General Chemistry
General Chemistry
7th Edition
ISBN: 9780073402758
Author: Chang, Raymond/ Goldsby
Publisher: McGraw-Hill College
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Chapter 8, Problem 8.27QP

(a)

Interpretation Introduction

Interpretation:

Ground–state electronic configuration of lithium ion Li+ has to be written.

Concept Introduction:

Electron configuration is the distribution of electrons in atomic orbitals. It gives an idea about the shape and energy of an atom.

There are 3 rules to decide the electronic configuration of an atom. They are,

  • Pauli Exclusion Principle: No two electrons should not have same four quantum numbers in an atom that is, it no two electrons should have same principal quantum number (n), same orbital angular momentum quantum number (l), the same magnetic quantum number (ml) or same spin magnetic quantum numbers (ms)
  • Aufbau Principle: In an atom, electrons fill according to the increasing energy of the orbital.
  • Hund's Rule: The orbital having maximum number of electrons with same spin in separate orbitals is the most stable arrangement in an orbital.

Cation is formed when one or more electrons get removed from the outermost subshell of an atom.

(a)

Expert Solution
Check Mark

Answer to Problem 8.27QP

The electronic configuration of Li+ is 1s2

Explanation of Solution

The orbitals are filled according to Pauli Exclusion Principle, Aufbau Principle and Hund's Rule. The maximum number of electrons that can be accommodating in each orbital is 2.

Since the ns orbitals have lower energy comparing to the np orbitals and ns orbital is filled first. The ns orbitals have lower energy comparing to the (n-1)d orbitals and are filled first.

The atomic number of Li is 3 and the electronic configuration is 1s22s1

For Li+, one electron is removed from the outermost subshell. Hence, the number of electrons becomes 2

Therefore,

The electronic configuration of Li+ is given as:

  1s2

(b)

Interpretation Introduction

Interpretation:

Ground–state electronic configuration of H ions has to be written.

Concept Introduction:

Electron configuration is the distribution of electrons in atomic orbitals. It gives an idea about the shape and energy of an atom.

There are 3 rules to decide the electronic configuration of an atom. They are,

  • Pauli Exclusion Principle: No two electrons should not have same four quantum numbers in an atom that is, it no two electrons should have same principal quantum number (n), same orbital angular momentum quantum number (l), the same magnetic quantum number (ml) or same spin magnetic quantum numbers (ms)
  • Aufbau Principle: In an atom, electrons fill according to the increasing energy of the orbital.
  • Hund's Rule: The orbital having maximum number of electrons with same spin in separate orbitals is the most stable arrangement in an orbital.

Anion is formed when one or more electrons get added to the outermost subshell of an atom.

(b)

Expert Solution
Check Mark

Answer to Problem 8.27QP

The electronic configuration of H is 1s2

Explanation of Solution

The orbitals are filled according to Pauli Exclusion Principle, Aufbau Principle and Hund's Rule. The maximum number of electrons that can be accommodating in each orbital is 2.

Since the ns orbitals have lower energy comparing to the np orbitals and ns orbital is filled first. The ns orbitals have lower energy comparing to the (n-1)d orbitals and are filled first.

The atomic number of H is 1 and the electronic configuration is 1s1

For H, one electron is added to the outermost subshell. Hence, the number of electrons becomes 2

Therefore,

The electronic configuration of H is given as:

  H-1s2

(b)

Interpretation Introduction

Interpretation:

Ground–state electronic configuration of N3 has to be written.

Concept Introduction:

Electron configuration is the distribution of electrons in atomic orbitals. It gives an idea about the shape and energy of an atom.

There are 3 rules to decide the electronic configuration of an atom. They are,

  • Pauli Exclusion Principle: No two electrons should not have same four quantum numbers in an atom that is, it no two electrons should have same principal quantum number (n), same orbital angular momentum quantum number (l), the same magnetic quantum number (ml) or same spin magnetic quantum numbers (ms)
  • Aufbau Principle: In an atom, electrons fill according to the increasing energy of the orbital.
  • Hund's Rule: The orbital having maximum number of electrons with same spin in separate orbitals is the most stable arrangement in an orbital.

