Anvendt Spektroskopi Applied Spectroscopy KJM3000 Varingr 2015
Curriculum rdquoIntroduction to Spectroscopyrdquo byPavia Lampman Kriz
Practical information
Teacher
Tore Bonge-Hansen rom Oslash303 torehanskjemiuiono
Lectures and problems Avogadro WedFri 1215 og 1015
Communication e-mail og homepage
80 of the problemsets must be approvedpassed in order to take the exam No grade on the problemsets
Goal The student should be able to use spectroscopic methods to determine the constitution of organic molecules
Plan ca 25 hours of lectures and ca 40 hours problem solvingLess focus on theory more on solving problems Last problem Fri 155 Exam beginning of june 4h written exam letter grade
Four spectrocopic methods UVVIS IR NMR og MS These methods give complementary info and together they are a a very powerful tool for identification and structure elucidationof small amounts (mg) of unknown compounds
Progress plan KJM3000 - Spring 2015 week Wed Fri 4 Gen NMR1NMR25 NMR3NMR4 NMR5NMR66 NMR7NMR8 NMR9NMR107 NMR11NMR12 K18 K2 K39 K4 MS1MS210 MS3MS4 K511 K6 K712 K8 UV1UV213 K9 IR1IR214 Easter Easter15 IR3IR4 K1016 K11 K1217 K13 K1418 K15 K1619 K17 K1820 K19 K20 Last colloquium K20 Friday 15th of MayExam Beginning of June 4 hours written
General
Spectroscopy The study of interaction between electro-magnetic radiation and matter (molecules)
Electromagnetic radiation
Electromagnetic radiation can be described as
a wave motion
= wavelength = frequency c = speed og light
a particle motion
E = energy = frequency h = Planckrsquos constant
bull = c
E = h bull
Frequency and wavelength will be inversely proportional to each other since c = constant
If the frequency of the electromagnetic radiation is the same as a frequency within a molecule (vibration) the molecule can absorb energy The lsquolightrsquo and the moleculersquos motion are in resonans
reorganization
= c
A molecular motion can be the vibration of a chemical bond
H Cl
= 9 1013 s-1
This frequency and wavelength corresponds to electromagnetic radiation in the IR-area
Interaction between light and matter in a more general way
A molecule has many stationary energy levels (E) For every energi level there is a wave funvtion (Ψ)
E2 _____________ Ψ2
E1
_____________ Ψ1
ΔE = E1 ndash E2 = hν
If we shine light on a molecule with a frequency corresponding to ΔE the molecule can absorb energy and move to a higher energy level
Emission spectroscopy
The molecule moves from a higher energy level (E2) to a lower
energy level (E1) by emitting a quantum of light
Absorption spectroscopy
The amount of light absorbed as a function of wavelength A quantum of light is absorbed and the molecule moves from a lower energy level (E1) to a higher energy level (E2)
E2 _____________ Ψ2
E1
_____________ Ψ1
ΔE = E1 ndash E2 = hν
A general spectroscopic experiment
Light source Often poly chromaticUVVis Light bulbs (Hg Na)IR Heater (Nernst filament) gt 1000 deg CNMR radio transmitter
Detectors
UVVIS diode array (photon counter)
IR heat sensitive electronic componen (semi conductor)
NMR radio receiver
The detected energy is converted to voltage and transferred to a computer
A spectrum is recorded by measuring absorbance whilechanging the wavelength of light (scanning)
Four methods
UV 200 ndash 380 nm Used primarily to detect conjugated systems Excitation of electrons inconjugated systems give absorbance in this area
IR 4000 ndash 400 cm-1 Used to detect and identify vibrations related to different functional groups
NMR Atomic nuclei absorbing radiowaves when placed in a strong magnetic field
MS Measures masscharge ratios of organic ions
200 MHz NMR-instrument
1H-NMR spectrum
UV og IR instruments
UV og IR spectrum
MS-instrument in series with GC
MS-spectrum
Practical information
Teacher
Tore Bonge-Hansen rom Oslash303 torehanskjemiuiono
Lectures and problems Avogadro WedFri 1215 og 1015
Communication e-mail og homepage
80 of the problemsets must be approvedpassed in order to take the exam No grade on the problemsets
