Structual characterisation Flashcards
heteroatoms
any element that is not carbon or hydrogen
eg nitrogen,oxygen, sulphur
empirical formula vs molecular formula
EF = simplest whole number ration of elements in the structure
MF = actual number
Double bond equivalence DBE
also called index of hydrogen deficiency IHD
H reference is the number of hydrogens required to make CnH2n+2 - saturated alkane
H molecule = number of hydrogens actually present
DBE = H ref - H mol /2
DBE = 1 = one double bond or ring
DBE = two double bonds or rings or one triple bond
molecules with heteroatoms
with oxygen - can be ignored as does not affect DBE so no change to H ref - so COH/COOH/COC
Subtract one H from H ref for every halogen present
Add one H to H ref for every nitrogen
mass spectrometry
this gives us the mass of molecules and can therefore distinguish between empirical and molecular formulas
- the mass and charge affects the acceleration as will have different path lengths so will produce different peaks
Base peak
largest peak to which the relative abundance of all other peaks are measured to
parent ion or molecular ion peak
the peak at which is produced by the original molecule before fragmentation
exact mass
measuring to 4 decimal places
- calculating the exact mass using the most common isotope. - this helps distinguish between compounds with similar RAM
electromagnetic radiation
is a wave consisting of orthogonal electrical magnetic fields that can travel through space
as energy decreases, frequency decreases but wavelength increases
defining waves
wavelength = lamdaba (metres)
frequency = v (s-1)
wavenumber -V (cm-1)
speed light = c = 2.998x108ms-1
c=vlamdaba
need to remember to convert these to m ->cm
wave particle duality
electromagnetic radiation can be a wave and small packet of energy
energy of photon is related to its frequency
converting to wave number for this allows us to put the information onto a better scale
wave particle duality equations
E = hv
h = 6.626x10-34Js = plancks constant
E=hc/lambada
E=hc-V
quantisation of energy levels
electronic, vibrational and rotational energy levels in molecules can be compared
- energy gap between electorns in valence orbitals is quite large
- energy gap between vibrational energy levels smaller
- energy gap between rotational energy levels smallest
decreasing energy gap between different states
UV/Visible spectroscopy
when photon in Uv or visible range is absorbed, an electron is promoted from a full bonding orbital to a empty anti bonding orbital
the electrons that do this are double bonded electrons, pi bonds - undergone a pi tranistion
energy gap between pi and sigma orbitals
energy gap of sigma orbitals are not in the UV/visible region of EM spectrum as the gap is too big to be associated with this region