View source for Van der Waals radius

{{DISPLAYTITLE:van der Waals radius}}
{{Short description|Size of an atom's imaginary sphere representing how close other atoms can get}}
{| class="wikitable floatright" align="right"
|+ van der Waals radii
|-
! Element !! radius ([[angstrom|Å]])
|-
| [[Hydrogen]] || 1.2 (1.09)<ref name="RowlandRS1996"/>
|-
| [[Carbon]] || 1.7
|-
| [[Nitrogen]] || 1.55
|-
| [[Oxygen]] || 1.52
|-
| [[Fluorine]] || 1.47
|-
| [[Phosphorus]] || 1.8
|-
| [[Sulfur]] || 1.8
|-
| [[Chlorine]] || 1.75
|-
| [[Copper]] || 1.4
|-
| colspan=2 | <small>van der Waals radii taken from<br/>Bondi's compilation (1964).<ref name="Bondi1964">{{cite journal | first = A. | last = Bondi | year =1964 | title = van der Waals Volumes and Radii | journal = [[Journal of Physical Chemistry|J. Phys. Chem.]] | volume = 68 | issue = 3 | pages = 441–451 | doi= 10.1021/j100785a001}}</ref><br/>Values from other sources may<br/>differ significantly (''see text'')</small>
|-
|}
{{Atomic radius}}

The '''van der Waals radius''', ''r''{{sub|w}}, of an [[atom]] is the [[radius]] of an imaginary hard [[sphere]] representing the [[distance of closest approach]] for another atom. 
It is named after [[Johannes Diderik van der Waals]], winner of the 1910 [[Nobel Prize in Physics]], as he was the first to recognise that atoms were not simply [[Point (geometry)|points]] and to demonstrate the physical consequences of their size through the [[van der Waals equation|van der Waals equation of state]].

== van der Waals volume ==
{{unreferenced section|date=June 2015}}
The '''van der Waals volume''', ''V{{sub|w}}'', also called the '''atomic volume''' or '''molecular volume''', is the atomic property most directly related to the van der Waals radius.<ref>{{Cite web |title=Van der Waals Radii of Elements |url=https://physlab.org/wp-content/uploads/2016/03/Franck_ref2.pdf}}</ref> It is the volume "occupied" by an individual atom (or molecule). The van der Waals volume may be calculated if the van der Waals radii (and, for molecules, the inter-atomic distances, and angles) are known. For a single atom, it is the volume of a sphere whose radius is the van der Waals radius of the atom:<math display="block">V_{\rm w} = {4\over 3}\pi r_{\rm w}^3.</math>

For a molecule, it is the volume enclosed by the [[van der Waals surface]]. 
The van der Waals volume of a molecule is always smaller than the sum of the van der Waals volumes of the constituent atoms: the atoms can be said to "overlap" when they form [[chemical bond]]s.

The van der Waals volume of an atom or molecule may also be determined by experimental measurements on gases, notably from the [[van der Waals constant]] ''b'', the [[polarizability]] ''α'', or the [[molar refractivity]] ''A''. 
In all three cases, measurements are made on macroscopic samples and it is normal to express the results as [[mole (unit)|molar]] quantities. 
To find the van der Waals volume of a single atom or molecule, it is necessary to divide by the [[Avogadro constant]] ''N''{{sub|A}}.

The molar van der Waals volume should not be confused with the [[molar volume]] of the substance. 
In general, at normal laboratory temperatures and pressures, the atoms or molecules of gas only occupy about {{frac|{{val|1000}}}} of the volume of the gas, the rest is empty space. 
Hence the molar van der Waals volume, which only counts the volume occupied by the atoms or molecules, is usually about {{val|1000}} times smaller than the molar volume for a gas at [[standard temperature and pressure]].

