Difference between revisions of "Lithium"

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'''Lithium''' is a an alkali metal, the lightest metal and least dense solid element at room temperature, with the atomic number 3. It is soft, silvery-white metal, with a density of 534 kg/m<sup>3</sup>. It is highly reactive, and it's usually stored in mineral oil. However, because of its extremely low density, it floats in mineral oil, storing the metal proves to be difficult.
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{{Infobox element
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<!-- top -->
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|image name= Lithium metal sheet from an Energizer battery by NurdRage.jpg
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|image alt=
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|image size=300
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|image name comment=Lithium metal from an Energizer battery
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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=Lithium
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|symbol=Li
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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=
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|alt names=
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|allotropes=
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|appearance=White-silvery metal
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<!-- Periodic table -->
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|above=[[Hydrogen|H]]
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|below=[[Sodium|Na]]
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|left=[[Helium]]
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|right=[[Beryllium]]
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|number=3
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|atomic mass=6.94
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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=Alkali metals
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|series ref=
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|series comment=
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|series color=
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|group=1
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|group ref=
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|group comment=I
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|period=2
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|period ref=
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|period comment=
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|block=s
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|block ref=
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|block comment=
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|electron configuration= [He] 2s<sup>1</sup>
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|electron configuration ref=
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|electron configuration comment=
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|electrons per shell=2, 1
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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=Silvery-white
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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=453.65
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|melting point C=180.5
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|melting point F=356.9
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|melting point ref=
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|melting point comment=
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|boiling point K=1603
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|boiling point C=1330
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|boiling point F=2426
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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=0.534
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|density gpcm3nrt ref=
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|density gpcm3nrt comment=
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|density gpcm3nrt 2=
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|density gpcm3nrt 2 ref=
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|density gpcm3nrt 2 comment=
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|density gpcm3nrt 3=
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|density gpcm3nrt 3 ref=
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|density gpcm3nrt 3 comment=
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|density gpcm3mp=0.512
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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=3220
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|critical point MPa=67
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|critical point ref=(extrapolated)
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|critical point comment=
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|heat fusion=3.00
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|heat fusion ref=
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|heat fusion comment=
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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=136
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|heat vaporization ref=
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|heat vaporization comment=
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|heat capacity=24.86
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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=797
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|vapor pressure 10=885
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|vapor pressure 100=995
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|vapor pressure 1 k=1144
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|vapor pressure 10 k=1337
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|vapor pressure 100 k=1610
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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=+1
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|oxidation states ref=
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|oxidation states comment=(a strongly basic oxide)
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|electronegativity=0.98
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|electronegativity ref=
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|electronegativity comment=
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|ionization energy 1=520.2
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|ionization energy 1 ref=
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|ionization energy 1 comment=
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|ionization energy 2=7298.1
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|ionization energy 2 ref=
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|ionization energy 2 comment=
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|ionization energy 3=11815
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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=152
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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=128±7
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|covalent radius ref=
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|covalent radius comment=
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|Van der Waals radius=182
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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=body-centered cubic
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|crystal structure prefix=
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|crystal structure ref=
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|crystal structure comment=
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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=6000
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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=46
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|thermal expansion at 25 ref=
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|thermal expansion at 25 comment=
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|thermal conductivity=84.8
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|thermal conductivity ref=
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|thermal conductivity comment=
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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=9.28·10<sup>-8</sup>
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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=
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|electrical resistivity at 20 ref=
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|electrical resistivity at 20 comment=
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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=Paramagnetic
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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=4.9
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|Young's modulus ref=
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|Young's modulus comment=
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|Shear modulus=4.2
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|Shear modulus ref=
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|Shear modulus comment=
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|Bulk modulus=11
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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=0.6
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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=5
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|Brinell hardness ref=
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|Brinell hardness comment=
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|CAS number=7439-93-2
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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=Johan August Arfwedson
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|discovery date ref=
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|discovery date=1817
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|first isolation by= William Thomas Brande
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|first isolation date ref=
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|first isolation date=1821
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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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'''Lithium''' is a an [[alkali metal]], the lightest metal and least dense solid element at room temperature, with the atomic number 3 and symbol '''Li'''. It is soft, silvery-white metal, with a density of 534 kg/m<sup>3</sup>. It is highly reactive, and it is usually stored in [[[mineral oil]]. However, because of its extremely low density, it floats in mineral oil, storing the metal proves to be difficult.
  
