CHEMISTRY SHENANIGANS

- there are more carbon compounds than all ionic compounds combined
- the study of carbon compounds is organic chem
- carbon can have multiple bonds and form many different shapes

Hydrocarbons have 3 types of formulas:
- molecular formulas (C6H14)
- condensed structural formula (CH3-CH2-CH2-CH2-CH2-CH3)
- structural formula


Nomenclature of Hydrocarbons
- One molecular formula can have a number of different structures
- Isomers are compounds that can be drawn in more than one way

How to name alkanes
1) Add "ane" to the longest chain with the correct suffix
2) Locate any branches by number carbon atoms (with the lowest numer)
3) Name branches with the appropriate suffix and -yl ending (Alkyl branches)
4) If there are more than one of the same alkyl group, number each one and add the multiplier number in front of the branch name

- the formation of a solution depends onthe ability of the solute to dissolve in the solvent
-solvation is the interaction btw solutes and solvents
-ionic solids (salts) are crystals made up of ions
-molecular solids are cystals made up of neutral molecules
-dissolving ionic solutions produces ions in a process called dissociation
-ionization is the break up of a neutral molecutle into charged particles

EX. CH3COOH--->CH3COO- + H+

-Determining concentrations is relatively easy

EX. What is the [Cl-] in a solution of 0.50M AgCl3
1)AgCl3--->Ag+ + 3Cl-
2)0.50 x 3 = 1.50M

- solvents and solutues can be polar or non-polar
- non-polar substances have equal charge distribution
- polar substances have unequal charge distribution
- in simpler terms, polarity depends on the symmetry of the structural diagram

Practice Questions: Determine whether each is polar or non-polar.
SiF4
SF4
PCl5
H2O
XeF4

Answers:
Non-polar
Polar
Non-polar
Polar
Non-Polar

Definition: bonds between molecules, there are 3 types

1. London Dispersion Force (L.D.F.)
- results from temporary electron diploes
- weakest intermolecular force
- increases as the number of electrons increases
- occurs in any compound that has electrons (aka EVERYTHING)

2. Dipole-Dipole Force
- results from a permanent dipole in molecules
- polar molecules experience this force
- polarity depends how much elements want electrons (electronegativity)
- the strength of the bond depends on the difference in electronegativity between the two atoms

3. Hydrogen Bonds (H-Bonds)
- this is a special type of dipole-dipole bond between H and O, F, or N.



Looking for a bit more information? Check out this site!

Want some practice? Check out this quiz!

- electrical condcution in solutions requires charged ions to be present
- ionic slutions dissociate when placed in water
NaCl(s)--H2O--> Na+(aq) + Cl-(aq)
- molecular solutions do not usually split into ions
C12H22O11(s)--H2O--> C12H22O11(aq)

Follow these steps to determine conductivity:
Is it a metal?
If yes, then its conductive. If no, is it a solid non-metal? If yes, then its non-conductive. If no, is it an acid or base? If yes, then its conductive. If no, is it ionic? If yes, then its conductive and if it's no, then its non-conductive.

Today's class was all about reviewing for the test on Friday. We were given an atomic theories review sheet and had to answer as many questions as possible and then check them over in class. As well, Mr. Doktor reminded us what we would need to know for the test:

1) Dalton, Thomson, Rutherford, Bohr models
2) Bohr energy level diagrams
3) The differences between ions, atoms, isotopes
4) Atomic Structure (atomic number, atomic mass, number of electrons, etc)
5) Trends on the Periodic Table (mass, charge, ionization energy, size, reactivity)
6) Metals, non-metals, metalloid properties
7) Lewis dot diagrams
8) Structural diagrams

G'luck!

In today's class, we separated ourselves into groups and used a conductivity sensor to determine the conductivity of 9 substances.

Here are my results:

SOLUTION | CONDUCTIVITY | IONIC OR MOLECULAR? | ACID OR BASE?
Acetic Acid | 1518μs/cm | molecular | acid
Hydrochloric Acid | 16650μs/cm | molecular | acid
Hydrogen Sulfate | 32350μs/cm | ionic | acid
Copper Chloric Acid | 4156μs/cm | ionic | acid
Sodium Chloride | 4167μs/cm | ionic | base
Ammonia | 1500μs/cm | molecular | base
Sodium Hydroxide | 3300μs/cm | ionic | base
Sucrose | 0μs/cm | molecular | acid
Ethyl Alcohol | 0μs/cm | molecular | base

Take a look at this video about conductivity and pH: