Hybridization - Online Tutor, Practice Problems & Exam Prep

Identify the type of orbitals that overlap to create the sigma bond between the highlighted carbons in each of the following structures.

What orbital accommodates the non-bonding pair of electrons in each of the structures shown below?

Determine the appropriate hybridization of all indicated atoms in the following organic compounds.

Draw the bonds between the given atoms using the orbital hybridization indicated.

C(sp²) with O(sp²)

Another class of reactive intermediates is carbene. It is a neutral species where carbon contains a lone pair of electrons. For the singlet carbene below, determine its central carbon's hybridization and molecular geometry.

Examine the given Lewis structure of propan-1-ol.

What is the hybridization of all the atoms (except for hydrogen)?

Determine the appropriate hybridization of all indicated atoms in the following organic compounds.

What is the hybridization of nitrogen atoms in each of the two resonance forms of butyramide given below?

What orbital accommodates the non-bonding pair of electrons in each of the structures shown below?

A Lewis structure of 1-butene is given below. If there are sp² hybridized atoms, determine the number of sp²-hybridized orbitals used for bonding and the number of unhybridized p orbitals. 

The Lewis structure of 2,2-dichloropropane is given below. Predict the hybridization of all the atoms that are not hydrogen.

Illustrate the overlap of the molecular orbitals in butane showing the hybridizations and shapes of all the carbon atoms. Also, label the σ bonds.

Determine the hybridization of the carbon atoms.

Look at the Lewis structure of 3-butenal below.

Determine the hybridization of all the atoms (except for hydrogen).

Provide an explanation for why the N-H σ bond length is greater in methanamine than in methanimine.

Determine the appropriate hybridization of every carbon, nitrogen, and oxygen atom in these chemical structures.

Predict the hybridization of each carbon atom.

Complete the blanks in each of these sentences with the appropriate number.
(i): __ s orbital, __ p orbital, and __ d orbital produce __ sp³d orbitals after hybridization.
(ii): __ s orbital __ p orbitals, and __ d orbitals produce __ sp³d² orbitals after hybridization.
(iii): __ s orbital, __ p orbitals, and __ d orbitals produce __ sp³d³ orbitals after hybridization.

Examine the given Lewis structure of  propan-1-ol.

If an atom is hybridized as sp², determine the number of sp²-hybridized orbitals utilized for bonding and the number of unhybridized p orbitals present.

Identify the hybridization (sp, sp², or sp³) of the highlighted atoms in the given molecule below.

What are the hybridizations and molecular geometries around the highlighted atoms?

Identify the hybridization of the orbitals that contain the lone pairs in serotonin.

Identify the hybridization of the orbitals used to form the bonds between the specified carbons.

Using resonance structures, determine the hybridization and geometry of the carbon and nitrogen atoms of the following ion:

Using resonance structures, predict the hybridization and geometry of the carbon and nitrogen atoms of the given ion:

Using resonance, determine the hybridization and geometry of the carbon and nitrogen atoms.

Draw the hybrid orbitals of the molecule given below.

• CH₃Cl

Draw the hybrid orbitals of the CH₃CH₂OH molecule.

Draw the hybrid orbitals of the formaldehyde (CH₂O) molecule.

Draw the hybrid orbitals of the acetonitrile (CH₃CN) molecule.

Draw the hybrid molecular orbitals of the BF₃ molecule and determine the number of electrons present in the p orbital of boron.

Draw the molecular orbitals of AlH ₃ and determine the number of electrons present in the  p-orbital of aluminum.

The oxygen-hydrogen bond in water is formed by the overlap of an s orbital with an sp³ orbital. Why is this bond stronger than the bond that would be formed by the overlap of an s orbital with a p orbital?

Determine the orbitals containing the electrons that are shown as lone pairs in pyridine and pyrrole.

Identify the hybridizations as well as approximate bond angles in these molecules:

 a. CH₄

 b. BF₃