==Table of van der Waals radii==
{| class="mw-collapsible {{#if:{{{state|collapsed}}}|collapsed|mw-collapsed}}" border="0" cellpadding="0" cellspacing="1" style="text-align:center; background:{{Element color|table background}}; border:1px solid {{Element color|table border}}; width:100%; max-width:1300px; margin:0 auto; padding:2px;"
! colspan=20 style="background:{{Element color|table title}}; padding:2px 4px;" | [[Van der Waals radius]] of the elements in the [[periodic table]]<!-- 

If r is the radius, then the colors follow the formula 
|7= 0xff0000 + (r-110) * 0x100 

Example: r = 140 for helium so: 
|7= 0xff0000 + (140-110) * 0x100
|7= 0xff0000 + 0x1e * 0x100 (since 30 = 0x1e)
|7= 0xff0000 + 0x1e00
|7= 0xff1e00
-->
|- style="background:{{Element color|table colheader}}"
! width="1.0%" | <small>[[Periodic table group|Group]]&nbsp;→</small>
! width="5.4%" | [[Alkali metal|1]]
! width="5.4%" | [[Alkaline earth metal|2]]
! width="1.8%" | 
! width="5.4%" | [[Group 3 element|3]]
! width="5.4%" | [[Group 4 element|4]]
! width="5.4%" | [[Group 5 element|5]]
! width="5.4%" | [[Group 6 element|6]]
! width="5.4%" | [[Group 7 element|7]]
! width="5.4%" | [[Group 8 element|8]]
! width="5.4%" | [[Group 9 element|9]]
! width="5.4%" | [[Group 10 element|10]]
! width="5.4%" | [[Group 11 element|11]]
! width="5.4%" | [[Group 12 element|12]]
! width="5.4%" | [[Boron group|13]]
! width="5.4%" | [[Carbon group|14]]
! width="5.4%" | [[Pnictogen|15]]
! width="5.4%" | [[Chalcogen|16]]
! width="5.4%" | [[Halogen|17]]
! width="5.4%" | [[Noble gas|18]]
|-
! <small>↓&nbsp;[[Periodic table period|Period]]</small>
| colspan="20"|<br />
|-
! [[Period 1 element|1]]
| {{element cell property|H |hydrogen  |110<ref name="RowlandRS1996">{{cite journal|title=Intermolecular nonbonded contact distances in organic crystal structures: comparison with distances expected from van der Waals radii|author=Rowland RS, Taylor R|journal=J. Phys. Chem.|year=1996|volume=100|issue=18|pages=7384–7391|doi=10.1021/jp953141+}}</ref><br/>or 120|s-block|Primordial|7=#ff0a00}}
| colspan="17"|<br />
| {{element cell property|He|helium    |140|s-block|Primordial|7=#ff1e00}}
|-
! [[Period 2 element|2]]
| {{element cell property|Li|lithium   |182|s-block|Primordial|7=#ff4800}}
| {{element cell property|Be|beryllium |153<ref name="Mantina">{{cite journal|last1=Mantina|first1=Manjeera|last2=Chamberlin|first2=Adam C.|last3=Valero|first3=Rosendo|last4=Cramer|first4=Christopher J.|last5=Truhlar|first5=Donald G.|year=2009|title=Consistent van der Waals Radii for the Whole Main Group.|journal=[[The Journal of Physical Chemistry A]]|volume=113|issue=19|pages=5806–5812|pmc=3658832|doi=10.1021/jp8111556|doi-access=free|pmid=19382751 |bibcode=2009JPCA..113.5806M }}</ref>|s-block|Primordial|7=#ff2b00}}
| colspan="11"|<br />
| {{element cell property|B |boron     |192<ref name="Mantina"/>|p-block|Primordial|7=#ff5200}}
| {{element cell property|C |carbon    |170|p-block|Primordial|7=#ff3c00}}
| {{element cell property|N |nitrogen  |155|p-block|Primordial|7=#ff2d00}}
| {{element cell property|O |oxygen    |152|p-block|Primordial|7=#ff2a00}}
| {{element cell property|F |fluorine  |147|p-block|Primordial|7=#ff2500}}
| {{element cell property|Ne|neon      |154|p-block|Primordial|7=#ff2c00}}
|-
! [[Period 3 element|3]]
