Chapter 9, Problem 28E

Give the expected hybridization of the central atom for the molecules or ions in Exercises 82 and 88 from Chapter 3.

Interpretation Introduction

Interpretation: The expected hybridization of the central atom, for the given species, is to be determined.

Concept introduction: The following steps are to be followed to determine the hybridization and the molecular structure of a given compound,

• The central atom is identified.
• Its valence electrons are determined.
• $1{\text{e}}^{-}$ is added to the total number of valence electrons for each monovalent atom present.
• The total number obtained is divided by $2$, to find the number of electron pairs.
• This further gives us the hybridization of the given compound.

For an atom, present in the structure of a compound, the sum of the number of bonded atoms and the number of lone pairs present on it gives its steric number. The value of the steric number gives us the hybridization of the atom.

To determine: The expected hybridization of the central atom in ${\text{POCl}}_3$.

Answer to Problem 28E

Answer

The given compound is ${\text{sp}}^3$ hybridized.

Explanation of Solution

The atomic number of phosphorous is 15 and its electronic configuration is,

${\text{1s}}^{\text{2}}{\text{2s}}^{\text{2}}{\text{2p}}^{6}3{\text{s}}^{2}3{\text{p}}^3$

The valence electron of phosphorous is 5

The formula of number of electron pairs is,

$X=\frac{V+M\pm C}{2}$

Where,

• $X$ is number of electron pairs.
• $V$ is valence electrons of central atom.
• $M$ is number of monovalent atoms.
• $C$ is charge on compound.

The number of electron pairs is,

$\begin{array}{c}X=\frac{V+M\pm C}{2}\\ X=\frac{5+3}{2}\\ =4\end{array}$

This means that the central atom shows ${\text{sp}}^{\text{3}}$ hybridization and should have a tetrahedral geometry.

Conclusion

The geometry of a given compound can be predicted using the hybridization of the central atom present.

Interpretation Introduction

Interpretation: The expected hybridization of the central atom, for the given species, is to be determined.

Concept introduction: The following steps are to be followed to determine the hybridization and the molecular structure of a given compound,

• The central atom is identified.
• Its valence electrons are determined.
• $1{\text{e}}^{-}$ is added to the total number of valence electrons for each monovalent atom present.
• The total number obtained is divided by $2$, to find the number of electron pairs.
• This further gives us the hybridization of the given compound.

For an atom, present in the structure of a compound, the sum of the number of bonded atoms and the number of lone pairs present on it gives its steric number. The value of the steric number gives us the hybridization of the atom.

To determine: The expected hybridization of the central atom in ${\text{SO}}_4{}^{2-}$.

Answer to Problem 28E

Answer

The given compound is ${\text{sp}}^3$ hybridized.

Explanation of Solution

The atomic number of sulfur is 16 and its electronic configuration is,

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

The valence electron of sulfur is 6

The formula of number of electron pairs is,

$X=\frac{V+M\pm C}{2}$

Where,

• $X$ is number of electron pairs.
• $V$ is valence electrons of central atom.
• $M$ is number of monovalent atoms.
• $C$ is charge on compound.

The number of electron pairs is,

$\begin{array}{c}X=\frac{V+M\pm C}{2}\\ X=\frac{6+2}{2}\\ =4\end{array}$

This means that the central atom shows ${\text{sp}}^{\text{3}}$ hybridization and should have a tetrahedral geometry.

Conclusion

The geometry of a given compound can be predicted using the hybridization of the central atom present.

Interpretation Introduction

Interpretation: The expected hybridization of the central atom, for the given species, is to be determined.

Concept introduction: The following steps are to be followed to determine the hybridization and the molecular structure of a given compound,

• The central atom is identified.
• Its valence electrons are determined.
• $1{\text{e}}^{-}$ is added to the total number of valence electrons for each monovalent atom present.
• The total number obtained is divided by $2$, to find the number of electron pairs.
• This further gives us the hybridization of the given compound.

For an atom, present in the structure of a compound, the sum of the number of bonded atoms and the number of lone pairs present on it gives its steric number. The value of the steric number gives us the hybridization of the atom.

To determine: The expected hybridization of the central atom in ${\text{XeO}}_4$.

Answer to Problem 28E

Answer

The given compound is ${\text{sp}}^{\text{3}}$ hybridized.

