For each of the following compounds and ions,
1. Draw a Lewis structure.
2. Show the kinds of orbitals that overlap to form each bond.
3. Give approximate bond angles around each atom except hydrogen.
c. CH₂=N–CH₃

Verified step by step guidance

Step 1: Draw the Lewis structure for CH2=NCH3. Start by counting the total number of valence electrons. Carbon has 4 valence electrons, nitrogen has 5, and hydrogen has 1. The total is 18 valence electrons.

Step 2: Arrange the atoms with carbon as the central atom for the CH2 group and nitrogen as the central atom for the NCH3 group. Connect the atoms with single bonds initially, and then adjust to satisfy the octet rule, forming a double bond between carbon and nitrogen.

Step 3: Identify the types of orbitals involved in bonding. The C-H bonds are formed by the overlap of sp3 hybrid orbitals from carbon with the s orbitals of hydrogen. The C=N double bond involves sp2 hybrid orbitals from carbon and nitrogen, with one sigma bond and one pi bond.

Step 4: Determine the hybridization of each atom. The carbon in CH2 is sp2 hybridized, the nitrogen is sp2 hybridized, and the carbon in CH3 is sp3 hybridized.

Step 5: Estimate the bond angles. Around the sp2 hybridized carbon and nitrogen, the bond angles are approximately 120 degrees. Around the sp3 hybridized carbon in CH3, the bond angles are approximately 109.5 degrees.

Verified video answer for a similar problem:

This video solution was recommended by our tutors as helpful for the problem above.

Was this helpful?

Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Lewis Structure

A Lewis structure is a diagram that represents the valence electrons of atoms within a molecule. It shows how atoms are bonded together and the lone pairs of electrons. For CH2=NCH3, the structure involves drawing the carbon-nitrogen double bond and ensuring the correct placement of hydrogen atoms and lone pairs on nitrogen.

Orbital Overlap

Orbital overlap refers to the interaction between atomic orbitals that leads to bond formation. In CH2=NCH3, the carbon-nitrogen double bond involves sp2 hybridized orbitals overlapping with a p orbital from nitrogen, while the single bonds between carbon and hydrogen involve sp3 hybridized orbitals overlapping with s orbitals from hydrogen.

Bond Angles

Bond angles are the angles between adjacent bonds at an atom. They are determined by the hybridization and geometry of the molecule. In CH2=NCH3, the bond angles around the sp2 hybridized carbon are approximately 120 degrees, while the angles around the sp3 hybridized carbon in CH3 are approximately 109.5 degrees.

Recommended video:

Guided course