Chapter 11, Problem 92E

Determine whether each statement that follows is true or false:

a) Electron energies are quantized in excited states but not in the ground state.

b) Line spectra of the elements are experimental evidence of the quantization of electron energies.

c) Energy is released as an electron passes from ground state to an excited state.

d) The energy of an electron may be between two quantized energy levels.

e) The Bohr model explanation of line spectra is still thought to be correct.

f) The quantum mechanical model of the atom describes orbitals in which electrons travel around the nucleus.

g) Orbitals are regions in which there is a high probability of finding an electron.

h) All energy sublevels have the same number of orbitals.

i) The $3p$ orbitals of an atom are larger than its $2p$ orbitals but smaller than its $4p$ orbitals.

j) At a given sublevel, the maximum number of $d$ electrons is $5$.

k) The halogens are found in Group $\text{7A}/17$ of the periodic table.

l) The dot structure of the alkaline earths is $\text{X}·$, where $\text{X}$ is the symbol of element in the family.

m) Stable ions formed by alkaline earth metals are isoelectronic with noble gas atoms.

n) Atomic numbers $23$ and $45$ both belong to transition elements.

o) Atomic number $52$, $35$, and $18$ are arranged in order of increasing atomic size.

p) Atomic number $7$, $16$, and $35$ are all nonmetals.

Interpretation Introduction

(a)

Interpretation:

Whether the statement, “Electron energies are quantized in excited states but not in the ground state” is true or false is to be stated.

Concept introduction:

An atom is made up of three subatomic particles-neutrons, protons, and electrons. Neutron and protons are present in the nucleus of the atom, whereas electrons are revolving outside the nucleus in an atom. The electrons are arranged in the orbit of atoms according to their energy.

Answer to Problem 92E

The statement, “Electron energies are quantized in excited states but not in the ground state” is false.

Explanation of Solution

The energy of each level of atom is quantized. The energies of electron in excited state and ground state are quantized. Therefore, the statement, “Electron energies are quantized in excited states but not in the ground state” is false.

Conclusion

The given statement is false.

Interpretation Introduction

(b)

Interpretation:

Whether the statement, “Line spectra of the elements are experimental evidence of the quantization of electron energies” is true or false is to be stated.

Concept introduction:

Electronic spectra are formed by the excitation and relaxation process of electrons. The excitation process is due to the transition of an electron from a lower energy level to a higher energy level. The relaxation process is due to the transition of an electron from a higher energy level to lower energy level.

Answer to Problem 92E

The statement, “Line spectra of the elements are experimental evidence of the quantization of electron energies” is true.

Explanation of Solution

Electronic spectra are formed by the excitation and relaxation process of electrons. The spectrum formed by an element has discrete discontinuous lines at specific wavelengths. The discrete lines are formed because the electronic energy levels of an atom are quantized. The electronic spectrum of an element is its characteristic. Therefore, the statement, “Line spectra of the elements are experimental evidence of the quantization of electron energies” is true.

Conclusion

The given statement is true.

Interpretation Introduction

(c)

Interpretation:

Whether the statement, “Energy is released as an electron passes from ground state to an excited state” is true or false is to be stated.

Concept introduction:

Electronic spectra are formed by the excitation and relaxation process of electrons. The excitation process is due to the transition of an electron from a lower energy level to a higher energy level. The relaxation process is due to the transition of an electron from a higher energy level to lower energy level.

Answer to Problem 92E

The statement, “Energy is released as an electron passes from ground state to an excited state” is false.

Explanation of Solution

The energy of ground state is lower than the energy of excited state. An electron requires some energy to excite from lower energy level to higher energy level. Therefore, the statement, “Energy is released as an electron passes from ground state to an excited state” is false.

Conclusion

The given statement is false.

Interpretation Introduction

(d)

Interpretation:

Whether the statement, “The energy of an electron may be between two quantized energy levels” is true or false is to be stated.

