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

 

Inter-molecular Bonds

-Inter-molecular bonds exist within a molecule such as the ionic and covalent bonds
-Inter-molecular bonds exist between molecules

• If the inter-molecular is stronger it gives you a higher a BP or MP 
• There are two types of inter-molecular bonds such as Van Der Waals bonds and Hydrogen Bonds
• They are based on electron distribution 
• And two categories 

1. Dipole- Dipole Bonds
-If a molecule is POLAR the positive end of one molecule will be attracted to the negative end of another molecule (One must be negative and one must be positive)

2. London Dispersion Forces (LDF) (Count the # of electrons)
-LDF is present in all molecules
-they create the weakest bonds
-If any substance is NON-POLAR you do not need to check if the substance is Dipole Dipole because it will not exist.
-electrons are free to move around and will randomly be grouped on one side of the molecule
-this can create a temporary dipole and can cause a weak bond to form
-the more electrons in the molecule the stronger the LDF can be

3. Hydrogen Bonding
-If hydrogen is bonded to a certain element such as Flourine, Oxygen or Nitrogen the bond is highly polar
-This forms a very strong intermolecular bond