Explanation of Solution

Explanation:

The atomic number of xenon is 54 and its electronic configuration is,

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

The valence electron of xenon is 8

The formula of number of electron pairs is,

$X=\frac{V+M\pm C}{2}$

Where,

• $X$ is number of electron pairs.
• $V$ is valence electrons of central atom.
• $M$ is number of monovalent atoms.
• $C$ is charge on compound.

The number of electron pairs is,

$\begin{array}{c}X=\frac{V+M\pm C}{2}\\ X=\frac{8}{2}\\ =4\end{array}$

This means that the central atom shows ${\text{sp}}^{\text{3}}$ hybridization and should have a tetrahedral geometry.

Conclusion

The geometry of a given compound can be predicted using the hybridization of the central atom present.

Interpretation Introduction

Interpretation: The expected hybridization of the central atom, for the given species, is to be determined.

Concept introduction: The following steps are to be followed to determine the hybridization and the molecular structure of a given compound,

• The central atom is identified.
• Its valence electrons are determined.
• $1{\text{e}}^{-}$ is added to the total number of valence electrons for each monovalent atom present.
• The total number obtained is divided by $2$, to find the number of electron pairs.
• This further gives us the hybridization of the given compound.

For an atom, present in the structure of a compound, the sum of the number of bonded atoms and the number of lone pairs present on it gives its steric number. The value of the steric number gives us the hybridization of the atom.

To determine: The expected hybridization of the central atom in ${\text{PO}}_4{}^{3-}$.

Answer to Problem 28E

Answer

The given compound is ${\text{sp}}^3$ hybridized.

Explanation of Solution

The atomic number of phosphorous is 15 and its electronic configuration is,

${\text{1s}}^{\text{2}}{\text{2s}}^{\text{2}}{\text{2p}}^{6}3{\text{s}}^{2}3{\text{p}}^3$

The valence electron of phosphorous is 5

The formula of number of electron pairs is,

$X=\frac{V+M\pm C}{2}$

Where,

• $X$ is number of electron pairs.
• $V$ is valence electrons of central atom.
• $M$ is number of monovalent atoms.
• $C$ is charge on compound.

The number of electron pairs is,

$\begin{array}{c}X=\frac{V+M\pm C}{2}\\ X=\frac{5+3}{2}\\ =4\end{array}$

This means that the central atom shows ${\text{sp}}^{\text{3}}$ hybridization and should have a tetrahedral geometry.

Conclusion

The geometry of a given compound can be predicted using the hybridization of the central atom present.

Interpretation Introduction

Interpretation: The expected hybridization of the central atom, for the given species, is to be determined.

Concept introduction: The following steps are to be followed to determine the hybridization and the molecular structure of a given compound,

• The central atom is identified.
• Its valence electrons are determined.
• $1{\text{e}}^{-}$ is added to the total number of valence electrons for each monovalent atom present.
• The total number obtained is divided by $2$, to find the number of electron pairs.
• This further gives us the hybridization of the given compound.

For an atom, present in the structure of a compound, the sum of the number of bonded atoms and the number of lone pairs present on it gives its steric number. The value of the steric number gives us the hybridization of the atom.

To determine: The expected hybridization of the central atom in ${\text{ClO}}_4{}^{-}$.

Answer to Problem 28E

Answer

The given compound is ${\text{sp}}^3$ hybridized.

Explanation of Solution

The atomic number of chlorine is 17 and its electronic configuration is,

${\text{1s}}^{\text{2}}{\text{2s}}^{\text{2}}{\text{2p}}^{\text{6}}{\text{3s}}^{\text{2}}{\text{3p}}^{\text{5}}$

The valence electron of chlorine is 7

The formula of number of electron pairs is,

$X=\frac{V+M\pm C}{2}$

Where,

• $X$ is number of electron pairs.
• $V$ is valence electrons of central atom.
• $M$ is number of monovalent atoms.
• $C$ is charge on compound.

The number of electron pairs is,

$\begin{array}{c}X=\frac{V+M\pm C}{2}\\ X=\frac{7+1}{2}\\ =4\end{array}$

This means that the central atom shows ${\text{sp}}^{\text{3}}$ hybridization and should have a tetrahedral geometry.

