Honors Chemistry Section 4.3
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Transcript of Honors Chemistry Section 4.3
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Honors ChemistrySection 4.3
Electron Configurations
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Electron Configuration
Electron Configuration is the arrangement of electrons in an atom
Every atom has a unique electron configuration
Atoms tend to lowest E state, so normally exist in ground state
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Rules for Electron Configuration
Aufbau Principle – Electrons occupy the lowest energy orbital available to them
Pauli Exclusion Principle – No two electrons can have the same 4 quantum numbers
Hund’s Rule – Orbitals of equal energy (called degenerate orbitals) are each occupied by one electron, before any is occupied by a second electron. All single electrons have the same spin.
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Orbital Energies
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Orbital Notation
Hydrogen◦ ↿
1s
Helium◦ ↿⇂
1s
Oxygen◦ ↿⇂ ↿⇂ ↿⇂ ↿⇂ ↿⇂ 1s 2s 2px 2py 2pz
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Electron Configuration
Hydrogen◦1s1
Helium◦1s2
Oxygen◦1s2 2s2 2p4
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Filling Order – Memory Aid
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Practice
What is the electron configuration of Carbon?
Write the electron configuration and orbital notation for Sulfur
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Definitions
Highest Occupied Level – The highest main energy level (highest n value) that contains an electron
Outer shell electrons – electrons in the Highest Occupied Level
Inner shell electrons – all those electrons EXCEPT those in the Highest Occupied Level
Example – Carbon◦2 inner shell electrons◦4 outer shell electrons
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Noble Gases
Noble gas – Has full s and p orbitalsNoble gas configuration
◦[symbol] stand for the complete electron configuration of the specified noble gas
◦Add electrons after noble gas required for element.
◦Na – [Ne] 3s1
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Important Note
All noble gases have full outer main energy levels◦He – 2 electrons (Energy Level n=1)◦All others – 8 electrons (Energy Level n = 2 to
7)
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Filling Orbtials and the Periodic Table
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Fourth Period
Fill 4s firstThen next lowest energy 3d – it fills nextFollowed by 4p
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4th Period Exceptions to the Expected Filling Order – KNOW THESE!!!!
Chromium◦Expected - [Ar] 3d4 4s2
◦Actual - [Ar] 3d5 4s1
◦Why? Two half filled orbitals have more stability and lower energy
than one full and one partially fullCopper
◦Expected - [Ar] 3d8 4s2
◦Actual - [Ar] 3d10 4s0
◦Why? A full d orbital and unfilled s orbital have more stability and
lower energy than one full and one partially full
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5th Block Exceptions to the Expected Filling Order
Deviates from Nb to Ag
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Practice
1. What element has 2 electrons in the p orbitals in the 2nd Energy Level?
2. What is the maximum number of electrons that can be found on the second energy level?
3. What element in the third period has the same outer electron configuration as the element in #1?
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More Practice
1. What element has 5 electrons in the p sublevel on the third energy level?
2. How many total electrons does this element have on the third energy level?
3. What element in the 4th Period has the same outer configuration as this element?
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Even More Practice
What element has the configuration [Ne]3s1?
How many inner shell electrons does this element have?
What is the Noble Gas configuration for Al?◦How many outer shell electrons?◦How many inner shell electrons?
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Are you Ready for More?
Write the electron configuration and Noble Gas configuration for Ti.
How many electron containing orbitals in Ti?
How many orbitals in Ti are completely filled?