Alkaline Earth Metal

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by kaela1124
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Alkaline Earth Metal

Alkaline Earth Metals

Appearance The Group 2 elements are all metals with a shiny, silvery-white colour. General Reactivity The alkaline earth metals are high in the reactivity series of metals, but not as high as the alkali metals of Group 1.

History of Alkaline metals• By the early 1800s it became clear that the earths, formerly considered to be elements, were in fact oxides, compounds of a metal and oxygen. • The metals whose oxides make up the alkaline earths then came to be known as the alkaline-earth metals and have been classified in Group 2 (IIa) of the periodic table ever since Russian chemist Dmitry Mendeleyev proposed his first table in 1869.• Radium is a rare element, and all its isotopes are radioactive. There has never been commercial production of the metal, and, although its compounds were frequently used in the first half of the 20th century for cancer treatment, they have largely been superseded by less expensive alternatives.

Group 2 - The Alkaline Earth Metals beryllium (Be) [He]2s2 magnesium (Mg) [Ne]3s2 calcium (Ca) [Ar]4s2 strontium (Sr) [Kr]5s2 barium (Ba) [Xe]6s2 radium (Ra) [Rn]7s2 *last element is radium and is radioactive. Not considered.

Chemical Properties The elements have strong reducing power of the metals. They become increasingly electropositive on descending the Group. Once started, the reactions with oxygen and chlorine are vigorous.All the metals except beryllium form oxides in air at room temperature which dulls the surface of the metal. Barium is so reactive it is stored under oil.

uses!Magnesium is the only Group 2 element used on a large scale. It is used in flares, tracer bullets and incendiary bombs as it burns with a brilliant white light. It is also alloyed with aluminium to produce a low-density, strong material used in aircraft. Magnesium oxide has such a high melting point it is used to line furnaces.

Humphry Davy was an English chemist who discovered several alkali and alkaline earth metals

Because magnesium is about five times lighter than steel and 50% lighter than aluminum, it was long considered the “material of the future,” as shown in this 1950 concept Buick LeSabre

Physical Properties The metals of Group 2 are harder and denser than sodium and potassium, and have higher melting points. These properties are due largely to the presence of two valence electrons on each atom, which leads to stronger metallic bonding than occurs in Group 1.

alkaline earth metal's reaction to water is very violent due to the metal donating its two electrons to the water molecule which splits apart yielding hydrogen gas and quite a bit of heat energy


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