CHEMISTRY: ATOMS FIRST VOL 1 W/CONNECT
CHEMISTRY: ATOMS FIRST VOL 1 W/CONNECT
14th Edition
ISBN: 9781259327933
Author: Burdge
Publisher: MCG
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Textbook Question
Chapter 4, Problem 4.84QP

Identify the atomic ground-state electron configurations that do not exist. For those that do exist, identify the element.

Chapter 4, Problem 4.84QP, Identify the atomic ground-state electron configurations that do not exist. For those that do exist,

(a)

Expert Solution
Check Mark
Interpretation Introduction

Interpretation: The atomic ground-state configuration that do not exist for the given sets need to be identified and the elements for atomic ground-state configuration that exists need to be identified.

Concept Introduction:

  • Electronic configuration is the arrangement of the electrons of atoms in the orbital.  For atoms and ions the electronic configuration are written by using Pauli Exclusion Principle and Hund’s rule.
  • According to Pauli Exclusion Principle, no two electrons having the same spin can occupy the same orbital.
  • According to Hund’s rule, the orbital in the subshell is filled singly by one electron before the same orbital is doubly filled.  When the orbitals is singly filled, all the electrons have same spin.  In a doubly filled orbital, there are two electrons with opposite spin.  The electrons are filled from lowest energy orbital first.
  • Half-filled orbitals are comparatively stable as completely filled orbitals.  Therefore if there is a possibility of forming half filled orbital then the electron will be moved to the respective orbitals giving rise to more stability instead of being incompletely filled orbital.
  • For simpler representation of ions or atoms, the electronic configuration of the completed octet noble gas configuration is considered and the remaining orbital alone is shown explicitly.  The ground-state configuration of the noble gases are given below,

[Ne] = 1s2 2s2 2p6[Ar] = 1s2 2s2 2p6 3s2 3p6[Kr] = 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6[Xe] = 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d105p6[Rn] = 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d105p6 6s2 4f14 5d10 6p6[Og] = 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d105p6 6s2 4f14 5d10 6p6 7s2 5f14 6d10 7p6

To identify: The given atomic ground-state configuration that do not exist and if it exists the element with the atomic ground-state configuration to be identified.

Answer to Problem 4.84QP

Answer

Atomic ground-state configuration exist for (a) and the element is identified as vanadium.

Explanation of Solution

Ground-state electronic configuration of the given element (a) is,

CHEMISTRY: ATOMS FIRST VOL 1 W/CONNECT, Chapter 4, Problem 4.84QP , additional homework tip  1

The atomic ground-state configuration is given in the problem statement.  From this we can find that this has a complete argon configuration along with two electrons in 4s orbital and three electrons in 3d subshell.  This is derived as shown above.  As the 3d subshell is filled singly, Hund’s rule is followed.  Hence this atomic ground-state configuration exists.

Element with the given atomic ground-state configuration is

CHEMISTRY: ATOMS FIRST VOL 1 W/CONNECT, Chapter 4, Problem 4.84QP , additional homework tip  2

Argon is a noble gas and has a complete octet electronic configuration as 1s22s22p63s23p6.  After the noble gas configuration, the given atomic ground-state configuration has two electrons in 4s orbital and three electrons in 3d subshell.  The filling of orbital in the subshell is done by following Hund’s rule and it complies with it.  The total number of electrons present in the given atomic ground-state configuration is 23.  The element with the atomic number 23 is identified as Vanadium.

(b)

Expert Solution
Check Mark
Interpretation Introduction

Interpretation: The atomic ground-state configuration that do not exist for the given sets need to be identified and the elements for atomic ground-state configuration that exists need to be identified.

Concept Introduction:

  • Electronic configuration is the arrangement of the electrons of atoms in the orbital.  For atoms and ions the electronic configuration are written by using Pauli Exclusion Principle and Hund’s rule.
  • According to Pauli Exclusion Principle, no two electrons having the same spin can occupy the same orbital.
  • According to Hund’s rule, the orbital in the subshell is filled singly by one electron before the same orbital is doubly filled.  When the orbitals is singly filled, all the electrons have same spin.  In a doubly filled orbital, there are two electrons with opposite spin.  The electrons are filled from lowest energy orbital first.
  • Half-filled orbitals are comparatively stable as completely filled orbitals.  Therefore if there is a possibility of forming half filled orbital then the electron will be moved to the respective orbitals giving rise to more stability instead of being incompletely filled orbital.
  • For simpler representation of ions or atoms, the electronic configuration of the completed octet noble gas configuration is considered and the remaining orbital alone is shown explicitly.  The ground-state configuration of the noble gases are given below,

