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: Which of the following elements has the lowest 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 reported in Pauling units

Data bring away from man Emsley, The Elements, 3rd edition. Oxford: Clarendon Press, 1998.

Electronegativity refers come the ability of one atom to tempt shared electrons in a covalent bond. The higher the worth of the electronegativity, the an ext strongly that aspect attracts the common electrons.

The ide of electronegativity was introduced by Linus Pauling in 1932; on the Pauling scale, fluorine is assigned one electronegativity of 3.98, and also the other aspects are scaled loved one to that value. Other electronegativity scales incorporate the Mulliken scale, propose by Robert S. Mulliken in 1934, in which the first ionization energy and also electron affinity are averaged together, and also the Allred-Rochow scale, which actions the electrostatic attraction between the nucleus of an atom and its valence electrons.

Electronegativity varies in a predictable method across the regular table. Electronegativity increases from bottom to optimal in groups, and increases from left come right across periods. Thus, fluorine is the many electronegative element, if francium is one of the the very least electronegative.(Helium, neon, and argon room not detailed in the Pauling electronegativity scale, return in the Allred-Rochow scale, helium has the greatest electronegativity.) The trends are not really smooth amongst the shift metals and the inner change metals, but are fairly regular because that the main team elements, and can be checked out in the charts below.

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The distinction in electronegativity between two bonded elements determines what kind of shortcut they will certainly form. Once atoms v an electronegativity difference of greater than two units room joined together, the bond the is created is an ionic bond, in i m sorry the much more electronegative facet has a an adverse charge, and also the less electronegative facet has a hopeful charge. (As an analogy, you have the right to think the it together a game of tug-of-war in i m sorry one team is strong enough to traction the rope away from the other team.) for example, sodium has an electronegativity the 0.93 and also chlorine has an electronegativity the 3.16, so as soon as sodium and also chlorine type an ionic bond, in which the chlorine take away an electron away from sodium, developing the salt cation, Na+, and also the chloride anion, Cl-. Certain sodium and also chloride ions room not "tied" together, however they tempt each various other very solid because of opposing charges, and kind a strong crystal lattice.

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

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When the electronegativity distinction is between 0 and 2, the much more electronegative aspect attracts the shared more strongly, yet not strongly sufficient to eliminate the electrons completely to kind an ionic compound. The electrons are shared unequally — that is, there is one unsymmetrical circulation of electrons between the bonded atoms. These bonds are dubbed polar covalent bonds. The more electronegative atom has a partial negative charge, d-, because the electrons spend much more time closer to the atom, while the much less electronegative atom has actually a partial hopeful charge, d+, because the electron are partially (but not completely) pulled away from the atom. For example, in the hydrogen chloride molecule, chlorine is much more electronegative than hydrogen through 0.96 electronegativity units. The mutual electrons spend more time close come the chlorine atom, making the chlorine end of the molecule an extremely slightly an adverse (indicated in the figure below by the blue shaded region), when the hydrogen finish of the molecule is very slightly positive (indicated through the red shaded region), and also the resulting molecule is polar:

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For molecules with much more than one covalent bond, the three-dimensional shape of the molecule and how the polar bonds are oriented with respect to each other, determines whether or no the molecule is polar. This polarity of molecules plays a big role in identify the physical properties of compounds.