1. Chemical Bonding

2. By the end of this lesson you will be able to:
Name and describe the 3 types of bonds and how they are different
List possible compounds in each and how elements are affected by the bonds they share
Describe how we know these bonds exist. What are properties of the bonds?

3. Ionic Bonds Bond most often between a metal and a nonmetal
Transfer of electrons from the metal to the nonmetal
Electrical attraction between large numbers of cations and anions called clusters
Ion = a charged particle

4. Ionic Bonds Cation = + charged particle Loves to give electrons away
Low Ionization Energy, Electron Affinity & Electronegativity
Typically are metals
Most metallic element = Fr

5. Ionic Bonds (cont.) Anion = - charged particle
Loves to accept electrons
High Ionization Energy, Electron Affinity & Electronegativity
Typically are nonmetals
Most nonmetallic element = F

6. Ionic Bonds (cont.) If a bond is ionic: The compound is solid
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!
-EN values 1.8 up to 4

7. In General
Ionic Bonds are the strongest bonds there are

8. Covalent Bonds Formed when 2 nonmetal atoms share electrons
Can be liquid, solid or gas

9. Polar Covalent Bonds Unequal sharing of electrons
Electrons attracted more to higher E.N. atom
Electronegativity difference range = 0.3 – 1.7 (for polar covalent bonds)
Polar Covalent Bonds dissolve in water
Why?
(Check out page 19 in your packet for EN of water)
The light bulb doesn’t light up.

10. Non-polar Covalent Bonds
Equal sharing of electrons
Electronegativity difference range = 0.0 – <0.3
Usually found between diatomic molecules – two of the same atoms
Non-polar covalent bonds don’t dissolve in water.

11. Metallic Bonds Bond formed between 2 metal atoms.
Excellent electrical conductors in solid state
Electrons are free to move within electron clouds of all metal ions =
Sea of Electrons

12. Metallic Bonds
In metals, p-orbitals and some d-orbitals are completely vacant and overlap each atom.
Electrons are delocalized – they don’t belong to any one atom anymore.

13. Quick Review Ionic bonds are between Answer A) metals and non-metals
B) non-metals
C) metals
Answer A) metals and non-metals

14. Quick Review Covalent bonds are between Answer B) non-metals
A) metals and non-metals
B) non-metals
C) metals
Answer B) non-metals

15. Quick Review Metallic bonds are between Answer C) metals
A) metals and non-metals
B) non-metals
C) metals
Answer C) metals

16. Quick Review The strongest bonds are between
A) metals and non-metals
B) non-metals
C) metals
Answer A) metals and non-metals (ionic)

17. Quick Review Ionic bonds at room temperature are Answer A) solid
B) liquid
C) gas
D) any
Answer A) solid
Can you name some?

18. Quick Review Covalent bonds at room temperature are Answer D) any
A) solid
B) liquid
C) gas
D) any
Answer D) any
Can you name some?
HCl (aq), Bromine (aq), Fluorine (g), Diamond (s)

19. Quick Review Metallic bonds at room temperature are
A) solid
B) liquid
C) gas
D) any
Answer A) solid and B) liquid
What metallic bonds can be liquid at room temperature?
Hg Any ideas why?
Bond strength not enough to make a solid yet strong enough to keep it from being a gas.

20. Quick Review Which bonds dissociate in water (water is polar)?
A) ionic
B) polar covalent
C) nonpolar covalent
D) Metallic
Answer A) ionic