[Ne] = 1s2 2s2 2p6[Ar] = 1s2 2s2 2p6 3s2 3p6[Kr] = 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6[Xe] = 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d105p6[Rn] = 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d105p6 6s2 4f14 5d10 6p6[Og] = 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d105p6 6s2 4f14 5d10 6p6 7s2 5f14 6d10 7p6

To identify: The given atomic ground-state configuration that do not exist and if it exists the element with the atomic ground-state configuration to be identified.

Answer to Problem 4.84QP

Answer

Atomic ground-state configuration does not exist for (b).

Explanation of Solution

Ground-state electronic configuration of (b)

CHEMISTRY: ATOMS FIRST VOL 1 W/CONNECT, Chapter 4, Problem 4.84QP , additional homework tip  3

The atomic ground-state configuration is given in the problem statement.  From this we can find that this has a complete neon configuration along with two electrons in 3s subshell and two electrons in 3p subshell.  This is derived as shown above.  From the above drawn configuration we can find that the all the orbitals in 3p subshell is not singly filled before pairing.  As this does not comply with Hund’s rule, the given atomic ground-state configuration does not exist.

(c)

Expert Solution
Check Mark
Interpretation Introduction

Interpretation: The atomic ground-state configuration that do not exist for the given sets need to be identified and the elements for atomic ground-state configuration that exists need to be identified.

Concept Introduction:

  • Electronic configuration is the arrangement of the electrons of atoms in the orbital.  For atoms and ions the electronic configuration are written by using Pauli Exclusion Principle and Hund’s rule.
  • According to Pauli Exclusion Principle, no two electrons having the same spin can occupy the same orbital.
  • According to Hund’s rule, the orbital in the subshell is filled singly by one electron before the same orbital is doubly filled.  When the orbitals is singly filled, all the electrons have same spin.  In a doubly filled orbital, there are two electrons with opposite spin.  The electrons are filled from lowest energy orbital first.
  • Half-filled orbitals are comparatively stable as completely filled orbitals.  Therefore if there is a possibility of forming half filled orbital then the electron will be moved to the respective orbitals giving rise to more stability instead of being incompletely filled orbital.
  • For simpler representation of ions or atoms, the electronic configuration of the completed octet noble gas configuration is considered and the remaining orbital alone is shown explicitly.  The ground-state configuration of the noble gases are given below,

[Ne] = 1s2 2s2 2p6[Ar] = 1s2 2s2 2p6 3s2 3p6[Kr] = 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6[Xe] = 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d105p6[Rn] = 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d105p6 6s2 4f14 5d10 6p6[Og] = 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d105p6 6s2 4f14 5d10 6p6 7s2 5f14 6d10 7p6

To identify: The given atomic ground-state configuration that do not exist and if it exists the element with the atomic ground-state configuration to be identified.

Answer to Problem 4.84QP

Answer

Atomic ground-state configuration does not exist for (c).

Explanation of Solution

Ground-state electronic configuration of the given element (c)

CHEMISTRY: ATOMS FIRST VOL 1 W/CONNECT, Chapter 4, Problem 4.84QP , additional homework tip  4

The atomic ground-state configuration is given in the problem statement.  From this we can find that this has a complete krypton configuration along with two electrons in “s” subshell and three electrons in “p” subshell.  This is derived as shown above.  From the above drawn configuration we can find that the filling of orbitals does not take place according to the increasing order of energy.  After filling of 5s orbital, 4d orbital has to be filled first before 5p orbital is getting filled.  But in this case 5p subshell is filled with electrons.  It does not comply with Hund’s rule and hence the given atomic ground-state configuration does not exist.

(d)

Expert Solution
Check Mark
Interpretation Introduction

Interpretation: The atomic ground-state configuration that do not exist for the given sets need to be identified and the elements for atomic ground-state configuration that exists need to be identified.

