Alkaline earth metal: Difference between revisions
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The '''alkaline earth metals''' and are the [[chemical series|series]] of [[chemical element|elements]] in [[Periodic table group|Group 2]] ([[IUPAC]] style) of the [[periodic table]]: [[beryllium]] ('''Be'''), [[magnesium]] ('''Mg'''), [[calcium]] ('''Ca'''), [[strontium]] ('''Sr'''), [[barium]] ('''Ba''') and [[radium]] ('''Ra''') (though radium is not always considered an alkaline earth due to its [[radioactivity]]). |
The '''alkaline earth metals''' and are the [[chemical series|series]] of [[chemical element|elements]] in [[Periodic table group|Group 2]] ([[IUPAC]] style) of the [[periodic table]]: [[beryllium]] ('''Be'''), [[magnesium]] ('''Mg'''), [[calcium]] ('''Ca'''), [[strontium]] ('''Sr'''), [[barium]] ('''Ba''') and [[radium]] ('''Ra''') (though radium is not always considered an alkaline earth due to its [[radioactivity]]). |
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The alkaline earth |
The alkaline earth metals are named after their [[oxide]]s, the ''alkaline earths'', whose old-fashioned names were [[beryllia]], [[Magnesium oxide|magnesia]], [[Calcium oxide|lime]], [[strontia]] and [[baryta]]. These were named ''alkaline earths'' because of their intermediate nature between the [[alkali]]s (oxides of the [[alkali metal]]s) and the [[rare earth]]s (oxides of rare earth metals). The classification of some apparently inert substances as 'earths' is millennia old. The earliest known system used by the ancient [[Greece|Greeks]] consisted of four [[classical element|elements]], including earth. This system was later refined by philosophers and [[alchemy|alchemists]] such as [[Aristotle]] ([[4th century BC]]), [[Paracelsus]] (first half of [[16th century]]), [[J. J. Becher|John Becher]] (mid [[17th century]]) and [[Georg Ernst Stahl|Georg Stahl]] (late 17th century), with later thinkers subdividing 'earth' into three or more types. The realization that 'earths' were not elements but [[chemical compound|compound]]s is attributed to the chemist [[Antoine Lavoisier]]. In his ''Traité Élémentaire de Chimie'' (''Elements of Chemistry'') of [[1789]] he called them ''Substances simples salifiables terreuses'', or salt-forming earth elements. Later, he suggested that the alkaline earths might be metal oxides, but admitted that this was mere conjecture. In [[1808]], acting on Lavoisier's idea, [[Humphry Davy]] became the first to obtain samples of the metals by [[electrolysis]] of their molten earths. |
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The alkaline earth metals are silvery colored, soft, low-density [[metal]]s, which react readily with [[halogen]]s to form [[ionic salt]]s, and with [[water]], though not as rapidly as the [[alkali metal]]s, to form strongly [[alkali|alkaline]] ([[base (chemistry)|basic]]) [[hydroxide]]s. For example, where [[sodium]] and [[potassium]] react with water at room temperature, [[magnesium]] reacts only with [[steam]] and [[calcium]] with hot water. |
The alkaline earth metals are silvery colored, soft, low-density [[metal]]s, which react readily with [[halogen]]s to form [[ionic salt]]s, and with [[water]], though not as rapidly as the [[alkali metal]]s, to form strongly [[alkali|alkaline]] ([[base (chemistry)|basic]]) [[hydroxide]]s. For example, where [[sodium]] and [[potassium]] react with water at room temperature, [[magnesium]] reacts only with [[steam]] and [[calcium]] with hot water. |
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Revision as of 19:15, 28 November 2006
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| Group | 2 |
|---|---|
| Period | |
| 2 | title="Be, Beryllium" style="text-align:center; color:#000000; background-color:#ffdead; border:2px solid #6e6e8e; ;"| 4 Be |
| 3 | title="Mg, Magnesium" style="text-align:center; color:#000000; background-color:#ffdead; border:2px solid #6e6e8e; ;"| 12 Mg |
| 4 | title="Ca, Calcium" style="text-align:center; color:#000000; background-color:#ffdead; border:2px solid #6e6e8e; ;"| 20 Ca |
| 5 | title="Sr, Strontium" style="text-align:center; color:#000000; background-color:#ffdead; border:2px solid #6e6e8e; ;"| 38 Sr |
| 6 | title="Ba, Barium" style="text-align:center; color:#000000; background-color:#ffdead; border:2px solid #6e6e8e; ;"| 56 Ba |
| 7 | title="Ra, Radium" style="text-align:center; color:#000000; background-color:#ffdead; border:2px dashed #773300; ;"| 88 Ra |
The alkaline earth metals and are the series of elements in Group 2 (IUPAC style) of the periodic table: beryllium (Be), magnesium (Mg), calcium (Ca), strontium (Sr), barium (Ba) and radium (Ra) (though radium is not always considered an alkaline earth due to its radioactivity).
The alkaline earth metals are named after their oxides, the alkaline earths, whose old-fashioned names were beryllia, magnesia, lime, strontia and baryta. These were named alkaline earths because of their intermediate nature between the alkalis (oxides of the alkali metals) and the rare earths (oxides of rare earth metals). The classification of some apparently inert substances as 'earths' is millennia old. The earliest known system used by the ancient Greeks consisted of four elements, including earth. This system was later refined by philosophers and alchemists such as Aristotle (4th century BC), Paracelsus (first half of 16th century), John Becher (mid 17th century) and Georg Stahl (late 17th century), with later thinkers subdividing 'earth' into three or more types. The realization that 'earths' were not elements but compounds is attributed to the chemist Antoine Lavoisier. In his Traité Élémentaire de Chimie (Elements of Chemistry) of 1789 he called them Substances simples salifiables terreuses, or salt-forming earth elements. Later, he suggested that the alkaline earths might be metal oxides, but admitted that this was mere conjecture. In 1808, acting on Lavoisier's idea, Humphry Davy became the first to obtain samples of the metals by electrolysis of their molten earths.
The alkaline earth metals are silvery colored, soft, low-density metals, which react readily with halogens to form ionic salts, and with water, though not as rapidly as the alkali metals, to form strongly alkaline (basic) hydroxides. For example, where sodium and potassium react with water at room temperature, magnesium reacts only with steam and calcium with hot water.
Mg + 2H2O → Mg(OH)2 + H2
Beryllium is an exception: It does not react with water or steam, and its halides are covalent.
All the alkaline earth metals have two electrons in their outermost shell, so the energetically preferred state of achieving a filled electron shell is to lose two electrons to form doubly charged positive ions.
| bgcolor="Template:Element color/Alkaline earth metals" | Alkaline earth metals | Atomic numbers in Template:Element color/Solid indicate solids | style="border:Template:Element frame/Primordial;" | Solid borders indicate primordial elements (older than the Earth) | style="border:Template:Element frame/Natural radio;" | Dashed borders indicate natural radioactive elements with no isotopes older than the Earth |
External Links
- Science aid: Group 2 Metals Study aid for teens
