Chapter 7, Problem 5PS

a)

Interpretation Introduction

Interpretation:

The Arsenic (As) electronic configurations has to be derived using its (s, p, d, f) notation and noble gas orbital box diagram.

Concept Introduction:

General properties of Arsenic (As): The arsenic occurs in many minerals and usually in combination with sulfur and metals but also as pure elemental crystal. Arsenic (As) is metalloid.

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

The important there rules for electronic configuration given below:

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)

Interpretation Introduction

Interpretation:

The Krypton (Kr) electronic configurations has to be derived using its (s, p, d, f) notation and noble gas orbital box diagram.

Concept Introduction:

General properties of Arsenic (As): The arsenic occurs in many minerals and usually in combination with sulfur and metals but also as pure elemental crystal. In another important think (As) is metalloid, it is various allotropes and this metal only uses for industry.

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

The important there rules for electronic configuration given below:

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.