1. Electronegativity
- Electronegativity is a measure of the tendency of an atom to attract a bonding pair of electrons. It is also the tendency of an atom to attract electrons in a molecule. Large differences in electronegativity between atoms in a given
2.Atomic Radius
- The atomic radius is defined as one-half the distance between the nuclei of identical atoms that are bonded together.The atomic radius (r) of an atom can be defined as one half the distance (d) between two nuclei in a diatomic molecule. Moreover, Atomic radius is generally stated as being the total distance from an atom's nucleus to the outermost orbital of electron.
3.Electron affinity
- Electron affinity is defined as the change in energy (in kJ/mole) of a neutral atom (in the gaseous phase) when an electron is added to the atom to form a negative ion. In other words, the neutral atom's likelihood of gaining an electron.
4.Ionization energy
- Ionization energy is the quantity of energy that an isolated, gaseous atom in the ground electronic state must absorb to discharge an electron, resulting in a cation. H(g)→H+(g)+e− This energy is usually expressed in kJ/mol, or the amount of energy it takes for all the atoms in a mole to lose one electron.
5.Metallic and nonmetallic property
- Metallic character refers to the level of reactivity of a metal. Non-metallic character relates to the tendency to accept electrons during chemical reactions. Metallic tendency increases going down a group. Non-metallic tendency increases going from left to right across the periodic table.
