What is the maximum number of bonds that can form in a molecule with a central...
What is the maximum number of bonds that can form in a molecule with a central atom containing five electrons in sp 3 hybrid orbitals?
Homework Answers
Hybridization is the concept of mixing atomic orbitals which have different shapes and energies to give an equal number of hybrid orbitals (to that of mixed orbitals), which have the same energy and shape. By using this concept, molecular geometry and bond angles can be explained for molecules.
In the question, hybridization is provided and number of maximum bonds is to be calculated.
Lewis dot structure is used to show bonding in a molecule. It also tells about the number of lone pairs around the central atom.
The table for hybridization with respect to electronic geometry using different combinations of bonds and lone pairs of electrons present on central atom is below:
A compound in which central atom is sp3 hybridized has a total of 4 sp3 hybrid orbitals.
The three single electrons present in three sp3 hybrid orbitals can form 3 sigma bonds with other atoms.
And the fourth hybrid orbital containing a pair of electron is left.
Ans:A maximum of three covalent bonds are formed with a central atom containing five electrons in sp3 hybrid orbitals.
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What is the maximum number of bonds that can form in a molecule with a central...
The hybridization of the central atom in a molecule is described as sp^2. The arrangement in...
The hybridization of the central atom in a molecule is described as sp^2. The arrangement in space of the hybrid orbitals about that atom is linear. trigonal planar. Tetrahedral. Trigonal bipyramidal. Octahedral. What is the hybridization of Br in BrF_3? sp: sp^2 sp^3 dsp^3 d^2 sp^3 Which of these statements is true? A pi bond is twice as strong as a single bond. At bond has cylindrical symmetry about the bonding axis A double bond consists of a pi bond...
18. In which molecule is the central atom sp'd hybridized A. NO B. CIO,C. SO D....
18. In which molecule is the central atom sp'd hybridized A. NO B. CIO,C. SO D. AsFs E. SFs 19. A molecule with the formula AB, and a trigonal planar molecular geometry uses to to f ts ơ bonds. A. sp hybrid orbitals B. sp2 hybrid orbitals C. sp3 hybrid orbitals E. sp'd hybrid orbitals
21) In 1,1,2,2-tetracyanoethylene, INC):CCCN), the nu tetracyanoethylene, (NCICCICN the number of bonds a bonds, and lone...
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I need help with questions 1-8
POST-LAB: LABORATORY 11 Complete on a separate sheet of paper. 1. Indicate whether the molecule is an ion. Then, indicate whether the molecule is polar m. I n. H,PO o. BrO, p. IF q CO2 a. HCN b. H,SO c. HNO, d. BF H,CO, i. SF j. BeCl k. PO, 1. SO, e. XeF f H,O Calculate the number of valence electrons in each structure in question 1 2. Draw a correct Lewis dot...
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U lad Relerences to acces important valaes if needed for this question n Bonding A bond arises from "sideways" overlap of two parallel p orbitals. The electron density lies above and below a plane containing the 2 nuclei that is perpendicular to the orbitals 8- p-orbital p-orbital atom bond atom The maximum number of a bonds that the atom can form is If an atom has sp hybridization in a molecule: The maximum number of p-pt bonds that the atom...
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Which molecule has a central atom that uses the set of hybrid orbitals shown below to form bonds with the non-central atoms?
A Tt bond arises from "sideways" overlap of two parallel p orbitals. The electron In Bonding...
A Tt bond arises from "sideways" overlap of two parallel p orbitals. The electron In Bonding density lies above and below a plane containing the 2 nuclei that is perpendicular to the orbitals p-orbital p-orbitalt bond atomi atom What atomic or hybrid orbitals make up the t bond between N and O in nitrosyl chloride, NOCI? orbital on N+orbital on How many σ bonds does N have in NOCI ? | How many T bonds does N have ? Submit...
Consider each of the following molecules and/or ions. Give the hybridization for the central atom in...
