General Chemistry
General Chemistry
7th Edition
ISBN: 9780073402758
Author: Chang, Raymond/ Goldsby
Publisher: McGraw-Hill College
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Chapter 7, Problem 7.83QP

(a)

Interpretation Introduction

Interpretation:

The ground-state electron configurations for the given elements should be identified.

Concept Introduction:

An orbital is an area of space in which electrons are orderly filled.  The maximum capacity in any type of orbital is two electrons.  An atomic orbital is defined as the region of space in which the probability of finding the electrons is highest.  It is subdivided into four orbitals such as s, p, d and f orbitals which depend upon the number of electrons present in the nucleus of a particular atom.

There are three basic principles in which orbitals are filled by the electrons.

  1. 1. Aufbau principle: In German, the word 'aufbau' means 'building up'.  The electrons are arranged in various orbitals in the order of increasing energies.
  2. 2. Pauli exclusion principle: An electron does not have all the four quantum numbers.
  3. 3. Hund’s rule: Each orbital is singly engaged with one electron having the maximum same spin capacity after that only pairing occurs.

The electron configuration is the allocation of electrons of an atom in atomic orbitals.  Electronic configuration of a particular atom is written by following the three basic principles.

To find: Identify the ground-state electron configuration for B

(a)

Expert Solution
Check Mark

Answer to Problem 7.83QP

The ground-state electron configuration for B is 1s22s22p1

Explanation of Solution

Boron (B) is placed in IIIA group of the periodic table. Its atomic number is 5.  Therefore, boron has five electrons in its shells.  Boron (B) is a p-block element.  So, its outermost electrons are located in a p-subshell.  

Put all the 5 electrons in the atomic orbitals by following Aufbau principle, Pauli exclusion principle and Hund’s rule

General Chemistry, Chapter 7, Problem 7.83QP , additional homework tip  1

All the 5 electrons of boron (B) occupy the atomic orbitals from lowest energy to highest energy orbitals.  The maximum capacity of each orbital has two electrons which have opposite spins.  s-atomic orbitals have a single shell whereas p-atomic orbitals have three sub-shells.  The 5 electrons are going into the 1s-atomic orbitals first, followed by 2s-atomic orbitals which are again followed by 2p-atomic orbitals.  Blue colored orbital corresponds to 1s-atomic orbital.  Black colored orbital corresponds to 2s-atomic orbital.  Red colored orbital corresponds to 2p-atomic orbitals.

There are 2 electrons present in 1s-atomic orbital, two electrons in 2s-atomic orbital and one electron in 2p-atomic orbital.  Therefore, the ground-state electron configuration for B is 1s22s22p1.

(b)

Interpretation Introduction

Interpretation:

The ground-state electron configurations for the given elements should be identified.

Concept Introduction:

An orbital is an area of space in which electrons are orderly filled.  The maximum capacity in any type of orbital is two electrons.  An atomic orbital is defined as the region of space in which the probability of finding the electrons is highest.  It is subdivided into four orbitals such as s, p, d and f orbitals which depend upon the number of electrons present in the nucleus of a particular atom.

There are three basic principles in which orbitals are filled by the electrons.

  1. 1. Aufbau principle: In German, the word 'aufbau' means 'building up'.  The electrons are arranged in various orbitals in the order of increasing energies.
  2. 2. Pauli exclusion principle: An electron does not have all the four quantum numbers.
  3. 3. Hund’s rule: Each orbital is singly engaged with one electron having the maximum same spin capacity after that only pairing occurs.

The electron configuration is the allocation of electrons of an atom in atomic orbitals.  Electronic configuration of a particular atom is written by following the three basic principles.

To find: Identify the ground-state electron configuration for V

(b)

Expert Solution
Check Mark

Answer to Problem 7.83QP

The ground-state electron configuration for V is [Ar]3d34s2

Explanation of Solution

Vanadium (V) is placed in VB group of the periodic table. Its atomic number is 23.  Therefore, vanadium has 23 electrons in its shells.  Vanadium (V) is a d-block element.  So, its outermost electrons are located in a d-subshell.  

The noble gas core for V is [Ar], where atomic number of Ar is 18.  So, the order of filling beyond the noble gas core is 4s and 3d. The electrons in V beyond its noble gas core are (23 – 18) = 5 electrons.  These 5 electrons enter into the 4s and 3d subshells.

Put all the 5 electrons in the atomic orbitals by following Aufbau principle, Pauli exclusion principle and Hund’s rule.

