Difference between revisions of "Nitrogen"

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[[File:Nitrogen_discharge_tube.jpg|thumb|Nitrogen discharge tube.]]
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{{Infobox element
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<!-- top -->
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|image name=Nitrogen_discharge_tube.jpg
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|image alt=
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|image size=
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|image name comment=Nitrogen discharge tube.
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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=Nitrogen
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|symbol=N
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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=Azote
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|alt names=
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|allotropes=
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|appearance=Colorless gas, liquid or solid
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<!-- Periodic table -->
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|above=-
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|below=[[Phosphorus|P]]
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|left=[[Carbon]]
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|right=[[Oxygen]]
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|number=7
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|atomic mass=14.007
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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=15
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|group ref=
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|group comment= (pnictogens)
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|period=2
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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=[He] 2s<sup>2</sup> 2p<sup>3</sup>
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|electron configuration ref=
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|electron configuration comment=
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|electrons per shell=2, 5
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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=Colorless
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|phase=Gas
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|phase ref=
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|phase comment=
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|melting point K=63.15
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|melting point C=−210.0
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|melting point F=−346.0
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|melting point ref=
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|melting point comment=
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|boiling point K=77.355
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|boiling point C=−195.795
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|boiling point F=−320.431
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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=1.251
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|density gplstp ref=
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|density gplstp comment=
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|density gpcm3nrt=
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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=
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|density gpcm3mp ref=
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|density gpcm3mp comment=
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|density gpcm3bp=0.808
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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=63.151
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|triple point kPa=12.52
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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=126.192
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|critical point MPa=3.3958
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|critical point ref=
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|critical point comment=
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|heat fusion=0.72
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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=5.56
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|heat vaporization ref=
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|heat vaporization comment=
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|heat capacity=29.124
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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=37
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|vapor pressure 10=41
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|vapor pressure 100=46
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|vapor pressure 1 k=53
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|vapor pressure 10 k=62
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|vapor pressure 100 k=77
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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='''5''', 4, '''3''', 2, 1, −1, −2, '''−3'''
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|oxidation states ref=
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|oxidation states comment=(a strongly acidic oxide)
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|electronegativity=3.04
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|electronegativity ref=
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|electronegativity comment=
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|ionization energy 1=1402.3
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|ionization energy 1 ref=
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|ionization energy 1 comment=
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|ionization energy 2=2856.0
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|ionization energy 2 ref=
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|ionization energy 2 comment=
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|ionization energy 3=4578.1
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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=71±1
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|covalent radius ref=
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|covalent radius comment=
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|Van der Waals radius=155
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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=Hexagonal
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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=353
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|speed of sound ref=
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|speed of sound comment=(gas, at 27 °C)
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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=25.83×10<sup>−3</sup>
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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=
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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=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=
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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=
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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=17778-88-0<br>7727-37-9 (N<sub>2</sub>)
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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=Daniel Rutherford
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|discovery date ref=
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|discovery date=1772
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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= Jean-Antoine Chaptal
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|named date ref=
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|named date=1790
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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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}}
 
'''Nitrogen''' is a chemical element with symbol '''N''' and atomic number 7. Nitrogen is a common element in the universe, estimated at about seventh in total abundance in our galaxy and the Solar System. On Earth, the element is primarily found as the gas molecule; it forms about 78% of Earth's atmosphere. The element nitrogen was discovered as a separable component of air, by Scottish physician Daniel Rutherford, in 1772.
 
'''Nitrogen''' is a chemical element with symbol '''N''' and atomic number 7. Nitrogen is a common element in the universe, estimated at about seventh in total abundance in our galaxy and the Solar System. On Earth, the element is primarily found as the gas molecule; it forms about 78% of Earth's atmosphere. The element nitrogen was discovered as a separable component of air, by Scottish physician Daniel Rutherford, in 1772.
  
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Nitrogen is a nonmetal, with an electronegativity of 3.04. It has five electrons in its outer shell and is, therefore, trivalent in most compounds. The triple bond in molecular nitrogen (N<sub>2</sub>) is one of the strongest. The resulting difficulty of converting nitrogen into other compounds, and the ease (and associated high energy release) of converting nitrogen compounds into elemental N<sub>2</sub>, have dominated the role of nitrogen in both nature and human economic activities.
 
