Concept explainers
(a)
Interpretation: Ground-state electronic configuration of the given set of ions has to be written.
Concept Introduction:
- Electronic configuration is the arrangement of the electrons of atoms in the orbital. For atoms and ions, the electronic configuration is written by using Pauli Exclusion Principle and Hund’s rule.
- According to Pauli Exclusion Principle, no two electrons having the same spin can occupy the same orbital.
- According to Hund’s rule, the orbital in the subshell is filled singly by one electron before the same orbital is doubly filled. When the orbital is singly filled, all the electrons have same spin. In a doubly filled orbital, there are two electrons with opposite spin.
- Half-filled orbitals are comparatively stable as completely filled orbitals. Therefore, if there is a possibility of forming half-filled orbital then the electrons will be moved to the respective orbitals giving rise to more stability.
- When ions are formed from the atoms the electrons are added or removed from the outermost orbital.
To write: Ground-state electronic configuration for the given ions,
(a)
Answer to Problem 4.68QP
Answer
The ground-state electronic configuration of (a) is
Explanation of Solution
Explanation
Electronic configuration of
The electronic configuration of
Electronic configuration of
The electronic configuration of
(b)
Interpretation: Ground-state electronic configuration of the given set of ions has to be written.
Concept Introduction:
- Electronic configuration is the arrangement of the electrons of atoms in the orbital. For atoms and ions, the electronic configuration is written by using Pauli Exclusion Principle and Hund’s rule.
- According to Pauli Exclusion Principle, no two electrons having the same spin can occupy the same orbital.
- According to Hund’s rule, the orbital in the subshell is filled singly by one electron before the same orbital is doubly filled. When the orbital is singly filled, all the electrons have same spin. In a doubly filled orbital, there are two electrons with opposite spin.
- Half-filled orbitals are comparatively stable as completely filled orbitals. Therefore, if there is a possibility of forming half-filled orbital then the electrons will be moved to the respective orbitals giving rise to more stability.
- When ions are formed from the atoms the electrons are added or removed from the outermost orbital.
To write: Ground-state electronic configuration for the given ions,
(b)
Answer to Problem 4.68QP
Answer
The ground-state electronic configuration of (b) is
Explanation of Solution
Electronic configuration of
The electronic configuration of
Electronic configuration of
The electronic configuration of
(c)
Interpretation: Ground-state electronic configuration of the given set of ions has to be written.
Concept Introduction:
- Electronic configuration is the arrangement of the electrons of atoms in the orbital. For atoms and ions, the electronic configuration is written by using Pauli Exclusion Principle and Hund’s rule.
- According to Pauli Exclusion Principle, no two electrons having the same spin can occupy the same orbital.
- According to Hund’s rule, the orbital in the subshell is filled singly by one electron before the same orbital is doubly filled. When the orbital is singly filled, all the electrons have same spin. In a doubly filled orbital, there are two electrons with opposite spin.
- Half-filled orbitals are comparatively stable as completely filled orbitals. Therefore, if there is a possibility of forming half-filled orbital then the electrons will be moved to the respective orbitals giving rise to more stability.
- When ions are formed from the atoms the electrons are added or removed from the outermost orbital.
To write: Ground-state electronic configuration for the given ions,
(c)
Answer to Problem 4.68QP
Answer
The ground-state electronic configuration of (c) is
Explanation of Solution
Electronic configuration of
The electronic configuration of
Electronic configuration of
The electronic configuration of
(d)
Interpretation: Ground-state electronic configuration of the given set of ions has to be written.
Concept Introduction:
- Electronic configuration is the arrangement of the electrons of atoms in the orbital. For atoms and ions, the electronic configuration is written by using Pauli Exclusion Principle and Hund’s rule.
- According to Pauli Exclusion Principle, no two electrons having the same spin can occupy the same orbital.
- According to Hund’s rule, the orbital in the subshell is filled singly by one electron before the same orbital is doubly filled. When the orbital is singly filled, all the electrons have same spin. In a doubly filled orbital, there are two electrons with opposite spin.
- Half-filled orbitals are comparatively stable as completely filled orbitals. Therefore, if there is a possibility of forming half-filled orbital then the electrons will be moved to the respective orbitals giving rise to more stability.
- When ions are formed from the atoms the electrons are added or removed from the outermost orbital.
