Bond lengths in alkali metal oxides

McGuire, N.K.; O’Keeffe, Michael

doi:10.1016/0022-4596(84)90129-4

Cited by 19 publications

(12 citation statements)

References 9 publications

Supporting

Mentioning

Contrasting

Order By: Relevance

“…This observation was a motivation for determining the structures unambiguously. It is noted, however, that anomalously long bonds are also found in the corresponding oxides (McGuire & O'Keeffe, 1984). …”

Section: --I Imentioning

confidence: 99%

Structures of RbD and CsD by time-of-flight neutron diffraction

Brese¹,

O’Keeffe²

1991

Acta Crystallogr C

Self Cite

View full text Add to dashboard Cite

Section: --I Imentioning

confidence: 99%

Structures of RbD and CsD by time-of-flight neutron diffraction

Brese¹,

O’Keeffe²

1991

Acta Crystallogr C

Self Cite

View full text Add to dashboard Cite

“…The difference in reactivity between MeOK and its lithium and sodium congeners hence likely stems from the tighter ion pairs formed between the MeO − anion and the hard Li + and Na + cations. This trend is reflected in the shortening of O−M bond length in the alkali oxides M 2 O from 2.9, 2.8, 2.4, to 2.0 Å across the series Rb, K, Na, Li . This interpretation is supported by the comparable catalytic activities of MeOK and MeONa/18‐C‐6 at 19 °C (Entries 4 and 6 in Table ).…”

Section: Methodsmentioning

confidence: 68%

Transition‐Metal‐Free Acceptorless Decarbonylation of Formic Acid Enabled by a Liquid Chemical‐Looping Strategy

2019

View full text Add to dashboard Cite

The selective decarbonylation of formic acid was achieved under transition‐metal‐free conditions. Using a liquid chemical‐looping strategy, the thermodynamically favored dehydrogenation of formic acid was shut down, yielding a pure stream of CO with no H2 or CO2 contamination. The transformation involves a two‐step sequence where methanol is used as a recyclable looping agent to yield methylformate, which is subsequently decomposed to carbon monoxide using alkoxides as catalysts.

show abstract

“…The agreement between the sum of the bond valences and the atomic valence could be used to confirm the correctness of a crystal structure or to locate the undetected hydrogen atoms. Brown subsequently applied the model to analyze the structural chemistry of lone pair cations [21], hydrogen bonds [22,23], and acetates and trifluoroacetate ions [24], and O'Keeffe and collaborators applied it to alkali metal oxides [25] and nitrides [26].…”

Section: The Origin and Development Of The Bond Valence Theorymentioning

confidence: 99%

Historical Introduction

Brown

2013

Structure and Bonding

View full text Add to dashboard Cite

The bond valence theory grew out of Linus Pauling's electrostatic valence principle, but its development was slow until crystal structure determination became sufficiently accurate to make clear how the valence of a bond correlates with its length. Armed with this quantitative link with experiment, the theory has subsequently found many uses in analysing, modelling and predicting the structures of complex crystals, surfaces and liquids. Its theorems show how the physical properties of complex materials can be understood as the consequence of their chemical structure. The theory is increasingly finding new uses in solidstate chemistry and condensed matter physics.Keywords Bond valence Á History of bond valence Á Pauling's electrostatic valence principle Contents

show abstract

Bond lengths in alkali metal oxides

Cited by 19 publications

References 9 publications

Structures of RbD and CsD by time-of-flight neutron diffraction

Structures of RbD and CsD by time-of-flight neutron diffraction

Transition‐Metal‐Free Acceptorless Decarbonylation of Formic Acid Enabled by a Liquid Chemical‐Looping Strategy

Historical Introduction

Contact Info

Product

Resources

About