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Electrons in Atoms Chap. 5
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Light (electromagnetic radiation)
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Light (electromagnetic radiation)
A. Two components
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Light (electromagnetic radiation)
A. Two components Electrical wave
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Light (electromagnetic radiation)
A. Two components Electrical wave Magnetic wave
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Light (electromagnetic radiation)
A. Two components B. Two natures
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Light (electromagnetic radiation)
A. Two components B. Two natures Particle
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Light (electromagnetic radiation)
A. Two components B. Two natures Particle Wave
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Light Characteristics of a Light Wave
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Light Characteristics of a Light Wave wavelength
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Light Characteristics of a Light Wave wavelength
The distance between successive wave crests
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Light Characteristics of a Light Wave wavelength frequency
The time it takes a wave to pass a given point
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Light Characteristics of a Light Wave wavelength frequency amplitude
The height of a wave
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Light Characteristics of a Light Wave wavelength frequency amplitude
speed
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Light Characteristics of a Light Wave The Wave Equation
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Light Characteristics of a Light Wave The Wave Equation
inverse relation of wavelength and frequency
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Light Characteristics of a Light Wave The Wave Equation
inverse relation of wavelength and frequency check the units
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The Wave Equation c = λ x υ
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Self Check – Ex. 1 A light wave has a frequency of 2.6 x 1014 Hz. What is the wavelength?
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Self Check – Ex. 2 What is the frequency of light with a wavelength of m?
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Light Characteristics of a Light Wave The Wave Equation
Planck’s Equation
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Planck’s Equation E = h x υ h = 6.63 x J·s
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Self Check – Ex. 3 A light photon has 4.2 x J of energy. What is the frequency of this light?
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Self Check – Ex. 4 How much energy does a photon of orange light have (λ = 630 nm)? 109 nm = 1 m
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Light Characteristics of a Light Wave The Wave Equation
Planck’s Equation The Electromagnetic Spectrum
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Electromagnetic Spectrum
Long waves Short waves
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Electromagnetic Spectrum
Long waves Short waves Radio waves
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Electromagnetic Spectrum
Long waves Short waves Radio waves Micro-waves
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Electromagnetic Spectrum
Long waves Short waves Radio waves Infra-red Micro-waves
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Electromagnetic Spectrum
Long waves Short waves Radio waves Infra-red Micro-waves Visible
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Electromagnetic Spectrum
Long waves Short waves Radio waves Infra-red Ultra-violet Micro-waves Visible
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Electromagnetic Spectrum
Long waves Short waves Radio waves Infra-red Ultra-violet Micro-waves Visible X-rays
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Electromagnetic Spectrum
Long waves Short waves Radio waves Infra-red Ultra-violet Gamma rays Micro-waves Visible X-rays
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Emission Spectra
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Emission Spectra Definition
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The various types of light given off when an atom is excited
Emission Spectrum: The various types of light given off when an atom is excited
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Emission Spectra Definition Examples
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Hydrogen’s Spectrum Note – only a few colors are present 400 nm 500 nm
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Mercury’s Spectrum 400 nm 500 nm 600 nm 700 nm
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Neon’s Spectrum 400 nm 500 nm 600 nm 700 nm
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Emission Spectra Definition Examples Explanation – Bohr’s Model
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Bohr’s Model of an Atom e-
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Bohr’s Model of an Atom e-
Electrons orbit the nucleus (like planets orbiting the sun) e-
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Bohr’s Model of an Atom e-
Electrons must be in a specific orbit (never between orbits) e- n=1 n=2 n=3
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Bohr’s Model of an Atom e-
Electron wants to be in the lowest unoccupied level e-
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Bohr’s Model of an Atom e-
The energy of the electrons depends on the distance from the nucleus e- high energy low energy
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Bohr’s Model of an Atom e-
Light is emitted when electrons fall to lower energy levels e-
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Bohr’s Model of an Atom Only certain sized falls are permitted. e-
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Hydrogen’s Spectrum What is the energy for each line produced? Color
410 nm 486 nm 656 nm 434 nm Color Wavelength Frequency Energy Red 6.56x10-7 m Green 4.86x10-7 m Blue 4.34x10-7 m Purple 4.10x10-7 m
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Hydrogen’s Spectrum What is the energy for each line produced? Color
410 nm 486 nm 656 nm 434 nm Color Wavelength Frequency Energy Red 6.56x10-7 m 4.57x1014 Hz Green 4.86x10-7 m 6.17x1014 Hz Blue 4.34x10-7 m 6.91x1014 Hz Purple 4.10x10-7 m 7.32x1014 Hz
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Hydrogen’s Spectrum What is the energy for each line produced? Color
410 nm 486 nm 656 nm 434 nm Color Wavelength Frequency Energy Red 6.56x10-7 m 4.57x1014 Hz 3.03x10-19 J Green 4.86x10-7 m 6.17x1014 Hz 4.09x10-19 J Blue 4.34x10-7 m 6.91x1014 Hz 4.58x10-19 J Purple 4.10x10-7 m 7.32x1014 Hz 4.85x10-19 J
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III. A new model
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III. A new model A. Quantum Mechanics
Electrons’ location cannot be accurately determined
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III. A new model A. Quantum Mechanics 1. Orbitals
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Orbital A region of space around the nucleus where an electron is likely to be found.
