Barium electronic configuration

Indicate the position of beryllium, magnesium, calcium, strontium, and barium in Mendeleev s periodic table of the elements, the electron configurations and size of their atoms, and their oxidation states. 

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. 

This group contains the elements beryllium (Be), magnesium (Mg), calcium (Ca), strontium (Sr), barium (Ba) and radium (Ra). After the alkali metals, they are the second most active metals. Their electron configurations end with ns2. They become positive two charged ions by giving of their two valence electrons in chemical reactions. At room temperature, they occur in a monoatomic structure and they are solid at room temperature. Radium, a solid element, is the only radioactive member of this group. 

Using electron configurations, diagram the formation of an ionic bond between barium and nitrogen. 

Write the electron configurations of calcium, strontium, and barium atoms. Relate the charges on calcium, strontium, and barium ions to the electron configurations of their respective atoms. 

Write the condensed ground state electronic configuration for iodine, manganese, and barium. 

This shared electronic configuration has a more pragmatic importance in medicine. The similarity in electron shells allows strontium, barium, and radium to be absorbed in the same way as calcium in human and animal physiology—a phenomenon that leads to both a cause and a treatment for cancer. 

Fireworks Barium is a metal that gives a green color to fireworks. Write the electron configuration for barium. Classify it according to group, period, and block in the periodic table. 

The elements after Xe have this electronic configuration, plus electrons in the orbits of 4f, 5d, 6s, and so on. There are three elements. Cesium (Cs), barium (Ba), and lanthanum (La), between Xe and the RE elements. Cs has one 6s electron and Ba has two 6s electrons, while La has two 6s and one 5d electrons. When it comes to RE elements, the electrons start to fill the inner vacant 4f orbits. For instance, the first RE element Ce has only one electron in the f orbit, so that its configuration is [Xe]6s 4f 5d, while neodymium (Nd) has four electrons in the f orbit, i.e., its electron structure is [Xe]6s 4f. ... 

Write the electron configurations you would expect for barium and technetium (Z = 43). 

The sixth period consists of 32 elements. It is much longer than the periods that precede it in the periodic table. To build up electron configurations for elements of this period, electrons are added first to the 6s orbital in cesium, Cs, and barium, Ba. Then, in lanthanum. La, an electron is added to the 5d orbital. 

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