Chapter 8, Problem 8.97P

Interpretation Introduction

Interpretation:

The ions from ${\text{Fe}}^{+}$ to ${\text{Fe}}^{14+}$ that are paramagnetic is to be determined. Also the ion that is most strongly attracted to a magnetic field is to be stated.

Concept introduction:

Paramagnetism is a form of magnetism where the materials are weakly attracted by an externally applied magnetic field. It is due to the presence of unpaired electrons in the materials so all the atoms with incompletely filled atomic orbital are paramagnetic.

The intensity of paramagnetism increases with the increase in the number of unpaired electrons. Due to their spin, the unpaired electrons have a magnetic dipole moment and act like tiny magnets.

Answer to Problem 8.97P

${\text{Fe}}^{+}$, ${\text{Fe}}^{2+}$, ${\text{Fe}}^{3+}$, ${\text{Fe}}^{4+}$, ${\text{Fe}}^{5+}$, ${\text{Fe}}^{6+}$, ${\text{Fe}}^{7+}$, ${\text{Fe}}^{9+}$, ${\text{Fe}}^{10+}$, ${\text{Fe}}^{11+}$, ${\text{Fe}}^{12+}$, ${\text{Fe}}^{13+}$ are paramagnetic. ${\text{Fe}}^{+}$ and ${\text{Fe}}^{3+}$ would be most strongly attracted to a magnetic field.

Explanation of Solution

The paramagnetic nature of the ions of iron can be determined by the presence of unpaired electrons. The atomic number of iron is 26 so its condensed electronic configuration is $\left[\text{Ar}\right]4s^{2}3d^6$.

The condensed electronic configuration of ${\text{Fe}}^{+}$ is as follows,

${\text{Fe}}^{+}\to \left[\text{Ar}\right]4s^{1}3d^6$

Its partial orbital diagram is as follows:

The condensed electronic configuration of ${\text{Fe}}^{2+}$ is as follows,

${\text{Fe}}^{2+}\to \left[\text{Ar}\right]3d^6$

Its partial orbital diagram is as follows:

The condensed electronic configuration of ${\text{Fe}}^{3+}$ is as follows,

${\text{Fe}}^{3+}\to \left[\text{Ar}\right]3d^5$

Its partial orbital diagram is as follows:

The condensed electronic configuration of ${\text{Fe}}^{4+}$ is as follows,

${\text{Fe}}^{4+}\to \left[\text{Ar}\right]3d^4$

Its partial orbital diagram is as follows:

The condensed electronic configuration of ${\text{Fe}}^{5+}$ is as follows,

${\text{Fe}}^{5+}\to \left[\text{Ar}\right]3d^3$

Its partial orbital diagram is as follows:

The condensed electronic configuration of ${\text{Fe}}^{6+}$ is as follows,

${\text{Fe}}^{6+}\to \left[\text{Ar}\right]3d^2$

Its partial orbital diagram is as follows:

The condensed electronic configuration of ${\text{Fe}}^{7+}$ is as follows,

${\text{Fe}}^{7+}\to \left[\text{Ar}\right]3d^1$

Its partial orbital diagram is as follows:

The condensed electronic configuration of ${\text{Fe}}^{8+}$ is as follows,

${\text{Fe}}^{8+}\to \left[\text{Ar}\right]$

Its partial orbital diagram is as follows:

The condensed electronic configuration of ${\text{Fe}}^{9+}$ is as follows,

${\text{Fe}}^{9+}\to \left[\text{Ne}\right]3s^{2}3p^5$

Its partial orbital diagram is as follows:

The condensed electronic configuration of ${\text{Fe}}^{10+}$ is as follows,

${\text{Fe}}^{10+}\to \left[\text{Ne}\right]3s^{2}3p^4$

Its partial orbital diagram is as follows:

The condensed electronic configuration of ${\text{Fe}}^{11+}$ is as follows,

${\text{Fe}}^{11+}\to \left[\text{Ne}\right]3s^{2}3p^3$

Its partial orbital diagram is as follows:

The condensed electronic configuration of ${\text{Fe}}^{12+}$ is as follows,

${\text{Fe}}^{12+}\to \left[\text{Ne}\right]3s^{2}3p^2$

Its partial orbital diagram is as follows:

The condensed electronic configuration of ${\text{Fe}}^{13+}$ is as follows,

${\text{Fe}}^{13+}\to \left[\text{Ne}\right]3s^{2}3p^1$

Its partial orbital diagram is as follows:

The condensed electronic configuration of ${\text{Fe}}^{14+}$ is as follows,

${\text{Fe}}^{14+}\to \left[\text{Ne}\right]3s^2$

Its partial orbital diagram is as follows:

${\text{Fe}}^{+}$, ${\text{Fe}}^{2+}$, ${\text{Fe}}^{3+}$, ${\text{Fe}}^{4+}$, ${\text{Fe}}^{5+}$, ${\text{Fe}}^{6+}$, ${\text{Fe}}^{7+}$, ${\text{Fe}}^{9+}$, ${\text{Fe}}^{10+}$, ${\text{Fe}}^{11+}$, ${\text{Fe}}^{12+}$, ${\text{Fe}}^{13+}$ are paramagnetic due to the presence of unpaired electrons. ${\text{Fe}}^{+}$ and ${\text{Fe}}^{3+}$ would be most strongly attracted to a magnetic field because they have 5 unpaired electrons which is the maximum among all the ions from ${\text{Fe}}^{+}$ to ${\text{Fe}}^{14+}$.

Conclusion

${\text{Fe}}^{+}$, ${\text{Fe}}^{2+}$, ${\text{Fe}}^{3+}$, ${\text{Fe}}^{4+}$, ${\text{Fe}}^{5+}$, ${\text{Fe}}^{6+}$, ${\text{Fe}}^{7+}$, ${\text{Fe}}^{9+}$, ${\text{Fe}}^{10+}$, ${\text{Fe}}^{11+}$, ${\text{Fe}}^{12+}$, ${\text{Fe}}^{13+}$ are paramagnetic. ${\text{Fe}}^{+}$ and ${\text{Fe}}^{3+}$ would be most strongly attracted to a magnetic field.