Goal The student should be able to use spectroscopic methods to determine the constitution of organic molecules
Plan ca 25 hours of lectures and ca 40 hours problem solvingLess focus on theory more on solving problems Last problem Fri 155 Exam beginning of june 4h written exam letter grade
Four spectrocopic methods UVVIS IR NMR og MS These methods give complementary info and together they are a a very powerful tool for identification and structure elucidationof small amounts (mg) of unknown compounds
Progress plan KJM3000 - Spring 2015 week Wed Fri 4 Gen NMR1NMR25 NMR3NMR4 NMR5NMR66 NMR7NMR8 NMR9NMR107 NMR11NMR12 K18 K2 K39 K4 MS1MS210 MS3MS4 K511 K6 K712 K8 UV1UV213 K9 IR1IR214 Easter Easter15 IR3IR4 K1016 K11 K1217 K13 K1418 K15 K1619 K17 K1820 K19 K20 Last colloquium K20 Friday 15th of MayExam Beginning of June 4 hours written
General
Spectroscopy The study of interaction between electro-magnetic radiation and matter (molecules)
Electromagnetic radiation
Electromagnetic radiation can be described as
a wave motion
= wavelength = frequency c = speed og light
a particle motion
E = energy = frequency h = Planckrsquos constant
bull = c
E = h bull
Frequency and wavelength will be inversely proportional to each other since c = constant
If the frequency of the electromagnetic radiation is the same as a frequency within a molecule (vibration) the molecule can absorb energy The lsquolightrsquo and the moleculersquos motion are in resonans
reorganization
= c
A molecular motion can be the vibration of a chemical bond
H Cl
= 9 1013 s-1
This frequency and wavelength corresponds to electromagnetic radiation in the IR-area
Interaction between light and matter in a more general way
A molecule has many stationary energy levels (E) For every energi level there is a wave funvtion (Ψ)
E2 _____________ Ψ2
E1
_____________ Ψ1
ΔE = E1 ndash E2 = hν
If we shine light on a molecule with a frequency corresponding to ΔE the molecule can absorb energy and move to a higher energy level
Emission spectroscopy
The molecule moves from a higher energy level (E2) to a lower
energy level (E1) by emitting a quantum of light
Absorption spectroscopy
The amount of light absorbed as a function of wavelength A quantum of light is absorbed and the molecule moves from a lower energy level (E1) to a higher energy level (E2)
E2 _____________ Ψ2
E1
_____________ Ψ1
ΔE = E1 ndash E2 = hν
A general spectroscopic experiment
Light source Often poly chromaticUVVis Light bulbs (Hg Na)IR Heater (Nernst filament) gt 1000 deg CNMR radio transmitter
Detectors
UVVIS diode array (photon counter)
IR heat sensitive electronic componen (semi conductor)
NMR radio receiver
The detected energy is converted to voltage and transferred to a computer
A spectrum is recorded by measuring absorbance whilechanging the wavelength of light (scanning)
Four methods
UV 200 ndash 380 nm Used primarily to detect conjugated systems Excitation of electrons inconjugated systems give absorbance in this area
IR 4000 ndash 400 cm-1 Used to detect and identify vibrations related to different functional groups
NMR Atomic nuclei absorbing radiowaves when placed in a strong magnetic field
MS Measures masscharge ratios of organic ions
200 MHz NMR-instrument
1H-NMR spectrum
UV og IR instruments
UV og IR spectrum
MS-instrument in series with GC
MS-spectrum
Goal The student should be able to use spectroscopic methods to determine the constitution of organic molecules
Plan ca 25 hours of lectures and ca 40 hours problem solvingLess focus on theory more on solving problems Last problem Fri 155 Exam beginning of june 4h written exam letter grade
Four spectrocopic methods UVVIS IR NMR og MS These methods give complementary info and together they are a a very powerful tool for identification and structure elucidationof small amounts (mg) of unknown compounds
Progress plan KJM3000 - Spring 2015 week Wed Fri 4 Gen NMR1NMR25 NMR3NMR4 NMR5NMR66 NMR7NMR8 NMR9NMR107 NMR11NMR12 K18 K2 K39 K4 MS1MS210 MS3MS4 K511 K6 K712 K8 UV1UV213 K9 IR1IR214 Easter Easter15 IR3IR4 K1016 K11 K1217 K13 K1418 K15 K1619 K17 K1820 K19 K20 Last colloquium K20 Friday 15th of MayExam Beginning of June 4 hours written
