**Question 9.**Ethyl amine (H₃CCH₂NH₂) and acetonitrile (H₃CCN) both have lone pairs on N. Draw structures for both of these molecules in the space below.Show each with its **3-dimensional geometry** using lines, wedges, and dashes to show all sigma bonds (note that the framework is provided for acetonitrile, but not ethyl amine). Do not change any of the lines already drawn.Draw orbitals for any **pi bonds** and orbitals containing **lone pairs**.[Diagram Explanation]- The left box is labeled "ethyl amine" and is currently blank.- The right box is labeled "acetonitrile," showing the molecular structure with: - A central carbon (C) triple-bonded to a nitrogen (N) atom. - Two hydrogen (H) atoms bonded to the carbon, showing the typical linear arrangement.**Questions:**What is the hybridization of the orbital that contains the lone pair in each?Ethyl amine: _______________Acetonitrile: _______________

Given molecules are: ethyl amine and acetonitrile. The structure of the molecules are:To know the hybridisation of the N-atom, in each molecule 1)Count the number of atoms that are directly bonded to N-atom. 2) Add number of lone pairs to the number of bonded atoms. 3)If the sum gives two, it corresponds to sp-hybridisation. 4)If the sum gives three, it corresponds to sp2 -hybridisation. 5)If the sum gives four, it corresponds to sp3 -hybridisation. Consider ethylamine molecule: In this, N-atom is in bond with two hydrogens and one carbon ,so total three atoms. It has one lone pair. Sum is 3+1 = 4 Hence, N-atom has sp3 hybridisation in this molecule.Consider acetonitrile molecule: In this, N-atom is in bond with one carbon atom. It has one lone pair. Sum is 1+1 = 2. Two corresponds to sp- hybridisation. Hence, N-atom has sp hybridisation in this molecule.Answer: .