3-Atomic Structure Overview Characteristics of Atoms Interaction b/tw matter and light...
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Transcript of 3-Atomic Structure Overview Characteristics of Atoms Interaction b/tw matter and light...
3-Atomic Structure
Overview
• Characteristics of Atoms
• Interaction b/tw matter and light– Photoelectric Effect
• Absorption and Emission Spectra
• Electron behavior
• Quantum numbers
Atomic Structure
• Atomic orbitals– Orbital energies– Electron configuration and the periodic
table
• Periodic table– Periodic properties– Energy
Characteristics of Atoms
• Atoms possess mass• Atoms contain positive nuclei• Atoms contain electrons• Atoms occupy volume• Atoms have various properties• Atoms attract one another• Atoms can combine with one another to form
molecules
Atomic Structure
• Atomic structure studied through atomic interaction with light
• Light: electromagnetic radiation– carries energy through space– moves at 3.00 x 108 m/s in vacuum– wavelike characteristics
Electromagnetic Spectrum
Visible Spectrum
Wavelength () & Frequency ()
= number of complete cycles to pass given point in 1 second
amplitude
Energy
c = x = 3.00 x 108 m/s
long wavelength low frequency
short wavelength high frequency
Low Energy
High Energy
Energy
Mathematical relationship:
E = hE = energy
h = Planck’s constant: 6.63 x 10–34 J s
= frequency in s–1
Energy
Mathematical relationship:E = hc = x
hc
E =
Energy: directly proportional to frequencyinversely proportional to wavelength
Problems 3-1, 2, & 3
1. a) Calculate the wavelength of light with a frequency = 5.77 x 1014 s–1 b) What is the energy of this light?
2. Which is higher in energy, light of wave-length of 250 nm or light of 5.4 x 10–7 m?
3. a) What is the frequency of light with an energy of 3.4 x 10–19 J?b) What is the wavelength of light with an energy of 1.4 x 10–20 J?
Photoelectric Effect
• Light on metal surface
• Electrons emitted
• Threshold frequency, o
If < o, no photoelectric effect
If > o, photoelectric effect
As , kinetic energy of electrons
Photoelectric Effect
Einstein: energy frequency
If < o electron doesn’t have enough energy to leave the atom
If > o electron does have enough energy to leave the atom
Energy is transferred from light to electron, extra is kinetic energy of electron
Ephoton = hphoton = ho + KEelectron
KEelectron = hphoton – ho
Animation
Problem 3-4
A given metal has a photoelectric threshold frequency of o = 1.3 x 1014
s1. If light of = 455 nm is used to produce the photoelectric effect, determine the kinetic energy of the electrons that are produced.
Bohr Model
Line spectra
Light through a prism continuous spectrum:
Ordinary white light
Bohr Model
Line spectra
Light from gas-discharge tube
through a prism line spectrum:
H2 discharge
tube
Line Spectra (emission)
White light
H
He
Ne
Line Spectra (absorption)
Light source
Gas-filled tube
Bohr Model
For hydrogen:
22 n
1
2
1 C C = 3.29 x 1015 s–1
Niels Bohr: Electron energy in the atom is quantized.
2n n
1RE H n = 1, 2, 3,….
RH = 2.18 x 10–18 J
Bohr ModelEatom = Eelectron = h
E = Ef – Ei = h
2
18
2Hn n
10 x 18.2
n
1RE
22
fi n
1
n
1
h
R
h
E H
Line spectrum
Photoelectric effect: n
Minus sign: free electron has zero energy
Bohr Energy Levels
Electrons
• All electrons have same charge and mass
• Electrons have properties of waves and particles (De Broglie)
mu
hparticle
Heisenberg Uncertainty Principle
Cannot simultaneously know the position and momentum of electron
x = h
Recognition that classical mechanics don’t work at atomic level.
Schrödinger Equation
Erwin Schrödinger 1926
Wave functions with discrete energies
Less empirical, more theoretical
n En
n wave functions or orbitals
n2
probability density functions
Quantum Numbers
Each orbital defined by 3 quantum numbers
Quantum number: number that labels state of electron and specifies the value of a property
Quantum Numbers
Principal quantum number, n (shell)
Specifies energy of electron (analogous to Bohr’s n)
Average distance from nucleus
n = 1, 2, 3, 4…..
