Chapter 8, Problem 8.89P

(a)

Interpretation Introduction

Interpretation:

The element with the smallest atomic radius in group $6\text{A}\left(16\right)$ is to be determined.

Concept introduction:

The atomic radius of an element is the measure of the size of its atoms. It is the mean distance from the center of the nucleus to the boundary of the surrounding shells of the electrons. But this boundary is not well defined so the atomic radius cannot be measured.

(b)

Interpretation Introduction

Interpretation:

The element with the largest atomic radius in the period $6$ is to be determined.

Concept introduction:

The atomic radius of an element is the measure of the size of its atoms. It is the mean distance from the center of the nucleus to the boundary of the surrounding shells of the electrons. But this boundary is not well defined so the atomic radius cannot be measured.

(c)

Interpretation Introduction

Interpretation:

The smallest metal in period 3 is to be determined.

Concept introduction:

The metallic character is characterized by the tendency of metals to lose their outermost valence shell electrons. Greater the ease of electron removal, higher will be the electropositivity of the corresponding elements and vice versa.

The metallic character increases from top to bottom in a group because the electrons are less tightly held by the nucleus of the atom and therefore removed easily. It decreases from left to right in a period because the electrons are more tightly held with the nucleus of the atom and therefore the removal becomes difficult.

(d)

Interpretation Introduction

Interpretation:

The element with the highest ${\text{IE}}_1$ in the group $4\text{A}\left(14\right)$ is to be determined.

Concept introduction:

The ionization energy is the amount of energy required to remove the most loosely bound valence electrons from an isolated neutral gaseous atom. It is represented by $\text{IE}$.

Its value varies with the ease of removal of the outermost valence electron. If the outermost electron is removed very easily then the value of ionization energy is very small. If the electron is removed with quite a difficulty then the value of ionization energy will be very high.

When the first electron is removed from a neutral, isolated gaseous atom then the ionization energy is known as the first ionization energy $\left({\text{IE}}_1\right)$. Similarly, when the second electron is removed from the positively charged cation the ionization energy is called the second ionization energy $\left({\text{IE}}_2\right)$ and so on.

(e)

Interpretation Introduction

Interpretation:

The element with the lowest ${\text{IE}}_1$ in period 5 is to be determined.

Concept introduction:

The ionization energy is the amount of energy required to remove the most loosely bound valence electrons from an isolated neutral gaseous atom. It is represented by $\text{IE}$.

Its value varies with the ease of removal of the outermost valence electron. If the outermost electron is removed very easily then the value of ionization energy is very small. If the electron is removed with quite a difficulty then the value of ionization energy will be very high.

When the first electron is removed from a neutral, isolated gaseous atom then the ionization energy is known as the first ionization energy $\left({\text{IE}}_1\right)$. Similarly, when the second electron is removed from the positively charged cation the ionization energy is called the second ionization energy $\left({\text{IE}}_2\right)$ and so on.

(f)

Interpretation Introduction

Interpretation:

The most metallic element in group $5\text{A}\left(15\right)$ is to be determined.

Concept introduction:

The metallic character is characterized by the tendency of metals to lose their outermost valence shell electrons. Greater the ease of electron removal, higher will be the electropositivity of the corresponding elements and vice versa.

The metallic character increases from top to bottom in a group because the electrons are less tightly held by the nucleus of the atom and therefore removed easily. It decreases from left to right in a period because the electrons are more tightly held with the nucleus of the atom and therefore the removal becomes difficult.

(g)

Interpretation Introduction

Interpretation:

The element of the group $\text{3A}\left(13\right)$ that forms the most basic oxide is to be determined.

Concept introduction:

Metal oxides are the chemical compounds formed between metals and oxygen. These oxides generally contain an oxide ion of $-\text{2}$ charge. These oxides are usually basic in nature and exist in a solid state.

Nonmetals react with oxygen to form nonmetal oxides. These are generally present in a gaseous state. These are usually acidic in nature because they release ${\text{H}}^{+}$ ions when dissolved in water.

(h)

Interpretation Introduction

Interpretation:

The element of period 4 that has the highest filled energy level is to be determined.

Concept introduction:

The electrons that are present inside an atom occupy only certain allowed orbitals with a specific energy. The energy corresponding to each of the allowed orbitals are called energy levels.

(i)

Interpretation Introduction

Interpretation:

The element with the condensed ground-state electronic configuration $\left[\text{Ne}\right]3s^{2}3p^2$.

Concept introduction:

The electronic configuration tells about the distribution of electrons in the various atomic orbitals of the element. It is used to predict the chemical properties of the element. The valence shell electronic configuration refers to the distribution of electrons in the outermost shell only.