General Chemistry, Chapter 7, Problem 7.83QP , additional homework tip  2

All the 5 electrons of vanadium (V) occupy the atomic orbitals from lowest energy to highest energy orbitals.  The maximum capacity of each orbital has two electrons which have opposite spins.  s-atomic orbitals have a single shell whereas d-atomic orbitals have five sub-shells.  The 5 electrons are going into the 4s-atomic orbitals first, followed by 3d-atomic orbitals.  Blue colored orbital corresponds to 4s-atomic orbital.  Black colored orbital corresponds to 3d-atomic orbital. 

There are 2 electrons present in 4s-atomic orbital, three electrons in 3d-atomic orbital.  Therefore, the ground-state electron configuration for V is [Ar]3d34s2.

(c)

Interpretation Introduction

Interpretation:

The ground-state electron configurations for the given elements should be identified.

Concept Introduction:

An orbital is an area of space in which electrons are orderly filled.  The maximum capacity in any type of orbital is two electrons.  An atomic orbital is defined as the region of space in which the probability of finding the electrons is highest.  It is subdivided into four orbitals such as s, p, d and f orbitals which depend upon the number of electrons present in the nucleus of a particular atom.

There are three basic principles in which orbitals are filled by the electrons.

  1. 1. Aufbau principle: In German, the word 'aufbau' means 'building up'.  The electrons are arranged in various orbitals in the order of increasing energies.
  2. 2. Pauli exclusion principle: An electron does not have all the four quantum numbers.
  3. 3. Hund’s rule: Each orbital is singly engaged with one electron having the maximum same spin capacity after that only pairing occurs.

The electron configuration is the allocation of electrons of an atom in atomic orbitals.  Electronic configuration of a particular atom is written by following the three basic principles.

To find: Identify the ground-state electron configuration for C

(c)

Expert Solution
Check Mark

Answer to Problem 7.83QP

The ground-state electron configuration for C is 1s22s22p2

Explanation of Solution

Carbon (C) is placed in IVA group of the periodic table. Its atomic number is 6.  Therefore, carbon has six electrons in its shells.  Carbon (C) is a p-block element.  So, its outermost electrons are located in a p-subshell.  

Put all the 6 electrons in the atomic orbitals by following Aufbau principle, Pauli exclusion principle and Hund’s rule.

General Chemistry, Chapter 7, Problem 7.83QP , additional homework tip  3

All the 6 electrons of carbon (C) occupy the atomic orbitals from lowest energy to highest energy orbitals.  The maximum capacity of each orbital has two electrons which have opposite spins.  s-atomic orbitals have a single shell whereas p-atomic orbitals have three sub-shells.  The 6 electrons are going into the 1s-atomic orbitals first, followed by 2s-atomic orbitals which are again followed by 2p-atomic orbitals.  Blue colored orbital corresponds to 1s-atomic orbital.  Black colored orbital corresponds to 2s-atomic orbital.  Red colored orbital corresponds to 2p-atomic orbitals.

There are 2 electrons present in 1s-atomic orbital, two electrons in 2s-atomic orbital and two electrons in 2p-atomic orbital.  Therefore, the ground-state electron configuration for C is 1s22s22p2.

(d)

Interpretation Introduction

Interpretation:

The ground-state electron configurations for the given elements should be identified.

Concept Introduction:

An orbital is an area of space in which electrons are orderly filled.  The maximum capacity in any type of orbital is two electrons.  An atomic orbital is defined as the region of space in which the probability of finding the electrons is highest.  It is subdivided into four orbitals such as s, p, d and f orbitals which depend upon the number of electrons present in the nucleus of a particular atom.

There are three basic principles in which orbitals are filled by the electrons.

  1. 1. Aufbau principle: In German, the word 'aufbau' means 'building up'.  The electrons are arranged in various orbitals in the order of increasing energies.
  2. 2. Pauli exclusion principle: An electron does not have all the four quantum numbers.
  3. 3. Hund’s rule: Each orbital is singly engaged with one electron having the maximum same spin capacity after that only pairing occurs.

The electron configuration is the allocation of electrons of an atom in atomic orbitals.  Electronic configuration of a particular atom is written by following the three basic principles.

To find: Identify the ground-state electron configuration for As

(d)

Expert Solution
Check Mark

Answer to Problem 7.83QP

The ground-state electron configuration for As is [Ar]3d104s24p3

Explanation of Solution

Arsenic (As) is placed in VA group of the periodic table. Its atomic number is 33.  Therefore, arsenic has 33 electrons in its shells.  Arsenic (As) is a p-block element.  So, its outermost electrons are located in a p-subshell.  

