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 element has an atom with the greatest attraction for electrons in a chemical bond

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, 3rd edition. Oxford: Clarendon Press, 1998.

Electronegativity refers to the capacity of one atom to entice shared electron in a covalent bond. The greater the worth of the electronegativity, the more strongly that element attracts the shared electrons.

The principle of electronegativity was introduced by Linus Pauling in 1932; ~ above the Pauling scale, fluorine is assigned an electronegativity of 3.98, and the other facets are scaled relative to that value. Various other electronegativity scales incorporate the Mulliken scale, proposed by Robert S. Mulliken in 1934, in which the very first ionization energy and also electron affinity room averaged together, and also the Allred-Rochow scale, which procedures the electrostatic attraction in between the cell nucleus of an atom and its valence electrons.

Electronegativity different in a predictable way across the routine table. Electronegativity increases from bottom to top in groups, and increases indigenous left come right across periods. Thus, fluorine is the many electronegative element, while francium is one of the the very least electronegative.(Helium, neon, and also argon space not provided in the Pauling electronegativity scale, return in the Allred-Rochow scale, helium has the highest electronegativity.) The trends are not an extremely smooth amongst the shift metals and also the inner shift metals, however are fairly regular because that the main group elements, and also can be watched in the charts below.

See more: Simplify Square Root Of Negative 121., Simplify Square Root Of

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The difference in electronegativity between two bonded elements determines what type of shortcut they will certainly form. Once atoms v an electronegativity distinction of higher than 2 units space joined together, the bond that is created is one ionic bond, in which the much more electronegative facet has a an adverse charge, and also the much less electronegative facet has a positive charge. (As an analogy, you can think of it as a video game of tug-of-war in which one team is solid enough to pull the rope far from the various other team.) because that example, sodium has actually an electronegativity the 0.93 and chlorine has an electronegativity the 3.16, so as soon as sodium and also chlorine form an ionic bond, in which the chlorine takes an electron away from sodium, forming the salt cation, Na+, and also the chloride anion, Cl-. Particular sodium and also chloride ions space not "tied" together, yet they entice each other very solid because of the contrary charges, and kind a solid crystal lattice.

When atoms with an electronegativity difference of less than two units room joined together, the bond that is developed is a covalent bond, in i m sorry the electron are mutual by both atoms. As soon as two of the same atom share electron in a covalent bond, there is no electronegativity difference in between them, and the electrons in the covalent bond are shared equally — the is, over there is a symmetrical distribution of electrons between the bonded atoms. These bonds are nonpolar covalent bonds. (As one analogy, you can think of it as a game of tug-of-war in between two equally solid teams, in i beg your pardon the rope doesn"t move.) because that example, when two chlorine atoms room joined through a covalent bond, the electron spend simply as lot time close come one chlorine atoms together they perform to the other, and also the result molecule is nonpolar:

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When the electronegativity distinction is in between 0 and 2, the much more electronegative facet attracts the shared more strongly, but not strongly sufficient to eliminate the electrons fully to form an ionic compound. The electron are shared unequally — the is, over there is one unsymmetrical distribution of electrons between the bonded atoms. These bonds are dubbed polar covalent bonds. The much more electronegative atom has a partial an unfavorable charge, d-, because the electron spend more time closer to the atom, if the less electronegative atom has a partial hopeful charge, d+, since the electron are partly (but no completely) pulled away from that atom. Because that example, in the hydrogen chloride molecule, chlorine is an ext electronegative than hydrogen by 0.96 electronegativity units. The mutual electrons spend more time close come the chlorine atom, do the chlorine finish of the molecule very slightly negative (indicated in the figure below by the blue shaded region), while the hydrogen finish of the molecule is an extremely slightly confident (indicated by the red shaded region), and also 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 room oriented with respect to each other, determines whether or not the molecule is polar. This polarity of molecules plays a big role in identify the physics properties that compounds.