C3 Flashcards
Principle quantum number
First shell = n1 second shell =n2
Same as row number in the periodic table
N
Tells us the main energy level and is always positive
The angular momentum quantum number (L)
Indicates the shape of the orbital
Can be negative
When’s=0 then it’s an S orbital which is a sphere
When L=1 that’s a p orbital
Magnetic quantum number (M)
Tells us the orientation of that orbital
When L=0 ml=o which is a sphere
When L= 1 ml= -1,0,+1 which means I’ve got 3 possible dumbbell shapes px,py, pz
Spin quantum number
Ms = +1/2 up
Ms= -1/2 down
Hund’s rule
In a half filled Subshell it is energetically more favourable to have electrons of parallel spins
ABmEn
Central atom A
Bonded pairs B
Electron pairs E
Tetrahedral
AB4
Trigonal pyramidal
AB3E
Bent
AB2E2
Order Of repulsion
Electron pair electron pair repel the most
Then electron pair bonded pair
Bonded pair bonded pair repel the least
What form of bonds does the hybridised orbitals form
Sigma bond
Which bond is stronger sigma bond or pi bond
Sigma bond is stronger
Hybridisation of carbon
4 2sp3 hybrid orbitals derived from combining the energies of one 2s orbital and 3 2p orbitals
The VSEPR
The placement of carbons 4 valence electrons since all 4 2sp3 orbitals are equivalent, each 2sp3 orbital repels the others with equal force resulting in identical bond angle