Concept Introduction:

  • Electronic configuration is the arrangement of the electrons of atoms in the orbital.  For atoms and ions the electronic configuration are written by using Pauli Exclusion Principle and Hund’s rule.
  • According to Pauli Exclusion Principle, no two electrons having the same spin can occupy the same orbital.
  • According to Hund’s rule, the orbital in the subshell is filled singly by one electron before the same orbital is doubly filled.  When the orbitals is singly filled, all the electrons have same spin.  In a doubly filled orbital, there are two electrons with opposite spin.  The electrons are filled from lowest energy orbital first.
  • Half-filled orbitals are comparatively stable as completely filled orbitals.  Therefore if there is a possibility of forming half filled orbital then the electron will be moved to the respective orbitals giving rise to more stability instead of being incompletely filled orbital.
  • For simpler representation of ions or atoms, the electronic configuration of the completed octet noble gas configuration is considered and the remaining orbital alone is shown explicitly.  The ground-state configuration of the noble gases are given below,

[Ne] = 1s2 2s2 2p6[Ar] = 1s2 2s2 2p6 3s2 3p6[Kr] = 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6[Xe] = 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d105p6[Rn] = 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d105p6 6s2 4f14 5d10 6p6[Og] = 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d105p6 6s2 4f14 5d10 6p6 7s2 5f14 6d10 7p6

To identify: The given atomic ground-state configuration that do not exist and if it exists the element with the atomic ground-state configuration to be identified.

Answer to Problem 4.84QP

Answer

Atomic ground-state configuration exists for (d) and the element is identified as phosphorous.

Explanation of Solution

Ground-state electronic configuration of the given element (d) is,

CHEMISTRY: ATOMS FIRST VOL 1 W/CONNECT, Chapter 4, Problem 4.84QP , additional homework tip  5

The atomic ground-state configuration is given in the problem statement.  From this we can find that this has a complete argon configuration along with two electrons in 4s orbital and three electrons in 3d orbital.  This is derived as shown above.  As the 3d subshell is filled singly, Hund’s rule is followed.  Hence this atomic ground-state configuration exists.

Element with the given atomic ground-state configuration

CHEMISTRY: ATOMS FIRST VOL 1 W/CONNECT, Chapter 4, Problem 4.84QP , additional homework tip  6

Neon is a noble gas and has a complete octet electronic configuration as 1s22s22p6.  After the noble gas configuration, the given atomic ground-state configuration has two electrons in 3s orbital and three electrons in 3p subshell.  The filling of orbital in the subshell is done by following Hund’s rule and it complies with it.  The total number of electrons present in the given atomic ground-state configuration is 15.  The element with the atomic number 15 is identified as Phosphorous.

(e)

Expert Solution
Check Mark
Interpretation Introduction

Interpretation: The atomic ground-state configuration that do not exist for the given sets need to be identified and the elements for atomic ground-state configuration that exists need to be identified.

Concept Introduction:

  • Electronic configuration is the arrangement of the electrons of atoms in the orbital.  For atoms and ions the electronic configuration are written by using Pauli Exclusion Principle and Hund’s rule.
  • According to Pauli Exclusion Principle, no two electrons having the same spin can occupy the same orbital.
  • According to Hund’s rule, the orbital in the subshell is filled singly by one electron before the same orbital is doubly filled.  When the orbitals is singly filled, all the electrons have same spin.  In a doubly filled orbital, there are two electrons with opposite spin.  The electrons are filled from lowest energy orbital first.
  • Half-filled orbitals are comparatively stable as completely filled orbitals.  Therefore if there is a possibility of forming half filled orbital then the electron will be moved to the respective orbitals giving rise to more stability instead of being incompletely filled orbital.
  • For simpler representation of ions or atoms, the electronic configuration of the completed octet noble gas configuration is considered and the remaining orbital alone is shown explicitly.  The ground-state configuration of the noble gases are given below,

[Ne] = 1s2 2s2 2p6[Ar] = 1s2 2s2 2p6 3s2 3p6[Kr] = 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6[Xe] = 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d105p6[Rn] = 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d105p6 6s2 4f14 5d10 6p6[Og] = 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d105p6 6s2 4f14 5d10 6p6 7s2 5f14 6d10 7p6

To identify: The given atomic ground-state configuration that do not exist and if it exists the element with the atomic ground-state configuration to be identified.

Answer to Problem 4.84QP

Answer

Atomic ground-state configuration does not exist for (e).

Explanation of Solution

Electronic configuration of given element (e) is,

CHEMISTRY: ATOMS FIRST VOL 1 W/CONNECT, Chapter 4, Problem 4.84QP , additional homework tip  7

The atomic ground-state configuration is given in the problem statement.  From this we can find that this has a complete argon configuration along with two electrons in 4s orbital and four electrons in 3d subshell.  This is derived as shown above.  As the 3d subshell is filled singly, Hund’s rule is followed.  Hence this configuration exists.