Conclusion

The geometry of a given compound can be predicted using the hybridization of the central atom present.

Interpretation Introduction

Interpretation: The expected hybridization of the central atom, for the given species, is to be determined.

Concept introduction: The following steps are to be followed to determine the hybridization and the molecular structure of a given compound,

• The central atom is identified.
• Its valence electrons are determined.
• $1{\text{e}}^{-}$ is added to the total number of valence electrons for each monovalent atom present.
• The total number obtained is divided by $2$, to find the number of electron pairs.
• This further gives us the hybridization of the given compound.

For an atom, present in the structure of a compound, the sum of the number of bonded atoms and the number of lone pairs present on it gives its steric number. The value of the steric number gives us the hybridization of the atom.

To determine: The expected hybridization of the central atom in ${\text{NF}}_3$.

Answer to Problem 28E

Answer

The given compound is ${\text{sp}}^3$ hybridized.

Explanation of Solution

The atomic number of nitrogen is 7 and its electronic configuration is,

${\text{1s}}^{\text{2}}{\text{2s}}^{\text{2}}{\text{2p}}^3$

The valence electron of nitrogen is 5

The formula of number of electron pairs is,

$X=\frac{V+M\pm C}{2}$

Where,

• $X$ is number of electron pairs.
• $V$ is valence electrons of central atom.
• $M$ is number of monovalent atoms.
• $C$ is charge on compound.

The number of electron pairs is,

$\begin{array}{c}X=\frac{V+M\pm C}{2}\\ X=\frac{5+3}{2}\\ =4\end{array}$

This means that the central atom shows ${\text{sp}}^{\text{3}}$ hybridization and should have a tetrahedral geometry.

Conclusion

The geometry of a given compound can be predicted using the hybridization of the central atom present.

Interpretation Introduction

Interpretation: The expected hybridization of the central atom, for the given species, is to be determined.

Concept introduction: The following steps are to be followed to determine the hybridization and the molecular structure of a given compound,

• The central atom is identified.
• Its valence electrons are determined.
• $1{\text{e}}^{-}$ is added to the total number of valence electrons for each monovalent atom present.
• The total number obtained is divided by $2$, to find the number of electron pairs.
• This further gives us the hybridization of the given compound.

For an atom, present in the structure of a compound, the sum of the number of bonded atoms and the number of lone pairs present on it gives its steric number. The value of the steric number gives us the hybridization of the atom.

To determine: The expected hybridization of the central atom in ${\text{SO}}_3{}^{2-}$.

Answer to Problem 28E

Answer

The given compound is ${\text{sp}}^{\text{3}}$ hybridized.

Explanation of Solution

The atomic number of sulfur is 16 and its electronic configuration is,

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

The valence electron of sulfur is 6

The formula of number of electron pairs is,

$X=\frac{V+M\pm C}{2}$

Where,

• $X$ is number of electron pairs.
• $V$ is valence electrons of central atom.
• $M$ is number of monovalent atoms.
• $C$ is charge on compound.

The number of electron pairs is,

$\begin{array}{c}X=\frac{V+M\pm C}{2}\\ X=\frac{6+2}{2}\\ =4\end{array}$

This means that the central atom shows ${\text{sp}}^{\text{3}}$ hybridization and should have a tetrahedral geometry.

Conclusion

The geometry of a given compound can be predicted using the hybridization of the central atom present.

Interpretation Introduction

Interpretation: The expected hybridization of the central atom, for the given species, is to be determined.

Concept introduction: The following steps are to be followed to determine the hybridization and the molecular structure of a given compound,

• The central atom is identified.
• Its valence electrons are determined.
• $1{\text{e}}^{-}$ is added to the total number of valence electrons for each monovalent atom present.
• The total number obtained is divided by $2$, to find the number of electron pairs.
• This further gives us the hybridization of the given compound.

For an atom, present in the structure of a compound, the sum of the number of bonded atoms and the number of lone pairs present on it gives its steric number. The value of the steric number gives us the hybridization of the atom.

To determine: The expected hybridization of the central atom in ${\text{PO}}_3{}^{3-}$.

Answer to Problem 28E

Answer

The given compound is ${\text{sp}}^3$ hybridized.

