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Chlorine Oxide
Chlorine and oxygen can bond in many ways: * chlorine monoxide, , chlorine (II) oxide * chlorine peroxide, , dimer of chlorine (II) oxide *chlorine dioxide, , chlorine (IV) oxide * chloroperoxyl, *chlorine trioxide, ClO3, chlorine (VI) oxide *dichlorine monoxide, Cl2O, chlorine (I) oxide *Three dichlorine dioxides: **ClO dimer, Cl2O2, chlorine (I) peroxide **chloryl chloride, ClO2Cl, chlorine (0,IV) oxide ** chlorine chlorite, ClOClO, chlorine (I,III) oxide * dichlorine trioxide, Cl2O3, chlorine (I,V) oxide *dichlorine tetroxide, also known as chlorine perchlorate, ClOClO3, chlorine (I,VII) oxide *dichlorine pentoxide, Cl2O5, is hypothetical *dichlorine hexoxide, chloryl perchlorate, Cl2O6, chlorine (V,VII) oxide *dichlorine heptoxide, Cl2O7, chlorine (VII) oxide *chlorine tetroxide, * chlorine (VII) oxide peroxide, (OClO3)2 Several ions are also chlorine oxides: *chloryl, * perchloryl, * hypochlorite, ClO− * chlorite, ClO2− * chlorate, ClO3− *perchlorate, ClO4− See a ... [...More Info...] [...Related Items...] OR: [Wikipedia] [Google] [Baidu] |
Dichlorine Pentoxide
Dichlorine pentoxide is a hypothetical chlorine oxide with a chemical formula Cl2O5. The most stable configuration of dichlorine pentoxide is unknown, but theory predicts that the perchloryl/chloride peroxide structure would be the most stable among various isomers, such as the anhydride of chloric acid or the chlorous acid/perchloric acid mixed anhydride. See also *Dichlorine heptoxide * Dichlorine trioxide *Dichlorine monoxide *Chlorine dioxide Chlorine dioxide is a chemical compound with the formula ClO2 that exists as yellowish-green gas above 11 °C, a reddish-brown liquid between 11 °C and −59 °C, and as bright orange crystals below −59 °C. It is usually ... References Chlorine oxides Acid anhydrides Hypothetical chemical compounds Chlorine(VII) compounds Peroxides {{theoretical-chem-stub ... [...More Info...] [...Related Items...] OR: [Wikipedia] [Google] [Baidu] |
Bromine Oxide
Bromine can form several different unstable oxides: * Dibromine monoxide (Br2O) * Bromine dioxide (BrO2) * Dibromine trioxide (Br2O3) * Dibromine pentoxide (Br2O5) * Tribromine octoxide (Br3O8) Also, a number of ions are bromine oxides: * Hypobromite (BrO−) * Bromous acid, Bromite (BrO2−) * Bromate (BrO3−) * Perbromate (BrO4−) And the bromine monoxide radical: * Bromine oxide (BrO) See also * Oxygen fluoride * Chlorine oxide * Iodine oxide {{Chemistry index Bromine compounds Oxides ... [...More Info...] [...Related Items...] OR: [Wikipedia] [Google] [Baidu] |
Oxygen Fluoride
Oxygen fluorides are chemical compound, compounds of chemical element, elements oxygen and fluorine with the general formula , where ''n'' = 1 to 6. Many different oxygen fluorides are known: *oxygen difluoride () *dioxygen difluoride () *trioxygen difluoride or ozone difluoride () *tetraoxygen difluoride () *pentaoxygen difluoride () *hexaoxygen difluoride () *dioxygen monofluoride or fluoroperoxyl () Oxygen fluorides are strong oxidizing agents with high energy and can release their energy either instantaneously or at a controlled rate. Thus, these compounds attracted much attention as potential fuels in Jet propulsion, jet propulsion systems. Synthesis Here are some synthesis methods and reactions of the three most common oxygen fluorides – oxygen difluoride (), dioxygen difluoride () and ozone difluoride (). Oxygen difluoride () A common preparative method involves fluorination of sodium hydroxide: : is a colorless gas at room temperature and a yellow liquid belo ... [...More Info...] [...Related Items...] OR: [Wikipedia] [Google] [Baidu] |
Perchlorate
