Alkanes, Alkenes, Alkynes & Halides, Nitro, Alcohol, Ketones, Aldehydes--By Nemo Jin

Alkane
--all carbon atoms bonded by single bond
--general form "CaH2a"
--alkyl groups: alkane lost one hydrogen

Alkene & Alkyne
--"ene" double bonded carbon atoms
--"yne" triple bonded carbon atoms
--same naming rules, give double/triple bond the lowest number
--larger groups are diagonal: trans
--larger groups are at either bottom or top: cis

Ex.

 Ex.

Functional Groups
--most reactive part of the molecule
--insoluble in water
--F is less reactive; Cl, Br are the most reactive ones
--NO2: tend to be explosive

           F = fluoro
            I = iodo
          Cl = chloro
          Br = bromo
      NO2 = nitro


Ex.

Alcohol
--using the largest chain containing the OH group
--replacing the "e" ending in parent hydrocarbon chain with "ol"
--give OH the lowest number

general form:

Ketone &Aldehyde

--Aldehyde:

   -double bonded oxygen at the end of main chain

   -change the ending to "al"

--Ketone:

   -double bonded oxygen that's not on either end

   -change the ending to "one"

for more info:

http://www.brooklyn.cuny.edu/bc/ahp/LAD/C4c/C4c_aldehydes.html

Ester, Ether, Carboxylic Acids and Amines - By Sally Chen

Ester
- formed by 
- alcohol + carboxylic acid = ester
- fruity smell
- main chain:  drop "e" add "oate"
- counting starts on the double bonded oxygen end

Ether
- formed by 
- highly flammable
- insoluble in water
- good solvent for organic compounds
- side chain:  drop "e" add "oxy"
- counting starts on the oxygen end


Carboxylic acids
- formed by 
- can be neutralized by a base
- main chain:  drop "e" add "oic acid"
- counting starts on the double bonded oxygen end


Amines
- formed by 
- base
- primary amine = 1 carbon chain
  secondary amine = 2 carbon chain
  tertiary amine = 3 carbon chain
- closely related to NH3
- soluble
- fishy smell
- add "amino" between parent chain and side chain(s)
- counting:  whichever way makes the numbers smaller

I don't know how it just doesn't work out with the "Insert a Video" button, so here:
http://www.youtube.com/watch?v=mAjrnZ-znkY

Electronegativity, Polarity and VSEPR--By Tina Zhao

Electronegativity
- The attraction an atom has for the shared pair of electrons in a chemical bond
- It is the difference in electronegativity between two atoms that determines the degree of electron sharing which occurs between the two atoms
- Electonegativity refers to how much atoms want to gain electrons
- The top right corner of the periodic table has the highest electronegativity.Fluorine is the MOSTelectronegativity element, and the lowest electronegativity value is Francium with a value of 0.7
- If an atom has high Electronegativity value indicates that it readily pull on electrons in  a bond
-If an atom has low Electronegativity value indicates that it doesn't readily pull on electrons within a bond
- Electronectivity increase as you go across a row from left to right, and decrease as you go down a group
- The scale that is most commonly used to messure electronegativity is called the Pauling scalt , this scale range from 0.7 to 4.0
-High electronegativity values have high ionization energy because they strongly attract their valence electron and they are difficult to remove
- If the electronegativity difference < 0.5 it is a COVALENT bond
- If the electonegativity difference greater and equal the 0.5 or less and equal than 1.8 it is A POLAR COVALENT bond

Polarity

- Describes a molecule's electrical balance

- If there is an imbalance with electrical charge, then a molecule is polar

- If the electrical charge is the same strength on all sides of the molecule, then it is nonpolat

Polar Covalent Bonding

- electonegativity difference between 0.3 and 1.6 are considered to be covalent but with unequal sharing of elecreons , because the bond has slightly positive and slightly negative poles that form at each end

- Higher electronegativity will form a PARIAL NEGATIVE charge, and lower electronegativity will form a PARTIAL POSITIVE charge 

- An arrow sigh is usually used to indicate the migration of electons towards the more electronegativity

EX:

For CH3C1, C has a value of 2.5; H has a value of 2.1 and Cl has a value of 3.0.

...................H (2.1)
....................|
H(2.1) --------- C(2.5) ----------- Cl (3.0)
....................|
...................H (2.1)

Between the Hydrogen's and carbon there is a difference of 0.4, and between the carbon and chlorine there is a difference of 0.5.

VSEPR (The Valence Shell Electron Pair Repulsion

- For polyatomic molecules containing 3 or more atoms, one of the atoms is called the central atom to which other atoms are linked.
- The geometry of a molecule depends upon the total number of valence shell electron pairs (bonded or not bonded) present around the central atom and their repulsion due to relative sizes and shapes.
- If the central atom is surrounded by bond pairs only. It gives the symmetrical shape to the molecule.
- If the central atom is surrounded by lone pairs (lp) as well as bond pairs (bp) of then the molecule has a distorted geometry.
- The relative order of repulsion between electron pairs is as follows: lp – lp > lp – bp > bp – bp.
A lone pair is concentrated around the central atom while a bond pair is pulled out between two bonded atoms. As such repulsion becomes greater when a lone pair is involved.

linear molecule :with a 180^o angle 

trigonal planar :with angle of 120

- If the electronegativity difference >1.8 it is an IONIC bond

Chemical Bonding & Electronic Dot Structure -- by Ria Park

Chemical Bonds

Chemical Bonds 

• are formed when the electrons of one atom are attracted by the nucleus if another atom.
• are formed with various degrees of sharing of electrons between two atoms
• COVALENT BOND is formed when the electrons are shared equally between two atoms
• When the electrons of one atom are given away completely to another atom, both a positively charged ion and a negatively charged ion are formed
• The force holding the two ions together is called an IONIC BONDS

Covalent Bond

Ionic Bond

Lewis Structure

• represents valance electrons.
• uses dots to represent electrons, focuses on an atom's valence electrons only.
• The electrons that are in pairs are Lone pairs or Nonbonding electrons.
• These are not used to bond since the orbital they are in already has its full complement if electrons.
• The unpaired electrons are Bonding electrons. They are capable of making one single covalent bond.
• An atom needs to have 2 bonding electrons when we make a double covalent bond.
• To make a triple covalent bond, an atom needs 3 bonding electrons.

Now single covalent bond is forme

Double Bond

Triple Bond

Example of Lewis Structure