General
Spectroscopy The study of interaction between electro-magnetic radiation and matter (molecules)
Electromagnetic radiation
Electromagnetic radiation can be described as
a wave motion
= wavelength = frequency c = speed og light
a particle motion
E = energy = frequency h = Planckrsquos constant
bull = c
E = h bull
Frequency and wavelength will be inversely proportional to each other since c = constant
If the frequency of the electromagnetic radiation is the same as a frequency within a molecule (vibration) the molecule can absorb energy The lsquolightrsquo and the moleculersquos motion are in resonans
reorganization
= c
A molecular motion can be the vibration of a chemical bond
H Cl
= 9 1013 s-1
This frequency and wavelength corresponds to electromagnetic radiation in the IR-area
Interaction between light and matter in a more general way
A molecule has many stationary energy levels (E) For every energi level there is a wave funvtion (Ψ)
E2 _____________ Ψ2
E1
_____________ Ψ1
ΔE = E1 ndash E2 = hν
If we shine light on a molecule with a frequency corresponding to ΔE the molecule can absorb energy and move to a higher energy level
Emission spectroscopy
The molecule moves from a higher energy level (E2) to a lower
energy level (E1) by emitting a quantum of light
Absorption spectroscopy
The amount of light absorbed as a function of wavelength A quantum of light is absorbed and the molecule moves from a lower energy level (E1) to a higher energy level (E2)
E2 _____________ Ψ2
E1
_____________ Ψ1
ΔE = E1 ndash E2 = hν
A general spectroscopic experiment
Light source Often poly chromaticUVVis Light bulbs (Hg Na)IR Heater (Nernst filament) gt 1000 deg CNMR radio transmitter
Detectors
UVVIS diode array (photon counter)
IR heat sensitive electronic componen (semi conductor)
NMR radio receiver
The detected energy is converted to voltage and transferred to a computer
A spectrum is recorded by measuring absorbance whilechanging the wavelength of light (scanning)
Four methods
UV 200 ndash 380 nm Used primarily to detect conjugated systems Excitation of electrons inconjugated systems give absorbance in this area
IR 4000 ndash 400 cm-1 Used to detect and identify vibrations related to different functional groups
NMR Atomic nuclei absorbing radiowaves when placed in a strong magnetic field
MS Measures masscharge ratios of organic ions
200 MHz NMR-instrument
1H-NMR spectrum
UV og IR instruments
UV og IR spectrum
MS-instrument in series with GC
MS-spectrum
Progress plan KJM3000 - Spring 2015 week Wed Fri 4 Gen NMR1NMR25 NMR3NMR4 NMR5NMR66 NMR7NMR8 NMR9NMR107 NMR11NMR12 K18 K2 K39 K4 MS1MS210 MS3MS4 K511 K6 K712 K8 UV1UV213 K9 IR1IR214 Easter Easter15 IR3IR4 K1016 K11 K1217 K13 K1418 K15 K1619 K17 K1820 K19 K20 Last colloquium K20 Friday 15th of MayExam Beginning of June 4 hours written
General
Spectroscopy The study of interaction between electro-magnetic radiation and matter (molecules)
Electromagnetic radiation
Electromagnetic radiation can be described as
a wave motion
= wavelength = frequency c = speed og light
a particle motion
E = energy = frequency h = Planckrsquos constant
bull = c
E = h bull
Frequency and wavelength will be inversely proportional to each other since c = constant
If the frequency of the electromagnetic radiation is the same as a frequency within a molecule (vibration) the molecule can absorb energy The lsquolightrsquo and the moleculersquos motion are in resonans
reorganization
= c
A molecular motion can be the vibration of a chemical bond
H Cl
= 9 1013 s-1
This frequency and wavelength corresponds to electromagnetic radiation in the IR-area
Interaction between light and matter in a more general way
A molecule has many stationary energy levels (E) For every energi level there is a wave funvtion (Ψ)
E2 _____________ Ψ2
E1
_____________ Ψ1
ΔE = E1 ndash E2 = hν