Explanation of Solution

The atomic number of phosphorous is 15 and its electronic configuration is,

${\text{1s}}^{\text{2}}{\text{2s}}^{\text{2}}{\text{2p}}^{6}3{\text{s}}^{2}3{\text{p}}^3$

The valence electron of phosphorous is 5

The formula of number of electron pairs is,

$X=\frac{V+M\pm C}{2}$

Where,

• $X$ is number of electron pairs.
• $V$ is valence electrons of central atom.
• $M$ is number of monovalent atoms.
• $C$ is charge on compound.

The number of electron pairs is,

$\begin{array}{c}X=\frac{V+M\pm C}{2}\\ X=\frac{5+3}{2}\\ =4\end{array}$

This means that the central atom shows ${\text{sp}}^{\text{3}}$ hybridization and should have a tetrahedral geometry.

Conclusion

The geometry of a given compound can be predicted using the hybridization of the central atom present.

Interpretation Introduction

Interpretation: The expected hybridization of the central atom, for the given species, is to be determined.

Concept introduction: The following steps are to be followed to determine the hybridization and the molecular structure of a given compound,

• The central atom is identified.
• Its valence electrons are determined.
• $1{\text{e}}^{-}$ is added to the total number of valence electrons for each monovalent atom present.
• The total number obtained is divided by $2$, to find the number of electron pairs.
• This further gives us the hybridization of the given compound.

For an atom, present in the structure of a compound, the sum of the number of bonded atoms and the number of lone pairs present on it gives its steric number. The value of the steric number gives us the hybridization of the atom.

To determine: The expected hybridization of the central atom in ${\text{ClO}}_3{}^{-}$.

Answer to Problem 28E

Answer

The given compound is ${\text{sp}}^3$ hybridized.

Explanation of Solution

The atomic number of chlorine is 17 and its electronic configuration is,

${\text{1s}}^{\text{2}}{\text{2s}}^{\text{2}}{\text{2p}}^{\text{6}}{\text{3s}}^{\text{2}}{\text{3p}}^{\text{5}}$

The valence electron of chlorine is 7

The formula of number of electron pairs is,

$X=\frac{V+M\pm C}{2}$

Where,

• $X$ is number of electron pairs.
• $V$ is valence electrons of central atom.
• $M$ is number of monovalent atoms.
• $C$ is charge on compound.

The number of electron pairs is,

$\begin{array}{c}X=\frac{V+M\pm C}{2}\\ X=\frac{7+1}{2}\\ =4\end{array}$

This means that the central atom shows ${\text{sp}}^{\text{3}}$ hybridization and should have a tetrahedral geometry.

Conclusion

The geometry of a given compound can be predicted using the hybridization of the central atom present.

Interpretation Introduction

Interpretation: The expected hybridization of the central atom, for the given species, is to be determined.

Concept introduction: The following steps are to be followed to determine the hybridization and the molecular structure of a given compound,

• The central atom is identified.
• Its valence electrons are determined.
• $1{\text{e}}^{-}$ is added to the total number of valence electrons for each monovalent atom present.
• The total number obtained is divided by $2$, to find the number of electron pairs.
• This further gives us the hybridization of the given compound.

For an atom, present in the structure of a compound, the sum of the number of bonded atoms and the number of lone pairs present on it gives its steric number. The value of the steric number gives us the hybridization of the atom.

To determine: The expected hybridization of the central atom in ${\text{ClO}}_2{}^{-}$.

Answer to Problem 28E

The given compound is ${\text{sp}}^3$ hybridized.

Explanation of Solution

The atomic number of chlorine is 17 and its electronic configuration is,

${\text{1s}}^{\text{2}}{\text{2s}}^{\text{2}}{\text{2p}}^{\text{6}}{\text{3s}}^{\text{2}}{\text{3p}}^{\text{5}}$

The valence electron of chlorine is 7

The formula of number of electron pairs is,

$X=\frac{V+M\pm C}{2}$

Where,

• $X$ is number of electron pairs.
• $V$ is valence electrons of central atom.
• $M$ is number of monovalent atoms.
• $C$ is charge on compound.

The number of electron pairs is,

$\begin{array}{c}X=\frac{V+M\pm C}{2}\\ X=\frac{7+1}{2}\\ =4\end{array}$

This means that the central atom shows ${\text{sp}}^{\text{3}}$ hybridization and should have a tetrahedral geometry.

