1A 2A 3A 4A 5A 6A 7A 8A
(1) (2) (13) (14) (15) (16) (17) (18)
3B 4B 5B 6B 7B 8B 1B 2B
(3) (4) (5) (6) (7) (8) (9) (10) (11) (12)
1

H

2.20

He

n.a.

You are watching: Arrange these elements in order of decreasing electronegativity:

2 Li

0.98

Be

1.57

B

2.04

C

2.55

N

3.04

O

3.44

F

3.98

Ne

n.a.

3 Na

0.93

Mg

1.31

Al

1.61

Si

1.90

P

2.19

S

2.58

Cl

3.16

Ar

n.a.

4 K

0.82

Ca

1.00

Sc

1.36

Ti

1.54

V

1.63

Cr

1.66

Mn

1.55

Fe

1.83

Co

1.88

Ni

1.91

Cu

1.90

Zn

1.65

Ga

1.81

Ge

2.01

As

2.18

Se

2.55

Br

2.96

Kr

3.00

5 Rb

0.82

Sr

0.95

Y

1.22

Zr

1.33

Nb

1.60

Mo

2.16

Tc

1.90

Ru

2.20

Rh

2.28

Pd

2.20

Ag

1.93

Cd

1.69

In

1.78

Sn

1.96

Sb

2.05

Te

2.10

I

2.66

Xe

2.60

6 Cs

0.79

Ba

0.89

La

1.10

Hf

1.30

Ta

1.50

W

2.36

Re

1.90

Os

2.20

Ir

2.20

Pt

2.28

Au

2.54

Hg

2.00

Tl

1.62

Pb

2.33

Bi

2.02

Po

2.00

At

2.20

Rn

n.a.

7 Fr

0.70

Ra

0.89

Ac

1.10

Rf

n.a.

Db

n.a.

Sg

n.a.

Bh

n.a.

Hs

n.a.

Mt

n.a.

Ds

n.a.

Rg

n.a.

Uub

n.a.

Uuq

n.a.

6 Ce

1.12

Pr

1.13

Nd

1.14

Pm

1.13

Sm

1.17

Eu

1.20

Gd

1.20

Tb

1.10

Dy

1.22

Ho

1.23

Er

1.24

Tm

1.25

Yb

1.10

Lu

1.27

7 Th

1.30

Pa

1.50

U

1.38

Np

1.36

Pu

1.28

Am

1.30

Cm

1.30

Bk

1.30

Cf

1.30

Es

1.30

Fm

1.30

Md

1.30

No

1.30

Lr

1.30


Electronegativities report in Pauling units

Data bring away from john Emsley, The Elements, third edition. Oxford: Clarendon Press, 1998.

Electronegativity refers to the capacity of an atom to attract shared electrons in a covalent bond. The greater the worth of the electronegativity, the much more strongly that aspect attracts the common electrons.

The concept of electronegativity was introduced by Linus Pauling in 1932; top top the Pauling scale, fluorine is assigned one electronegativity of 3.98, and also the other elements are scaled relative to that value. Various other electronegativity scales incorporate the Mulliken scale, suggest by Robert S. Mulliken in 1934, in i beg your pardon the very first ionization energy and also electron affinity are averaged together, and also the Allred-Rochow scale, which procedures the electrostatic attraction in between the cell core of an atom and its valence electrons.

Electronegativity different in a predictable method across the periodic table. Electronegativity increases from bottom to height in groups, and increases from left come right across periods. Thus, fluorine is the many electronegative element, if francium is among the the very least electronegative.(Helium, neon, and also argon space not detailed in the Pauling electronegativity scale, return in the Allred-Rochow scale, helium has actually the highest electronegativity.) The trends are not really smooth among the transition metals and also the inner change metals, yet are fairly regular because that the main team elements, and can be watched in the charts below.

See more: The Chemical Messengers Released Into The Junctions Between Neurons Are Called

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The difference in electronegativity between two bonded facets determines what form of bond they will certainly form. When atoms through an electronegativity difference of better than two units are joined together, the bond the is formed is an ionic bond, in which the an ext electronegative facet has a an unfavorable charge, and also the much less electronegative facet has a hopeful charge. (As an analogy, you have the right to think of it together a game of tug-of-war in i beg your pardon one team is solid enough to pull the rope away from the various other team.) for example, sodium has actually an electronegativity the 0.93 and chlorine has actually an electronegativity the 3.16, so when sodium and chlorine type an ionic bond, in i beg your pardon the chlorine take away an electron away from sodium, creating the salt cation, Na+, and also the chloride anion, Cl-. Details sodium and chloride ions space not "tied" together, however they entice each various other very solid because of the contrary charges, and form a strong crystal lattice.

When atoms v an electronegativity distinction of less than two units room joined together, the bond the is formed is a covalent bond, in i m sorry the electron are shared by both atoms. As soon as two the the very same atom share electrons in a covalent bond, over there is no electronegativity difference between them, and also the electron in the covalent bond are common equally — the is, over there is a symmetrical circulation of electrons between the bonded atoms. These bonds space nonpolar covalent bonds. (As one analogy, you can think the it together a game of tug-of-war between two equally strong teams, in i m sorry the rope doesn"t move.) for example, when two chlorine atoms room joined by a covalent bond, the electrons spend just as lot time close come one chlorine atoms together they perform to the other, and also the resulting molecule is nonpolar:

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When the electronegativity distinction is between 0 and 2, the an ext electronegative element attracts the shared more strongly, but not strongly sufficient to remove the electrons fully to type an ionic compound. The electron are mutual unequally — the is, over there is an unsymmetrical circulation of electrons in between the bonded atoms. These bonds are referred to as polar covalent bonds. The an ext electronegative atom has a partial an adverse charge, d-, because the electrons spend much more time closer to that atom, when the much less electronegative atom has actually a partial optimistic charge, d+, due to the fact that the electron are partly (but not completely) pulled away from the atom. Because that example, in the hydrogen chloride molecule, chlorine is much more electronegative than hydrogen by 0.96 electronegativity units. The mutual electrons spend more time close come the chlorine atom, making the chlorine finish of the molecule very slightly an unfavorable (indicated in the figure below by the blue shaded region), if the hydrogen end of the molecule is really slightly confident (indicated by the red shaded region), and the result molecule is polar:

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For molecule with an ext than one covalent bond, the three-dimensional shape of the molecule and how the polar bonds are oriented v respect to each other, determines whether or not the molecule is polar. This polarity of molecule plays a big role in determining the physical properties the compounds.