Nonmetal Chlorides

As might be expected, basic solutions may be titrated with acidic solutions and the neutralization followed by conductometric, potenliometric, photometric, and similar methods. Some metal and nonmetal chlorides are amphoteric in phosphorus oxychloride ... 

Name three nonmetal chlorides for which this method of preparation will not work. 

Nonmetal Chlorides - Compounds such as phosphorous trichloride and corresponding bromides react violently with water and are a common cause of laboratory accidents. 

Nickel Aluminum, aluminum(III) chloride, ethylene, 1,4-dioxan, hydrogen, methanol, nonmetals, oxidants, sulfur compounds... 

Compounds containing fluorine and chlorine are also donors to BF3. Aqueous fluoroboric acid and the tetrafluoroborates of metals, nonmetals, and organic radicals represent a large class of compounds in which the fluoride ion is coordinating with trifluoroborane. Representative examples of these compounds are given in Table 5. Coordination compounds of boron trifluoride with the chlorides of sodium, aluminum, iron, copper, 2inc, tin, and lead have been indicated (53) they are probably chlorotrifluoroborates. 

Berzehus (19) further appHed and amplified the nomenclature introduced by Guyton de Morveau and Lavoisier. It was he who divided the elements into metalloids (nonmetals) and metals according to their electrochemical character, and the compounds of oxygen with positive elements (metals) into suboxides, oxides, and peroxides. His division of the acids according to degree of oxidation has been Httie altered. He introduced the terms anhydride and amphoteric and designated the chlorides in a manner similar to that used for the oxides. 

Zirconium chloride and bromide have closely related but dissimilar stmctures. Both contain two metal layers enclosed between two nonmetal layers which both have hexagonal stmcture. In ZrCl, the four-layer sandwich repeats in layers stacked up according to /abca/bcab/cabc/, whereas the ZrBr stacking order is /abca/cabc/bcab/ (188). Both are metallic conductors, but the difference in packing results in different mechanical properties the bromide is much more brittle. 

The main metals in brines throughout the world are sodium, magnesium, calcium, and potassium. Other metals, such as lithium and boron, are found in lesser amounts. The main nonmetals ate chloride, sulfate, and carbonate, with nitrate occurring in a few isolated areas. A significant fraction of sodium nitrate and potassium nitrate comes from these isolated deposits. Other nonmetals produced from brine ate bromine and iodine. 

Chemical reaction A process in which one or more substances, called reactants, are converted to product(s), 67. See also Reaction, nonmetals, 575q, 555-558 Chernobyl nuclear accident, 525-526 Chiral center Carbon atom bonded to four different groups, 600 Chiral drugs, 601 Chloride ores, 535-536 Chlorinated water, 556 Chlorine... 

In general, binary compounds of two nonmetals are molecular, whereas binary compounds formed by a metal and a nonmetal are ionic. Water (H20) is an example of a binary molecular compound, and sodium chloride (NaCl) is an example of a binary ionic compound. As we shall see, these two types of compounds have... 

A salt derived from a hydracid is named according to the nonmetal present in the parent acid, and the salt will end in - ide . The metallic part of the salt is named first. The prefix hydro is dropped and suffix - ic (of the acid) is changed to - ide . HC1 HBr HCN H2S Sodium chloride (NaCl) Magnesium chloride (MgCl2) Potassium bromide (KBr) Zinc bromide (ZnBr2) Sodium cyanide (NaCN) Potassium sulfide (K2S)... 

Naming bases is a little more straightforward. For a base name, chemists just use the name of the chemical compound. They do the same thing for the salts that are produced when acids and bases react with one another. The salt sodium chloride (NaCl), for example, is named for the two elements that are present in the salt—sodium and chlorine. The only rule is to change the ending for the name of the nonmetal (in this case, chlorine) to -ide, giving us the name sodium chloride. 

Nitrogen trichloride. Although this is a binary compound of two nonmetals, it can be named with Roman numeral designations. It is indeed possible to call this nitrogen(III) chloride in the most modern usage, but most chemists do not do that yet. 

If you electrolyze a solution containing a compound of a very active metal and/or a very active nonmetal, the water (or other solvent) might be electrolyzed instead of the ion. For example, if you electrolyze molten sodium chloride, you get the free elements ... 

Atomic hydrogen is a powerful reducing agent, even at room temperature. For example, it reacts with the oxides and chlorides of many metals, including silver, copper, lead, bismuth, and mercury, to produce the free metals. It reduces some salts, such as nitrates, nitrites, and cyanides of sodium and potassium, to the metallic state. It reacts with a number of elements, both metals and nonmetals, to yield hydrides such as NH3, NaH, KH, and PH3. Sulfur forms a number of hydrides the simplest is H2S. Combining with oxygen, atomic... 

Nitropropane Nitrosyl fluoride Nitrosyl perchlorate Nitrourea Nitrous acid Nitryl chloride Oxalic acid See under Nitromethane chlorosulfonic acid, oleum Haloalkenes, metals, nonmetals Acetones, amines, diethyl ether, metal salts, organic materials Mercury(II) and silver salts Phosphine, phosphorus trichloride, silver nitrate, semicarbazone Ammonia, sulfur trioxide, tin(IV) bromide and iodide Furfuryl alcohol, silver, mercury, sodium chlorate, sodium chlorite, sodium hypochlorite... 

Assume that the oxygen array is perfect and identical to the nonmetal atom array in the sodium chloride structure and that the unit cell contains some vacancies on the iron positions. In this case, one unit cell will contain 4 atoms of oxygen and (4/1.058) atoms of iron, that is, 4Feo.94sO. The density is calculated to 5741 kg m-3. 

Cadmium oxide, CdO, like nickel oxide, also adopts the sodium chloride structure (Fig. 1.14). However, unlike nickel oxide, this compound can be made to contain more metal than oxygen. The defects that cause this metal excess are usually considered to be interstitial Cd atoms or ions. In this case the reaction is one in which the solid formally loses oxygen. Because of the rules of equation writing, this must involve the removal of neutral oxygen atoms. Each oxygen lost results in the loss of a nonmetal site. In order to keep the site ratio correct, a metal site must also be lost, forcing the metal into interstitial sites ... 

The most stable cluster consists of an aggregation of four cation vacancies in a tetrahedral geometry surrounding an Fe3+ ion, called a 4 1 cluster. Cations in the sodium chloride structure normally occupy octahedral sites in which each metal is coordinated to six nonmetal atoms. The central Fe3+ ion in the 4 1 cluster is displaced into a normally unoccupied tetrahedral site in which the cation is coordinated to four oxygen ions. Because tetrahedral sites in the sodium chloride structure are normally empty, the Fe3+ is in an interstitial site. Equation (4.1) can now be written correctly as... 

Ionization is the process whereby a chemical reaction forms ions (atoms with a negative or positive charge) from the breakup of neutral molecules of some inorganic compounds. A common example is the neutral molecule of sodium chloride (NaCl, salt). When it dissociates (breaks apart) into positive metalhc ions of Na by the loss of an electron, the nonmetal chlorine ion Cl" gains the negative charge given up by the sodium atom. 

Chlorine forms ionic bonds with almost all the metals and molecular bonds with the semimetals and nonmetals. With group 1 metals it produces well-known salts when chlorine s —1 ion combines with this group s +1 ions (e.g, NaCl, LiCl, and KCl). Group 2 metals have +2 ions and thus, when combined with —1 ions of chlorine, form salts such as magnesium chloride (MgCl ), calcium chloride (CaCy, and barium chloride (BaCy. 

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