Finding Hybridization Practice Worksheet Answer Key

Hybridization Practice Worksheet Answer Key:

 

Hybridization Counting Rule: Count all sigma bonds + 1 lone pair*

1) s

  2) sp

    3) sp2

   4) sp3

*exception for nitrogen atoms -> see “The Nitrogen Exception” video in Module 1.

 

Clearly label the hybridization of each non-hydrogen atom and lone pair directly on each molecular structure:

1.

The carbon on the left side of the molecule is sp3 hybridized because it has 4 sigma bonds that are all counted in the hybridization. Note that there are 3 implicit hydrogens not shown on that carbon.

The two carbons in the double bond are sp2 hybridized because they have 3 sigma bonds that are counted in the hybridization, and 1 pi bond that is not counted in the hybridization. Note that the implicit hydrogens on those carbons are not shown.

 

2.

The carbon on the left side of the molecule is sp3 hybridized because it has 4 sigma bonds that are all counted in the hybridization. Note that there are 3 implicit hydrogens not shown on that carbon.

The carbon in the triple bond is sp hybridized because it is bonded to 2 sigma bonds, and 2 pi bonds. The 2 sigma bonds are counted in the hybridization, and the 2 pi bonds are not.

The nitrogen atom in the triple bond is sp hybridized. It has 1 sigma bond that is counted in the hybridization, and 2 pi bonds that are not. The lone pair on the nitrogen is counted in the hybridization because the nitrogen is directly bonded to pi bonds, which tells us that the lone pair will be in a hybridized orbital. The lone pair has the same hybridization as the nitrogen its on, but there is an ~ sign added to its hybridization because it is a lone pair.

*Note that the ~ sign being added to the hybridization of a hybridized lone pair is technically correct, however some notations will not include it. Either way, a hybridized lone pair will always have the same hybridization as the atom its on, and a non-hybridized lone pair will always be in a p-orbital.

 

3.

The two carbons on the ends of the molecule are sp3 hybridized because they have 4 sigma bonds that are all counted in the hybridization. Note that there are 3 implicit hydrogens not shown on each carbon.

The carbon double bonded to the oxygen is sp2 hybridized because it has 3 sigma bonds that are counted in the hybridization, and 1 pi bond that is not counted in the hybridization.

The oxygen is sp hybridized. It has 1 sigma bond that is counted in the hybridization, and 1 pi bond that is not. One lone pair on the oxygen is in a hybridized orbital and is therefore counted in the hybridization, however the second lone pair does not hybridize and is in a p-orbital. This is because only 1 lone pair can ever be in a hybridized orbital.

The hybridized lone pair has the same hybridization as the oxygen atom its on with an about (~) sign included. The non-hybridized lone pair is in a p-orbital.

*Note that the ~ sign being added to the hybridization of a hybridized lone pair is technically correct, however some notations will not include it. Either way, a hybridized lone pair will always have the same hybridization as the atom its on, and a non-hybridized lone pair will always be in a p-orbital.

 

4.

The carbons on the left and right ends of the molecule are sp3 hybridized because they have 4 sigma bonds that are all counted in the hybridization. Note that there are 3 implicit hydrogens not shown on each carbon.

The carbon double bonded to the oxygen is sp2 hybridized because it has 3 sigma bonds that are counted in the hybridization, and 1 pi bond that is not counted in the hybridization.

The oxygen is sp hybridized. It has 1 sigma bond that is counted in the hybridization, and 1 pi bond that is not. One lone pair on the oxygen is in a hybridized orbital and is therefore counted in the hybridization, however the second lone pair does not hybridize and is in a p-orbital. This is because only 1 lone pair can ever be in a hybridized orbital. The hybridized lone pair has the same hybridization as the oxygen atom its on with an about (~) sign included. The non-hybridized lone pair is in a p-orbital.

The nitrogen is sp2 hybridized. It has 3 sigma bonds that are counted in the hybridization and 1 lone pair, but the lone pair is not counted in the hybridization due to the nitrogen being adjacent to a pi bond. Therefore, the lone pair is in a p-orbital.

*Note that the ~ sign being added to the hybridization of a hybridized lone pair is technically correct, however some notations will not include it. Either way, a hybridized lone pair will always have the same hybridization as the atom its on, and a non-hybridized lone pair will always be in a p-orbital.

 

5.

