By means of orbital diagrams, write electron configurations for the following
(a)
Interpretation:
To write the electronic configuration of V by using orbital diagram.
Concept introduction:
Orbital Diagram: It is pictorial representation of electrons in any atom. It represents shell number “n”, subshell “l” as well as spin of electrons. The orbitals present in subshell are represented by lines or boxes. In one orbital there can be maximum 2 electrons.
Subshell | Number of orbitals | Number of maximum electrons |
s | 1 | 2 |
p | 3 | 6 |
d | 5 | 10 |
f | 7 | 14 |
The spin of electron is represented by arrows. The up arrow means 1/2 spin and down arrow means - 1/2 spin. There are some rules to fill electrons in these orbitals as:
- Aufbau Principle:
- Pauli’s Exclusion Principle:
It states that no two electron can have all the same quantum number, that’ why in an orbital, the spin or one electron is up and spin of second electrons is down.
- Hund’s Rule:
It states that each orbital in a subshell is single occupied with one electron before any one electron is occupied double and also the spin of all electrons
It states that the electron goes in orbital which has lowest energy.
The series of orbital from lowest to highest energy:
Electronic configuration:
It is notation which shows the distribution of electrons in orbitals of atoms, ion or molecule. The configuration lists the shell by principal quantum number, n= 1,2,3,4…. and subshell by azimuthal quantum number, l = s, p, d, f and electrons that can be present in it. With the help of orbital diagram electronic configuration can be written.
Answer to Problem 1E
The electronic configuration of V is
Explanation of Solution
The atomic number of Vanadium, V is 23. V is neutral atom, hence the total number of electrons = 23
According to Aufbau principle, the lowest energy orbital is 1s which can have maximum 2 electrons. Next is 2s which has 2 electrons. Similarly, 2p has 6 electrons, 3s has 2 electrons 3p can have 6 electrons, 4s has 2 electrons. So far, total electrons added to orbitals are 20 electrons out of 23. Next comes 3d, it can have 10 electrons maximum but V has only 3 electrons left, which goes in 3d. The orbital diagram of V is:
The electronic configuration of V is:
(b)
Interpretation:
To write the electronic configuration of
Concept introduction:
Orbital Diagram: It is pictorial representation of electrons in any atom. It represents shell number “n”, subshell “l” as well as spin of electrons. The orbitals present in subshell are represented by lines or boxes. In one orbital there can be maximum 2 electrons.
Subshell | Number of orbitals | Number of maximum electrons |
s | 1 | 2 |
p | 3 | 6 |
d | 5 | 10 |
f | 7 | 14 |
The spin of electron is represented by arrows. The up arrow means 1/2 spin and down arrow means - 1/2 spin. There are some rules to fill electrons in these orbitals as:
- Aufbau Principle:
It states that the electron goes in orbital which has lowest energy.
- Pauli’s Exclusion Principle:
It states that no two electron can have all the same quantum number, that’ why in an orbital, the spin or one electron is up and spin of second electrons is down.
- Hund’s Rule:
It states that each orbital in a subshell is single occupied with one electron before any one electron is occupied double and also the spin of all electrons.
The series of orbital from lowest to highest energy:
Electronic configuration:
It is notation which shows the distribution of electrons in orbitals of atoms, ion or molecule. The configuration lists the shell by principal quantum number, n= 1,2,3,4…. and subshell by azimuthal quantum number, l = s, p, d, f and electrons that can be present in it. With the help of orbital diagram electronic configuration can be written.
Answer to Problem 1E
The electronic configuration of Cr2+ is
Explanation of Solution
The atomic number of chromium ion, Cr is 24.
In the electronic configuration of Cr, there is an exception and the electronic configuration is written as:
Here, Cr has +2 charge on it, which means 2 electrons have been lost so total electrons present in Cr2+ is 24 − 2 = 22 electrons. The electrons start losing from outermost orbital.
Here, outermost orbital is 4s so it loses one electron and one from 3d.
The orbital diagram is:
The electronic configuration of Cr2+ is
Interpretation:
To write the electronic configuration of
Concept introduction:
Orbital Diagram: It is pictorial representation of electrons in any atom. It represents shell number “n”, subshell “l” as well as spin of electrons. The orbitals present in subshell are represented by lines or boxes. In one orbital there can be maximum 2 electrons.
Subshell | Number of orbitals | Number of maximum electrons |
s | 1 | 2 |
p | 3 | 6 |
d | 5 | 10 |
f | 7 | 14 |
The spin of electron is represented by arrows. The up arrow means 1/2 spin and down arrow means - 1/2 spin. There are some rules to fill electrons in these orbitals as:
- Aufbau Principle:
It states that the electron goes in orbital which has lowest energy.
- Pauli’s Exclusion Principle:
It states that no two electron can have all the same quantum number, that’ why in an orbital, the spin or one electron is up and spin of second electrons is down.
- Hund’s Rule:
It states that each orbital in a subshell is single occupied with one electron before any one electron is occupied double and also the spin of all electrons.
The series of orbital from lowest to highest energy:
Electronic configuration:
It is notation which shows the distribution of electrons in orbitals of atoms, ion or molecule. The configuration lists the shell by principal quantum number, n= 1,2,3,4…. and subshell by azimuthal quantum number, l = s, p, d, f and electrons that can be present in it. With the help of orbital diagram electronic configuration can be written.
Answer to Problem 1E
The electronic configuration of Mn2+ is
Explanation of Solution
The atomic number of Manganese, Mn is 25.
The electronic configuration of Mn is
Here, Mn shows charge of +2 means 2 electrons are lost from outermost orbital, 4d.
Hence, total electrons present in Mn2+ are 23.
The electronic configuration of Mn2+ is
(d)
Interpretation:
To write the electronic configuration of Fe2+ by using orbital diagram.
