Table of Contents
Electronegativity Trend ;
The electronegativity trend is the way in which the electronegativity of atoms increases as you move from left to right across a period on the periodic table. The electronegativity of an atom is a measure of how strongly it attracts electrons to itself. The higher the electronegativity of an atom, the more it will pull electrons away from other atoms.
Ionic Bonding
In ionic bonding, atoms lose or gain electrons to form ions with a net positive or negative charge. These oppositely charged ions then attract each other to form a stable ionic bond. Ionic bonding typically occurs between a metal and a non-metal.
Covalent Bonding
A covalent bond is a chemical bond that occurs when two atoms share one or more pairs of electrons. Covalent bonds are the strongest type of chemical bond and are responsible for the stability of molecules.
Patterns of Electronegativity In The Periodic Table
The periodic table is a chart that shows the chemical elements and their properties. It is organized by the number of protons in the nucleus of an atom of that element. The farther to the right on the table an element is, the more protons it has in its nucleus.
The periodic table is also organized by the amount of electron charge an atom has. The more positive the number is, the more electron charge the atom has. The more negative the number is, the less electron charge the atom has.
The elements are also organized by their electronegativity. Electronegativity is a measure of how much an atom wants to hold on to its electrons. The higher the number, the more an atom wants to hold on to its electrons.
The most electronegative element is fluorine. It has a number of 4.0. The least electronegative element is francium. It has a number of 0.7.
Electronegativity Across a Period
The electronegativity of an atom decreases as you move from left to right across a period. This is because as you move from left to right, the distance between the nucleus and the electrons increases. This increase in distance means that the electrons are less tightly bound to the nucleus and are, therefore, less strongly attracted to it.
