Английская Википедия:Binary compounds of hydrogen

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Шаблон:Short description Binary compounds of hydrogen are binary chemical compounds containing just hydrogen and one other chemical element. By convention all binary hydrogen compounds are called hydrides even when the hydrogen atom in it is not an anion. These hydrogen compounds can be grouped into several types.

Overview

Binary hydrogen compounds in group 1 are the ionic hydrides (also called saline hydrides) wherein hydrogen is bound electrostatically. Because hydrogen is located somewhat centrally in an electronegative sense, it is necessary for the counterion to be exceptionally electropositive for the hydride to possibly be accurately described as truly behaving ionic. Therefore, this category of hydrides contains only a few members.

Hydrides in group 2 are polymeric covalent hydrides. In these, hydrogen forms bridging covalent bonds, usually possessing mediocre degrees of ionic character, which make them difficult to be accurately described as either covalent or ionic. The one exception is beryllium hydride, which has definitively covalent properties.

Hydrides in the transition metals and lanthanides are also typically polymeric covalent hydrides. However, they usually possess only weak degrees of ionic character. Usually, these hydrides rapidly decompose into their component elements at ambient conditions. The results consist of metallic matrices with dissolved, often stoichiometric or near so, concentrations of hydrogen, ranging from negligible to substantial. Such a solid can be thought of as a solid solution and is alternately termed a metallic- or interstitial hydride. These decomposed solids are identifiable by their ability to conduct electricity and their magnetic properties (the presence of hydrogen is coupled with the delocalisation of the valence electrons of the metal), and their lowered density compared to the metal. Both the saline hydrides and the polymeric covalent hydrides typically react strongly with water and air.

It is possible to produce a metallic hydride without requiring decomposition as a necessary step. If a sample of bulk metal is subjected to any one of numerous hydrogen absorption techniques, the characteristics, such as luster and hardness of the metal is often retained to a large degree. Bulk actinoid hydrides are only known in this form. The affinity for hydrogen for most of the d-block elements are low. Therefore, elements in this block do not form hydrides (the hydride gap) under standard temperature and pressure with the notable exception of palladium. Palladium can absorb up to 900 times its own volume of hydrogen and is therefore actively researched in the field hydrogen storage.

Elements in group 13 to 17 (p-block) form covalent hydrides (or nonmetal hydrides). In group 12 zinc hydride is a common chemical reagent but cadmium hydride and mercury hydride are very unstable and esoteric. In group 13 boron hydrides exist as a highly reactive monomer BH₃, as an adduct for example ammonia borane or as dimeric diborane and as a whole group of BH cluster compounds. Alane (AlH₃) is a polymer. Gallium exists as the dimer digallane. Indium hydride is only stable below Шаблон:Convert. Not much is known about the final group 13 hydride, thallium hydride.

Due to the total number of possible binary saturated compounds with carbon of the type C_nH_2n+2 being very large, there are many group 14 hydrides. Going down the group the number of binary silicon compounds (silanes) is small (straight or branched but rarely cyclic) for example disilane and trisilane. For germanium only 5 linear chain binary compounds are known as gases or volatile liquids. Examples are n-pentagermane, isopentagermane and neopentagermane. Of tin only the distannane is known. Plumbane is an unstable gas.

The hydrogen halides, hydrogen chalcogenides and pnictogen hydrides also form compounds with hydrogen, whose lightest members show many anomalous properties due to hydrogen bonding.

Non-classical hydrides are those in which extra hydrogen molecules are coordinated as a ligand on the central atoms. These are very unstable but some have been shown to exist.

Polyhydrides or superhydrides are compounds in which the number of hydrogen atoms exceed the valency of the combining atom. These may only be stable under extreme pressure, but may be high temperature superconductors, such as H₃S, superconducting at up to 203 K. Polyhydrides are actively studied with the hope of discovering a room temperature superconductor.

The periodic table of the stable binary hydrides

The relative stability of binary hydrogen compounds and alloys at standard temperature and pressure can be inferred from their standard enthalpy of formation values.