All of the carbons in the ring are sp2 hybridized. Each carbon has 3 sigma bonds that are counted in the hybridization, and 1 pi bond that is not counted in the hybridization. Note that the carbons have an implicit hydrogen that is not shown that counts for 1 of the sigma bonds.

The nitrogen is sp2 hybridized. It has 3 sigma bonds that are counted in the hybridization, and 1 lone pair that is not counted in the hybridization. The lone pair is not counted because the nitrogen is adjacent to a pi bond, so the lone pair stays in a p-orbital.

*Note that the ~ sign being added to the hybridization of a hybridized lone pair is technically correct, however some notations will not include it. Either way, a hybridized lone pair will always have the same hybridization as the atom its on, and a non-hybridized lone pair will always be in a p-orbital.

 

6.

The carbons are all sp3 hybridized because they have 4 sigma bonds that are all counted in the hybridization. Note that the implicit hydrogens on the carbons are not shown.

The oxygen is sp2 hybridized. It has 2 sigma bonds which are both counted in the hybridization. Note that the sigma bond to the hydrogen is now shown. One lone pair on the oxygen is in a hybridized orbital and is therefore counted in the hybridization, however the second lone pair does not hybridize and is in a p-orbital. This is because only 1 lone pair can ever be in a hybridized orbital. The hybridized lone pair has the same hybridization as the oxygen its on with an about (~) sign included. The non-hybridized lone pair is in a p-orbital.

The nitrogen is sp3 hybridized. It has 3 sigma bonds which are all counted in the hybridization, and its lone pair is in a hybridized orbital because it is not adjacent to a pi bond. The hybridized lone pair has the same hybridization as the nitrogen its on, with an about (~) sign included. Note that the bonds between the two hydrogens and the nitrogen are not shown in this example.

*Note that the ~ sign being added to the hybridization of a hybridized lone pair is technically correct, however some notations will not include it. Either way, a hybridized lone pair will always have the same hybridization as the atom its on, and a non-hybridized lone pair will always be in a p-orbital.

 

7.

The terminal carbons on the left and right side of the molecule are sp3 hybridized because they have 4 sigma bonds which are all counted in the hybridization. Note that there are 3 implicit hydrogens on each of those carbons that are not shown.

The two carbons in the double bond are sp2 hybridized. They each have 3 sigma bonds that are counted in the hybridization, and 1 pi bond that is not counted in the hybridization. Note that there is 1 implicit hydrogen on each of those carbons that is not shown.

The formally positive carbon is sp2 hybridized because it has 3 sigma bonds that are counted in the hybridization, and no other bonds or lone pairs. Note that there is 1 implicit hydrogen not shown on that carbon.

 

8.

The carbons on the left and right terminal ends of the molecule are sp3 hybridized. Both carbons have 4 sigma bonds that are all counted in the hybridization. Note that there are 3 implicit hydrogens not shown on each of these carbons.

The two carbons in the double bond are sp2 hybridized. Each carbon has 3 sigma bonds that are counted in the hybridization, and 1 pi bond that is not counted in the hybridization. Note that there is 1 implicit hydrogen not shown on each of these carbons.

The carbon with the formal negative charge is sp2 hybridized. It has 3 sigma bonds that are counted in the hybridization, and 1 lone pair that is not counted in the hybridization. The lone pair is in a p-orbital because lone pairs on negatively charged carbons are in p-orbitals when there is an adjacent pi bond. Note there is an implicit hydrogen not shown on this carbon.

 

9.

All of the carbons in the ring are sp2 hybridized. Each carbon has 3 sigma bonds that are counted in the hybridization, and 1 pi bond that is not counted in the hybridization. Note that the carbons have an implicit hydrogen that is not shown.

The nitrogen is sp2 hybridized. It has 2 sigma bonds that are counted in the hybridization and 1 pi bond that is not counted in the hybridization. The lone pair on the nitrogen is in a hybridized orbital due to the nitrogen being directly connected to a pi bond. Therefore, the lone pair is also counted in the hybridization. The lone pair has the same hybridization as the nitrogen with an about (~) sign added.

*Note that the ~ sign being added to the hybridization of a hybridized lone pair is technically correct, however some notations will not include it. Either way, a hybridized lone pair will always have the same hybridization as the atom its on, and a non-hybridized lone pair will always be in a p-orbital.

 

10.

The methyl group on the left end of the molecule is sp3 hybridized. It has 4 sigma bonds that are all counted in the hybridization. Note that there are 3 implicit hydrogens not shown on this carbon.

