Chapter 7.1, Problem 5SSC

Interpretation Introduction

(a)

Interpretation:

The electron configuration of Nitrogen and the change to achieve a noble gas configuration needs to be explained.

Concept introduction:

In chemistry, an electron configuration is the arrangement of electrons in a molecule, an atom, or a different physical structure.

Answer to Problem 5SSC

The electronic configuration of Nitrogen is $\left[He\right]2s^2,2p^3$ and it gains $3$ electrons to achieve a noble gas configuration.

Explanation of Solution

The elements have their electrons, which are distributed in its atomic orbital and this distribution is known as that element’s electron configuration. This distribution or filling is done as per standard notation, in which filling is at subshell levels and is placed in sequence.

Nitrogen has $5$ valence electrons. The electrons are distributed in orbitals $1s^{2}2s^{2}2p^3$. It is also depicted as $\left[He\right]2s^{2}2p^3$. Thus, nitrogen needs to gain $3$ electrons to reach the nearest noble gas configuration of Neon.

(b)

Interpretation Introduction

Interpretation:

The electronic configuration of Sulphur and the change occur to achieve a noble gas configuration needs to be explained.

Concept introduction:

In chemistry, an electron configuration is the arrangement of electrons in a molecule, an atom, or a different physical structure.

Answer to Problem 5SSC

The electronic configuration of Sulphur is $\left[Ne\right]3s^{2}3p^4$ and needs $2$ electrons to achieve a noble gas configuration.

Explanation of Solution

The elements have their electrons, which are distributed in its atomic orbital and this distribution is known as that element’s electron configuration. This distribution or filling is done as per standard notation, in which filling is at subshell levels and is placed in sequence.

Sulfur has $6$ valence electrons. Initially, the electrons will distribute in orbital $2p$ and then the next $2$ electrons will fill inan orbital $3s$. After $3s$, the next filling will be in orbital $3p$ where the last $4$ electronsfilled. Hence, the electronic configuration is $1s^{2}2s^{2}2p^{6}3s^{2}3p^4$. It is also depicted as $\left[Ne\right]3s^{2}3p^4$.

So, sulfur needs to gain $2$ electrons to reach the nearest noble gas configuration of Argon.

(c)

Interpretation Introduction

Interpretation:

The electronic configuration of Barium and the change that occur to achieve a noble gas configuration needs to be explained.

Concept introduction:

In chemistry, an electron configuration is the arrangement of electrons in a molecule, an atom, or a different physical structure.

Answer to Problem 5SSC

The electronic configuration of Barium is $\left[Xe\right]6s^2$ and needs to lose $2$ electrons to achieve a noble gas configuration.

Explanation of Solution

The elements have their electrons, which are distributed in its atomic orbital and this distribution is known as that element’s electron configuration. This distribution or filling is done as per standard notation, in which filling is at subshell levels and is placed in sequence.

Atomic Barium has $2$ valence electrons. The electronic configuration of Barium is $1s^2 2s^2 2p^6 3s^2 3p^6 3d^{10} 4s^2 4p^6 4d^{10} 5s^2 5p^6 6s^2$. It is also depicted as $\left[Xe\right]6s^2$. As it has $2$ electrons in ‘p’ shell, indicates it can lose $2$ electrons and forms a cation.

So, barium needs to lose $2$ electrons to reach the nearest noble gas configuration of xenon.

(d)

Interpretation Introduction

Interpretation:

The electronic configuration of Lithium and the change that occur to achieve a noble gas configuration needs to be determined.

Concept introduction:

In chemistry, an electron configuration is the arrangement of electrons in a molecule, an atom, or a different physical structure.

Answer to Problem 5SSC

The electronic configuration of Lithium is $\left[Xe\right]6s^2$ and it can lose $2$ electrons.

Explanation of Solution

The elements have their electrons, which are distributed in its atomic orbital and this distribution is known as that element’s electron configuration. This distribution or filling is done as per standard notation, in which filling is at subshell levels and is placed in sequence.

Atomic Lithium has $1$ valence electrons. The electronic configuration of Lithium is $1s^{2}2s^1$.

It is also depicted as $\left[He\right]2s^1$. As it has $1$ an electron in ‘p’ shell, it can easily lose one electron and become a positively charged ion.

Hence, lithium needs to lose an electron to reach the nearest noble gas configuration of helium.