Chapter 5, Problem 41A

a)

Interpretation Introduction

Interpretation: The electronic configurations for atoms of the elements are to be represented.

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

Answer to Problem 41A

The electronic configuration of the sodium atom is $1s^{2}2s^{2}2p^{6}3s^1$ .

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 symbol $\text{Na}$ represents sodium.

The atomic number of sodium is 11.

Sodium contains 11 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

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

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

  $1s^{2}2s^{2}2p^{6}3s^1$

b)

Interpretation Introduction

Interpretation: The electronic configurations for atoms of the elements are to be represented.

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

Answer to Problem 41A

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

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 symbol $\text{K}$ represents potassium.

The atomic number of potassium is 19.

Potassium contains 19 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

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

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

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

c)

Interpretation Introduction

Interpretation: The electronic configurations for atoms of the elements are to be represented.

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

Answer to Problem 41A

The electronic configuration of the iodine atom is $1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{2}3d^{10}4p^{6}5s^{2}4d^{10}5p^5$ .

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 symbol $\text{I}$ represents iodine.

The atomic number of iodine is 53.

Iodine contains 53 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

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

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

  $1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{2}3d^{10}4p^{6}5s^{2}4d^{10}5p^5$

d)

Interpretation Introduction

Interpretation: The electronic configurations for atoms of the elements are to be represented.

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

Answer to Problem 41A

The electronic configuration of the neon atom is $1s^{2}2s^{2}2p^6$ .

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 symbol $\text{Ne}$ represents neon.

The atomic number of neon is 10.

Neon contains 10 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

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

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

  $1s^{2}2s^{2}2p^6$