Conclusion

The geometry of a given compound can be predicted using the hybridization of the central atom present.

Interpretation Introduction

Interpretation: The expected hybridization of the central atom, for the given species, is to be determined.

Concept introduction: The following steps are to be followed to determine the hybridization and the molecular structure of a given compound,

• The central atom is identified.
• Its valence electrons are determined.
• $1{\text{e}}^{-}$ is added to the total number of valence electrons for each monovalent atom present.
• The total number obtained is divided by $2$, to find the number of electron pairs.
• This further gives us the hybridization of the given compound.

For an atom, present in the structure of a compound, the sum of the number of bonded atoms and the number of lone pairs present on it gives its steric number. The value of the steric number gives us the hybridization of the atom.

To determine: The expected hybridization of the central atom in ${\text{SCl}}_2$.

Answer to Problem 28E

The given compound is ${\text{sp}}^3$ hybridized.

Explanation of Solution

The atomic number of chlorine is 17 and its electronic configuration is,

${\text{1s}}^{\text{2}}{\text{2s}}^{\text{2}}{\text{2p}}^{\text{6}}{\text{3s}}^{\text{2}}{\text{3p}}^{\text{5}}$

The valence electron of chlorine is 7

The formula of number of electron pairs is,

$X=\frac{V+M\pm C}{2}$

Where,

• $X$ is number of electron pairs.
• $V$ is valence electrons of central atom.
• $M$ is number of monovalent atoms.
• $C$ is charge on compound.

The number of electron pairs is,

$\begin{array}{c}X=\frac{V+M\pm C}{2}\\ X=\frac{6+2}{2}\\ =4\end{array}$

This means that the central atom shows ${\text{sp}}^{\text{3}}$ hybridization and should have a tetrahedral geometry.

Conclusion

The geometry of a given compound can be predicted using the hybridization of the central atom present.

Interpretation Introduction

Interpretation: The expected hybridization of the central atom, for the given species, is to be determined.

Concept introduction: The following steps are to be followed to determine the hybridization and the molecular structure of a given compound,

• The central atom is identified.
• Its valence electrons are determined.
• $1{\text{e}}^{-}$ is added to the total number of valence electrons for each monovalent atom present.
• The total number obtained is divided by $2$, to find the number of electron pairs.
• This further gives us the hybridization of the given compound.

For an atom, present in the structure of a compound, the sum of the number of bonded atoms and the number of lone pairs present on it gives its steric number. The value of the steric number gives us the hybridization of the atom.

To determine: The expected hybridization of the central atom in ${\text{PCl}}_2{}^{-}$.

Answer to Problem 28E

Answer

The given compound is ${\text{sp}}^3$ hybridized.

Explanation of Solution

The atomic number of chlorine is 17 and its electronic configuration is,

${\text{1s}}^{\text{2}}{\text{2s}}^{\text{2}}{\text{2p}}^{\text{6}}{\text{3s}}^{\text{2}}{\text{3p}}^{\text{5}}$

The valence electron of chlorine is 7

The formula of number of electron pairs is,

$X=\frac{V+M\pm C}{2}$

Where,

• $X$ is number of electron pairs.
• $V$ is valence electrons of central atom.
• $M$ is number of monovalent atoms.
• $C$ is charge on compound.

The number of electron pairs is,

$\begin{array}{c}X=\frac{V+M\pm C}{2}\\ X=\frac{5+2+1}{2}\\ =4\end{array}$

This means that the central atom shows ${\text{sp}}^{\text{3}}$ hybridization and should have a tetrahedral geometry.

Conclusion

The geometry of a given compound can be predicted using the hybridization of the central atom present.

Interpretation Introduction

Interpretation: The expected hybridization of the central atom, for the given species, is to be determined.

Concept introduction: The following steps are to be followed to determine the hybridization and the molecular structure of a given compound,

• The central atom is identified.
• Its valence electrons are determined.
• $1{\text{e}}^{-}$ is added to the total number of valence electrons for each monovalent atom present.
• The total number obtained is divided by $2$, to find the number of electron pairs.
• This further gives us the hybridization of the given compound.

For an atom, present in the structure of a compound, the sum of the number of bonded atoms and the number of lone pairs present on it gives its steric number. The value of the steric number gives us the hybridization of the atom.