Anion is formed when one or more electrons get added to the outermost subshell of an atom.

(b)

Expert Solution
Check Mark

Answer to Problem 8.27QP

The electronic configuration of N3 is 1s22s22p6

Explanation of Solution

The orbitals are filled according to Pauli Exclusion Principle, Aufbau Principle and Hund's Rule. The maximum number of electrons that can be accommodating in each orbital is 2.

Since the ns orbitals have lower energy comparing to the np orbitals and ns orbital is filled first. The ns orbitals have lower energy comparing to the (n-1)d orbitals and are filled first.

The atomic number of N is 7 and the electronic configuration is 1s22s22p3

For N3, three electrons are added to the outermost subshell. Hence, the number of electrons becomes 10

Therefore,

The electronic configuration of N3 is given as:

  1s22s22p6

(d)

Interpretation Introduction

Interpretation:

Ground–state electronic configuration of F has to be written.

Concept Introduction:

Electron configuration is the distribution of electrons in atomic orbitals. It gives an idea about the shape and energy of an atom.

There are 3 rules to decide the electronic configuration of an atom. They are,

  • Pauli Exclusion Principle: No two electrons should not have same four quantum numbers in an atom that is, it no two electrons should have same principal quantum number (n), same orbital angular momentum quantum number (l), the same magnetic quantum number (ml) or same spin magnetic quantum numbers (ms)
  • Aufbau Principle: In an atom, electrons fill according to the increasing energy of the orbital.
  • Hund's Rule: The orbital having maximum number of electrons with same spin in separate orbitals is the most stable arrangement in an orbital.

Anion is formed when one or more electrons get added to the outermost subshell of an atom.

(d)

Expert Solution
Check Mark

Answer to Problem 8.27QP

The electronic configuration of F is 1s22s22p5

Explanation of Solution

The orbitals are filled according to Pauli Exclusion Principle, Aufbau Principle and Hund's Rule. The maximum number of electrons that can be accommodating in each orbital is 2.

Since the ns orbitals have lower energy comparing to the np orbitals and ns orbital is filled first. The ns orbitals have lower energy comparing to the (n-1)d orbitals and are filled first.

The atomic number of F is 9 and the electronic configuration is 1s22s22p5

For F, one electron is added to the outermost subshell. Hence, the number of electrons becomes 10

Therefore,

The electronic configuration of F is given as:

  F----1s22s22p6

(e)

Interpretation Introduction

Interpretation:

Ground–state electronic configuration of S2 ion has to be written.

Concept Introduction:

Electron configuration is the distribution of electrons in atomic orbitals. It gives an idea about the shape and energy of an atom.

There are 3 rules to decide the electronic configuration of an atom. They are,

  • Pauli Exclusion Principle: No two electrons should not have same four quantum numbers in an atom that is, it no two electrons should have same principal quantum number (n), same orbital angular momentum quantum number (l), the same magnetic quantum number (ml) or same spin magnetic quantum numbers (ms)
  • Aufbau Principle: In an atom, electrons fill according to the increasing energy of the orbital.
  • Hund's Rule: The orbital having maximum number of electrons with same spin in separate orbitals is the most stable arrangement in an orbital.

Anion is formed when one or more electrons get added to the outermost subshell of an atom.

(e)

Expert Solution
Check Mark

Answer to Problem 8.27QP

The electronic configuration of S2 is 1s22s22p63s23p6

Explanation of Solution

The orbitals are filled according to Pauli Exclusion Principle, Aufbau Principle and Hund's Rule. The maximum number of electrons that can be accommodating in each orbital is 2.

Since the ns orbitals have lower energy comparing to the np orbitals and ns orbital is filled first. The ns orbitals have lower energy comparing to the (n-1)d orbitals and are filled first.

