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(a)
Interpretation:
The full ground state electronic configuration of
Concept introduction:
The electronic configuration of an element tells about the distribution of electrons in the atomic orbitals. The energy level that has lower energy is considered to be the ground state. Due to its lower energy, the ground state is taken as a stable state.
The electronic configuration is used to predict the physical, chemical, electrical and magnetic properties of the substance.
The electrons are filled up in accordance with the following three rules:
1. Aufbau principle which states that the electrons are filled up in the increasing order of their orbitals which follows as:
2. Hund’s rule which states that the pairing of electrons will not start until each of the orbitals is singly occupied.
3. Pauli’s exclusion principle states that no two electrons can have the same value of all the four quantum numbers.
(b)
Interpretation:
The full ground state electronic configuration of
Concept introduction:
The electronic configuration shows the distribution of electrons of atoms in the atomic orbitals. It is used to predict the physical, chemical, electrical and magnetic properties of the substance.
The electrons are filled up in accordance with the following three rules:
1. Aufbau principle which states that the electrons are filled up in the increasing order of their orbitals which follows as:
2. Hund’s rule which states that the pairing of electrons will not start until each of the orbitals is singly occupied.
3. Pauli’s exclusion principle states that no two electrons can have the same value of all the four quantum numbers.
(c)
Interpretation:
The full ground state electronic configuration of
Concept introduction:
The electronic configuration shows the distribution of electrons of atoms in the atomic orbitals. It is used to predict the physical, chemical, electrical and magnetic properties of the substance.
The electrons are filled up in accordance with the following three rules:
1. Aufbau principle which states that the electrons are filled up in the increasing order of their orbitals which follows as:
2. Hund’s rule which states that the pairing of electrons will not start until each of the orbitals is singly occupied.
3. Pauli’s exclusion principle states that no two electrons can have the same value of all the four quantum numbers.
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Chapter 8 Solutions
Chemistry: The Molecular Nature of Matter and Change (Looseleaf)
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