Nitrogen is a nonmetal, with an electronegativity of 3.04. It has five electrons in its outer shell and is, therefore, trivalent in most compounds. The triple bond in molecular nitrogen (N<sub>2</sub>) is one of the strongest. The resulting difficulty of converting nitrogen into other compounds, and the ease (and associated high energy release) of converting nitrogen compounds into elemental N<sub>2</sub>, have dominated the role of nitrogen in both nature and human economic activities.
  
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While nitrogen is relative inert, [[magnesium]], [[lithium]] will burn in a nitrogen atmosphere.
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While nitrogen is relative inert, certain metals such as [[magnesium]] or [[lithium]] will burn in a nitrogen atmosphere.
  
 
===Physical===
 
===Physical===
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Nitrogen can be isolated from air via reduction of oxygen with [[copper]] turning or other reducing agents (except metals that will burn in a nitrogen atmosphere, such as [[lithium]], [[magnesium]] or [[titanium]]). The purified gas will contain ~1% [[argon]]. Smaller, but purer amounts of nitrogen can also be obtained by decomposing [[sodium azide]]. [[Nitrous oxide]] can also be used.
 
Nitrogen can be isolated from air via reduction of oxygen with [[copper]] turning or other reducing agents (except metals that will burn in a nitrogen atmosphere, such as [[lithium]], [[magnesium]] or [[titanium]]). The purified gas will contain ~1% [[argon]]. Smaller, but purer amounts of nitrogen can also be obtained by decomposing [[sodium azide]]. [[Nitrous oxide]] can also be used.
  
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Liquid nitrogen can be made at home, by employing an air compressor and a cooling installation. A good tutorial can be found [http://www.instructables.com/id/Homemade-liquid-nitrogen-generator/ here].
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Liquid nitrogen can be made at home, by employing an air compressor and a cooling installation, though making such an installation requires skill. A good tutorial can be found [http://www.instructables.com/id/Homemade-liquid-nitrogen-generator/ here].
  
 
==Projects==
 
==Projects==
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==Handling==
 
==Handling==
 
===Safety===
 
===Safety===
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Gaseous nitrogen is inert, but in an enclosed space at high concentrations can displace oxygen, and therefore presents an asphyxiation hazard.
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Gaseous nitrogen is inert and is non-toxic, but in an enclosed space at high concentrations can displace oxygen, and therefore presents an asphyxiation hazard.
  
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Direct skin contact with liquid nitrogen will cause severe frostbite (cryogenic "burns"), either instantly or a second or more after direct exposure, depending on the form of liquid nitrogen.
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Direct skin contact with liquid nitrogen will cause severe frostbite (cryogenic "burns"), either instantly or a second or more after direct exposure, depending on the form of liquid nitrogen. Normally, small amounts of liquid nitrogen will not cause anything but superficial frost on the surface of the skin if the contact is brief. However, if the liquid nitrogen lingers for too long, the tissue will freeze. It gets worse if a droplet of liquid nitrogen gets between your palm and a hard surface, like when grabbing the dewar handle, as this will instantly give you a frostbit.
  
 
===Storage===
 
===Storage===
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Compressed nitrogen tanks should be stored away from any heat sources. Liquid nitrogen dewars should be kept away from any source of heat and light and MUST have a pressure release valve to prevent a pressure build-up. The valve must be checked from time to time for any problems.
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Compressed nitrogen gas cylinders should be stored away from any heat sources. Liquid nitrogen dewars should be kept away from any source of heat and light and MUST have a pressure release valve to prevent a pressure build-up. The valve must be checked from time to time for any defects.
  
