Chapter 5, Problem 5.18P

(a)

Interpretation Introduction

Interpretation:

Reason for the electronic configuration $1s^{2}2s^{3}2p^3$ is not possible has to be given.

Concept Introduction:

Principal quantum number is the one that specifies the extent or the effective size of an orbital.  This is denoted by $n$.  Shape of the orbital is denoted by the azimuthal quantum number.  This is denoted by $l$ and the values of azimuthal quantum number will be from zero to $n-1$.  The subshell $s,p,d$, and $f$ is denoted by the value of azimuthal quantum number as $0,1,2$, and $3$ respectively.

Magnetic quantum number has a value of $+l$ to $-l$.  This determines the spatial orientation of orbital and it is designated as $m_l$.  Spin state of an electron is designated by the spin quantum number.  It is denoted by $m_s$ and it can have only two possible values.  They are $+1/2\text{or}-1/2$.

No two electrons of an atom can have same set of four quantum numbers is known as Pauli exclusion principle.  According to Pauli Exclusion principle, the number of electrons that can be present in $s,p,d$ and $f$ orbitals are $2,6,10$ and $14$ electrons respectively.  Filling of orbitals takes place in the order of increasing energy of orbital and this is known as Aufbau principle.

(b)

Interpretation Introduction

Interpretation:

Reason for the electronic configuration $1s^{2}2s^{2}2p^{3}3s^6$ is not possible has to be given.

Concept Introduction:

Refer part (a).

(c)

Interpretation Introduction

Interpretation:

Reason for the electronic configuration $1s^{2}2s^{2}2p^{7}3s^{2}3p^8$ is not possible has to be given.

Concept Introduction:

Refer part (a).

(d)

Interpretation Introduction

Interpretation:

Reason for the electronic configuration $1s^{2}2s^{2}2p^{6}3s^{2}3p^{1}4s^{2}3d^{14}$ is not possible has to be given.

Concept Introduction:

Refer part (a).