Quantum Numbers
Azimuthal quantum number, (subshell) = 0, 1, 2… n–1
n = 1, = 0
n = 2, = 0 or 1
n = 3, = 0, 1, or 2
Etc. 0 1 2 3 4
s p d f g
Quantum Numbers
Magnetic quantum number, m
Describes the orientation of orbital in space
m = –….+
If = 2, m = –2, –1, 0, +1, +2
Problem 3-5
Fill in the quantum numbers in the table below.
n m
3 0 0 3s
2 –2, –1, 0, 1, 2
0
2p
Schrödinger Equation
Wave equations: Each electron has & E associated w/ it
Probability Density Functions: 2
-graphical depiction of high probability of finding electron
Probability Density Functions
energy
2 probability density function
s, p, d, f, g
1s 2s
3s
Node: area of 0 electron density
Link to Ron Rinehart’s page
Probability Density Functions
2p
Node: area of 0 electron density
3p
nodes
Link to Ron Rinehart’s page
Electrons and Orbitals
Pauli Exclusion Principle: no two electrons in the same atom may have the same quantum numbers
Electron spin quantum number ms = ½
Electrons are spin paired within a given orbital
Electrons and Orbitals
n = 1
= 0, m = 0, ms = ½
2 electrons possible:
1,0,0,+½ and 1,0,0,–½
2 electrons per orbital
1s1 H
1s2 He
Electrons and Orbitals
n = 2
= 0, m = 0, ms = ½2,0,0, ½2 electrons possible
n = 2
= 1, m = –1,0,+1, ms = ½2,1,–1, ½ 2,1,0, ½ 2,1,+1, ½6 electrons possible
Electron Configurations
n = 1
1s 2 electrons possible
H 1e– 1s1
He 2e– 1s2
Electron Configurations
n = 2
2s 2 electrons possible
Li 3e– 1s2 2s1
1s
2s
Be 4e– 1s2 2s2
1s
2s
Electron Configurations
n = 2
2p = 1, m = –1, 0, +1
3 x 2p orbitals (px, py, pz): 6 electrons possible
B 5e– 1s2 2s2 2p1
1s
2s
2p
Electron Configurations
n = 2
2p = 1, m = –1, 0, +1
3 x 2p orbitals (px, py, pz): 6 electrons possible
B 5e– 1s2 2s2 2p1
1s
2s
2p
Electron Configurations
n = 2
2p = 1, m = –1, 0, +1
C 6e– 1s2 2s2 2p2
1s
2s
2p
Hund’s Rule: for degenerate orbitals, the lowest energy is attained when electrons w/ same spin is maximized
Problem 3-6
Write electron configurations and depict the electrons for N, O, F, and Ne.
Electron Configurations
n = 3
3s, 3p, 3d
Na 11e– 1s2 2s2 2p63s1
1s
2s
2p
3s
3p
Electron Configurations
n = 3
3s, 3p, 3d
Mg 12e– 1s2 2s2 2p63s2
1s
2s
2p
3s
3p
Electron Configurations
n = 3
3s, 3p, 3d
Al 13e– 1s2 2s2 2p63s23p1
1s
2s
2p
3s
3p
Electron Configurations
n = 3
3s, 3p, 3d
Si 14e– 1s2 2s2 2p63s23p2
1s
2s
2p
3s
3p
Electron Configurations
n = 3
3s, 3p, 3d
P 15e– 1s2 2s2 2p63s23p3
1s
2s
2p
3s
3p
Electron Configurations
n = 3
3s, 3p, 3d
S 16e– 1s2 2s2 2p63s23p4
1s
2s
2p
3s
3p
Electron Configurations
n = 3
3s, 3p, 3d
Cl 17e– 1s2 2s2 2p63s23p5
1s
2s
2p
3s
3p
Electron Configurations
n = 3
3s, 3p, 3d
Ar 18e– 1s2 2s2 2p63s23p6
1s
2s
2p
3s
3p
Electron Configurations
3d vs. 4s
Filling order 1s
2s 2p
3s 3p 3d
4s 4p 4d 4f
5s 5p 5d 5f 5g
6s 6p 6d
7s 7p
Electron Configurations
1s
2s2p
3s
3p
4s
4p
3dK
Electron Configurations
1s
2s2p
3s
3p
4s
4p
3dCa
Electron Configurations
1s
2s2p
3s
3p
4s
4p
3dSc
Electron Configurations
1s
2s2p
3s
3p
4s
4p
3dTi
Link to OSU site
Problem 3-7
Write the electron configurations for the transition metals V – Zn. Fill in the corresponding boxes to denote the electronic spin.