1. Warmup: Think back to the structure of the atom and draw a Carbon atom
Warmup: Think back to the structure of the atom and draw a Carbon atom. How many valence electrons does carbon have?

2. Chapter 18 Chemical Bonding

3. 18-1 - Stability in Bonding
Combined Elements
Elements combine to form compounds
Compounds have properties very different from original elements
Compounds have chemical formulas to show the atoms and ratios that make them up.

4. 18-1 - Stability in Bonding
Chemical Formula Practice

5. 18-1 - Stability in Bonding
Unfilled & filled energy shells
Filling Outer energy shells
Valence electrons
Gain/lose electrons
Share electrons
Forming chemical bonds

6. An Atomic Model is Needed to Understand How Atoms Bond
Review shell model of atom (Ch 16)
Valence electrons –
Electron Dot Diagrams –
Tells valence electrons
How many (ve) are paired

7. Electron Shells K= L= M=
N =
O =
P =
Q =

8. 18-2 - Types of Bonds Atoms are electrically neutral
Why?
Ions are not electrically neutral
Ion –
Can be negative or positive
Atoms tend to lose or gain electrons so they end up with an outermost occupied shell that is filled to capacity
The Periodic table can be used to determine the type of ion that an atom tends to form

9. Types of Bonds
Positive Ion (cation)
Negative Ion (anion)

10. Ionic Bonds Result from an Transfer of Valence Electrons
Result of transfer of electrons forms a positive ion and a negative ion
Ionic Bond –
Ionic Compounds –
Characteristics of Ionic Bonds –

11. Types of Bonds

12. Ionic Bonds: One big greedy thief dog
Ionic Bonds: One big greedy thief dog! Ionic bonding can be best imagined as one big greedy dog steeling the other dog's bone.  If the bone represents the electron that is up for grabs, then when the big dog gains an electron he becomes negatively charged and the little dog who lost the electron becomes positively charged.  The two ions (that's where the name ionic comes from) are attracted very strongly to each other as a result of the opposite charges.

13. Types of Bonds

14. Covalent Bonds Result from a Sharing of Valence Electrons
Covalent Compound –
Molecule –
Characteristics of Covalent Bonds –
Can be single, double, or triple

16. Covalent Bonds: Dogs of equal strength
Covalent Bonds: Dogs of equal strength. Covalent bonds can be thought of as two or more dogs with equal attraction to the bones.  Since the dogs (atoms) are identical, then the dogs share the pairs of available bones evenly.  Since one dog does not have more of the bone than the other dog, the charge is evenly distributed among both dogs.  The molecule is not "polar" meaning one side does not have more charge than the other.

17. Polar Covalent Bonds Result from an Uneven Sharing or Electrons
Dipole –
Electronegativity –
Difference in electronegativity
Nonpolar Bond –
Polar Bond -

19. Polar Covalent Bonds: Unevenly matched but willing to share
Polar Covalent Bonds: Unevenly matched but willing to share. These bonds can be thought of as two or more dogs that have different desire for bones.  The bigger dog has more strength to possess a larger portion of the bones.  Sharing still takes place but is an uneven sharing.  In the case of the atoms, the electrons spend more time on the end of the molecule near the atom with the greater electronegativity (desire for the electron) making it seem more negative and the other end of the molecule seem more positive.

21. Molecular Polarity Results from an Uneven Distribution of Electrons
Polar and nonpolar are easy when 2 atoms, more complex when more than 2 atoms are bonded
End result may be a even distribution or an uneven distribution
Can make the dipole stronger
Explains why water is “sticky”
May explain other macroscopic properties

22. This molecular polarity causes water to be a powerful solvent and is responsible for its strong surface tension. The molecular arrangement taken by ice (the solid form of the water molecule) leads to an increase in volume and a decrease in density. Expansion of the water molecule at freezing allows ice to float on top of liquid water.