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The magnet in the following photo is made from neodymium, iron, and boron.
A magnet mode of on alloy containing the elements Nd, Fe, and B.
- (a) Write the electron configuration of each of these elements using an orbital box diagram and noble gas notation.
- (b) Are these elements paramagnetic or diamagnetic?
- (c) Write the electron configurations of Nd3+ and Fe3+ using orbital box diagrams and noble gas notation. Are these ions paramagnetic or diamagnetic?
a)
![Check Mark](/static/check-mark.png)
Interpretation:
The electron configuration of Neodymium, iron, and boron has to be written using orbital box diagram.
Concept Introduction:
Electronic configuration: The electronic configuration is the distribution of electrons (e-) of an given molecule or respective atoms in atomic or molecular orbital’s.
Aufbau principle: This rule statues that ground state of an atom or ions electrons fill atomic orbitals of the lowest available energy levels before occupying higher levels. If consider the 1s shell is filled the 2s subshell is occupied.
Hund's Rule: The every orbital in a subshell is singly occupied with one electron before any one orbital is doubly occupied, and all electrons in singly occupied orbitals have the same spin.
Pauli exclusion rule: an atomic orbital may describe at most two electrons, each with opposite spin direction.
Paramagnetic: The Paramagnetic properties are due to the presence of some unpaired electrons, and from the realignment of the electron paths caused by the external magnetic field.
Diamagnetic properties: In diamagnetic materials all the electron are paired so there is no permanent net magnetic moment per atom.
Answer to Problem 49GQ
Statement (a): The atomic number of Neodymium (Nd) (Z=60) electronic configuration of Neodymium (Nd)=
The electronic configuration of Iron (Fe) =
The electronic configuration of Boron (B) =
Statement (b): The all elements (
Statement (c): The orbital notation of Neodymium (Nd3+) ions=
To determine: The orbital notation method, noble gas configuration methods and Magnetic property should be explained given the different type of Neodymium (Nd), Iron (Fe) and Boron (B) element and its (Nd3+, Fe3+) ions.
Explanation of Solution
The electron configuration of Neodymium (Nd) element:
The orbital box diagram as follows,
Hence, the Noble gas configuration of
The electron configuration of Iron (Fe):
The orbital box diagram as follows,
Hence, the Noble gas configuration of
The electron configuration of Boron (B):
The orbital box diagram as follows,
Hence, the Noble gas configuration of
b)
![Check Mark](/static/check-mark.png)
Interpretation:
The magnetic property for the elements neodymium, iron, and Boron has to be predicted.
Concept Introduction:
Electronic configuration: The electronic configuration is the distribution of electrons (e-) of an given molecule or respective atoms in atomic or molecular orbital’s.
Aufbau principle: This rule statues that ground state of an atom or ions electrons fill atomic orbitals of the lowest available energy levels before occupying higher levels. If consider the 1s shell is filled the 2s subshell is occupied.
Hund's Rule: The every orbital in a subshell is singly occupied with one electron before any one orbital is doubly occupied, and all electrons in singly occupied orbitals have the same spin.
Pauli exclusion rule: an atomic orbital may describe at most two electrons, each with opposite spin direction.
Paramagnetic: The Paramagnetic properties are due to the presence of some unpaired electrons, and from the realignment of the electron paths caused by the external magnetic field.
Diamagnetic properties: In diamagnetic materials all the electron are paired so there is no permanent net magnetic moment per atom.
Explanation of Solution
Analyzing for Magnetic properties:
The given Neodymium (Nd), Iron (Fe) and Boron (B) elements shows good paramagnetic character, because unpaired electrons are present.
The Iron (Fe) system is we discussed below,
It has four unpaired electrons which show paramagnetic property.
The Boron (B) system is we discussed below,
It has one unpaired electrons which shows paramagnetic property.
c)
![Check Mark](/static/check-mark.png)
Interpretation:
The electron configuration of Nd3+ and Fe3+ using orbital box diagram and its paramagnetic property has to be predicted.
Concept Introduction:
Electronic configuration: The electronic configuration is the distribution of electrons (e-) of an given molecule or respective atoms in atomic or molecular orbital’s.
Aufbau principle: This rule statues that ground state of an atom or ions electrons fill atomic orbitals of the lowest available energy levels before occupying higher levels. If consider the 1s shell is filled the 2s subshell is occupied.
Hund's Rule: The every orbital in a subshell is singly occupied with one electron before any one orbital is doubly occupied, and all electrons in singly occupied orbitals have the same spin.
Pauli exclusion rule: an atomic orbital may describe at most two electrons, each with opposite spin direction.
Paramagnetic: The Paramagnetic properties are due to the presence of some unpaired electrons, and from the realignment of the electron paths caused by the external magnetic field.
Diamagnetic properties: In diamagnetic materials all the electron are paired so there is no permanent net magnetic moment per atom.
Explanation of Solution
Electronic configuration of Neodymium (Nd3+) system
The Neodymium (Nd) was oxidized to Neodymium (Nd3+) ions, it lost for three electrons in outermost (4f and 6s) shells. Than this orbital filling method are shown below.
Electronic configuration of Iron (Fe3+) system
The Iron (Fe) was oxidized to Iron (Fe3+) ions, it lost for three electrons in outermost (4f and 6s) shells. Than this orbital filling method are shown below.
Analyzing for Magnetic properties for (Nd3+) and (Fe3+) systems:
The given Statement (c) Neodymium (Nd3+)and Iron (Fe3+) elements are very good paramagnetic character, because all electrons in unpaired only see the above orbital notation method. Than the both system electron filling method are shown below.
The Iron (Fe3+) system is we discussed below,
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