To determine: The expected hybridization of the central atom in $\left({\text{O}}_3\right)$.

Answer to Problem 28E

The given compound is ${\text{sp}}^2$ hybridized.

Explanation of Solution

The atomic number of oxygen $\left(\text{O}\right)$ is 8 and its electronic configuration is,

${\text{1s}}^{\text{2}}{\text{2s}}^{\text{2}}{\text{2p}}^4$

The valence electron of oxygen is 6

The formula of number of electron pairs is,

$X=\frac{V+M\pm C}{2}$

Where,

• $X$ is number of electron pairs.
• $V$ is valence electrons of central atom.
• $M$ is number of monovalent atoms.
• $C$ is charge on compound.

The number of electron pairs is,

$\begin{array}{c}X=\frac{V+M\pm C}{2}\\ X=\frac{6}{2}\\ =3\end{array}$

This means that the central atom shows ${\text{sp}}^2$ hybridization and should have a triangular planar geometry.

Conclusion

The geometry of a given compound can be predicted using the hybridization of the central atom present.

Interpretation Introduction

Interpretation: The expected hybridization of the central atom, for the given species, is to be determined.

Concept introduction: The following steps are to be followed to determine the hybridization and the molecular structure of a given compound,

• The central atom is identified.
• Its valence electrons are determined.
• $1{\text{e}}^{-}$ is added to the total number of valence electrons for each monovalent atom present.
• The total number obtained is divided by $2$, to find the number of electron pairs.
• This further gives us the hybridization of the given compound.

For an atom, present in the structure of a compound, the sum of the number of bonded atoms and the number of lone pairs present on it gives its steric number. The value of the steric number gives us the hybridization of the atom.

To determine: The expected hybridization of the central atom in ${\text{SO}}_2$.

Answer to Problem 28E

The given compound is ${\text{sp}}^2$ hybridized.

Explanation of Solution

The atomic number of sulfur $\left(\text{S}\right)$ is 16 and its electronic configuration is,

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

The valence electron of sulfur is 6

The formula of number of electron pairs is,

$X=\frac{V+M\pm C}{2}$

Where,

• $X$ is number of electron pairs.
• $V$ is valence electrons of central atom.
• $M$ is number of monovalent atoms.
• $C$ is charge on compound.

The number of electron pairs is,

$\begin{array}{c}X=\frac{V+M\pm C}{2}\\ X=\frac{6}{2}\\ =3\end{array}$

This means that the central atom shows ${\text{sp}}^2$ hybridization and should have a triangular planar geometry.

Conclusion

The geometry of a given compound can be predicted using the hybridization of the central atom present.

Interpretation Introduction

Interpretation: The expected hybridization of the central atom, for the given species, is to be determined.

Concept introduction: The following steps are to be followed to determine the hybridization and the molecular structure of a given compound,

• The central atom is identified.
• Its valence electrons are determined.
• $1{\text{e}}^{-}$ is added to the total number of valence electrons for each monovalent atom present.
• The total number obtained is divided by $2$, to find the number of electron pairs.
• This further gives us the hybridization of the given compound.

For an atom, present in the structure of a compound, the sum of the number of bonded atoms and the number of lone pairs present on it gives its steric number. The value of the steric number gives us the hybridization of the atom.

To determine: The expected hybridization of the central atom in ${\text{SO}}_3$.

Answer to Problem 28E

The given compound is ${\text{sp}}^2$ hybridized.

Explanation of Solution

The atomic number of sulfur $\left(\text{S}\right)$ is 16 and its electronic configuration is,

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

The valence electron of sulfur is 6.

The formula of number of electron pairs is,

$X=\frac{V+M\pm C}{2}$

Where,

• $X$ is number of electron pairs.
• $V$ is valence electrons of central atom.
• $M$ is number of monovalent atoms.
• $C$ is charge on compound.

The number of electron pairs is,

$\begin{array}{c}X=\frac{V+M\pm C}{2}\\ X=\frac{6}{2}\\ =3\end{array}$

This means that the central atom shows ${\text{sp}}^2$ hybridization and should have a triangular planar geometry.

Conclusion

The geometry of a given compound can be predicted using the hybridization of the central atom present.