
(a)
Interpretation: The number of orbital present in one set g-orbital should be determined.
Concept introduction: The electrons that are present in an outermost orbital are known as valence electrons whereas those present in the orbitals with lower quantum numbers are termed as core electrons. Electrons are filled within orbitals by following three rules: Aufbau principle, Hund’s rule, and Pauli’s exclusion principle. Aufbau principle states, electrons are filled in the orbitals from lower to higher energy level as follows:
Hund’s rule states, initially each orbital is singly occupied and then pairing occurs and Pauli’s exclusion principle states, spin of two different electrons in one orbital is always different.
(b)
Interpretation: The angular nodes of g-orbital should be explained.
Concept introduction: The electrons that are present in an outermost orbital are known as valence electrons whereas those present in the orbitals with lower quantum numbers are termed as core electrons. Electrons are filled within orbitals by following three rules: Aufbau principle, Hund’s rule, and Pauli’s exclusion principle. Aufbau principle states, electrons are filled in the orbitals from lower to higher energy level as follows:
Hund’s rule states, initially each orbital is singly occupied and then pairing occurs and Pauli’s exclusion principle states, spin of two different electrons in one orbital is always different.
(c)
Interpretation: The relation between principal quantum number and radial nodes should be explained.
Concept introduction: The electrons that are present in an outermost orbital are known as valence electrons whereas those present in the orbitals with lower quantum numbers are termed as core electrons. Electrons are filled within orbitals by following three rules: Aufbau principle, Hund’s rule, and Pauli’s exclusion principle. Aufbau principle states, electrons are filled in the orbitals from lower to higher energy level as follows:
Hund’s rule states, initially each orbital is singly occupied and then pairing occurs and Pauli’s exclusion principle states, spin of two different electrons in one orbital is always different.

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Chapter 2 Solutions
EBK INORGANIC CHEMISTRY
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- 2. Draw the missing structure(s) in each of the following reactions. The missing structure(s) can be a starting material or the major reaction product(s). C5H10 Br H-Br CH2Cl2 + enant.arrow_forwardDraw the products of the stronger acid protonating the other reactant. KEq H₂C-O-H H3C OH Product acid Product basearrow_forwardDraw the products of the stronger acid protonating the other reactant. OH KEq CH H3C H3C `CH3 Product acid Product basearrow_forward
- 2. Draw the missing structure(s) in each of the following reactions. The missing structure(s) can be a starting material or the major reaction product(s). Ph H-I CH2Cl2arrow_forward3 attempts left Check my work Draw the products formed in the following oxidative cleavage. [1] 03 [2] H₂O draw structure ... lower mass product draw structure ... higher mass productarrow_forward2. Draw the missing structure(s) in each of the following reactions. The missing structure(s) can be a starting material or the major reaction product(s). H-Br CH2Cl2arrow_forward
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