Write periodic trends in the ionization energy across a period and along a group of the periodic table.
Write periodic trends in the ionization energy across a period and along a group of the periodic table.
Step 1:
The elements are arranged in groups and periods on similarity in chemical property and in increasing atomic number is called modern periodic table.
The horizontal rows in modern periodic table are called periods. There are totally 7 periods. The elements of a period have different atomic numbers and different valence electrons.
The vertical columns in modern periodic table are called groups. There are totally 18 groups.
Step 2:
The ionization energy is the energy needed to remove an electron from the outer shell of isolated atom. It is denoted as IE.
The atomic size, effective nuclear charge and screening effect are the factors that influence the ionization energy.
Step 3:
Trend of Ionization enthalpy across a period: The ionization energy increases on moving from left to right across the period due to the decrease in size of atom on increasing the atomic number and thus, the electrons in valence shell goes closer to the nucleus. There is more energy needed to remove an electron from outermost shell.
Trend of Ionization enthalpy down the group: The ionization energy decreases down the group because of the increase in number of shells. Thus, the atomic size increases thereby decreasing the ionization energy.
Step 1:
The elements are arranged in groups and periods on similarity in chemical property and in increasing atomic number is called modern periodic table.
The horizontal rows in modern periodic table are called periods. There are totally 7 periods. The elements of a period have different atomic numbers and different valence electrons.
The vertical columns in modern periodic table are called groups. There are totally 18 groups.
Step 2:
The ionization energy is the energy needed to remove an electron from the outer shell of isolated atom. It is denoted as IE.
The atomic size, effective nuclear charge and screening effect are the factors that influence the ionization energy.
Step 3:
Trend of Ionization enthalpy across a period: The ionization energy increases on moving from left to right across the period due to the decrease in size of atom on increasing the atomic number and thus, the electrons in valence shell goes closer to the nucleus. There is more energy needed to remove an electron from outermost shell.
Trend of Ionization enthalpy down the group: The ionization energy decreases down the group because of the increase in number of shells. Thus, the atomic size increases thereby decreasing the ionization energy.
