1. Bonding

2. Valence Electrons Highest energy electrons (outer shell)
Only s and p block elements contain valence electrons, so how many valence electrons can there be?????
Noble gas=most stable
How many electrons? 8
Octet Rule: 8 valence electron’s are most stable.
Elements will find the easiest route to get 8 electrons (either gain or lose electrons)

3. Lewis Dot structures Lewis Dot Structures/ Structural Formulas
Write the atomic symbol; place the appropriate number of dots around the element to show the valence electrons.
C, K, Cl, Kr
Ionic Compounds
Write the elements that are bonding, place appropriate number of valence dots, use an arrow to show where the electrons get traded, end equation with ions, one complete, one empty element
Example: NaCl, CaBr2

4. Lewis dot structures/covalent cmpd
Covalent Compounds
Lewis Dot: same concept as ionic, but electrons do not transfer
Structural Formulas: place a line in between bonded elements, these lines represent paired electrons, left over dots are unpaired electrons.
Number of bonds:
Single bond: one line, one pair of electrons
Double bond: two lines, two pairs of electrons
Triple Bond: three lines, three pairs of electrons

5. Lewis dot structures/covalent cmpd
Rules of writing Covalent Compounds:
Count valence electrons (add for negative charges, subtract for positive charges)
write skeleton with single bonds already in place
Place remaining valence electrons around elements
make stable octet, increase bond number if needed
E.G.: CO2, N2, CH4
Exceptions:
H, Li satisfied with 2 electrons
Boron family satisfied with 6 electrons (metals)
P, S more than 8 electrons is OK
When one element is satisfied, but partner is not, the satisfied element with donate a pair of electrons to make another bond = Coordinate Covalent Bonds

6. Solids, liquids, and gases
States of matter

7. Kinetic-Molecular Theory
Particles are hard spheres with insignificant volume, mostly empty space, no attractive or repulsive forces
Particles in constant, rapid motion
All collisions are perfectly elastic

8. Solids Particles vibrate about fixed points
Highly organized, dense, and incompressible
Do NOT take shape of container

9. Liquids Particles are in motion and are free to slide past one another
Vibrate and spin as they move
Particles are attracted to each other through intermolecular forces
Holds shape of container
Less dense than a solid
Not enough energy to escape as a gas

10. gases Particles are in constant motion Take shape of container
Less dense than solids or liquids
Forces of attraction are weaker

11. Phase diagram
Pressure
Temperature

12. Triple Point Video

13. Graph of phase change Molecules separating into gas formation
Molecules separating into liquid formation
Boiling Point
Gas
Melting Point
Temperature
Liquid
Solid
Time

15. Bond Polarity

16. Bond polarity
Covalent bonds differ in how bonded atoms share electrons
Electrons are being pulled by both nuclei
Non-polar covalent bond:
Bonds are pulled equally (usually between two like atoms) H2
Polar Covalent Bonds:
Two different atoms bond and electrons are shared unequally
More electronegative atoms will have the stronger electron attraction, will acquire a slightly negative charge (Example)
Less electronegative atom will acquire a slightly positive charge(Example)
Charges are represented by lower case delta  (the atoms charges are less than +1 and -1) (Example)

17. Determining Polar Molecules
A molecule is polar when the atoms do not share electrons equally
This creates a slightly positive charge on one end and slightly negative charge on the other
Look for:
Unshared electrons on the central atom (called lone pairs)
Different atoms surrounding the central atom
Examples: NH3
What about H2O? CH2Cl2

18. Ionic, metallic, and network
Other types of bonds

19. Types of bonds Transfer of electrons
Compound
Description of Bond
Functional Unit (drawing)
Elements Combined
Do They Follow the Octet Rule?
Ionic
Transfer of electrons
Attraction between (+) and (-) Charges Metals lose electrons
Non metals gain electrons
Crystalline structure
Positive attracts to negative (metal to nonmetals)
Draw
Metals (cations)
Non-metals (anions)
Yes, non-metals accepts e- to complete outer shell, metals donate e- to revert back to complete outer shell
Covalent
Sharing of e-
No set structure, molecules near one another
Two or more non-metals bound together
All but Hydrogen
Metal
Metal ions that are surrounded by free-flowing e-
Positive nucleus surrounded by electrons
Two or more metals
No octet, no full energy level

20. Properties of bonds Bond Strength of bond Covalent Properties
Melting/Boiling
Solubility
Conductor of electricity?
Ionic
Strongest
Very stable
Brittle solid
High melting point
Usually high solubility
Good conductors in solution
Weak strong
Easiest to break
Solid, liquid, and gas states
Low melting and boiling point
Low to high solubility
Poor to non-conductors
Metal
Not as strong as ionic, stronger than covalent
Varied stability
Ductile and malleable
Solid, except mercury
Medium melting point
Not soluble
Good conductors of electricity (electrons flow freely)

21. FOrces

22. Forces between Molecules
Intermolecular forces
Attraction between molecules
Weaker than atom bonding
Used to determine physical properties of the molecule (such as state of the molecule solid, liquid, or gas)
Strongest  Weak
Ionic bond  Hydrogen Bonds  dipole Interaction  Van der Waals

23. Van der Waals/London Dispersion
Types of Forces
Van der Waals/London Dispersion
Dipole-dipole
Hydrogen bonds
Strength
Increase strength of forces as electron number increases
Mimic ionic compounds (attracted by charges, but weaker)
Strongest (includes all 3 forces)
Types of Molecules
Any covalent compound with electrons (non-polar)
A force between 2 polar molecules
Force between 2 very polar, hydrogen containing molecules
Description of force
More electrons=stronger the force
Positive atom on one molecule attracts the negative atom of another molecule
Created with O, F, & N ONLY
Examples
Diatomic elements:
Br I N Cl H O F
CH3COCH3
H2O where H of one water is attracted to the O of another water

24. Forces and properties
Physical properties depend on type of bond (ionic or covalent)
The variety in covalent compounds are due to intermolecular forces
Properties
Melting point: only the weak attractions need to be broken.
Boiling Point: break apart molecules of liquid
Solubility: stronger the intermolecular force the harder it is to be soluble.

25. Questions Define the following:
Boiling point
Melting point
Evaporation
How do each of the above relate to the type of bond in a molecule?
What role does intermolecular forces play in the strength of bonds?
Draw Isopropyl Alcohol ((CH3)2CHOH), methanol (CH3OH), acetone (CH3COCH3), and water.
What type of forces are present in each?