The noble gas core for As is [Ar], where atomic number of Ar is 18.  So, the order of filling beyond the noble gas core is 4s,3d and 4p. The electrons in As beyond its noble gas core are (33 – 18) = 15 electrons.  These 15 electrons enter into the 4s,3d and 4p subshells.

Put all the 15 electrons in the atomic orbitals by following Aufbau principle, Pauli exclusion principle and Hund’s rule.

General Chemistry, Chapter 7, Problem 7.83QP , additional homework tip  4

All the 15 electrons of arsenic (As) occupy the atomic orbitals from lowest energy to highest energy orbitals.  The maximum capacity of each orbital has two electrons which have opposite spins.  s-atomic orbitals have a single shell whereas p-atomic orbitals have three sub-shells.  d-atomic orbitals have five sub-shells.  The 15 electrons are going into the 4s-atomic orbitals first, followed by 3d-atomic orbitals which is again followed by 4p- atomic orbitals.  Blue colored orbital corresponds to 4s-atomic orbital.  Black colored orbital corresponds to 3d-atomic orbital.  Red colored orbital corresponds to 4p-atomic orbitals.

There are 2 electrons present in 4s-atomic orbital, ten electrons in 3d-atomic orbitals and three electrons in 4p-atomic orbitals.  Therefore, the ground-state electron configuration for As is [Ar]3d104s24p3.

(e)

Interpretation Introduction

Interpretation:

The ground-state electron configurations for the given elements should be identified.

Concept Introduction:

An orbital is an area of space in which electrons are orderly filled.  The maximum capacity in any type of orbital is two electrons.  An atomic orbital is defined as the region of space in which the probability of finding the electrons is highest.  It is subdivided into four orbitals such as s, p, d and f orbitals which depend upon the number of electrons present in the nucleus of a particular atom.

There are three basic principles in which orbitals are filled by the electrons.

  1. 1. Aufbau principle: In German, the word 'aufbau' means 'building up'.  The electrons are arranged in various orbitals in the order of increasing energies.
  2. 2. Pauli exclusion principle: An electron does not have all the four quantum numbers.
  3. 3. Hund’s rule: Each orbital is singly engaged with one electron having the maximum same spin capacity after that only pairing occurs.

The electron configuration is the allocation of electrons of an atom in atomic orbitals.  Electronic configuration of a particular atom is written by following the three basic principles.

To find: Identify the ground-state electron configuration for I

(e)

Expert Solution
Check Mark

Answer to Problem 7.83QP

The ground-state electron configuration for I is [Kr]4d105s25p5

Explanation of Solution

Iodine (I) is placed in VIIA group of the periodic table. Its atomic number is 53.  Therefore, iodine has 53 electrons in its shells.  Iodine (I) is a p-block element.  So, its outermost electrons are located in a p-subshell.  

The noble gas core for I is [Kr], where atomic number of Kr is 36.  So, the order of filling beyond the noble gas core is 5s, 4d and 5p. The electrons in I beyond its noble gas core is (53 – 36) = 17 electrons.  These 17 electrons enter into the 5s, 4d and 5p subshells.

Put all the 17 electrons in the atomic orbitals by following Aufbau principle, Pauli exclusion principle and Hund’s rule.

General Chemistry, Chapter 7, Problem 7.83QP , additional homework tip  5

All the 17 electrons of iodine (I) occupy the atomic orbitals from lowest energy to highest energy orbitals.  The maximum capacity of each orbital has two electrons which have opposite spins.  s-atomic orbitals have a single shell whereas p-atomic orbitals have three sub-shells.  d-atomic orbitals have five sub-shells.  The 17 electrons are going into the 5s-atomic orbitals first, followed by 4d-atomic orbitals which is again followed by 5p- atomic orbitals.  Blue colored orbital corresponds to 5s-atomic orbital.  Black colored orbital corresponds to 4d-atomic orbital.  Red colored orbital corresponds to 5p-atomic orbitals.

There are 2 electrons present in 5s-atomic orbital, ten electrons in 4d-atomic orbitals and five electrons in 5p-atomic orbitals.  Therefore, the ground-state electron configuration for I is [Kr]4d105s25p5.

(f)

Interpretation Introduction

Interpretation:

The ground-state electron configurations for the given elements should be identified.

Concept Introduction:

An orbital is an area of space in which electrons are orderly filled.  The maximum capacity in any type of orbital is two electrons.  An atomic orbital is defined as the region of space in which the probability of finding the electrons is highest.  It is subdivided into four orbitals such as s, p, d and f orbitals which depend upon the number of electrons present in the nucleus of a particular atom.

