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A2.4 Magnetic Properties of Metal Compounds

Paramagnetism: is a property of a substance which has unpaired electrons in its atomic structure allowing  it to be drawn into a magnetic field.
Diamagnetism: is a property of a substance with paired electrons. It will be repelled by a magnetic field. This is a much weaker effect than paramagnetism therefore  paramagnetism will always dominate.
d-block elements (transition metals) exhibit paramagnetism most strongly because their ions often have several unpaired electrons.

 Consider the  Fe2+\textsf{Fe}^\textsf{2+}Fe2+
, Mn2+\textsf{Mn}^\textsf{2+}Mn2+
 and Cu+\textsf{Cu}^\textsf{+}Cu+
 ions
​
Mn 2+^{\textsf2+}2+
 
Fe 3+^{\textsf3+}3+
 
Cu +^{+}+
 
Electronic configuration
All are 1s22s22p63s23p6\textsf{1s}^\textsf{2}\textsf{2s}^\textsf{2}\textsf{2p}^\textsf{6}\textsf{3s}^\textsf{2}\textsf{3p}^\textsf{6}1s22s22p63s23p6
 
 3d5\textsf{3d}^\textsf{5}3d5
 
​3d4\textsf{3d}^\textsf{4}3d4
 
​3d10\textsf{3d}^\textsf{10}3d10
 
in the d orbitals
5 unpaired
electrons
3 unpaired electrons
0 unpaired electrons
Magnetic property
Paramagnetic
Less Paramagnetic
Diamagnetic
The magnetic behaviour of the metals themselves requires a much more complicated explanation.

A2.3 Alloys

A2.5 Inductively Coupled Plasma Detection

Last modified 2yr ago

	Mn $^{\textsf2+}$	Fe $^{\textsf3+}$	Cu $^{+}$
Electronic configuration All are $\textsf{1s}^\textsf{2}\textsf{2s}^\textsf{2}\textsf{2p}^\textsf{6}\textsf{3s}^\textsf{2}\textsf{3p}^\textsf{6}$	$\textsf{3d}^\textsf{5}$	$\textsf{3d}^\textsf{4}$	$\textsf{3d}^\textsf{10}$
in the d orbitals	5 unpaired electrons	3 unpaired electrons	0 unpaired electrons
Magnetic property	Paramagnetic	Less Paramagnetic	Diamagnetic