A perchlorate is a chemical compound containing the perchlorate ion, . The majority of perchlorates are commercially produced salts. They are mainly used as oxidizers for pyrotechnic devices and to control static electricity in food packaging. Perchlorate contamination in food, water, and other parts of the environment has been studied in the U.S. because of harmful effects on human health. Perchlorate ions are somewhat toxic to the thyroid gland. Most perchlorates are colorless solids that are soluble in water. Four perchlorates are of primary commercial interest: ammonium perchlorate , perchloric acid , potassium perchlorate and sodium perchlorate . Perchlorate is the anion resulting from the dissociation of perchloric acid and its salts upon their dissolution in water. Many perchlorate salts are soluble in non-aqueous solutions. Production Perchlorate salts are produced industrially by the oxidation of aqueous solutions of sodium chlorate by electrolysis. This method is used ... [...More Info...] [...Related Items...] OR: [Wikipedia] [Google] [Baidu] |
Chlorate
The chlorate anion has the formula ClO3-. In this case, the chlorine atom is in the +5 oxidation state. "Chlorate" can also refer to chemical compounds containing this anion; chlorates are the salts of chloric acid. "Chlorate", when followed by a Roman numeral in parentheses, e.g. chlorate (VII), refers to a particular oxyanion of chlorine. As predicted by valence shell electron pair repulsion theory, chlorate anions have trigonal pyramidal structures. Chlorates are powerful oxidizers and should be kept away from organics or easily oxidized materials. Mixtures of chlorate salts with virtually any combustible material (sugar, sawdust, charcoal, organic solvents, metals, etc.) will readily deflagrate. Chlorates were once widely used in pyrotechnics for this reason, though their use has fallen due to their instability. Most pyrotechnic applications that formerly used chlorates now use the more stable perchlorates instead. Structure and bonding The chlorate ion cannot be satisf ... [...More Info...] [...Related Items...] OR: [Wikipedia] [Google] [Baidu] |
Chlorite
The chlorite ion, or chlorine dioxide anion, is the halite with the chemical formula of . A chlorite (compound) is a compound that contains this group, with chlorine in the oxidation state of +3. Chlorites are also known as salts of chlorous acid. Compounds The free acid, chlorous acid HClO2, is the least stable oxoacid of chlorine and has only been observed as an aqueous solution at low concentrations. Since it cannot be concentrated, it is not a commercial product. The alkali metal and alkaline earth metal compounds are all colorless or pale yellow, with sodium chlorite (NaClO2) being the only commercially important chlorite. Heavy metal chlorites (Ag+, Hg+, Tl+, Pb2+, and also Cu2+ and ) are unstable and decompose explosively with heat or shock. Sodium chlorite is derived indirectly from sodium chlorate, NaClO3. First, the explosively unstable gas chlorine dioxide, ClO2 is produced by reducing sodium chlorate with a suitable reducing agent such as methanol, hydrogen perox ... [...More Info...] [...Related Items...] OR: [Wikipedia] [Google] [Baidu] |
Hypochlorite
In chemistry, hypochlorite is an anion with the chemical formula ClO−. It combines with a number of cations to form hypochlorite salts. Common examples include sodium hypochlorite (household bleach) and calcium hypochlorite (a component of bleaching powder, swimming pool "chlorine"). The Cl-O distance in ClO− is 1.69 Å. The name can also refer to esters of hypochlorous acid, namely organic compounds with a ClO– moiety (chemistry), group covalent bond, covalently bound to the rest of the molecule. The principal example is tert-butyl hypochlorite, which is a useful chlorinating agent. Most hypochlorite salts are handled as aqueous solutions. Their primary applications are as bleaching, disinfection, and water treatment agents. They are also used in chemistry for Halogenation, chlorination and oxidation reactions. Reactions Acid reaction Acidification of hypochlorites generates hypochlorous acid, which exists in an equilibrium with chlorine. A high pH drives the reactio ... [...More Info...] [...Related Items...] OR: [Wikipedia] [Google] [Baidu] |
Perchloryl Fluoride