 
==Properties==
 
==Properties==
 
===Chemical===
 
===Chemical===
−
Lithium, like all the alkali metals reacts violently with water, releasing hydrogen and can ignite, but this reaction is slightly less violent than the other alkali metals. In open air, it quickly forms a layer of oxide as well as nitride, and if the air also contains water vapors and [[carbon dioxide]], [[lithium hydroxide]] and [[lithium carbonate]]. Lithium will burn in air, and it tends to burn with a red-crimson flame. As noted by NurdRage, in his video where he extracted lithium from an energizer battery, this flame is incredibly bright, so welding goggles should be used if this reaction is attempted. Such fires are difficult to extinguish, requiring dry powder extinguishers (class D).
+
Lithium, like all the alkali metals reacts violently with water, releasing hydrogen and can ignite, but this reaction is slightly less violent than the other alkali metals.  
  
−
Lithium is also a strong reducing agent. It is also used in organometallic synthesis in the form of organolithium compounds such as [[n-butyllithium]] and [[tert-butyllithium]], although they are extremely rarely used by the amateur chemist, mainly because they're very dangerous (pyrophoric and caustic). Molten lithium is probably the most powerful reducing agent known, and will explode on contact with almost anything non-metallic, including wood and glass.
+
: Li + H<sub>2</sub>O → LiOH + ½ H<sub>2</sub>
  
−
Contrary to popular belief, lithium, not cesium, is the most reactive element on the periodic table. It has the lowest reduction potential in aqueous solution, and gram-for-gram (as well as mole-for-mole) has a higher energy content than [[cesium]].
+
In open air, it quickly forms a layer of oxide as well as nitride, and if the air also contains [[water]] vapors and [[carbon dioxide]], [[lithium hydroxide]] and [[lithium carbonate]].
  
−
Lithium metal is able to dissolve in anhydrous [[Ammonia|ammonia]] and [[ethylenediamine]], forming its electride salt.
+
: 4 Li + O<sub>2</sub> → 2 Li<sub>2</sub>O
 +
: 6 Li + 2 N<sub>2</sub> → 2 Li<sub>3</sub>N<sub>2</sub>
 +
 
 +
Lithium will burn in air, and it tends to burn with a red-crimson flame. As noted by NurdRage in his video where he extracted lithium from an energizer battery, this flame is incredibly bright, so welding goggles should be used if this reaction is attempted. Such fires are difficult to extinguish, requiring dry powder extinguishers (class D).
 +
 
 +
Lithium is also a strong reducing agent. It is also used in organometallic synthesis in the form of organolithium compounds such as [[n-butyllithium]] and [[tert-butyllithium]], although they are extremely rarely used by the amateur chemist, mainly because they're very dangerous (pyrophoric and caustic). Molten lithium is probably the most powerful reducing agent known, and will explode on contact with almost anything non-metallic, including wood, glass and concrete. It is the only alkali metal that cannot be safely melted in a glass container, as it reacts exothermically with glass almost immediately.<ref>https://www.youtube.com/watch?v=GE-NkVqUiHs</ref>
 +
 
 +
Contrary to popular belief, lithium, not cesium, is the most reactive element on the periodic table. It has the lowest reduction potential in aqueous solution, and gram-for-gram (as well as mole-for-mole) has a higher energy content than [[caesium|cesium]].
 +
 
 +
Lithium metal can dissolve in anhydrous [[ammonia]] and [[ethylenediamine]], forming its electride salt.
  
 
===Physical===
 
===Physical===
−
Lithium is a soft, silver-white metal. It is soft enough to be cut with a knife.  
+
Lithium is a soft, silver-white metal. It is soft enough to be cut with a knife.
−
Lithium has the highest specific heat capacity of any solid element, 3.58 kJ/(kg*K), the highest of all solids. Because of this, lithium metal is often used in coolants for heat transfer applications.<ref>http://hilltop.bradley.edu/~spost/THERMO/solidcp.pdf</ref>
+
 +
Lithium has the highest specific heat capacity of any solid element, 3.58 kJ/(kg·K), the highest of all solids. Because of this, lithium metal is often used in coolants for heat transfer applications.<ref>http://hilltop.bradley.edu/~spost/THERMO/solidcp.pdf</ref>
  
−
Lithium has a density of only 534 kg/m<sup>3</sup>, making it the lightest metal and solid element at standard conditions. It is lighter than any hydrocarbon oils, which causes the metal to float in the oil is stored. The only organic hydrocarbons lighter than lithium are liquid methane (465 kg/m<sup>3</sup>), liquid propane (493.5 kg/m<sup>3</sup>), liquid propylene (514.4 kg/m<sup>3</sup>).<ref>http://www.engineeringtoolbox.com/liquids-densities-d_743.html</ref> Since these solvents are liquid only at very low temperatures or under high pressure, storing lithium in them is impractical.
+
Lithium has a density of only 534 kg/m<sup>3</sup>, making it the lightest metal and solid element at standard conditions. It is lighter than any hydrocarbon oil, which causes the metal to float in the oil is stored. The only organic hydrocarbons lighter than lithium are liquid methane (465 kg/m<sup>3</sup>), liquid propane (493.5 kg/m<sup>3</sup>), liquid propylene (514.4 kg/m<sup>3</sup>).<ref>http://www.engineeringtoolbox.com/liquids-densities-d_743.html</ref> Since these solvents are liquid only at very low temperatures or under high pressure, storing lithium in them is impractical.
  
