electronic structure. all waves have a characteristic wavelength,, and amplitude, a. frequency,, of...
TRANSCRIPT
![Page 1: Electronic Structure. All waves have a characteristic wavelength,, and amplitude, A. Frequency,, of a wave is the number of cycles which pass a point](https://reader035.vdocument.in/reader035/viewer/2022081519/56649e705503460f94b6d752/html5/thumbnails/1.jpg)
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
Electronic StructureElectronic Structure
![Page 2: Electronic Structure. All waves have a characteristic wavelength,, and amplitude, A. Frequency,, of a wave is the number of cycles which pass a point](https://reader035.vdocument.in/reader035/viewer/2022081519/56649e705503460f94b6d752/html5/thumbnails/2.jpg)
• 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!! (As of today!!)
The Wave Nature of LightThe Wave Nature of Light
c
![Page 3: Electronic Structure. All waves have a characteristic wavelength,, and amplitude, A. Frequency,, of a wave is the number of cycles which pass a point](https://reader035.vdocument.in/reader035/viewer/2022081519/56649e705503460f94b6d752/html5/thumbnails/3.jpg)
The Wave Nature of LightThe Wave Nature of Light
![Page 4: Electronic Structure. All waves have a characteristic wavelength,, and amplitude, A. Frequency,, of a wave is the number of cycles which pass a point](https://reader035.vdocument.in/reader035/viewer/2022081519/56649e705503460f94b6d752/html5/thumbnails/4.jpg)
The Wave Nature of LightThe Wave Nature of Light
![Page 5: Electronic Structure. All waves have a characteristic wavelength,, and amplitude, A. Frequency,, of a wave is the number of cycles which pass a point](https://reader035.vdocument.in/reader035/viewer/2022081519/56649e705503460f94b6d752/html5/thumbnails/5.jpg)
The Wave Nature of LightThe Wave Nature of Light
![Page 6: Electronic Structure. All waves have a characteristic wavelength,, and amplitude, A. Frequency,, of a wave is the number of cycles which pass a point](https://reader035.vdocument.in/reader035/viewer/2022081519/56649e705503460f94b6d752/html5/thumbnails/6.jpg)
• Planck: energy can only be absorbed or released from atoms in certain amounts called quanta.
• The relationship between energy and frequency is
where h is Planck’s constant ( 6.626 10-34 J s ) .
Quantized Energy and PhotonsQuantized Energy and Photons
hE
![Page 7: Electronic Structure. All waves have a characteristic wavelength,, and amplitude, A. Frequency,, of a wave is the number of cycles which pass a point](https://reader035.vdocument.in/reader035/viewer/2022081519/56649e705503460f94b6d752/html5/thumbnails/7.jpg)
The Photoelectric Effect and Photons
When light of a sufficiently high energy strikes a metal surface, electrons are knocked off its surface.
• Einstein assumed that light traveled in energy packets called photons.
• The energy of one photon is:
Quantized Energy and PhotonsQuantized Energy and Photons
hE
![Page 8: Electronic Structure. All waves have a characteristic wavelength,, and amplitude, A. Frequency,, of a wave is the number of cycles which pass a point](https://reader035.vdocument.in/reader035/viewer/2022081519/56649e705503460f94b6d752/html5/thumbnails/8.jpg)
Observations:
1. Electrons are ejected only if the light is of sufficiently high energy. This wavelegth limit is different for different metals.
2. The number of electrons emitted per second (current) increases as the intensity of the light increases.
![Page 9: Electronic Structure. All waves have a characteristic wavelength,, and amplitude, A. Frequency,, of a wave is the number of cycles which pass a point](https://reader035.vdocument.in/reader035/viewer/2022081519/56649e705503460f94b6d752/html5/thumbnails/9.jpg)
Nature of Waves: Quantized Energy and PhotonsNature of Waves: Quantized Energy and Photons
X – rays Microwaves Comment(s)
Wavelength: λ (m) 1.00x10-10 m 1.00x10-2 m
Frequency: ν (s-1)
Energy: E (J)
3 x 10103 x 1018
Microwaves arelonger
X-rays = high v
![Page 10: Electronic Structure. All waves have a characteristic wavelength,, and amplitude, A. Frequency,, of a wave is the number of cycles which pass a point](https://reader035.vdocument.in/reader035/viewer/2022081519/56649e705503460f94b6d752/html5/thumbnails/10.jpg)
Line Spectra• Radiation composed of only one wavelength is called
monochromatic.• Radiation that spans a whole array of different
wavelengths is called continuous.• White light can be separated into a continuous spectrum
of colors.• Note that there are no dark spots on the continuous
spectrum that would correspond to different lines.
