Group magnesium radium strontium

FIGURE 14.19 The elements of Croup 2 (a) beryllium (b) magnesium (c) calcium id) strontium and (c) barium. The four central elements of the group (magnesium through barium) were discovered bv I lumphry Davy in a single year (1 808). The two outer elements were discovered later beryllium in 1828 (by Friedrich Wohler) and radium (which is not shown here) in 1898 (by Pierre and Marie Curie). 

In many of its chemical properties, radium is like the elements magnesium, caldum, strontium and barium, and it is placed in group 2, as is consistent with its 6s26pcls2 electron configuraUon. Its sulfate (Ksp — 4.2 a 10-1 ) is even more insoluble in water than barium sulfate, with which it is conveniently coprecipitated, Like barium and other alkaline earth metals, it forms a soluble chloride (X p = 0,4) and bromide, which can also be obtained as dihydrates, Radium also resembles the other group 2 elements in forming an insoluble carbonate and a very slightly soluble lodate (Xsp = 8.8 x 1(T10). 

Group II consists of the five metals beryllium, magnesium, calcium, strontium and barium, and the radioactive element radium. Magnesium and calcium are generally available for use in school. These metals have the following properties. 

Beryllium, magnesium, calcium, strontium, barium, and radium constitute Group 2 in the Periodic Table. These elements (or simply the Ca, Sr, and Ba triad) are often called alkaline-earth metals. Some important properties of group 2 elements are summarized in Table 12.5.1. 

Alkali metals lithium, sodium, potassium, rubidium, cesium, and francium. Metals such as sodium and potassium (the alkali metals) react violently with water—too violently to conduct experiments. The group 2 metals (also called alkaline earth metals) react less readily and can be used in the laboratory. Alkaline earth metals, including beryllium, magnesium, calcium, strontium, barium, and radium. 

In previous arrangements of the Periodic Table see Periodic Table Trends in the Properties of the Elements), the elements beryllium, magnesium, calcium, strontium, barium, and radium were referred to as members of Group Ila, or 2A. As inclusion of the word metaT in their title implies, these elements are both malleable and extrudable however, they are rather brittle. They are electrical conductors. When pure, all except the lightest, beryllium, react with atmospheric... 

Barium is a member of the alkaline earth metals. The alkaline earth metals make up Group 2 (IIA) of the periodic table. The other elements in this group are beryllium, magnesium, calcium, strontium, and radium. These elements tend to be relatively active chemically and form a number of important and useful compounds. They also tend to occur abundantly in Earth s crust in a number of familiar minerals such as aragonite, calcite, chalk, limestone, marble, travertine, magnesite, and dolomite. Alkaline earth compounds are widely used as building materials. 

Radium is a radioactive element in Group 2 (IIA) and Row 7 of the periodic table. The periodic table is a chart that shows how chemical elements are related to each other. Radium was discovered in 1898 by Marie Curie (1867-1934) and her husband, Pierre Curie (1859-1906). It was found in an ore of uranium called pitchblende. The alkaline earth metals also include beryllium, magnesium, calcium, strontium, and barium. 

The alkaline earths, beryllium, magnesium, calcium, strontium, barium, and radium, together constitute Group 2 of the periodic table. They are usually found in relatively un-reactive forms, bound to oxygen the free metals still have a tendency to lose their outer electrons, but less easily than the Group 1 elements, and are a little less reactive. 

Group 2 of the periodic table contains the alkaline earth metals beryllium, magnesium, calcium, strontium, barium, and radium. These elements are similar to the alkali metals in that they are shiny, ductile, and malleable. The alkaline earth metals have two electrons in their outermost shell. Although they are not as reactive as the alkali metals, the alkaline earth metals are rarely found pure in nature. 

BERYLLIUM AND THE GROUP II elements Mg, Ca, Sr, Ba, Ra 215 MAGNESIUM, CALCIUM, STRONTIUM, BARIUM AND RADIUM 7-8. Occurrence the Elements... 

The Group HA elements are called alkaline earfli metals. The alkaline earth metals consist of beiyllium, magnesium, calcium, strontium, baritim, and radium. Their oxides are basic. They have a valence shell configuration of ns, and exhibit an oxidation state of +2. These elements are not as reactive as alkali metals. 

The metals of group 11 of the periodic table —beryllium, magnesium, calcium, strontium, barium, and radium—are called the alkaline-earth metals. Some of their properties are listed in Table 18-2. These metals are much harder and less reactive than the alkali metals because there are twice as many valence electrons. The compounds of all the alkaline-earth metals are similar in composition they all form oxides MO, hydroxides M(0H)2, carbonates MCO3, sulfates MSO4, and other compounds (M = Be, Mg, Ca, Sr, Ba, or Ra). 

Notice that they are numbered from 1 to 18 from left to right. Each group contains elements with similar chemical properties. For example, the elements in Group 2 are beryllium, magnesium, calcium, strontium, barium, and radium. All of these elements are reactive metals with similar abilities to bond to other kinds of atoms. The two major categories of elements are metals and nonmetals. Metalloids have properties intermediate between those of metals and nonmetals. 

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). 

Beryllium and magnesium belong to the 2nd group of the Periodic Table together with calcium, strontium, barium and radium. Characteristic differences, however, may be noticed between the chemistry of Be and Mg and that of the alkaline earth s proper. Be has a unique chemical behaviour with a predominantly covalent character. The heavier elements (Ca, Sr, Ba, Ra) have a predominant ionic behaviour in their compounds. Mg has a chemistry in a way intermediate but closer to that of Be. Analogies between the Mg and Zn chemistries may also be underlined. 

Strontium has four naturally occurring isotopes (Table 4.2). It is a member of the alkaline earths (Group 2A) along with beryllium, magnesium, calcium, barium, and radium (Fig. 2.4). Strontium substitutes for calcium and is abundant in minerals such as plagioclase, apatite, and calcium carbonate. 

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