Trend in first ionization energy using third period of periodic table has to be explained. Concept Introduction: An atom can be converted into an ion by removing an electron from its outermost shell or adding electron to the outermost shell. An amount of energy is required to remove an electron from the outermost shell of an atom to form a cation. The minimum energy required for removing an electron from an atom in gaseous phase is known as ionization energy . If one electron is removed from the atom to form a cation, the energy required is known as first ionization energy . If another electron is removed from the formed ion, the energy required is known as second ionization energy and this goes on. Second ionization energy is higher than the first ionization energy because the effective nuclear charge increases. The trend followed in a periodic table for ionization energy is, it increases across the period and decreases down the group. This is because; across the period, the electrons are added to the same orbital and hence decrease in shielding. However, down the group, the electrons are added to a new sub-shell and hence increase in shielding. To explain the trend in first ionization energy

Question

Want to see the full answer?

Answer 1

Question

Chapter 4, Problem 4.52QP

Interpretation Introduction

Interpretation: Trend in first ionization energy using third period of periodic table has to be explained.

Concept Introduction:

An atom can be converted into an ion by removing an electron from its outermost shell or adding electron to the outermost shell. An amount of energy is required to remove an electron from the outermost shell of an atom to form a cation. The minimum energy required for removing an electron from an atom in gaseous phase is known as ionization energy.

If one electron is removed from the atom to form a cation, the energy required is known as first ionization energy. If another electron is removed from the formed ion, the energy required is known as second ionization energy and this goes on. Second ionization energy is higher than the first ionization energy because the effective nuclear charge increases.

The trend followed in a periodic table for ionization energy is, it increases across the period and decreases down the group. This is because; across the period, the electrons are added to the same orbital and hence decrease in shielding. However, down the group, the electrons are added to a new sub-shell and hence increase in shielding.

To explain the trend in first ionization energy

Expert Solution & Answer

Want to see the full answer?

Check out a sample textbook solution

See solution

Students have asked these similar questions

Elements on the left side of the periodic table are more likely to form positive ions than those on the right. Use the trend in the ionization energy of the elements to explain this observation.

Consider Si, S, and P.1) Based purely on ideas of electron screening and effective nuclear charge, which of these elements do you expect to have the highest first ionization energy?2) Based on experimental data, P has the highest first ionization energy. Explain this observation in terms of electron configuration arguments.

11. The first five ionization energies of an element in period 3 is shown in the graph below. Predict the element and explain why there is a large jump in energy between the 3rd and 4th ionization. Your explanation should reference the attractive forces within an atom and include an energy orbital diagram. IE5 IE4 IE3 IE, IE, Energy (kJ/mol)