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.

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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 taken from john Emsley, The Elements, 3rd edition. Oxford: Clarendon Press, 1998.

Electronegativity refers to the capability of an atom to lure shared electrons in a covalent bond. The higher the worth of the electronegativity, the an ext strongly that element attracts the shared electrons.

The concept of electronegativity was presented by Linus Pauling in 1932; on the Pauling scale, fluorine is assigned an electronegativity the 3.98, and the other aspects are scaled family member to the value. Other electronegativity scales incorporate the Mulliken scale, proposed by Robert S. Mulliken in 1934, in which the first ionization energy and also electron affinity space averaged together, and also the Allred-Rochow scale, which procedures the electrostatic attraction between the cell nucleus of one atom and its valence electrons.

Electronegativity different in a predictable method across the routine table. Electronegativity increases from bottom to optimal in groups, and increases native left come right throughout periods. Thus, fluorine is the most electronegative element, if francium is one of the the very least electronegative.(Helium, neon, and also argon space not provided in the Pauling electronegativity scale, back in the Allred-Rochow scale, helium has actually the greatest electronegativity.) The trends are not really smooth amongst the shift metals and also the inner transition metals, yet are reasonably regular because that the main group elements, and can be seen in the charts below.

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The distinction in electronegativity between two bonded elements determines what form of link they will certainly form. When atoms with an electronegativity distinction of better than 2 units are joined together, the bond the is developed is an ionic bond, in i beg your pardon the much more electronegative element has a an unfavorable charge, and the much less electronegative aspect has a optimistic charge. (As one analogy, you have the right to think the it as a video game of tug-of-war in which one team is solid enough to traction the rope far from the various other team.) because that example, sodium has actually an electronegativity that 0.93 and chlorine has an electronegativity the 3.16, so once sodium and chlorine kind an ionic bond, in i m sorry the chlorine bring away an electron far from sodium, forming the sodium cation, Na+, and also the chloride anion, Cl-. Specific sodium and also chloride ions room not "tied" together, yet they lure each various other very strong because of the contrary charges, and kind a solid crystal lattice.

When atoms with an electronegativity difference of less than 2 units room joined together, the bond the is created is a covalent bond, in i beg your pardon the electrons are common by both atoms. Once two of the very same atom share electrons in a covalent bond, over there is no electronegativity difference in between them, and also the electron in the covalent shortcut are shared equally — the is, there is a symmetrical distribution of electrons between the external inspection atoms. These bonds are nonpolar covalent bonds. (As an analogy, you can 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, once two chlorine atoms room joined by a covalent bond, the electrons spend just as lot time close come one chlorine atoms as they carry out to the other, and also the resulting molecule is nonpolar:

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When the electronegativity distinction is between 0 and also 2, the an ext electronegative facet attracts the shared more strongly, yet not strongly enough to eliminate the electrons fully to type an ionic compound. The electron are mutual unequally — the is, there is an unsymmetrical distribution of electrons between the bonded atoms. These bonds are called polar covalent bonds. The more electronegative atom has actually a partial an adverse charge, d-, due to the fact that the electron spend more time closer to that atom, when the less electronegative atom has actually a partial optimistic charge, d+, since the electrons are partly (but not completely) pulled away from that atom. Because that example, in the hydrogen chloride molecule, chlorine is much more electronegative 보다 hydrogen by 0.96 electronegativity units. The mutual electrons spend an ext time close come the chlorine atom, make the chlorine finish of the molecule an extremely slightly an adverse (indicated in the figure listed below by the blue shaded region), if the hydrogen finish of the molecule is really slightly hopeful (indicated by the red shaded region), and the result molecule is polar:

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For molecule with more than one covalent bond, the three-dimensional form of the molecule and how the polar bonds are oriented through respect to each other, determines even if it is or not the molecule is polar. This polarity of molecules plays a huge role in identify the physical properties of compounds.