H2 0

He

LiH −91

BeH2 negative

BH3 41

CH4 −74.8

NH3 −46.8

H2O −243

HF −272

Ne

NaH −57

MgH2 −75

AlH3 −46

SiH4 31

PH3 5.4

H2S −20.7

HCl −93

Ar

KH −58

CaH2 −174

ScH2

TiH2

VH

CrH

Mn

FeH, FeH2

Co

Ni

CuH

ZnH2

GaH3

GeH4 92

AsH3 67

H2Se 30

HBr −36.5

Kr

RbH −47

SrH2 −177

YH2

ZrH2

NbH

Mo

Tc

Ru

Rh

PdH

Ag

CdH2

InH3

SnH4 163

SbH3 146

H2Te 100

HI 26.6

Xe

CsH −50

BaH2 −172

LuH2

HfH2

TaH

W

Re

Os

Ir

Pt

Au

Hg

Tl

PbH4 252

BiH3 247

H2Po 167

HAt positive

Rn

Fr

Ra

Lr

Rf

Db

Sg

Bh

Hs

Mt

Ds

Rg

Cn

Nh

Fl

Mc

Lv

Ts

Og

↓

LaH2

CeH2

PrH2

NdH2

PmH2

SmH2

EuH2

GdH2

TbH2

DyH2

HoH2

ErH2

TmH2

YbH2

Ac

Th

Pa

U

Np

Pu

Am

Cm

Bk

Cf

Es

Fm

Md

No

Binary compounds of hydrogen

Covalent hydrides	metallic hydrides
Ionic hydrides	Intermediate hydrides
Do not exist	Not assessed

Molecular hydrides

The isolation of monomeric molecular hydrides usually require extremely mild conditions, which are partial pressure and cryogenic temperature. The reason for this is threefold - firstly, most molecular hydrides are thermodynamically unstable toward decomposition into their elements; secondly, many molecular hydrides are also thermodynamically unstable toward polymerisation; and thirdly, most molecular hydrides are also kinetically unstable toward these types of reactions due to low activation energy barriers.

Instability toward decomposition is generally attributable to poor contribution from the orbitals of the heavier elements to the molecular bonding orbitals. Instability toward polymerisation is a consequence of the electron-deficiency of the monomers relative to the polymers. Relativistic effects play an important role in determining the energy levels of molecular orbitals formed by the heavier elements. As a consequence, these molecular hydrides are commonly less electron-deficient than otherwise expected. For example, based on its position in the 12th column of the periodic table alone, mercury(II) hydride would be expected to be rather deficient. However, it is in fact satiated, with the monomeric form being much more energetically favourable than any oligomeric form.

The table below shows the monomeric hydride for each element that is closest to, but not surpassing its heuristic valence. A heuristic valence is the valence of an element that strictly obeys the octet, duodectet, and sexdectet valence rules. Elements may be prevented from reaching their heuristic valence by various steric and electronic effects. In the case of chromium, for example, stearic hindrance ensures that both the octahedral and trigonal prismatic molecular geometries for Шаблон:Chem are thermodynamically unstable to rearranging to a Kubas complex structural isomer.

Where available, both the enthalpy of formation for each monomer and the enthalpy of formation for the hydride in its standard state is shown (in brackets) to give a rough indication of which monomers tend to undergo aggregation to lower enthalpic states. For example, monomeric lithium hydride has an enthalpy of formation of 139 kJ mol⁻¹, whereas solid lithium hydride has an enthalpy of −91 kJ mol⁻¹. This means that it is energetically favourable for a mole of monomeric LiH to aggregate into the ionic solid, losing 230 kJ as a consequence. Aggregation can occur as a chemical association, such as polymerisation, or it can occur as an electrostatic association, such as the formation of hydrogen-bonding in water.

