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Hydroxide Ion

Hydroxide Ion

The hydroxide ion (OH⁻) is a polyatomic ion. It is formed when oxygen covalently bonds with hydrogen and carries an extra negative charge. It plays an important role in acid–base chemistry, especially in aqueous solutions.

Let us understand the structure of the hydroxide ion. Read on to learn how it leads to its bonding and geometrical shape.

What is the Hydroxide ion?

When bases dissolve in water, they release hydroxide ions (OH⁻)

For example,

NaOH → Na⁺ + OH⁻

Hydroxide ion particularly acts as a strong nucleophile, and readily forms water (i.e., H₂O) by accepting H⁺ ions.

Breakdown of Hydroxide Ion

Here is a complete understanding of the hydroxide ion.

Electronic Configuration of Oxygen

The atomic number of oxygen is 8.

The ground state of oxygen :

1s² 2s² 2p⁴

OH⁻ ion → bonded to one hydrogen atom, along with which it also carries a negative charge

Formation of bonds in Hydroxide ion

In the hydroxide ion:

  • Oxygen forms a σ bond with hydrogen
  • Due to the negative charge on the ion -
  •      The ion becomes highly reactive
  •      Oxygen now has 3 lone pairs of electrons present on it

Result:

  • 1 O–H σ bonds
  • 3 Lone Pair on O
  • Overall charge: –1

Geometry of Hydroxide Ion

According to VSEPR theory, OH⁻ has 4 regions of electron density (1 bond + 3 lone pairs), giving it a tetrahedral electron geometry. However, since there is only one O–H bond, the actual molecular geometry is bent, with the O–H bond angle close to 104.5° (slightly affected by the negative charge).

Screenshot 2025-12-24 131703.png

 Lewis Structure of OH⁻

Details At A Glance

Property Details
Species Hydroxide (OH⁻)
Bonding 1 O–H σ bond, 3 lone pairs on O
Charge –1
Geometry (VSEPR Theory) Electron geometry: Tetrahedral (4 electron domains).
Molecular geometry: Bent (like water, but only one H atom).
Bond angle: ≈ 104.5° (slightly affected by extra negative charge).
Bond angle ~104.5° (affected a bit by negative charge)
Formal charge on O –1
Stability Stable due to a complete octet

Formal Charge in Hydroxide Ion

To determine if the Lewis structure of OH⁻ is stable, we calculate the formal charge on each atom using the formula:

Formal charge = Valence electrons – (Lone pair electrons + ½ × Bonding electrons)

Step-by-step for each atom:

Oxygen (O) :

  • Valence electrons: 6
  • Lone pairs: 3
  • Bonding electrons: 2 (from one single bond with H)

Formal charge = 6 – (6 + ½ × 2) = 6 – (6 + 1) = 6 – (7) = –1

Hydrogen (H):

  • Valence electrons: 1
  • Lone pairs: 0
  • Bonding electrons: 2 (1 single bond with oxygen)

Formal charge = 1 – (0 + ½ × 2) = 1 – 1 = 0

Thus, the overall charge is -1, which is the same as that of OH⁻, which confirms that the Lewis structure is stable and correct.

Summing Up

We have understood that, hydroxide ion (OH⁻) consists: 1 H and 1 O atom along with a -ve charge. It has one covalent bond along with 3 lone pairs. The ion is very important in acid-base chemistry, along with its applications in the field of biological sectors.

Frequently Asked Questions

Q1. Why is OH⁻ considered a base?

Since this ion readily accepts protons (H⁺) to form water (H₂O), it is considered a base.

Q2. What is the geometry of OH⁻?

The ion has tetrahedral electronic geometry due to 4 electron domains, but with only one bond, the molecular structure is bent around the O–H bond.

Q3. Is OH⁻ polar or non-polar?

Since there is a negative charge on oxygen and also there is a difference in electronegativity between O and H, OH⁻ is highly polar.

Q4. In which compounds is hydroxide found?

It is in bases such as NaOH, KOH, Ca(OH)₂, Mg(OH)₂, and many metal hydroxides.

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