Bonding – forces that hold atoms together 1.ionic 2.covalent 3.metallic ionic bonding – ions...
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Transcript of Bonding – forces that hold atoms together 1.ionic 2.covalent 3.metallic ionic bonding – ions...
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bonding – forces that hold atoms together
1. ionic2. covalent3. metallic
ionic bonding – ions that are held together via unlike charges
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Lewis dot symbol – shorthand method of showing the number of valence electrons available for bonding in atoms
Gilbert Lewis 1875 – 1946
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octet rule – atoms gain or lose or share electrons in an effort to obtain8 valence electrons
What is so special about 8 valence electrons ?
8 valence electrons = noble gas configuration
noble gas configuration is energetically stable !
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Determine the empirical formula expected for a compound containing Ca and F.
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covalent bonding – 2 electrons are “shared” between 2 atoms.
Covalently bound species are different than ionic• exist as individual, discrete species (vs. 3-D
crystal lattice structure for ionic)• tend to exhibit much lower melting and boiling
points (vs. ionic)
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single bond – 2 electrons (1 pair of electrons) are shared between 2 atoms
double bond – 4 electrons (2 pairs of electrons) are shared between 2 atoms
triple bond – 6 electrons (3 pairs of electrons) are shared between 2 atoms
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a double bond is shorter and stronger than a single bond
a triple bond is shorter and stronger than a double bond
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Cl2
nonpolar bond – electrons are shared equally in the bond
polar bond – electrons are NOT shared equally
HCl
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Linus Pauling 1901 – 1994
electronegativity – the ability of an element to attract electron density to itself in a molecule
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electronegativity increases from left right
electronegativity decreases from top bottom
electronegativity – the ability of an element to attract electron density to itself in a molecule
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Arrange the following in order of increasing electronegativity: Na, F, O, K, Al, Si, Mg
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Drawing Lewis Structures
1. count the total number of valence electrons2. make an intelligent guess as to the central
element and connectivitya) heavier element is often the central elementb) many molecules are symmetric
3. Add electron pairs to satisfy octet rule4. start making multiple bonds (first double, then
triple if single bonds not getting the job done.)5. Do NOT (under any circumstance…..ever) form a
multiple bond to a halogen or hydrogen
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Draw the Lewis structure for F2
bonding pair of e- – e- that hold two atoms (bonding pair) together
nonbonding pair of e- – e- that are NOT holding (lone pair) 2 atoms together
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Draw the Lewis structure for H2O
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Draw the Lewis structure for ethene, C2H4
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Draw the Lewis structure for PO43-
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Draw the Lewis structure for NO+
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Draw the Lewis structure for PF5
octet expansion – some atoms can exceed8 valence electrons(usually P & S)
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Draw the Lewis structure for BCl3
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Resonance – the “real” molecule can NOT be described by a single Lewis structure
Consider NO2-
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Barium + Cobalt + Nitrogen
Ba2+ + Co+ + N3 BaCoN
The only ionic compound you ever really need !!
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Determine the Lewis structure for NO2-
What are your bond expectations for nitrite ?
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A single Lewis structure can NOT be drawn to describe the “real” nitrite species
go to lab and measure the actual bond lengths in a real nitrite anion
The N-O bonds in nitrite are identical (in every sense; same length; same strength)
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The Real molecule is somewhere in between these two extremes