Consider each of the following molecules and/or ions. Give the hybridization for the central atom in each case, and also give the molecular geometry. Ignore any distortions in the geometry due to non-equivalent terminal atoms. molecule or ion central atom hybridization for central atom molecular geometry CIO; (b) Seot (c) coza CO2 Cl2 Answer the following questions about the hybrid orbitals on the phosphorus atom in the POCl; and PClz molecules. What are the expected geometries of these molecules? Ignore...
5. Give the hybridization, electron pair geometry, and molecular geometry of the centrail atom(s) in the...
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The hybridization of the central atom in a molecule is described as sp^2. The arrangement in space of the hybrid orbitals about that atom is linear. trigonal planar. Tetrahedral. Trigonal bipyramidal. Octahedral. What is the hybridization of Br in BrF_3? sp: sp^2 sp^3 dsp^3 d^2 sp^3 Which of these statements is true? A pi bond is twice as strong as a single bond. At bond has cylindrical symmetry about the bonding axis A double bond consists of a pi bond...
18. In which molecule is the central atom sp'd hybridized A. NO B. CIO,C. SO D. AsFs E. SFs 19. A molecule with the formula AB, and a trigonal planar molecular geometry uses to to f ts ơ bonds. A. sp hybrid orbitals B. sp2 hybrid orbitals C. sp3 hybrid orbitals E. sp'd hybrid orbitals
21) In 1,1,2,2-tetracyanoethylene, INC):CCCN), the nu tetracyanoethylene, (NCICCICN the number of bonds a bonds, and lone pairs electrons in the molecule is it bonds bonds lone pairs coge 9 22) Which of the following species would not be expected to have a tetrahedral shape? a) Sif b) BeF, c) BF NF, XeF. 23) All of the following molecules would be polar except HO b) c) d) e) SO, H.O OF F.CO What is the hybridization of the central atom in...
I need help with questions 1-8
POST-LAB: LABORATORY 11 Complete on a separate sheet of paper. 1. Indicate whether the molecule is an ion. Then, indicate whether the molecule is polar m. I n. H,PO o. BrO, p. IF q CO2 a. HCN b. H,SO c. HNO, d. BF H,CO, i. SF j. BeCl k. PO, 1. SO, e. XeF f H,O Calculate the number of valence electrons in each structure in question 1 2. Draw a correct Lewis dot...
U lad Relerences to acces important valaes if needed for this question n Bonding A bond arises from "sideways" overlap of two parallel p orbitals. The electron density lies above and below a plane containing the 2 nuclei that is perpendicular to the orbitals 8- p-orbital p-orbital atom bond atom The maximum number of a bonds that the atom can form is If an atom has sp hybridization in a molecule: The maximum number of p-pt bonds that the atom...
Which molecule has a central atom that uses the set of hybrid orbitals shown below to form bonds with the non-central atoms?
A Tt bond arises from "sideways" overlap of two parallel p orbitals. The electron In Bonding density lies above and below a plane containing the 2 nuclei that is perpendicular to the orbitals p-orbital p-orbitalt bond atomi atom What atomic or hybrid orbitals make up the t bond between N and O in nitrosyl chloride, NOCI? orbital on N+orbital on How many σ bonds does N have in NOCI ? | How many T bonds does N have ? Submit...
Consider each of the following molecules and/or ions. Give the hybridization for the central atom in each case, and also give the molecular geometry. Ignore any distortions in the geometry due to non-equivalent terminal atoms. molecule or ion central atom hybridization for central atom molecular geometry CIO; (b) Seot (c) coza CO2 Cl2 Answer the following questions about the hybrid orbitals on the phosphorus atom in the POCl; and PClz molecules. What are the expected geometries of these molecules? Ignore...
5. Give the hybridization, electron pair geometry, and molecular geometry of the centrail atom(s) in the structures in question 3, 6. For any molecule in question 1 containing lone pair electrons on the central atom, look up and record the literature values for the bond angles of the molecular structure 7. Read the section on hybrid orbitals in your book. Explain how hybrid orbitals are formed using the sp' hybrid orbitals as the example. 8. Double and triple bonds also...
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