The atomic number of S is 16 and the electronic configuration is 1s22s22p63s23p4

For S2, three electrons are added to the outermost subshell. Hence, the number of electrons becomes 18

Therefore,

The electronic configuration of S2 is given as:

  1s22s22p63s23p6

(f)

Interpretation Introduction

Interpretation:

Ground–state electronic configuration of Al3+ has to be written.

Concept Introduction:

Electron configuration is the distribution of electrons in atomic orbitals. It gives an idea about the shape and energy of an atom.

There are 3 rules to decide the electronic configuration of an atom. They are,

  • Pauli Exclusion Principle: No two electrons should not have same four quantum numbers in an atom that is, it no two electrons should have same principal quantum number (n), same orbital angular momentum quantum number (l), the same magnetic quantum number (ml) or same spin magnetic quantum numbers (ms)
  • Aufbau Principle: In an atom, electrons fill according to the increasing energy of the orbital.
  • Hund's Rule: The orbital having maximum number of electrons with same spin in separate orbitals is the most stable arrangement in an orbital.

Cation is formed when one or more electrons get removed from the outermost subshell of an atom.

(f)

Expert Solution
Check Mark

Answer to Problem 8.27QP

The electronic configuration of Al3+ is 1s22s22p6

Explanation of Solution

The orbitals are filled according to Pauli Exclusion Principle, Aufbau Principle and Hund's Rule. The maximum number of electrons that can be accommodating in each orbital is 2.

Since the ns orbitals have lower energy comparing to the np orbitals and ns orbital is filled first. The ns orbitals have lower energy comparing to the (n-1)d orbitals and are filled first.

The atomic number of Al is 13 and the electronic configuration is 1s22s22p63s23p1

For Al3+, three electrons are removed from the outermost subshell. Hence, the number of electrons becomes 10

Therefore,

The electronic configuration of Al3+ is given as:

  Al3+----1s22s22p6

(g)

Interpretation Introduction

Interpretation:

Ground–state electronic configuration of Se2 has to be written.

Concept Introduction:

Electron configuration is the distribution of electrons in atomic orbitals. It gives an idea about the shape and energy of an atom.

There are 3 rules to decide the electronic configuration of an atom. They are,

  • Pauli Exclusion Principle: No two electrons should not have same four quantum numbers in an atom that is, it no two electrons should have same principal quantum number (n), same orbital angular momentum quantum number (l), the same magnetic quantum number (ml) or same spin magnetic quantum numbers (ms)
  • Aufbau Principle: In an atom, electrons fill according to the increasing energy of the orbital.
  • Hund's Rule: The orbital having maximum number of electrons with same spin in separate orbitals is the most stable arrangement in an orbital.

Anion is formed when one or more electrons get added to the outermost subshell of an atom.

(g)

Expert Solution
Check Mark

Answer to Problem 8.27QP

The electronic configuration of Se2 is [Ar]4s23d104p6

Explanation of Solution

The orbitals are filled according to Pauli Exclusion Principle, Aufbau Principle and Hund's Rule. The maximum number of electrons that can be accommodating in each orbital is 2.

Since the ns orbitals have lower energy comparing to the np orbitals and ns orbital is filled first. The ns orbitals have lower energy comparing to the (n-1)d orbitals and are filled first.

The atomic number of Se is 34 and the electronic configuration is [Ar]4s23d104p4

For Se2, three electrons are added to the outermost subshell. Hence, the number of electrons becomes 36

Therefore,

The electronic configuration of Se2 is given as:

  [Ar]4s23d104p6

(h)

Interpretation Introduction

Interpretation:

Ground–state electronic configuration of Br has to be written.

Concept Introduction:

Electron configuration is the distribution of electrons in atomic orbitals. It gives an idea about the shape and energy of an atom.