Atomic ground-state configuration

CHEMISTRY: ATOMS FIRST VOL 1 W/CONNECT, Chapter 4, Problem 4.84QP , additional homework tip  8

Argon is a noble gas and has a complete octet electronic configuration as 1s22s22p63s23p6.  After the noble gas configuration, the given atomic ground-state configuration has two electrons in 4s orbital and four electrons in 3d subshell.  The filling of orbital in the subshell is done by following Hund’s rule and it complies with it, that is shown above.  But in ground-state the filled subshell is less stable compared to the half filled subshell as highlighted in red colour.  Eventhough Hund’s rule is followed in filling of orbitals, the given atomic ground-state configuration in the problem statement does not exist because of the less stability of incompletely filled orbital compared to half filled orbitals.

(f)

Expert Solution
Check Mark
Interpretation Introduction

Interpretation: The atomic ground-state configuration that do not exist for the given sets need to be identified and the elements for atomic ground-state configuration that exists need to be identified.

Concept Introduction:

  • Electronic configuration is the arrangement of the electrons of atoms in the orbital.  For atoms and ions the electronic configuration are written by using Pauli Exclusion Principle and Hund’s rule.
  • According to Pauli Exclusion Principle, no two electrons having the same spin can occupy the same orbital.
  • According to Hund’s rule, the orbital in the subshell is filled singly by one electron before the same orbital is doubly filled.  When the orbitals is singly filled, all the electrons have same spin.  In a doubly filled orbital, there are two electrons with opposite spin.  The electrons are filled from lowest energy orbital first.
  • Half-filled orbitals are comparatively stable as completely filled orbitals.  Therefore if there is a possibility of forming half filled orbital then the electron will be moved to the respective orbitals giving rise to more stability instead of being incompletely filled orbital.
  • For simpler representation of ions or atoms, the electronic configuration of the completed octet noble gas configuration is considered and the remaining orbital alone is shown explicitly.  The ground-state configuration of the noble gases are given below,

[Ne] = 1s2 2s2 2p6[Ar] = 1s2 2s2 2p6 3s2 3p6[Kr] = 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6[Xe] = 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d105p6[Rn] = 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d105p6 6s2 4f14 5d10 6p6[Og] = 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d105p6 6s2 4f14 5d10 6p6 7s2 5f14 6d10 7p6

To identify: The given atomic ground-state configuration that do not exist and if it exists the element with the atomic ground-state configuration to be identified.

Answer to Problem 4.84QP

Answer

Atomic ground-state configuration exists for (f) and the element is identified as silver.

Explanation of Solution

Ground-state electronic configuration of given element (f) is,

CHEMISTRY: ATOMS FIRST VOL 1 W/CONNECT, Chapter 4, Problem 4.84QP , additional homework tip  9

The atomic ground-state configuration is given in the problem statement.  From this we can find that this has a complete Krypton configuration along with one electrons in 5s orbital and ten electrons in 4d subshell.  This is derived as shown above.  As the filling of subshells follows the Hund’s rule, the given atomic ground-state configuration exist.

Element with the given atomic ground-state configuration

CHEMISTRY: ATOMS FIRST VOL 1 W/CONNECT, Chapter 4, Problem 4.84QP , additional homework tip  10

Argon is a noble gas and has a complete octet electronic configuration as 1s22s22p63s23p6.  After the noble gas configuration, the given atomic ground-state configuration has one electron in 5s orbital and ten electrons in 4d subshell.  The filling of orbital in the subshell is done by following Hund’s rule and it complies with it.  The total number of electrons present in the given atomic ground-state configuration is 47.  The element with the atomic number 47 is identified as Silver.

