Alkenes and Alkynes? Really now? Do Intelligent Chemists Really Not Know How to Make Up More Exciting Names?

Alkenes, Alkynes, who cares? They're the same thing.

WRONG.

Even though they both form bonds that contain fewer Hydrogen atoms attached to Carbon atoms, THEY ARE VERY DIFFERENT!
Naming these compounds are relatively easy, as they follow the same rules as naming Alkanes. Just remember to change the ENDING to the appropriate one!

Let's start with Alkenes.

Alkenes-->contain one or more double bonds
-->classified as unsaturated hydrocarbons
-->CHANGE ENDING TO "-ENE"

eg. CH3-CH2-C=CH-CH3
                               |
                             CH3-CH3-CH3
            
                 2-propyl-2-pentene

*notice how the ending of the parent chain changed

Alkenes have a many possible structures (same), BUT have different geometrical shape
-->this is special to ONLY ALKENES called geometric insomers

Geometric insomers-->occur when double bond is formed, having side chains attached (top & bottom)
-->2 types:
                  -trans: (top&bottom, bottom&top)
                  -cis: same side (top&top, bottom&bottom)


So, practice what you've learned!
Draw these structures:

4-methyl-2-pentene
3-propyl-2-heptene

Now, for the Alkynes!
Alkynes-->contain one or more triple bonds (yes, now you use 3 LINES!!)
-->also unsaturated hydrocarbons
-->naming rules are still the same, but CHANGE ENDINGS to "-YNE"


 eg. CH3-CH-CH3-C(insert triple bond here)C-CH3
        |         |
       C    CH3
  
                   5,6-methyl-2-heptyne


It's simple...REALLY!


Make sure you do some extra practice from the textbook!!
Memorize all the prefixes (it'll help)!




Jialynn.

Organic Chemistry - May 26, 2011 - Isabelle Cheng

Isabelle Cheng

Block 2-2

Chemistry 11 Ms. Chen

Organic Chemistry

What is organic chemistry anyway?.....

Organic Chemistry:

introduction to the diverse chemistry of carbon

scientific study of the structure of carbon-based compounds and hydrocarbon

can vary from small to large

has a specific naming system 

different kinds of structures to represent a molecular formula

form chains of carbon atoms

Properties:

A carbon that has 4 bonds

A carbon atom that has 4 hydrogen atoms

A carbon-carbon bond

Branched Chain

Rings

Naming:

There are certain names for each molecular formula!

1 - meth

2 - eth

3 - prop

4 - but

5 - pent

6 - hex

7 - hept

8 - oct

9 - non

10 - dec 

You use these prefixes in the beginning and the endings for alkanes is “-ane.”

The formula is CnH2n+2, if you plug in the numbers and it doesn’t work then that means that it is not from the alkane group!

When looking at the structures: Always look at the longest chain and write the molecular formula from there!

For example:

It is called Propane because there are three of the longest chain. 

For the Alkayl group, they have a different formula and different naming system:

The ending is “-yl,” so an example would be methyl. 

For example:

This structure is called 3-methyl-pentane because the bond is on the third position and it is called methyl because it is from the alkyl group. It is called pentane because the longest chain has 5 of them. 

Extra facts: The sum of all valence e- of each atom in the molecular formula must equal the number of electrons in your Lewis Dot Structure.

Except for a few elements, ex. H, most elements want a full valence shell. 

chemical bonding (by: mandy)

                                                         CHEMICAL BONDING
There are 3 types of chemical bondings: Ionic Bonding, Nonpolor Covalent Bonding, and Polar Covalent Bonding.
Nonpolor Covalent Bonding: electrons are shared equally
Polar Covalent Bonding: electrons are shared unequally
Ionic Bonding: electrons are transferred between two atoms

Electrostatic Force
Electronegativity: the measure of the ability of an atom to attract electron from other atoms.
Metals have LOW electronegativity
Non-metals have HIGH electronegativity
*The greater the difference of electronegativity, it is more likely to be Ionic Bond
      
           ENeg Diff. = | ENeg1- ENeg2 |

ENeg Diff. <0.5 (non-polar covalent)
ENeg Diff. 0.5 to 1.8 (polar covalent)
ENeg Diff. >1.8 (ionic)

London Forces

Polar Covalent Bonds

A molecule is polar if there is an imbalance with electrical charge. [This is called: Polarity]

Atoms with higher electronegativity (delta -)
Atoms with lower electronegativity (delta +)

For example:

Hydrogen has an electronegativity of 2.1
Oxygen has an electronegativity of 3.5
therefore, O, with the higher electronegativity is labelled delta- and two H are labelled delta+

Arrow should be pointing at the negative atom.

study hard!



Electron Dots and Lewis Structures - Isabelle Cheng

Isabelle Cheng

Block 2-2

Chem 11 Ms. Chen

The Lewis Structure involves using dots. It is very simple and easy to understand!

Here are some examples!

Number of Valence Electrons	1		2		3	4	5	6	7	8
Example	Hydrogen	Group I (Alkali metals)	Helium	Group II (alkali earth metals)	Group III	Group IV	Group V	Group VI	Group VII (Halogens)	Group VIII except Helium (Noble Gases)
Lewis Structure (electron dot diagram)

That is what Lewis structures look like and how the dots are formed with the symbol in the middle to identify which element it is. The purpose of the Lewis Structure is that it shows the valence electrons that are distributed in a molecule. Also there is a rule called the octet rule which is saying that most of the atoms want the electrons to form covalent bonds. This rule does not necessarily apply to all of the atoms. 

Here is an example of H20!

Here are some practice ones!

    H

              ● ●

NH4 + = H   ●     N ●    H

        ●  ●

  ● ●

                  H

The first step is to first draw 4 H’s because the element is H4.

Then you write a N in the middle with the surrounding H’s because it is the only element and it only has one. 

The third step is to then daw two dots for every H surrounding the N. 

You apply the same rules and the same procedure for the other elements.

Then that helps you get the Lewis Structure! 

Periodic Table Familes and Trends.

#trending, teehee.


Who knew the periodic table created trends?
They're such fashionistas!

That was just for laughs...

ANYWAY, here's a video that explains everything. (:
Enjoy.