Classical hydrides

Classical hydrides

1	2	3	4	5	6	5	4	3	2	1	2	3	4	3	2	1
Шаблон:Chem 0
LiH Шаблон:Sup sub	[[dihydridoberyllium|Шаблон:Chem]] Шаблон:Sup											[[borane|Шаблон:Chem]] Шаблон:Sup sub	[[methane|Шаблон:Chem]] −75	[[ammonia|Шаблон:Chem]] −46	[[properties of water|Шаблон:Chem]] Шаблон:Sup sub	HF −273
NaH Шаблон:Sup sub	[[magnesium hydride#structure and bonding|Шаблон:Chem]] Шаблон:Sup sub											[[aluminium hydride#molecular forms of alane|Шаблон:Chem]] Шаблон:Sup sub	[[silane|Шаблон:Chem]] 34	[[phosphine|Шаблон:Chem]] 5	[[hydrogen sulfide|Шаблон:Chem]] −21	HCl −92
KH Шаблон:Sup sub	[[calcium hydride|Шаблон:Chem]] Шаблон:Sup sub	[[scandium(III) hydride|Шаблон:Chem]]	[[titanium(IV) hydride|Шаблон:Chem]]	Шаблон:Chem	[[chromium(II) hydride#mononuclear form|Шаблон:Chem]]	Шаблон:Chem (−12)	[[iron(II) hydride|Шаблон:Chem]] 324	Шаблон:Chem	Шаблон:Chem 168	CuH Шаблон:Sup sub	[[zinc(II) hydride#molecular form|Шаблон:Chem]] 162	[[gallane|Шаблон:Chem]] 151	[[germane|Шаблон:Chem]] 92	[[arsine|Шаблон:Chem]] 67	[[hydrogen selenide|Шаблон:Chem]] 30	HBr −36
RbH Шаблон:Sup sub	Шаблон:Chem Шаблон:Sup sub	Шаблон:Chem	Шаблон:Chem	Шаблон:Chem	Шаблон:Chem	Tc	Шаблон:Chem	Шаблон:Chem	PdH 361	AgH 288	[[cadmium hydride#molecular cdh2|Шаблон:Chem]] 183	[[indium hydride#indigane|Шаблон:Chem]] 222	[[stannane|Шаблон:Chem]] 163	[[stibine|Шаблон:Chem]] 146	[[hydrogen telluride|Шаблон:Chem]] 100	HI 27
CsH Шаблон:Sup sub	Шаблон:Chem Шаблон:Sup sub	Шаблон:Chem	Шаблон:Chem	Шаблон:Chem	Шаблон:Chem 586	Шаблон:Chem	Os	Ir	Шаблон:Chem	AuH 295	[[mercury(II) hydride|Шаблон:Chem]] 101	[[thallium hydride|Шаблон:Chem]] 293	[[plumbane|Шаблон:Chem]] 252	[[bismuthine|Шаблон:Chem]] 247	[[polonium hydride|Шаблон:Chem]] 167	HAt 88
Fr	Ra	Lr	Rf	Db	Sg	Bh	Hs	Mt	Ds	Rg	Cn	Nh	Fl	Mc	Lv	Ts
		↓
		3	4	5	6	7	8	7	6	5	4	3	2	1	2
		Шаблон:Chem	Шаблон:Chem	Шаблон:Chem	Шаблон:Chem	Pm	Шаблон:Chem	Шаблон:Chem	Шаблон:Chem	Шаблон:Chem	Шаблон:Chem	Шаблон:Chem	Шаблон:Chem	TmH	Шаблон:Chem
		Ac	Шаблон:Chem	Pa	[[uranium(IV) hydride|Шаблон:Chem]]	Np	Pu	Am	Cm	Bk	Cf	Es	Fm	Md	No

Legend

Monomeric covalent	Файл:Methane-CRC-MW-3D-balls.png	Oligomeric covalent	Файл:Diborane-3D-balls-A.png
Polymeric covalent	Файл:Beryllium-hydride-3D-balls.png	Ionic	Файл:Lithium-hydride-3D-vdW.png
Polymeric delocalised covalent
Unknown solid structure	Файл:Question mark alternate.svg	Not assessed

This table includes the thermally unstable dihydrogen complexes for the sake of completeness. As with the above table, only the complexes with the most complete valence is shown, to the negligence of the most stable complex.