 
===Disposal===
 
===Disposal===

Latest revision as of 18:47, 7 November 2019

Nitrogen,  7N
Nitrogen discharge tube.jpg
Nitrogen discharge tube.
General properties
Name, symbol Nitrogen, N
Alternative name Azote
Appearance Colorless gas, liquid or solid
Nitrogen in the periodic table
-
↑
N
↓
P
Carbon ← Nitrogen → Oxygen
Atomic number 7
Standard atomic weight (Ar) 14.007
Group, block (pnictogens); p-block
Period period 2
Electron configuration [He] 2s2 2p3
per shell
 2, 5
Physical properties
Colorless
Phase Gas
Melting point 63.15 K ​(−210.0 °C, ​−346.0 °F)
Boiling point 77.355 K ​(−195.795 °C, ​−320.431 °F)
Density at  (0 °C and 101.325 kPa) 1.251 g/L
when liquid, at  0.808 g/cm3
Triple point 63.151 K, ​12.52 kPa
Critical point 126.192 K, 3.3958 MPa
Heat of fusion 0.72 kJ/mol
Heat of 5.56 kJ/mol
Molar heat capacity 29.124 J/(mol·K)
 pressure
Atomic properties
Oxidation states 5, 4, 3, 2, 1, −1, −2, −3 ​(a strongly acidic oxide)
Electronegativity Pauling scale: 3.04
energies 1st: 1402.3 kJ/mol
2nd: 2856.0 kJ/mol
3rd: 4578.1 kJ/mol
Covalent radius 71±1 pm
Van der Waals radius 155 pm
Miscellanea
Crystal structure ​Hexagonal
Speed of sound 353 m/s (gas, at 27 °C)
Thermal conductivity 25.83×10−3 W/(m·K)
Magnetic ordering Diamagnetic
CAS Registry Number 17778-88-0
7727-37-9 (N2)
History
Discovery Daniel Rutherford (1772)
Named by Jean-Antoine Chaptal (1790)
· references

Nitrogen is a chemical element with symbol N and atomic number 7. Nitrogen is a common element in the universe, estimated at about seventh in total abundance in our galaxy and the Solar System. On Earth, the element is primarily found as the gas molecule; it forms about 78% of Earth's atmosphere. The element nitrogen was discovered as a separable component of air, by Scottish physician Daniel Rutherford, in 1772.

Properties

Chemical

Nitrogen is a nonmetal, with an electronegativity of 3.04. It has five electrons in its outer shell and is, therefore, trivalent in most compounds. The triple bond in molecular nitrogen (N2) is one of the strongest. The resulting difficulty of converting nitrogen into other compounds, and the ease (and associated high energy release) of converting nitrogen compounds into elemental N2, have dominated the role of nitrogen in both nature and human economic activities.

While nitrogen is relative inert, certain metals such as magnesium or lithium will burn in a nitrogen atmosphere.

Physical

At room temperature, nitrogen is a colorless and odorless gas. At atmospheric pressure, molecular nitrogen condenses (liquefies) at 77 K (−195.79 °C) and freezes at 63 K (−210.01 °C) into the beta hexagonal close-packed crystal allotropic form. Below 35.4 K (−237.6 °C) nitrogen assumes the cubic crystal allotropic form (called the alpha phase). Liquid nitrogen, a fluid resembling water in appearance, but with 80.8% of the density (the density of liquid nitrogen at its boiling point is 0.808 g/mL), is a common cryogen.

Availability

Nitrogen cylinders can be bought at hardware stores and welding supply stores. Liquid nitrogen can be bought from chemical suppliers, and while it's not expensive, the container used for storage, Dewar, is.

Preparation

Nitrogen can be isolated from air via reduction of oxygen with copper turning or other reducing agents (except metals that will burn in a nitrogen atmosphere, such as lithium, magnesium or titanium). The purified gas will contain ~1% argon. Smaller, but purer amounts of nitrogen can also be obtained by decomposing sodium azide. Nitrous oxide can also be used.

Liquid nitrogen can be made at home, by employing an air compressor and a cooling installation, though making such an installation requires skill. A good tutorial can be found here.

Projects

  • Cooling baths (liquid nitrogen)
  • Haber process (small scale)
  • Make lithium nitride
  • Inert atmosphere

Handling

Safety

Gaseous nitrogen is inert and is non-toxic, but in an enclosed space at high concentrations can displace oxygen, and therefore presents an asphyxiation hazard.

Direct skin contact with liquid nitrogen will cause severe frostbite (cryogenic "burns"), either instantly or a second or more after direct exposure, depending on the form of liquid nitrogen. Normally, small amounts of liquid nitrogen will not cause anything but superficial frost on the surface of the skin if the contact is brief. However, if the liquid nitrogen lingers for too long, the tissue will freeze. It gets worse if a droplet of liquid nitrogen gets between your palm and a hard surface, like when grabbing the dewar handle, as this will instantly give you a frostbit.

Storage

Compressed nitrogen gas cylinders should be stored away from any heat sources. Liquid nitrogen dewars should be kept away from any source of heat and light and MUST have a pressure release valve to prevent a pressure build-up. The valve must be checked from time to time for any defects.

Disposal

Nitrogen can be safely released in atmosphere. Avoid doing this in a closed chamber.

References

Relevant Sciencemadness threads

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