Ketones

Few things to remember when finding out a Ketone

1. There is a double bonded oxygen that is NOT on either end meaning that the double bonded O will not be bonded to the last CH it will bonded to a CH in the middle. 
2. A ketone will have a one ending 

Halides

Few steps to naming a Halide and knowing which compound is a Halide:

1. Same nomenclature 
2. Still use di, tri, tetra and so on. 
3. The endings for each of the Halides will still be the same, such as ane, ene, or yne. Depending on what kind of compound you get. 
4. Cl will not be chlorine but will be changed to chloro
5. Br will not be bromine but will be changed to bromo
6. I will not iodine but will be changed to iodo
7. Prefixes will also be the same as well 

Alcohols

3 important rules in naming Alcohols 

1. Same nomenclature 
2. Ends in ol   instead of ending in ane, ene, or yne
3. An alcohol is a hydrocarbon with a OH bonded to it 

You will know if this is an alcohol if you see that it is bonded to an OH, this is a big hint on naming compounds. 
The following compounds below are methanol and ethanol. 

Organic Chemistry

Organic Chemistry is the study of carbon compounds. Carbon can form multiple covalent bonds such as chains, rings, or bracelets. There are less than 100,000 non-organic compounds while, organic compounds number more than 17,000,000. The simplest organic compounds are made of carbon and hydrogen.
Ex.

CHCCH3

CH3CH3

CH4

Saturated compounds have no double or triple bonds. Compounds with only single bonds are called Alkanes and always end in -ane.

Nomenclature (naming)
There are 3 forms of bonds in Organic Chemistry:
Straight chains, Cyclic chains, and Aromatics

1) Straight chains
To name Straight chains:

• Circle the longest continuous chain and name this as the base chain.

The base chain can either be the red or green from the drawing above because both chains are in equal length.

• Number the base chain so side chains can have the lowest possible numbers

• Name each side chain using the suffix -yl

"Meth" has 1 so theres a methyl, and "eth" has 2  so it's ethyl

• Give each side chain the "appropriate number" ( if there is more than 1 identical side chain numbers/labels are slightly different: 2 methyl 4 ethyl
• List side chains alphabetically

So the Name for this structure is 4 ethyl 2 methyl hexane

Ion Concentration

DISSOCIATION

• ionic compounds are made up of two parts
• Cation: positively charged particles
• Anion: negatively charged particles
• when ionic compounds are dissolved in water, the cation and anion separate from each other
• this process is called dissociation
• when writing dissociation equation, the atoms and charges must balance.
• the dissociation of sodium chloride is:

NaCl -> Na+ + Cl-

• if the volume does not change then the concentration of individual ions depends on the ba;anced coefficient in the dissociation

ex. Determine the [Na+] and [PO4 3-] in a 1.5 M solution of Na3PO4

Na3PO4 -> 3Na+ + PO4 3-

1.5 M = [PO4 3-]

1.5 x 3 = 4.5 M = [Na+] 

Dilution

DILUTION SOLUTIONS

• when two solutions are mixed, the concentration changes
• dilution is the process of decreasing the concentration by adding a solvent (usually water)
• the amount of solute does not change

• because concentration is mol/L, we can write:

C = n/V                C1V1 = C2V2

n = CV

ex. determine the concentration when 100 ml of 0.10 M HCl is diluted to a final volume of 400 mL.

V1 = 100mL

C1 = 0.10 M

V2 = 400 mL

C2 = ?

C1V1 = C2V2

(0.1)(100) = C2(400)

C2 = 0.025 M

ex. how much water must be added to 10.0 mL of 10.0 M Na2SO4 to give a solution with a concentration of 0.50 M?

V1 = 10.0 mL

C1 = 0.1 M

V2 = ?

C2 = 0.50 M

C1V1 = C2V2                                  ΔV = 200 - 10 = +190 mL

(10.0)(10.0) = (0.5)V2

V2 = 200 mL

Bonds and Electronegativity

There are 3 types of bonds:

Ionic.
Covalent.
Metallic.

Ionic bonds are when electrons are transfered from metal to non-metal. Covalent bonds are when electrons are transfered between non-metals. Metallic bonds are when pure metals are held together by electronegativity attraction.

electronegativity - (EN) is a measure of an atoms attractions for electrons in a bond

1. Atoms with a greater EN can attract more e- 
2. polar convalent bonds form from an unequal sharing
3. non-polar covalent bonds form from an equal sharing

Electronegativity has a specific rule for each elements.

• EN > 1.7 = ionic bond
• EN < 1.7 = polar covalent bond
• EN = 0 = non-polar convalent bond

Example:

1. Ba-I
   0.89-2.66
   1.77 = ionic bond
2. Co-P
   1.88-2.19
   0.31 = polar covalent bond
3. Hg-Po
   2.0-2.0
   0 = non-polar convalent bon