The carbon double bonded to the nitrogen is sp2 hybridized. It has 3 sigma bonds that are counted in the hybridization, and 1 pi bond that is not counted in the hybridization.

The nitrogen double bonded to the carbon is sp2 hybridized. It has 2 sigma bonds that are counted in the hybridization, and 1 pi bond that is not counted in the hybridization. The lone pair does not hybridize due to the nitrogen being adjacent to a pi bond. The lone pair is therefore in a p-orbital and is not counted in the hybridization.

The two single bonded carbons to the right of the sp2 carbon double bonded to the nitrogen are both sp3 hybridized. These carbons both have 4 sigma bonds that are all counted in the hybridization. Note that there are 2 implicit hydrogens not shown on each of those carbons.

The nitrogen on the right end of the molecule is sp3 hybridized. It has 3 sigma bonds that are all counted in the hybridization, and it has 1 lone pair that is also counted in the hybridization. The lone pair is in a hybridized orbital because they nitrogen is not adjacent to a pi bond. The hybridized lone pair has the same hybridization as the nitrogen its on, with an about (~) sign included. The non-hybridized lone pair stays in a p-orbital. Note that the bonds to each hydrogen are not shown in this example.

*Note that the ~ sign being added to the hybridization of a hybridized lone pair is technically correct, however some notations will not include it. Either way, a hybridized lone pair will always have the same hybridization as the atom its on, and a non-hybridized lone pair will always be in a p-orbital.

 

11. 

The two carbons on the right side of the molecule in the ethyl chain are both sp3 hybridized. They each have 4 sigma bonds which are all included in the hybridization. Note that there are implicit hydrogens not shown on each of those carbons.

All of the carbons in the 6-carbon benzene ring, and the two carbons with the pi bond connected to the ethyl group are all sp2 hybridized. They each have 3 sigma bonds which are counted in the hybridization, and 1 pi bond that is not counted in the hybridization. Note that some of those carbons have implicit hydrogens that are not shown.

The oxygen is sp2 hybridized. It has 2 sigma bonds that are counted in the hybridization, and 1 lone pair that is counted in the hybridization. However, the second lone pair does not hybridize and is in a p-orbital. This is because only 1 lone pair can ever be in a hybridized orbital. The hybridized lone pair has the same hybridization as the oxygen its on with an about (~) sign included. The non-hybridized lone pair is in a p-orbital.

*Note that the ~ sign being added to the hybridization of a hybridized lone pair is technically correct, however some notations will not include it. Either way, a hybridized lone pair will always have the same hybridization as the atom its on, and a non-hybridized lone pair will always be in a p-orbital.

 

12.

The carbon on the left end of the molecule and the carbon on the right end of the molecule bonded to bromine are both sp3 hybridized. Both carbons have 4 sigma bonds that are all counted in the hybridization. Note that there are implicit hydrogens not shown on each of those carbons.

The two carbons in the double bond are sp2 hybridized. They each have 3 sigma bonds that are counted in the hybridization, and 1 pi bond that is not counted in the hybridization. Note that there is 1 implicit hydrogen not shown on each of those carbons.

The bromine is sp hybridized. It has 1 sigma bond that is counted in the hybridization, and 1 lone pair that is counted in the hybridization. However, the second and third lone pairs do not hybridize and are in p-orbitals. This is because only 1 lone pair can ever be in a hybridized orbital. The hybridized lone pair has the same hybridization as the bromine its on with an about (~) sign included. The non-hybridized lone pairs are in p-orbitals.

*Note that the ~ sign being added to the hybridization of a hybridized lone pair is technically correct, however some notations will not include it. Either way, a hybridized lone pair will always have the same hybridization as the atom its on, and a non-hybridized lone pair will always be in a p-orbital.

 

13.

The carbons in the ring that have pi bonds are all sp2 hybridized. They have 3 sigma bonds which are all counted in the hybridization, and 1 pi bond that is not counted in the hybridization. Note that these carbons all have an implicit hydrogen that is not shown.

The two carbons without any pi bonds in the ring are sp3 hybridized. Both carbons have 4 sigma bonds that are all counted in the hybridization. Note that there are implicit hydrogens not shown on each of those carbons.

The carbon double bonded to the sulfur is sp2 hybridized. It has 3 sigma bonds that are counted in the hybridization, and it has 1 pi bond which is not counted in the hybridization.

