Group II - the alkaline earth metals

Group I The alkali metals Group II The alkaline earth metals Group VII The halogens Group 0 Inert gases or noble gases... 

Group II, the alkaline-earth metals These metals, beryllium, magnesium, calcium, strontium, barium, and radium, and their compounds are discussed in Chapter 9. 

Group II. The alkaline-earths metals Magnesium 12 Calcium 20 Strontium 43.8 Barium 68.5. In this group, the strontium is the average between calcium and barium. 

Compounds of the first of the above-mentioned classes are conveniently called "metal-like refractory compounds, in view of their external and, particularly, internal resemblance to metals and intermetallic compounds The chemical bond in the lattices of these compounds, in addition to the s and p electrons of the metallic and nonmetallic components, respectively, is also formed by the electrons of the deeper, incomplete d and / levels of the transition metals, to which belong almost all metallic components of the metal-like refractory compounds. Isolated atoms of metals of the odd subgroup of group II, the alkaline earth metals, do not have any electrons in the d and / shells, but in compounds with nonmetals, energy states corresponding to these shells may occur. 

The Alkaline Earth Metals and their Associates (Group II. of the Periodic Table). By Miss M S. Leslie, D.Sc. 

The Alkaline Earth Metals and their Associates (Group II. of the Periodic Table). By Miss M. S. Leslie, D.Sc. Aluminium and its Congeners, including the Rare Earth Metals (Group III. of the Periodic Table). By H. F. V. Little, B.Sc. (Lond.), A.R.C.S., Chief Chemist to Thorium, Ltd. 

Group 2 cations form sulfide salts which are insoluble in dilute hydrochloric acid, HCl, solution. Be careful not to confuse these cations with the alkaline earth metal cations from group II in the periodic table which all form sulfide salts that are soluble even in water. We shall consider only Bi t, Cd2+, Cu2+, Pb2+, and Hg2+, though additional cations also form insoluble sulfide salts in dilute HCl solution. Assuming that Ag+ and <32 t and much of the Pb2+, have already been isolated (since they also exhibit this behavior), the group 2 cations are isolated from a mixture of cations because they precipitate black (except for yellow CdS), insoluble... 

However, copper forms two positive ions copper(i), Cu and copper(ii), Cu. Hence the name copper is ambiguous. The names of copper compounds should start with either copper(i) or copper(ii). These Roman numbers actually represent the oxidation state (Chapter 9) but this is related to the charge. The elements that form just one positive ion are the alkali metals (Group 1 metals) and the alkaline earth metals (Group 2 metals). The transition metals often form a range of stable positive ions. For example, iron forms iron(ii), Fe, and iron(iii), Fe ... 

Group 1 is often called the alkali metals Group II is the alkaline earth metals Group Vn is the halogens Group O is the noble gases. 

These elements form two groups, often called the alkali (Group I) and alkaline earth (Group II) metals. Some of the physical properties usually associated with metals—hardness, high m.p. and b.p.—are noticeably lacking in these metals, but they all have a metallic appearance and are good electrical conductors. Table 6.1 gives some of the physical properties. 

The elements in Group II of the Periodic Table (alkaline earth metals) are. in alphabetical order, barium (Ba). beryllium (Be), calcium (Ca). magnesium (Mg), radium (Ra) and strontium (Sr). 

The alchemists of the Middle Ages found that some substances could not be dissolved in water or transformed by fire. They called these substances earths. If the alchemists had known how to break them apart, as chemists can today, they would have found them to be composed of oxygen and the metals from Group II. The six alkaline-earth metals comprising Group II on the periodic chart are ... 

Alkali and alkaline earth metals. Results obtained for the group I and group II atoms are encouraging. As Table 5.6 shows, calculations for the alkali atoms are slightly more reliable than those for the alkaline earths. The largest error obtains for the quasidegenerate Be atom. ECP bases provide a convenient alternative to all-electron treatments. 

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