1. Chapter 6 – Chemical Bonds
Unit 9
Chapter 6 – Chemical Bonds

2. Some elements combine chemically and no longer have the same properties they did before forming a compound.
Atoms form compounds when the compound is more stable than the separate atoms.

3. Stability in Bonding
Noble gases are more chemically stable than other elements because they have a complete outer energy level.
Elements that do not have full outer energy levels are more stable in compounds.

4. A chemical bond is the force that holds atoms together in a compound.
Atoms can lose, gain, or share electrons to get a stable outer energy level.
A chemical bond is the force that holds atoms together in a compound.

5. Bonds
Atoms bond when their valence electrons interact.
Remember – everyone wants to be happy like the noble gases.

6. Shows each valence electron as a single dot. Examples:
Lewis Dot Diagrams
Shows each valence electron as a single dot.
Examples:
Fluorine
Carbon
Sodium

7. Connecting the dots
You can show how the two elements will combine using the dots. Cl

8. There are three types of atomic bonds:
Ionic
Covalent
Metallic
I did not say
atomic bombs

9. Bonds ionic bonds Between a metal and a non-metal.
The metal loses it’s electrons and the non-metal
takes the electron
from the metal.

10. Ionic Bonds

11. The two non-metals share electrons.
Bonds cont.
covalent bonds
Two non-metals
The two non-metals share electrons.

12. bonds cont.
metallic bonds – positively charged metal ions are surrounded by a cloud of electrons, the outer energy level held loosely so the electrons can flow easily between the ions. These metals conduct electricity because the outer electrons can easily move around.

13. Ionic Bonds
When an atom gains or loses an electron it becomes charged (no longer neutral) this is called ionization.
An ion is a charged
atom.

14. oppositely charged ions
Metals become positively charged when they give away valence electrons
Non-metals become negatively charged when they gain valence electrons.

15. Anion Cation Positive ion Made when an atom loses an electron.
Negative ion
Made when
an atom gains
an electron.
Protons = 3
Electrons =
Protons = 9
Electrons = 3 2 10 9

16. Formed between two non-metals. Is the sharing of electrons
Covalent Bonds
Formed between two non-metals.
Is the sharing of electrons
Neither atom gives up valence electrons, they share them.

17. Covalent bonds form molecules.
Atoms may share more than one pair of electrons.
Atoms do not always share electrons equally.
Polar and non-polar molecules

19. Polyatomic Ions
Compounds with both ionic and covalent bonds.
Acts the same as any other ion.

20. Examples: Polyatomic Ions Ammonium NH4+ Hydroxide OH- Sulfate SO4+2
Carbonate CO3-2
Calcium Carbonate CaCO3

21. Naming Binary Compounds
Coming Soon
Naming Binary Compounds