−
In addition, lithium has the highest melting point of all alkali metals, at roughly 180 degrees Celsius. Because of this, it is difficult to melt under oil (a common tactic for removing tarnish from the other alkali metals). It also has a high boiling point, of 1330 °C.
+
In addition, lithium has the highest melting point of all alkali metals, at roughly 180 degrees Celsius. This  makes it difficult to melt it under oil (a common tactic for removing tarnish from the other alkali metals). Molten lithium is extremely reactive and will react with almost all ceramic materials, therefore lithium is only melted in crucibles made of special metals, such as molybdenum. It also has a high boiling point, of 1330 °C.
  
 
Lithium dissolves in liquid ammonia.<ref>http://pubs.acs.org/doi/abs/10.1021/j150343a013</ref>
 
Lithium dissolves in liquid ammonia.<ref>http://pubs.acs.org/doi/abs/10.1021/j150343a013</ref>
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==Preparation==
 
==Preparation==
−
Industrially, elemental lithium is produced electrolytically from a mixture of fused 55% [[lithium chloride]] and 45% [[potassium chloride]] at about 450 <sup>o</sup>C. As molten lithium is highly reactive, this process should be performed in instalations made of corrosion resistant alloys.
+
Industrially, elemental lithium is produced electrolytically from a mixture of fused 55% [[lithium chloride]] and 45% [[potassium chloride]] at about 450 <sup>o</sup>C.<ref>https://www.youtube.com/watch?v=cIII542y0C8</ref>
 +
 
 +
As molten lithium is highly reactive, this process should be performed in installations made of corrosion resistant alloys and under inert atmosphere, such as argon.
  
 
==Projects==
 
==Projects==
−
*Buthyllithium synthesis (DANGER! PYROPHORIC!)
+
*Butyllithium synthesis (pyrophoric)
−
*Lanthanide extraction
+
*Isolation of reactive metals, including lanthanides
 
*Lithium lubricating grease
 
*Lithium lubricating grease
 
*Aluminium-lithium alloys
 
*Aluminium-lithium alloys
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==Safety==
 
==Safety==
 
===Handling===
 
===Handling===
−
Contrary to what one may think, '''NEVER HANDLE LITHIUM WITH GLOVES OF ANY KIND.''' You can easily tell if your hands are wet, but not if your gloves are wet, and if you get lithium wet (or it ignites) while handling it with gloves, it will burn through your gloves (and potentially explode) faster than you can remove them.<ref>Thunderf00t knows what he's talking about. https://www.youtube.com/watch?v=Nn3M1hfjxMU</ref> Pliers are another safe option. Glove boxes are also very good for work with lithium.
+
Contrary to what one may think, '''NEVER HANDLE LITHIUM WITH GLOVES OF ANY KIND!''' You can easily tell if your hands are wet, but not if your gloves are wet, and if you get lithium wet (or it ignites) while handling it with gloves, it will burn through your gloves (and potentially explode) faster than you can remove them.<ref>Thunderf00t knows what he's talking about. https://www.youtube.com/watch?v=Nn3M1hfjxMU</ref> Pliers are another safe option. Glove boxes are also very good for work with lithium.
  
 
===Toxicity===
 
===Toxicity===
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===Storage===
 
===Storage===
−
Like every other alkali metal, it must be kept away from any fire source. Keeping lithium under mineral oil is difficult because lithium floats on mineral oil. The best solution is to keep it in an inert argon atmosphere (nitrogen will react to form lithium nitride). [[Sulfur hexafluoride]] can also be used, except when it's molten (it will react).
+
Like every other alkali metal, it must be kept away from any fire source. Keeping lithium under mineral oil is difficult because lithium floats on mineral oil, though a small rock may be used to keep it down. The best solution is to keep it in an inert argon atmosphere (nitrogen will react to form lithium nitride). [[Sulfur hexafluoride]] can also be used, except when it's molten (it will react).
  
