Electron configurations alkaline earth metals

In addition to having similar electron configurations, some blocks have common chemical characteristics, too. The block of elements on the far left of the illustration, for example, are all metals. The two groups in the block are called the alkali metals (first column) and alkaline earth metals (second column). The alkali metals are remarkably similar soft, silvery, highly reactive metals. The alkaline earth metals form another distinctive group that are much harder that the alkaline metals and have higher melting points. 

The alkaline earth metals in Group 2 of the periodic table must lose two electrons to reach a more stable state. Magnesium is an alkaline earth metal with an electron configuration of... 

As a consequence of its closed-shell electron configuration, zinc has a negative electron affinity, that is, the removal of an electron from Zn is exothermic. The electronegativity of zinc (1.588 PU) is intermediate between those of the alkaline earth metals and the first row transition metals and remarkably similar to that of beryllium (1.57 PU). 

The block s, on the left of the Table, contains the alkali and alkaline earth metals. Each atom of these metals possesses an inert gas core and one or two electrons in the s orbital of the valence shell, that is, an external electron configuration ns1 or ns2 where n is the value of the principal quantum number, and also the period number in the Periodic Table. Notice however that He, owing to its general chemical inertness and to the behaviour similarity with the other noble gasses is generally placed at the far right of the Table. The p block contains elements corresponding to electron... 

Symbol Be atomic number 4 atomic weight 9.012 a Group IIA (Group 2) metal the lightest alkaline-earth metallic element atomic radius l.OOA ionic radius (Be2+) 0.30A electronic configuration Is22s2 ionization potential, Be 9.32eV, Be + 18.21 eV oxidation state +2... 

Symbol Mg atomic number 12 atomic weight 24.305 a Group II A (Group 2) alkaline-earth metal atomic radius 1.60A ionic radius (Mg2+) 0.72A atomic volume 14.0 cm /mol electron configuration [Ne]3s2 valence +2 ionization potential 7.646 and 15.035eV for Mg+ and Mg2+, respectively three natural isotopes Mg-24(78.99%), Mg-25(10.00%), Mg-26(11.01%). 

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. 

The alkaline earth elements in group 2A—Be, Mg, Ca, Sr, Ba, and Ra—are similar to the alkali metals in many respects. They differ, however, in that they have ns2 valence-shell electron configurations and can therefore lose two electrons in redox reactions. Alkaline earth metals are thus powerful reducing agents and form ions with a +2 charge. 

The transition metals are our premier metals for jewelry making. They have electron configurations that are different from the alkali metals and the alkaline earth metals. Therefore, transition metals exhibit different chemical and physical properties. It is necessary to determine just where electrons reside in transition-metal atoms so we can understand the properties of transition metals and how they bond. To understand these properties and manners of bonding, we must revisit the electron cloud atomic model. 

The alkali metals have one outermost electron in an s orbital. This is a very unstable electron configuration, so the alkali metals are very reactive. The alkaline earth metals have two outermost electrons in an s orbital, making them somewhat reactive because an arrangement with eight outermost electrons is the most stable. The larger alkaline earth metals, strontium (Sr) and barium (Ba), are very reactive because those two outermost electrons are far from the nucleus. 

The alkali metals are the most chemically active metals. Alkaline earth metals are second in reactivity. Elements in the same family have the same outermost electron configuration. Alkali metals have one outermost electron that is easily transferred to needy atoms. Alkaline earth metals have two outermost electrons to share or transfer. The transition metals are the least active. 

Rare earth elements have similar configurations in the two outermost shells. They exhibit typical metallic properties in chemical reactions. They tend to lose three electrons and exhibit a 3+ valence state. From the Periodic Table of the elements, rare earth elements are classed as less reactive than alkali metals and alkaline earth metals but more reactive than other metals. They should be stored in an inert liquid otherwise they will be oxidized and lose their metal luster. The metal reactivity increases gradually from scandium to lanthanum and decreases gradually from lanthanum to lutetium. That is to say, lanthanum is the most reactive metal of the 17 rare earth elements. Rare earth metals can react with water and release hydrogen. They react more vigorously with acids but do not react with bases. 

The Group 2A elements (with the valence electron configuration ns2) are very reactive, losing their two valence electrons to form ionic compounds that contain M2+ cations. These elements are commonly called the alkaline earth metals because of the basicity of their oxides ... 

The alkaline-earth metals are slightly less reactive than the alkali metals. The alkaline-earth metals have two valence electrons and must lose both their valence electrons to get to a stable electron configuration. It takes more energy to lose two electrons than it takes to lose just the one electron that the alkali metals must give up to become stable. Although the alkaline-earth metals are not as reactive, they are harder and have higher melting points than the alkali metals. 

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