The sulfur is sp hybridized. It has 1 sigma bond which is counted in the hybridization, and it has 1 pi bond that is not counted in the hybridization. One lone pair on the sulfur is in a hybridized orbital and is therefore counted in the hybridization, however the second lone pair does not hybridize and is in a p-orbital. This is because only 1 lone pair can ever be in a hybridized orbital. The hybridized lone pair has the same hybridization as the sulfur atom its on with an about (~) sign included.

The carbon bonded to the ring with a wedge is sp3 hybridized. It has 4 sigma bonds that are all counted in the hybridization. Note that there are 2 implicit hydrogens not shown on that carbon.

The carbon triple bonded to the nitrogen is sp hybridized because it is bonded to 2 sigma bonds, and 2 pi bonds. The 2 sigma bonds are counted in the hybridization, and the 2 pi bonds are not.

The nitrogen is sp hybridized. It has 1 sigma bond that is counted in the hybridization, and 2 pi bonds that are not counted in the hybridization. The lone pair on the nitrogen is counted in the hybridization because the nitrogen is directly bonded to a pi bond, so the lone pair will hybridize. The hybridized lone pair has the same hybridization as the nitrogen atom its on with an about (~) sign included.

*Note that the ~ sign being added to the hybridization of a hybridized lone pair is technically correct, however some notations will not include it. Either way, a hybridized lone pair will always have the same hybridization as the atom its on, and a non-hybridized lone pair will always be in a p-orbital.

 

14.  

The carbons in the ring that are part of the triple bond are sp hybridized. They have 2 sigma bonds that are counted in the hybridization, and 2 pi bonds that are not counted in the hybridization.

The remaining 4 carbons in the ring are all sp2 hybridized. They have 3 sigma bonds that are counted in the hybridization, and 1 pi bond that is not counted in the hybridization. Note that there is an implicit hydrogen not shown on 3 of those carbons.

The methyl group substituent coming off the ring is sp3 hybridized. It has 4 sigma bonds that are all counted in the hybridization. Note that there are 3 implicit hydrogens not shown on that carbon.

The chlorine is sp hybridized. It has 1 sigma bond that is counted in the hybridization, and 1 lone pair that is counted in the hybridization. However, the second and third lone pairs do not hybridize and are in a p-orbital. This is because only 1 lone pair can ever be in a hybridized orbital. The hybridized lone pair has the same hybridization as the chlorine its on with an about (~) sign included. The non-hybridized lone pairs are in p-orbitals.

*Note that the ~ sign being added to the hybridization of a hybridized lone pair is technically correct, however some notations will not include it. Either way, a hybridized lone pair will always have the same hybridization as the atom its on, and a non-hybridized lone pair will always be in a p-orbital.

 

15.

All 4 carbons in the tert-butyl substituent on the ring are sp3 hybridized. They all have 4 sigma bonds that are all counted in the hybridization. Note that there are 3 implicit hydrogens on the terminal carbons that are not shown.

The 4 carbons in the ring are all sp2 hybridized. They all have 3 sigma bonds that are counted in the hybridization, and 1 pi bond that is not counted in the hybridization. Note that there is an implicit hydrogen not shown on 3 of those carbons.

The nitrogen is sp2 hybridized. It has 3 sigma bonds that are counted in the hybridization, and 1 lone pair that is not counted in the hybridization. This is due to the nitrogen being adjacent to a pi bond. The lone pair is therefore in a p-orbital.

 

16.

The carbon on the left end of the molecule is sp3 hybridized. It has 4 sigma bonds which are all counted in the hybridization. Note that there are 3 implicit hydrogens not shown.

The carbon double bonded to the oxygen is sp2 hybridized. It has 3 sigma bonds that are counted in the hybridization, and 1 pi bond that is not counted in the hybridization.

The oxygen double bonded to the carbon is sp hybridized. It has 1 sigma bond that is counted in the hybridization, and 1 pi bond that is not. One lone pair on the oxygen is in a hybridized orbital and is therefore counted in the hybridization, however the second lone pair does not hybridize and is in a p-orbital. This is because only 1 lone pair can ever be in a hybridized orbital. The hybridized lone pair has the same hybridization as the oxygen atom its on with an about (~) sign included.

The nitrogen is sp2 hybridized. It has 3 sigma bonds that are counted in the hybridization, and 1 lone pair that is not counted in the hybridization. The lone pair does not hybridize due to the nitrogen being adjacent to a pi bond. The lone pair is therefore in a p-orbital. Note that the bond between the hydrogen and nitrogen is not shown in this example.

