Group 14 hydride

The tetrahydride series has the chemical formula XH₄, with X representing any of the carbon family. Methane is commonly the result of the decomposition of organic matter and is a greenhouse gas. The other hydrides are generally unstable, poisonous metal hydrides.

They take on a pyramidal structure, and as such are not polar molecules like the other p-block hydrides.

Unlike other light hydrides such as ammonia, water and hydrogen fluoride, methane does not exhibit any anomalous effects attributed to hydrogen bonding, and so its properties conform well to the prevailing trend of heavier group 14 hydrides.

Compound	Chemical formula	Bond length	Space-filling model
carbon tetrahydride hydrogen carbide methane (carbane)	CH4
silicon tetrahydride hydrogen silicide (silane)	SiH4
germanium tetrahydride hydrogen germanide (germane)	GeH4
tin tetrahydride hydrogen stannide (stannane)	SnH4
lead tetrahydride hydrogen plumbide (plumbane)	PbH4

This series has the chemical formula X₂H₆. Ethane is commonly found alongside methane in natural gas. The other hydrides are even less stable than the tetrahydrides.

Compound	Chemical formula	Bond length	model
dicarbon hexahydride ethane (dicarbane)	C2H6
disilicon hexahydride (disilane)	Si2H6
digermanium hexahydride (digermane)	Ge2H6
ditin hexahydride (distannane)	Sn2H6

All straight-chain saturated group 14 hydrides follow the formula X_nH_2n+2, the same formula for the alkanes.

Cubane, a Platonic hydrocarbon and prismane

Many other group 14 hydrides are known. Carbon forms a huge variety of hydrocarbons (with propane and butane following methane and ethane among the alkanes, but also including alkenes, alkynes, cyclic and branched compounds, as well as aromatic hydrocarbons such as benzene, toluene and limonene), whose study forms the core of organic chemistry.[1]

Alongside hydrogen, carbon can form compounds with the chemically similar halogens, forming haloalkanes. The simplest of this series, the halomethanes, contain compounds such as dichloromethane and iodoform. Other such important chemicals include vinyl chloride, which is used in the production of PVC.

The other group 14 elements have a lower tendency to catenate. Silanes Si_nH_2n+2 are known for n = 1–8 (thermal stability decreasing as n increases), as are cyclosilanes Si₅H₁₀ and Si₆H₁₂. They are very reactive, pyrophoric colourless gases or volatile liquids. Their volatility is intermediate between the alkanes and the germanes.[2] Unsaturated silanes, the silenes and silynes, have been characterized spectroscopically. The first members of each respectively are disilene and disilyne, the silicon analogues of ethylene and acetylene). The first five germanes Ge_nH_2n+2 are known and are fairly similar to the silanes.[3] Stannane, a strong reducing agent slowly decomposes at room temperature to tin and hydrogen gas, and is decomposed by concentrated aqueous acids or alkalis; distannane, Sn₂H₆ is still more unstable, and longer stannanes are unknown. Plumbane is very poorly characterised and is only known in trace amounts: even at low temperatures, synthesis methods that yield the other MH₄ compounds fail to give PbH₄. No other plumbanes are known.[4]

Compounds containing hydrogen and multiple group 14 elements are known, one of the most famous of these being tetraethyllead.

Group 14 hydrides radical:

• Methylene
• Methylidyne

• Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. ISBN 978-0-08-037941-8.