Chemistry & Chemical Reactivity
Chemistry & Chemical Reactivity
9th Edition
ISBN: 9781133949640
Author: John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher: Cengage Learning
Question
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Chapter 7, Problem 18PS

(a)

Interpretation Introduction

Interpretation:

The electronic configuration has to be depicted for Na+ using orbital box diagram and noble gas electronic configuration method.

Concept Introduction:

Electronic configuration: The electronic configuration is the distribution of electrons of an given molecule or respective atoms in atomic or molecular orbitals.

Aufbau principle: This rule statues that ground state of an atom or ions electrons fill atomic orbitals of the lowest available energy levels before occupying higher levels. If consider the 1s shell is filled the 2s subshell is occupied.

Hund's Rule: The every orbital in a subshell is singly occupied with one electron before any one orbital is doubly occupied, and all electrons in singly occupied orbitals have the same spin.

Pauli exclusion rule: an atomic orbital may describe at most two electrons, each with opposite spin direction.

(a)

Expert Solution
Check Mark

Explanation of Solution

Let us consider the orbital filling method of Sodium (Na+) ions.

Given the Sodium atom has loss of one electron from outermost shells.

 Atomicnumberofsodium(Na)=11spdfwith orbtital notation=[1s22s22p63s1]Orbital filling method       1s22s22p63s1spdfwith noble gas notation=[Ne]3s1Orbitalboxnotation       = [Ne]3s1

When (Na) was oxidized to (Na+) ions, it lose one electron from outermost (3s) orbitals, hence this orbital notation method shows below.

   Atomicnumberofsodium(Na)=11spdfwith orbtital notation=[1s22s22p63s0]Orbital filling method       1s22s22p53s0spdfwith noble gas notation=[Ne]3s0Orbitalboxnotation       = [Ne]3s0

Hence, the electronic configuration of Sodium ions (Na+) = 1s22s22p63s0 and noble gas configuration of [Ne]3s0 

(b)

Interpretation Introduction

Interpretation:

The electronic configuration has to be depicted for Al3+ using orbital box diagram and noble gas electronic configuration method.

Concept Introduction:

Electronic configuration: The electronic configuration is the distribution of electrons of an given molecule or respective atoms in atomic or molecular orbitals.

Aufbau principle: This rule statues that ground state of an atom or ions electrons fill atomic orbitals of the lowest available energy levels before occupying higher levels. If consider the 1s shell is filled the 2s subshell is occupied.

Hund's Rule: The every orbital in a subshell is singly occupied with one electron before any one orbital is doubly occupied, and all electrons in singly occupied orbitals have the same spin.

Pauli exclusion rule: an atomic orbital may describe at most two electrons, each with opposite spin direction.

(b)

Expert Solution
Check Mark

Explanation of Solution

Let us consider the orbital filling method of Aluminium ions (Al3+) ions.

The single Aluminium toms having (13) electrons in (s, p, d) orbital shells and its atomic number (Z=13). Moreover the (Ge) atoms has loss of one electrons in outermost (4s, 4p) shells.

Hence we can write oxidation reaction has shown below.

               AtomicnumberofAluminium(Al)=13spdfwith orbtital notation=[1s22s22p63s23p1]Orbital filling method       1s22s22p63s23p1spdfwith noble gas notation=[Ne]3s23p1Orbitalboxnotation       = [Ne]3s23p1

When (Al) was oxidized to (Al3+) ions, it lose three electrons from outermost (3s and 3p) orbitals, hence this orbital notation method shows below.

              AtomicnumberofAluminium(Al)=13spdfwith orbtital notation=[1s22s22p63s03p0]Orbital filling method       1s22s22p63s03p0spdfwith noble gas notation=[Ne]3s03p0Orbitalboxnotation       = [Ne]3s03p0

Hence, the electronic configuration of Aluminium (III) ions (Al3+) = 1s22s22p63s03p0 and noble gas configuration of [Ne]3s03p0 

(c)

Interpretation Introduction

Interpretation:

The electronic configuration has to be depicted for Ge2+ using orbital box diagram and noble gas electronic configuration method.

