A to m ic H S p ectru m H e ise n b e rg U n certain ty E le c tro n C onfiguration E le c tro n A ffinity Io n iza tio n Energy E lectro n eg ativity Size A p plications Q u a n tu m N um bers E n e rg y L e ve ls Q u a n tu m M echanics Q u an tizatio n B o h r M odel W a ve /P a rtic le Concept Atomic Structure
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Atomic Structure. Wave-Particle Duality All waves have a characteristic wavelength,, and amplitude, A. Frequency,, of a wave is the number of cycles.
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Atom ic H Spectrum
Heisenberg Uncertainty
Electron ConfigurationElectron AffinityIonization EnergyElectronegativityS ize
Applications
Quantum Num bers Energy Levels
Quantum M echanics
Quantization Bohr M odel
W ave/Partic le Concept
Atomic StructureAtomic Structure
Wave-Particle DualityWave-Particle Duality
• All waves have a characteristic wavelength, , and amplitude, A.• Frequency, , of a wave is the number of cycles which pass a
point in one second.• Speed of a wave, c, is given by its frequency multiplied by its
wavelength:
• For light, speed = c = 3.00x108 m s-1 . • The speed of light is constant! • Higher Quality video (2:30 into video).
Orbitals and Quantum Numbers• Schrödinger’s equation requires 3 quantum numbers:
1. Principal Quantum Number, n. This is the same as Bohr’s n. As n becomes larger, the atom becomes larger and the electron is further from the nucleus. ( n = 1 , 2 , 3 , 4 , …. )
2. Angular Momentum Quantum Number, . This quantum number depends on the value of n. The values of begin at 0 and increase to (n - 1). We usually use letters for (s, p, d and f for = 0, 1, 2, and 3). Usually we refer to the s, p, d and f-orbitals.
3. Magnetic Quantum Number, m. This quantum number depends on . The magnetic quantum number has integral values between - and + . Magnetic quantum numbers give the 3D orientation of each orbital.
Quantum Mechanics and Atomic OrbitalsQuantum Mechanics and Atomic Orbitals
Quantum Numbers of WavefuntionsQuantum Numbers of Wavefuntions
Quantum # Symbol Values Description
Principal n 1,2,3,4,… Size & Energy of orbital
Angular Momentum
0,1,2,…(n-1)
for each n
Shape of orbital
Magnetic m…,0,…+ for each
Relative orientation of orbitals within same
Spin ms +1/2 or –1/2 Spin up or Spin down
Angular Momentum Quantum # () Name of Orbital
0 s (sharp)
1 p (principal)
2 d (diffuse)
3 f (fundamental)
4 g
Quantum Mechanics and Atomic OrbitalsQuantum Mechanics and Atomic OrbitalsQuantum Mechanics and Atomic OrbitalsQuantum Mechanics and Atomic Orbitals
n ℓ Orbital Name mℓ (“sub-orbitals) Comment
Orbitals and Quantum Numbers
Quantum Mechanics and Atomic OrbitalsQuantum Mechanics and Atomic Orbitals
The s-Orbitals
Representations of OrbitalsRepresentations of Orbitals
The p-Orbitals
Representations of OrbitalsRepresentations of Orbitals
d-orbitals
Many-Electron Atoms Many-Electron Atoms
Orbitals and Their Energies
Orbitals CD
Electron Spin and the Pauli Exclusion Principle
Many-Electron Atoms Many-Electron Atoms
Electron Spin and the Pauli Exclusion Principle
• Since electron spin is quantized, we define ms = spin quantum number = ½.
• Pauli’s Exclusions Principle:: no two electrons can have the same set of 4 quantum numbers.• Therefore, two electrons in the same orbital must have
opposite spins.
Many-Electron Atoms Many-Electron Atoms
Figure 6.27
Figure 6.27 Orbitals CD
Figure 6.28 Orbitals CD
Many-Electron Atoms Many-Electron Atoms
Orbitals and Their Energies
Orbitals CD
Electron Configurations – I Electron Configurations – I Species Electron Configuration Box Orbital Comment
Electron Configurations - II Electron Configurations - IISpecies Electron Configuration Box Orbital Comment
Metals, Nonmetals, and MetalloidsMetals, Nonmetals, and Metalloids
Metals
Figure 7.14
Two Major Factors:
•principal quantum number, n, and
•the effective nuclear charge, Zeff.
Periodic Trends Periodic Trends
Figure 7.5: Radius video Clip
Figure 7.6
Figure 7.10 IE clip
Figure 7.9
Electron AffinitiesElectron Affinities
• Electron affinity is the opposite of ionization energy.• Electron affinity: the energy change when a gaseous atom
gains an electron to form a gaseous ion:
Cl(g) + e- Cl-(g)• Electron affinity can either be exothermic (as the above
example) or endothermic:
Ar(g) + e- Ar-(g)
Figure 7.11: Electron AffinitiesFigure 7.11: Electron Affinities
Group Trends for the Active MetalsGroup Trends for the Active Metals
Group 1A: The Alkali Metals
Group Trends for the Active MetalsGroup Trends for the Active Metals
Group 2A: The Alkaline Earth Metals
Group Trends for Selected NonmetalsGroup Trends for Selected Nonmetals
Group 6A: The Oxygen Group
Group Trends for Selected NonmetalsGroup Trends for Selected Nonmetals
Group 7A: The Halogens
Group Trends for the Active MetalsGroup Trends for the Active Metals
Group 1A: The Alkali Metals• Alkali metals are all soft.• Chemistry dominated by the loss of their single s
electron:M M+ + e-
• Reactivity increases as we move down the group.• Alkali metals react with water to form MOH and
hydrogen gas:2M(s) + 2H2O(l) 2MOH(aq) + H2(g)
Group Trends for the Active MetalsGroup Trends for the Active Metals
Group 2A: The Alkaline Earth Metals• Alkaline earth metals are harder and more dense than the alkali
metals.
• The chemistry is dominated by the loss of two s electrons:M M2+ + 2e-.
Mg(s) + Cl2(g) MgCl2(s)2Mg(s) + O2(g) 2MgO(s)
• Be does not react with water. Mg will only react with steam. Ca onwards:
Ca(s) + 2H2O(l) Ca(OH)2(aq) + H2(g)
Atom ic H Spectrum
Heisenberg Uncertainty
Electron ConfigurationElectron AffinityIonization EnergyElectronegativityS ize