Concept introduction:

An atom is made up of three subatomic particles-neutrons, protons, and electrons. Neutron and protons are present in the nucleus of the atom, whereas electrons are revolving outside the nucleus in an atom. The electrons are arranged in the orbit of atoms according to their energy.

Answer to Problem 92E

The statement, “The energy of an electron may be between two quantized energy levels” is false.

Explanation of Solution

The spectrum formed by an element has discrete discontinuous lines at specific wavelengths. The discrete lines are formed because the electronic energy levels of an atom are quantized. Therefore, the statement, “The energy of an electron may be between two quantized energy levels” is false.

Conclusion

The given statement is false.

Interpretation Introduction

(e)

Interpretation:

Whether the statement, “The Bohr model explanation of line spectra is still thought to be correct” is true or false is to be stated.

Concept introduction:

Electronic spectra are formed by the excitation and relaxation process of electrons. The excitation process is due to the transition of an electron from a lower energy level to a higher energy level. The relaxation process is due to the transition of an electron from a higher energy level to lower energy level.

Answer to Problem 92E

The statement, “The Bohr model explanation of line spectra is still thought to be correct” is true.

Explanation of Solution

The Bohr model states that the energy of each level of atom is quantized. The spectrum formed by an element has discrete discontinuous lines at specific wavelengths. The discrete lines are formed because the electronic energy levels of an atom are quantized. Therefore, the statement, “The Bohr model explanation of line spectra is still thought to be correct” is true.

Conclusion

The given statement is true.

Interpretation Introduction

(f)

Interpretation:

Whether the statement, “The quantum mechanical model of the atom describes orbitals in which electrons travel around the nucleus” is true or false is to be stated.

Concept introduction:

An atom is made up of three subatomic particles-neutrons, protons, and electrons. Neutron and protons are present in the nucleus of the atom, whereas electrons are revolving outside the nucleus in an atom. The electrons are arranged in the orbit of atoms according to their energy.

Answer to Problem 92E

The statement, “The quantum mechanical model of the atom describes orbitals in which electrons travel around the nucleus” is false.

Explanation of Solution

Quantum mechanical model states that it is impossible to find the location of electron in an atom. The orbitals are the region where the electrons are most probable to find. Therefore, it is not a strong acid. Therefore, the statement, “The quantum mechanical model of the atom describes orbitals in which electrons travel around the nucleus” is false.

Conclusion

The given statement is false.

Interpretation Introduction

(g)

Interpretation:

Whether the statement, “Orbitals are regions in which there is a high probability of finding an electron” is true or false is to be stated.

Concept introduction:

An atom is made up of three subatomic particles-neutrons, protons, and electrons. Neutron and protons are present in the nucleus of the atom, whereas electrons are revolving outside the nucleus in an atom. The electrons are arranged in the orbital of atoms according to their energy.

Answer to Problem 92E

The statement, “Orbitals are regions in which there is a high probability of finding an electron” is true.

Explanation of Solution

Quantum mechanical model states that it is impossible to find the location of electron in an atom. The orbitals are the region where the electrons are most probable to find. Therefore, they are not included in the net ionic equation. Therefore, the statement, “Orbital are regions in which there is a high probability of finding an electron” is true.

Conclusion

The given statement is true.

Interpretation Introduction

(h)

Interpretation:

Whether the statement, “All energy sublevels have the same number of orbitals” is true or false is to be stated.

Concept introduction:

An atom is made up of three subatomic particles-neutrons, protons, and electrons. Neutron and protons are present in the nucleus of the atom, whereas electrons are revolving outside the nucleus in an atom. The electrons are arranged in the orbit of atoms according to their energy.

Answer to Problem 92E

The statement, “All energy sublevels have the same number of orbitals” is false.

Explanation of Solution

The number of orbitals in sublevels increases as their energy increases. The number of orbitals in $s$ is one and number of orbitals $p$ sublevel is three. Therefore, the statement, “All energy sublevels have the same number of orbitals” is false.

