Identify the general electronic configuration | vedclass

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(B) $1$. The $2^{nd}$ transition series corresponds to the $4d$ series, which starts from Yttrium $(Z=39)$ and ends at Cadmium $(Z=48)$.$2$. These ele

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$[Kr] 4d^{1-10} 5s^{0-2}$

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(B) $1$. The $2^{nd}$ transition series corresponds to the $4d$ series, which starts from Yttrium $(Z=39)$ and ends at Cadmium $(Z=48)$.$2$. These elements follow the noble gas core of Krypton ($[Kr]$, $Z=36$).$3$. The general valence shell electronic configuration for the $d$-block elements is $(n-1)d^{1-10} ns^{1-2}$.$4$. For the $2^{nd}$ transition series, $n=5$. Therefore, the configuration is $[Kr] 4d^{1-10} 5s^{0-2}$ (where $5s$ can have $0, 1,$ or $2$ electrons depending on the element, such as $Pd$ which is $4d^{10} 5s^0$).

$I. \ Zn^{2+}$	$(i) \ d^8 \ \text{configuration}$
$II. \ Cu^{2+}$	$(ii) \ \text{Colourless}$
$III. \ Ni^{2+}$	$(iii) \ \mu = 1.73 \ \text{BM}$

Identify the general electronic configuration exhibited by the $2^{nd}$ series of transition elements.

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Match the following:
$I. \ Zn^{2+}$ $(i) \ d^8 \ \text{configuration}$
$II. \ Cu^{2+}$ $(ii) \ \text{Colourless}$
$III. \ Ni^{2+}$ $(iii) \ \mu = 1.73 \ \text{BM}$

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