Chapter 5, Problem 57A

Interpretation Introduction

Interpretation: The electronic configurations for arsenic to be represented and the total number of electrons in each energy level state that energy levels are not full to be calculated.

Concept Introduction: Electronic configurations refer to the arrangements of electrons in different orbitals around atoms' nuclei.

Answer to Problem 57A

The electronic configuration of the arsenic atom is $1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}3d^{10}4s^{2}4p^3$ .

The total number of electrons in $n=1$ is 2 electrons, $n=2$ is 8 electrons, $n=3$ is 18 electrons, $n=4$ is 5 electrons.

The energy level $n=4$ is not fully filled.

Explanation of Solution

Electronic configurations refer to the arrangements of electrons in different orbitals around atoms' nuclei.

The Aufbau principle, the Pauli exclusion principle, and Hund's rule are three rules that can be used to determine the electronic configuration of atoms.

The atomic number of Arsenic is 33.

Arsenic contains 3e electrons.

The energy levels and symbols for each sub-level occupied by an electron are written for an atom's electrical configuration.

Each sub-level is superscripted with the number of electrons occupied. The number of electrons in an atom is equal to the sum of the superscripts.

The order of orbital filling of the atoms is given as

  $1s,2s,3p,3s,3p,4s,3d,4p,5s,4d,5p,6s,4f,5d,6p,7s,5f,6d,7p$

Where, s orbitals accommodate 2 electrons, p orbitals 6 electrons, d orbitals 10 electrons, and f orbitals 14 electrons.

The electronic configuration of the arsenic atom is written as follows:

  $1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}3d^{10}4s^{2}4p^3$

There are four energy levels in arsenic atom.

The number of electrons in $n=1$ is 2 electrons.

The number of electrons in $n=2$ is 8 electrons.

The number of electrons in $n=3$ is 18 electrons.

The number of electrons in $n=4$ is 5 electrons.

The energy level $n=4$ is not fully filled.