Ionic Radius & its Trends
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Ionic radius is calculated by measuring the distance between two ion nuclei according to their sizes. Cations have a smaller radius than their parent atoms due to electron loss increasing the effective nuclear charge. Anions have a larger radius than their parent atoms due to electron gain decreasing the effective nuclear charge. Ionic radius decreases across a period as proton number and effective nuclear charge increase, making the nucleus attract electrons more strongly. Ionic radius increases down a group as the energy level and shielding effect increase, weakening nuclear attraction.
Ionic Radius & its Trends
- 1. Submitted by:- Haseeb Shafqat Chem18111127(6B) Submitted to:- DR Sumreen ASIM TOPIC:- IONIC RADIUS
- 2. Ionic Radius Ionic radius is calculated by dividing the distance b/w two nuclei of two ions according to their sizes.
- 3. Cation:-by loss of electron Cation<parents atom? formation of effective nuclear charges increases sometime a shell may also decrease Anion:- by gain of electron anions>parents atom? formation of effective nuclear charges decreases.
- 7. Trends in periodic table Decrease across a period • Proton number increases • Effective nuclear charge increases • Stronger attraction between nucleus and valence electron • Thus, atomic radius decreases Increases down a group • Energy level increases • Shielding effect increases • Weaker attraction between nucleus and valence electrons • Thus, atomic radius increases.
- 8. Ionic Radius in a Period • Ionic Radius tends to decrease in size across the Periodic Table
- 9. Ionic Radius in a Group • Ionic Radius tends to increase down a Group
- 11. Summary Diagram
- 12. Question 1 • Which of the following is the smallest in size? • 1) N3- • 2) O2- • 3) F- • 4) Na+
- 13. Thank you