There are 3 rules to decide the electronic configuration of an atom. They are,

  • Pauli Exclusion Principle: No two electrons should not have same four quantum numbers in an atom that is, it no two electrons should have same principal quantum number (n), same orbital angular momentum quantum number (l), the same magnetic quantum number (ml) or same spin magnetic quantum numbers (ms)
  • Aufbau Principle: In an atom, electrons fill according to the increasing energy of the orbital.
  • Hund's Rule: The orbital having maximum number of electrons with same spin in separate orbitals is the most stable arrangement in an orbital.

Anion is formed when one or more electrons get added to the outermost subshell of an atom.

(h)

Expert Solution
Check Mark

Answer to Problem 8.27QP

The electronic configuration of Br is [Ar]4s23d104p6

Explanation of Solution

The orbitals are filled according to Pauli Exclusion Principle, Aufbau Principle and Hund's Rule. The maximum number of electrons that can be accommodating in each orbital is 2.

Since the ns orbitals have lower energy comparing to the np orbitals and ns orbital is filled first. The ns orbitals have lower energy comparing to the (n-1)d orbitals and are filled first.

The atomic number of Br is 35 and the electronic configuration is [Ar]4s23d104p5

For Br, one electron is added to the outermost subshell. Hence, the number of electrons becomes 36

Therefore,

The electronic configuration of Br is given as:

  Br-[Ar]4s23d104p6

(i)

Interpretation Introduction

Interpretation:

Ground–state electronic configuration of Rb+ has to be written.

Concept Introduction:

Electron configuration is the distribution of electrons in atomic orbitals. It gives an idea about the shape and energy of an atom.

There are 3 rules to decide the electronic configuration of an atom. They are,

  • Pauli Exclusion Principle: No two electrons should not have same four quantum numbers in an atom that is, it no two electrons should have same principal quantum number (n), same orbital angular momentum quantum number (l), the same magnetic quantum number (ml) or same spin magnetic quantum numbers (ms)
  • Aufbau Principle: In an atom, electrons fill according to the increasing energy of the orbital.
  • Hund's Rule: The orbital having maximum number of electrons with same spin in separate orbitals is the most stable arrangement in an orbital.

Cation is formed when one or more electrons get removed from the outermost subshell of an atom.

(i)

Expert Solution
Check Mark

Answer to Problem 8.27QP

The electronic configuration of Rb+ is [Ar]4s23d104p6

Explanation of Solution

The orbitals are filled according to Pauli Exclusion Principle, Aufbau Principle and Hund's Rule. The maximum number of electrons that can be accommodating in each orbital is 2.

Since the ns orbitals have lower energy comparing to the np orbitals and ns orbital is filled first. The ns orbitals have lower energy comparing to the (n-1)d orbitals and are filled first.

The atomic number of Rb is 37 and the electronic configuration is [Ar]4s23d104p65s1

For Rb+, one electron is removed from the outermost subshell. Hence, the number of electrons becomes 36

Therefore,

The electronic configuration of Rb+ is given as:

  Rb+[Ar]4s23d104p6

(j)

Interpretation Introduction

Interpretation:

Ground–state electronic configuration of Sr2+ has to be written.

Concept Introduction:

Electron configuration is the distribution of electrons in atomic orbitals. It gives an idea about the shape and energy of an atom.

There are 3 rules to decide the electronic configuration of an atom. They are,

  • Pauli Exclusion Principle: No two electrons should not have same four quantum numbers in an atom that is, it no two electrons should have same principal quantum number (n), same orbital angular momentum quantum number (l), the same magnetic quantum number (ml) or same spin magnetic quantum numbers (ms)
  • Aufbau Principle: In an atom, electrons fill according to the increasing energy of the orbital.
  • Hund's Rule: The orbital having maximum number of electrons with same spin in separate orbitals is the most stable arrangement in an orbital.

Cation is formed when one or more electrons get removed from the outermost subshell of an atom.

