Question

The first ionization energies of an element are approximately 738 kj/mol, 1450 kj/mol, 7.7 × 103 kj/mol, and 1.1 × 104 kj/mol. to which periodic group does this element belong?

Answer 1

Theres a big jump between the 2nd and 3rd I.E. so the element has 2 valence electrons hence Group 2

Answer 2

The given element belongs to $\boxed{{\text{second}}}$ group of the periodic table.

Further Explanation:

Ionization energy:

The amount of energy that is required to remove the most loosely bound valence electrons from the isolated neutral gaseous atom is known as ionization energy. It is represented by IE. Its value is related to the ease of removing the outermost valence electrons. If these electrons are removed so easily, small ionization energy is required and vice-versa. It is inversely proportional to the size of the atom.

Successive ionization energies are evaluated when the electrons are to be removed from successive shells. When the first electron is removed from the isolated neutral gaseous atom, ionization energy is termed as the first ionization energy $\left({{\text{I}}{{\text{E}}_{\text{1}}}}\right)$. Similarly, when the second electron is removed from the monoatomic cation, ionization energy is called the second ionization energy $\left({{\text{I}}{{\text{E}}_{\text{2}}}}\right)$ and so on…

Ionization energy trends in the periodic table:

While moving from left to right in a period, IE increases due to the decrease in the atomic size of the succeeding members. This results in the strong attraction of electrons and hence are difficult to remove.

While moving from top to bottom in a group, IE decreases due to the increase in the atomic size of the succeeding members. This results in the lesser attraction of electrons and hence are easy to remove.

We are provided with the first four ionization energies of an element. These are 738 kJ/mol, 1450 kJ/mol, $7.7 \times {10^3}\;{\text{kJ/mol}}$ and $1.1 \times {10^4}\;{\text{kJ/mol}}$ respectively

The first ionization energy of an element is 738 kJ.mol and its second ionization energy is 1450 kJ/mol. There is small difference in the first and second ionization energies. But the value of third ionization energy is $7.7 \times {10^3}\;{\text{kJ/mol}}$. So when we go from second ionization energy to the third one, a large difference in the ionization energy of the element is observed. This indicates the removal of two electrons occurs with great ease but third electron is removed with high difficulty. So the element can easily lose two electrons and therefore it belongs to the 2nd group of the periodic table.

Learn more:

1. Rank the elements according to first ionization energy: brainly.com/question/1550767

2. Write the chemical equation for the first ionization energy of lithium: brainly.com/question/5880605

Answer details:

Grade: Senior School

Subject: Chemistry

Chapter: Periodic classification of elements

Keywords: ionization energy, isolated, neutral gaseous atom, valence electrons, successive ionization energy, IE, IE1, IE2, first ionization energy, second ionization energy, 2nd, group, period, periodic table, 738 kJ/mol, 1450 kJ/mol, 7.7*10^3 kJ/mol, 1.1*10^4 kJ/mol.