If we shine light on a molecule with a frequency corresponding to ΔE the molecule can absorb energy and move to a higher energy level
Emission spectroscopy
The molecule moves from a higher energy level (E2) to a lower
energy level (E1) by emitting a quantum of light
Absorption spectroscopy
The amount of light absorbed as a function of wavelength A quantum of light is absorbed and the molecule moves from a lower energy level (E1) to a higher energy level (E2)
E2 _____________ Ψ2
E1
_____________ Ψ1
ΔE = E1 ndash E2 = hν
A general spectroscopic experiment
Light source Often poly chromaticUVVis Light bulbs (Hg Na)IR Heater (Nernst filament) gt 1000 deg CNMR radio transmitter
Detectors
UVVIS diode array (photon counter)
IR heat sensitive electronic componen (semi conductor)
NMR radio receiver
The detected energy is converted to voltage and transferred to a computer
A spectrum is recorded by measuring absorbance whilechanging the wavelength of light (scanning)
Four methods
UV 200 ndash 380 nm Used primarily to detect conjugated systems Excitation of electrons inconjugated systems give absorbance in this area
IR 4000 ndash 400 cm-1 Used to detect and identify vibrations related to different functional groups
NMR Atomic nuclei absorbing radiowaves when placed in a strong magnetic field
MS Measures masscharge ratios of organic ions
200 MHz NMR-instrument
1H-NMR spectrum
UV og IR instruments
UV og IR spectrum
MS-instrument in series with GC
MS-spectrum
General
Spectroscopy The study of interaction between electro-magnetic radiation and matter (molecules)
Electromagnetic radiation
Electromagnetic radiation can be described as
a wave motion
= wavelength = frequency c = speed og light
a particle motion
E = energy = frequency h = Planckrsquos constant
bull = c
E = h bull
Frequency and wavelength will be inversely proportional to each other since c = constant
If the frequency of the electromagnetic radiation is the same as a frequency within a molecule (vibration) the molecule can absorb energy The lsquolightrsquo and the moleculersquos motion are in resonans
reorganization
= c
A molecular motion can be the vibration of a chemical bond
H Cl
= 9 1013 s-1
This frequency and wavelength corresponds to electromagnetic radiation in the IR-area
Interaction between light and matter in a more general way
A molecule has many stationary energy levels (E) For every energi level there is a wave funvtion (Ψ)
E2 _____________ Ψ2
E1
_____________ Ψ1
ΔE = E1 ndash E2 = hν
If we shine light on a molecule with a frequency corresponding to ΔE the molecule can absorb energy and move to a higher energy level
Emission spectroscopy
The molecule moves from a higher energy level (E2) to a lower
energy level (E1) by emitting a quantum of light
Absorption spectroscopy
The amount of light absorbed as a function of wavelength A quantum of light is absorbed and the molecule moves from a lower energy level (E1) to a higher energy level (E2)
E2 _____________ Ψ2
E1
_____________ Ψ1
ΔE = E1 ndash E2 = hν
A general spectroscopic experiment
Light source Often poly chromaticUVVis Light bulbs (Hg Na)IR Heater (Nernst filament) gt 1000 deg CNMR radio transmitter
Detectors
UVVIS diode array (photon counter)
IR heat sensitive electronic componen (semi conductor)
NMR radio receiver
The detected energy is converted to voltage and transferred to a computer
A spectrum is recorded by measuring absorbance whilechanging the wavelength of light (scanning)
Four methods
UV 200 ndash 380 nm Used primarily to detect conjugated systems Excitation of electrons inconjugated systems give absorbance in this area
IR 4000 ndash 400 cm-1 Used to detect and identify vibrations related to different functional groups
NMR Atomic nuclei absorbing radiowaves when placed in a strong magnetic field
MS Measures masscharge ratios of organic ions
200 MHz NMR-instrument
1H-NMR spectrum
UV og IR instruments
UV og IR spectrum
MS-instrument in series with GC
MS-spectrum
Electromagnetic radiation
Electromagnetic radiation can be described as
