by reducing sulfur dioxide with hydrogen sulfide, process known as "Claus process", used in industry to remove hydrogen sulfide. This is a very useful way to neutralize hydrogen sulfide, as opposed to burning it, as it produces elemental sulfur and water and does not generate dangerous gases.

Sulfur can also be made from thioethers, which take the form R-S-R':

R-S-R + 2 H2 → 2 RH + H2S
2 H2S + SO2 → 3 S + 2 H2O

Projects

  • Make polymeric sulfur
  • Make gunpowder
  • Make sulfides
  • Make sulfuric acid
  • Make aluminium sulfide
  • Make hydrogen sulfide
  • Make thermate
  • Neutralize mercury and other toxic heavy metal spills
  • Make sulfur chlorides and sulfur bromides

Handling

Safety

Elemental sulfur is not toxic, but when burned or melted it produces highly toxic sulfur dioxide gas. Care must be taken to perform any experiments involving sulfur dioxide in a fume hood or an otherwise well-ventilated area.

Sulfides react with many acids to produce extremely toxic hydrogen sulfide, which smells like rotten eggs.

Storage

Sulfur should be kept in closed bottles away from any flame source or acidic vapors.

Disposal

Burning sulfur is not recommended as it releases the toxic and corrosive sulfur dioxide. Although it may be dumped in the soil, large quantities will be oxidized by the microorganisms to sulfuric acid, which increases the acidity of the soil. Sulfur wastes are best disposed by mixing it with lime.[5]

Gallery

References

  1. http://en.wikipedia.org/wiki/Sulfur
  2. http://www.sciencemadness.org/talk/viewthread.php?tid=2467
  3. Shakhashiri, Chemical Demonstrations, Vol. 1
  4. http://www.dudadiesel.com/search.php?query=sulfur
  5. http://environment.gov.ab.ca/info/library/7417.pdf

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