Respuesta :
a) figure describe ionization energy , electron affinity & electron negativity
b) figure describe Atomic Radius
c) does represent anything
Electronegativity : An atom attracted the bond pair of electrons in a covalent bond is called electronegativity of an element. H-->Cl
Ionization energy : The amount of energy is required to remove of an electron from an isolated gas atom is called Ionization energy. M + IP-----> M+ + e-
Electron affinity: The amount of enery is released when an electron added to an isolated atom is called electron affinity.
X + e- ------> X- =- EA
Atomic radius ; The distance between the center of neuclies and outer most shell is called atomic radius.
Answer:
From the given diagrams, figure (a) represents the trend, ionization energy, electron affinity, and electronegativity. Figure (b) describes the trend in atomic radius
Explanation:
Atomic radius: It can be defined as the distance between the nuclei f the two identical atoms. In the periodic table on moving from left to right, the atomic radius decreases and there is an increase in the atomic radius on moving down the group.
Ionization energy: It can be defined as the energy required to remove one electron. In the periodic table on moving left to right ionization energy decreases because of electrons bound away from nuclei. On moving down the group there is an increase in the ionization energy.
Electron affinity: It is the amount of energy released from the atom on addition of an electron. Electron affinity increases on moving from left to right in the periodic table. The electron affinity decreases going down the group in a periodic table.
Electronegativity: It can be defined as the increase in the nuclear charge. Electronegativity increases across the group from left to right and decreases down the group.
In the diagram given, Figure (a) represents the trend in ionization energy and electron affinity.
Figure (b) represents the trend in atomic radius, and (c) does not represent any trend.
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