Hybridisation (Cambridge (CIE) AS Chemistry)

Orbitals & Hybridisation in Covalent Bonding

Bond overlap in covalent bonds

• A single covalent bond is formed when two nonmetals combine

• Each atom that combines has an atomic orbital containing a single unpaired electron

• When a covalent bond is formed, the atomic orbitals overlap to form a combined orbital containing two electrons

  • This new orbital is called the molecular orbital

• The greater the atomic orbital overlap, the stronger the bond

• Sigma (σ) bonds are formed by direct overlap of orbitals between the bonding atoms

• Pi (π) bonds are formed by the sideways overlap of adjacent above and below the σ bond

σ bonds

• Sigma (σ) bonds are formed from the end-on overlap of atomic orbitals

• S orbitals overlap this way as well as p orbitals

Forming sigma bonds

Sigma orbitals can be formed from the end-on overlap of s orbitals

• The electron density in a σ bond is symmetrical about a line joining the nuclei of the atoms forming the bond

• The pair of electrons is found between the nuclei of the two atoms

• There is an electrostatic force of attraction between the electrons and nuclei which bonds the atoms to each other

π bonds

• Pi (π) bonds are formed from the sideways overlap of adjacent p orbitals

• The two lobes that make up the π bond lie above and below the plane of the σ bond

• This maximises the overlap of the p orbitals

• A single π bond is drawn as two electron clouds one arising from each lobe of the p orbitals

• The two clouds of electrons in a π bond represent one bond containing two electrons

Forming pi bonds

π orbitals can be formed from the end-on overlap of p orbitals

Examples of sigma & pi bonds

• Hydrogen

  • The hydrogen atom has only one s orbital

  • The s orbitals of the two hydrogen atoms will overlap to form a σ bond

 Sigma bonding in hydrogen

Direct overlap of the 1s orbitals of the hydrogen atoms results in the formation of a σ bond

• Ethene

  • Each carbon atom uses three of its four electrons to form σ bonds

  • Two σ bonds are formed with the hydrogen atoms

  • One σ bond is formed with the other carbon atom

  • The fourth electron from each carbon atom occupies a p orbital which overlaps sideways with another p orbital on the other carbon atom to form a π bond

  • This means that the C-C is a double bond: one σ and one π bond

 Pi bonding in ethene

Overlap of the p orbitals results in the forming of a π bond in ethene

Sigma and pi bonding in ethene

Each carbon atom in ethene forms two sigma bonds with hydrogen atoms and one σ bond with another carbon atom. The fourth electron is used to form a π bond between the two carbon atoms

• Ethyne

  • This molecule contains a triple bond formed from two π bonds (at right angles to each other) and one σ bond

  • Each carbon atom uses two of its four electrons to form σ bonds

  • One σ bond is formed with the hydrogen atom

  • One σ bond is formed with the other carbon atom

  • Two electrons are used to form two π bonds with the other carbon atom

 Sigma and pi bonding in ethyne

Ethyne has a triple bond formed from two π bonds and one σ bond between the two carbon atoms

• Hydrogen cyanide

  • Hydrogen cyanide contains a triple bond

  • One σ bond is formed between the H and C atom (overlap of an sp C hybridised orbital with the 1s H orbital)

  • A second σ bond is formed between the C and N atom (overlap of an sp C hybridised orbital with an sp orbital of N)

  • The remaining two sets of p orbitals of nitrogen and carbon will overlap to form two π bonds at right angles to each other

Sigma and pi bonding in hydrogen cyanide

Hydrogen cyanide has a triple bond formed from the overlap of two sets of p orbitals of nitrogen and carbon and the overlap of an sp hybridised carbon orbital and a p orbital on the nitrogen

• Nitrogen

  • Nitrogen too contains a triple bond

  • The triple bond is formed from the overlap of the sp orbitals on each N to form a σ bond and the overlap of two sets of p orbitals on the nitrogen atoms to form two π bonds

  • These π bonds are at right angles to each other

   

Sigma and pi bonding in nitrogen molecules

The triple bond is formed from two π bonds and one σ bond

Hybridisation

• The p atomic orbitals can also overlap end-on to form σ bonds

• In order for them to do this, they first need to become modified in order to gain s orbital character

• The orbitals are therefore slightly changed in shape to make one of the p orbital lobes bigger

• This mixing of atomic orbitals to form covalent bonds is called hybridisation

  • Mixing one s orbital with three p orbitals is called sp³ hybridisation (each orbital has ¼ s character and ¾ p character)

  • Mixing one s orbital with two p orbitals is called sp² hybridisation

  • Mixing one s orbital with one p orbital forms sp hybridised orbitals

 sp hybridisation

π orbitals can be formed from the end-on overlap of p orbitals

sp hybrid orbitals

The mixing of s orbitals with p orbitals to form molecular bonds is called hybridisation