To write: Ground-state electronic configuration for the given ions,
(d)
Answer to Problem 4.68QP
Answer
The ground-state electronic configuration of (d) is
Explanation of Solution
Electronic configuration of
The electronic configuration of
Electronic configuration of
The electronic configuration of
(e)
Interpretation: Ground-state electronic configuration of the given set of ions has to be written.
Concept Introduction:
- Electronic configuration is the arrangement of the electrons of atoms in the orbital. For atoms and ions, the electronic configuration is written by using Pauli Exclusion Principle and Hund’s rule.
- According to Pauli Exclusion Principle, no two electrons having the same spin can occupy the same orbital.
- According to Hund’s rule, the orbital in the subshell is filled singly by one electron before the same orbital is doubly filled. When the orbital is singly filled, all the electrons have same spin. In a doubly filled orbital, there are two electrons with opposite spin.
- Half-filled orbitals are comparatively stable as completely filled orbitals. Therefore, if there is a possibility of forming half-filled orbital then the electrons will be moved to the respective orbitals giving rise to more stability.
- When ions are formed from the atoms the electrons are added or removed from the outermost orbital.
To write: Ground-state electronic configuration for the given ions,
(e)
Answer to Problem 4.68QP
Answer
The ground-state electronic configuration of (e) is
Explanation of Solution
Electronic configuration of
The electronic configuration of
Electronic configuration of
The electronic configuration of
(f)
Interpretation: Ground-state electronic configuration of the given set of ions has to be written.
Concept Introduction:
- Electronic configuration is the arrangement of the electrons of atoms in the orbital. For atoms and ions, the electronic configuration is written by using Pauli Exclusion Principle and Hund’s rule.
- According to Pauli Exclusion Principle, no two electrons having the same spin can occupy the same orbital.
- According to Hund’s rule, the orbital in the subshell is filled singly by one electron before the same orbital is doubly filled. When the orbital is singly filled, all the electrons have same spin. In a doubly filled orbital, there are two electrons with opposite spin.
- Half-filled orbitals are comparatively stable as completely filled orbitals. Therefore, if there is a possibility of forming half-filled orbital then the electrons will be moved to the respective orbitals giving rise to more stability.
- When ions are formed from the atoms the electrons are added or removed from the outermost orbital.
To write: Ground-state electronic configuration for the given ions,
(f)
Answer to Problem 4.68QP
Answer
The ground-state electronic configuration of (f) is
Explanation of Solution
Electronic configuration of
The electronic configuration of
Electronic configuration of
The electronic configuration of
(g)
Interpretation: Ground-state electronic configuration of the given set of ions has to be written.
Concept Introduction:
- Electronic configuration is the arrangement of the electrons of atoms in the orbital. For atoms and ions, the electronic configuration is written by using Pauli Exclusion Principle and Hund’s rule.
- According to Pauli Exclusion Principle, no two electrons having the same spin can occupy the same orbital.
- According to Hund’s rule, the orbital in the subshell is filled singly by one electron before the same orbital is doubly filled. When the orbital is singly filled, all the electrons have same spin. In a doubly filled orbital, there are two electrons with opposite spin.
- Half-filled orbitals are comparatively stable as completely filled orbitals. Therefore, if there is a possibility of forming half-filled orbital then the electrons will be moved to the respective orbitals giving rise to more stability.
- When ions are formed from the atoms the electrons are added or removed from the outermost orbital.
To write: Ground-state electronic configuration for the given ions,
(g)
Answer to Problem 4.68QP
Answer
The ground-state electronic configuration of (g) is
Explanation of Solution
Electronic configuration of
The electronic configuration of
Electronic configuration of
The electronic configuration of
(h)
Interpretation: Ground-state electronic configuration of the given set of ions has to be written.
Concept Introduction:
- Electronic configuration is the arrangement of the electrons of atoms in the orbital. For atoms and ions, the electronic configuration is written by using Pauli Exclusion Principle and Hund’s rule.
- According to Pauli Exclusion Principle, no two electrons having the same spin can occupy the same orbital.
- According to Hund’s rule, the orbital in the subshell is filled singly by one electron before the same orbital is doubly filled. When the orbital is singly filled, all the electrons have same spin. In a doubly filled orbital, there are two electrons with opposite spin.
- Half-filled orbitals are comparatively stable as completely filled orbitals. Therefore, if there is a possibility of forming half-filled orbital then the electrons will be moved to the respective orbitals giving rise to more stability.
- When ions are formed from the atoms the electrons are added or removed from the outermost orbital.
