General Chemistry
General Chemistry
7th Edition
ISBN: 9780073402758
Author: Chang, Raymond/ Goldsby
Publisher: McGraw-Hill College
Question
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Chapter 8, Problem 8.28QP

(a)

Interpretation Introduction

Interpretation:

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

Concept Introduction:

Electron configuration is the distribution of electrons in the atomic orbitals. It gives an idea about the shape and energy of electrons in 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 atoms 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 gets removed from the outermost subshell of an atom.

(a)

Expert Solution
Check Mark

Answer to Problem 8.28QP

The electronic configuration of Na+ 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 Na is 11 and the electronic configuration is 1s22s22p63s1

For Na+ , one electron is removed from the outermost subshell. Hence, the atomic number becomes 10

Therefore,

The electronic configuration of Na+ is given as:

1s22s22p6

(b)

Interpretation Introduction

Interpretation:

Ground–state electronic configuration of Mg2+ has to be written.

Concept Introduction:

Electron configuration is the distribution of electrons in the atomic orbitals. It gives an idea about the shape and energy of electrons in 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 atoms 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 gets removed from the outermost subshell of an atom.

(b)

Expert Solution
Check Mark

Answer to Problem 8.28QP

The electronic configuration of Mg2+ 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 Mg is 12 and the electronic configuration is 1s22s22p63s2

For Mg2+, two electrons are removed from the outermost subshell. Hence, the atomic number becomes 10

Therefore,

The electronic configuration of Mg2+ is given as:

1s22s22p6

(c)

Interpretation Introduction

Interpretation:

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

Concept Introduction:

Electron configuration is the distribution of electrons in the atomic orbitals. It gives an idea about the shape and energy of electrons in 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 atoms 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 gets removed from the outermost subshell of an atom.

(c)

Expert Solution
Check Mark

Answer to Problem 8.28QP

The electronic configuration of Cl 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 Cl is 17 and the electronic configuration is 1s22s22p63s23p5

For Cl, one electron is added to the outermost subshell. Hence, the atomic number becomes 18

Therefore,

The electronic configuration of Cl is given as:

1s22s22p63s23p6

(d)

Interpretation Introduction

Interpretation:

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

Concept Introduction:

Electron configuration is the distribution of electrons in the atomic orbitals. It gives an idea about the shape and energy of electrons in 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 atoms 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 gets removed from the outermost subshell of an atom.

(d)

Expert Solution
Check Mark

Answer to Problem 8.28QP

The electronic configuration of K+ 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 K is 19 and the electronic configuration is 1s22s22p63s23p64s1

For K+, one electron is removed from the outermost subshell. Hence, the atomic number becomes 18

Therefore,

The electronic configuration of K+ is given as:

1s22s22p63s23p6

(e)

Interpretation Introduction

Interpretation: Ground–state electronic configuration of Ca2+ has to be written.

Concept Introduction:

Electron configuration is the distribution of electrons in the atomic orbitals. It gives an idea about the shape and energy of electrons in 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 atoms 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 gets removed from the outermost subshell of an atom.

(e)

Expert Solution
Check Mark

Answer to Problem 8.28QP

The electronic configuration of Ca2+ 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 Ca is 20 and the electronic configuration is 1s22s22p63s23p64s2

For Ca2+, two electrons are removed from the outermost subshell. Hence, the atomic number becomes 18

Therefore,

The electronic configuration of Ca2+ is given as:

1s22s22p63s23p6

(f)

Interpretation Introduction

Interpretation:

Ground–state electronic configuration of Fe2+ has to be written.

Concept Introduction:

Electron configuration is the distribution of electrons in the atomic orbitals. It gives an idea about the shape and energy of electrons in 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 atoms 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 gets removed from the outermost subshell of an atom.

(f)

Expert Solution
Check Mark

Answer to Problem 8.28QP

The electronic configuration of Fe2+ is 1s22s22p63s23p63d6

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 Fe is 26 and the electronic configuration is 1s22s22p63s23p63d64s2

For Fe2+, two electrons are removed from the outermost subshell. Hence, the atomic number becomes 24

Therefore,

The electronic configuration of Fe2+ is given as:

1s22s22p63s23p63d6

(g)

Interpretation Introduction

Interpretation:

Ground–state electronic configuration of Cu2+ has to be written.

Concept Introduction:

Electron configuration is the distribution of electrons in the atomic orbitals. It gives an idea about the shape and energy of electrons in 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 atoms 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 gets removed from the outermost subshell of an atom.

(g)

Expert Solution
Check Mark

Answer to Problem 8.28QP

The electronic configuration of Cu2+ is 1s22s22p63s23p63d9

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 Cu is 29 and the electronic configuration is 1s22s22p63s23p63d104s1

For Cu2+, two electrons are removed from the outermost subshell. Hence, the atomic number becomes 27

Therefore,

The electronic configuration of Cu2+ is given as:

1s22s22p63s23p63d9

(h)

Interpretation Introduction

Interpretation:

Ground–state electronic configuration of Zn2+ has to be written.

Concept Introduction:

Electron configuration is the distribution of electrons in the atomic orbitals. It gives an idea about the shape and energy of electrons in 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 atoms 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 gets removed from the outermost subshell of an atom.

(h)

Expert Solution
Check Mark

Answer to Problem 8.28QP

The electronic configuration of Zn2+ is 1s22s22p63s23p63d10

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 Zn is 30 and the electronic configuration is 1s22s22p63s23p63d104s2

For Zn2+, two electrons are removed from the outermost subshell. Hence, the atomic number becomes 28

Therefore,

The electronic configuration of Zn2+ is given as:

1s22s22p63s23p63d10

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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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