Alkaline metals

Oxygen Acetaldehyde, acetone, alcohols, alkali metals, alkaline earth metals, Al-Ti alloys, ether, carbon disulflde, halocarbons, hydrocarbons, metal hydrides, 1,3,5-trioxane... 

Alkaline cell Alkaline chlorination Alkaline coupling Alkakne-earth metals Alkaline earths... 

D very weak or inactive many metal, alkaline-earth, and rare-earth element haUdes... 

Alkali metal haHdes can be volatile at incineration temperatures. Rapid quenching of volatile salts results in the formation of a submicrometer aerosol which must be removed or else exhaust stack opacity is likely to exceed allowed limits. Sulfates have low volatiHty and should end up in the ash. Alkaline earths also form basic oxides. Calcium is the most common and sulfates are formed ahead of haHdes. Calcium carbonate is not stable at incineration temperatures (see Calcium compounds). Transition metals are more likely to form an oxide ash. Iron (qv), for example, forms ferric oxide in preference to haHdes, sulfates, or carbonates. SiHca and alumina form complexes with the basic oxides, eg, alkaH metals, alkaline earths, and some transition-metal oxidation states, in the ash. 

Orthophosphate salts are generally prepared by the partial or total neutralization of orthophosphoric acid. Phase equiUbrium diagrams are particularly usehil in identifying conditions for the preparation of particular phosphate salts. The solution properties of orthophosphate salts of monovalent cations are distincdy different from those of the polyvalent cations, the latter exhibiting incongment solubiUty in most cases. The commercial phosphates include alkah metal, alkaline-earth, heavy metal, mixed metal, and ammonium salts of phosphoric acid. Sodium phosphates are the most important, followed by calcium, ammonium, and potassium salts. 

From Metals and Alcohol. Alkali metals, alkaline earth metals, and aluminum react with alcohols to give metal alkoxides (2,3,65) ... 

The speed of the reaction depends both on the metal and on the alcohol, increasing as electropositivity iacreases and decreasiag with length and branching of the chain. Thus sodium reacts strongly with ethanol, but slowly with tertiary butyl alcohol. The reaction with alkaU metals is sometimes carried out ia ether, ben2ene, or xylene. Some processes use the metal amalgam or hydride iastead of the free metal. Alkaline earth metals and aluminum are often covered with an oxide film which hinders the reaction. 

Boron tnhahdes can be reduced to elemental boron by heating and presence of alkah metals, alkaline-earth metals, or (22—26) such reductions... 

Hydrogen can be prepared by the reaction of water or dilute acids on electropositive metals such as the alkali metals, alkaline earth metals, the metals of Groups 3, 4 and the lanthanoids. The reaction can be explosively violent. Convenient laboratory methods employ sodium amalgam or calcium with water, or zinc with hydrochloric acid. The reaction of aluminium or ferrosilicon with aqueous sodium hydroxide has also been used. For small-scale preparations the hydrolysis of metal hydrides is convenient, and this generates twice the amount of hydrogen as contained in the hydride, e.g. ... 

Using tables of free energies of formation it is clear that most metals will react with most HX. Moreover, in many cases, e.g. with the alkali metals, alkaline earth metals, Zn, A1 and the lanthanide elements, such reactions are extremely exothermic. It is also clear that Ag should react with HCl, HBr and HI but not with HF, and... 

For all three halates (in the absence of disproportionation) the preferred mode of decomposition depends, again, on both thermodynamic and kinetic considerations. Oxide formation tends to be favoured by the presence of a strongly polarizing cation (e.g. magnesium, transition-metal and lanthanide halates), whereas halide formation is observed for alkali-metal, alkaline- earth and silver halates. 

Cations with noble gas configurations. The alkali metals, alkaline earths and aluminium belong to this group which exhibit Class A acceptor properties. Electrostatic forces predominate in complex formation, so interactions... 

