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Trends in Stability of Higher Oxidation States of Transition Elements Video Lecture - JEE
FAQs on Trends in Stability of Higher Oxidation States of Transition Elements Video Lecture - JEE
| 1. What are the trends in the stability of higher oxidation states of transition elements? |  |
Ans. The stability of higher oxidation states of transition elements generally increases across a period and decreases down a group in the periodic table. This trend can be attributed to factors such as effective nuclear charge, atomic size, and the presence of d-electrons.
| 2. How does effective nuclear charge affect the stability of higher oxidation states of transition elements? | |
Ans. Effective nuclear charge refers to the net positive charge experienced by the outermost electrons in an atom, taking into account the shielding effect of inner electrons. Higher effective nuclear charge increases the attraction between the nucleus and the outer electrons, making it harder to remove them and stabilize higher oxidation states.
| 3. Why does the stability of higher oxidation states decrease down a group in the periodic table? | |
Ans. Down a group, the atomic size of transition elements increases, resulting in an increase in the distance between the nucleus and the outermost electrons. As a result, the effective nuclear charge experienced by the outer electrons decreases, making it easier to remove them and destabilizing higher oxidation states.
| 4. How do the presence of d-electrons influence the stability of higher oxidation states? | |
Ans. The presence of d-electrons in transition elements allows for the formation of multiple oxidation states. However, as the number of d-electrons increases, the stability of higher oxidation states decreases. This is because the repulsion between the electrons in the same d-orbital makes it energetically unfavorable to promote electrons to higher energy levels.
| 5. Can you provide an example of the trend in stability of higher oxidation states of transition elements? | |
Ans. Sure! Let's take the example of manganese (Mn) and iron (Fe). Manganese exhibits higher oxidation states such as +4 and +7, while iron primarily shows oxidation states of +2 and +3. This is due to the larger effective nuclear charge and smaller atomic size of manganese, which stabilize higher oxidation states compared to iron.
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