Concept explainers
(a)
Interpretation:
The hybridization change of boron in the following reaction is to be determined.
BF3+NaF→Na+BF−4
Concept introduction:
The atomic orbital is the wave function that is used to find the probability to find an electron around the nucleus of an atom. It is the space around the nucleus of an atom where the electrons are supposed to be found.
Hybridization is the process of intermixing of atomic orbital of slightly different energies to form hybrid orbitals that have similar energy. These orbital have lower energy and more stability than the atomic orbital.
Hybridization of the central atom can be determined from the number of electron groups around the central atom in the Lewis structure of the molecule. Single bond, double bond, triple bond and lone pair all are considered as single electron group.
(a)
Answer to Problem 11.44P
The hybridization of boron changes from sp2 to sp3.
Explanation of Solution
The Lewis structure of BF3 is as follows:
Boron forms three single bonds with three fluorine atoms so three hybrid orbitals are required and therefore the hybridization of boron in BF3 is sp2.
The Lewis structure of BF−4 is as follows:
Boron forms four single bonds with four fluorine atoms so four hybrid orbitals are required and therefore the hybridization of boron in BF−4 is sp3.
The hybridization of boron changes from sp2 to sp3.
Hybridization is determined from the number of electron groups around the central atom in the Lewis structure of the molecule.
(b)
Interpretation:
The hybridization change for phosphorus in the following reaction is to be determined.
PCl3+Cl2→PCl5
Concept introduction:
The atomic orbital is the wave function that is used to find the probability to find an electron around the nucleus of an atom. It is the space around the nucleus of an atom where the electrons are supposed to be found.
Hybridization is the process of intermixing of atomic orbital of slightly different energies to form hybrid orbitals that have similar energy. These orbital have lower energy and more stability than the atomic orbital.
Hybridization of the central atom can be determined from the number of electron groups around the central atom in the Lewis structure of the molecule. Single bond, double bond, triple bond and lone pair all are considered as single electron group.
(b)
Answer to Problem 11.44P
The hybridization of phosphorus changes from sp3 to sp3d.
Explanation of Solution
The Lewis structure of PCl3 is as follows:
Phosphorus forms three single bonds with three chlorine atoms and has a lone pair on it so four hybrid orbitals are required and therefore the hybridization of phosphorus in PCl3 is sp3.
The Lewis structure of PCl5 is as follows:
Phosphorus forms five single bonds with five chlorine atoms so five hybrid orbitals are required and therefore the hybridization of phosphorus in PCl5 is sp3d.
The hybridization of phosphorus changes from sp3 to sp3d.
Hybridization is determined from the number of electron groups around the central atom in the Lewis structure of the molecule.
(c)
Interpretation:
The hybridization change for carbon in the following reaction is to be determined.
Concept introduction:
The atomic orbital is the wave function that is used to find the probability to find an electron around the nucleus of an atom. It is the space around the nucleus of an atom where the electrons are supposed to be found.
Hybridization is the process of intermixing of atomic orbital of slightly different energies to form hybrid orbitals that have similar energy. These orbital have lower energy and more stability than the atomic orbital.
Hybridization of the central atom can be determined from the number of electron groups around the central atom in the Lewis structure of the molecule. Single bond, double bond, triple bond and lone pair all are considered as single electron group.
(c)
Answer to Problem 11.44P
The hybridization of carbon changes from sp to sp2.
Explanation of Solution
The Lewis structure of acetylene is as follows:
Carbon forms one triple bond with other carbon atom and one single bond with hydrogen atom so two hybrid orbitals are required and therefore the hybridization of carbon in acetylene is sp.
The Lewis structure of ethene is as follows:
Carbon forms two single bonds with two hydrogen atoms and one double bond with another carbon atom so three hybrid orbitals are required and therefore the hybridization of carbon in ethene is sp2.
The hybridization of carbon changes from sp to sp2.
Hybridization is determined from the number of electron groups around the central atom in the Lewis structure of the molecule.
(d)
Interpretation:
The hybridization change for silicon in the following reaction is to be determined.
SiF4+2F−→SiF2−6
Concept introduction:
The atomic orbital is the wave function that is used to find the probability to find an electron around the nucleus of an atom. It is the space around the nucleus of an atom where the electrons are supposed to be found.
Hybridization is the process of intermixing of atomic orbital of slightly different energies to form hybrid orbitals that have similar energy. These orbital have lower energy and more stability than the atomic orbital.
Hybridization of the central atom can be determined from the number of electron groups around the central atom in the Lewis structure of the molecule. Single bond, double bond, triple bond and lone pair all are considered as single electron group.
(d)
Answer to Problem 11.44P
The hybridization of silicon changes from sp3 to sp3d2.
Explanation of Solution
The Lewis structure of SiF4 is as follows:
Silicon forms four single bonds with four fluorine atoms so four hybrid orbitals are required and therefore the hybridization of silicon in SiF4 is sp3.
The Lewis structure of SiF2−6 is as follows:
Silicon forms six single bonds with six fluorine atoms so six hybrid orbitals are required and therefore the hybridization of silicon in SiF2−6 is sp3d2.
The hybridization of silicon changes from sp3 to sp3d2.
Hybridization is determined from the number of electron groups around the central atom in the Lewis structure of the molecule.
(e)
Interpretation:
The hybridization of sulphur in the following reaction is to be determined.
SO2+12O2→SO3
Concept introduction:
The atomic orbital is the wave function that is used to find the probability to find an electron around the nucleus of an atom. It is the space around the nucleus of an atom where the electrons are supposed to be found.
Hybridization is the process of intermixing of atomic orbital of slightly different energies to form hybrid orbitals that have similar energy. These orbital have lower energy and more stability than the atomic orbital.
Hybridization of the central atom can be determined from the number of electron groups around the central atom in the Lewis structure of the molecule. Single bond, double bond, triple bond and lone pair all are considered as single electron group.
(e)
Answer to Problem 11.44P
There is no change in the hybridization of sulphur.
Explanation of Solution
The Lewis structure of SO2 is as follows:
Sulphur forms one single, one double bond with two oxygen atoms separately. It has a lone pair of electrons on it. So three hybrid orbitals are required and therefore the hybridization of sulphur in SO2 is sp2.
The Lewis structure of SO3 is as follows:
Sulphur forms two single bonds and one double bond with three oxygen atoms separately so three hybrid orbitals are required and therefore the hybridization of sulphur in SO3 is sp2.
The hybridization of sulphur remains the same in going from SO2 to SO3.
Hybridization is determined from the number of electron groups around the central atom in the Lewis structure of the molecule.
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Chapter 11 Solutions
Student Solutions Manual For Silberberg Chemistry: The Molecular Nature Of Matter And Change With Advanced Topics
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