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Silicon monoxide is the chemical compound with the formula SiO where silicon is present in the oxidation state +2. In the vapour phase, it is a diatomic molecule. [ 1 ] It has been detected in stellar objects [ 2 ] and has been described as the most common oxide of silicon in the universe.
A suboxide of caesium is Cs 11 O 3, where the charge on Cs is clearly less than 1+, but the oxide is still described as O 2−. Suboxides typically feature extensive bonding between the electropositive element, often leading to clusters. Examples of suboxides other than alkali metal derivatives: [2] Carbon suboxide, C 3 O 2; Boron suboxide, B 6 O;
A silicon–oxygen bond (Si−O bond) is a chemical bond between silicon and oxygen atoms that can be found in many inorganic and organic compounds. [1] In a silicon–oxygen bond, electrons are shared unequally between the two atoms, with oxygen taking the larger share due to its greater electronegativity.
Again there is variation in composition: magnesium silicide is represented by Mg 2 Si, [9] calcium silicide can be represented by Ca 2 Si, CaSi, CaSi 2, Ca 5 Si 3 and by Ca 14 Si 19, [10] strontium silicide can be represented by Sr 2 Si, SrSi 2 and Sr 5 Si 3 [11] and barium silicide can be represented by Ba 2 Si, BaSi 2, Ba 5 Si 3 and Ba 3 Si 4 ...
Glucose (C 6 H 12 O 6), ribose (C 5 H 10 O 5), Acetic acid (C 2 H 4 O 2), and formaldehyde (CH 2 O) all have different molecular formulas but the same empirical formula: CH 2 O.This is the actual molecular formula for formaldehyde, but acetic acid has double the number of atoms, ribose has five times the number of atoms, and glucose has six times the number of atoms.
When there is a shortage of oxygen, cerium(IV) oxide is oxidizes carbon monoxide to the benign dioxide: [3] [4] 2 CeO 2 + CO → Ce 2 O 3 + CO 2. When oxygen is in surplus, the process is reversed and cerium(III) oxide is oxidized to cerium(IV) oxide: 2 Ce 2 O 3 + O 2 → 4 CeO 2
Two oxides of germanium are known: germanium dioxide (GeO 2, germania) and germanium monoxide, (GeO). [4] The dioxide, GeO 2 can be obtained by roasting germanium disulfide (GeS 2) or by allowing elemental germanium to slowly oxidze in air, [5] and is a white powder that is only slightly soluble in water but reacts with alkalis to form germanates. [4]
The SO molecule has a triplet ground state similar to O 2 and S 2, that is, each molecule has two unpaired electrons. [2] The S−O bond length of 148.1 pm is similar to that found in lower sulfur oxides (e.g. S 8 O, S−O = 148 pm) but is longer than the S−O bond in gaseous S 2 O (146 pm), SO 2 (143.1 pm) and SO 3 (142 pm).