are alkaline earth metals radioactive?
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All of the alkaline earth metals, except magnesium and strontium, have at least one naturally occurring radioisotope: beryllium-7, beryllium-10, and calcium-41 are trace radioisotopes. Calcium-48 and barium-130 have very long half-lives and thus occur naturally. All isotopes of radium are radioactive.
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Alkali metals are the elements in group 1 of the periodic table. Alkaline earth metals are the elements in group 2 of the periodic table. ... The main difference between alkaline and alkali is that alkali metals have one valence electron, whereas alkaline earth metals have two valence electrons.
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So we just covered the alkali metals in Group I. You will find the alkaline earth metals right next door in Group II. This is the second most reactive family of elements in the periodic table.
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Elements in this group are called alkaline Earth metals. These metals are silver or gray in color. They are relatively soft and low in density, although not as soft and lightweight as alkali metals.
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Reactions of Alkaline Earth Metals All the alkaline earth metals except beryllium also react with water to form strongly alkaline hydroxides which should be handled with great care. The heavier alkaline earth metals react more vigorously than the lighter ones.
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The alkaline earth elements are metallic elements found in the second group of the periodic table. All alkaline earth elements have an oxidation number of +2, making them very reactive. Because of their reactivity, the alkaline metals are not found free in nature.
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The Brainliest Answer! The alkaline earth metals are six chemical elements in group 2 of the periodic table. They are beryllium(Be), magnesium (Mg), calcium (Ca), strontium (Sr), barium (Ba), and radium (Ra).
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Alkaline Earth Metal Properties Atoms have a low electron affinity and low electronegativity. All of the alkaline earths are shiny, silver-colored metals at ordinary temperatures and pressure. These metals are malleable and ductile.
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Interesting Facts about Alkaline Earth Metals The name "alkaline earths" comes from an old name for the oxides of the elements. They are called alkaline because they form solutions with a pH greater than 7, making them bases or "alkaline." Radium is formed from the decay of uranium.
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Radium is the sixth element of the second column in the periodic table. It is the heaviest of the alkaline earth metals. Radium atoms have 88 electrons and 88 protons with 2 valence electrons in the outer shell. Under standard conditions radium is a silvery metal.
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Alkaline earth metals react with halogens and (except for beryllium) with water and oxygen. Magnesium, being less reactive, reacts only at higher temperatures than the other alkaline earth metals. ... Salts of beryllium are toxic, and water-soluble or acid-soluble salts of barium are toxic.
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The alkaline earth elements are metallic elements found in the second group of the periodic table.
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Because of this charge increase, the atoms of the alkaline earth metals are smaller and have higher first ionization energies than the alkali metals within the same period. The higher ionization energy makes the alkaline earth metals less reactive than the alkali metals; however, they are still very reactive elements.
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All alkaline Earth metals have similar properties because they all have two valence electrons. They readily give up their two valence electrons to achieve a full outer energy level, which is the most stable arrangement of electrons.
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Term. Alkaline earth metalsA group of chemical elements in the periodic table with similar properties: shiny, silvery-white, somewhat reactive at standard temperature and pressure. They readily lose their two outermost electrons to form cations with charge +2.
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Beryllium is a silvery-white, lustrous, relatively soft metal of group 2 of the periodic table. ... Beryllium has but a single isotope, beryllium-9 which is not radioactive but beryllium-10, which cosmic rays produce in the upper atmosphere, is radioactive with a half-life of 1.5 million years.
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All the alkaline earth metals have two electrons in their valence shell, so they lose two electrons to form cations with a 2+ charge. Most of the chemistry has been observed only for the first five members of the group; the chemistry of radium is not well established due to its radioactivity.