Alkaline-earth metal An element

Alkaline earth metal An element found in Group 2 (IIA) of the periodic table. 

The s blink elements Croups lA and IIA (Cuhtmns I ami 2). the alkali and alkaline earth metals. These elements arc also sometimes called the light metals . They are characterized by an electron configuration of ns1 or ns2 over a core with a noble gas configuration. 

As shown in Table 8 the stability of metal complexes of EDTA increases as the charge on the cation M"H increases and it is greater for transition metals than for the alkaline earths. If an element exists in more than one valency state, that in the higher oxidation state forms the more stable complex. The position of equilibrium in the reaction... 

Chloride-Containing Catalyst. Two patent applications were submitted by Wohlfahrt et al. involving many catalysts PbO on various supports chlorides, bromides, and iodides of the alkali and alkaline earth metals the elements of Group IIIB elements having an atomic number of 24 to 30 the La elements and Ag Cd Pb and Bi. A conversion of 14.4% and 90% C,+... 

You can often determine the charge an ion normally has by the element s position on the periodic table. For example, all the alkali metals (the lA elements) lose a single electron to form a cation with a 1+ charge. In the same way, the alkaline earth metals (OA elements) lose two electrons to form a 2+ cation. Aluminum, a member of the mA family, loses three electrons to form a 3+ cation. 

The Group IIA elements are also known as the alkaline earth metals. These metals illustrate the expected periodic trends. If you compare an alkaline earth metal with the alkali metal in the same period, you see that the alkaline earth metal is less reactive and a harder metal. For example, lithium reacts readily with water, but beryllium reacts hardly at all even with steam. Lithium is a soft metal, whereas berylUum is hard enough to scratch glass. You also see the expected trend within the column of alkaline earth metals the elements at the bottom of the column are more reactive and are softer metals than those at the top of the column (Figure 22.9). Barium, in the sixth period, is a very reactive metal and, when placed in watCT, reacts much like an alkali metal. It is also a soft metal, much like the alkah metals. Magnesium, in the third period, is much less reactive and a harder metal (comparable to aluminum). 

Classify each of the following as an alkali metal, alkaline earth metal, transition element, halogen, or noble gas ... 

The calculations indicate that the 8 subsheU should fiU at elements 119 and 120, thus making these an alkaH and alkaline earth metal, respectively. Next, the calculations point to the filling, after the addition of a 7t7 electron at element 121 of the inner 5 and (if subsheUs, 32 places in aU, which the author has termed the superactinide elements and which terminates at element 153. This is foUowed by the filling of the 7d subsheU (elements 154 through 162) and 8 subsheU (elements 163 through 168). 

BeryUium reacts with fused alkaU haUdes releasing the alkaU metal until an equUibrium is estabUshed. It does not react with fused haUdes of the alkaline-earth metals to release the alkaline-earth metal. Water-insoluble fluoroberyUates, however, are formed in a fused-salt system whenever barium or calcium fluoride is present. BeryUium reduces haUdes of aluminum and heavier elements. Alkaline-earth metals can be used effectively to reduce beryUium from its haUdes, but the use of alkaline-earths other than magnesium [7439-95-4] is economically unattractive because of the formation of water-insoluble fluoroberyUates. Formation of these fluorides precludes efficient recovery of the unreduced beryUium from the reaction products in subsequent processing operations. 

Calcium [7440-70-2J, Ca, a member of Group 2 (IIA) of the Periodic Table between magnesium and strontium, is classified, together with barium and strontium, as an alkaline-earth metal and is the lightest of the three. Calcium metal does not occur free in nature however, in the form of numerous compounds, it is the fifth most abundant element constituting 3.63% of the earth s cmst. 

The carbides of the lanthanoids and actinoids can be prepared by heating M2O3 with C in an electric furnace or by arc-melting compressed pellets of the elements in an inert atmosphere. They contain the C2 unit and have a stoichiometry MC2 or M4(C2)3. MC2 have the CaC2 structure or a related one of lower symmetry in which the C2 units lie at right-angles to the c-axis of an orthogonal NaCl-type cell. They are more reactive than the alkaline-earth metal... 

A mercury cathode finds widespread application for separations by constant current electrolysis. The most important use is the separation of the alkali and alkaline-earth metals, Al, Be, Mg, Ta, V, Zr, W, U, and the lanthanides from such elements as Fe, Cr, Ni, Co, Zn, Mo, Cd, Cu, Sn, Bi, Ag, Ge, Pd, Pt, Au, Rh, Ir, and Tl, which can, under suitable conditions, be deposited on a mercury cathode. The method is therefore of particular value for the determination of Al, etc., in steels and alloys it is also applied in the separation of iron from such elements as titanium, vanadium, and uranium. In an uncontrolled constant-current electrolysis in an acid medium the cathode potential is limited by the potential at which hydrogen ion is reduced the overpotential of hydrogen on mercury is high (about 0.8 volt), and consequently more metals are deposited from an acid solution at a mercury cathode than with a platinum cathode.10... 

Quaternary chalcogenides of the type A Ln M X, containing three metal elements from different blocks of the Periodic Table (A is an alkali or alkaline earth metal, Ln is an /-block lanthanide or scandium, M is a p-block main group or a r/-block transition metal, and X is S or Se) are also known [65]. 

Metal hydrides containing transition metal (TM)-hydrogen complexes, with the transition metal in a formally low oxidation state, are of fundamental interest for clarifying how an electron-rich metal atom can be stabilized without access to the conventional mechanism for relieving the electron density by back-donation to suitable ligand orbitals. By reacting electropositive alkali or alkaline earth metals ( -elements) with group 7, 8, 9, and 10 transition metals in... 

King, R. B. (1995). Inorganic Chemistry of the Main Group Elements. VCH Publishers, New York. An excellent introduction to the descriptive chemistry of many elements. Chapter 10 deals with the alkali and alkaline earth metals. 

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