 
===Disposal===
 
===Disposal===
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<references />
 
<references />
 
===Relevant Sciencemadness threads===
 
===Relevant Sciencemadness threads===
 +
*[http://www.sciencemadness.org/talk/viewthread.php?tid=156445 What are some interesting uses for lithium metal]
 
*[http://www.sciencemadness.org/talk/viewthread.php?tid=32593 Lithium electride in ethylenediamine]
 
*[http://www.sciencemadness.org/talk/viewthread.php?tid=32593 Lithium electride in ethylenediamine]
 +
*[http://www.sciencemadness.org/talk/viewthread.php?tid=156454 Making Lithium Powder]
 +
 
[[Category:Elements]]
 
[[Category:Elements]]
−
[[Category:Reducing agents]]
 
 
[[Category:Metals]]
 
[[Category:Metals]]
 
[[Category:Alkali metals]]
 
[[Category:Alkali metals]]
 +
[[Category:Reducing agents]]
 +
[[Category:Materials unstable in acidic solution]]
 
[[Category:Materials that react with water]]
 
[[Category:Materials that react with water]]
 
[[Category:Materials that react with glass]]
 
[[Category:Materials that react with glass]]
−
[[Category:DEA SS List]]
 
−
[[Category:Materials unstable in acidic solution]]
 
 
[[Category:S-block]]
 
[[Category:S-block]]
 +
[[Category:DEA SS List]]
 +
[[Category:Air-sensitive materials]]

Latest revision as of 18:05, 23 November 2022

Lithium,  3Li
Lithium metal sheet from an Energizer battery by NurdRage.jpg
Lithium metal from an Energizer battery
General properties
Name, symbol Lithium, Li
Appearance White-silvery metal
Lithium in the periodic table
H
↑
Li
↓
Na
Helium ← Lithium → Beryllium
Atomic number 3
Standard atomic weight (Ar) 6.94
Group, block I; s-block
Period period 2
Electron configuration [He] 2s1
per shell
 2, 1
Physical properties
Silvery-white
Phase Solid
Melting point 453.65 K ​(180.5 °C, ​356.9 °F)
Boiling point 1603 K ​(1330 °C, ​2426 °F)
Density near r.t. 0.534 g/cm3
when liquid, at  0.512 g/cm3
Critical point 3220 K, 67 MPa(extrapolated)
Heat of fusion 3.00 kJ/mol
Heat of 136 kJ/mol
Molar heat capacity 24.86 J/(mol·K)
 pressure
Atomic properties
Oxidation states +1 ​(a strongly basic oxide)
Electronegativity Pauling scale: 0.98
energies 1st: 520.2 kJ/mol
2nd: 7298.1 kJ/mol
3rd: 11815 kJ/mol
Atomic radius empirical: 152 pm
Covalent radius 128±7 pm
Van der Waals radius 182 pm
Miscellanea
Crystal structure ​
Speed of sound thin rod 6000 m/s (at 20 °C)
Thermal expansion 46 µm/(m·K) (at 25 °C)
Thermal conductivity 84.8 W/(m·K)
Electrical resistivity 9.28·10-8 Ω·m
Magnetic ordering Paramagnetic
Young's modulus 4.9 GPa
Shear modulus 4.2 GPa
Bulk modulus 11 GPa
Mohs hardness 0.6
Brinell hardness 5 MPa
CAS Registry Number 7439-93-2
History
Discovery Johan August Arfwedson (1817)
First isolation William Thomas Brande (1821)
· references

Lithium is a an alkali metal, the lightest metal and least dense solid element at room temperature, with the atomic number 3 and symbol Li. It is soft, silvery-white metal, with a density of 534 kg/m3. It is highly reactive, and it is usually stored in [[[mineral oil]]. However, because of its extremely low density, it floats in mineral oil, storing the metal proves to be difficult.

Properties

Chemical

Lithium, like all the alkali metals reacts violently with water, releasing hydrogen and can ignite, but this reaction is slightly less violent than the other alkali metals.

Li + H2O → LiOH + ½ H2

In open air, it quickly forms a layer of oxide as well as nitride, and if the air also contains water vapors and carbon dioxide, lithium hydroxide and lithium carbonate.

4 Li + O2 → 2 Li2O
6 Li + 2 N2 → 2 Li3N2

Lithium will burn in air, and it tends to burn with a red-crimson flame. As noted by NurdRage in his video where he extracted lithium from an energizer battery, this flame is incredibly bright, so welding goggles should be used if this reaction is attempted. Such fires are difficult to extinguish, requiring dry powder extinguishers (class D).