| {{element cell property|Na|sodium    |227|s-block|Primordial|7=#ff7500}}
| {{element cell property|Mg|magnesium |173|s-block|Primordial|7=#ff3f00}}
| colspan="11"|<br />
| {{element cell property|Al|aluminium |184<ref name="Mantina"/>|p-block|Primordial|7=#ff4a00}}
| {{element cell property|Si|silicon   |210|p-block|Primordial|7=#ff6400}}
| {{element cell property|P |phosphorus|180|p-block|Primordial|7=#ff4600}}
| {{element cell property|S |sulfur    |180|p-block|Primordial|7=#ff4600}}
| {{element cell property|Cl|chlorine  |175|p-block|Primordial|7=#ff4100}}
| {{element cell property|Ar|argon     |188|p-block|Primordial|7=#ff4e00}}
|-
! [[Period 4 element|4]]
| {{element cell property|K |potassium |275|s-block|Primordial|7=#ffa500}}
| {{element cell property|Ca|calcium   |231<ref name="Mantina"/>|s-block|Primordial|7=#ff7900}}
|
| {{element cell property|Sc|scandium  |211<ref name="Mantina"/>|d-block|Primordial|7=#ff6400}}
| {{element cell property|Ti|titanium  |&nbsp;|d-block|Primordial|7=#bbbbbb}}
| {{element cell property|V |vanadium  |&nbsp;|d-block|Primordial|7=#bbbbbb}}
| {{element cell property|Cr|chromium  |&nbsp;|d-block|Primordial|7=#bbbbbb}}
| {{element cell property|Mn|manganese |&nbsp;|d-block|Primordial|7=#bbbbbb}}
| {{element cell property|Fe|iron      |&nbsp;|d-block|Primordial|7=#bbbbbb}}
| {{element cell property|Co|cobalt    |&nbsp;|d-block|Primordial|7=#bbbbbb}}
| {{element cell property|Ni|nickel    |163|d-block|Primordial|7=#ff3500}}
| {{element cell property|Cu|copper    |140|d-block|Primordial|7=#ff1e00}}
| {{element cell property|Zn|zinc      |139|d-block|Primordial|7=#ff1d00}}
| {{element cell property|Ga|gallium   |187|p-block|Primordial|7=#ff4d00}}
| {{element cell property|Ge|germanium |211<ref name="Mantina"/>|p-block|Primordial|7=#ff6500}}
| {{element cell property|As|arsenic   |185|p-block|Primordial|7=#ff4b00}}
| {{element cell property|Se|selenium  |190|p-block|Primordial|7=#ff5000}}
| {{element cell property|Br|bromine   |185|p-block|Primordial|7=#ff4b00}}
| {{element cell property|Kr|krypton   |202|p-block|Primordial|7=#ff5c00}}
|-
! [[Period 5 element|5]]
| {{element cell property|Rb|rubidium  |303<ref name="Mantina"/>|s-block|Primordial|7=#ffc100}}
| {{element cell property|Sr|strontium |249<ref name="Mantina"/>|s-block|Primordial|7=#ff8b00}}
|
| {{element cell property|Y |yttrium   |&nbsp;|d-block|Primordial|7=#bbbbbb}}
| {{element cell property|Zr|zirconium |&nbsp;|d-block|Primordial|7=#bbbbbb}}
| {{element cell property|Nb|niobium   |&nbsp;|d-block|Primordial|7=#bbbbbb}}
| {{element cell property|Mo|molybdenum|&nbsp;|d-block|Primordial|7=#bbbbbb}}
| {{element cell property|Tc|technetium|&nbsp;|d-block|from decay|7=#bbbbbb}}
| {{element cell property|Ru|ruthenium |&nbsp;|d-block|Primordial|7=#bbbbbb}}
| {{element cell property|Rh|rhodium   |&nbsp;|d-block|Primordial|7=#bbbbbb}}
| {{element cell property|Pd|palladium |163|d-block|Primordial|7=#ff3500}}
| {{element cell property|Ag|silver    |172|d-block|Primordial|7=#ff3e00}}
| {{element cell property|Cd|cadmium   |158|d-block|Primordial|7=#ff3000}}
| {{element cell property|In|indium    |193|p-block|Primordial|7=#ff5300}}
| {{element cell property|Sn|tin       |217|p-block|Primordial|7=#ff6b00}}
| {{element cell property|Sb|antimony  |206<ref name="Mantina"/>|p-block|Primordial|7=#ff6000}}
