Concept explainers
(a)
Interpretation:
The hybridization of carbon atom, total C-C σ bonds and π bonds with 1â—¦,2â—¦,3â—¦ and 4â—¦ carbon atoms should be determined.
Concept introduction:
Hybridization is the process of mixing of atomic orbitals to form same energy and same shape hybrid orbitals which form covalent bond with overlapping of atomic orbitals of other atoms. The number of
1â—¦ orPrimary C atom = C atom which is bonded with one another C atom
2â—¦ orSecondary C atom= C atom which is bonded with two other C atoms
3â—¦ orTertiary C atom= C atom which is bonded with three other C atoms
4â—¦ or Quaternary C atom= C atom which is bonded with four other C atoms
(b)
Interpretation:
The hybridization of carbon atom, total C-C σ bonds and π bonds with 1â—¦, 2â—¦,3â—¦ and 4â—¦ carbon atoms should be determined.
Concept introduction:
Hybridization is the process of mixing of atomic orbitals to form same energy and same shape hybrid orbitals which form covalent bond with overlapping of atomic orbitals of other atoms. The number of chemical bonds formed by the atom always determine type of hybridization. Sigma bonds could only form by hybrid orbitals whereas pi bonds are always formed by overlapping of un-hybrid orbitals hence hybridization is not part of pi bond formation.
1â—¦ or Primary C atom = C atom which is bonded with one another C atom
2â—¦ or Secondary C atom= C atom which is bonded with two other C atoms
3â—¦ or Tertiary C atom= C atom which is bonded with three other C atoms
4â—¦ or Quaternary C atom= C atom which is bonded with four other C atoms
(c)
Interpretation:
The hybridization of carbon atom, total C-C σ bonds and π bonds with 1â—¦, 2â—¦,3â—¦ and 4â—¦ carbon atoms should be determined.
Concept introduction:
Hybridization is the process of mixing of atomic orbitals to form same energy and same shape hybrid orbitals which form covalent bond with overlapping of atomic orbitals of other atoms. The number of chemical bonds formed by the atom always determine type of hybridization. Sigma bonds could only form by hybrid orbitals whereas pi bonds are always formed by overlapping of un-hybrid orbitals hence hybridization is not part of pi bond formation.
1â—¦ or Primary C atom = C atom which is bonded with one another C atom
2â—¦ or Secondary C atom= C atom which is bonded with two other C atoms
3â—¦ or Tertiary C atom= C atom which is bonded with three other C atoms
4â—¦ or Quaternary C atom= C atom which is bonded with four other C atoms
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Check out a sample textbook solutionChapter 26 Solutions
General Chemistry: Principles and Modern Applications (11th Edition)
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- 5a) Construct a model of butene, C4H8, using two carbon atoms with planar geometry and two carbon atoms with tetrahedral geometry. How many other isomers of C₂H, can you construct? Draw a dash structural representation of each structure. 5b) How many bonds in butene enjoy free rotation?arrow_forwardSketch the hydrogen bond(s) that form between ethanol and nitrogen trihydride and dihydrogen monoxide. Show the proper VSEPR shapes of all molecules (meaning VSEPR shapes with proper bond angles) and use dotted or dashed lines to indicate the hydrogen bonds. Indicate 4 different H-bonds between: 1) ethanol and nitrogen trihydride 2) ethanol and dihydrogen monoxide 3) dihydrogen monoxide and nitrogen trihydride and then 4) between the two ethanol molecules.arrow_forwardConsider the skeletal structure in line‑angle (line‑bond) mode of 1‑isopropyl‑2‑methylcyclohexane. Identify the number of hydrogen atoms bound to each carbon in the structure.arrow_forward
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