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Chapter 4 Solutions

CHEMISTRY: ATOMS FIRST VOL 1 W/CONNECT

Ch. 4.2 - Prob. 2PPCCh. 4.2 - Prob. 4.2.1SRCh. 4.2 - Prob. 4.2.2SRCh. 4.4 - Referring only to a periodic table, arrange the...Ch. 4.4 - Prob. 3PPACh. 4.4 - Prob. 3PPBCh. 4.4 - Prob. 3PPCCh. 4.4 - Prob. 4.4WECh. 4.4 - Which element. Mg or Al, will have the higher...Ch. 4.4 - Explain why Rb has a lower IE1 than Sr, but Sr has...Ch. 4.4 - Imagine an arrangement of atomic orbitals in an...Ch. 4.4 - For each pair of elements, indicate which one you...Ch. 4.4 - Prob. 5PPACh. 4.4 - Explain why the EA1 for Ge is greater than the EA1...Ch. 4.4 - In the same hypothetical arrangement described in...Ch. 4.4 - For carbon and nitrogen, use the effective nuclear...Ch. 4.4 - Between which two charges is the attractive force...Ch. 4.4 - What must the distance be between charges of +2.25...Ch. 4.4 - Rank these pairs of charged objects in order of...Ch. 4.4 - Prob. 4.4.1SRCh. 4.4 - Prob. 4.4.2SRCh. 4.4 - Prob. 4.4.3SRCh. 4.4 - Prob. 4.4.4SRCh. 4.4 - Prob. 4.4.5SRCh. 4.4 - Prob. 4.4.6SRCh. 4.5 - Write electron configurations for the following...Ch. 4.5 - Write electron configurations for (a) O2, (b)...Ch. 4.5 - Prob. 7PPBCh. 4.5 - Prob. 7PPCCh. 4.5 - Prob. 4.8WECh. 4.5 - Prob. 8PPACh. 4.5 - Prob. 8PPBCh. 4.5 - Select the correct valence orbital diagram for the...Ch. 4.5 - Prob. 4.5.1SRCh. 4.5 - Prob. 4.5.2SRCh. 4.5 - Prob. 4.5.3SRCh. 4.5 - Prob. 4.5.4SRCh. 4.5 - Prob. 4.5.5SRCh. 4.6 - Identify the isoelectronic series in the following...Ch. 4.6 - Arrange the following isoelectronic series in...Ch. 4.6 - List all the common ions that are isoelectronic...Ch. 4.6 - Prob. 9PPCCh. 4.6 - Prob. 4.6.1SRCh. 4.6 - Prob. 4.6.2SRCh. 4.6 - Prob. 4.6.3SRCh. 4.6 - Prob. 4.6.4SRCh. 4 - Briefly describe the significance of Mendeleevs...Ch. 4 - What is Moseleys contribution to the modem...Ch. 4 - Describe the general layout of a modern periodic...Ch. 4 - What is the most important relationship among...Ch. 4 - Prob. 4.5QPCh. 4 - Prob. 4.6QPCh. 4 - Prob. 4.7QPCh. 4 - Prob. 4.8QPCh. 4 - Without referring to a periodic table, write the...Ch. 4 - Prob. 4.10QPCh. 4 - Prob. 4.11QPCh. 4 - Prob. 4.12QPCh. 4 - For centuries, arsenic has been the poison of...Ch. 4 - In the periodic table, the element hydrogen is...Ch. 4 - An atom of a certain clement has 16 electrons....Ch. 4 - Prob. 4.16QPCh. 4 - Prob. 4.17QPCh. 4 - Prob. 4.18QPCh. 4 - Prob. 4.19QPCh. 4 - For each of the following ground-state electron...Ch. 4 - Determine what element is designated by each of...Ch. 4 - Prob. 4.22QPCh. 4 - Explain why there is a greater increase in...Ch. 4 - The election configuration of B is1s22s22p1. (a)...Ch. 4 - The election configuration of C is1s22s22p1. (a)...Ch. 4 - Prob. 4.26QPCh. 4 - Prob. 4.27QPCh. 4 - Equation 4.2 is used to calculate the force...Ch. 4 - Use the second period of the periodic table as an...Ch. 4 - Prob. 4.30QPCh. 4 - Prob. 4.31QPCh. 4 - Prob. 4.32QPCh. 4 - Prob. 4.33QPCh. 4 - Prob. 4.34QPCh. 4 - Prob. 4.35QPCh. 4 - Prob. 4.36QPCh. 4 - Prob. 4.37QPCh. 4 - Prob. 4.38QPCh. 4 - Prob. 4.39QPCh. 4 - Consider two ions with opposite charges separated...Ch. 4 - Prob. 4.41QPCh. 4 - Prob. 4.42QPCh. 4 - Prob. 4.43QPCh. 4 - On the basis of their positions in the periodic...Ch. 4 - Prob. 4.45QPCh. 4 - Prob. 4.46QPCh. 4 - Prob. 4.47QPCh. 4 - Prob. 4.48QPCh. 4 - Prob. 4.49QPCh. 4 - Prob. 4.50QPCh. 4 - Prob. 4.51QPCh. 4 - Prob. 4.52QPCh. 4 - In general, the first ionization energy increases...Ch. 4 - Prob. 4.54QPCh. 4 - Prob. 4.55QPCh. 4 - Prob. 4.56QPCh. 4 - Prob. 4.57QPCh. 4 - Prob. 4.58QPCh. 4 - Specify which of the following elements you would...Ch. 4 - Considering their electron affinities, do you...Ch. 4 - Prob. 4.61QPCh. 4 - Prob. 4.62QPCh. 4 - Prob. 4.63QPCh. 4 - Prob. 4.64QPCh. 4 - Prob. 4.65QPCh. 4 - Prob. 4.66QPCh. 4 - Prob. 4.67QPCh. 4 - Prob. 4.68QPCh. 4 - Prob. 4.69QPCh. 4 - Write the ground-state electron configurations of...Ch. 4 - Write the ground-state electron configurations of...Ch. 4 - Prob. 4.72QPCh. 4 - Prob. 4.73QPCh. 4 - Identify the ions, each with a net charge of +1,...Ch. 4 - Prob. 4.75QPCh. 4 - Prob. 4.76QPCh. 4 - Group the species that are isoelectronic: Be2+, F,...Ch. 4 - For each pair of ions, determine which will have...Ch. 4 - Rank the following ions in order of increasing...Ch. 4 - Prob. 4.80QPCh. 4 - Prob. 4.81QPCh. 4 - Prob. 4.82QPCh. 4 - A metal ion with a net +3 charge has five...Ch. 4 - Identify the atomic ground-state electron...Ch. 4 - Each of the following ground-state electron...Ch. 4 - Prob. 4.86QPCh. 4 - Prob. 4.87QPCh. 4 - Prob. 4.88QPCh. 4 - Indicate which one of the two species in each of...Ch. 4 - Prob. 4.90QPCh. 4 - Prob. 4.91QPCh. 4 - Prob. 4.92QPCh. 4 - Prob. 4.93QPCh. 4 - Prob. 4.94QPCh. 4 - Prob. 4.95QPCh. 4 - Prob. 4.96QPCh. 4 - Prob. 4.97QPCh. 4 - Prob. 4.98QPCh. 4 - Prob. 4.99QPCh. 4 - Prob. 4.100QPCh. 4 - Arrange the following species in isoelectronic...Ch. 4 - Prob. 4.102QPCh. 4 - Prob. 4.103QPCh. 4 - Prob. 4.104QPCh. 4 - Prob. 4.105QPCh. 4 - Prob. 4.106QPCh. 4 - Prob. 4.107QPCh. 4 - Prob. 4.108QPCh. 4 - Contrary to the generalized trend that atomic...Ch. 4 - Prob. 4.110QPCh. 4 - Prob. 4.111QPCh. 4 - Prob. 4.112QPCh. 4 - Prob. 4.113QPCh. 4 - Prob. 4.114QPCh. 4 - Prob. 4.115QPCh. 4 - Prob. 4.116QPCh. 4 - Prob. 4.117QPCh. 4 - Prob. 4.118QPCh. 4 - Prob. 4.119QPCh. 4 - The energy needed for the following process is...Ch. 4 - Using your knowledge of the periodic trends with...Ch. 4 - Prob. 4.122QPCh. 4 - Prob. 4.123QPCh. 4 - Prob. 4.124QPCh. 4 - Explain, in terms of their electron...Ch. 4 - Prob. 4.126QPCh. 4 - Prob. 4.127QPCh. 4 - This graph charts the first six ionization...Ch. 4 - Prob. 4.129QPCh. 4 - Prob. 4.130QPCh. 4 - Prob. 4.131QPCh. 4 - Prob. 4.132QPCh. 4 - Predict the atomic number and ground-state...Ch. 4 - Prob. 4.134QPCh. 4 - Prob. 4.135QPCh. 4 - Prob. 4.136QPCh. 4 - The first six ionizations of a gaseous atom can be...Ch. 4 - Prob. 4.138QPCh. 4 - Prob. 4.139QPCh. 4 - Prob. 4.1KSPCh. 4 - Prob. 4.2KSPCh. 4 - Prob. 4.3KSPCh. 4 - Prob. 4.4KSP
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