Lithium is also a strong reducing agent. It is also used in organometallic synthesis in the form of organolithium compounds such as n-butyllithium and tert-butyllithium, although they are extremely rarely used by the amateur chemist, mainly because they're very dangerous (pyrophoric and caustic). Molten lithium is probably the most powerful reducing agent known, and will explode on contact with almost anything non-metallic, including wood, glass and concrete. It is the only alkali metal that cannot be safely melted in a glass container, as it reacts exothermically with glass almost immediately.[1]

Contrary to popular belief, lithium, not cesium, is the most reactive element on the periodic table. It has the lowest reduction potential in aqueous solution, and gram-for-gram (as well as mole-for-mole) has a higher energy content than cesium.

Lithium metal can dissolve in anhydrous ammonia and ethylenediamine, forming its electride salt.

Physical

Lithium is a soft, silver-white metal. It is soft enough to be cut with a knife.

Lithium has the highest specific heat capacity of any solid element, 3.58 kJ/(kg·K), the highest of all solids. Because of this, lithium metal is often used in coolants for heat transfer applications.[2]

Lithium has a density of only 534 kg/m3, making it the lightest metal and solid element at standard conditions. It is lighter than any hydrocarbon oil, which causes the metal to float in the oil is stored. The only organic hydrocarbons lighter than lithium are liquid methane (465 kg/m3), liquid propane (493.5 kg/m3), liquid propylene (514.4 kg/m3).[3] Since these solvents are liquid only at very low temperatures or under high pressure, storing lithium in them is impractical.

In addition, lithium has the highest melting point of all alkali metals, at roughly 180 degrees Celsius. This makes it difficult to melt it under oil (a common tactic for removing tarnish from the other alkali metals). Molten lithium is extremely reactive and will react with almost all ceramic materials, therefore lithium is only melted in crucibles made of special metals, such as molybdenum. It also has a high boiling point, of 1330 °C.

Lithium dissolves in liquid ammonia.[4]

Availability

Lithium can be extracted from lithium batteries, as shown by NurdRage is his video. It comes as a long sheet of lithium metal, that quickly tarnishes in air. It's risky, as the battery can short and overheat. One safer method is to use a pipe cutter and split the battery case in the middle. Larger quantities of lithium can be bought from Galliumsource, though it's pretty expensive (150$/100g). Due to its low molar mass, one may get away with using much smaller amounts of lithium than expected.

In recent years, some jurisdictions in United States limit the sale of lithium batteries, as elemental lithium can be used to reduce pseudoephedrine and ephedrine to the illegal drug methamphetamine.

Preparation

Industrially, elemental lithium is produced electrolytically from a mixture of fused 55% lithium chloride and 45% potassium chloride at about 450 oC.[5]

As molten lithium is highly reactive, this process should be performed in installations made of corrosion resistant alloys and under inert atmosphere, such as argon.

Projects

  • Butyllithium synthesis (pyrophoric)
  • Isolation of reactive metals, including lanthanides
  • Lithium lubricating grease
  • Aluminium-lithium alloys
  • Cesium synthesis by distillation (DANGER!)

Safety

Handling

Contrary to what one may think, NEVER HANDLE LITHIUM WITH GLOVES OF ANY KIND! You can easily tell if your hands are wet, but not if your gloves are wet, and if you get lithium wet (or it ignites) while handling it with gloves, it will burn through your gloves (and potentially explode) faster than you can remove them.[6] Pliers are another safe option. Glove boxes are also very good for work with lithium.

Toxicity

Breathing lithium dust or lithium compounds irritate the nose and throat, while higher exposure can cause a buildup of fluid in the lungs, leading to pulmonary edema. Acetic acid a good neutralizing agent.

Storage

Like every other alkali metal, it must be kept away from any fire source. Keeping lithium under mineral oil is difficult because lithium floats on mineral oil, though a small rock may be used to keep it down. The best solution is to keep it in an inert argon atmosphere (nitrogen will react to form lithium nitride). Sulfur hexafluoride can also be used, except when it's molten (it will react).

Disposal

Lithium compounds are not particularly dangerous to the environment, but it's recommended to recycle them when possible.

References

  1. ↑ https://www.youtube.com/watch?v=GE-NkVqUiHs
  2. ↑ http://hilltop.bradley.edu/~spost/THERMO/solidcp.pdf
  3. ↑ http://www.engineeringtoolbox.com/liquids-densities-d_743.html
  4. ↑ http://pubs.acs.org/doi/abs/10.1021/j150343a013
  5. ↑ https://www.youtube.com/watch?v=cIII542y0C8
  6. ↑ Thunderf00t knows what he's talking about. https://www.youtube.com/watch?v=Nn3M1hfjxMU

Relevant Sciencemadness threads

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