The condensed electronic configuration is a way to write the electronic configuration where the inner shell configurations are compressed to the nearest noble gas configuration and only the valence shell configuration is written in the expanded form.

(j)

Interpretation Introduction

Interpretation:

The element with the condensed ground-state electronic configuration $\left[\text{Kr}\right]5s^{2}4d^6$ is to be determined.

Concept introduction:

The electronic configuration tells about the distribution of electrons in the various atomic orbitals of the element. It is used to predict the chemical properties of the element. The valence shell electronic configuration refers to the distribution of electrons in the outermost shell only.

The condensed electronic configuration is a way to write the electronic configuration where the inner shell configurations are compressed to the nearest noble gas configuration and only the valence shell configuration is written in the expanded form.

(k)

Interpretation Introduction

Interpretation:

The element that forms $+2$ ion with the electronic configuration $\left[\text{Ar}\right]3d^3$ is to be determined.

Concept introduction:

The electronic configuration tells about the distribution of electrons in the various atomic orbitals of the element. It is used to predict the chemical properties of the element. The valence shell electronic configuration refers to the distribution of electrons in the outermost shell only.

(l)

Interpretation Introduction

Interpretation:

The element of the 5^th period that forms $+3$ ion with pseudo-noble gas configuration is to be determined.

Concept introduction:

The noble gas configuration refers to the stable electronic configuration of the elements with their complete octet. The elements with the noble gas configuration have no or very less tendency to react with the other species and therefore these are extremely stable. This is also used to write the condensed electronic configuration of the elements.

The elements that possess stable electronic configurations in their outermost valence shell but are not actually noble gas configurations. Such electronic configurations are called pseudo noble gas configuration.

The $\left(n-1\right)d^{10}n{s}^{0}n{p}^0$ electronic configuration is known as pseudo noble gas configuration.

The stability of a pseudo noble gas configuration is comparable to that of the noble gas configuration.

(m)

Interpretation Introduction

Interpretation:

The transition element of period 4 that forms $+3$ diamagnetic ion is to be determined.

Concept introduction:

Diamagnetism is the property of materials due to which they are slightly repelled by an externally applied magnetic field. It occurs due to the presence of paired electrons so the atoms with all the filled orbitals are diamagnetic.

(n)

Interpretation Introduction

Interpretation:

The transition element of period 4 that forms $+2$ ion with a half-filled $d$ sublevel is to be determined.

Concept introduction:

The electronic configuration tells about the distribution of electrons in a various atomic orbital. The condensed electronic configuration is a way to write the electronic configuration where the inner shell configurations are compressed to the nearest noble gas configuration and only the valence shell configuration is written in the expanded form.

When a neutral atom gains electrons, it acquires a negative charge on it due to the presence of excess electrons as compared to the protons. This results in the formation of the anion. When a neutral atom loses electrons, it acquires a positive charge on it due to the presence of excess protons as compared to the electrons. This results in the formation of the cation.

(o)

Interpretation Introduction

Interpretation:

The heaviest lanthanide is to be determined.

Concept introduction:

The lanthanide consists of 15 chemical elements from atomic numbers 57 to 71, from lanthanum to lutetium. The elements present in this series have $+3$ as their common oxidation state. There is a large similarity in the atomic radii of the lanthanide elements and therefore these are very difficult to separate.

(p)

Interpretation Introduction

Interpretation:

The element of the 3^rd period that forms $-2$ ion that is isoelectronic with $\text{Ar}$ is to be determined.

Concept introduction:

The isoelectronic species are the atoms, molecules or ions that have the same number of electrons. They differ in their chemical and physical properties. ${\text{Na}}^{+}$, ${\text{Mg}}^{2+}$ and ${\text{Al}}^{3+}$ all have ten electrons so they are isoelectronic species.

(q)

Interpretation Introduction

Interpretation:

The alkaline earth metal whose cation is isoelectronic with $\text{Kr}$ is to be determined.

Concept introduction:

The isoelectronic species are the atoms, molecules or ions that have the same number of electrons. They differ in their chemical and physical properties. ${\text{Na}}^{+}$, ${\text{Mg}}^{2+}$ and ${\text{Al}}^{3+}$ all have ten electrons so they are isoelectronic species.

(r)

Interpretation Introduction

Interpretation:

The metalloid of the group $5\text{A}\left(15\right)$ that forms the most acidic oxide is to be determined.

Concept introduction:

Metal oxides are the chemical compounds formed between metals and oxygen. These oxides generally contain an oxide ion of $-\text{2}$ charge. These oxides are usually basic in nature and exist in a solid state.

Nonmetals react with oxygen to form nonmetal oxides. These are generally present in a gaseous state. These are usually acidic in nature because they release ${\text{H}}^{+}$ ions when dissolved in water.