133A inorganic - covalent bonding Flashcards
What would the result of this anti bonding be
Which one has highest and lowest electron density
Why are there no circles around the hydrogens?
their e- density is very hard to see as there is just one e- orbiting around the H nucleus/ 2e- shared between C-H
Why do all C-H bonds have the same enthalpy even though we would predict them to be different
hybridisation- makes 4 sp3 orbitals when the s of the hydrogens and p of the carbons overlap
What does an sp3 hybridised orbital look like
What does CH4 look like with the 4 sp3 hybridised orbitals (tetrahedral)
What does the CH3+ cation look like the 3 sp3 hybridised orbitals (trigonal planar)
Any carbon that is sp2 hybridised will aim for what bond angle
120°
need all the MO diagrams from my notes ‘atoms and molecules in bonding’/ got up to lecture notes 11
What are equations for the first second and third ionisation energies
What are the only electrons used for bonding
valenece electrons. In the case of CH4, the ‘core electrons’ (2s) are promoted to valence status
Why would the top bond be favoured
pi bonds are weaker than sigma bonds, which have better overlap
What would each of these look like once interacting to form a π bond
A shorter bond is stronger/weaker
stronger
What would these sp hybridised orbitals look like
What would two sp hybridised orbitals together look like
tetrahedral molecules have what hybridisation
sp3
trigonal planar molecules have what hybridisation
sp2
What do the bonds in a C2H4 molecule look like; what hybridisation does it have
-hybridised orbitals make σ bonds
-unhybridised orbitals make π bonds
Linear molecules have what hybridisation
sp
BeH2 is linear so it is sp hybridised. Show how the Be electrons become hybridised and then bond with the H orbitals
nitrogen in N2 looks like this. Show how an N2 molecule has a triple bond
Phosphorus can form PF5, so can make 5 bonds. Show how its electrons are excited to make 5 bonds with F of equal strength
sp3d (1 s , 3 p orbitals and 1 d)
What hybridisation/combination of orbitals would give octahedral geometry (6 bonds)
s+p+p+p+d+d= 6 orbitals of equal strength