# Atomic spacing

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Distance between two nucleus

(Top) Diamond [crystal structure](/source/Crystal_structure), depicting an atomic spacing of 0.154 nm. (Bottom) Graphite crystal structure, depicting an atomic spacing of 0.142 nm.

**Atomic spacing** refers to the distance between the [nuclei](/source/Atomic_nucleus) of [atoms](/source/Atom) in a material. This space is extremely large compared to the [size](/source/Nuclear_size) of the [atomic nucleus](/source/Atomic_nucleus), and is related to the [chemical bonds](/source/Chemical_bond) which bind atoms together.[1] In solid materials, the atomic spacing is described by the [bond lengths](/source/Bond_length) of its atoms. In ordered solids, the atomic spacing between two bonded atoms is generally around a few [ångströms](/source/%C3%85ngstr%C3%B6m) (Å), which is on the order of 10−10 meters (see [Lattice constant](/source/Lattice_constant)). However, in very low density gases (for example, in [outer space](/source/Outer_space#Environment)) the average distance between atoms can be as large as a [meter](/source/Meter). In this case, the atomic spacing is not referring to bond length.

The atomic spacing of crystalline structures is usually determined by passing an [electromagnetic wave](/source/Electromagnetic_wave) of known [frequency](/source/Frequency) through the material, and using the laws of [diffraction](/source/Bragg_diffraction) to determine its atomic spacing. The atomic spacing of [amorphous materials](/source/Amorphous_solid) (such as [glass](/source/Glass)) varies substantially between different pairs of atoms, therefore diffraction cannot be used to accurately determine atomic spacing. In this case, the average bond length is a common way of expressing the distance between its atoms.[*[citation needed](https://en.wikipedia.org/wiki/Wikipedia:Citation_needed)*]

## Example

[Bond length](/source/Bond_length) can be determined between different elements in molecules by using the [atomic radii](/source/Atomic_radius) of the atoms. [Carbon](/source/Carbon) bonds with itself to form two covalent network solids.[2] [Diamond](/source/Diamond)'s C-C bond has a distance of 3 a 4 ≈ 0.154 nm {\displaystyle {\frac {{\sqrt {3}}a}{4}}\approx 0.154\ {\text{nm}}} away from each carbon since a diamond ≈ 0.357 nm {\displaystyle a_{\text{diamond}}\approx 0.357\ {\text{nm}}} , while [graphite](/source/Graphite)'s C-C bond has a distance of a 3 ≈ 0.142 nm {\displaystyle {\frac {a}{\sqrt {3}}}\approx 0.142\ {\text{nm}}} away from each carbon since a graphite ≈ 0.246 nm {\displaystyle a_{\text{graphite}}\approx 0.246\ {\text{nm}}} . Although both bonds are between the same pair of elements they can have different bond lengths.[3]

## References

1. **[^](#cite_ref-1)** Kittel, Charles (2004-11-11). *[Introduction to Solid State Physics](/source/Introduction_to_Solid_State_Physics)* (8th ed.). Wiley. [ISBN](/source/ISBN_(identifier)) [047141526X](https://en.wikipedia.org/wiki/Special:BookSources/047141526X).

1. **[^](#cite_ref-2)** Rossi, Miriam. ["How can graphite and diamond be so different if they are both composed of pure carbon?"](https://www.scientificamerican.com/article/how-can-graphite-and-diam/). *Scientific American*. Scientific American. Retrieved October 9, 2007.

1. **[^](#cite_ref-3)** Brown; Lemay; Bursten (1997). *Chemistry the Central Science*. Upper Saddle River, NJ: Simon and Schuster. pp. 412–413.

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