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A simple example of a polyatomic ion is the hydroxide ion, which consists of one oxygen atom and one hydrogen atom, jointly carrying a net charge of −1; its chemical formula is O H −. In contrast, an ammonium ion consists of one nitrogen atom and four hydrogen atoms, with a charge of +1; its chemical formula is N H + 4.
For ions, the charge on a particular atom may be denoted with a right-hand superscript. For example, Na +, or Cu 2+. The total charge on a charged molecule or a polyatomic ion may also be shown in this way, such as for hydronium, H 3 O +, or sulfate, SO 2− 4. Here + and − are used in place of +1 and −1, respectively.
Number of consonants denotes number of oxygen atoms. Number of vowels denotes negative charge quantity. Inclusion of the word "ate" signifies that each ends with the letters a-t-e. To use this for the -ite ions, simply subtract one oxygen but keep the charge the same.
The best known example is the Hg 2+ 2 ion, found in mercury(I) (mercurous) compounds. The existence of the metal–metal bond in Hg(I) compounds was established using X-ray studies in 1927 [ 2 ] [ page needed ] and Raman spectroscopy in 1934 [ 3 ] making it one of the earliest, if not the first, metal–metal covalent bonds to be characterised.
The resulting electron configuration can be described in terms of bond type, parity and occupancy for example dihydrogen 1σ g 2. Alternatively it can be written as a molecular term symbol e.g. 1 Σ g + for dihydrogen. Sometimes, the letter n is used to designate a non-bonding orbital. For a stable bond, the bond order defined as
The metatellurate ion TeO 2− 4 is analogous to the sulfate ion, SO 2− 4 and the selenate ion, SeO 2− 4.Whereas many sulfates and selenates form isomorphous salts [5] the tetrahedral metatellurate ion is only found in a few compounds such as the tetraethylammonium salt (NEt 4) 2 TeO 4. [6]