Line Spectra and the Bohr ModelLine Spectra and the Bohr Model
![Page 11: Electronic Structure. All waves have a characteristic wavelength,, and amplitude, A. Frequency,, of a wave is the number of cycles which pass a point](https://reader035.vdocument.in/reader035/viewer/2022081519/56649e705503460f94b6d752/html5/thumbnails/11.jpg)
![Page 12: Electronic Structure. All waves have a characteristic wavelength,, and amplitude, A. Frequency,, of a wave is the number of cycles which pass a point](https://reader035.vdocument.in/reader035/viewer/2022081519/56649e705503460f94b6d752/html5/thumbnails/12.jpg)
Bohr Model• Colors from excited gases arise because electrons move between energy states
in the atom. (Electronic Transition)
Line Spectra and the Bohr ModelLine Spectra and the Bohr Model
![Page 13: Electronic Structure. All waves have a characteristic wavelength,, and amplitude, A. Frequency,, of a wave is the number of cycles which pass a point](https://reader035.vdocument.in/reader035/viewer/2022081519/56649e705503460f94b6d752/html5/thumbnails/13.jpg)
Bohr Model• Since the energy states are quantized, the light emitted
from excited atoms must be quantized and appear as line spectra.
• After lots of math, Bohr showed that
where n is the principal quantum number (i.e., n = 1, 2, 3, … and nothing else).
Line Spectra and the Bohr ModelLine Spectra and the Bohr Model
2
18 1J 10178.2
nEn
![Page 14: Electronic Structure. All waves have a characteristic wavelength,, and amplitude, A. Frequency,, of a wave is the number of cycles which pass a point](https://reader035.vdocument.in/reader035/viewer/2022081519/56649e705503460f94b6d752/html5/thumbnails/14.jpg)
• Knowing that light has a particle nature, it seems reasonable to ask if matter has a wave nature.
• Using Einstein’s and Planck’s equations, de Broglie showed:
• The momentum, mv, is a particle property, whereas is a wave property.
• de Broglie summarized the concepts of waves and particles, with noticeable effects if the objects are small.
The Wave Behavior of MatterThe Wave Behavior of Matter
mvh
![Page 15: Electronic Structure. All waves have a characteristic wavelength,, and amplitude, A. Frequency,, of a wave is the number of cycles which pass a point](https://reader035.vdocument.in/reader035/viewer/2022081519/56649e705503460f94b6d752/html5/thumbnails/15.jpg)
The Uncertainty Principle• Heisenberg’s Uncertainty Principle: on the mass scale
of atomic particles, we cannot determine exactly the position, direction of motion, and speed simultaneously.
• For electrons: we cannot determine their momentum and position simultaneously.
• If x is the uncertainty in position and mv is the uncertainty in momentum, then
The Wave Behavior of MatterThe Wave Behavior of Matter
4·
hmvx
![Page 16: Electronic Structure. All waves have a characteristic wavelength,, and amplitude, A. Frequency,, of a wave is the number of cycles which pass a point](https://reader035.vdocument.in/reader035/viewer/2022081519/56649e705503460f94b6d752/html5/thumbnails/16.jpg)
Energy and MatterEnergy and Matter
Size of Matter Particle Property Wave Property
Large – macroscopic
Mainly Unobservable
Intermediate – electron
Some Some
Small – photon Few Mainly
E = m c2E = m c2
![Page 17: Electronic Structure. All waves have a characteristic wavelength,, and amplitude, A. Frequency,, of a wave is the number of cycles which pass a point](https://reader035.vdocument.in/reader035/viewer/2022081519/56649e705503460f94b6d752/html5/thumbnails/17.jpg)
• Schrödinger proposed an equation that contains both wave and particle terms.
• Solving the equation leads to wave functions. • The wave function gives the shape of the electronic
orbital. [“Shape” really refers to density of electronic charges.]
• The square of the wave function, gives the probability of finding the electron ( electron density ).
Quantum Mechanics and Atomic OrbitalsQuantum Mechanics and Atomic Orbitals
EH^
![Page 18: Electronic Structure. All waves have a characteristic wavelength,, and amplitude, A. Frequency,, of a wave is the number of cycles which pass a point](https://reader035.vdocument.in/reader035/viewer/2022081519/56649e705503460f94b6d752/html5/thumbnails/18.jpg)
Quantum Mechanics and Atomic OrbitalsQuantum Mechanics and Atomic Orbitals
Solving Schrodinger’s Equation gives rise to ‘Orbitals.’
These orbitals provide the electron density distributed about the nucleus.
