Electronic Configuration of D Block Elements

Match the following:

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

Why Cu and Cr have exceptional electronic configuration?

Predict the position of the element in the periodic table satisfying the outer electronic configuration, $\left(\mathrm{n}-1\right){\mathrm{d}}^1 {\mathrm{ns}}^2$ for $\mathrm{n}=4$.

Explain why transition elements have many irregularities in their electronic configuration.

General electronic configuration of d-block elements is

Account for the following:

$\mathrm{Ti}\left(\mathrm{IV}\right)$ is more stable than the $\mathrm{Ti}\left(\mathrm{II}\right)$ or $\mathrm{Ti}\left(\mathrm{III}\right)$.

Transition metal elements exhibit general electronic configuration________

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.

Among the following series of transition metal ions, the one in which all the metal ions have $3{\mathrm{d}}^2 3{\mathrm{p}}^6$ electronic configuration is

(Atomic number of $\mathrm{Ti}=22, \mathrm{V}=23, \mathrm{Cr}=24, \mathrm{Mn}=25$)

The correct statements(s) about ${\mathrm{Cr}}^{2+}$and ${\mathrm{Mn}}^{3+}$ is (are)

Which of the following ions have the same numbers of unpaired electrons?

Write down electronic configuration of chromium $(\mathrm{Z}=24)$ and indicate in it.
($i$) number of sub-shells
($ii$) number of orbitals
($iii$) number of electrons in $\mathrm{M}$-shell

Write down electronic configuration of ${\mathrm{Fe}}^{3+}$ ion and answer the following:
($i$) What is the number of electrons having $n+\ell =3$ in it?
($ii$) How many electrons in it have $\mathrm{n}=3$ and $m=0 ?$
($iii$) How many electrons in it have $\ell =1$ ?
($iv$) What is the number of electrons in $\mathrm{M}$-shell?

Strongest reducing ion 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?

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 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-

Which of the following compounds is colored and paramagnetic?