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Types of Orbitals s orbital
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Types of Orbitals s orbital p orbitals
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Types of Orbitals s orbital p orbitals d orbitals
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Types of Orbitals s orbital p orbitals d orbitals f orbitals
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III. A new model A. Quantum Mechanics Orbitals Sublevels
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Sub-level A group of orbitals that have the same shape and energy.
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III. A new model A. Quantum Mechanics Orbitals Sublevels
A few examples
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III. A new model A. Quantum Mechanics Orbitals Sublevels
A few examples Their electron capacity
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Sublevels Capacity Each orbital can hold 2 electrons
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Sublevels Capacity Each orbital can hold 2 electrons
An ‘s’ sublevel is made of ONE orbital, so it holds ___ electrons
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Sublevels Capacity Each orbital can hold 2 electrons
An ‘s’ sublevel is made of ONE orbital, so it holds _2_ electrons
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Sublevels Capacity Each orbital can hold 2 electrons
An ‘s’ sublevel is made of ONE orbital, so it holds _2_ electrons A ‘p’ sublevel is made of THREE orbitals, so it holds ___ electrons
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Sublevels Capacity Each orbital can hold 2 electrons
An ‘s’ sublevel is made of ONE orbital, so it holds _2_ electrons A ‘p’ sublevel is made of THREE orbitals, so it holds _6_ electrons
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Sublevels Capacity Each orbital can hold 2 electrons
An ‘s’ sublevel is made of ONE orbital, so it holds _2_ electrons A ‘p’ sublevel is made of THREE orbitals, so it holds _6_ electrons A ‘d’ sublevel is made of FIVE orbitals, so it holds ____ electrons
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Sublevels Capacity Each orbital can hold 2 electrons
An ‘s’ sublevel is made of ONE orbital, so it holds _2_ electrons A ‘p’ sublevel is made of THREE orbitals, so it holds _6_ electrons A ‘d’ sublevel is made of FIVE orbitals, so it holds _10_ electrons
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Sublevels Capacity Each orbital can hold 2 electrons
An ‘s’ sublevel is made of ONE orbital, so it holds _2_ electrons A ‘p’ sublevel is made of THREE orbitals, so it holds _6_ electrons A ‘d’ sublevel is made of FIVE orbitals, so it holds _10_ electrons An ‘f’ sublevel is made of SEVEN orbitals, so it holds ____ electrons
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Sublevels Capacity Each orbital can hold 2 electrons
An ‘s’ sublevel is made of ONE orbital, so it holds _2_ electrons A ‘p’ sublevel is made of THREE orbitals, so it holds _6_ electrons A ‘d’ sublevel is made of FIVE orbitals, so it holds _10_ electrons An ‘f’ sublevel is made of SEVEN orbitals, so it holds _14_ electrons
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III. A new model A. Quantum Mechanics Orbitals Sublevels
A few examples Their electron capacity The ordered list
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III. A new model B. Arrangement of electrons
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III. A new model B. Arrangement of electrons Aufbau principle
Electrons fill the lowest energy level first.
