Atomic radius (empirical)

These values derived by J.C. Slater are an empirical set of atomic radii derived by the careful comparison of bond lengths in over 1200 bond types in ionic, metallic, and covalent crystals and molecules (reference 1).

The idea is that for a bond A-B, the atomic radius of A added to the atomic radius of B will give a reasonable estimate for the A-B separation in whatever environment. A single set of radii is very useful for most purposes, however, for very accurate work adjustments would have to be made to the values quoted to reflect the specific environment of the element (such as coordination number). Values are given to an accuracy of about 5 pm.

Image showing periodicity of the chemical elements for atomic radius (empirical) in a periodic table cityscape style.
Image showing periodicity of the chemical elements for atomic radius (empirical) in a periodic table cityscape style.
Image showing periodicity of the chemical elements for atomic radius (empirical) in a periodic table heatscape style.
Image showing periodicity of the chemical elements for atomic radius (empirical) in a periodic table heatscape style.
Image showing periodicity of the chemical elements for atomic radius (empirical) in a spiral periodic table heatscape style.
Image showing periodicity of the chemical elements for atomic radius (empirical) in a spiral periodic table heatscape style.
Image showing periodicity of the chemical elements for atomic radius (empirical) in a 3D spiral periodic table column style.
Image showing periodicity of the chemical elements for atomic radius (empirical) in a 3D spiral periodic table column style.
Image showing periodicity of the chemical elements for atomic radius (empirical) in a 3D periodic table column style.
Image showing periodicity of the chemical elements for atomic radius (empirical) in a 3D periodic table column style.

Units

pm

Notes

None

Select from the following links to see visual periodicity representations for atomic radii, covalent radii, and van der Waals radii. Ionic radii are also available.

Literature sources

  1. J.C. Slater, J. Chem. Phys. 1964, 39, 3199.
Explore the element of your choice through this periodic table.
1 2   3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18
1
H
2
He
3
Li
4
Be
5
B
6
C
7
N
8
O
9
F
10
Ne
11
Na
12
Mg
13
Al
14
Si
15
P
16
S
17
Cl
18
Ar
19
K
20
Ca
21
Sc
22
Ti
23
V
24
Cr
25
Mn
26
Fe
27
Co
28
Ni
29
Cu
30
Zn
31
Ga
32
Ge
33
As
34
Se
35
Br
36
Kr
37
Rb
38
Sr
39
Y
40
Zr
41
Nb
42
Mo
43
Tc
44
Ru
45
Rh
46
Pd
47
Ag
48
Cd
49
In
50
Sn
51
Sb
52
Te
53
I
54
Xe
55
Cs
56
Ba
 *
71
Lu
72
Hf
73
Ta
74
W
75
Re
76
Os
77
Ir
78
Pt
79
Au
80
Hg
81
Tl
82
Pb
83
Bi
84
Po
85
At
86
Rn
87
Fr
88
Ra
 **
103
Lr
104
Rf
105
Db
106
Sg
107
Bh
108
Hs
109
Mt
110
Ds
111
Rg
112
Cn
113
Nh
114
Fl
115
Mc
116
Lv
117
Ts
118
Og
 
*Lanthanoids *
57
La
58
Ce
59
Pr
60
Nd
61
Pm
62
Sm
63
Eu
64
Gd
65
Tb
66
Dy
67
Ho
68
Er
69
Tm
70
Yb
**Actinoids **
89
Ac
90
Th
91
Pa
92
U
93
Np
94
Pu
95
Am
96
Cm
97
Bk
98
Cf
99
Es
100
Fm
101
Md
102
No