Electronegativity

electronegativity - atoms tendency to attract a bonding pair of electrons

ELECTRONEGATIVITY

electronegativity - atoms tendency to attract a bonding pair of electrons

Electronegativity is a measure of how strongly an atom – in a molecule – is able to attract electrons to itself.

ELECTRONEGATIVITY IS AFFECTED BY

1) The atomic number

The atomic number is the number of protons in the nucleus of an atom.
It determines the chemical properties of an element and its place in the periodic table.
The higher the atomic number, the stronger the electronegativity.
atomic-number-ant

2) The atomic radius

The atomic radius of a chemical element is usually measured by the distance from the center of the nucleus to the boundary of the outermost layer of electrons.
The bigger the atomic radii, the weaker the electronegativity.
Atomic radius ant

Example of atomic radius of an oxygen atom
Atomic radius of an oxygen atom

What is electronegativity measured in?

The most common measurement for electronegativity is the Pauling scale, designed by two-time Noble prize winner Linus Pauling. Electronegativity scale for elements tell how strong each element (relative to each other) can attract electrons to iteself. The higher the electronegativity number, the more the atom will attempt to pull electrons to itself.
Electronegativity is measured in Pauling

Why is oxygen more electronegative than nitrogen?

Oxygen is higher in atomic number

  • Oxygen has 8 protons in the nucleus whereas nitrogen only has 7.
  • A bonding pair of electrons will experience more attraction from the oxygen’s nucleus that from nitrogen, thus the electronegativity of oxygen is greater.

electronegativity-oxygen-nitrogen

The positively charged protons in the nucleus attract the negatively charged electrons.

Atomic number of an atom has an influence on the negativity of the atom

Why is sulphur less electronegative than oxygen?

Electronegativity oxygen vs sulphur

The reason why Oxygen is more electronegative is
Oxygen has a smaller atomic radius, the bonding electrons are closer to the nucleus and therefore exerts a higher pull
Bonding electrons in sulphur are further away from the nucleus therefore it exerts a weaker force
There is one layer of shielding electrons in oxygen whereas in sulphur, there are two layers.

Please read up on valence electrons before you proceed. Valence Electrons

enlargeroxygen-sulphur-electronegativity

  • Sulphur’s bonding electrons are in the 3rd-level and shielded from the 16 protons in the nucleus by a total of 10 electrons in the 1st and 2nd level.
  • Oxygen’s bonding electrons are at the 2nd-level, and shielded from the 8 protons in the nucleus by the 2 electrons in the 1s orbital.
  • Sulphur is less electronegative than oxygen because in the sulphur element, the bonding electrons (or valence electrons) are further from the nucleus, so they are less tightly held by the forces of its protons.

The smaller atom has a higher electronegativity.

The shielding electrons

Electronegativity trends present in the periodic table

electronegativity-and-the-periodic-table

When you move across the period table, the number of protons in the nucleus increases, therefore the electonegativity increases.

ELECTRONEGATIVITY TRENDS ACROSS TABLE
ELECTRONEGATIVITY GENERALLY INCREASES ACROSS THE PERIODIC TABLE

When the atomic number increases down a group, there is also an increase in the valence electrons and nucleus. The atomic radius is greater therefore electronegativity decreases.

Electronegativity trends down periodic table
ELECTRONEGATIVITY GENERALLY DECREASES DOWN GROUPS IN A PERIODIC TABLE

PERIODIC TABLE OF ELECTRONEGATIVITY

periodic table pauling scale of electronegativityDiagram from Wikipedia issued under Creative Common Licenses

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