To determine the order of electronegativity of the elements B (Boron), C (Carbon), At (Astatine), and S (Sulfur), we need to understand the concept of electronegativity. Electronegativity is defined as a chemical property that describes the tendency of an atom to attract a shared pair of electrons towards itself in a covalent bond.
Factors Influencing Electronegativity:
The electronegativity generally increases across a period from left to right in the periodic table due to an increase in nuclear charge, which attracts the bonding pair of electrons more strongly.
The electronegativity generally decreases down a group in the periodic table because the added electron shells increase the distance between the nucleus and the valence electron shells, reducing the nuclear attraction.
Electronegativity Values:
Boron (B): Approximately 2.04
Carbon (C): Approximately 2.55
Sulfur (S): Approximately 2.58
Astatine (At): Approximately 2.2
Using the above electronegativity values, we can arrange the elements in order of decreasing electronegativity:
