Chapter 4, Problem 4.29EP

Fill in the blanks in each line of the following table. The first line is already completed as an example.

Interpretation Introduction

Interpretation:

Filling of each blank in the following table has to be done:

  $\begin{array}{ccccc}\text{a)}& \begin{array}{l}\text{Chemical}\\ \text{symbol}\end{array}& \begin{array}{l}\text{Ion}\\ \text{formed}\end{array}& \begin{array}{l}\text{Number of }\\ \text{electrons in ion}\end{array}& \begin{array}{l}\text{Number of }\\ \text{protons in ion}\end{array}\\ & \text{Be}& & \text{2e}& \end{array}$

Concept Introduction:

Atoms are composed of three types of particles called subatomic particles.  They are as follows:

• Protons: Positively charged particles in an atom.
• Neutrons: Neutral charged particles in an atom.
• Electrons: Negatively charged particles in an atom.

The neutral atom has equal number of protons and electrons.  Gaining or loosing of electrons of an atom forms ion.

Negative charged ions are formed by gaining one or more electrons and it has more electrons than protons.

Positive charged ions are formed by losing one or more electrons and it has more protons than electrons.

Answer to Problem 4.29EP

Complete table is shown below:

  $\begin{array}{ccccc}\text{a)}& \begin{array}{l}\text{Chemical}\\ \text{symbol}\end{array}& \begin{array}{l}\text{Ion}\\ \text{formed}\end{array}& \begin{array}{l}\text{Number of }\\ \text{electrons in ion}\end{array}& \begin{array}{l}\text{Number of }\\ \text{protons in ion}\end{array}\\ & \text{Be}& {\text{Be}}^{\text{2+}}& \text{2e}& \text{4p}\end{array}$

Explanation of Solution

The chemical symbol of the element is $\text{Be}$.  Beryllium atomic number is $4$ thus the number of protons is $4$.

Two electrons are lesser than the total number protons thatmeans it lost two electrons and the charge of the beryllium ion is ${\text{Be}}^{\text{2+}}$.

Hence, the symbol of ion is ${\text{Be}}^{\text{2+}}$, it has $\text{4}$ protons, $2$ electrons and lost two electrons.

Interpretation Introduction

Interpretation:

Filling of each blank in the following table has to be done:

  $\begin{array}{ccccc}\text{b)}& \begin{array}{l}\text{Chemical}\\ \text{symbol}\end{array}& \begin{array}{l}\text{Ion}\\ \text{formed}\end{array}& \begin{array}{l}\text{Number of }\\ \text{electrons in ion}\end{array}& \begin{array}{l}\text{Number of }\\ \text{protons in ion}\end{array}\\ & & & 54& 53\end{array}$

Concept Introduction:

Atoms are composed of three types of particles called subatomic particles. They are as follows:

• Protons: Positively charged particles in an atom.
• Neutrons: Neutral charged particles in an atom.
• Electrons: Negatively charged particles in an atom.

The neutral atom has equal number of protons and electrons.  Gaining or loosing of electrons of an atom form ion.

Negative charged ions are formed by gaining one or more electrons and it has more electrons than protons.

Positive charged ions are formed by losing one or more electrons and it has more protons than electrons.

Answer to Problem 4.29EP

Complete table is shown below:

  $\begin{array}{ccccc}\text{b)}& \begin{array}{l}\text{Chemical}\\ \text{symbol}\end{array}& \begin{array}{l}\text{Ion}\\ \text{formed}\end{array}& \begin{array}{l}\text{Number of }\\ \text{electrons in ion}\end{array}& \begin{array}{l}\text{Number of }\\ \text{protons in ion}\end{array}\\ & \text{I}& {\text{I}}^{\text{-}}& \text{54}& \text{53}\end{array}$

Explanation of Solution

The element has $\text{53}$ protons thus the element is Iodine the chemical symbol of element is $\text{I}$.  One proton is lesser than the total number of electrons means it gained one electron.  The charge of the symbol is ${\text{I}}^{\text{-}}$.

Hence, the number of protons are $\text{53}$, number of electrons are $\text{54}$, gain one electron and the symbol of the ion is ${\text{I}}^{\text{-}}$.