| {{element cell property|Te|tellurium |206|p-block|Primordial|7=#ff6000}}
| {{element cell property|I |iodine    |198|p-block|Primordial|7=#ff5800}}
| {{element cell property|Xe|xenon     |216|p-block|Primordial|7=#ff6a00}}
|-
! [[Period 6 element|6]]
| {{element cell property|Cs|caesium   |343<ref name="Mantina"/>|s-block|Primordial|7=#ffe900}}
| {{element cell property|Ba|barium    |268<ref name="Mantina"/>|s-block|Primordial|7=#ff9e00}}
| {{element cell-asterisk|1}}
| {{element cell property|Lu|lutetium  |&nbsp;|d-block|Primordial|7=#bbbbbb}}
| {{element cell property|Hf|hafnium   |&nbsp;|d-block|Primordial|7=#bbbbbb}}
| {{element cell property|Ta|tantalum  |&nbsp;|d-block|Primordial|7=#bbbbbb}}
| {{element cell property|W |tungsten  |&nbsp;|d-block|Primordial|7=#bbbbbb}}
| {{element cell property|Re|rhenium   |&nbsp;|d-block|Primordial|7=#bbbbbb}}
| {{element cell property|Os|osmium    |&nbsp;|d-block|Primordial|7=#bbbbbb}}
| {{element cell property|Ir|iridium   |&nbsp;|d-block|Primordial|7=#bbbbbb}}
| {{element cell property|Pt|platinum  |175|d-block|Primordial|7=#ff4100}}
| {{element cell property|Au|gold      |166|d-block|Primordial|7=#ff3800}}
| {{element cell property|Hg|mercury   |155|d-block|Primordial|mercury (element)|7=#ff2d00}}
| {{element cell property|Tl|thallium  |196|p-block|Primordial|7=#ff5600}}
| {{element cell property|Pb|lead      |202|p-block|Primordial|7=#ff5c00}}
| {{element cell property|Bi|bismuth   |207<ref name="Mantina"/>|p-block|Primordial|7=#ff6100}}
| {{element cell property|Po|polonium  |197<ref name="Mantina"/>|p-block|from decay|7=#ff5700}}
| {{element cell property|At|astatine  |202<ref name="Mantina"/>|p-block|from decay|7=#ff5c00}}
| {{element cell property|Rn|radon     |220<ref name="Mantina"/>|p-block|from decay|7=#ff6e00}}
|-
! [[Period 7 element|7]]
| {{element cell property|Fr|francium     |348<ref name="Mantina"/>|s-block|from decay|7=#ffee00}}
| {{element cell property|Ra|radium       |283<ref name="Mantina"/>|s-block|from decay|7=#ffad00}}
| {{element cell-asterisk|2vert}}
| {{element cell property|Lr|lawrencium   |&nbsp;|d-block|Synthetic|7=#bbbbbb}}
| {{element cell property|Rf|rutherfordium|&nbsp;|d-block|Synthetic|7=#bbbbbb}}
| {{element cell property|Db|dubnium      |&nbsp;|d-block|Synthetic|7=#bbbbbb}}
| {{element cell property|Sg|seaborgium   |&nbsp;|d-block|Synthetic|7=#bbbbbb}}
| {{element cell property|Bh|bohrium      |&nbsp;|d-block|Synthetic|7=#bbbbbb}}
| {{element cell property|Hs|hassium      |&nbsp;|d-block|Synthetic|7=#bbbbbb}}
| {{element cell property|Mt|meitnerium   |&nbsp;|d-block|Synthetic|7=#bbbbbb}}
| {{element cell property|Ds|darmstadtium |&nbsp;|d-block|Synthetic|7=#bbbbbb}}
| {{element cell property|Rg|roentgenium  |&nbsp;|d-block|Synthetic|7=#bbbbbb}}
| {{element cell property|Cn|copernicium  |&nbsp;|d-block|Synthetic|7=#bbbbbb}}
| {{element cell property|Nh|nihonium     |&nbsp;|p-block|Synthetic|7=#bbbbbb}}
| {{element cell property|Fl|flerovium    |&nbsp;|p-block|Synthetic|7=#bbbbbb}}
| {{element cell property|Mc|moscovium    |&nbsp;|p-block|Synthetic|7=#bbbbbb}}
| {{element cell property|Lv|livermorium  |&nbsp;|p-block|Synthetic|7=#bbbbbb}}
| {{element cell property|Ts|tennessine   |&nbsp;|p-block|Synthetic|7=#bbbbbb}}
