Question

the decrease in atomic size is not much prominent across rows containing elements of s block p block dblock fblock​

Answer 1

Answer:

Because of this, 85% of the attraction force produced by z* is counterbalanced by interelectronic repulsion therefore only 0.15 more z* decreases in size which is very small so almost equal size and no significant decrease in size treds in priods of the d block.

Answer 2

Answer:

Along the d block, the decrease in atomic size is not much prominent across rows.

Explanation:

• The decrease is not much prominent because the effect of increased nuclear charge is cancelled by Shielding effect.
• Shielding effect - Due to a variation in the attraction forces acting on the atom's electrons, the shielding effect is characterised as a reduction in the effective nuclear charge on the electron cloud.
• Atomic radii of the first transition series grow from Cu to Zn after decreasing from Sc to Cr, where they thereafter nearly remain constant.
• The increase in nuclear charge at the start of the series has been suggested as the cause of this variance in atomic radii.
• However, as the d-orbitals fill up, the electrons shield the outer 4s electrons from the effects of nuclear charge. The atomic radii become nearly constant in the middle of transition series when the increasing nuclear charge and the increased screening effect balance each other out (Mn to Fe).
• The series ends with a strong emphasis on the repulsive interaction between electrons in orbitals. a result of which the electron cloud is expanding.

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