All 6 carbons in the ring are sp2 hybridized. They all have 3 sigma bonds that are counted in the hybridization, and 1 pi bond that is not counted in the hybridization. Note that there is an implicit hydrogen not shown on 4 of those carbons.

The oxygen bonded to the ring is sp2 hybridized. It has 2 sigma bonds which are counted in the hybridization, and 1 lone pair that is counted in the hybridization. However, the second lone pair does not hybridize and is in a p-orbital. This is because only 1 lone pair can ever be in a hybridized orbital. The hybridized lone pair has the same hybridization as the oxygen its on with an about (~) sign included. The non-hybridized lone pair is in a p-orbital.

*Note that the ~ sign being added to the hybridization of a hybridized lone pair is technically correct, however some notations will not include it. Either way, a hybridized lone pair will always have the same hybridization as the atom its on, and a non-hybridized lone pair will always be in a p-orbital.

 

17.

The 4 single bonded carbons on the left side of the molecule are all sp3 hybridized. Each carbon has 4 sigma bonds that are counted in the hybridization. Note that there are implicit hydrogens not shown on these carbons.

All 6 carbons in the benzene ring are sp2 hybridized. Each carbon has 3 sigma bonds that are counted in the hybridization and 1 pi bond that is not counted in the hybridization. Note that there are implicit hydrogens not shown on some of these carbons.

The carbon directly bonded to the right side of the benzene ring is sp3 hybridized. It has 4 sigma bonds that are counted in the hybridization. Note that there is an implicit hydrogen not shown on this carbon.

The dashed methyl group on the right side of the molecule is sp3 hybridized. It has 4 sigma bonds that are counted in the hybridization. Note that there are 3 implicit hydrogens not shown on this carbon.

The carbon double bonded to the oxygen is sp2 hybridized. It has 3 sigma bonds that are counted in the hybridization, and 1 pi bond that is not counted in the hybridization.

The oxygen double bonded to the carbon is sp hybridized. It has 1 sigma bond that is counted in the hybridization, and 1 pi bond that is not. One lone pair on the oxygen is in a hybridized orbital and is therefore counted in the hybridization, however the second lone pair does not hybridize and is in a p-orbital. This is because only 1 lone pair can ever be in a hybridized orbital. The hybridized lone pair has the same hybridization as the oxygen atom its on with an about (~) sign included.

The single bonded oxygen on the right side of the molecule is sp2 hybridized. It has 2 sigma bonds which are counted in the hybridization, and 1 lone pair that is counted in the hybridization. However, the second lone pair does not hybridize and is in a p-orbital. This is because only 1 lone pair can ever be in a hybridized orbital. The hybridized lone pair has the same hybridization as the oxygen its on with an about (~) sign included.

*Note that the ~ sign being added to the hybridization of a hybridized lone pair is technically correct, however some notations will not include it. Either way, a hybridized lone pair will always have the same hybridization as the atom its on, and a non-hybridized lone pair will always be in a p-orbital.

 

18.

The two carbons on the ethyl chain on the left side of the molecule are sp3 hybridized. Both carbons have 4 sigma bonds which are all counted in the hybridization. Note that there are implicit hydrogens on these carbons that are not shown.

The carbon double bonded to the oxygen is sp2 hybridized. It has 3 sigma bonds that are counted in the hybridization, and 1 pi bond that is not counted in the hybridization.

The oxygen double bonded to the carbon is sp hybridized. It has 1 sigma bond that is counted in the hybridization, and 1 pi bond that is not. One lone pair on the oxygen is in a hybridized orbital and is therefore counted in the hybridization, however the second lone pair does not hybridize and is in a p-orbital. This is because only 1 lone pair can ever be in a hybridized orbital. The hybridized lone pair has the same hybridization as the oxygen atom its on with an about (~) sign included.

The nitrogen bonded to the carbonyl functional group is sp2 hybridized. It has 3 sigma bonds that are counted in the hybridization, and 1 lone pair that is not counted in the hybridization. The lone pair does not hybridize due to the nitrogen being adjacent to a pi bond. The lone pair is therefore in a p-orbital.

Both benzene rings in the molecule have all sp2 carbons. Each of these carbons has 3 sigma bonds that are counted in the hybridization, and 1 pi bond that is not counted in the hybridization. Note that some of the carbons in the rings have an implicit hydrogen that is not shown.

The single bonded carbons in the 6-membered ring that includes the nitrogen are all sp3 hybridized. All of these carbons have 4 sigma bonds which are all counted in the hybridization. Note that there are implicit hydrogens on these carbons that are not shown.