| {{element cell property|Og|oganesson    |&nbsp;|p-block|Synthetic|7=#bbbbbb}}
|-
| colspan="22"|<br />
|-
| colspan="4" {{element cell-asterisk|1|align=right}}
| {{element cell property|La|lanthanum   |&nbsp;|f-block|Primordial|7=#bbbbbb}}
| {{element cell property|Ce|cerium      |&nbsp;|f-block|Primordial|7=#bbbbbb}}
| {{element cell property|Pr|praseodymium|&nbsp;|f-block|Primordial|7=#bbbbbb}}
| {{element cell property|Nd|neodymium   |&nbsp;|f-block|Primordial|7=#bbbbbb}}
| {{element cell property|Pm|promethium  |&nbsp;|f-block|from decay|7=#bbbbbb}}
| {{element cell property|Sm|samarium    |&nbsp;|f-block|Primordial|7=#bbbbbb}}
| {{element cell property|Eu|europium    |&nbsp;|f-block|Primordial|7=#bbbbbb}}
| {{element cell property|Gd|gadolinium  |&nbsp;|f-block|Primordial|7=#bbbbbb}}
| {{element cell property|Tb|terbium     |&nbsp;|f-block|Primordial|7=#bbbbbb}}
| {{element cell property|Dy|dysprosium  |&nbsp;|f-block|Primordial|7=#bbbbbb}}
| {{element cell property|Ho|holmium     |&nbsp;|f-block|Primordial|7=#bbbbbb}}
| {{element cell property|Er|erbium      |&nbsp;|f-block|Primordial|7=#bbbbbb}}
| {{element cell property|Tm|thulium     |&nbsp;|f-block|Primordial|7=#bbbbbb}}
| {{element cell property|Yb|ytterbium   |&nbsp;|f-block|Primordial|7=#bbbbbb}}
|-
| colspan="4" {{element cell-asterisk|2vert|align=right}}
| {{element cell property|Ac|actinium    |&nbsp;|f-block|from decay|7=#bbbbbb}}
| {{element cell property|Th|thorium     |&nbsp;|f-block|Primordial|7=#bbbbbb}}
| {{element cell property|Pa|protactinium|&nbsp;|f-block|from decay|7=#bbbbbb}}
| {{element cell property|U |uranium     |186|f-block|Primordial|7=#ff4c00}}
| {{element cell property|Np|neptunium   |&nbsp;|f-block|from decay|7=#bbbbbb}}
| {{element cell property|Pu|plutonium   |&nbsp;|f-block|from decay|7=#bbbbbb}}
| {{element cell property|Am|americium   |&nbsp;|f-block|Synthetic|7=#bbbbbb}}
| {{element cell property|Cm|curium      |&nbsp;|f-block|Synthetic|7=#bbbbbb}}
| {{element cell property|Bk|berkelium   |&nbsp;|f-block|Synthetic|7=#bbbbbb}}
| {{element cell property|Cf|californium |&nbsp;|f-block|Synthetic|7=#bbbbbb}}
| {{element cell property|Es|einsteinium |&nbsp;|f-block|Synthetic|7=#bbbbbb}}
| {{element cell property|Fm|fermium     |&nbsp;|f-block|Synthetic|7=#bbbbbb}}
| {{element cell property|Md|mendelevium |&nbsp;|f-block|Synthetic|7=#bbbbbb}}
| {{element cell property|No|nobelium    |&nbsp;|f-block|Synthetic|7=#bbbbbb}}
|-
| colspan=19 style="text-align:left;" |'''Legend'''
|-
| colspan=19 style="text-align:left;" |Values for the van der Waals radii are in [[picometers]] (pm or {{val|1|e=-12|u=m}})
|-
| colspan=19 style="text-align:left;" |The shade of the box ranges from red to yellow as the radius increases; Gray indicate a lack of data.<!-- |7=#bbbbbb  sets the background color to gray-->
|-
| colspan=19 style="text-align:left;" |Unless indicated otherwise, the data is from ''[[Mathematica]]'''s [https://reference.wolfram.com/language/ref/ElementData.html ElementData] function from [[Wolfram Research|Wolfram Research, Inc.]]<ref name="slater64">{{cite web|title=van der Waals Radius of the elements|url=http://periodictable.com/Properties/A/VanDerWaalsRadius.an.html|work=Wolfram}}</ref>
|-
| colspan=19 | 
{{periodic table legend
|theme1=Occurrence
|unknown2=yes}}
|}

