Question

Give the correct order of electronegativity of the following elements :

F Cl O Br


PLEASE EXPLAIN WITH QUALITY REASONS..!!

NO SPAMMING !!!

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Answer 1

Answer:

F>O>Cl>Br

fluorine is highly electronegative because it has 5 electron in it's 2p shell.

oxygen is situated at right part of the pereodic tables . as you move from left to right electronegative increases. and oxygen has 6 valence electron it can still attract 2more electron .

cl has more electronegative because it has got greater tedency to attract an electronic from another atom.

Br , the electron are further away from nucleus and better shielded from the neclear charge and thus not as attracted from the nucleus thats why electronegative is less in Br

Answer 2

Solution :-

First Thing to know - What is electronegativity ?

It is the property of any atom of a element to form a Covalent bond.

How to relate Electronegativity between two or more elements ?

Electronegativity of elements increases from the bottom of the periodic table to top.

Electronegativity of elements increases from left to right of the periodic table

Note :- We are not considering Nobel gasses as they have complete octate/duet .

So we are here with the elements :-

F :- Florine

Atomic No :- 9

Period :- 2

Group :- VII A or 17

Cl :- Chlorine

Atomic No :- 17

Period :- 3

Group :- VII A or 17

O :- Oxygen

Atomic No :- 8

Period :- 2

Group :- VI A or 16

Br :- Bromine

Atomic No :- 35

Period :- 4

Group :- VII A or 17

Now via group :-

In Group 2 :- O , F

In Group 3 :- Cl

In Group 4 :- Br

So we have got in electronegativity series :-

( O , F ) > Cl > Br

Now the comparison Between O and F

Period of O :- VI A or 16

Period of F :- VII A or 17

→ F > O

So electronegativity series

→ F > O > Cl > Br