Non-classical covalent hydrides

A molecular hydride may be able to bind to hydrogen molecules acting as a ligand. The complexes are termed non-classical covalent hydrides. These complexes contain more hydrogen than the classical covalent hydrides, but are only stable at very low temperatures. They may be isolated in inert gas matrix, or as a cryogenic gas. Others have only been predicted using computational chemistry.

Non-classical covalent hydrides

8		18								8
Шаблон:Chem	Be											Шаблон:Chem
Na	Шаблон:Chem											Шаблон:Chem
K	Ca	Шаблон:Chem	Шаблон:Chem	Шаблон:Chem	CrH2(H2)2	Mn	Шаблон:Chem	Шаблон:Chem	Шаблон:Chem	CuH(H2)	Шаблон:Chem	Шаблон:Chem
Rb	Sr	Шаблон:Chem	Zr	Шаблон:Chem	Mo	Tc	Шаблон:Chem	RhH3(H2)	Шаблон:Chem	AgH(H2)	Шаблон:Chem	Шаблон:Chem
Cs	Ba	Lu	Hf	Шаблон:Chem	Шаблон:Chem	Re	Os	Ir	Шаблон:Chem	Шаблон:Chem	Hg	Tl
Fr	Ra	Lr	Rf	Db	Sg	Bh	Hs	Mt	Ds	Rg	Cn	Nh
		↓
		32												18
		Шаблон:Chem	Шаблон:Chem	Шаблон:Chem	Nd	Pm	Sm	Eu	Шаблон:Chem	Tb	Dy	Ho	Er	Tm	Yb
		Ac	ThH4(H2)4	Pa	Шаблон:Chem	Np	Pu	Am	Cm	Bk	Cf	Es	Fm	Md	No

Legend

AssessedШаблон:By whom

Not assessed

Hydrogen solutions

Hydrogen has a highly variable solubility in the elements. When the continuous phase of the solution is a metal, it is called a metallic hydride or interstitial hydride, on account of the position of the hydrogen within the crystal structure of the metal. In solution, hydrogen can occur in either the atomic or molecular form. For some elements, when hydrogen content exceeds its solubility, the excess precipitates out as a stoichiometric compound. The table below shows the solubility of hydrogen in each element as a molar ratio at Шаблон:Convert and 100 kPa.

He

Шаблон:Chem

Be

B

C

N

O

F

Ne

Шаблон:Chem

Шаблон:Chem

Шаблон:Chem

Si

P

S

Cl

Ar

Шаблон:Chem

Шаблон:Chem

Шаблон:Chem

Шаблон:Chem

Шаблон:Chem

Cr

Шаблон:Chem

Шаблон:Chem

Co

Шаблон:Chem

Шаблон:Chem

Шаблон:Chem

Ga

Ge

As

Se

Br

Kr

Шаблон:Chem

Sr

Шаблон:Chem

Шаблон:Chem

Шаблон:Chem

Mo

Tc

Ru

Rh

Шаблон:Chem

Шаблон:Chem

Cd

In

Sn

Sb

Te

I

Xe

Шаблон:Chem

Ba

Lu

Hf

Шаблон:Chem

W

Re

Os

Ir

Pt

Шаблон:Chem

Шаблон:Chem

Tl

Pb

Bi

Po

At

Rn

Fr

Ra

Lr

Rf

Db

Sg

Bh

Hs

Mt

Ds

Rg

Cn

Nh

Fl

Mc

Lv

Ts

Og

↓

Шаблон:Chem

Шаблон:Chem

Pr

Nd

Pm

Шаблон:Chem

Eu

Gd

Tb

Dy

Ho

Er

Tm

Yb

Ac

Th

Pa

Шаблон:Chem

Np

Pu

Am

Cm

Bk

Cf

Es

FM

Md

No

Legend

Miscible

Undetermined