The reaction between trimethyl amine and HCl is to be shown and the expected hybridization state for the nitrogen atom in the product is to be predicted. Concept Introduction: ▸ Lewis acids are electron pair acceptors. ▸ Lewis bases are electron pair donors. ▸ The valence shell electron pair repulsion (VSEPR) theory predicts the arrangement of atoms in molecules and ions. ▸ Amines are the organic compounds that contain an amino group ( − NH 2 ) . ▸ They can act as nucleophiles and electrophiles in organic reactions. ▸ Amines can be classified into three categories: primary amines, secondary amines, and tertiary amines. ▸ If the nitrogen atom is directly attached to only one other carbon atom, the amine is a primary amine. ▸ If the nitrogen atom is directly attached to two other carbon atoms, the amine is a secondary amine. ▸ If the nitrogen atom is directly attached to three other carbon atoms, the amine is a tertiary amine. ▸ Higher the electron density around the nitrogen atom, more available is the electron pair to donate. Electron donors are Lewis bases. ▸ The reaction is Lewis acid- base reaction. The trimethyl amine donates a pair of electrons, so it acts as a Lewis base and HCl accepts a pair of electrons, and so acts as a Lewis acid. ▸ Hybridization is the concept of mixing atomic orbitals into new hybrid orbitals which are suitable for pairing of electrons to form chemical bonds in valence bond theory . ▸ Hybrid orbitals are very useful in the explanation of molecular geometry. ▸ A trigonal planar geometry has s p 2 hybridization which has a bond angle of 120 o . ▸ A tetrahedral geometry has s p 3 hybridization which has a bond angle of 109 .5 o . ▸ When one s-orbital and one p-orbital combine, it forms two s p 3 hybrid orbitals. ▸ When one s-orbital and two p-orbital combine, it forms three s p 3 hybrid orbitals. ▸ When one s-orbital and three p-orbital combine, it forms four s p 3 hybrid orbitals.

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Chapter 2, Problem 18PP

Interpretation Introduction

Interpretation:

The reaction between trimethyl amine and HCl is to be shown and the expected hybridization state for the nitrogen atom in the product is to be predicted.

Concept Introduction:

▸ Lewis acids are electron pair acceptors.

▸ Lewis bases are electron pair donors.

▸ The valence shell electron pair repulsion (VSEPR) theory predicts the arrangement of atoms in molecules and ions.

▸ Amines are the organic compounds that contain an amino group (−NH2).

▸ They can act as nucleophiles and electrophiles in organic reactions.

▸ Amines can be classified into three categories: primary amines, secondary amines, and tertiary amines.

▸ If the nitrogen atom is directly attached to only one other carbon atom, the amine is a primary amine.

▸ If the nitrogen atom is directly attached to two other carbon atoms, the amine is a secondary amine.

▸ If the nitrogen atom is directly attached to three other carbon atoms, the amine is a tertiary amine.

▸ Higher the electron density around the nitrogen atom, more available is the electron pair to donate. Electron donors are Lewis bases.

▸ The reaction is Lewis acid- base reaction. The trimethyl amine donates a pair of electrons, so it acts as a Lewis base and HCl accepts a pair of electrons, and so acts as a Lewis acid.

▸ Hybridization is the concept of mixing atomic orbitals into new hybrid orbitals which are suitable for pairing of electrons to form chemical bonds in valence bond theory.

▸ Hybrid orbitals are very useful in the explanation of molecular geometry.

▸ A trigonal planar geometry has sp2 hybridization which has a bond angle of 120o.

▸ A tetrahedral geometry has sp3 hybridization which has a bond angle of 109.5o.

▸ When one s-orbital and one p-orbital combine, it forms two sp3 hybrid orbitals.

▸ When one s-orbital and two p-orbital combine, it forms three sp3 hybrid orbitals.

▸ When one s-orbital and three p-orbital combine, it forms four sp3 hybrid orbitals.

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