Knowra Alkaline earth metal Alkaline earth metal An element in group 2 of the periodic table: beryllium, magnesium, calcium, strontium, barium, or radium. These metals typically form ions with a +2 charge.
Periodic table : A tabular arrangement of chemical elements ordered by atomic number and organized to show recurring properties. Group 2 is one vertical family within this map of elemental properties.
Ionization energy : The energy required to remove an electron from an atom or ion in the gas phase. Removing two outer electrons produces the characteristic group 2 cation.
Magnesium alloy : A metallic material whose principal constituent is magnesium, often alloyed to improve strength or corrosion resistance. Magnesium’s low density makes its alloys useful where reducing weight matters.
Alkali metal : An element in group 1 of the periodic table, excluding hydrogen, typically forming ions with a +1 charge. Group 1 metals lose one outer electron, unlike group 2 metals, which commonly lose two.
Periodic trend : A recurring change in elemental properties across periods or down groups of the periodic table. Trends in size and ionization energy explain differences among group 2 elements.
Alkaline earth metal hydroxide : A compound containing a group 2 metal cation and hydroxide ions, with general formula M(OH)₂. These products account for the alkaline solutions formed by several group 2 metals.
Portland cement : A hydraulic cement made by grinding clinker, chiefly calcium silicates, with a small amount of gypsum. Calcium compounds are the principal mineral ingredients of its clinker.
Transition metal : An element whose atom has an incomplete d subshell or that forms cations with an incomplete d subshell. Transition metals often show variable oxidation states, unlike the usual +2 state here.
Valence electron : An electron in an atom’s outermost shell that participates in chemical bonding. Group 2 atoms have two outer-shell electrons available for bonding.
Alkaline earth metal oxide : A binary compound of a group 2 metal and oxygen, typically with formula MO. Oxides form when group 2 metals react with oxygen and reflect their +2 charge.
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