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Questions and Answers
What is the reason for transition elements exhibiting less electro positivity than the s-block elements?
What is the reason for transition elements exhibiting less electro positivity than the s-block elements?
- High ionization energy due to large size
- High ionization energy due to small size (correct)
- Low ionization energy due to small size
- Low ionization energy due to large size
Why do the d-block elements exhibit an increase in ionization potentials from left to right?
Why do the d-block elements exhibit an increase in ionization potentials from left to right?
- Increase in the size of the (n-1) d subshell
- Decrease in the screening effect of new electrons
- Decrease in the number of electrons in the (n-1) d subshell
- Screening effect of new electrons in the (n-1) d subshell (correct)
What happens to the second ionization energies of the first transition series with the increase in atomic number?
What happens to the second ionization energies of the first transition series with the increase in atomic number?
- They fluctuate due to stable electronic configuration
- They remain constant due to stable electronic configuration
- They increase due to stable electronic configuration (correct)
- They decrease due to stable electronic configuration
What trend is observed for ionization energy across a period?
What trend is observed for ionization energy across a period?
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Study Notes
Transition Elements vs. S-Block Elements
- Transition elements exhibit less electro positivity than s-block elements because the outermost d-subshell in transition elements shields the nuclear charge less effectively, resulting in a lower electro positive character.
Ionization Potentials in D-Block Elements
- The d-block elements exhibit an increase in ionization potentials from left to right due to the increase in nuclear charge, which leads to a stronger attraction between the nucleus and the electrons, making it more difficult to remove an electron.
Second Ionization Energies in the First Transition Series
- The second ionization energies of the first transition series increase with the increase in atomic number, as the nuclear charge increases, resulting in a stronger attraction between the nucleus and the electrons, making it more difficult to remove a second electron.
Ionization Energy Across a Period
- The ionization energy increases across a period due to the increasing nuclear charge and the decreasing atomic radius, resulting in a stronger attraction between the nucleus and the electrons, making it more difficult to remove an electron.
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Description
Test your knowledge of transition elements and their properties with this quiz. Explore topics such as ionization energy, covalent compounds, and electro positivity in d-block elements.