Conclusion

The given statement is false.

Interpretation Introduction

(i)

Interpretation:

Whether the statement, “The $3p$ orbitals of an atom are larger than its $2p$ orbitals but smaller than its $4p$ orbitals” is true or false is to be stated.

Concept introduction:

An atom is made up of three subatomic particles-neutrons, protons, and electrons. Neutron and protons are present in the nucleus of the atom, whereas electrons are revolving outside the nucleus in an atom. The electrons are arranged in the orbit of atoms according to their energy.

Answer to Problem 92E

The statement, “The $3p$ orbitals of an atom are larger than its $2p$ orbitals but smaller than its $4p$ orbitals” is true.

Explanation of Solution

The size of the orbital increases as their energy increases. The energy of $3p$ is higher than $2p$. The energy of $4p$ is higher than $3p$. Therefore, the statement, “The $3p$ orbitals of an atom are larger than its $2p$ orbitals but smaller than its $4p$ orbitals” is true.

Conclusion

The given statement is true.

Interpretation Introduction

(j)

Interpretation:

Whether the statement, “At a given sublevel, the maximum number of $d$ electrons is $5$“ is true or false is to be stated.

Concept introduction:

An atom is made up of three subatomic particles-neutrons, protons, and electrons. Neutron and protons are present in the nucleus of the atom, whereas electrons are revolving outside the nucleus in an atom. The electrons are arranged in the orbit of atoms according to their energy.

Answer to Problem 92E

The statement, “At a given sublevel, the maximum number of $d$ electrons is $5$“ is false.

Explanation of Solution

The number of orbital in $d$ subshell is $5$.

The maximum number of electrons that can be occupied by a sublevel can be represented as shown below.

${\text{N}}_{\text{e}}=2{\text{N}}_{\text{o}}$

Where,

• ${\text{N}}_{\text{e}}$ represents the maximum number of electron in a sublevel.

• ${\text{N}}_{\text{o}}$ represents the number of orbital in the sublevel.

Substitute the value of $N_{\text{o}}$ in the above equation.

$\begin{array}{rll}{N}_{\text{e}}& =& 2\left(5\right)\\ & =& 10\end{array}$

Therefore, the statement, “At a given sublevel, the maximum number of $d$ electrons is $5$“ is false.

Conclusion

The given statement is false.

Interpretation Introduction

(k)

Interpretation:

Whether the statement, “The halogens are found in Group $\text{7A}/17$ of the periodic table” is true or false is to be stated.

Concept introduction:

The periodic table represents elements in order of their atomic number. In the modern periodic table, the horizontal rows are known as periods and vertical columns are known as groups. There are seven periods and eighteenth groups in the modern periodic table.

Answer to Problem 92E

The statement, “The halogens are found in Group $\text{7A}/17$ of the periodic table” is true.

Explanation of Solution

The general configuration for the valance shell of the halogen is $\text{n}{s}^2\text{n}{p}^5$. This electronic configuration corresponds to Group $\text{7A}/17$. Therefore, the statement, “The halogens are found in Group $\text{7A}/17$ of the periodic table” is true.

Conclusion

The given statement is true.

Interpretation Introduction

(l)

Interpretation:

Whether the statement, “The dot structure of the alkaline earths is $\text{X}·$, where $\text{X}$ is the symbol of element in the family” is true or false is to be stated.

Concept introduction:

Lewis structure is a representation of a chemical formula of substance with valance electrons of atoms. The Lewis structures are also called electron dot structures. In the Lewis structure, electrons are denoted by dots. Only the valence electrons are presented as dots in the Lewis structure.

Answer to Problem 92E

The statement, “The dot structure of the alkaline earth metals is $\text{X}·$, where $\text{X}$ is the symbol of element in the family” is false.

