Concept explainers
(a)
Interpretation:
The hybridization change of boron 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.
(a)
Answer to Problem 11.44P
The hybridization of boron changes from
Explanation of Solution
The Lewis structure of
Boron forms three single bonds with three fluorine atoms so three hybrid orbitals are required and therefore the hybridization of boron in
The Lewis structure of
Boron forms four single bonds with four fluorine atoms so four hybrid orbitals are required and therefore the hybridization of boron in
The hybridization of boron changes from
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.
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
Explanation of Solution
The Lewis structure of
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
The Lewis structure of
Phosphorus forms five single bonds with five chlorine atoms so five hybrid orbitals are required and therefore the hybridization of phosphorus in
The hybridization of phosphorus changes from
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
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
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
The hybridization of carbon changes from
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.
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
Explanation of Solution
The Lewis structure of
Silicon forms four single bonds with four fluorine atoms so four hybrid orbitals are required and therefore the hybridization of silicon in
The Lewis structure of
Silicon forms six single bonds with six fluorine atoms so six hybrid orbitals are required and therefore the hybridization of silicon in
The hybridization of silicon changes from
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.
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
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
The Lewis structure of
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
The hybridization of sulphur remains the same in going from
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
- Reagan is doing an atomic absorption experiment that requires a set of zinc standards in the 0.4- 1.6 ppm range. A 1000 ppm Zn solution was prepared by dissolving the necessary amount of solid Zn(NO3)2 in water. The standards can be prepared by diluting the 1000 ppm Zn solution. Table 1 shows one possible set of serial dilutions (stepwise dilution of a solution) that Reagan could perform to make the necessary standards. Solution A was prepared by diluting 5.00 ml of the 1000 ppm Zn standard to 50.00 ml. Solutions C-E are called "calibration standards" because they will be used to calibrate the atomic absorption spectrometer. Table 1: Dilutions of Zinc Solutions Solution Zinc Solution Volume Diluted Solution Concentration used volume (ppm Zn) (mL) (mL) concentration (ppm Zn) Solution concentration A 1000 5.00 50.00 1.00×10² (ppm Zn(NO3)2) 2.90×10² Solution concentration (M Zn(NO3)2 1.53×10-3 B Solution A 5.00 100.00 5.00 C Solution B 5.00 50.00 0.50 7.65×10-6 D Solution B 10.00 50.00…arrow_forwardNonearrow_forwardNonearrow_forward
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