1. Electronegativity What is it? Electronegativity is the power of an atom to attract electrons in a bond

2. Why does this matter? Chemical reactions take place when electrons are shuffled (moved) around between atoms! A chemical bond: the attraction between the electrons shared between atoms and the atoms’ protons. The amount of “shuffling” changes depending on the atoms involved!

3. Elements with a HIGH electronegativity have a STRONG pull on electrons. Elements with a LOW electronegativity have a WEAK pull on electrons.

4. difference in electronegativity When two atoms bond their DIFFERENCE in electronegativity determines the bond type.

5. difference in electronegativity An Ionic Bond: When one atom will win the “tug of war” and take the electrons completely. This comes from a large difference in electonegativities of atoms.

6. A Covalent Bond: When the electronegativity of two bonding atoms is very similar, neither atom wins the “tug of war” and the electrons are shared equally.

7. In a true covalent bond electrons are shared equally

8. IONIC COVALENT Transfer electrons Share electrons Between an atom of high electronegativity and an atom of low electronegativity Between two atoms of equal or very close electronegativities NaCl N 2

9. If the electronegativity difference between two bonded atoms is very high the bond is ionic. If the electronegativity difference is very low the bond is covalent. What if the difference in electronegativity between the two bonded atoms is in-between? Hold on to that question!

10. SO….. Ionic and covalent bonds are very different, but how do we predict if a bond will be ionic or covalent?

11. Electronegativity Pauling’s electronegativity scale The higher the value, the more electronegative the element Fluorine is the most electronegative element It has an electronegativity value of 4.0

12. Electronegativity Pauling’s electronegativity scale

13. Electronegativity

14. Electronegativity F 4.0

15. Electronegativity Pauling’s electronegativity scale Li 1.0 F 4.0

16. Electronegativity Pauling’s electronegativity scale Li 1.0 Be 1.5 F 4.0

17. Electronegativity Pauling’s electronegativity scale Li 1.0 Be 1.5 B 2.0 F 4.0

18. Electronegativity Pauling’s electronegativity scale Li 1.0 Be 1.5 B 2.0 C 2.5 F 4.0

19. Electronegativity Pauling’s electronegativity scale Li 1.0 Be 1.5 B 2.0 C 2.5 N 3.0 F 4.0

20. Electronegativity Pauling’s electronegativity scale Li 1.0 Be 1.5 B 2.0 C 2.5 N 3.0 O 3.5 F 4.0

21. Electronegativity Pauling’s electronegativity scale Li 1.0 Be 1.5 B 2.0 C 2.5 N 3.0 O 3.5 F 4.0 Na 0.9 Mg 1.2 Al 1.5 Si 1.8 P 2.1 S 2.5 Cl 3.0

22. Electronegativity Pauling’s electronegativity scale HHe Li 1.0 Be 1.5 B 2.0 C 2.5 N 3.0 O 3.5 F 4.0 Ne Na 0.9 Mg 1.2 Al 1.5 Si 1.8 P 2.1 S 2.5 Cl 3.0 Ar

23. Electronegativity Pauling’s electronegativity scale H 2.1 He Li 1.0 Be 1.5 B 2.0 C 2.5 N 3.0 O 3.5 F 4.0 Ne Na 0.9 Mg 1.2 Al 1.5 Si 1.8 P 2.1 S 2.5 Cl 3.0 Ar

24. Electronegativity Pauling’s electronegativity scale H 2.1 He - Li 1.0 Be 1.5 B 2.0 C 2.5 N 3.0 O 3.5 F 4.0 Ne - Na 0.9 Mg 1.2 Al 1.5 Si 1.8 P 2.1 S 2.5 Cl 3.0 Ar -

25. That means that the most electronegative elements are in the upper-right corner of the table.

26. With only a few exceptions, electronegativity values increase as you move from left to right in any period of the periodic table. Within any group, electronegativity values decrease as you go down the group.

31. 0 is less than.5, so the bond is a nonpolar covalent bond!

34. .9 is less than 1.7, but above.5, so the bond is a polar covalent bond!

35. Salt crystals are repeating patterns of positive + and negative - ions held together by electrostatic attraction. IONIC COMPOUNDS

36. COVALENT COMPOUNDS Biological molecules are covalently bound Most consist of the non-metals Carbon, Oxygen, Hydrogen, and Nitrogen.