Question

Answer the following questions based on the given electron configurations, and identify the elements.

1. Arrange these atoms in order of increasing size:

$\left[\mathrm{Kr}\right]\mathbf{5}{\mathit{s}}^{\mathbf{2}}\mathbf{4}{\mathit{d}}^{\mathbf{10}}\mathbf{5}{\mathit{p}}^{\mathbf{6}}\mathbf{;}\mathbf{}\left[\mathrm{Kr}\right]\mathbf{5}{\mathit{s}}^{\mathbf{2}}\mathbf{4}{\mathit{d}}^{\mathbf{10}}\mathbf{5}{\mathit{p}}^{\mathbf{1}}\mathbf{;}\mathbf{}\left[\mathrm{Kr}\right]\mathbf{5}{\mathit{s}}^{\mathbf{2}}\mathbf{4}{\mathit{d}}^{\mathbf{10}}\mathbf{5}{\mathit{p}}^{\mathbf{3}}\mathbf{;}\mathbf{}\mathbf{}$

1. Arrange these atoms in order of decreasing the first ionization energy: $\left[\mathrm{Ne}\right]\mathbf{3}{\mathit{s}}^{\mathbf{2}}\mathbf{3}{\mathit{p}}^{\mathbf{5}}\mathbf{;}\mathbf{}\left[\mathit{A}\mathit{r}\right]\mathbf{4}{\mathit{s}}^{\mathbf{2}}\mathbf{3}{\mathbf{d}}^{\mathbf{10}}\mathbf{4}{\mathbf{p}}^{\mathbf{3}}\mathbf{;}\mathbf{}\mathbf{}\left[\mathit{A}\mathit{r}\right]\mathbf{3}{\mathit{s}}^{\mathbf{2}}\mathbf{3}{\mathbf{d}}^{\mathbf{10}}\mathbf{4}{\mathbf{p}}^{\mathbf{5}}$

Short answer

1. In a periodic table, the nuclear size of atoms diminishes from left to right and increments moving down.

$\mathrm{Xe}<\mathrm{Sb}<\mathrm{In}$

1. In a periodic table, the first ionization energy of molecules diminishes moving down in the groups and increments from left to right across the period.

$\mathrm{Cl}>\mathrm{Br}>\mathrm{As}$

Step-by-step solution

Determine the order of atoms in increasing size.

Identifying the elements:

The electron configuration$\left[\mathrm{Kr}\right]5s^{2}4d^{10}5p^6$ resembles with the atom $\mathrm{Xe}$.

The electron configuration $\left[\mathrm{Kr}\right]5s^{2}4d^{10}5p^1$resembles with the atom $\mathrm{In}$.

The electron configuration $\left[\mathrm{Kr}\right]5s^{2}4d^{10}5p^3$resembles with the atom $\mathrm{Sb}$.

Since thenuclear size diminishes along the period from left to right.So, the order of the particles in expanding size:$\mathrm{Xe}<\mathrm{Sb}<\mathrm{In}$

Determine the order of atoms in decreasing the first ionization energy.

Identifying the elements:

The electron configuration$\left[\mathrm{Ne}\right]3s^{2}3p^5$resembles with the atom $\mathrm{Cl}$.

The electron configuration $\left[\mathrm{Ar}\right]4s^{2}3d^{10}4p^3$ resembles with the atom $\mathrm{As}$.

The electron configuration $\left[\mathrm{Ar}\right]3s^{2}3{\mathrm{d}}^{10}4{\mathrm{p}}^5$resembles with the atom $\mathrm{Br}$.

As the first ionization energy increments across the period from left to right and diminishes in the down of a group.The order of atoms in diminishing first ionization energy: $\mathrm{Cl}>\mathrm{Br}>\mathrm{As}$.

Therefore, $\left[\mathrm{Kr}\right]5s^{2}4d^{10}5p^6;\left[\mathrm{Kr}\right]5s^{2}4d^{10}5p^1;\left[\mathrm{Kr}\right]5s^{2}4d^{10}5p^3;$and in order of increasing size:

$\left[\mathrm{Kr}\right]5s^{2}4d^{10}5p^6\mathit{<}\left[\mathrm{Kr}\right]5s^{2}4d^{10}5p^3\mathit{<}\left[\mathrm{Kr}\right]5s^{2}4d^{10}5p^1$or$\mathrm{Xe}<\mathrm{Sb}<\mathrm{In}$

And , $\left[\mathrm{Ne}\right]3s^{2}3p^5;\left[\mathrm{Ar}\right]4s^{2}3{\mathrm{d}}^{10}4{\mathrm{p}}^3;\mathrm{and}\left[\mathrm{Ar}\right]3s^{2}3{\mathrm{d}}^{10}4{\mathrm{p}}^5$and in order of decreasing first ionization energy:

$\left[\mathrm{Ne}\right]3s^{2}3p^5\mathit{>}\left[\mathrm{Ar}\right]4s^{2}3{\mathrm{d}}^{10}4{\mathrm{p}}^3>\left[\mathrm{Ar}\right]3s^{2}3{\mathrm{d}}^{10}4{\mathrm{p}}^5$or$\mathrm{Cl}>\mathrm{Br}>\mathrm{As}$