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Transcript of Arrangement of Electrons in Atoms Chapter 4. The New Atomic Model Investigations relationship...
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Arrangement of Electrons in Atoms
Chapter 4
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The New Atomic Model Investigations relationship between light
and atom’s electrons How are electrons arranged? Why don’t
they fall into the nucleus?
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Light a wave or particle? Wave Description:
Electromagnetic Radiation: energy that acts like a wave in space
All forms create Electromagnetic Spectrum
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Electromagnetic Spectrum
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Electromagnetic Spectrum All forms move at speed of light, c,
3.00x108 m/s Forms identified by:
wavelength, , the distance b/ corresponding points on adjacent waves. Units: nm, cm, or m
Frequency, , # of waves that pass a given point in a specific time, 1 sec. Unit: 1/s = Hertz, Hz
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Wavelength and Frequency
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Wavelength and Frequency
c =
Inverse proportion equation!!
speed of light, m/s
wavelength, m
Frequency, 1/s
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Calculation Calculate the wavelength of a radio wave
with a frequency of 102.7 x 106s-1
Determine the frequency of light whose wavelength is 5.267 nm.
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Particle Nature of Light
Photoelectric Effect: emission of electrons from a metal when light shines on the metal
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Photoelectric Effect Light had to be certain frequency to knock
e- loose Wave theory any frequency should
work (just might take a while) Light must also be a particle! Max Planck(1900) explanation: objects
emit energy in small packets called quanta Video - 16
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Max Planck Quantum of energy is the smallest amount
of energy that can be lost or gained by an atom
E = hEnergy of quantum, in joules, J
Planck’s constant,
6.626x10-34 Js
Frequency, s-1
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Energy Calculation What is the energy of green light, with a
wavelength of 500. nm?
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Albert Einstein Light is both wave and particle! Particle of light = photon, having zero
mass and a quantum of energy Photons hit metal and knock e- out, but
photon has to have enough energy
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H-atom Emission Spectrum Pass a current through gas at low pressure
it excites the atoms Ground state: lowest energy state of an
atom Excited state: atom has higher potential
energy than it has in ground state
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H – Atom Spectrum When atom jumps from excited state to
ground state it gives off energy LIGHT!
Ephoton = E2 – E1 = hv
E2
E1
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Bohr Model of H-atom
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H-atom Line Emission Spectrum
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Element Emission SpectrasHelium – 23 lines
Neon – 75 lines
Argon - 159 lines
Xenon – 139 lines
Mercury – 40 lines
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H-atom Line Emission Spectrum More lines in UV (Lyman series) and
IR(Paschen series) Why did H-atom only emit certain colors
of light? Explanation led to new atomic theory
Quantum Theory
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Bohr Model of H-atom 1913 – Niels Bohr e- circles nucleus in certain paths, orbits or
atomic energy levels e- is higher in energy the farther away from
nucleus e- cannot be between orbits Video - 23
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Bohr Model of H-atom
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Bohr Model of H-atom From wavelengths of emission spectrum
Bohr calculated energy levels of H-atom Model worked ONLY for H-atom
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Quantum Model of Atom Can e- behave as a wave?
Yes! To find e- use a photon, but photon will
knock the e- off course Heisenberg Uncertainty Principle:
impossible to determine position and velocity of a particle at the same time.
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Schrödinger Wave Equation 1926 – developed equation and only e-
waves of certain frequencies were solutions Quantization of e- probability of finding
e- in atom No neat orbits probability clouds or
orbitals
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Electron Configurations
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Atomic Orbitals Def: 3-D region around nucleus that
indicates the probable location of an electron
Energy levels or shells: Numbered 1-7 Smaller number = closer to nucleus, lower
energy
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Sublevels Each shell has sublevels s
1 – s orbital p
3 – p orbitals d
5 – d orbitals f
7 – f orbitals
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Shells and Sublevels Shells and sublevels together: 1s 2s, 2p 3s, 3p, 3d 4s, 4p, 4d, 4f, etc. s is the lowest energy and f is the highest
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Orbitals
Each orbital in a sublevel can hold a maximum of 2 e-
1 – s 2 e- max. 3 – p orbitals 6 e- max. 5 – d orbitals 10 e- max. 7 – f orbitals 14 e- max.
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Electron Configurations Arrangement of e- in atom Orbital Notation: H has 1e- Rules:
1. Aufbau Principle: electron occupies lowest energy level that can receive it
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Electron Configurations2. Pauli Exclusion Principle: no two e- in
an sublevel orbital can have the same spin3. Hund’s Rule: orbitals of equal energy are
occupied by one e- before pairing up e-. All single occupied orbitals must have same spin.
He – 2e-
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Energy of sublevels
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Electron Configurations N S Ti I
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Electron Configuration Notation B Ni Hg
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Noble Gas Notation Use noble gas from previous row
Al Pb
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Special Cases d sublevel more stable with half-filled or
completely filled sublevel Cr Cu