a wave motion
= wavelength = frequency c = speed og light
a particle motion
E = energy = frequency h = Planckrsquos constant
bull = c
E = h bull
Frequency and wavelength will be inversely proportional to each other since c = constant
If the frequency of the electromagnetic radiation is the same as a frequency within a molecule (vibration) the molecule can absorb energy The lsquolightrsquo and the moleculersquos motion are in resonans
reorganization
= c
A molecular motion can be the vibration of a chemical bond
H Cl
= 9 1013 s-1
This frequency and wavelength corresponds to electromagnetic radiation in the IR-area
Interaction between light and matter in a more general way
A molecule has many stationary energy levels (E) For every energi level there is a wave funvtion (Ψ)
E2 _____________ Ψ2
E1
_____________ Ψ1
ΔE = E1 ndash E2 = hν
If we shine light on a molecule with a frequency corresponding to ΔE the molecule can absorb energy and move to a higher energy level
Emission spectroscopy
The molecule moves from a higher energy level (E2) to a lower
energy level (E1) by emitting a quantum of light
Absorption spectroscopy
The amount of light absorbed as a function of wavelength A quantum of light is absorbed and the molecule moves from a lower energy level (E1) to a higher energy level (E2)
E2 _____________ Ψ2
E1
_____________ Ψ1
ΔE = E1 ndash E2 = hν
A general spectroscopic experiment
Light source Often poly chromaticUVVis Light bulbs (Hg Na)IR Heater (Nernst filament) gt 1000 deg CNMR radio transmitter
Detectors
UVVIS diode array (photon counter)
IR heat sensitive electronic componen (semi conductor)
NMR radio receiver
The detected energy is converted to voltage and transferred to a computer
A spectrum is recorded by measuring absorbance whilechanging the wavelength of light (scanning)
Four methods
UV 200 ndash 380 nm Used primarily to detect conjugated systems Excitation of electrons inconjugated systems give absorbance in this area
IR 4000 ndash 400 cm-1 Used to detect and identify vibrations related to different functional groups
NMR Atomic nuclei absorbing radiowaves when placed in a strong magnetic field
MS Measures masscharge ratios of organic ions
200 MHz NMR-instrument
1H-NMR spectrum
UV og IR instruments
UV og IR spectrum
MS-instrument in series with GC
MS-spectrum
Frequency and wavelength will be inversely proportional to each other since c = constant
If the frequency of the electromagnetic radiation is the same as a frequency within a molecule (vibration) the molecule can absorb energy The lsquolightrsquo and the moleculersquos motion are in resonans
reorganization
= c
A molecular motion can be the vibration of a chemical bond
H Cl
= 9 1013 s-1
This frequency and wavelength corresponds to electromagnetic radiation in the IR-area
Interaction between light and matter in a more general way
A molecule has many stationary energy levels (E) For every energi level there is a wave funvtion (Ψ)
E2 _____________ Ψ2
E1
_____________ Ψ1
ΔE = E1 ndash E2 = hν
If we shine light on a molecule with a frequency corresponding to ΔE the molecule can absorb energy and move to a higher energy level
Emission spectroscopy
The molecule moves from a higher energy level (E2) to a lower
energy level (E1) by emitting a quantum of light
Absorption spectroscopy
The amount of light absorbed as a function of wavelength A quantum of light is absorbed and the molecule moves from a lower energy level (E1) to a higher energy level (E2)
E2 _____________ Ψ2
E1
_____________ Ψ1
ΔE = E1 ndash E2 = hν
A general spectroscopic experiment
Light source Often poly chromaticUVVis Light bulbs (Hg Na)IR Heater (Nernst filament) gt 1000 deg CNMR radio transmitter
Detectors
UVVIS diode array (photon counter)
IR heat sensitive electronic componen (semi conductor)
NMR radio receiver
The detected energy is converted to voltage and transferred to a computer
A spectrum is recorded by measuring absorbance whilechanging the wavelength of light (scanning)
Four methods