== Methods of determination ==
{{refimprove science|date=June 2015}}
Van der Waals radii may be determined from the [[mechanics|mechanical]] properties of gases (the original method), from the [[critical point (thermodynamics)|critical point]], from measurements of atomic spacing between pairs of unbonded atoms in [[crystal]]s or from measurements of electrical or optical properties (the [[polarizability]] and the [[molar refractivity]]). 
These various methods give values for the van der Waals radius which are similar (1–2&nbsp;[[angstrom|Å]], 100–200&nbsp;[[picometre|pm]]) but not identical. 
Tabulated values of van der Waals radii are obtained by taking a [[weighted mean]] of a number of different experimental values, and, for this reason, different tables will often have different values for the van der Waals radius of the same atom. 
Indeed, there is no reason to assume that the van der Waals radius is a fixed property of the atom in all circumstances: rather, it tends to vary with the particular chemical environment of the atom in any given case.<ref name="Bondi1964"/>

=== Van der Waals equation of state ===
{{main|Van der Waals equation}}

The van der Waals equation of state is the simplest and best-known modification of the [[ideal gas law]] to account for the behaviour of [[real gas]]es:
<math display="block">\left (p + a\left (\frac{n}{\tilde{V}}\right )^2\right ) (\tilde{V} - nb) = nRT,</math>
where {{mvar|p}} is pressure, {{mvar|n}} is the number of moles of the gas in question and {{mvar|a}} and {{mvar|b}} depend on the particular gas, <math>\tilde{V}</math> is the volume, {{mvar|R}} is the specific gas constant on a unit mole basis and {{mvar|T}} the absolute temperature; {{mvar|a}} is a correction for intermolecular forces and {{mvar|b}} corrects for finite atomic or molecular sizes; the value of {{mvar|b}} equals the van der Waals volume per mole of the gas. 
[[van der Waals constants (data page)|Their values]] vary from gas to gas.

The van der Waals equation also has a microscopic interpretation: molecules interact with one another. 
The interaction is strongly repulsive at a very short distance, becomes mildly attractive at the intermediate range, and vanishes at a long distance. 
The ideal gas law must be corrected when attractive and repulsive forces are considered. 
For example, the mutual repulsion between molecules has the effect of excluding neighbors from a certain amount of space around each molecule. 
Thus, a fraction of the total space becomes unavailable to each molecule as it executes random motion. 
In the equation of state, this volume of exclusion ({{math|''nb''}}) should be subtracted from the volume of the container ({{mvar|V}}), thus: ({{math|''V'' - ''nb''}}). 
The other term that is introduced in the van der Waals equation, <math display="inline">a\left (\frac{n}{\tilde{V}}\right )^2</math>, describes a weak attractive force among molecules (known as the [[van der Waals force]]), which increases when {{mvar|n}} increases or {{mvar|V}} decreases and molecules become more crowded together.

{| class="wikitable floatright" align=right
|-
! Gas
! ''d'' ([[Ångström|Å]])
! ''b'' (cm{{sup|3}}mol{{sup|–1}})
! ''V''{{sub|w}} (Å{{sup|3}})
! ''r''{{sub|w}} (Å)
|-
| [[Hydrogen]]
| 0.74611
| align=center | 26.61
| 34.53
| 2.02
|-
| [[Nitrogen]]
| 1.0975
| align=center | 39.13
| 47.71
| 2.25
|-
| [[Oxygen]]
| 1.208
| align=center | 31.83
| 36.62
| 2.06
|-
| [[Chlorine]]
| 1.988
| align=center | 56.22
| 57.19
| 2.39
|-
| colspan=5 | <small>van der Waals radii ''r''{{sub|w}} in Å (or in 100 picometers) calculated from the [[van der Waals constant]]s<br/>of some diatomic gases. Values of ''d'' and ''b'' from Weast (1981).</small>
|}

The [[van der Waals constant]] ''b'' volume can be used to calculate the van der Waals volume of an atom or molecule with experimental data derived from measurements on gases.

