Chapter 7, Problem 7.67PAE

a.

Interpretation Introduction

Interpretation:

Whether ${\text{XeF}}_{\text{2}}$ molecule would be linear or not and does it have lone pairs around the central atom should be identified.

Concept Introduction:

We can predict the shape of a particular molecule by the knowledge of their atomic numbers and VSEPR theory. According to this theory, the atoms take such a position in which there is a minimum possible repulsion between the bonded atoms and the lone pair of electrons if any. For Linear Molecular geometry, the molecules of an atom are arranged in a straight line making an angle of 180^o with the lone pairs if any. A lonepair is the pair of an electron occupying the orbital but not taking part in the bonding.

The main concept behind this theory is that the electron pairs are always present in the outermost shell i.e. valence shell of an atom of a molecule and they repel each other due to which they try to attain the best possible position so that the value of their repulsion is the least. Hence, the electrons occupy such positions around the atom that reduces their repulsion and provides a molecule to their shape.

Here the electrons that take part in the bonding of a molecule are known as the bonding pair and the electrons that do not take part in the bonding are known as the lone pairs. The bond pairs are in the influence of the two bonding atoms whereas the lone pairs are in the influence of only of the atom.

Due to the presence of lone pairs, there is more space occupied between the atoms of the molecules. Now they suffer the repulsion between the lone pair-lone pair and bond pair-lone pair. Their repulsion can be represented as:-

lp-lp>lp-bp>bp-bp

Answer to Problem 7.67PAE

Solution:

The geometry of ${\text{XeF}}_2$ is Linear and it has 3 lone pairs of an electron on the central atom

Explanation of Solution

The electronic configuration of Xeis $4d^{10}5s^{2}5p^{6}5d^0$. In the excited state, the configuration becomes $4d^{10}5s^{1}5p^{3}5d^4$. Thus there is mixing of the s, p and d orbitals to form two half filledsp³d hybrid orbitals. These orbitals combine with hydrogen to form their respective sigma bonds. The arrangement of the bond pair and three lone pair is such that each of them suffers the minimum repulsion. Hence, the shape is Linear Structure of ${\text{XeF}}_2$

The geometry of ${\text{XeF}}_2$ is Linear

The central atom has three lone pairs of electrons

b.

Interpretation Introduction

Interpretation:

Whether ${\text{CO}}_{\text{2}}$ molecule would be linear or not and does it have lone pairs around the central atom should be identified.

Concept Introduction:

We can predict the shape of a particular molecule by the knowledge of their atomic numbers and VSEPR theory. According to this theory, the atoms take such a position in which there is a minimum possible repulsion between the bonded atoms and the lone pair of electrons if any. For Linear Molecular geometry, the molecules of an atom are arranged in a straight line making an angle of 180^o with the lone pairs if any. A lonepair is the pair of an electron occupying the orbital but not taking part in the bonding.

The main concept behind this theory is that the electron pairs are always present in the outermost shell i.e. valence shell of an atom of a molecule and they repel each other due to which they try to attain the best possible position so that the value of their repulsion is the least. Hence, the electrons occupy such positions around the atom that reduces their repulsion and provides a molecule to their shape.

Here the electrons that take part in the bonding of a molecule are known as the bonding pair and the electrons that do not take part in the bonding are known as the lone pairs. The bond pairs are in the influence of the two bonding atoms whereas the lone pairs are in the influence of only of the atom.

Due to the presence of lone pairs, there is more space occupied between the atoms of the molecules. Now they suffer the repulsion between the lone pair-lone pair and bond pair-lone pair. Their repulsion can be represented as:-

lp-lp>lp-bp>bp-bp

Explanation of Solution

The geometry of ${\text{CO}}_2$

is linear and it has 0 lone pairs of an electron on the central atom The electronic configuration of C is $2s^{2}2p^2$. In the excited state, the configuration becomes $2s^{1}2p^3$. Thus there is mixing of the s, p and d orbitals to form two half filled sp hybrid orbitals. These orbitals combine with hydrogen to form their respective pi bonds. The arrangement of the bond pair is such that each of them suffers the minimum repulsion. Hence, the shape is Linear Structure of ${\text{CO}}_2$

The geometry of ${\text{CO}}_2$ is Linear

The central atom has no lone pair of electrons

c.

