Basic oxide

Basic oxides are oxides that show basic properties in opposition to acidic oxides and that either

  • react with water to form a base; or
  • react with an acid to form a salt and water which are called neutralization reactions.
Acids and bases
Diagrammatic representation of the dissociation of acetic acid in aqueous solution to acetate and hydronium ions.
Acid types
Base types

Etymology

"Basic oxides" is a compound of the words "Basic" and "oxides". The word oxides referred to the chemical compounds that one or more oxygen atoms combined with another element such as H2O or CO2. Based on their acid-base characteristics oxides can be classified into four categories: acidic oxides, basic oxides, and amphoteric oxides and neutral oxides.

Basic oxides, can also called base anhydrides which means "a base without water", are usually formed by reacting of oxygen with metals, especially alkali (+1 oxidation state) and alkaline earth metals (+2 oxidation state). Both of them are ionic oxide and can dissolve in water to form basic solutions of the metal hydroxide, whereas non-metals usually form acidic oxides. Basic oxide Li2O becomes base LiOH and BaO becomes Ba(OH)2 after react with water. In general, basicity of their oxides increases when the elements located downward at the left side of a periodic table (group 1 & 2), as the element become more metallic.[1]

Alkali Metals (Group 1)

X2O + H2O → 2XOH (X means group 1)

Alkaline Earth Metals (Group 2)

XO + H2O → X(OH)2 (X means group 2)

Examples include:

Formation

Examples of Oxides (Group 1 elements react with oxygen):

  • Lithium reacts with oxygen to give oxide. Li2O

4 Li(s) + O2(g) → 2 Li2O(s)

  • Sodium reacts with oxygen to give peroxide. Na2O2

2 Na(s) + O2(g) → Na2O2(s)

  • Potassium reacts with oxygen to form superoxide. KO2

K(s) + O2(g) → KO2(s)

Examples
  • Magnesium oxide
    Magnesium oxide
  • Calcium oxide
    Calcium oxide
  • Sodium hydroxide
    Sodium hydroxide

See also
Wikimedia Commons has media related to Basic oxides.

References
  1. Dr.Verma, Khanna, Dr.Kapila (2017). Comprehensive Chemistry XI. Laxmi Publications. p. 164.{{cite book}}: CS1 maint: multiple names: authors list (link)
  2. Atkins, P.; Overton, T.; Rourke, J.; Weller, M.; Armstrong, F. (2006). Inorganic Chemistry. Oxford University Press. pp. 263–278.{{cite book}}: CS1 maint: multiple names: authors list (link)
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