Difference between revisions of "Hydroxide Ion (Chemistry)"
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[[Metal Oxide]]s [[Chemical Reaction|react]] with [[water]] to form [[Metal Hydroxides]]. | [[Metal Oxide]]s [[Chemical Reaction|react]] with [[water]] to form [[Metal Hydroxides]]. | ||
: NaO(s) + H<sub>2</sub>O → Na<sup>+</sup>(aq)+OH<sup>-</sup>(aq) | : NaO(s) + H<sub>2</sub>O → Na<sup>+</sup>(aq)+OH<sup>-</sup>(aq) | ||
| − | : | + | : KO(aq) + H<sub>2</sub>O → K<sup>+</sup>(aq)+OH<sup>-</sup>(aq) |
| − | : Mg( | + | : Mg(O)<sub>2</sub>(aq) + 2H<sub>2</sub>O → Mg<sup>+2</sup>(aq)+2OH<sup>-</sup>(aq) |
| − | : Ca( | + | : Ca(O)<sub>2</sub>(aq) + 2H<sub>2</sub>O → Ca<sup>+2</sup>(aq)+2OH<sup>-</sup>(aq) |
| − | : Al( | + | : Al(O)<sub>3</sub>(aq) + 3H<sub>2</sub>O → Al<sup>+3</sup>(aq)+3OH<sup>-</sup>(aq) |
Revision as of 11:35, 6 January 2019
Key Stage 4
Meaning
A Hydroxide ion (OH-), is a positive ion of Hydrogen found in acid solutions.
About Hydroxide Ions
- When a basic compound dissolves in water it forms Hydroxide ions.
- Hydroxide ions are responsible for the corrosive properties of alkalis.
Examples
Metal Hydroxides form Hydroxide ions in water.
- NaOH(aq) → Na+(aq)+OH-(aq)
- KOH(aq) → K+(aq)+OH-(aq)
- Mg(OH)2(aq) → Mg+2(aq)+2OH-(aq)
- Ca(OH)2(aq) → Ca+2(aq)+2OH-(aq)
- Al(OH)3(aq) → Al+3(aq)+3OH-(aq)
Metal Oxides react with water to form Metal Hydroxides.
- NaO(s) + H2O → Na+(aq)+OH-(aq)
- KO(aq) + H2O → K+(aq)+OH-(aq)
- Mg(O)2(aq) + 2H2O → Mg+2(aq)+2OH-(aq)
- Ca(O)2(aq) + 2H2O → Ca+2(aq)+2OH-(aq)
- Al(O)3(aq) + 3H2O → Al+3(aq)+3OH-(aq)