!Electrons in Atoms Chapter 13.1 and 13.2. Atomic Models !Atomic models help explain the nature of...
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Transcript of !Electrons in Atoms Chapter 13.1 and 13.2. Atomic Models !Atomic models help explain the nature of...
![Page 1: !Electrons in Atoms Chapter 13.1 and 13.2. Atomic Models !Atomic models help explain the nature of elements—part of atomic theory –We can not see atoms,](https://reader036.fdocuments.in/reader036/viewer/2022081516/5697bfec1a28abf838cb86cf/html5/thumbnails/1.jpg)
!Electrons in Atoms
Chapter 13.1 and 13.2
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Atomic Models
• !Atomic models help explain the nature of elements—part of atomic theory– We can not see atoms,
so how do we know they exist?
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!Scanning Tunneling Microscope
• !Can “see” atoms! Can even be used to rearrange individual atoms!
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!Thompson’s Plum Pudding Model
• Thompson imagined a positively charged ball of “pudding” with electrons (which he discovered) as the “plums” inside
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Niels Bohr’s Model• 1913: !Bohr imagined electrons follow
circular orbits around the nucleus, like a solar system
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Energy Levels
• !The energy level of an electron is the region around the nucleus where the electron is moving
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!Energy Levels are Fixed
• !Energy levels are like rungs on a ladder– !Electrons exist on rungs– !Electrons can jump
between rungs– !Electrons can’t exist
between rungs
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It takes energy to jump between energy levels
• !Quantum: The amount of energy required to move from one energy level to another– Part of the Quantum Theory
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Neils Bohr
• "If quantum mechanics hasn't profoundly shocked you, you haven't understood it yet."
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Light and Atomic Spectra
• !Spectrum: a series of energies (like light) arranged according to wavelength, or frequency
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!Atomic Emission Spectrum
• !Every element (vapor) emits light when it is excited by the passage of electric discharge.
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Atomic Emission Spectrum
• !Passing this light through a prism creates a spectrum, different for every element.– !Each line
represents one exact amount of energy
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More on Quantum Theory:• Subatomic particles don’t
follow the rules of classical physics– Gravity doesn’t apply!– Time doesn’t apply!– Can move without
occupying space!– Superposition—can’t
locate position!– Order of operations don’t
always apply!
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Neils Bohr
• "If quantum mechanics hasn't profoundly shocked you, you haven't understood it yet."
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The Quantum Mechanical Model
• Erwin Schrodinger, in 1926, used quantum theories to solve a mathematical equation concerning the location and energy of an electron.
• (But not both at once)
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!Electron Orbitals—Quantum Theory
• !The area where an electron is likely to be found. (90% chance)
• !An orbital can contain two electrons.
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Energy levels and
orbitals•!Types of orbitals
!s orbital = sphere shaped (1 type)
!p orbitals = dumbell shaped (3 types)
!d orbitals = clover shaped (5 types)
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Electron Configurations
• High energy = unstable, higher energy levels, further away from nucleus
• Low energy = stable
• Three major rules tell you how to find where electrons will be:
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!Rule 1: Aufbau Principle• !Electrons enter orbitals of
lowest energy first.
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!Rule 2: Pauli Exclusion Principle
• !An atomic orbital is one or two electrons– To be in the same orbital, two electrons must be
“opposite”
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!Rule 3: Hund’s Rule
• !Electrons in the same energy level must enter each orbital until all the orbitals contain one electron with parallel spins.
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!Electron Cloud
• !All the electrons in all the orbitals.