Polarity Ch 6.2b.  Diatomic compounds share electrons equally.  Equal forces pulling on the shared electrons  What happens when atoms do NOT share.

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Presentation transcript:

Polarity Ch 6.2b

 Diatomic compounds share electrons equally.  Equal forces pulling on the shared electrons  What happens when atoms do NOT share electrons equally?  Unequal forces pulling on the shared electrons

 Electronegativity = Atom’s attraction for electrons  Larger value  stronger attraction  Electronegativity trends (attraction for electrons):  Right side of periodic table: high  Exception for noble gases (Group #8A) - none  Left side of periodic table: low  Top of a group: higher  Bottom of a group: lower

Polar Covalent Bond :  Determine by electronegativity  Higher electronegativity  partial negative charge  Lower electronegativity  partial positive charge.

 Shared electrons in a hydrogen chloride molecule spend less time near the hydrogen atom than near the chlorine atom.

 Non-polar covalent  Electronegativity difference is <0.5  Polar covalent  Electronegativity difference is >0.5 and <2.0 (Between )  Ionic bond  Electronegativity difference is >2.0

 Boron and Hydrogen  Electronegativities: B = 2.0 H = 2.1  Difference:   Potassium and Iodine:  Electronegativities: K = 0.8 I = 2.7  Difference:   Sodium and Chlorine  Electronegativities: Na = 0.9 Cl = 3.0  Difference: 

 Boron and Hydrogen  Electronegativities: B = 2.0 H = 2.1  Difference: 0.1  non-polar covalent  Potassium and Iodine:  Electronegativities: K = 0.8 I = 2.7  Difference:   Sodium and Chlorine  Electronegativities: Na = 0.9 Cl = 3.0  Difference: 

 Boron and Hydrogen  Electronegativities: B = 2.0 H = 2.1  Difference: 0.1  non-polar covalent  Potassium and Iodine:  Electronegativities: K = 0.8 I = 2.7  Difference: 1.9  polar covalent  Sodium and Chlorine  Electronegativities: Na = 0.9 Cl = 3.0  Difference: 

 Boron and Hydrogen  Electronegativities: B = 2.0 H = 2.1  Difference: 0.1  non-polar covalent  Potassium and Iodine:  Electronegativities: K = 0.8 I = 2.7  Difference: 1.9  polar covalent  Sodium and Chlorine  Electronegativities: Na = 0.9 Cl = 3.0  Difference: 2.1  ionic