Perchloryl fluoride is a reactive gas with the chemical formula . It has a characteristic sweet odor that resembles gasoline and kerosene. It is toxic and is a powerful oxidizing and fluorinating agent. It is the acid fluoride of perchloric acid. In spite of its small enthalpy of formation (Δ''H''f° = −5.2 kcal/mol), it is kinetically stable, decomposing only at 400 °C. It is quite reactive towards reducing agents and anions, however, with the chlorine atom acting as an electrophile. It reacts explosively with reducing agents such as metal amides, metals, hydrides, etc. Its hydrolysis in water occurs very slowly, unlike that of chloryl fluoride. Synthesis and chemistry Perchloryl fluoride is produced primarily by the fluorination of perchlorates. Antimony pentafluoride is a commonly used fluorinating agent: : + 3 HF + 2 → + + 2 reacts with alcohols to produce alkyl perchlorates, which are extremely shock-sensitive explosives. In the presence of a Lewis acid, ... [...More Info...] [...Related Items...] OR: [Wikipedia] [Google] [Baidu] |
Chloryl
In chemistry, chloryl refers to a triatomic cation with chemical formula . This species has the same general structure as chlorite () but it is electronically different, with chlorine having a +5 oxidation state (rather than the +3 of chlorite). This makes it a rare example of a positively charged oxychloride. Chloryl compounds, such as and lO2RuF6], are all highly reactive and react violently with water and most organic compounds. Structure The cation is isoelectronic with , and has a bent structure with a bond angle close to 120°. The Cl–O bond is of bond order 1.5, with its Lewis structure consisting of a double bond and a dative bond which does not utilize d-orbitals. The red color of is caused by electron transitions into an antibonding orbital. The analogous transition in is not in the visible spectrum, so is colorless. The strength of interaction with the counterion affects the energy of this antibonding orbital; thus, in colorless chloryl compounds, strong inter ... [...More Info...] [...Related Items...] OR: [Wikipedia] [Google] [Baidu] |
Chlorine Tetroxide
Chlorine tetroxide is an unstable chlorine oxide with the chemical formula . History Gomberg's mistaken 1923 production In 1923, the famous radical chemist Moses Gomberg proposed a production method of chlorine tetroxide. He claimed that treating iodine and silver perchlorate in anhydrous diethyl ether produced it. :I2 + 2 AgClO4 → 2 AgI + (ClO4)2 However, later researchers claimed that the product was iodine perchlorate. So far, however, there is no certain evidence for the existence of iodine perchlorate either. Eachus' 1968 production In 1968, Eachus synthesized it by exposing potassium chlorate to gamma rays at 77 K. It is a reaction intermediate of the decomposition of dichlorine heptoxide. Properties The electron affinity energy of chlorine tetroxide can be figured out using the Born–Haber cycle and the lattice energy data of perchlorates. It is about 561 kJ/mol. The structure of chlorine tetroxide is uncertain; the molecular point group Molecular symmetry i ... [...More Info...] [...Related Items...] OR: [Wikipedia] [Google] [Baidu] |
Dichlorine Heptoxide
Dichlorine heptoxide is the chemical compound with the formula Cl2O7. This chlorine oxide is the anhydride of perchloric acid. It is produced by the careful distillation of perchloric acid in the presence of the dehydrating agent phosphorus pentoxide: :2 HClO4 + P4O10 → Cl2O7 + H2P4O11 The chlorine(VII) oxide can be distilled off from the mixture. It may also be formed by illumination on mixtures of chlorine and ozone. It slowly hydrolyzes back to perchloric acid. Structure Cl2O7 is an endergonic molecule, meaning it is intrinsically unstable, decomposing to its constituent elements with release of energy: :2 Cl2O7 → 2 Cl2 + 7 O2 (Δ''H°'' = –132 kcal/mol) Cl2O7 is bent with Cl−O−Cl angle of 118.6° giving the molecule C2 symmetry. The terminal Cl−O distances are 1.709 Å and the Cl=O distances are 1.405 Å. In this compound, chlorine exists in its highest formal oxidation state of +7, although the bonding in this molecule is significantly c ... [...More Info...] [...Related Items...] OR: [Wikipedia] [Google] [Baidu] |
