Chapter 12, Problem 58A

(a)

Interpretation Introduction

Interpretation:

The electronic configuration of given atom and its most stable ion is to be written.

Concept introduction:

Electronic configuration is arrangement of electrons in an atom. The atoms lose or gain electrons to acquire noble gas configuration because the ion which achieve nearest noble gas configuration is most stable.

Answer to Problem 58A

  $Na$ forms $N{a}^{+}$ :

It attains configuration as $Ne$

Explanation of Solution

Sodium belongs to first group. So it has tendency to loss one electron and form most stable ion $N{a}^{+}$

Electronic configuration of $Na$ according to Aufbau’s Principle is:

  $\left[Ne\right]3s^1$

Therefore, Electronic configuration of $N{a}^{+}$ :

  $\left[Ne\right]$

(b)

Interpretation Introduction

Interpretation:

The electronic configuration of given atom and its most stable ion is to be written.

Concept introduction:

Electronic configuration is arrangement of electrons in an atom. The atoms lose or gain electrons to acquire noble gas configuration because the ion which achieve nearest noble gas configuration is most stable.

Answer to Problem 58A

  $I$ forms $I^{-}$

It attains configuration as $Xe$

Explanation of Solution

Iodine belongs to 17^th group. So it has tendency to gain one electron and form most stable ion $I^{-}$

Electronic configuration of $I$ according to Aufbau’s Principle is:

  $\left[Kr\right]5s^{2}4d^{10}5p^5$

Therefore, Electronic configuration of $I^{-}$ :

  $\left[Kr\right]5s^{2}4d^{10}5p^6$

(c)

Interpretation Introduction

Interpretation:

The electronic configuration of given atom and its most stable ion is to be written.

Concept introduction:

Electronic configuration is arrangement of electrons in an atom. The atoms lose or gain electrons to acquire noble gas configuration because the ion which achieve nearest noble gas configuration is most stable.

Answer to Problem 58A

  $K$ forms $K^{+}$ :

It attains configuration as $Ar$

Explanation of Solution

Potassium belongs to first group. So it has tendency to loss one electron and form most stable ion $K^{+}$

Electronic configuration of $K$ according to Aufbau’s Principle is:

  $\left[Ar\right]4s^1$

Therefore, Electronic configuration of $K^{+}$ :

  $\left[Ar\right]$

(d)

Interpretation Introduction

Interpretation:

The electronic configuration of given atom and its most stable ion is to be written.

Concept introduction:

Electronic configuration is arrangement of electrons in an atom. The atoms lose or gain electrons to acquire noble gas configuration because the ion which achieve nearest noble gas configuration is most stable.

Answer to Problem 58A

  $CaformsC{a}^{2+}$and attains configuration as argon.

Explanation of Solution

Calcium belongs to 2^nd group. So it has tendency to loss two electrons and form most stable ion $C{a}^{2+}$

Electronic configuration of $Ca$ according to Aufbau’s Principle is:

  $1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^2$

Therefore, Electronic configuration of $C{a}^{2+}$ :

  $1s^{2}2s^{2}2p^{6}3s^{2}3p^6$

It attains configuration as $Ar$

(e)

Interpretation Introduction

Interpretation:

The electronic configuration of given atom and its most stable ion is to be written.

Concept introduction:

Electronic configuration is arrangement of electrons in an atom. The atoms lose or gain electrons to acquire noble gas configuration because the ion which achieve nearest noble gas configuration is most stable.

Answer to Problem 58A

Sulphur forms $S^{2-}ion$ and get configuration as argon.

Explanation of Solution

Sulphur belongs to 16^th group. So it has tendency to gain two electrons and form most stable ion $S^{2-}$

Electronic configuration of $S$ according to Aufbau’s Principle is:

  $\left[Ne\right]3s^{2}3p^4$

Therefore, Electronic configuration of $S^{2-}$ :

  $\left[Ar\right]$

(f)

Interpretation Introduction

Interpretation:

The electronic configuration of given atom and its most stable ion is to be written.

Concept introduction:

Electronic configuration is arrangement of electrons in an atom. The atoms lose or gain electrons to acquire noble gas configuration because the ion which achieve nearest noble gas configuration is most stable.

Answer to Problem 58A

  $Mg$ forms $M{g}^{2+}$ :

It attains configuration as $Ne$

Explanation of Solution

Magnesium belongs to 2^nd group. So it has tendency to loss two electrons and form most stable ion $M{g}^{2+}$

Electronic configuration of $Mg$ according to Aufbau’s Principle is:

  $\left[Ne\right]3s^2$

Therefore, Electronic configuration of $M{g}^{2+}$ :

  $\left[Ne\right]$

(g)

Interpretation Introduction

Interpretation:

The electronic configuration of given atom and its most stable ion is to be written.

Concept introduction:

Electronic configuration is arrangement of electrons in an atom. The atoms lose or gain electrons to acquire noble gas configuration because the ion which achieve nearest noble gas configuration is most stable.

Answer to Problem 58A

  $Al$ forms $A{l}^{3+}$ :

It attains configuration as $Ne$

Explanation of Solution

Aluminium belongs to 3^rd group. So it has tendency to loss three electrons and form most stable ion $A{l}^{3+}$

Electronic configuration of $Al$ according to Aufbau’s Principle is:

  $\left[Ne\right]3s^{2}3p^1$

Therefore, Electronic configuration of $A{l}^{3+}$ :

  $\left[Ne\right]$

(h)

Interpretation Introduction

Interpretation:

The electronic configuration of given atom and its most stable ion is to be written.

Concept introduction:

Electronic configuration is arrangement of electrons in an atom. The atoms lose or gain electrons to acquire noble gas configuration because the ion which achieve nearest noble gas configuration is most stable.

Answer to Problem 58A

Nitrogen forms $N^{3-}ion$ and attain configuration as neon.

Explanation of Solution

Nitrogen belongs to 15^th group. So it has tendency to gain three electrons and form most stable ion $N^{3-}ion$

Electronic configuration of $N$ according to Aufbau’s Principle is:

  $1s^{2}2s^{2}2p^3$

Therefore, Electronic configuration of $N^{3-}ion$ :

  $1s^{2}2s^{2}2p^6$