Concept introduction:
Orbital Diagram: It is pictorial representation of electrons in any atom. It represents shell number “n”, subshell “l” as well as spin of electrons. The orbitals present in subshell are represented by lines or boxes. In one orbital there can be maximum 2 electrons.
Subshell | Number of orbitals | Number of maximum electrons |
s | 1 | 2 |
p | 3 | 6 |
d | 5 | 10 |
f | 7 | 14 |
The spin of electron is represented by arrows. The up arrow means 1/2 spin and down arrow means - 1/2 spin. There are some rules to fill electrons in these orbitals as:
- Aufbau Principle:
It states that the electron goes in orbital which has lowest energy.
- Pauli’s Exclusion Principle:
It states that no two electron can have all the same quantum number, that’ why in an orbital, the spin or one electron is up and spin of second electrons is down.
- Hund’s Rule:
It states that each orbital in a subshell is single occupied with one electron before any one electron is occupied double and also the spin of all electrons.
The series of orbital from lowest to highest energy:
Electronic configuration:
It is notation which shows the distribution of electrons in orbitals of atoms, ion or molecule. The configuration lists the shell by principal quantum number, n= 1,2,3,4…. and subshell by azimuthal quantum number, l = s, p, d, f and electrons that can be present in it. With the help of orbital diagram electronic configuration can be written.
Answer to Problem 1E
The electronic configuration of Fe2+ is
Explanation of Solution
The atomic number of Iron, Fe is 26.
The electronic configuration of Fe is
Here, Fe shows charge of +2 means 2 electrons are lost from outermost orbital, 4d.
Hence, total electrons present in Fe2+ are 24.
The orbital diagram of Fe2+ is:
The electronic configuration of Fe2+ is
(e)
Interpretation:
To write the Electronic configuration of Cu2+ by using orbital diagram.
Concept introduction:
Orbital Diagram: It is pictorial representation of electrons in any atom. It represents shell number “n”, subshell “l” as well as spin of electrons. The orbitals present in subshell are represented by lines or boxes. In one orbital there can be maximum 2 electrons.
Subshell | Number of orbitals | Number of maximum electrons |
s | 1 | 2 |
p | 3 | 6 |
d | 5 | 10 |
f | 7 | 14 |
The spin of electron is represented by arrows. The up arrow means 1/2 spin and down arrow means - 1/2 spin. There are some rules to fill electrons in these orbitals as:
- Aufbau Principle:
It states that the electron goes in orbital which has lowest energy.
- Pauli’s Exclusion Principle:
It states that no two electron can have all the same quantum number, that’ why in an orbital, the spin or one electron is up and spin of second electrons is down.
- Hund’s Rule:
It states that each orbital in a subshell is single occupied with one electron before any one electron is occupied double and also the spin of all electrons.
The series of orbital from lowest to highest energy:
Electronic configuration:
It is notation which shows the distribution of electrons in orbitals of atoms, ion or molecule. The configuration lists the shell by principal quantum number, n= 1,2,3,4…. and subshell by azimuthal quantum number, l = s, p, d, f and electrons that can be present in it. With the help of orbital diagram electronic configuration can be written.
Answer to Problem 1E
The electronic configuration of Cu2+ is
Explanation of Solution
The atomic number of Copper, Cu is 29.
The electronic configuration of Cu is 1s2 2s2 2p6 3s2 3p6 4s1 3d10. Cu shows exception in configuration as 4s1 3d10 instead 4s2 3d9 because 10 electron in 3d orbital is stable configuration so out of 2 electrons, one electron from 4s jumps to 3d leaving 1 electron in 4s and 10 electron in 3d.
Here, Cu shows charge of +2 means 1 electron from outermost 4s and one electron from 3d are lost. Hence, total electrons present in Cu2+ are 27.
The orbital diagram of Cu2+ is:
The electronic configuration of Cu2+ is
(f)
Interpretation:
To write the electronic configuration of Ni2+ by using orbital diagram.
Concept introduction:
Orbital Diagram: It is pictorial representation of electrons in any atom. It represents shell number “n”, subshell “l” as well as spin of electrons. The orbitals present in subshell are represented by lines or boxes. In one orbital there can be maximum 2 electrons.
Subshell | Number of orbitals | Number of maximum electrons |
s | 1 | 2 |
p | 3 | 6 |
d | 5 | 10 |
f | 7 | 14 |
The spin of electron is represented by arrows. The up arrow means 1/2 spin and down arrow means - 1/2 spin. There are some rules to fill electrons in these orbitals as:
- Aufbau Principle:
It states that the electron goes in orbital which has lowest energy.
- Pauli’s Exclusion Principle:
It states that no two electron can have all the same quantum number, that’ why in an orbital, the spin or one electron is up and spin of second electrons is down.
- Hund’s Rule:
It states that each orbital in a subshell is single occupied with one electron before any one electron is occupied double and also the spin of all electrons.
The series of orbital from lowest to highest energy:
Electronic configuration:
It is notation which shows the distribution of electrons in orbitals of atoms, ion or molecule. The configuration lists the shell by principal quantum number, n= 1,2,3,4…. and subshell by azimuthal quantum number, l = s, p, d, f and electrons that can be present in it. With the help of orbital diagram electronic configuration can be written.
Answer to Problem 1E
The electronic configuration of Ni2+ is
Explanation of Solution
The atomic number of Nickel, Ni is 28.
The electronic configuration of Ni is
Here, Ni shows charge of +2 means 2 electrons from outermost 4s are lost. Hence total electrons present in Ni2+ are 26.
The orbital diagram of Ni2+ is:
The electronic configuration of Ni2+ is
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Chapter 23 Solutions
General Chemistry: Principles and Modern Applications (11th Edition)
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