1 Electronegativity? The ability of an atom in a molecule to attract shared electrons to itself. The ability of an atom in a molecule to attract shared.

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Presentation transcript:

1 Electronegativity? The ability of an atom in a molecule to attract shared electrons to itself. The ability of an atom in a molecule to attract shared electrons to itself. Linus Pauling

2 Table of Electronegativities

3 l Electronegativity differences determine bond type. –0 – 0.4 = nonpolar Covalent bond –0.5 – 1.7 = polar Covalent bond –> 1.7 = Ionic bond

4 Bond Polarity l Covalent bonding means shared electrons –but, do they share equally? l Electrons are pulled, as in a tug-of- war, between the atoms nuclei –In equal sharing (such as diatomic molecules), the bond that results is called a nonpolar covalent bond

5 Bond Polarity l When two different atoms bond covalently, there is an unequal sharing –the more electronegative atom will have a stronger attraction, and will acquire a slightly negative charge –called a polar covalent bond, or simply polar bond.

6 Bond Polarity l Refer to Handout l Consider HCl H = electronegativity of 2.1 Cl = electronegativity of 3.0 –the bond is polar –the chlorine acquires a slight negative charge, and the hydrogen a slight positive charge

7 Bond Polarity l Only partial charges, much less than a true 1+ or 1- as in ionic bond l Written as: HCl l the positive and minus signs (with the lower case delta: ) denote partial charges.    and  

8 Bond Polarity l Can also be shown: –the arrow points to the more electronegative atom. HCl

9 Polar molecules l A polar bond tends to make the entire molecule “polar” –areas of “difference” l HCl has polar bonds, thus is a polar molecule. –A molecule that has two poles is called dipole, like HCl

10 Polar molecules l The effect of polar bonds on the polarity of the entire molecule depends on the molecule shape –carbon dioxide has two polar bonds, and is linear = nonpolar molecule!

11 Polar molecules l The effect of polar bonds on the polarity of the entire molecule depends on the molecule shape –water has two polar bonds and a bent shape; the highly electronegative oxygen pulls the e - away from H = very polar!

12 Practice l N 2 l CO 2

13 l HCl l NaBr

14 l NH 3 l CCl 4

15 l CuCl 2 l Fe(NO 3 ) 3