ppt14 b - ucsbdevries/chem1c/handouts/ppt14 b.pdf · title: microsoft powerpoint - ppt14 b...
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Covalent Bonding:
b
Covalent Bonding: Orbitals
Figure 13.1: (a) The interaction of two hydrogen atoms (b) Energy profile as a function of the distance
between the nuclei of the hydrogen atoms.
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Figure 13.1: (a) The interaction of two hydrogen atoms (b) Energy profile as a function of the distance
between the nuclei of the hydrogen atoms.
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Figure 14.25: The combination of hydrogen 1s atomic orbitals to form MOs
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- (- sign flips phase of the sound wave function)
- = 0
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Auto mufflers use destructive interferenceof sound waves to reduce engine noises.
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Bose is $200. Want todo it yourself?See Web site.
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An analogy between light waves and atomic wave functions.
NOTE: +/- signs show PHASES of waves, NOTCHARGES!
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Amplitudes of wave functions added
Amplitudes of wave functions subtracted.
Figure 14.26: (a) The MO energy-level diagram for the H2 molecule (b) The shapes of the Mos are obtained
by squaring the wave functions for MO1 and MO2.
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Figure 14.27: Bonding and anitbonding MOs
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Figure 14.28: MO energy-level diagram for the H2 molecule
# ANTIBONDING e’s = 0
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# BONDING e’s = 2
# ANTIBONDING e s = 0
Bond order = ½(2-0) = 1
Figure 14.29: The MO energy-level diagram for the He2 molecule
# ANTIBONDING e’s = 2
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# BONDING e’s = 2
Bond order = ½(2-2) = 0
Figure 14.29: The MO energy-level diagram for the He2 molecule
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Figure 14.30: The MO energy-level diagram for the He2
+ ion.
# ANTIBONDING e’s = 1
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# BONDING e’s = 2
Bond order = ½(2-1) = ½
Figure 14.31: The MO energy-level diagram for the H2
+ ion
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Figure 14.32: The MO energy-level diagram for the H2
- ion
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Figure 14.33: The relative sizes of the lithium 1s and 2s atomic orbitals
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Figure 14.34: The MO energy-level diagram for the Li2 molecule
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Figure 14.35: The three mutually perpendicular 2p orbitals on tow adjacent boron atoms.
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Figure 14.37: The expected MO energy-level diagram for the combustion of the 2P orbitals
on two boron atoms.
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Figure 14.36: The two p oribitals on the boron atom that overlap head-on combine to form
bonding and antibonding orbitals.
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Figure 14.36: The two p oribitals on the boron atom that overlap head-on combine to form
bonding and antibonding orbitals.
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Figure 14.37: The expected MO energy-level diagram for the combustion of the 2P orbitals
on two boron atoms.
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Figure 14.37: The expected MO energy-level diagram for the combustion of the 2P orbitals
on two boron atoms.
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Figure 14.37: The expected MO energy-level diagram for the combustion of the 2P orbitals
on two boron atoms.
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Figure 14.38: The expected MO energy-level diagram for the B2 molecule
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Figure 14.39: An apparatus used to measure the paramagnetism of a sample
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Figure 14.40: The correct MO energy-level diagram for the B2 molecule.
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Figure 14.41: The MO energy-level diagrams, bond orders, bond energies, and bond lengths for the
diatomic molecules, B2 through F2.
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Figure 14.42: When liquid oxygen is poured into the space between the poles of a strong magnet, it remains
there until it boils away.
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Source: Donald Clegg
Figure 14.43: The MO energy-level diagram for the NO molecule
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Figure 14.44: The MO energy-level diagram for both the NO+ and CN- ions
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Figure 14.45: A partial MO energy-level diagram for the HF molecule
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Figure 14.46: The electron probability distribution in the bonding MO of the HF molecule
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Spectroscopy
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Electromagnetic spectrum
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(wavelength) x (frequency) = speed [m/s]E = h ν
EnergyPer photon:
λν = c [108 m/s]
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Electromagnetic spectrum
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λν
WHAT MAKES A MOLECULE ABSORB LIGHT?
When should you push?
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AT THE RESONANTFREQUENCY
λν=cAT THE RESONANTFREQUENCY
14* Electronic transitions: ~ 6 x 10 sec.
500 nm (UV-VIS)
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Figure 14.55: The molecular orbital diagram for the ground state of NO+
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λν=cAT THE RESONANTFREQUENCY
14* Electronic transitions: ~ 6 x 10 sec.
500 nm (UV-VIS)
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13* Nuclear vibration: ~ 3 x 10 sec.
10,000 nm (
* molecular rotation:
mi
IR)
crowaves
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What makes a molecule absorb light?
[cm-1] = 1/λ = ν/c =E/hc
Figure 14.60: The three fundamental vibrations for sulfur dioxide
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What makes a molecule absorb light?
3200 cm−1 broad, strong O-H stretch (alcohols)3000 cm−1 broad, medium O-H stretch (carboxylic acids)1200 cm−1 strong, O-H bending2800 cm−1 strong, C-H stretch 1400 cm−1 variable C H bending1400 cm 1 variable, C-H bending1700 cm−1 strong, C=O stretch 1200 cm−1 strong, C-O stretch
What makes a molecule absorb light? Figure 14.61: The infrared spectrum of CH2Cl2.
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What makes a molecule absorb light? Figure 14.52: Schematic representation of two electronic energy levels in a molecule
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Figure 14.53: The various types of transitions are shown by vertical arrows.
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Figure 14.54: Spectrum corresponding to the changes indicated in Fig. 14.53.
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The molecular structure of beta-carotene
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Figure 14.57: The electronic absorption spectrum of beta-carotene.
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VIBRATIONS VIBRATIONS
Figure 14.58: The potential curve for a diatomic molecule
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Figure 14.59: Morse energy curve for a diatomic molecule.
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Figure 14.62: Representations of the two spin states of the proton interacting
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Figure 14.63: The molecular structure of bromoethane
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Figure 14.64: The expected NMR spectrum for bromoethane
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Figure 14.65: The spin of proton Hy
can by "up" or "down"
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Figure 14.66: The spins for protons Hy
can be "up", can be opposed (in 2
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ways) or can both be "down"
Figure 14.67: The spins for the protons Hy can by arranged as shown in (a) leading to four different
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magnetic environments
Figure 14.68: The NMR spectrum of CH3CH2Br (bromoethane) with TMS reference
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Figure 14.69: The molecule (2-butanone)
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Figure 14.70: A technician speaks to a patient before heis moved intot eh cavity of a magnetic
resonance imaging (MRI) machine.
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Figure 14.71: A colored Magnetic Resonance Imaging (MRI) scan through a human head,
showing a healthy brain in side view.
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