1. Chemical Bonding

2. Covalent Bonds
Formed when 2 atoms share electrons

3. Polar Covalent Bonds Unequal sharing of electrons
Electrons attracted more to atom with the higher electronegativity
Electronegativity difference is between 0.4 – 1.7
Polar Covalent Bonds dissolve in water

4. Polar Covalent Bonds

5. Non-polar Covalent Bonds
Equal sharing of electrons
Electronegativity difference is between basically 0.
Usually found between diatomic molecules – two of the same atoms
Non-polar covalent bonds don’t dissolve in water.

6. Non-polar Covalent Bonds

7. Ionic Bonds
Electrical attraction between large numbers of cations and anions
Ion = a charged particle
Cation = + charged particle
Loves to give electrons away
Low Ionization Energy & Electronegativity
Typically are metals

8. Ionic Bonds (cont.) Anion = - charged particle
Loves to accept electrons
High Ionization Energy & Electronegativity
Typically are nonmetals
Electronegativity difference >1.7

9. Ionic Bonds (cont.)

10. Ionic Bonds (cont.) If a bond is ionic:
The compound will fall apart (dissociate) into its original ions when dissolved in water
If a conductivity test is performed, the light bulb will…
light!

11. Metallic Bonds Bond formed between multiple metal atoms.
Electrons are free to move within electron clouds of all metal ions =
Sea of Electrons
Electrons are delocalized – they don’t belong to any one atom anymore.

12. Metallic Bonds

13. Hydrogen Bonds Intermolecular – attraction between molecules
One molecule is polar and has Hydrogen in a H-F, H-O or H-N bond
Other molecule has an unshared pair of electrons, usually F, O, N

14. Hydrogen Bond Example:

15. Van der Waals Bonds These bonds are important for Noble Gases
Very weak bonds
Electrons of Noble Gases get shifted to one side causing it to attract a slightly positive atom that is nearby.

16. Van der Waals Bond Example: