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As a strong Lewis acid, BCl 3 forms adducts with tertiary amines, phosphines, ethers, thioethers, and halide ions. [5] Adduct formation is often accompanied by an increase in B-Cl bond length. BCl 3 •S(CH 3 ) 2 (CAS# 5523-19-3) is often employed as a conveniently handled source of BCl 3 because this solid (m.p. 88-90 °C) releases BCl 3 :
602 12051 Ensembl ENSG00000069399 ENSMUSG00000053175 UniProt P20749 Q9Z2F6 RefSeq (mRNA) NM_005178 NM_033601 RefSeq (protein) NP_005169 NP_291079 Location (UCSC) Chr 19: 44.75 – 44.76 Mb Chr 7: 19.54 – 19.56 Mb PubMed search Wikidata View/Edit Human View/Edit Mouse B-cell lymphoma 3-encoded protein is a protein that in humans is encoded by the BCL3 gene. This gene is a proto- oncogene ...
[1] [2] [3] Introduced by Gilbert N. Lewis in his 1916 article The Atom and the Molecule, a Lewis structure can be drawn for any covalently bonded molecule, as well as coordination compounds. [4] Lewis structures extend the concept of the electron dot diagram by adding lines between atoms to represent shared pairs in a chemical bond.
The number of electron pairs in the valence shell of a central atom is determined after drawing the Lewis structure of the molecule, and expanding it to show all bonding groups and lone pairs of electrons. [1]: 410–417 In VSEPR theory, a double bond or triple bond is treated as a single bonding group. [1]
Lewis structures (or "Lewis dot structures") are flat graphical formulas that show atom connectivity and lone pair or unpaired electrons, but not three-dimensional structure. This notation is mostly used for small molecules. Each line represents the two electrons of a single bond. Two or three parallel lines between pairs of atoms represent ...
The most common Lewis bases are anions. The strength of Lewis basicity correlates with the pK a of the parent acid: acids with high pK a 's give good Lewis bases. As usual, a weaker acid has a stronger conjugate base. Examples of Lewis bases based on the general definition of electron pair donor include: simple anions, such as H − and F −
In its pure state, boron triiodide forms colorless, otherwise reddish, shiny, air and hydrolysis-sensitive [3] crystals, which have a hexagonal crystal structure (a = 699.09 ± 0.02 pm, c = 736.42 ± 0.03 pm, space group P6 3 /m (space group no. 176)). [4] Boron triiodide is a strong Lewis acid and soluble in carbon disulfide. [2]
Boron trifluoride is a versatile Lewis acid that forms adducts with such Lewis bases as fluoride and ethers: CsF + BF 3 → Cs[BF 4] O(CH 2 CH 3) 2 + BF 3 → BF 3 ·O(CH 2 CH 3) 2. Tetrafluoroborate salts are commonly employed as non-coordinating anions.