The electronic configuration and orbital diagram for bromine atom having atomic number 35 is to be written. Concept introduction: The number of electrons in an element is equal to its atomic number. The orbital diagram represents the electrons in the form of an arrow. The arrows are drawn in the box and the box represents the orbital. General rules for writing electronic configuration: Electrons will reside in the available orbitals of lowest possible energy. Each orbital can accommodate a maximum of two electrons. Electrons will not pair in degenerate orbitals if an empty orbital is available. Orbitals will fill in order of increasing energy 1 s 2 s 2 p 3 s 3 p 4 s 3 d 4 p 5 s 4 d 5 p 6 s 4 f . The electrons are filled in the increasing order of energy. The lowest energy orbitals are filled first. In an orbital, only two electrons are present. The spin of the electrons must be opposite. The s orbital can hold up to two electrons and the p orbital can hold up to six electrons, d -orbital can have 0–10 electrons, and f -orbital can have 0–14 electrons. Electrons are filled according to the Hund’s rule, which states that while filling the orbitals of equal energy, first the electrons are singly filled and then, they are filled with the parallel spin.

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Chapter 6.9, Problem 1PPB

Interpretation Introduction

Interpretation:

The electronic configuration and orbital diagram for bromine atom having atomic number 35 is to be written.

Concept introduction:

The number of electrons in an element is equal to its atomic number.

The orbital diagram represents the electrons in the form of an arrow. The arrows are drawn in the box and the box represents the orbital.

General rules for writing electronic configuration:

Electrons will reside in the available orbitals of lowest possible energy.

Each orbital can accommodate a maximum of two electrons.

Electrons will not pair in degenerate orbitals if an empty orbital is available.

Orbitals will fill in order of increasing energy 1s 2s 2p 3s 3p 4s 3d 4p 5s 4d 5p 6s 4f.

The electrons are filled in the increasing order of energy. The lowest energy orbitals are filled first.

In an orbital, only two electrons are present. The spin of the electrons must be opposite.

The s orbital can hold up to two electrons and the p orbital can hold up to six electrons, d-orbital can have 0–10 electrons, and f-orbital can have 0–14 electrons.

Electrons are filled according to the Hund’s rule, which states that while filling the orbitals of equal energy, first the electrons are singly filled and then, they are filled with the parallel spin.

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