Amberger, E. Will, G. Becher, H. Google Scholar. Download references. You can also search for this author in PubMed Google Scholar. Reprints and Permissions. WILL, G. Crystal structure of I-tetragonal boron. Nature , — Download citation. Received : 07 February Revised : 18 June Issue Date : 04 October Further information about storage conditions: Keep container tightly sealed. Store in cool, dry conditions in well-sealed containers.
Specific end use s No data available. Additional information about design of technical systems: Properly operating chemical fume hood designed for hazardous chemicals and having an average face velocity of at least feet per minute.
Control parameters Components with limit values that require monitoring at the workplace: None. Additional information: No data Exposure controls Personal protective equipment Follow typical protective and hygienic practices for handling chemicals.
Keep away from foodstuffs, beverages and feed. Remove all soiled and contaminated clothing immediately. Wash hands before breaks and at the end of work. Maintain an ergonomically appropriate working environment. Breathing equipment: Use suitable respirator when high concentrations are present. Protection of hands: Impervious gloves Inspect gloves prior to use.
Suitability of gloves should be determined both by material and quality, the latter of which may vary by manufacturer. Penetration time of glove material in minutes No data available Eye protection: Safety glasses Body protection: Protective work clothing. Danger of explosion: No data available.
Reactivity No data available Chemical stability Stable under recommended storage conditions. Possibility of hazardous reactions No dangerous reactions known Conditions to avoid No data available Incompatible materials: Oxidizing agents Halogens Interhalogens Hazardous decomposition products: Boron oxide.
Information on toxicological effects Acute toxicity: Harmful if swallowed. Germ cell mutagenicity: No effects known. Specific target organ system toxicity - repeated exposure: No effects known. Specific target organ system toxicity - single exposure: No effects known.
Aspiration hazard: No effects known. Subacute to chronic toxicity: No effects known. Additional toxicological information: To the best of our knowledge the acute and chronic toxicity of this substance is not fully known. Toxicity Aquatic toxicity: No data available Persistence and degradability No data available Bioaccumulative potential No data available Mobility in soil No data available Additional ecological information: Do not allow material to be released to the environment without official permits.
Avoid transfer into the environment. Waste treatment methods Recommendation Consult official regulations to ensure proper disposal. Uncleaned packagings: Recommendation: Disposal must be made according to official regulations. California Proposition 65 Prop 65 - Chemicals known to cause cancer Substance is not listed. Prop 65 - Developmental toxicity Substance is not listed. Prop 65 - Developmental toxicity, female Substance is not listed.
Prop 65 - Developmental toxicity, male Substance is not listed. Information about limitation of use: For use only by technically qualified individuals. Substance is not listed. Chemical safety assessment: A Chemical Safety Assessment has not been carried out. The above information is believed to be correct but does not purport to be all inclusive and shall be used only as a guide.
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See reverse side of invoice or packing slip for additional terms and conditions of sale. See more Boron products. Boron atomic symbol: B, atomic number: 5 is a Block P, Group 13, Period 2 element with an atomic weight of These are semiconductors, whose electronic properties, such as their band gaps, differ from those that can be achieved using either pure or doped group 14 elements.
All group 13 oxides dissolve in dilute acid, but Al 2 O 3 and Ga 2 O 3 are amphoteric. Unlike boron, the heavier group 13 elements do not react directly with hydrogen. Only the aluminum and gallium hydrides are known, but they must be prepared indirectly; AlH 3 is an insoluble, polymeric solid that is rapidly decomposed by water, whereas GaH 3 is unstable at room temperature.
Boron has a relatively limited tendency to form complexes, but aluminum, gallium, indium, and, to some extent, thallium form many complexes. Group 13 metal ions also form stable complexes with species that contain two or more negatively charged groups, such as the oxalate ion. The stability of such complexes increases as the number of coordinating groups provided by the ligand increases.
Compounds of the group 13 elements with oxygen are thermodynamically stable. Many of the anomalous properties of the group 13 elements can be explained by the increase in Z eff moving down the group. Isolation of the group 13 elements requires a large amount of energy because compounds of the group 13 elements with oxygen are thermodynamically stable.
Boron behaves chemically like a nonmetal, whereas its heavier congeners exhibit metallic behavior. Instead of forming a metallic lattice with delocalized valence electrons, boron forms unique aggregates that contain multicenter bonds, including metal borides, in which boron is bonded to other boron atoms to form three-dimensional networks or clusters with regular geometric structures.
All neutral compounds of the group 13 elements are electron deficient and behave like Lewis acids. The trivalent halides of the heavier elements form halogen-bridged dimers that contain electron-pair bonds, rather than the delocalized electron-deficient bonds characteristic of diborane.
Their oxides dissolve in dilute acid, although the oxides of aluminum and gallium are amphoteric. None of the group 13 elements reacts directly with hydrogen, and the stability of the hydrides prepared by other routes decreases as we go down the group. Learning Objectives To understand the trends in properties and the reactivity of the group 13 elements. Preparation and General Properties of the Group 13 Elements As reductants, the group 13 elements are less powerful than the alkali metals and alkaline earth metals.
Reaction with F 2 gives the trifluorides MF 3 for all group 13 elements. Reactions and Compounds of Boron Elemental boron is a semimetal that is remarkably unreactive; in contrast, the other group 13 elements all exhibit metallic properties and reactivity. Unlike metallic solids, elemental boron consists of a regular array of B 12 icosahedra rather than individual boron atoms.
Note that each boron atom in the B 12 icosahedron is connected to five other boron atoms within the B 12 unit. Solution: Molecular oxygen is an oxidant. If the other reactant is a potential reductant, we expect that a redox reaction will occur. Because hydride is a strong reductant, a redox reaction will probably occur. A reasonable guess is B 2 O 3 and H 2 O, both stable compounds.
Neither BCl 3 nor water is a powerful oxidant or reductant, so a redox reaction is unlikely; a hydrolysis reaction is more probable. Nonmetal halides are acidic and react with water to form a solution of the hydrohalic acid and a nonmetal oxide or hydroxide. In this case, the most probable boron-containing product is boric acid [B OH 3 ]. We normally expect a boron trihalide to behave like a Lewis acid.
In this case, however, the other reactant is elemental hydrogen, which usually acts as a reductant. Consequently, we can write a redox reaction in which hydrogen is oxidized and boron is reduced. Because compounds of boron in lower oxidation states are rare, we expect that boron will be reduced to elemental boron.
The other product of the reaction must therefore be HI. Of the group 13 halides, only the fluorides behave as typical ionic compounds. Complexes of Group 13 Elements Boron has a relatively limited tendency to form complexes, but aluminum, gallium, indium, and, to some extent, thallium form many complexes. Hence a redox reaction is probable, producing metallic Fe and Al 2 O 3.
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