(j)

Expert Solution
Check Mark

Answer to Problem 8.27QP

The electronic configuration of Sr2+ is [Ar]4s23d104p6

Explanation of Solution

The orbitals are filled according to Pauli Exclusion Principle, Aufbau Principle and Hund's Rule. The maximum number of electrons that can be accommodating in each orbital is 2.

Since the ns orbitals have lower energy comparing to the np orbitals and ns orbital is filled first. The ns orbitals have lower energy comparing to the (n-1)d orbitals and are filled first.

The atomic number of Sr is 38 and the electronic configuration is [Ar]4s23d104p65s2

For Sr2+, two electrons are removed from the outermost subshell. Hence, the number of electrons becomes 36

Therefore,

The electronic configuration of Sr2+ is given as:

  Sr2+[Ar]4s23d104p6

(k)

Interpretation Introduction

Interpretation:

Ground–state electronic configuration of Sn2+ has to be written.

Concept Introduction:

Electron configuration is the distribution of electrons in atomic orbitals. It gives an idea about the shape and energy of an atom.

There are 3 rules to decide the electronic configuration of an atom. They are,

  • Pauli Exclusion Principle: No two electrons should not have same four quantum numbers in an atom that is, it no two electrons should have same principal quantum number (n), same orbital angular momentum quantum number (l), the same magnetic quantum number (ml) or same spin magnetic quantum numbers (ms)
  • Aufbau Principle: In an atom, electrons fill according to the increasing energy of the orbital.
  • Hund's Rule: The orbital having maximum number of electrons with same spin in separate orbitals is the most stable arrangement in an orbital.

Cation is formed when one or more electrons get removed from the outermost subshell of an atom.

(k)

Expert Solution
Check Mark

Answer to Problem 8.27QP

The electronic configuration of Sn2+ is [Kr]5s24d10

Explanation of Solution

The orbitals are filled according to Pauli Exclusion Principle, Aufbau Principle and Hund's Rule. The maximum number of electrons that can be accommodating in each orbital is 2.

Since the ns orbitals have lower energy comparing to the np orbitals and ns orbital is filled first. The ns orbitals have lower energy comparing to the (n-1)d orbitals and are filled first.

The atomic number of Sn is 50 and the electronic configuration is [Kr]5s24d104p2

For Sn2+, two electrons are removed from the outermost subshell. Hence, the number of electrons becomes 48

Therefore,

The electronic configuration of Sn2+ is given as:

