chemistry chapter 5
DESCRIPTION
Chemistry Chapter 5. Electrons in Atoms. Light. Is a form of electromagnetic radiation . In some ways it behaves as a wave . . Wavelength. The distance from a point in one wave to the same point in the next wave. Frequency. The number of waves that pass a point in a second . - PowerPoint PPT PresentationTRANSCRIPT
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Chemistry Chapter 5Electrons in Atoms
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Light• Is a form of electromagnetic radiation. • In some ways it behaves as a wave.
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WavelengthThe distance from a point in one wave
to the same point in the next wave.
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FrequencyThe number of waves that pass a
point in a second. Measured in Hertz (Hz)
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AmplitudeThe height of a wave from the origin to
the crest or the origin to the trough.
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Electromagnetic Wave Relationship•c=luC- speedl - wavelengthu - frequency
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Electromagnetic Spectrum• All of the different types of
electromagnetic radiation. The only difference is the wavelength and frequency.
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Light as a dual nature• Light has wave properties, but in
some ways it acts just like a particle. • Quantum – the minimum amount of
energy an atom can lose.
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Photoelectric effect
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Atomic Emission Spectrum• The electromagnetic wavelengths or
frequencies emitted by the atoms of an element.
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Atomic Absorption Spectrum• The electromagnetic wavelengths or
frequencies absorbed by the atoms of an element.
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Bohr’s Model of the Atom• Niels Bohr explained the hydrogen
emission spectrum.• Ground State is the lowest energy
level possible for an atom
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Electron’s Location• An atomic orbital describes the
probable location of an electron in an atom.
• Each orbital can hold 2 electrons spinning in the opposite direction.
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Principle Quantum Number = Principle Energy Level
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Energy sublevelsEach energy level is made up of
sublevels. Sublevels are identified by the letters
s, p, d and f.Each increase in energy level adds 1
sublevel.
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S sublevel (spherical)Each energy level starts with an S
sublevel. The S sublevel only has one orbital and
can hold 2 electrons.
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P sublevel • P sublevels are made up of 3 dumbbell
shaped orbitals. • P sublevels can hold 6 total electrons.
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D sublevels• D sublevels contain 5 orbitals.
– This allows them to hold 10 electrons
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Energy Level
Sublevels Number of orbitals in each sublevel
Number of orbitals in energy level
Number of Electrons
1 s 1 1 2
2 sp
13
4 8
3 spd
135
9 18
4 spdf
1357
16 32
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Electron Configuration• The arrangement of electrons in an
atom– Aufbau principle– Pauli exclusion principle– Hund’s Rule
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Aufbau principle• Electrons will occupy the lowest
energy orbital available.
1s2s 2p3s 3p 3d4s 4p 4d 4f5s 5p 5d 5f6s 6p 6d 7s 7p1
2
3 4 5
6
7 8 910
11 1213 14 1516 17 18
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Pauli Exclusion PrincipleStates that each orbital can hold 2
electrons, but only if the electrons have opposite spin.
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Hund’s RuleEach orbital in the same sublevel must
have one electron with the same spin before any electrons will pair up in the same orbital.
2p
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Orbital Diagrams
1s 2s 2p 3s 3p
Notation1s1
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Orbital Diagrams
1s 2s 2p 3s 3p
Notation1s2
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Orbital Diagrams
1s 2s 2p 3s 3p
Notation1s22s22p2
Nobel Gas Notation[He]2s22p2
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Orbital Diagrams
1s 2s 2p 3s 3p
Notation1s22s22p4
Nobel Gas Notation[He]2s22p4
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Orbital Diagrams
1s 2s 2p 3s 3p
Notation1s22s22p6
Nobel Gas Notation[He] 2s22p6
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Orbital Diagrams
1s 2s 2p 3s 3p
Notation1s22s22p63s23p2
Nobel Gas Notation[Ne]3s23p2
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Orbital Diagrams
1s 2s 2p 3s 3p
Notation1s22s22p63s23p5
Nobel Gas Notation[Ne]3s23p5
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Orbital Diagrams
1s 2s 2p 3s 3p
Notation1s22s22p63s23p6
Nobel Gas Notation[Ne] 3s23p6
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Orbital Diagrams
Notation1s22s22p63s23p64s2
Nobel Gas Notation[Ar]4s2
4s 3d 4p
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Orbital Diagrams
Notation1s22s22p63s23p64s23d6
Nobel Gas Notation[Ar]4s23d6
4s 3d 4p
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Exceptions• Sublevels are more stable when
they are full or half full. • Some elements will move an
electron up in energy to half fill or fill a d sublevel
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Predicted Orbital Diagrams
Predicted Notation1s22s22p63s23p64s23d4
Nobel Gas Notation[Ar]4s23d4
4s 3d 4p
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Predicted Orbital Diagrams
Actual Notation1s22s22p63s23p64s13d5
Nobel Gas Notation[Ar]4s13d5
4s 3d 4p
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Predicted Orbital Diagrams
Predicted Notation1s22s22p63s23p64s23d9
Nobel Gas Notation[Ar]4s23d9
4s 3d 4p
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Actual Orbital Diagrams
Actual Notation1s22s22p63s23p64s13d10
Nobel Gas Notation[Ar]4s13d10
4s 3d 4p
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Valence Electrons• Electrons that are located in the
outermost energy level
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Electron dot structures• (aka Lewis dot diagrams)
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Lewis Dot Diagrams• Symbols that show an element and
it’s valence electrons
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Draw Lewis Dot Diagrams for the following
1. Cl2. O3. Al4. Sr5. Pb