Chapter 5, Problem 69A

a)

Interpretation Introduction

Interpretation : The electron transitions emit energy or require the absorption of energy to be indicated.

Concept Introduction: The energies or energy levels that an electron can have are determined by the Schrodinger equation's solution. The atomic orbital, which is derived from the Schrodinger equation for each energy level, expresses the probability that an electron will be found at a particular place around the nucleus.

Answer to Problem 69A

The electron transition for $3p$ to $3s$ emits energy.

Explanation of Solution

Each energy sublevel has an associated orbital or orbitals with a variety of forms. In which an electron is most likely to be found is described by its orbitals.

When atoms absorb energy, their electrons move to higher energy levels. These electrons lose energy by emitting light when they return to lower energy levels.

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.

In the given electronic transition $3p$ to $3s$ , the electrons are lost by emitting energy.

Since the transition is from a higher energy level to a lower energy level.

b)

Interpretation Introduction

Interpretation : The electron transitions emit energy or require the absorption of energy to be indicated.

Concept Introduction: The energies or energy levels that an electron can have are determined by the Schrodinger equation's solution. The atomic orbital, which is derived from the Schrodinger equation for each energy level, expresses the probability that an electron will be found at a particular place around the nucleus.

Answer to Problem 69A

The electron transition for $3p$ to $4p$ absorbs energy.

Explanation of Solution

Each energy sublevel has an associated orbital or orbitals with a variety of forms. In which an electron is most likely to be found is described by its orbitals.

When atoms absorb energy, their electrons move to higher energy levels. These electrons lose energy by emitting light when they return to lower energy levels.

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.

In the given electronic transition $3p$ to $4p$ , the electrons absorb energy.

Since the transition is from a lower energy level to a higher energy level.

c)

Interpretation Introduction

Interpretation : The electron transitions emit energy or require the absorption of energy to be indicated.

Concept Introduction: The energies or energy levels that an electron can have are determined by the Schrodinger equation's solution. The atomic orbital, which is derived from the Schrodinger equation for each energy level, expresses the probability that an electron will be found at a particular place around the nucleus.

Answer to Problem 69A

The electron transition for $2s$ to $2p$ absorbs energy.

Explanation of Solution

Each energy sublevel has an associated orbital or orbitals with a variety of forms. In which an electron is most likely to be found is described by its orbitals.

When atoms absorb energy, their electrons move to higher energy levels. These electrons lose energy by emitting light when they return to lower energy levels.

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.

In the given electronic transition $2s$ to $2p$ , the electrons absorb energy.

Since the transition is from a lower energy level to a higher energy level.

d)

Interpretation Introduction

Interpretation : The electron transitions emit energy or require the absorption of energy to be indicated.

Concept Introduction: The energies or energy levels that an electron can have are determined by the Schrodinger equation's solution. The atomic orbital, which is derived from the Schrodinger equation for each energy level, expresses the probability that an electron will be found at a particular place around the nucleus.

Answer to Problem 69A

The electron transition for $1s$ to $2s$ absorbs energy.

Explanation of Solution

Each energy sublevel has an associated orbital or orbitals with a variety of forms. In which an electron is most likely to be found is described by its orbitals.

When atoms absorb energy, their electrons move to higher energy levels. These electrons lose energy by emitting light when they return to lower energy levels.

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.

In the given electronic transition $1s$ to $2s$ , the electrons absorb energy.

Since the transition is from a lower energy level to a higher energy level.