PEO is found to be an ideal solvent for alkali-metal, alkaline-earth metal, transition-metal, lanthanide, and rare-earth metal cations. Its solvating properties parallel those of water, since water and ethers have very similar donicites and polarizabilities. Unlike water, ethers are unable to solvate the anion, which consequently plays an important role in polyether polymer-electrolyte formation. 

An important class of expl materials contains metallic fuels and inorganic oxidants. Examples are Tritonal (TNT/A1, 80/20), Amatols (TNT/AN, 28/80 80/20), and Minol-2 (TNT/AN/A1, 40/40/20). Oxidants other than nitrates, such as chlorates and perchlorates, may be employed. Water solns containing these cations are highly corrosive to metals. Alkaline metal salts, for example, in the presence of moisture, will pit A1 quickly (Ref 6)... 

In these cases, one is limited to the growth of single crystals of the transition metals since it is those metals which form volatile carbonyl compounds. The alkali metals, alkaline earth metals and certain of those elements which are allotropic in nature are not at aH suited for this type of crystal growth. 

A borate crosslinking agent can be boric acid, borax, an alkaline earth metal borate, or an alkali metal alkaline earth metal borate. The borate source, calculated as boric oxide, must be present in an amount of 5% to 30% by weight. 

Store OPA in a cool, well-ventilated area away from heat, open flame. Avoid contact with water mists or sprays, metals, alkaline materials, and some organics. Reacts readily with DF or DC, producing extremely toxic compounds (GB or a chlorine compound similar to GB). 

Stability Does not spontaneously decomposes but is reactive. Avoid contact with water mists or sprays, metals, alkaline materials, and some organics. 

Greenberg and Kingston [821,822] used a solid Chelex 100 resin to preconcentrate these elements from 100-500 ml of estuarine and seawater prior to their determination. A procedure is described for the preconcentration of 100 ml of estuarine and seawater into a solid sample using Chelex 100 resin. This solid sample weighs less than 0.5 g, and contains the transition metals and many other elements of interest, but is essentially free of alkali metals, alkaline earth metals, and halogens. 

The considerable difficulty of trace element analysis in a high salt matrix such as seawater, estuarine water, or brine is clearly reflected in the literature. The extremely high concentrations of the alkali metals, alkaline earth metals, and... 

Relationships in the periodic table horizontal, vertical, and diagonal with examples from alkali metals, alkaline earth metals, halogens, and the first series of transition elements... 

Salt effects (chlorides and bromides of alkali metal, alkaline earth, and ammonium cations) on rate constants for aquation of [Fe(bipy3] " " and [Fe(phen)3] " " in aqueous solution have been interpreted in terms of added cation effects on the activity of the water. 

When small amounts of alkali metals, alkaline earth metals, or their salts are introduced into a gaseous flame, flame reactions occur relatively easily at low temperatures.The liberated metal atoms are promoted to excited states and then return to their normal states. Radiation corresponding to the characteristic line spectra of the individual metal atoms is emitted as a result of this energy transition. Colored radiation discernible by the human eye, ranging from red to blue, is dependent on the type of metal atoms, as shown in Table 12AP- i... 

Sulfides s - Insoluble, except alkali metals, alkaline earths, and ammonium. 

Toxicity Variable. The hydrides of phosphorus, arsenic, sulfur, selenium, tellurium and boron which are highly toxic, produce local irritation and destroy red blood cells. They are particularly dangerous because of their volatility and ease of entry into the body. The hydrides of the alkali metals, alkaline earths, aluminum, zirconium and titanium react with moisture to evolve hydrogen and leave behind the hydroxide of the metallic element. This hydroxide is usually caustic. See also sodium hydroxide... 

In fact, the oxidation of metals with very low work functions (alkali metals, alkaline earth metals) proceeds very quickly at room temperatures and more slowly at 83 K. If the work function of the metal has a medium-sized value, it is increased by oxygen, e.g., that of tungsten from 4.53 to 6.27 volts, or by 1.74 volts, according to the measurements of the contact potential by Bosworth and Rideal (12). In this case oxygen is adsorbed in the form of atoms. No oxidation was observed at low tem-... 

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