Electronic Configuration of d-Block Elements

Match the following:

$\begin{array}{cccc}\left(\mathrm{a}\right)& {\mathrm{Cr}}^{3+}& \left(\mathrm{i}\right)& \left[\mathrm{Ar}\right]3{\mathrm{d}}^{10}\\ \left(\mathrm{b}\right)& {\mathrm{Cu}}^{+}& \left(\mathrm{ii}\right)& \left[\mathrm{Xe}\right]4{\mathrm{f}}^4\\ \left(\mathrm{c}\right)& {\mathrm{Co}}^{2+}& \left(\mathrm{iii}\right)& \left[\mathrm{Ar}\right]3{\mathrm{d}}^5\\ \left(\mathrm{d}\right)& {\mathrm{Mn}}^{2+}& \left(\mathrm{iv}\right)& \left[\mathrm{Ar}\right]3{\mathrm{d}}^7\\ \left(\mathrm{e}\right)& {\mathrm{Pm}}^{3+}& \left(\mathrm{v}\right)& \left[\mathrm{Ar}\right]3{\mathrm{d}}^3\end{array}$

Zinc has completely filled $\mathrm{d}$ orbital in its oxidation state, copper also has completely filled electrons in its oxidation state but why only zinc is considered as non transition metal.

Identify a coinage metal.

Define coinage metals.

Identify the value of $\mathrm{k}$ in the electronic configuration of chromium, $\left[\mathrm{Ar}\right]3{\mathrm{d}}^5$_____ from the given options:
(A) $4{\mathrm{s}}^1$
(B) $4{\mathrm{s}}^2$
(C) $4{\mathrm{s}}^3$

Enter your correct answer as A, B or C.

Which of the following $3\mathrm{d}$ series elements having correct electronic configuration:

Which of the following elements belongs to $3\mathrm{d}$ series:

Which element doesnot belong to transition metal.

The general electronic configuration of transition element is

Why does copper show abnormal electronic configuration?

Why chromium has electronic configuration $3{\mathrm{d}}^5 4{\mathrm{s}}^1$ and not $3{\mathrm{d}}^{4 }4{\mathrm{s}}^2$?

Why is manganese more stable in the $+2$ state than the $+3$ state and the reverse is true for iron?

Why do the transition elements show variable oxidation states?

Explain why any metal shows the highest oxidation state only in oxides and fluorides?

Explain why $\mathrm{Zn}$ is not considered as transition element?

From the following, the correct statement is/are?
a. Oxidation potential $\left(\mathrm{M}/{\mathrm{M}}^{2+}\right)$ of $\mathrm{Cu}$ is least in $3\mathrm{d}$ series.
b. ${\mathrm{Fe}}^{3+}$ is more stable than ${\mathrm{Mn}}^{3+}$ in aqeous solution.
c. Exchange energy is more in case of ${\mathrm{Fe}}^{3+}$ than ${\mathrm{Mn}}^{3+}$.
d. First IE of Mn is more than that of Fe.

The melting point of copper is higher than that of zinc because:

The group of the element in periodic table having electronic configuration  $\left[\mathrm{A}\mathrm{r}\right]3{\mathrm{d}}^6\mathrm{ }4{\mathrm{s}}^2$ is-

Group of Coinage metals is-

Which of the following compounds is colored and paramagnetic?