The nitrogen in the 6-membered ring with single bonds is sp3 hybridized. It has 3 sigma bonds which are all counted in the hybridization, and its lone pair is in a hybridized orbital because it is not adjacent to a pi bond. The hybridized lone pair has the same hybridization as the nitrogen its on, with an about (~) sign included.

The two single bonded carbons attached to the sp3 hybridized nitrogen are both sp3 hybridized. Both carbons have 4 sigma bonds that are all counted in the hybridization. Note that there are 2 implicit hydrogens not shown on each of these carbons.

*Note that the ~ sign being added to the hybridization of a hybridized lone pair is technically correct, however some notations will not include it. Either way, a hybridized lone pair will always have the same hybridization as the atom its on, and a non-hybridized lone pair will always be in a p-orbital.

 

19. 

The carbon on the left end of the molecule is sp3 hybridized. It has 4 sigma bonds which are all counted in the hybridization. Note that there are 3 implicit hydrogens not shown.

The formally negative carbon with the lone pair is sp2 hybridized. It has 3 sigma bonds that are counted in the hybridization, and 1 lone pair that is not counted in the hybridization. The lone pair is in a p-orbital because lone pairs on negatively charged carbons are in p-orbitals when there is an adjacent pi bond. Note there is an implicit hydrogen not shown on this carbon.

The carbon double bonded to the oxygen is sp2 hybridized because it has 3 sigma bonds that are counted in the hybridization, and 1 pi bond that is not counted in the hybridization.

The oxygen is sp hybridized. It has 1 sigma bond that is counted in the hybridization, and 1 pi bond that is not. One lone pair on the oxygen is in a hybridized orbital and is therefore counted in the hybridization, however the second lone pair does not hybridize and is in a p-orbital. This is because only 1 lone pair can ever be in a hybridized orbital. The hybridized lone pair has the same hybridization as the oxygen atom its on with an about (~) sign included.

The nitrogen is sp3 hybridized. It has 4 sigma bonds that are all counted in the hybridization. The formal positive charge on the nitrogen has no effect on its hybridization.

*Note that the ~ sign being added to the hybridization of a hybridized lone pair is technically correct, however some notations will not include it. Either way, a hybridized lone pair will always have the same hybridization as the atom its on, and a non-hybridized lone pair will always be in a p-orbital.

 

20.

The carbon on the left end of the molecule is sp3 hybridized. It has 4 sigma bonds that are counted in the hybridization. Note that there are 3 implicit hydrogens not shown.

The two carbons involved in the double bond are sp2 hybridized. They each have 3 sigma bonds that are counted in the hybridization, and 1 pi bond that is not counted in the hybridization.

The single bonded nitrogen is sp2 hybridized. It has 3 sigma bonds that are counted in the hybridization, and 1 lone pair that is not counted in the hybridization. The lone pair does not hybridize due to the nitrogen being adjacent to a pi bond. The lone pair is therefore in a p-orbital. Note that the bonds to each hydrogen are not shown in this example.

The carbon double bonded to the nitrogen is sp2 hybridized. It has 3 sigma bonds that are counted in the hybridization, and 1 pi bond that is not counted in the hybridization.

The nitrogen double bonded to the carbon is sp2 hybridized. It has 2 sigma bonds that are counted in the hybridization, and 1 pi bond that is not counted in the hybridization. The lone pair does not hybridize due to the nitrogen being adjacent to a pi bond. The lone pair is therefore in a p-orbital.

The two single bonded carbons to the right of the double bonded nitrogen are sp3 hybridized. Both carbons have 4 sigma bonds that are all counted in the hybridization. Note that there are 2 implicit hydrogens not shown on each carbon.

The nitrogen on the right end of the molecule is sp3 hybridized. It has 3 sigma bonds that are all counted in the hybridization, and it has 1 lone pair that is also counted in the hybridization. The lone pair is in a hybridized orbital because the nitrogen is not adjacent to a pi bond. The hybridized lone pair has the same hybridization as the nitrogen its on, with an about (~) sign included. The non-hybridized lone pair stays in a p-orbital. Note that the bonds to each hydrogen are not shown in this example.

*Note that the ~ sign being added to the hybridization of a hybridized lone pair is technically correct, however some notations will not include it. Either way, a hybridized lone pair will always have the same hybridization as the atom its on, and a non-hybridized lone pair will always be in a p-orbital.