1. Chemical Bonding

2. Ionic Bonds Transfer of electrons from the metal to the nonmetal
Electrical attraction between large numbers of cations and anions. “clusters”
Cation = Positively charged particle
Typically metals
Loves to give electrons away
Low Ionization Energy & Electronegativity
Most metallic element = Francium

3. Ionic Bonds (cont.) Anion = Negatively charged particle
Typically nonmetals.
Loves to accept electrons
Higher Ionization Energy
Higher Electronegativity
Most nonmetallic element= Fluorine

4. Ionic Bonds (cont.)

5. Ionic Bonds (cont.) Ionic compounds are strong
Ionic bonds dissociate in water
fall apart into cations and anions.
Will conduct electricity when in water.
These compounds are solids at room temp.

6. Covalent Bonds
Formed when 2 nonmetal atoms share electrons

7. A. Polar Covalent Bonds
Unequal sharing of electrons Cl

8. Electronegativity difference is between> 0.4 – 1.6
Electrons attracted more to the higher EN (electronegative) atom, so density is greater around atom with higher EN value.
Electronegativity difference is between> 0.4 – 1.6
Polar Covalent Bonds
dissolve in water
Don’t fall apart into ions (don’t dissociate)
Little to no conductivity

9. B. Non-polar Covalent Bonds
Equal sharing of electrons Br Br

10. Electrons are shared equally between two atoms.
Electronegativity (EN) difference is
Usually found between diatomic molecules – two of the same atoms (element)
Non-polar covalent bonds
don’t dissolve in water.
No conductivity
Can be gas, liquid, or solid (also true for polar covalent compounds).

11. Metallic Bonds Bond formed between 2 or multiple metal atoms.
Larger outer electron shells- which overlap

12. Metallic Bonds
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.

13. Metallic Bonds

14. p. 12 Intermolecular Bonds
-occurs between 2 different molecules

15. Hydrogen Bonds
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

16. Hydrogen Bond Example:

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

18. Van der Waals Bond Example: