General Chemistry
General Chemistry
7th Edition
ISBN: 9780073402758
Author: Chang, Raymond/ Goldsby
Publisher: McGraw-Hill College
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Chapter 8, Problem 8.29QP

(a)

Interpretation Introduction

Interpretation:

Ground–state electronic configuration of Sc3+ 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 get removed from the outermost subshell of an atom.

(a)

Expert Solution
Check Mark

Answer to Problem 8.29QP

The electronic configuration of Sc3+ 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 Sc is 21 and the electronic configuration is 1s22s22p63s23p63d1 4s2

For Sc3+, three electrons are removed from the outermost subshell. Hence, the atomic number becomes 18

Therefore,

The electronic configuration of Sc3+ is given as: 1s22s22p63s23p6

(b)

Interpretation Introduction

Interpretation:

Ground–state electronic configuration of Ti4+ 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 get removed from the outermost subshell of an atom.

(b)

Expert Solution
Check Mark

Answer to Problem 8.29QP

The electronic configuration of Ti4+ 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 Ti is 22 and the electronic configuration is 1s22s22p63s23p63d24s2

For Ti4+, four electrons are removed from the outermost subshell. Hence, the atomic number becomes 18

Therefore,

The electronic configuration of Ti4+ is given as:

1s22s22p63s23p6

(c)

Interpretation Introduction

Interpretation:

Ground–state electronic configuration of V5+ 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 get removed from the outermost subshell of an atom.

(c)

Expert Solution
Check Mark

Answer to Problem 8.29QP

The electronic configuration of V5+ 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 V is 23 and the electronic configuration is 1s22s22p63s23p63d34s2

For V5+, five electrons are removed from the outermost subshell. Hence, the atomic number becomes 18

Therefore,

The electronic configuration of V5+ is given as:

1s22s22p63s23p6

(d)

Interpretation Introduction

Interpretation:

Ground–state electronic configuration of Cr3+ 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 get removed from the outermost subshell of an atom.

(d)

Expert Solution
Check Mark

Answer to Problem 8.29QP

The electronic configuration of Cr3+ is 1s22s22p63s23p63d3

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 chromium is 24 an the electronic configuration is 1s22s22p63s23p64s13d5

For Cr3+, three electrons are removed from the outermost subshell. Hence, the atomic number becomes 21

Therefore,

The electronic configuration of Cr3+ is given as:

1s22s22p63s23p63d3

(e)

Interpretation Introduction

Interpretation:

Ground–state electronic configuration of Mn2+ 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 get removed from the outermost subshell of an atom.

(e)

Expert Solution
Check Mark

Answer to Problem 8.29QP

The electronic configuration of Mn2+ is 1s22s22p63s23p63d5

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 Mn is 25 and the electronic configuration is 1s22s22p63s23p63d54s2

For Mn2+, two electrons are removed from the outermost subshell. Hence, the atomic number becomes 23

Therefore,

The electronic configuration of Mn2+ is given as:

1s22s22p63s23p63d5

(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 get removed from the outermost subshell of an atom.

(f)

Expert Solution
Check Mark

Answer to Problem 8.29QP

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 Fe3+ 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 get removed from the outermost subshell of an atom.

(g)

Expert Solution
Check Mark

Answer to Problem 8.29QP

The electronic configuration of Fe3+ is 1s22s22p63s23p63d5

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 Fe3+, three electrons are removed from the outermost subshell. Hence, the atomic number becomes 23

Therefore,

The electronic configuration of Fe2+ is given as:

1s22s22p63s23p63d5

(h)

Interpretation Introduction

Interpretation:

Ground–state electronic configuration of Co2+ 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 get removed from the outermost subshell of an atom.

(h)

Expert Solution
Check Mark

Answer to Problem 8.29QP

The electronic configuration of Co2+ is 1s22s22p63s23p63d7

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 Co is 27 and the electronic configuration is 1s22s22p63s23p63d74s2

For Co2+, two electrons are removed from the outermost subshell. Hence, the atomic number becomes 25

Therefore,

The electronic configuration of Co2+ is given as:

1s22s22p63s23p63d7

(i)

Interpretation Introduction

Interpretation: Ground–state electronic configuration of Ni2+ 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 get removed from the outermost subshell of an atom.

(i)

Expert Solution
Check Mark

Answer to Problem 8.29QP

The electronic configuration of Ni2+ is 1s22s22p63s23p63d8

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 Ni is 28 and the electronic configuration is 1s22s22p63s23p63d84s2

For Ni2+, two electrons are removed from the outermost subshell. Hence, the atomic number becomes 26

Therefore,

The electronic configuration of Ni2+ is given as:

1s22s22p63s23p63d8

(j)

Interpretation Introduction

Interpretation:

Ground–state electronic configuration of Cu+ 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 get removed from the outermost subshell of an atom.

(j)

Expert Solution
Check Mark

Answer to Problem 8.29QP

The electronic configuration of Cu+ 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 Cu is 29 and the electronic configuration is 1s22s22p63s23p63d104s1

For Cu+, one electron is removed from the outermost subshell. Hence, the atomic number becomes 28

Therefore,

The electronic configuration of Cu+ is given as:

1s22s22p63s23p63d10

(k)

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 get removed from the outermost subshell of an atom.

(k)

Expert Solution
Check Mark

Answer to Problem 8.29QP

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

(l)

Interpretation Introduction

Interpretation:

Ground–state electronic configuration of Ag+ 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 get removed from the outermost subshell of an atom.

(l)

Expert Solution
Check Mark

Answer to Problem 8.29QP

The electronic configuration of Ag+ is [Kr]4d10

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 Ag is 47 and the electronic configuration is [Kr]4d105s2

For Ag+, one electron is removed from the outermost subshell. Hence, the atomic number becomes 46

Therefore,

The electronic configuration of Ag+ is given as:

[Kr]4d10

(m)

Interpretation Introduction

Interpretation:

Ground–state electronic configuration of Au+ 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 get removed from the outermost subshell of an atom.

(m)

Expert Solution
Check Mark

Answer to Problem 8.29QP

The electronic configuration of Au+ is [Xe]4f145d10

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 Au is 79 and the electronic configuration is [Xe]4f145d106s1

For Au+, one electron is removed from the outermost subshell. Hence, the atomic number becomes 78

Therefore,

The electronic configuration of Au+ is given as:

[Xe]4f145d10

(n)

Interpretation Introduction

Interpretation:

Ground–state electronic configuration of Au3+ 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 get removed from the outermost subshell of an atom.

(n)

Expert Solution
Check Mark

Answer to Problem 8.29QP

The electronic configuration of Au3+ is [Xe]4f145d8

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 Au is 79 and the electronic configuration is [Xe]4f145d106s1

For Au3+, three electrons are removed from the outermost subshell. Hence, the atomic number becomes 76

Therefore,

The electronic configuration of Au3+ is given as:

[Xe]4f145d8

(o)

Interpretation Introduction

Interpretation:

Ground–state electronic configuration of Pt2+ 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 get removed from the outermost subshell of an atom.

(o)

Expert Solution
Check Mark

Answer to Problem 8.29QP

The electronic configuration of Pt2+ is [Xe]4f145d8

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 Pt is 78 and the electronic configuration is [Xe]4f145d96s1

For Pt2+, two electrons are removed from the outermost subshell.  Hence, the atomic number becomes 76

Therefore,

The electronic configuration of Pt2+ is given as:

[Xe]4f145d8

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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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Publisher:Cengage Learning
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ISBN:9781259911156
Author:Raymond Chang Dr., Jason Overby Professor
Publisher:McGraw-Hill Education
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ISBN:9781305577213
Author:Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:Cengage Learning
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ISBN:9780078021558
Author:Janice Gorzynski Smith Dr.
Publisher:McGraw-Hill Education
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ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:Cengage Learning
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Elementary Principles of Chemical Processes, Bind...
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ISBN:9781118431221
Author:Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
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Stoichiometry - Chemistry for Massive Creatures: Crash Course Chemistry #6; Author: Crash Course;https://www.youtube.com/watch?v=UL1jmJaUkaQ;License: Standard YouTube License, CC-BY
Bonding (Ionic, Covalent & Metallic) - GCSE Chemistry; Author: Science Shorts;https://www.youtube.com/watch?v=p9MA6Od-zBA;License: Standard YouTube License, CC-BY
General Chemistry 1A. Lecture 12. Two Theories of Bonding.; Author: UCI Open;https://www.youtube.com/watch?v=dLTlL9Z1bh0;License: CC-BY