Concept Introduction:

Electronic configuration: The electronic configuration is the distribution of electrons of an given molecule or respective atoms in atomic or molecular orbitals.

Aufbau principle: This rule statues that ground state of an atom or ions electrons fill atomic orbitals of the lowest available energy levels before occupying higher levels. If consider the 1s shell is filled the 2s subshell is occupied.

Hund's Rule: The every orbital in a subshell is singly occupied with one electron before any one orbital is doubly occupied, and all electrons in singly occupied orbitals have the same spin.

Pauli exclusion rule: an atomic orbital may describe at most two electrons, each with opposite spin direction.

(c)

Expert Solution
Check Mark

Explanation of Solution

 Let us consider the orbital filling method of Germanium ions (Ge2+) ions.

The single Ge atoms having (32) electrons in (s, p) orbital shells and its atomic number (Z=32). Moreover the (Ge) atoms has loss of two electrons in outermost (3p, 3s) shells.

Hence we can write gains of electron (Oxidation method) process are presented below.

  AtomicnumberofGermanium(Ge)=32spdfwith orbtital notation=[1s22s22p63s23p63d104s24p2]Orbital filling method       1s22s22p63s23p63d104s24p2spdfwith noble gas notation=[Ar]3d104s24p2Orbitalboxnotation       = [Ar]3d104s24p2

When (Ge) was oxidized to (Ge2+) ions, it lost for two electrons in outermost (4s and 4p) orbitals, hence this orbital notation method shows below.

   AtomicnumberofGermanium(Ge)=32spdfwith orbtital notation=[1s22s22p63s23p63d104s24p0]Orbital filling method       1s22s22p63s23p63d104s24p0spdfwith noble gas notation=[Ar]3d104s24p2Orbitalboxnotation       = [Ar]3d104s24p0

Hence, the electronic configuration of germanium ions (Ge2+) = 1s22s22p63s23p63d104s24p0 and noble gas configuration of [Ar]4s24p0 

(d)

Interpretation Introduction

Interpretation:

The electronic configuration has to be depicted for F- ion using orbital box diagram and noble gas electronic configuration method.

Concept Introduction:

Electronic configuration: The electronic configuration is the distribution of electrons of an given molecule or respective atoms in atomic or molecular orbitals.

Aufbau principle: This rule statues that ground state of an atom or ions electrons fill atomic orbitals of the lowest available energy levels before occupying higher levels. If consider the 1s shell is filled the 2s subshell is occupied.

Hund's Rule: The every orbital in a subshell is singly occupied with one electron before any one orbital is doubly occupied, and all electrons in singly occupied orbitals have the same spin.

Pauli exclusion rule: an atomic orbital may describe at most two electrons, each with opposite spin direction.

(d)

Expert Solution
Check Mark

Explanation of Solution

 Let us consider the orbital filling method of Florine ions (F-) ions.

The single chlorine atoms having (9) electrons in (s, p) orbital shells and its atomic number (Z=9). Moreover the (F) atom has gain of one electron in outermost (2p) shells.

Hence we can write gains of electron (Reduction method) process are presented below.

                AtomicnumberofFluorine(F)=9spdfwith orbtital notation=[1s22s22p5]Orbital filling method       1s22s22p5spdfwith noble gas notation=[He]2s22p5Orbitalboxnotation       = [He]2s22p5

When (F) was gain to (F-) ions, it gain one electron to outermost (2p) orbitals, hence this orbital notation method shows below.

         AtomicnumberofFlurine(F)= 9spdfwith orbtital notation=[1s22s22p6]Orbital filling method       1s22s22p6spdfwith noble gas notation=[He]2s22p6Orbitalboxnotation       = [He]2s22p6

Hence, the electronic configuration of fluorine ions (F-) = 1s22s22p6 and noble gas configuration of [He]2s22p6

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Chapter 7 Solutions

Chemistry & Chemical Reactivity

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