  [Kr]5s24d10

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Chapter 8 Solutions

General Chemistry

Ch. 8.6 - Prob. 1PECh. 8.6 - Prob. 1RCCh. 8 - Prob. 8.1QPCh. 8 - Prob. 8.2QPCh. 8 - Prob. 8.3QPCh. 8 - Prob. 8.4QPCh. 8 - Prob. 8.5QPCh. 8 - Prob. 8.6QPCh. 8 - Prob. 8.7QPCh. 8 - Prob. 8.8QPCh. 8 - Prob. 8.9QPCh. 8 - Prob. 8.10QPCh. 8 - Prob. 8.11QPCh. 8 - Prob. 8.12QPCh. 8 - Prob. 8.13QPCh. 8 - 8.14 Use die first-row transition metals (Sc to...Ch. 8 - 8.15 In the periodic table, the element hydrogen...Ch. 8 - 8.16 A neutral atom of a certain element has 17...Ch. 8 - Prob. 8.17QPCh. 8 - Prob. 8.18QPCh. 8 - Prob. 8.19QPCh. 8 - Prob. 8.20QPCh. 8 - Prob. 8.21QPCh. 8 - 8.21 An ion M2+ derived from a metal in the first...Ch. 8 - Prob. 8.23QPCh. 8 - Prob. 8.24QPCh. 8 - Prob. 8.25QPCh. 8 - Prob. 8.26QPCh. 8 - Prob. 8.27QPCh. 8 - Prob. 8.28QPCh. 8 - Prob. 8.29QPCh. 8 - Prob. 8.30QPCh. 8 - 8.31 Which of these species are isoelectronic with...Ch. 8 - 8.32 Group the species that are isoelectronic:...Ch. 8 - Prob. 8.33QPCh. 8 - 8.34 How does atomic radius change as we move (a)...Ch. 8 - Prob. 8.35QPCh. 8 - Prob. 8.36QPCh. 8 - 8.37 On the basis of their positions in the...Ch. 8 - Prob. 8.38QPCh. 8 - 8.39 Which is the largest atom in Group 4A? Ch. 8 - Prob. 8.40QPCh. 8 - Prob. 8.41QPCh. 8 - Prob. 8.42QPCh. 8 - Prob. 8.43QPCh. 8 - Prob. 8.44QPCh. 8 - Prob. 8.45QPCh. 8 - Prob. 8.46QPCh. 8 - Prob. 8.47QPCh. 8 - Prob. 8.48QPCh. 8 - 8.49 Define ionization energy. Ionization energy...Ch. 8 - Prob. 8.50QPCh. 8 - Prob. 8.51QPCh. 8 - Prob. 8.52QPCh. 8 - Prob. 8.53QPCh. 8 - Prob. 8.54QPCh. 8 - Prob. 8.55QPCh. 8 - Prob. 8.56QPCh. 8 - Prob. 8.57QPCh. 8 - Prob. 8.58QPCh. 8 - Prob. 8.59QPCh. 8 - Prob. 8.60QPCh. 8 - Prob. 8.61QPCh. 8 - Prob. 8.62QPCh. 8 - Prob. 8.63QPCh. 8 - Prob. 8.64QPCh. 8 - Prob. 8.65QPCh. 8 - Prob. 8.66QPCh. 8 - Prob. 8.67QPCh. 8 - 8.68 Why are the Group 1B elements more stable...Ch. 8 - Prob. 8.69QPCh. 8 - Prob. 8.70QPCh. 8 - Prob. 8.71QPCh. 8 - Prob. 8.72QPCh. 8 - Prob. 8.73QPCh. 8 - Prob. 8.74QPCh. 8 - Prob. 8.75QPCh. 8 - Prob. 8.76QPCh. 8 - Prob. 8.77QPCh. 8 - Prob. 8.78QPCh. 8 - Prob. 8.79QPCh. 8 - Prob. 8.80QPCh. 8 - Prob. 8.81QPCh. 8 - Prob. 8.82QPCh. 8 - Prob. 8.83QPCh. 8 - Prob. 8.84QPCh. 8 - Prob. 8.85QPCh. 8 - Prob. 8.86QPCh. 8 - Prob. 8.87QPCh. 8 - Prob. 8.88QPCh. 8 - Prob. 8.89QPCh. 8 - 8.90 Write the formulas and names of the oxides of...Ch. 8 - Prob. 8.91QPCh. 8 - Prob. 8.92QPCh. 8 - Prob. 8.93QPCh. 8 - Prob. 8.94QPCh. 8 - Prob. 8.95QPCh. 8 - Prob. 8.96QPCh. 8 - Prob. 8.97QPCh. 8 - Prob. 8.98QPCh. 8 - 8.99 Explain why the electron affinity of nitrogen...Ch. 8 - Prob. 8.100QPCh. 8 - Prob. 8.101QPCh. 8 - Prob. 8.102QPCh. 8 - Prob. 8.103QPCh. 8 - Prob. 8.104QPCh. 8 - Prob. 8.105QPCh. 8 - Prob. 8.106QPCh. 8 - Prob. 8.107SPCh. 8 - 8.108 In the late 1800s the British physicist Lord...Ch. 8 - Prob. 8.109SPCh. 8 - Prob. 8.110SPCh. 8 - Prob. 8.111SPCh. 8 - Prob. 8.112SPCh. 8 - Prob. 8.113SPCh. 8 - Prob. 8.114SP
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