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: An atom of which element has the strongest attraction for electrons

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 man Emsley, The Elements, third edition. Oxford: Clarendon Press, 1998.

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

The principle of electronegativity was presented by Linus Pauling in 1932; ~ above the Pauling scale, fluorine is assigned an electronegativity that 3.98, and also the other elements are scaled family member to the value. Various other electronegativity scales include 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 the Allred-Rochow scale, which procedures the electrostatic attraction in between the cell nucleus of one atom and its valence electrons.

Electronegativity different in a predictable means across the routine table. Electronegativity increases from bottom to optimal in groups, and increases indigenous left to right across periods. Thus, fluorine is the most electronegative element, when francium is among the the very least electronegative.(Helium, neon, and also argon room not provided in the Pauling electronegativity scale, back in the Allred-Rochow scale, helium has the greatest electronegativity.) The trends room not very smooth among the shift metals and also the inner transition metals, yet are relatively regular for the main team elements, and can be viewed in the charts below.

See more: Three Primary Activities Of A Typical Program Are, 5 Information Systems Software

*

*

*

The difference in electronegativity between two bonded elements determines what kind of bond they will certainly form. Once atoms with an electronegativity distinction of higher than two units are joined together, the bond the is formed is one ionic bond, in i beg your pardon the more electronegative aspect has a an adverse charge, and also the less electronegative aspect has a optimistic charge. (As one analogy, you can think of it as a video game of tug-of-war in which one team is solid enough to traction the rope far from the other team.) because that example, sodium has actually an electronegativity that 0.93 and chlorine has an electronegativity that 3.16, so once sodium and chlorine type an ionic bond, in which the chlorine takes an electron away from sodium, forming the salt cation, Na+, and the chloride anion, Cl-. Certain sodium and chloride ions space not "tied" together, however they lure each various other very strong because of the opposite charges, and kind a solid crystal lattice.

When atoms through an electronegativity difference of less than 2 units space joined together, the bond the is formed is a covalent bond, in i beg your pardon the electron are mutual by both atoms. When two of the same atom share electrons in a covalent bond, over there is no electronegativity difference between them, and the electrons in the covalent link are mutual equally — that is, over there is a symmetrical circulation of electrons between the bonded atoms. These bonds are nonpolar covalent bonds. (As an analogy, you have the right to think the it together a video game of tug-of-war in between two equally solid teams, in i beg your pardon the rope doesn"t move.) for example, when two chlorine atoms space joined through a covalent bond, the electrons spend just as much time close to one chlorine atoms as they do to the other, and the resulting molecule is nonpolar:

*

*

When the electronegativity difference is between 0 and also 2, the more electronegative element attracts the shared more strongly, yet not strongly sufficient to remove the electrons fully to type an ionic compound. The electrons are common unequally — that is, there is one unsymmetrical distribution of electrons in between the bonded atoms. This bonds are dubbed polar covalent bonds. The much more electronegative atom has a partial an adverse charge, d-, due to the fact that the electrons spend an ext time closer to the atom, if the less electronegative atom has a partial optimistic charge, d+, due to the fact that the electron are partially (but not completely) pulled away from the atom. Because that example, in the hydrogen chloride molecule, chlorine is much more electronegative 보다 hydrogen through 0.96 electronegativity units. The mutual electrons spend much more time close to the chlorine atom, do the chlorine end of the molecule an extremely slightly an unfavorable (indicated in the figure listed below by the blue shaded region), when the hydrogen end of the molecule is really slightly hopeful (indicated by the red shaded region), and also the resulting molecule is polar:

*

*

For molecule with an ext than one covalent bond, the three-dimensional shape of the molecule and how the polar bonds room oriented with respect to each other, determines even if it is or no the molecule is polar. This polarity of molecule plays a big role in identify the physical properties of compounds.