There are three basic principles in which orbitals are filled by the electrons.

  1. 1. Aufbau principle: In German, the word 'aufbau' means 'building up'.  The electrons are arranged in various orbitals in the order of increasing energies.
  2. 2. Pauli exclusion principle: An electron does not have all the four quantum numbers.
  3. 3. Hund’s rule: Each orbital is singly engaged with one electron having the maximum same spin capacity after that only pairing occurs.

The electron configuration is the allocation of electrons of an atom in atomic orbitals.  Electronic configuration of a particular atom is written by following the three basic principles.

To find: Identify the ground-state electron configuration for Au

(f)

Expert Solution
Check Mark

Answer to Problem 7.83QP

The ground-state electron configuration for Au is [Xe]4f145d106s1

Explanation of Solution

Gold (Au) is placed in IB group of the periodic table.  Its atomic number is 79.  Therefore, gold has 79 electrons in its shells.  Gold (Au) is a d-block element.  So, its outermost electrons are located in a d-subshell.  

The noble gas core for Au is [Xe], where atomic number of Xe is 54.  So, the order of filling beyond the noble gas core is 4f, 5d and 6s. The electrons in Au beyond its noble gas core is (79 – 54) = 25 electrons.  These 25 electrons enter into the 4f, 5d and 6s subshells.

Put all the 25 electrons in the atomic orbitals by following Aufbau principle, Pauli exclusion principle and Hund’s rule.

General Chemistry, Chapter 7, Problem 7.83QP , additional homework tip  6

All the electrons of gold (Au) occupy the atomic orbitals from lowest energy to highest energy orbitals.  The maximum capacity of each orbital has two electrons which have opposite spins.  s-atomic orbitals have a single shell whereas d-atomic orbitals have five sub-shells.  f-atomic orbitals have seven sub-shells.  The 25 electrons are going into the 4f -atomic orbitals first, followed by 6s-atomic orbitals which are again followed by 5d-atomic orbitals.  Green colored orbital corresponds to 4f-atomic orbitals.  Blue colored orbital corresponds to 6s-atomic orbital.  Black colored orbital corresponds to 5d-atomic orbital.  One electron in 6s-orbital is jumped into the 5d-orbital because completely filled d-orbitals are more stable.

There are 14 electrons present in 4f-atomic orbital, one electron in 6s-atomic orbital and ten electrons in 5d-atomic orbital.  Therefore, the ground-state electron configuration of gold (Au) is [Xe]4f145d106s1.

