electrons in atoms. electromagnetic radiation form of energy that exhibits both wavelike behaviors...
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Electrons In Atoms
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Electromagnetic Radiation• Form of energy that exhibits
both wavelike behaviors and particle behaviors
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Electromagnetic Spectrum
• Shows all forms of electromagnetic radiation
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Quanta• Electrons gain/lose energy in
set increments only• Each set amount of energy is
called a quantum• Lost energy is released as
electromagnetic radiation, with more energy = higher frequency
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Photoelectric Effect• Emission of electrons from
metal’s surface when light of specific frequency shines on surface
METAL
light e-
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Wrap-Up #1• If electrons will only be
emitted by light of high energy, which of the following is more likely to release electrons?
–Blue light with low intensity
(dim)
–Red light with high intensity
(bright)
–Radio waves with high intensity
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Bohr Model – Electron States
• Ground State– Lowest energy state of an electron– Where the electron is “naturally”
• Excited State– State when an electron gains
energy– Only exists while energy is being
absorbed by the atom• Glow in the dark materials – the
electrons absorb energy from light and re-release it as light when its surroundings are dark
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Bohr Model
E1E2
E3
E1 = lowest energy level
E3 > E2 > E1
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Ground State to Excited State
1. in ground state, no energy radiated
2. in excited state, electrons jump to higher energy level (because they’ve absorbed energy from an external source)
3. electrons go from high E level to low E level
4. photon emitted
1
2
3
456
En
erg
y o
f at
om
1
2
3
4
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Atomic Orbitals• Volume surrounding the
nucleus in which an electron is 90% likely to be found
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Principle Quantum Number (n)
• Indicates the energy level an electron is on–Use periodic table to tell–The period number
corresponds to the principle quantum number (n = 1,2,3…)
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Energy Orbitals• Shape of orbital that tells the
path of the electrons–4 orbitals: s, p, d, f–The letter tells you the shape of the orbital
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s orbital• Shape: electrons travel in a
sphere
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s orbital
1s
2s
3s
The greater the energy level, the bigger the orbital
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p orbital• Shape: dumbbell or figure 8
shaped
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d orbital• Shape – double dumbbells or
a dumbell with a ring around it
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Electron Configuration• Description of the
arrangement of electrons in an atom
• Allows us to visualize where the electrons in an atom can be found
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Rules Governing Electron Configurations1) Aufbau Principle – electrons
occupy lowest energy orbital available- fill up level 1 first, then level 2, etc.
2) Pauli Exclusion Principle – there is a max number of electrons that occupy a single orbital (2) and they must have opposite spin
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Rules Governing Electron Configurations3) Hund’s Rule – if orbitals
have equal energy, one e- will go in each orbital before doubling up1 2
4
3
5 6
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Rules Governing Electron Configurations3b) Hund’s Rule – all electrons
in singly occupied orbitals must have the same spin
Yes
NO NO NO
Yes Yes
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Blocks On Periodic Table
sd
p
f
s
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Divisions of Orbitals• s orbital – 1 sublevel (2 e-
max)
• p orbital – 3 sublevels (6 e- max)
• d orbital – 5 sublevels (10 e- max)
• f orbital – 7 sublevels (14 e- max)
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Orbital Diagram• Nitrogen• How many electrons? 7
1s 2s 2p
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Orbital Diagram• Silicon• How many electrons?14
1s 2s 2p 3s 3p
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Wrap-Up #2: Orbital Diagram
• Copper• How many electrons?29
1s 2s 2p 3s 3p
4s 3d
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Electron Configuration Notation• Oxygen (8 e-)
• Sulfur (16 e-)
• Vanadium (23 e-)
1s 2s 2p2 2 4
1s 2s 2p2 2 6 3s 3p2 4
1s 2s 2p2 2 6 3s 3p 264s2 3d 3
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• Rule: start from previous noble gas, then write the configuration
• Oxygen
• Sulfur
• Vanadium
Noble Gas Notation
[He]2s 2p2 4
[Ne]3s 3p2 4
[Ar] 4s 3d2 3
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Valence Electrons• Electrons in outer most
energy level- located in highest s & p orbitals
N:
Mg:
Se:
2s 2p2 31s2 5 valence e-
2s 2p2 61s2 3s2 2 valence e-
2s 2p2 61s2 3p 4s6 23s2 3d 4p10 4
6 valence e-
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Electron Dot Structure• Shows valence electrons in a
diagram• Nitrogen (5 v.e.)
• Magnesium (2 v.e.)
• Selenium (6 v.e.)
N
Mg
Se