Group 1 Lithium Potassium Rubidium Sodium

The group in the Periodic Table with the least complicated chemistry is almost certainly the alkali-metal group lithium (Z — 3), sodium (Z 11), potassium (Z = 19), rubidium (Z 37), cesium (Z = 55), and the recently discovered francium (Z = 87). These elements follow directly after the inert gases and thus have one single valence electron beyond a well-shielded nucleus. 

Sodium is a member of the alkali metals family. The alkali family consists of elements in Group 1 (lA) of the periodic table. The periodic table is a chart that shows how chemical elements are related to one another. Other Group 1 (lA) elements are lithium, potassium, rubidium, cesium, and francium. The members of the alkali metals family are among the most active elements. 

The first group object of study was the alkali metals salts. By looking at the data some similarities between all of these salts of sodium, lithium, potassium, rubidium, and cesium (Tables 2.1-2.4, respectively) can be perceived. Although not from this group, the values of mean distance of closest approach of ions for silver salts presents some common features with the former ones (Table 2.9). It can be noticed that the ab initio values model I) and the values calculated fi om MM2-0 (or MM+ in case of silver) and Marcus data a = Rj+R ) are similar, whereas the values found from MM2-1 and the other Marcus data (a=d, + d, ), that is,... 

The table contains vertical groups of elements each member of a group having the same number of electrons in the outermost quantum level. For example, the element immediately before each noble gas, with seven electrons in the outermost quantum level, is always a halogen. The element immediately following a noble gas, with one electron in a new quantum level, is an alkali metal (lithium, sodium, potassium, rubidium, caesium, francium). 

Group l A (1). Lithium, Sodium, Potassium, Rubidium, Cesium... 

The ability of a metal alcoholate to accommodate an additional molecule of carbohydrate increases with increasing ionic radius " Li < Na < K < Cs. The difference in stoichiometry between lithium and sodium is much greater than that between either sodium and potassium, or potassium and cesium. The coordination number of an alkali metal is known to increase with increasing ionic radius. Brewer148 reported that the maximum number of donor groups oriented about an alkali metal cation is four for lithium, and as many as six for sodium, potassium, rubidium, or cesium. A greater surface area would allow accommodation of more than one carbohydrate moiety but, in addition, solvent molecules are more strongly attached to cations of smaller radius, and these may not be readily displaced by carbohydrate molecules. 

Group I consists of the five metals lithium, sodium, potassium, rubidium and caesium, and the radioactive element francium. Lithium, sodium and potassium are commonly available for use in school. They are all very reactive metals and they are stored under oil to... 

The alkali metals — lithium, sodium, potassium, rubidium, cesium, and francium — are members of Group 1 of the Periodic Table, and each has a single ns1 valence electron outside a rare gas core in its ground state. Some important properties of alkali metals are given in Table 12.1.1. 

The Equation of State of the Alkali Halides.—The alkali halides, the fluorides, chlorides, bromides, and iodides of lithium, sodium, potassium, rubidium, and caesium have been more extensively studied experimentally than any other group of ionic crystals. For most of these materials, enough data are available to make a fairly satisfactory comparison between experiment and theory. The observations include the compressibility and its change with pressure, at room temperature, from which the quantities ai(T), o2(r) of Eq. (1.1), Chap. XIII, can be found... 

The inclusion of iron, cobalt, nickel, and certain other metals in Group VIII.4 enables the alkali-metals lithium, sodium, potassium, rubidium, and caesium to be placed in their natural position as a subgroup of Group I. of the periodic system, in juxtaposition to the related sub-group containing copper, silver, and gold (p. 3). This arrangement... 

Moissan 7 found that the hydrides of lithium, sodium, potassium, rubidium, and caesium are non-conductors of electricity, and therefore cannot be regarded as alloys. He considered that in these compounds hydrogen has a metalloidic character, and that it is not comparable with the metals, an argument against its inclusion in Group I.8... 

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. 

Compared to lithium and sodium borohydride, potassium borohydride has the highest hydrogen desorption temperature of 584 °C and melting temperature of 607 °C [25]. The hydrogen content is 7.7 wt.%. Potassium borohydride crystallizes in the cubic NaCl-type structure (space group Fm3m) as do sodium, rubidium, and caesium borohydrides. [BH4] units are octahedrally coordinated by K atoms. 

II. GROUP 1 LITHIUM, SODIUM, POTASSIUM, RUBIDIUM AND CESIUM... 

The elements of the first group, lithium, sodium, potassium, rubidium, and cesium, are soft, silvery-white metals with great chemical reactivity. These elements are called the alkali metals. These metals are excellent conductors of electricity. Some of their physical properties are given in Table 91. It can be seen from the table that they melt at low temperatures—four of the five metals melt below the boiling point of water. The metals lithium, sodium, and potassium are lighter than water. 

Pure elements at room temperature and atmospheric pressure can be solids, liquids, or gases. Some elements are colorless. Others, like the ones shown in Figure 1, are colored. Despite the differences between elements, groups of elements share certain properties. For example, the elements lithium, sodium, potassium, rubidium, and cesium can combine with chlorine in a 1 1 ratio to form LiCl, NaCl, KCl, RbCl, and CsCl. All of these compounds are white solids that dissolve in water to form solutions that conduct electricity. 

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