Orbitals are described by quantum numbers.
![Page 19: Electronic Structure. All waves have a characteristic wavelength,, and amplitude, A. Frequency,, of a wave is the number of cycles which pass a point](https://reader035.vdocument.in/reader035/viewer/2022081519/56649e705503460f94b6d752/html5/thumbnails/19.jpg)
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
![Page 20: Electronic Structure. All waves have a characteristic wavelength,, and amplitude, A. Frequency,, of a wave is the number of cycles which pass a point](https://reader035.vdocument.in/reader035/viewer/2022081519/56649e705503460f94b6d752/html5/thumbnails/20.jpg)
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
![Page 21: Electronic Structure. All waves have a characteristic wavelength,, and amplitude, A. Frequency,, of a wave is the number of cycles which pass a point](https://reader035.vdocument.in/reader035/viewer/2022081519/56649e705503460f94b6d752/html5/thumbnails/21.jpg)
Orbitals and Quantum Numbers
Quantum Mechanics and Atomic OrbitalsQuantum Mechanics and Atomic Orbitals
![Page 22: Electronic Structure. All waves have a characteristic wavelength,, and amplitude, A. Frequency,, of a wave is the number of cycles which pass a point](https://reader035.vdocument.in/reader035/viewer/2022081519/56649e705503460f94b6d752/html5/thumbnails/22.jpg)
The s-Orbitals
Representations of OrbitalsRepresentations of Orbitals
![Page 23: Electronic Structure. All waves have a characteristic wavelength,, and amplitude, A. Frequency,, of a wave is the number of cycles which pass a point](https://reader035.vdocument.in/reader035/viewer/2022081519/56649e705503460f94b6d752/html5/thumbnails/23.jpg)
The p-Orbitals
Representations of OrbitalsRepresentations of Orbitals
![Page 24: Electronic Structure. All waves have a characteristic wavelength,, and amplitude, A. Frequency,, of a wave is the number of cycles which pass a point](https://reader035.vdocument.in/reader035/viewer/2022081519/56649e705503460f94b6d752/html5/thumbnails/24.jpg)
d-orbitals
![Page 25: Electronic Structure. All waves have a characteristic wavelength,, and amplitude, A. Frequency,, of a wave is the number of cycles which pass a point](https://reader035.vdocument.in/reader035/viewer/2022081519/56649e705503460f94b6d752/html5/thumbnails/25.jpg)
Atomic OrbitalsAtomic Orbitals• f orbital shapes
![Page 26: Electronic Structure. All waves have a characteristic wavelength,, and amplitude, A. Frequency,, of a wave is the number of cycles which pass a point](https://reader035.vdocument.in/reader035/viewer/2022081519/56649e705503460f94b6d752/html5/thumbnails/26.jpg)
Many-Electron Atoms Many-Electron Atoms
Orbitals and Their Energies
Orbitals CD
![Page 27: Electronic Structure. All waves have a characteristic wavelength,, and amplitude, A. Frequency,, of a wave is the number of cycles which pass a point](https://reader035.vdocument.in/reader035/viewer/2022081519/56649e705503460f94b6d752/html5/thumbnails/27.jpg)
Electron Spin and the Pauli Exclusion Principle
Many-Electron Atoms Many-Electron Atoms
![Page 28: Electronic Structure. All waves have a characteristic wavelength,, and amplitude, A. Frequency,, of a wave is the number of cycles which pass a point](https://reader035.vdocument.in/reader035/viewer/2022081519/56649e705503460f94b6d752/html5/thumbnails/28.jpg)
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
![Page 29: Electronic Structure. All waves have a characteristic wavelength,, and amplitude, A. Frequency,, of a wave is the number of cycles which pass a point](https://reader035.vdocument.in/reader035/viewer/2022081519/56649e705503460f94b6d752/html5/thumbnails/29.jpg)
Figure 6.27
Figure 6.27 Orbitals CD
![Page 30: Electronic Structure. All waves have a characteristic wavelength,, and amplitude, A. Frequency,, of a wave is the number of cycles which pass a point](https://reader035.vdocument.in/reader035/viewer/2022081519/56649e705503460f94b6d752/html5/thumbnails/30.jpg)
Electron Configurations Electron ConfigurationsSpecies Electron Configuration Orbital Notation Comment
![Page 31: Electronic Structure. All waves have a characteristic wavelength,, and amplitude, A. Frequency,, of a wave is the number of cycles which pass a point](https://reader035.vdocument.in/reader035/viewer/2022081519/56649e705503460f94b6d752/html5/thumbnails/31.jpg)
Two Major Factors:
•principal quantum number, n, and
•the effective nuclear charge, Zeff.