UV 200 ndash 380 nm Used primarily to detect conjugated systems Excitation of electrons inconjugated systems give absorbance in this area
IR 4000 ndash 400 cm-1 Used to detect and identify vibrations related to different functional groups
NMR Atomic nuclei absorbing radiowaves when placed in a strong magnetic field
MS Measures masscharge ratios of organic ions
200 MHz NMR-instrument
1H-NMR spectrum
UV og IR instruments
UV og IR spectrum
MS-instrument in series with GC
MS-spectrum
A molecular motion can be the vibration of a chemical bond
H Cl
= 9 1013 s-1
This frequency and wavelength corresponds to electromagnetic radiation in the IR-area
Interaction between light and matter in a more general way
A molecule has many stationary energy levels (E) For every energi level there is a wave funvtion (Ψ)
E2 _____________ Ψ2
E1
_____________ Ψ1
ΔE = E1 ndash E2 = hν
If we shine light on a molecule with a frequency corresponding to ΔE the molecule can absorb energy and move to a higher energy level
Emission spectroscopy
The molecule moves from a higher energy level (E2) to a lower
energy level (E1) by emitting a quantum of light
Absorption spectroscopy
The amount of light absorbed as a function of wavelength A quantum of light is absorbed and the molecule moves from a lower energy level (E1) to a higher energy level (E2)
E2 _____________ Ψ2
E1
_____________ Ψ1
ΔE = E1 ndash E2 = hν
A general spectroscopic experiment
Light source Often poly chromaticUVVis Light bulbs (Hg Na)IR Heater (Nernst filament) gt 1000 deg CNMR radio transmitter
Detectors
UVVIS diode array (photon counter)
IR heat sensitive electronic componen (semi conductor)
NMR radio receiver
The detected energy is converted to voltage and transferred to a computer
A spectrum is recorded by measuring absorbance whilechanging the wavelength of light (scanning)
Four methods
UV 200 ndash 380 nm Used primarily to detect conjugated systems Excitation of electrons inconjugated systems give absorbance in this area
IR 4000 ndash 400 cm-1 Used to detect and identify vibrations related to different functional groups
NMR Atomic nuclei absorbing radiowaves when placed in a strong magnetic field
MS Measures masscharge ratios of organic ions
200 MHz NMR-instrument
1H-NMR spectrum
UV og IR instruments
UV og IR spectrum
MS-instrument in series with GC
MS-spectrum
Interaction between light and matter in a more general way
A molecule has many stationary energy levels (E) For every energi level there is a wave funvtion (Ψ)
E2 _____________ Ψ2
E1
_____________ Ψ1
ΔE = E1 ndash E2 = hν
If we shine light on a molecule with a frequency corresponding to ΔE the molecule can absorb energy and move to a higher energy level
Emission spectroscopy
The molecule moves from a higher energy level (E2) to a lower
energy level (E1) by emitting a quantum of light
Absorption spectroscopy
The amount of light absorbed as a function of wavelength A quantum of light is absorbed and the molecule moves from a lower energy level (E1) to a higher energy level (E2)
E2 _____________ Ψ2
E1
_____________ Ψ1
ΔE = E1 ndash E2 = hν
A general spectroscopic experiment
Light source Often poly chromaticUVVis Light bulbs (Hg Na)IR Heater (Nernst filament) gt 1000 deg CNMR radio transmitter
Detectors
UVVIS diode array (photon counter)
IR heat sensitive electronic componen (semi conductor)
NMR radio receiver
The detected energy is converted to voltage and transferred to a computer
A spectrum is recorded by measuring absorbance whilechanging the wavelength of light (scanning)
Four methods
UV 200 ndash 380 nm Used primarily to detect conjugated systems Excitation of electrons inconjugated systems give absorbance in this area
IR 4000 ndash 400 cm-1 Used to detect and identify vibrations related to different functional groups
NMR Atomic nuclei absorbing radiowaves when placed in a strong magnetic field
MS Measures masscharge ratios of organic ions
200 MHz NMR-instrument
1H-NMR spectrum
UV og IR instruments
UV og IR spectrum
MS-instrument in series with GC