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Chapter 7 Solutions

General Chemistry

Ch. 7.5 - Prob. 1RCCh. 7.6 - Prob. 1RCCh. 7.7 - Prob. 1PECh. 7.7 - Prob. 2PECh. 7.7 - Prob. 1RCCh. 7.8 - Prob. 1PECh. 7.8 - Prob. 2PECh. 7.8 - Prob. 3PECh. 7.8 - Prob. 1RCCh. 7.9 - Prob. 1PECh. 7.9 - Prob. 1RCCh. 7 - Prob. 7.1QPCh. 7 - Prob. 7.2QPCh. 7 - Prob. 7.3QPCh. 7 - Prob. 7.4QPCh. 7 - Prob. 7.5QPCh. 7 - Prob. 7.6QPCh. 7 - Prob. 7.7QPCh. 7 - 7.8 (a) What is the frequency of tight having a...Ch. 7 - Prob. 7.9QPCh. 7 - Prob. 7.10QPCh. 7 - Prob. 7.11QPCh. 7 - 7.12 The SI unit of length is the meter, which...Ch. 7 - 7.13 What are photons? What role did Einstein's...Ch. 7 - Prob. 7.14QPCh. 7 - Prob. 7.15QPCh. 7 - Prob. 7.16QPCh. 7 - Prob. 7.17QPCh. 7 - Prob. 7.18QPCh. 7 - Prob. 7.19QPCh. 7 - Prob. 7.20QPCh. 7 - Prob. 7.21QPCh. 7 - Prob. 7.22QPCh. 7 - Prob. 7.23QPCh. 7 - Prob. 7.24QPCh. 7 - Prob. 7.25QPCh. 7 - Prob. 7.26QPCh. 7 - Prob. 7.27QPCh. 7 - Prob. 7.28QPCh. 7 - Prob. 7.29QPCh. 7 - Prob. 7.30QPCh. 7 - Prob. 7.31QPCh. 7 - Prob. 7.32QPCh. 7 - Prob. 7.33QPCh. 7 - Prob. 7.34QPCh. 7 - Prob. 7.35QPCh. 7 - Prob. 7.36QPCh. 7 - Prob. 7.37QPCh. 7 - Prob. 7.38QPCh. 7 - Prob. 7.39QPCh. 7 - Prob. 7.40QPCh. 7 - Prob. 7.41QPCh. 7 - 7.42 What is the de Broglie wavelength (in nm)...Ch. 7 - Prob. 7.43QPCh. 7 - Prob. 7.44QPCh. 7 - Prob. 7.45QPCh. 7 - Prob. 7.46QPCh. 7 - Prob. 7.47QPCh. 7 - Prob. 7.48QPCh. 7 - 7.49 Why is a boundary surface diagram useful in...Ch. 7 - Prob. 7.50QPCh. 7 - Prob. 7.51QPCh. 7 - Prob. 7.52QPCh. 7 - Prob. 7.53QPCh. 7 - Prob. 7.54QPCh. 7 - Prob. 7.55QPCh. 7 - Prob. 7.56QPCh. 7 - Prob. 7.57QPCh. 7 - 7.58 What is the difference between a 2px and a...Ch. 7 - Prob. 7.59QPCh. 7 - Prob. 7.60QPCh. 7 - Prob. 7.61QPCh. 7 - Prob. 7.62QPCh. 7 - Prob. 7.63QPCh. 7 - Prob. 7.64QPCh. 7 - 7.65 Make a chart of all allowable orbitals in the...Ch. 7 - 7.66 Why do the 3s, 3p, and 3d orbitals have the...Ch. 7 - Prob. 7.67QPCh. 7 - Prob. 7.68QPCh. 7 - Prob. 7.69QPCh. 7 - Prob. 7.70QPCh. 7 - Prob. 7.71QPCh. 7 - Prob. 7.72QPCh. 7 - Prob. 7.73QPCh. 7 - Prob. 7.74QPCh. 7 - Prob. 7.75QPCh. 7 - Prob. 7.76QPCh. 7 - Prob. 7.77QPCh. 7 - 7.78 Comment on the correctness of the following...Ch. 7 - Prob. 7.79QPCh. 7 - Prob. 7.80QPCh. 7 - Prob. 7.81QPCh. 7 - Prob. 7.82QPCh. 7 - Prob. 7.83QPCh. 7 - Prob. 7.84QPCh. 7 - Prob. 7.85QPCh. 7 - Prob. 7.86QPCh. 7 - Prob. 7.87QPCh. 7 - Prob. 7.88QPCh. 7 - Prob. 7.89QPCh. 7 - Prob. 7.90QPCh. 7 - Prob. 7.91QPCh. 7 - Prob. 7.92QPCh. 7 - Prob. 7.93QPCh. 7 - Prob. 7.94QPCh. 7 - 7.95 Identify the following individuals and their...Ch. 7 - Prob. 7.96QPCh. 7 - Prob. 7.97QPCh. 7 - Prob. 7.98QPCh. 7 - Prob. 7.99QPCh. 7 - 7.100 A laser is used in treating retina...Ch. 7 - 7.101 A 368-g sample of water absorbs infrared...Ch. 7 - Prob. 7.102QPCh. 7 - Prob. 7.103QPCh. 7 - Prob. 7.104QPCh. 7 - Prob. 7.105QPCh. 7 - Prob. 7.106QPCh. 7 - Prob. 7.107QPCh. 7 - Prob. 7.108QPCh. 7 - Prob. 7.109QPCh. 7 - Prob. 7.110QPCh. 7 - Prob. 7.111QPCh. 7 - 7.112 An atom moving at its root-mean-square speed...Ch. 7 - Prob. 7.113QPCh. 7 - Prob. 7.114QPCh. 7 - Prob. 7.115QPCh. 7 - Prob. 7.116QPCh. 7 - Prob. 7.117SPCh. 7 - Prob. 7.118SPCh. 7 - Prob. 7.119SPCh. 7 - Prob. 7.120SPCh. 7 - 7.121 According to Einstein’s special theory of...Ch. 7 - Prob. 7.122SPCh. 7 - Prob. 7.123SPCh. 7 - Prob. 7.124SPCh. 7 - Prob. 7.125SPCh. 7 - 7.126 The wave function for the 2s orbital in the...Ch. 7 - Prob. 7.127SPCh. 7 - Prob. 7.128SPCh. 7 - Prob. 7.129SP
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