Periodic Trends Periodic Trends
![Page 32: Electronic Structure. All waves have a characteristic wavelength,, and amplitude, A. Frequency,, of a wave is the number of cycles which pass a point](https://reader035.vdocument.in/reader035/viewer/2022081519/56649e705503460f94b6d752/html5/thumbnails/32.jpg)
Figure 7.5: Radius video Clip
![Page 33: Electronic Structure. All waves have a characteristic wavelength,, and amplitude, A. Frequency,, of a wave is the number of cycles which pass a point](https://reader035.vdocument.in/reader035/viewer/2022081519/56649e705503460f94b6d752/html5/thumbnails/33.jpg)
Figure 7.6
![Page 34: Electronic Structure. All waves have a characteristic wavelength,, and amplitude, A. Frequency,, of a wave is the number of cycles which pass a point](https://reader035.vdocument.in/reader035/viewer/2022081519/56649e705503460f94b6d752/html5/thumbnails/34.jpg)
Figure 7.10 IE clip
![Page 35: Electronic Structure. All waves have a characteristic wavelength,, and amplitude, A. Frequency,, of a wave is the number of cycles which pass a point](https://reader035.vdocument.in/reader035/viewer/2022081519/56649e705503460f94b6d752/html5/thumbnails/35.jpg)
Figure 7.9
![Page 36: Electronic Structure. All waves have a characteristic wavelength,, and amplitude, A. Frequency,, of a wave is the number of cycles which pass a point](https://reader035.vdocument.in/reader035/viewer/2022081519/56649e705503460f94b6d752/html5/thumbnails/36.jpg)
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)
![Page 37: Electronic Structure. All waves have a characteristic wavelength,, and amplitude, A. Frequency,, of a wave is the number of cycles which pass a point](https://reader035.vdocument.in/reader035/viewer/2022081519/56649e705503460f94b6d752/html5/thumbnails/37.jpg)
Figure 7.11: Electron AffinitiesFigure 7.11: Electron Affinities
![Page 38: Electronic Structure. All waves have a characteristic wavelength,, and amplitude, A. Frequency,, of a wave is the number of cycles which pass a point](https://reader035.vdocument.in/reader035/viewer/2022081519/56649e705503460f94b6d752/html5/thumbnails/38.jpg)
Group Trends for the Active MetalsGroup Trends for the Active Metals
Group 1A: The Alkali Metals
![Page 39: Electronic Structure. All waves have a characteristic wavelength,, and amplitude, A. Frequency,, of a wave is the number of cycles which pass a point](https://reader035.vdocument.in/reader035/viewer/2022081519/56649e705503460f94b6d752/html5/thumbnails/39.jpg)
Group Trends for the Active MetalsGroup Trends for the Active Metals
Group 2A: The Alkaline Earth Metals
![Page 40: Electronic Structure. All waves have a characteristic wavelength,, and amplitude, A. Frequency,, of a wave is the number of cycles which pass a point](https://reader035.vdocument.in/reader035/viewer/2022081519/56649e705503460f94b6d752/html5/thumbnails/40.jpg)
Group Trends for Selected NonmetalsGroup Trends for Selected Nonmetals
Group 6A: The Oxygen Group
![Page 41: Electronic Structure. All waves have a characteristic wavelength,, and amplitude, A. Frequency,, of a wave is the number of cycles which pass a point](https://reader035.vdocument.in/reader035/viewer/2022081519/56649e705503460f94b6d752/html5/thumbnails/41.jpg)
Group Trends for Selected NonmetalsGroup Trends for Selected Nonmetals
Group 7A: The Halogens
![Page 42: Electronic Structure. All waves have a characteristic wavelength,, and amplitude, A. Frequency,, of a wave is the number of cycles which pass a point](https://reader035.vdocument.in/reader035/viewer/2022081519/56649e705503460f94b6d752/html5/thumbnails/42.jpg)
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)
![Page 43: Electronic Structure. All waves have a characteristic wavelength,, and amplitude, A. Frequency,, of a wave is the number of cycles which pass a point](https://reader035.vdocument.in/reader035/viewer/2022081519/56649e705503460f94b6d752/html5/thumbnails/43.jpg)
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)
![Page 44: Electronic Structure. All waves have a characteristic wavelength,, and amplitude, A. Frequency,, of a wave is the number of cycles which pass a point](https://reader035.vdocument.in/reader035/viewer/2022081519/56649e705503460f94b6d752/html5/thumbnails/44.jpg)
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
c
)( photonperch
E
2218 11
10178.2if
fi nnJE],,,[ smmn