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III. A new model B. Arrangement of electrons Aufbau principle
Pauli Exclusion Principle Two electrons per orbital with opposite spin
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III. A new model B. Arrangement of electrons Aufbau principle
Pauli Exclusion Principle Hund’s Rule Half fill all orbitals in a sublevel before completely filling them
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III. A new model B. Arrangement of electrons Aufbau principle
Pauli Exclusion Principle Hund’s Rule A pictorial representation ‘The Aufbau Hotel’
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IV. Orbital Diagrams A representation of the electrons in an atom
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IV. Orbital Diagrams Boxes represent . . .
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IV. Orbital Diagrams Boxes represent . . .
An ‘f’ sublevel should have 7 boxes
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IV. Orbital Diagrams Boxes represent . . .
An ‘f’ sublevel should have 7 boxes ‘d’ = 5 boxes
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IV. Orbital Diagrams Boxes represent . . .
An ‘f’ sublevel should have 7 boxes ‘d’ = 5 boxes ‘p’ = 3 boxes
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IV. Orbital Diagrams Boxes represent . . .
An ‘f’ sublevel should have 7 boxes ‘d’ = 5 boxes ‘p’ = 3 boxes ‘s’ = 1 box
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IV. Orbital Diagrams Boxes represent . . . Arrows represent . . .
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IV. Orbital Diagrams Boxes represent . . . Arrows represent . . .
These boxes are filled in a specific order See Aufbau, Pauli Exclusion, and Hund above
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Self Check – Ex. 5 Write the orbital diagrams for: Fluorine Vanadium
Germanium
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V. Electron Configuration
A shorthand notation of electron positions in an atom
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V. Electron Configuration
Number represents energy level
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V. Electron Configuration
Number represents energy level Letter shows the type of sublevel
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V. Electron Configuration
Number represents energy level Letter shows the type of sublevel Electrons are counted and written as an exponent
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V. Electron Configuration
The ordered list
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V. Electron Configuration
The ordered list 1s22s22p63s23p64s23d104p65s24d105p66s24f145d106p67s25f146d107p6
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Self Check – Ex. 6 Write the electron configurations for: Magnesium
Sulfur Silver
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VI. Electron Config. using P.T.
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VI. Electron Config. using P.T.
The s-block
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VI. Electron Config. using P.T.
The s-block The p-block
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VI. Electron Config. using P.T.
The s-block The p-block The d-block
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VI. Electron Config. using P.T.
The s-block The p-block The d-block The f-block
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VI. Electron Config. using P.T.
The s-block The p-block The d-block The f-block The order of sublevels (made easy!)
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Self Check – Ex. 7 Use your P.T. to write electron configurations for:
Potassium Arsenic Rhodium
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VII. Electron Config. using abbreviations
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VII. Electron Config. using abbreviations
Abbreviate the previous noble gas in brackets
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VII. Electron Config. using abbreviations
Abbreviate the previous noble gas in brackets Write configuration of remaining electrons
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Self Check – Ex. 8 Write the abbreviated electron configurations for:
Iridium Terbium Radon
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VII. Exceptions to Aufbau
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VII. Exceptions to Aufbau
Copper 1s22s22p63s23p64s13d9
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VII. Exceptions to Aufbau
Copper Chromium 1s22s22p63s23p64s13d5
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VII. Exceptions to Aufbau
Copper Chromium There are others
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IX. Lewis Dot Diagrams A diagram that uses dots to represent valence electrons
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IX. Lewis Dot Diagrams Valence electron
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IX. Lewis Dot Diagrams Valence electron
The outermost electrons (the ones that bond)
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IX. Lewis Dot Diagrams Valence electron
The outermost electrons (the ones that bond) Determined by adding the highest energy s and p electrons
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Self Check – Ex. 9 How many valence electrons do the following have?
Nitrogen Arsenic Chlorine
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IX. Lewis Dot Diagrams Valence electron
We write these for representative elements Representative elements are found in the ‘s’ and ‘p’ blocks
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Self Check – Ex. 5 Write Lewis structures for: Strontium Iodine
1s22s22p63s23p64s23d104p65s24d105p3
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The End
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