For [[helium]],<ref name="CRC">{{RubberBible62nd}}, p. D-166.</ref> ''b''&nbsp;= 23.7&nbsp;cm{{sup|3}}/mol. Helium is a [[monatomic gas]], and each mole of helium contains {{val|6.022|e=23}} atoms (the [[Avogadro constant]], ''N''{{sub|A}}):
<math display="block">V_{\rm w} = {b\over{N_{\rm A}}}</math>
Therefore, the van der Waals volume of a single atom ''V''{{sub|w}}&nbsp;= 39.36&nbsp;Å{{sup|3}}, which corresponds to ''r''{{sub|w}}&nbsp;= 2.11&nbsp;Å (≈ 200 picometers). 
This method may be extended to diatomic gases by approximating the molecule as a rod with rounded ends where the diameter is {{math|2''r''{{sub|w}}}} and the internuclear distance is {{mvar|d}}. 
The algebra is more complicated, but the relation
<math display="block">V_{\rm w} = {4\over 3}\pi r_{\rm w}^3 + \pi r_{\rm w}^2d</math>
can be solved by the normal methods for [[cubic functions]].

=== Crystallographic measurements ===

The molecules in a [[molecular crystal]] are held together by [[van der Waals force]]s rather than [[chemical bond]]s. 
In principle, the closest that two atoms belonging to ''different'' molecules can approach one another is given by the sum of their van der Waals radii. 
By examining a large number of structures of molecular crystals, it is possible to find a minimum radius for each type of atom such that other non-bonded atoms do not encroach any closer. 
This approach was first used by [[Linus Pauling]] in his seminal work ''The Nature of the Chemical Bond''.<ref name="Pauling1945">{{cite book | first = Linus | last = Pauling | author-link = Linus Pauling | year = 1945 | title = The Nature of the Chemical Bond | location = Ithaca, NY | publisher = Cornell University Press | isbn = 978-0-8014-0333-0| title-link = The Nature of the Chemical Bond }}</ref> 
Arnold Bondi also conducted a study of this type, published in 1964,<ref name="Bondi1964"/> although he also considered other methods of determining the van der Waals radius in coming to his final estimates. 
Some of Bondi's figures are given in the table at the top of this article, and they remain the most widely used "consensus" values for the van der Waals radii of the elements. 
Scott Rowland and Robin Taylor re-examined these 1964 figures in the light of more recent crystallographic data: on the whole, the agreement was very good, although they recommend a value of 1.09&nbsp;Å for the van der Waals radius of [[hydrogen]] as opposed to Bondi's 1.20&nbsp;Å.<ref name="RowlandRS1996"/> A more recent analysis of the [[Cambridge Structural Database]], carried out by Santiago Alvareza, provided a new set of values for 93 naturally occurring elements.<ref name="Alvarez2013">{{cite journal | first = Santiago | last = Alvareza  | year =2013 | title = A cartography of the van der Waals territories | journal = [[Dalton Trans.]] | volume = 42 | issue = 24  | pages = 8617–36 | doi= 10.1039/C3DT50599E| pmid = 23632803  | doi-access = free | hdl = 2445/48823 | hdl-access = free }}</ref>

A simple example of the use of crystallographic data (here [[neutron diffraction]]) is to consider the case of solid helium, where the atoms are held together only by van der Waals forces (rather than by [[Covalent bond|covalent]] or [[metallic bond]]s) and so the distance between the nuclei can be considered to be equal to twice the van der Waals radius. 
The density of solid helium at 1.1&nbsp;K and 66&nbsp;[[Atmosphere (unit)|atm]] is {{val|0.214|(6)|u=g/cm3}},<ref name="Henshaw1958">{{cite journal | first = D.G. | last = Henshaw | year = 1958 | title = Structure of Solid Helium by Neutron Diffraction | journal = [[Physical Review]] | volume = 109 | issue = 2 | pages = 328–330 | doi = 10.1103/PhysRev.109.328|bibcode = 1958PhRv..109..328H }}</ref> corresponding to a [[molar volume]] ''V''{{sub|m}}&nbsp;= {{val|18.7|e=-6|u=m3/mol}}. 
The van der Waals volume is given by
<math display="block">V_{\rm w} = \frac{\pi V_{\rm m}}{N_{\rm A}\sqrt{18}}</math>
where the factor of π/√18 arises from the [[Sphere packing|packing of spheres]]: ''V''{{sub|w}}&nbsp;= {{val|2.30|e=-29|u=m3}}&nbsp;= 23.0&nbsp;Å{{sup|3}}, corresponding to a van der Waals radius ''r''{{sub|w}}&nbsp;= 1.76&nbsp;Å.

