(a)
Interpretation:
The ground-state electronic configuration of
Concept Introduction:
The electronic configuration is defined as the distribution of electrons in various atomic orbitals of the atom. 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 called core electrons. The general outer electronic configuration of
Electrons are filled in orbitals in accordance with three rules: Aufbau principle, Hund’s rule, and Pauli’s exclusion principle. Aufbau principle states that electrons are filled in the orbitals from lower to higher energy level as follows:
Hund’s rule states that initially each orbital is singly occupied and then pairing occurs and Pauli’s exclusion principle states that the spin of two electrons in one orbital is always different.
(b)
Interpretation:
The ground-state electronic configuration of
Concept Introduction:
Refer to part (a).
(c)
Interpretation:
The ground-state electronic configuration of
Concept Introduction:
Refer to part (a).
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Chapter 8 Solutions
Chemistry: Principles and Practice
- Write the electron configurations for the following atoms or ions:(a) B3+(b) O–(c) Cl3+(d) Ca2+(e) Tiarrow_forwardWrite the electron configurations for the following atoms or ions: (a) B3+ (b) O– (c) Cl3+ (d) Ca2+ (e) Tiarrow_forwardWhat is the electron configuration and orbital diagram of:(a) Na+(b) P3–(c) Al2+ (d) Fe2+(e) Sm3+arrow_forward
- Write the ground-state electron configurations of the following transition metal ions. (a) Sc3+ (b) Cr3+ (c) Cu+ (d) Au+arrow_forwardWrite the electron configuration and orbital diagram for each ion and determine whether each is diamagnetic or paramagnetic.(a) Al3 + (b) S2 - (c) Fe3 +arrow_forwardProvide a brief explanation for each of the following: (a) O2-is larger than O. (b) S2- is larger than O2-. (c) S2- is largerthan K+. (d) K+ is larger than Ca2+.arrow_forward
- Discuss each conclusion from a study of redox reactions:(a) The nitride ion functions only as a reducing agent.(b) The nitrate ion functions only as an oxidizing agent.(c) The nitrite ion functions as an oxidizing or a reducing agentarrow_forwardWrite the ground-state electron configurations of the following ions/transition metal ions.. (a) Li+ (b) N3− (c) In3+ (d) Tl+ (a) Sc3+ (b) Cr3+ (c) Cu+ (d) Au+arrow_forwardChoosing from the elements in the third row of the Periodic Table write out thechemical formula of(i) A basic oxide.(ii) An amphoteric oxide.(iii) An acidic oxidearrow_forward
- Discuss each conclusion from a study of redox reactions:(a) The sulfide ion functions only as a reducing agent.(b) The sulfate ion functions only as an oxidizing agent.(c) Sulfur dioxide functions as an oxidizing or a reducing agentarrow_forward4. Write an appropriate set of four quantum numbers (n, l, ml & ms) that could be representative of a valence electron in each of the following atoms or ions. (a) Bi (m (b) Sr (c) Mo (d) Ru2+ (e) Euarrow_forwardWhich of the following is isoelectronic pair? (i) ICl2, ClO2 (ii) BrO2– , BrF2+ (iii) ClO2, BrF (iv) CN–, O3arrow_forward
- Physical ChemistryChemistryISBN:9781133958437Author:Ball, David W. (david Warren), BAER, TomasPublisher:Wadsworth Cengage Learning,