Hydride ion Lewis Structure

Hydride ion Lewis Structure: H Lewis Structure, monatomic (no molecular geometry) Geometry, not applicable Hybridization & Polarity

Hydride ion Key Facts

The Hydride ion Lewis structure is isolated H atom with 2 electron(s) in the valence shell and no bonds; the central H has 0 electron domains (1 lone pair), giving a spherical electron-domain arrangement and a monatomic (no molecular geometry) molecular geometry with a — bond angle. H is best described as not applicable-hybridized, and Hydride ion is nonpolar because the bond dipoles cancel by molecular symmetry.

Figure 1: Lewis Structure of Hydride ion (H)

Chemical Formula	H
CAS Number	12184-80-6
Net Charge	-1
Total Valence Electrons	2
Lewis Structure	isolated H atom with 2 electron(s) in the valence shell and no bonds
Electron-Domain Geometry	spherical
Molecular Geometry	monatomic (no molecular geometry)
Hybridization Model	not applicable (central H)
Bond Angle	—
Polarity	Nonpolar molecule

PubChem and NIST list Hydride ion as H with CAS 12184-80-6; molecular weight ≈ None g/mol. View CAS 12184-80-6 dictionary details on Guidechem →

Applications of Hydride ion (CAS 12184-80-6)

In aqueous and process chemistry, H exists as the anion Hydride ion ion. It is encountered as a counterion and a controlled source of H in salts, buffers, electrochemistry and analytical protocols, and as a reactant in syntheses that require a defined equivalent of H-containing material.

Step 1 - Valence Electrons & Central Atom

To draw the Hydride ion Lewis structure we first count the total valence electrons. H contains 1 (H) − 1 (net anion); the net charge of -1 gives a total of 2 valence electrons to place.

The central atom is H. It is the least electronegative atom capable of forming multiple bonds and is surrounded by the more electronegative terminal atom(s); hydrogen, when present, always occupies a terminal position. Electronegativity considerations place the electron density toward the terminal atom(s).

Step 2 - Lewis Structure & Electron Distribution

Place H at the center and connect each surrounding atom with a single bond, complete octets on the terminal atoms, and place any remaining electrons on the central atom. The resulting electron distribution is: isolated H atom with 2 electron(s) in the valence shell and no bonds.

Counting bonding and nonbonding electrons around H therefore satisfies the octet/expanded-octet requirement for the drawn structure.

Step 3 - VSEPR Theory & Geometry

VSEPR theory states that the 0 electron domains around H arrange to minimize mutual repulsion, giving an spherical electron-domain geometry.

Because 1 of these domains are lone pair(s) — and lone pairs repel more strongly than bonding pairs — the observed molecular geometry is monatomic (no molecular geometry); the H bond angle is set to — rather than the ideal value for the electron-domain geometry.

Hybridization & Formal Charge

In the conventional localized-bond model, H uses not applicable hybrid orbitals to form the 0 equivalent electron-domain directions (0 bonding + 1 lone pair).

Is Hydride ion Polar or Nonpolar?

Hydride ion is nonpolar. Although individual H–terminal bonds are polar when the atoms differ in electronegativity, the monatomic (no molecular geometry) geometry makes their vector sum zero, so there is no net molecular dipole.

Its nonpolar character governs solvation and intermolecular behavior; specify grade and handling when sourcing.

Structural Comparison Table

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