Chalcogen Hydrogen

Hydrogen chalcogenes is the common name for compounds formed from hydrogen and chalcogenes (elements of the oxygen subgroup). They have the general formula H ₂ X, where X is chalcogen.

Compound	Formula	Molar mass	Bond length d (HX) / pm	Valence angle (HXH), °	Dipole moment μ / D	G ° _f	t _melt ° C	t _bale ° C
Water	H ₂ O	eighteen	95.8	104.45	1.85	-285.83	0	one hundred
Hydrogen sulfide	H ₂ s	34	133.6	92.1	0.93	-20.15	-82.3	-60.28
Hydrogen selenium	H ₂ se	81	146	91		85.77	-65.73	-41.25
Tellurium hydrogen	H ₂ te	130	169	90		154.39	-49	-2.2
Hydrogen sulfide	H ₂ Po	212	171	88			-35.3	36.1

Under normal conditions, hydrogen sulfide, hydrogen selenide and hydrogen telluride are gases, water and hydrogen sulfide are liquids. All chalcogen hydrogen is extremely toxic (water is the exception).

Chalcogenes in chalcogen hydrogen have an oxidation state of −2. Since they have a maximum negative oxidation state, they exhibit only reducing properties. The regenerative ability of chalcogen hydrogen grows from oxygen to polonium.

Gaseous chalcogen hydrogen is slightly soluble in water.

Content

1 Chemical properties
2 Production Methods
3 See also
4 Literature

Chemical Properties

Upon dissolution of gaseous chalcogen hydrogen in water, dissociation occurs in two stages (dissociation in the second stage occurs very weakly):

{\mathsf {H_{2}X+H_{2}O\rightleftarrows H_{3}O^{+}+HX^{-}}}

{\ displaystyle {\ mathsf {H_ {2} X + H_ {2} O \ rightleftarrows H_ {3} O ^ {+} + HX ^ {-}}}}

{\mathsf {HX^{-}+H_{2}O\rightleftarrows H_{3}O^{+}+X^{2}-}}

{\ displaystyle {\ mathsf {HX ^ {-} + H_ {2} O \ rightleftarrows H_ {3} O ^ {+} + X ^ {2} -}}}

Hydrogen chalcogen react with hydroxides with the formation of the corresponding salts and water:

{\mathsf {H_{2}S+2NaOH\rightarrow Na_{2}S+2H_{2}O}}

{\ displaystyle {\ mathsf {H_ {2} S + 2NaOH \ rightarrow Na_ {2} S + 2H_ {2} O}}}

{\mathsf {H_{2}Se+2KOH\rightarrow K_{2}Se+2H_{2}O}}

{\ displaystyle {\ mathsf {H_ {2} Se + 2KOH \ rightarrow K_ {2} Se + 2H_ {2} O}}}

With a ratio of 1: 1 chalcogen hydrogen and hydroxide, an acid salt is formed:

{\mathsf {H_{2}S+KOH\rightarrow KSH+H_{2}O}}

{\ displaystyle {\ mathsf {H_ {2} S + KOH \ rightarrow KSH + H_ {2} O}}}

Water can be decomposed into elements by electrolysis :

{\mathsf {2H_{2}O\rightarrow 2H_{2}\uparrow +O_{2}\uparrow }}

{\ displaystyle {\ mathsf {2H_ {2} O \ rightarrow 2H_ {2} \ uparrow + O_ {2} \ uparrow}}}

In this case, it is necessary to supply a voltage of about 6V.

Water and hydrogen sulfide interact with some metals:

{\mathsf {2Na+2H_{2}O\rightarrow 2NaOH+H_{2}\uparrow }}

{\ displaystyle {\ mathsf {2Na + 2H_ {2} O \ rightarrow 2NaOH + H_ {2} \ uparrow}}}

{\mathsf {H_{2}S+Fe\rightarrow FeS+H_{2}\uparrow }}

{\ displaystyle {\ mathsf {H_ {2} S + Fe \ rightarrow FeS + H_ {2} \ uparrow}}}

Telluride and hydrogen sulfide are unstable substances that decompose even at low temperatures:

{\mathsf {H_{2}Te\rightarrow H_{2}\uparrow +Te}}

{\ displaystyle {\ mathsf {H_ {2} Te \ rightarrow H_ {2} \ uparrow + Te}}}

{\mathsf {H_{2}Po\rightarrow H_{2}\uparrow +Po}}

{\ displaystyle {\ mathsf {H_ {2} Po \ rightarrow H_ {2} \ uparrow + Po}}}

Retrieval Methods

The direct reaction of chalcogenes with hydrogen:

{\mathsf {2H_{2}+O_{2}\rightarrow 2H_{2}O}}

{\ displaystyle {\ mathsf {2H_ {2} + O_ {2} \ rightarrow 2H_ {2} O}}}

{\mathsf {H_{2}+S\rightarrow H_{2}S\uparrow }}

{\ displaystyle {\ mathsf {H_ {2} + S \ rightarrow H_ {2} S \ uparrow}}}

A large amount of heat is released, the reactions are exothermic .

Hydrogen sulfide can be obtained by the interaction of iron sulfide with acid:

{\mathsf {FeS+2CH_{3}COOH\rightarrow (CH_{3}COO)_{2}Fe+H_{2}S\uparrow }}

{\ displaystyle {\ mathsf {FeS + 2CH_ {3} COOH \ rightarrow (CH_ {3} COO) _ {2} Fe + H_ {2} S \ uparrow}}}

Literature

Blumental G. N. “Anorganicum. T.1. "
Kan R. S. "Introduction to Chemical Nomenclature"

Chalcogen Hydrogen

Content

Chemical Properties

Retrieval Methods

See also

Literature

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