Interpretation: From the given elements the element with greater first ionization energy and the element with greater second ionization energy should be determined.
Concept Introduction:
Periodic Table: The available chemical elements are arranged considering their
In periodic table the horizontal rows are called periods and the vertical column are called group.
There are seven periods and 18 groups present in the table and some of those groups are given special name as follows,
Cation: Removal of electron from the atom results to form positively charged ion called cation.
Anion: Addition of electron to atom results to form negatively charged ion called anion.
The net charge present in the element denotes the presence or absence of electrons in the element.
First ionization energy:
The ionization energy is the minimum energy required to remove the electron from an isolated atom which is in the gaseous state results to give gaseous ion with one positive charge.
Second ionization:
Repeating the same process that is removal of another electron that is second electron from the resulting ion of first ionization is called second ionization.
Third ionization energy:
Removal of electron from ion that results from the second ionization is called third ionization which results to give ion with three positive charges which shows, three electrons gets removed from the atom and the energy associated with it is called third ionization energy.
Atomic Number: Atomic number of the element is equal to the number of protons presents in nucleus of the element which is denoted by symbol Z. The superscript presents on the left side of the
To determine: The element that has larger first ionization energy and the element with larger second ionization energy.

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Chapter 4 Solutions
CHEMISTRY: ATOMS FIRST VOL 1 W/CONNECT
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