Basic oxides are oxides that show basic properties in opposition to acidic oxides and that either
- reacts with water to form a base; or
- reacts with an acid to form a salt and water which called [neutralization reactions].
They are usually formed by reacting 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. In general, basicity increases down at the left side (group 1A & 2A) of a periodic table.[1]
Alkali Metals (Group 1A)
- X2O + H2O → 2XOH (X means group 1A)
Alkaline Earth Metals (Group 2A)
- XO + H2O → X(OH)2 (X means group 2A)
Examples include:
- Sodium oxide, which reacts with water to produce sodium hydroxide
- Magnesium oxide, which reacts with hydrochloric acid to form magnesium chloride
- Copper(II) oxide, which reacts with nitric acid to form copper nitrate
Properties of Oxide
editThe molecules that contain the group of H-O-X can behave normally as acids but when the hydroxide ion is produced they can behave as bases.[2] The O-X bond will remain intact and become polar and the weak O-H bond will tend to break, releasing a proton when the H-O-X grouping is dissolved in water. The O-X bond will become ionic and breakdown in polar water if X has very low electronegativity. For example, when NaOH and KOH which are ionic substances dissolve in water they will produce basic solutions of the metal hydroxide.[3] These principles can explain the base behavior when they are dissolved in water.
References
edit- ^ Dr.Verma, Khanna, Dr.Kapila (2017). Comprehensive Chemistry XI. Laxmi Publications. p. 164.
{{cite book}}: CS1 maint: multiple names: authors list (link) - ^ Zumdahl (2019). Chemistry 10e. Cengage Learning. p. 589.
- ^ Zumdahl, Steven S. "Oxide". Britannica.
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