Explanation of Solution

The general configuration for the valance shell of the alkaline earth metals is $\text{n}{s}^2$. The number of valance electrons in alkaline earth metals is two. The general dot structure of the alkaline earth metals is $\text{X:}$. Therefore, the statement, “The dot structure of the alkaline earth metals is $\text{X}·$, where $\text{X}$ is the symbol of element in the family” is false.

Conclusion

The given statement is false.

Interpretation Introduction

(m)

Interpretation:

Whether the statement, “Stable ions formed by alkaline earth metals are isoelectronic with noble gas atoms” is true or false is to be stated.

Concept introduction:

The ions or atoms which possess the same electron configuration are known as the isoelectronic species. The meaning of isoelectronic species is the species which contains the equal charge. The isoelectronic species shows the similar chemical properties.

Answer to Problem 92E

The statement, “Stable ions formed by alkaline earth metals are isoelectronic with noble gas atoms” is true.

Explanation of Solution

Every element wants to attain an electronic configuration same as noble gas configuration, to do so elements either gain electrons or lose electrons. When an atom of element gains electrons, it forms an anion. When an atom of element loses electrons, it forms a cation. The alkaline earth metals will loss electron to achieve noble gas configuration. Therefore, the statement, “Stable ions formed by alkaline earth metals are isoelectronic with noble gas atoms” is true.

Conclusion

The given statement is true.

Interpretation Introduction

(n)

Interpretation:

Whether the statement, “Atomic numbers $23$ and $45$ both belong to transition elements” is true or false is to be stated.

Concept introduction:

The periodic table represents elements in order of their atomic number. In the modern periodic table, the horizontal rows are known as periods and vertical columns are known as groups. There are seven periods and eighteenth groups in the modern periodic table.

Answer to Problem 92E

The statement, “Atomic numbers $23$ and $45$ both belong to transition elements” is true.

Explanation of Solution

The atomic number of vanadiumis $23$ and it is transition element.

The atomic number of rhodium is $45$ and it is transition element.

Therefore, statement, “Atomic numbers $23$ and $45$ both belong to transition elements” is true.

Conclusion

The given statement is true.

Interpretation Introduction

(o)

Interpretation:

Whether the statement, “Atomic number $52$, $35$, and $18$ are arranged in order of increasing atomic size” is true or false is to be stated.

Concept introduction:

An atom is made up of three subatomic particles-neutrons, protons, and electrons. Neutron and protons are present in the nucleus of the atom, whereas electrons are revolving outside the nucleus in an atom. The electrons are arranged in the orbit of atoms according to their energy.

Answer to Problem 92E

The statement, “Atomic number $52$, $35$, and $18$ are arranged in order of increasing atomic size” is false.

Explanation of Solution

The element with atomic number $52$ is tellurium.

The element with atomic number $35$ is bromine.

The element with atomic number $18$ is argon.

The atomic size of element increases on going from up to down. The size of tellurium is higher than bromine. The size of tellurium is higher than argon.

Therefore, statement, “Atomic number $52$, $35$, and $18$ are arranged in order of increasing atomic size” is false.

Conclusion

The given statement is false.

Interpretation Introduction

(p)

Interpretation:

Whether the statement, “Atomic number $7$, $16$, and $35$ are all nonmetals” is true or false is to be stated.

Concept introduction:

An atom is made up of three subatomic particles-neutrons, protons, and electrons. Neutron and protons are present in the nucleus of the atom, whereas electrons are revolving outside the nucleus in an atom. The electrons are arranged in the orbit of atoms according to their energy.

Answer to Problem 92E

The statement, “Atomic number $7$, $16$, and $35$ are all nonmetals” is true.

Explanation of Solution

The element with atomic number $7$ is nitrogen.

The element with atomic number $16$ is sulfur.

The element with atomic number $35$ is bromine.

All of these elements are nonmetals. Therefore, statement, “Atomic number $7$, $16$, and $35$ are all nonmetals” is true.

Conclusion

The given statement is true.