=== Molar refractivity ===

The [[molar refractivity]] {{mvar|A}} of a gas is related to its [[refractive index]] {{mvar|n}} by the [[Lorentz–Lorenz equation]]:
<math display="block">A = \frac{R T (n^2 - 1)}{3p}</math>
The refractive index of helium ''n''&nbsp;= {{val|1.0000350}} at 0&nbsp;°C and 101.325&nbsp;kPa,<ref>Kaye & Laby Tables, [http://www.kayelaby.npl.co.uk/general_physics/2_5/2_5_7.html Refractive index of gases].</ref> which corresponds to a molar refractivity ''A''&nbsp;= {{val|5.23|e=-7|u=m3/mol}}. 
Dividing by the Avogadro constant gives ''V''{{sub|w}}&nbsp;= {{val|8.685|e=-31|u=m3}}&nbsp;= 0.8685&nbsp;Å{{sup|3}}, corresponding to ''r''{{sub|w}}&nbsp;= 0.59&nbsp;Å.

=== Polarizability ===

The [[polarizability]] ''α'' of a gas is related to its [[electric susceptibility]] ''χ''{{sub|e}} by the relation
<math display="block">\alpha = {\varepsilon_0 k_{\rm B}T\over p}\chi_{\rm e}</math>
and the electric susceptibility may be calculated from tabulated values of the [[Permittivity|relative permittivity]] ''ε''{{sub|r}} using the relation ''χ''{{sub|e}}&nbsp;= ''ε''{{sub|r}}&nbsp;−&nbsp;1. 
The electric susceptibility of helium ''χ''{{sub|e}}&nbsp;= {{val|7|e=-5}} at 0&nbsp;°C and 101.325&nbsp;kPa,<ref>Kaye & Laby Tables, [http://www.kayelaby.npl.co.uk/general_physics/2_6/2_6_5.html Dielectric Properties of Materials].</ref> which corresponds to a polarizability ''α''&nbsp;= {{val|2.307|e=-41|u=C⋅m<sup>2</sup>/V}}. 
The polarizability is related the van der Waals volume by the relation
<math display="block">V_{\rm w} = {1\over{4\pi\varepsilon_0}}\alpha ,</math>
so the van der Waals volume of helium ''V''{{sub|w}}&nbsp;= {{val|2.073|e=-31|u=m3}}&nbsp;= 0.2073&nbsp;Å{{sup|3}} by this method, corresponding to ''r''{{sub|w}}&nbsp;= 0.37&nbsp;Å.

When the atomic polarizability is quoted in units of volume such as Å{{sup|3}}, as is often the case, it is equal to the van der Waals volume. 
However, the term "atomic polarizability" is preferred as polarizability is a precisely defined (and measurable) [[physical quantity]], whereas "van der Waals volume" can have any number of definitions depending on the method of measurement.

== See also ==

* [[Atomic radii of the elements (data page)]]
* [[van der Waals force]]
* [[van der Waals molecule]]
* [[van der Waals strain]]
* [[van der Waals surface]]

== References ==
{{reflist|30em}}

==Further reading==

* {{cite book | first1 = James E. | last1 = Huheey | last2 = Keiter | first2 = Ellen A. | last3 = Keiter | first3 = Richard L. | year = 1997 | title = Inorganic Chemistry: Principles of Structure and Reactivity | edition = 4th | location = New York | publisher = Prentice Hall | isbn = 978-0-06-042995-9 | url-access = registration | url = https://archive.org/details/inorganicchemist00huhe_0 }}

== External links ==

* [http://periodictable.com/Properties/A/VanDerWaalsRadius.v.html van der Waals Radius of the elements] at PeriodicTable.com
* [http://www.webelements.com/periodicity/van_der_waals_radius/ van der Waals Radius – Periodicity] at WebElements.com

[[Category:Chemical properties]]
[[Category:Intermolecular forces]]
[[Category:Johannes Diderik van der Waals|Radius]]
[[Category:Atomic radius]]