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6.1 Introduction to Chemical Bonding
Ch. 6 Bonding 6.1 Introduction to Chemical Bonding
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Chemical Bonds atoms rarely exist alone
when atoms are bonded together, they have less potential energy and are more stable chemical bond – mutual electrical attraction between the nuclei and valence electrons of different atoms that binds the atoms together
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Ionic Bonds results from electrical attraction between large numbers of cations and anions atoms donate or accept electrons from each other
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Covalent Bonds results from sharing of electron pairs between two atoms the electrons shared belong to both atoms
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Covalent Bonds when electrons are shared unevenly Polar Covalent
Nonpolar Covalent when electrons are shared evenly
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Ionic vs. Covalent
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Ionic vs. Covalent bonding usually does not fall in one category or the other, but somewhere in between type of bond depends on the elements differences in electronegativities 0.3
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Ionic vs. Covalent Difference in electronegativites
Percent Ionic Character Ionic > 1.7 > 50 % Polar Covalent 0.3 – 1.7 5 – 50 % Nonpolar Covalent 0 – 0.3 0 – 5 %
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Polarity Polar- uneven distribution of charge
Show partial charges on structure by using (lowercase delta)
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Practice Determine whether each of the following bonds will be:
ionic, polar covalent, OR nonpolar covalent
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Practice S and H 2.5-2.1=0.4 polar covalent S and Cs 2.5-0.7=1.8 ionic
Cl and C =0.5
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Practice Cl and Ca 3.0-1.0=2.0 ionic Cl and O 3.5-3.0=0.5
polar covalent Cl and Br =0.2 nonpolar covalent
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Patterns What kind of patterns do you see? metals + nonmetals = ionic
nonmetals + nonmetals = covalent
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