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Trends in Periodic Table: Effective Nuclear Charge & Nuclear Radius Video Lecture | Chemistry for JEE Main & Advanced
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FAQs on Trends in Periodic Table: Effective Nuclear Charge & Nuclear Radius Video Lecture - Chemistry for JEE Main & Advanced
| 1. How does effective nuclear charge affect the periodic trends in the periodic table? |  |
Ans. The effective nuclear charge is the net positive charge experienced by an electron in an atom after taking into account the shielding effect of other electrons. It plays a crucial role in determining the atomic size, ionization energy, and electron affinity of elements in the periodic table. As the effective nuclear charge increases across a period, the atomic size decreases, and the ionization energy increases.
| 2. How is nuclear radius related to the trends in the periodic table? | |
Ans. Nuclear radius is the size of the nucleus of an atom, which affects the overall size of the atom. In general, as you move down a group in the periodic table, the nuclear radius increases due to the addition of more energy levels. However, across a period, the nuclear radius remains relatively constant while the atomic size decreases due to the increasing effective nuclear charge.
| 3. How does the effective nuclear charge impact the chemical reactivity of elements in the periodic table? | |
Ans. The effective nuclear charge influences the ability of an atom to attract and hold onto electrons, which in turn affects its chemical reactivity. Elements with higher effective nuclear charges tend to have higher ionization energies and electron affinities, making them less reactive. On the other hand, elements with lower effective nuclear charges are more likely to lose or gain electrons, leading to higher reactivity.
| 4. How do the trends in effective nuclear charge and nuclear radius explain the periodic behavior of elements in terms of their properties? | |
Ans. The trends in effective nuclear charge and nuclear radius help explain the periodic behavior of elements in terms of their properties. For example, elements with higher effective nuclear charges tend to have higher melting and boiling points, as well as higher ionization energies, while elements with larger nuclear radii are more likely to form ionic compounds due to their lower ionization energies.
| 5. How do changes in the nuclear charge and radius affect the size of ions in the periodic table? | |
Ans. Changes in the nuclear charge and radius directly impact the size of ions in the periodic table. As the effective nuclear charge increases, cations (positively charged ions) tend to be smaller than their parent atoms, while anions (negatively charged ions) tend to be larger due to the addition of extra electrons. The nuclear radius plays a key role in determining the overall size of ions in compounds.
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Dec 18, 2024 Last updated |
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