Chapter 5, Problem 5.135MP

Interpretation Introduction

(a)

Interpretation:

An orbital filling diagram for the element with Z=25 and the number of partially filled orbitals present in the element needs to be determined.

Concept introduction:

Aufbau principle explains the rule of the filling order of orbitals. There are three rules in Aufbau principle. They are as follows:

1) The filling of lower energy orbitals should be done before higher-energy orbitals.

2) The maximum capacity of an orbital is two electrons, where both electrons possess opposite spins.

3) In case, if two or more orbitals (degenerate) present; one electron goes into each until all the orbitals are half-filled.

Interpretation Introduction

(b)

Interpretation:

The atomic number of the element in the third column of the fourth row needs to be determined under the new rules also determine the block does it belongs to (s, p, d or f).

Concept introduction:

The periodic table is divided into 4 blocks, according to the filling of orbitals of the elements. The group 1A and 2A are present on the left side and known as s-block element as electrons are filled in s orbitals. The group 3A-8A elements on the right side of the table are the p-block elements because here p-orbitals are filled. The d-block elements are present n middle of periodic table here, valence electrons are present ind-orbitals, and the lanthanide/actinide f-block elements present at the bottom of the table where valence electrons are in f-orbitals.