MS-spectrum
Emission spectroscopy
The molecule moves from a higher energy level (E2) to a lower
energy level (E1) by emitting a quantum of light
Absorption spectroscopy
The amount of light absorbed as a function of wavelength A quantum of light is absorbed and the molecule moves from a lower energy level (E1) to a higher energy level (E2)
E2 _____________ Ψ2
E1
_____________ Ψ1
ΔE = E1 ndash E2 = hν
A general spectroscopic experiment
Light source Often poly chromaticUVVis Light bulbs (Hg Na)IR Heater (Nernst filament) gt 1000 deg CNMR radio transmitter
Detectors
UVVIS diode array (photon counter)
IR heat sensitive electronic componen (semi conductor)
NMR radio receiver
The detected energy is converted to voltage and transferred to a computer
A spectrum is recorded by measuring absorbance whilechanging the wavelength of light (scanning)
Four methods
UV 200 ndash 380 nm Used primarily to detect conjugated systems Excitation of electrons inconjugated systems give absorbance in this area
IR 4000 ndash 400 cm-1 Used to detect and identify vibrations related to different functional groups
NMR Atomic nuclei absorbing radiowaves when placed in a strong magnetic field
MS Measures masscharge ratios of organic ions
200 MHz NMR-instrument
1H-NMR spectrum
UV og IR instruments
UV og IR spectrum
MS-instrument in series with GC
MS-spectrum
A general spectroscopic experiment
Light source Often poly chromaticUVVis Light bulbs (Hg Na)IR Heater (Nernst filament) gt 1000 deg CNMR radio transmitter
Detectors
UVVIS diode array (photon counter)
IR heat sensitive electronic componen (semi conductor)
NMR radio receiver
The detected energy is converted to voltage and transferred to a computer
A spectrum is recorded by measuring absorbance whilechanging the wavelength of light (scanning)
Four methods
UV 200 ndash 380 nm Used primarily to detect conjugated systems Excitation of electrons inconjugated systems give absorbance in this area
IR 4000 ndash 400 cm-1 Used to detect and identify vibrations related to different functional groups
NMR Atomic nuclei absorbing radiowaves when placed in a strong magnetic field
MS Measures masscharge ratios of organic ions
200 MHz NMR-instrument
1H-NMR spectrum
UV og IR instruments
UV og IR spectrum
MS-instrument in series with GC
MS-spectrum
Detectors
UVVIS diode array (photon counter)
IR heat sensitive electronic componen (semi conductor)
NMR radio receiver
The detected energy is converted to voltage and transferred to a computer
A spectrum is recorded by measuring absorbance whilechanging the wavelength of light (scanning)
Four methods
UV 200 ndash 380 nm Used primarily to detect conjugated systems Excitation of electrons inconjugated systems give absorbance in this area
IR 4000 ndash 400 cm-1 Used to detect and identify vibrations related to different functional groups
NMR Atomic nuclei absorbing radiowaves when placed in a strong magnetic field
MS Measures masscharge ratios of organic ions
200 MHz NMR-instrument
1H-NMR spectrum
UV og IR instruments
UV og IR spectrum
MS-instrument in series with GC
MS-spectrum
Four methods
UV 200 ndash 380 nm Used primarily to detect conjugated systems Excitation of electrons inconjugated systems give absorbance in this area
IR 4000 ndash 400 cm-1 Used to detect and identify vibrations related to different functional groups
NMR Atomic nuclei absorbing radiowaves when placed in a strong magnetic field
MS Measures masscharge ratios of organic ions
200 MHz NMR-instrument
1H-NMR spectrum
UV og IR instruments
UV og IR spectrum
MS-instrument in series with GC
MS-spectrum
200 MHz NMR-instrument
1H-NMR spectrum
UV og IR instruments
UV og IR spectrum
MS-instrument in series with GC
MS-spectrum
1H-NMR spectrum
UV og IR instruments
UV og IR spectrum
MS-instrument in series with GC
MS-spectrum
UV og IR instruments
UV og IR spectrum
MS-instrument in series with GC
MS-spectrum
UV og IR spectrum
MS-instrument in series with GC
MS-spectrum
MS-instrument in series with GC
MS-spectrum
MS-spectrum