Interpretation Introduction

Interpretation:

Filling of each blank in the following table has to be done:

  $\begin{array}{ccccc}\text{c)}& \begin{array}{l}\text{Chemical}\\ \text{symbol}\end{array}& \begin{array}{l}\text{Ion}\\ \text{formed}\end{array}& \begin{array}{l}\text{Number of }\\ \text{electrons in ion}\end{array}& \begin{array}{l}\text{Number of }\\ \text{protons in ion}\end{array}\\ & & {\text{Al}}^{\text{3+}}& \text{10}& \end{array}$

Concept Introduction:

Atoms are composed of three types of particles called subatomic particles.  They are as follows:

• Protons: Positively charged particles in an atom.
• Neutrons: Neutral charged particles in an atom.
• Electrons: Negatively charged particles in an atom.

The neutral atom has equal number of protons and electrons.  Gaining or loosing of electrons of an atom forms ion.

Negative charged ions are formed by gaining one or more electrons and it has more electrons than protons.

Positive charged ions are formed by losing one or more electrons and it has more protons than electrons.

Answer to Problem 4.29EP

Complete table is shown below:

  $\begin{array}{ccccc}\text{c)}& \begin{array}{l}\text{Chemical}\\ \text{symbol}\end{array}& \begin{array}{l}\text{Ion}\\ \text{formed}\end{array}& \begin{array}{l}\text{Number of }\\ \text{electrons in ion}\end{array}& \begin{array}{l}\text{Number of }\\ \text{protons in ion}\end{array}\\ & \text{Al}& {\text{Al}}^{\text{3+}}& \text{10}& \text{13}\end{array}$

Explanation of Solution

The ion ${\text{Al}}^{\text{3+}}$ has $\text{10}$ electrons.  Atomic number of aluminium is $\text{13}$.  Thus, the number of protons in aluminium element is $\text{13}$.  The chemical symbol of aluminium is $\text{Al}$.

Hence, ion ${\text{Al}}^{\text{3+}}$ has $\text{13}$ protons, $\text{10}$ electrons , lost three electrons and the chemical symbol of aluminium element is ${\text{Al}}^{\text{3+}}$.

Interpretation Introduction

Interpretation:

Filling of each blank in the following table has to be done:

  $\begin{array}{ccccc}\text{d)}& \begin{array}{l}\text{Chemical}\\ \text{symbol}\end{array}& \begin{array}{l}\text{Ion}\\ \text{formed}\end{array}& \begin{array}{l}\text{Number of }\\ \text{electrons in ion}\end{array}& \begin{array}{l}\text{Number of }\\ \text{protons in ion}\end{array}\\ & & {\text{S}}^{\text{2-}}& & \end{array}$

Concept Introduction:

Atoms are composed of three types of particles called subatomic particles.  They are as follows:

• Protons: Positively charged particles in an atom.
• Neutrons: Neutral charged particles in an atom.
• Electrons: Negatively charged particles in an atom.

The neutral atom has equal number of protons and electrons.  Gaining or loosing of electrons of an atom forms ion.

Negative charged ions are formed by gaining one or more electrons and it has more electrons than protons.

Positive charged ions are formed by losing one or more electrons and it has more protons than electrons.

Answer to Problem 4.29EP

Complete table is shown below:

  $\begin{array}{ccccc}\text{d)}& \begin{array}{l}\text{Chemical}\\ \text{symbol}\end{array}& \begin{array}{l}\text{Ion}\\ \text{formed}\end{array}& \begin{array}{l}\text{Number of }\\ \text{electrons in ion}\end{array}& \begin{array}{l}\text{Number of }\\ \text{protons in ion}\end{array}\\ & \text{S}& {\text{S}}^{\text{2-}}& \text{18}& \text{16}\end{array}$

Explanation of Solution

The given ion is ${\text{S}}^{\text{2-}}$.  The chemical symbol of sulfur atom is $\text{S}$.  Atomic number of sulfur atom is $\text{16}$ thus the number protons are $\text{16}$.

The charge of sulfur atom is $\text{2-}$ means it gains two electrons.  So, the total number of electrons in sulfur ion is $\text{(16 + 2 =18)}$.

Hence, ion is ${\text{S}}^{\text{2-}}$, it has $\text{16}$ protons, $18$ electrons, lost two electrons and the chemical symbol of sulphur element is $\text{S}$.