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 would you expect to have a higher electronegativity than nitrogen (n)?

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 taken from john Emsley, The Elements, third edition. Oxford: Clarendon Press, 1998.

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

The principle of electronegativity was introduced by Linus Pauling in 1932; top top the Pauling scale, fluorine is assigned an electronegativity of 3.98, and the other elements are scaled family member to that value. Various other electronegativity scales include the Mulliken scale, propose by Robert S. Mulliken in 1934, in which the first ionization energy and also electron affinity room averaged together, and also the Allred-Rochow scale, which steps the electrostatic attraction between the cell core of one atom and also its valence electrons.

Electronegativity varies in a predictable way across the periodic table. Electronegativity increases from bottom to peak in groups, and increases from left to right across periods. Thus, fluorine is the most electronegative element, if francium is just one of the least electronegative.(Helium, neon, and also argon are not listed in the Pauling electronegativity scale, return in the Allred-Rochow scale, helium has actually the highest electronegativity.) The trends room not really smooth among the transition metals and the inner change metals, but are relatively regular for the main team elements, and also can be checked out in the charts below.

See more: Cov A Covalent Bond In Which Electrons Are Shared Unequally Is

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The distinction in electronegativity in between two bonded aspects determines what kind of shortcut they will certainly form. As soon as atoms v an electronegativity distinction of better than 2 units room joined together, the bond that is created is an ionic bond, in i m sorry the much more electronegative element has a an unfavorable charge, and the less electronegative aspect has a confident charge. (As one analogy, you can think that it as a game of tug-of-war in which one team is solid enough to pull the rope far from the various other team.) for example, sodium has an electronegativity that 0.93 and chlorine has an electronegativity the 3.16, so when sodium and also chlorine form an ionic bond, in i beg your pardon the chlorine take away an electron far from sodium, developing the sodium cation, Na+, and the chloride anion, Cl-. Certain sodium and also chloride ions space not "tied" together, but they tempt each various other very strong because of the contrary charges, and form a solid crystal lattice.

When atoms with an electronegativity difference of less than two units room joined together, the bond that is created is a covalent bond, in i m sorry the electrons are mutual by both atoms. Once 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 common equally — the is, there is a symmetrical circulation of electrons in between the bonded atoms. These bonds are nonpolar covalent bonds. (As an analogy, you have the right to think that it as a game of tug-of-war in between two equally strong teams, in i m sorry the rope doesn"t move.) for example, as soon as two chlorine atoms space joined through a covalent bond, the electron spend just as much time close come one chlorine atoms as they execute to the other, and the result molecule is nonpolar:

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When the electronegativity difference is between 0 and also 2, the much more electronegative facet attracts the shared an ext strongly, yet not strongly sufficient to eliminate the electrons completely to kind an ionic compound. The electron are common unequally — the is, over there is an unsymmetrical distribution of electrons in between the bonded atoms. This bonds are called polar covalent bonds. The much more electronegative atom has a partial negative charge, d-, due to the fact that the electrons spend much more time closer to that atom, when the less electronegative atom has a partial confident charge, d+, because 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 by 0.96 electronegativity units. The shared electrons spend an ext time close to the chlorine atom, making the chlorine finish of the molecule really slightly an unfavorable (indicated in the figure below by the blue shaded region), when the hydrogen finish of the molecule is really slightly optimistic (indicated by the red shaded region), and also the resulting molecule is polar:

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For molecules with more than one covalent bond, the three-dimensional form of the molecule and also how the polar bonds space oriented v respect to each other, determines whether or not the molecule is polar. This polarity of molecule plays a large role in identify the physics properties that compounds.