Electron Configuration and Chemical Bonding
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Transcript of Electron Configuration and Chemical Bonding
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Electron ConfigurationChemical Bonding
Amalene Cooper-Morgan, Ph.D.
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General Ordering for Multi Electron Atoms
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Recall…• Remember • S sublevel holds 2 electrons• P sublevel holds 6 electrons• D sublevel holds 10 electrons• F sublevel holds 14 electrons
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Electron Configuration for Bromine
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Use Noble Gases to Represent Inner Electrons
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Valence Electrons• Located in the outermost principal energy level• For transition elements, d electrons are counted among the valence
electrons, although they aren’t in the outermost principal energy level• Core electrons are electrons in complete principal energy levels
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Valence vs Core Electrons
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Main Group Elements• Don’t include transition elements• Valence electrons are in their outermost principal energy level• Example:• Germanium, atomic number 32 is a main group element• Ge n=1, 2 and 3 principal energy levels are complete (Core electrons)• Ge n=4 is the outermost principal level (Valence electrons)
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Electron Configuration for Ge
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Principal Quantum Number
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Orbital blocks of the Periodic Table
Except for the transition metals, main group elementss valence electrons are equal to the lettered groupe.g Chlorine has 7 valence electrons and it’s in group 7A
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Periodic Trends- Size of atoms and Effective Nuclear Charge• Orbitals do not represent a physical boundary but a statistical
probability distribution of where to find an electron• Non bonding atomic radius or van der Waals radius- is the radius of an
atom when it is not bonded to another atom
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Periodic Trends- Size of atoms and Effective Nuclear Charge• Bonding atomic radius or covalent radius• Non-metals- ½ the distance between 2 of the atoms bonded together• Metals- ½ the distance between 2 of the atoms that are next to each other in
a crystal of a metal
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Exceptions..• Bonding radii of He and Ne are approximated• They do not form either chemical bonds or metallic crystals
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Atomic Radius• Average bonding radii• Radius of an atom when its bonded to another atom• Always smaller than van der waals radius
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Approximate bond length• Sum of the atomic radii for 2 covalently bonded atoms• Approx. bond length for ICl:• I atomic radius = 133 pm + Cl atomic radius = 99 pm• Total bond length = 232 pm• Actual bond length is 232.07 pm
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Trends across periodic table• Atomic radii peak with Alkali metals• Atomic radii is mainly determined by the valence electron• As we move• down a column, atomic radius decreases
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Effective Nuclear Charge or Net Charge
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Screening and Effective Nuclear Charge
Core electrons = 1s2 electronNucleus = 3+ Zeff ~ (3+) – 2 ~ 1+
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Trends across the Periodic Table for Effective Nuclear Charge
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Trends across periodic table• As we move across a row to the right the atomic radius decreases• Transition elements, except the first couple of elements in a column,
do NOT follow the same trend for atomic radii as main group elements• Atomic radius does not decrease as you cross the row from L to R• Atomic radii stay constant• The outermost electrons stay constant and experience a constant nuclear
charge, keeping the radius approx. constant