To write: Ground-state electronic configuration for the given ions,
(h)
Answer to Problem 4.68QP
Answer
The ground-state electronic configuration of (h) is
Explanation of Solution
Explanation:
Electronic configuration of
The electronic configuration of
Electronic configuration of
The electronic configuration of
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Chapter 4 Solutions
Chemistry: Atoms First
- Use the periodic table to (i) predict electron configurations for the following species: Arsenic ion, As3– Magnesium ion, Mg2+ Vanadium(II) ion, V2+ (ii) Write the electron configurations of each species in the noble gas notation. (iii) Draw an orbital diagram to represent 1 c above. Draw the Lewis electron dot structures of the following chemical species. In each case you must say whether or not the central atom obeys the Octet Rule. CS2 and H2S CF4 and SiH4 NH2Cl CO32– and BF3 PCl5 ClF3, XeF2, Calculate the formal charge on the Sulphur atom in the Sulphate anion structure shown below(picture attatched) Give the electron-pair and molecular geometries for NF3 and XeF4.arrow_forwardUse the noble-gas notation and write the ground-state electronic configurations of the following ions:(a) Ca2+ (b) Ga3+ (c) Cr3+arrow_forwardConsider these ground-state ionization energies of one-electron species:H=1.31X10³kJ/mol ,He⁺=5.24X10³kJ/mol Li²⁺=1.41X10⁴kJ/mol (a) Write a general expression for the ionization energy of anyone-electron species. (b) Use your expression to calculate theionization energy of B⁴⁺. (c) What is the minimum wavelengthrequired to remove the electron from the n=3 level of He⁺?(d) What is the minimum wavelength required to remove the electron from the n=2 level of Be³⁺?arrow_forward
- Write the electron configurations for (a) Ga3 + , (b) Cr3 + ,and (c) Br-.arrow_forward7. Which element has the smallest first ionization energy? (a) Cs (b) Ga (c) K (d) Bi (e) As 8. Which element has the smallest second ionization energy? (a) Mg (b) Li (c) S (d) O (e) Ca 9. Which of the following sets contain all linear molecules? (a) H2S, HCN, CO2. (b) HCN, O2, CO2 (c) H2O, CO, Cl2. (d) H2S, CO, CO2. (e) BF3, Cl2, O2 10. The molecular geometry of SnCl3-ion is: (a) trigonal planar (b) T-shaped. (c) trigonal pyramidal. (d) Tetrahedral (e) see-saw 11. The geometry of the molecule SPC13 is best described as: (a) square planar (b) trigonal pyramidal (c) trigonal bipyramidal. (d) octahedral (e) tetrahedral 12. The O-S-Cl bond angles in O2SCl2 are expected to be approximately: (a) 90° (b) 109.5° (c) 120° (d)180 ° (e) 90° and 120°arrow_forward5. The atoms and ions Ne, N³-, F, Mg2+, and Si4+ are part of an isoelectronic series. (a) Which of these will have the smallest effective nuclear charge acting on the outermost electron? (b) Which one possess the greatest effective nuclear charge? (c) Which ion will be the largest in size? Explain why.arrow_forward
- Q1. This question is about atomic structure. (a) Write the full electron configuration for each of the following species. CH Fe2+ (b) Write an equation, including state symbols, to represent the process that occurs when the third ionisation energy of manganese is measured. (c) State which of the elements magnesium and aluminium has the lower first ionisation energy Explain your answer. (d) A sample of nickel was analysed in a time of flight (TOF) mass spectrometer. The sample was ionised by electron impact ionisation. The spectrum produced showed three peaks with abundances as set out in the table. m/z Abundance /% 58 61.0 60 29.1 61 9.9 Give the symbol, including mass number, of the ion that would reach the detector first in the sample. Calculate the relative atomic mass of the nickel in the sample. Give your answer to one decimal place. Page 2 of 12 Symbol of ion Relative atomic massarrow_forwardUsing complete subshell notation (1s^22s^22p^6, and so forth), predict the electron configurations of the following ions. (a) N3– (b) Ca2+ (c) S– (d) Cs2+ (e) Cr2+ (f) Gd3+arrow_forwardWrite ground-state electron configurations for the following ions: K+, Mg2+, O2-, I-, Al3+,arrow_forward
- Chemistry: Principles and PracticeChemistryISBN:9780534420123Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward MercerPublisher:Cengage LearningChemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage Learning