Interpretation Introduction

Interpretation:

Whether ${\text{BeF}}_{\text{2}}$ molecule would be linear or not and does it have lone pairs around the central atom should be identified.

Concept Introduction We can predict the shape of a particular molecule by the knowledge of their atomic numbers and VSEPR theory. According to this theory, the atoms take such a position in which there is a minimum possible repulsion between the bonded atoms and the lone pair of electrons if any. For Linear Molecular geometry, the molecules of an atom are arranged in a straight line making an angle of 180^o with the lone pairs if any. A lonepair is the pair of an electron occupying the orbital but not taking part in the bonding.

The main concept behind this theory is that the electron pairs are always present in the outermost shell i.e. valence shell of an atom of a molecule and they repel each other due to which they try to attain the best possible position so that the value of their repulsion is the least. Hence, the electrons occupy such positions around the atom that reduces their repulsion and provides a molecule to their shape.

Here the electrons that take part in the bonding of a molecule are known as the bonding pair and the electrons that do not take part in the bonding are known as the lone pairs. The bond pairs are in the influence of the two bonding atoms whereas the lone pairs are in the influence of only of the atom.

Due to the presence of lone pairs, there is more space occupied between the atoms of the molecules. Now they suffer the repulsion between the lone pair-lone pair and bond pair-lone pair. Their repulsion can be represented as:-

Answer to Problem 7.67PAE

lp-lp>lp-bp>bp-bp

Solution: The geometry of ${\text{BeF}}_2$ is Linear and it has 0 lone pairs of an electron on the central atom

Explanation of Solution

The electronic configuration of Be is $2s^2$. In the excited state, the configuration becomes $2s^{1}2p^3$. Thus there is mixing of the s, p and d orbitals to form two half filled sp hybrid orbitals. These orbitals combine with hydrogen to form their respective sigma bonds. The arrangement of the bond pair is such that each of them suffers the minimum repulsion. Hence, the shape is Linear

Structure of ${\text{BeF}}_2$

The geometry of ${\text{BeF}}_2$ is Linear

The central atom has no lone pair of electrons

d.

Interpretation Introduction

Interpretation:

Whether ${\text{OF}}_{\text{2}}$ molecule would be linear or not and does it have lone pairs around the central atom should be identified.

Concept Introduction We can predict the shape of a particular molecule by the knowledge of their atomic numbers and VSEPR theory. According to this theory, the atoms take such a position in which there is a minimum possible repulsion between the bonded atoms and the lone pair of electrons if any. For Linear Molecular geometry, the molecules of an atom are arranged in a straight line making an angle of 180^o with the lone pairs if any. A lonepair is the pair of an electron occupying the orbital but not taking part in the bonding.

The main concept behind this theory is that the electron pairs are always present in the outermost shell i.e. valence shell of an atom of a molecule and they repel each other due to which they try to attain the best possible position so that the value of their repulsion is the least. Hence, the electrons occupy such positions around the atom that reduces their repulsion and provides a molecule to their shape.

Here the electrons that take part in the bonding of a molecule are known as the bonding pair and the electrons that do not take part in the bonding are known as the lone pairs. The bond pairs are in the influence of the two bonding atoms whereas the lone pairs are in the influence of only of the atom.

Due to the presence of lone pairs, there is more space occupied between the atoms of the molecules. Now they suffer the repulsion between the lone pair-lone pair and bond pair-lone pair. Their repulsion can be represented as:-

lp-lp>lp-bp>bp-bp

Answer to Problem 7.67PAE

Solution:

The geometry of ${\text{OF}}_2$ is Bent and it has 2 lone pairs of an electron on the central atom

Explanation of Solution

The electronic configuration of O is $2s^{2}2p^4$ In the excited state the configuration becomes $2s^{1}2p^5$. Thus there is mixing of the s, p and d orbitals to form four half filledsp³ hybrid orbitals. These orbitals combine with fluorine to form their respective pi bonds. The arrangement of the bond pair and two lone pairs on oxygen is such that each of them suffers the minimum repulsion. Hence, the shape is Bent Structure of ${\text{OF}}_2$

The geometry of ${\text{OF}}_2$ is Bent

The central atom has two lone pairs of electrons