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A. Naming and Formula Writing Rules: 1. Find and name the parent chain. 2. Determine the side chains and write their names with the use of the suffix "-yl". 3. Determine the carbon atom where the side chains are connected to. This number should be the lowest possible number when starting from just one direction. 4. Separate numbers with a "," Separate a letter from a number with a "-" 5. If multiple side chains of the same kind are present, use the prefixes "di", "tri", etc. If multiple side chains of different kinds are present, arrange the side chains in alphabetical order. (do not include prefixes in alphabetization.)
 * I. ALKANES**

B. Properties Homologous series are organic compounds with similar chemical properties and shows a gradation of physical properties due to possessing the same functional group.

1. Structural Formula All the members of the same homologous series have the same structural formula.

2.



As it becomes more complex, the boiling point increases.



3. Isomers are each of two or more compounds with the same formula but a different arrangement of atoms in the molecule and different properties. BUTANE: The C4 alkane is called butane, having the molecular formula C4H10. However, their are two constitutional isomers having this formula, so one isomer is called butane and informally, the other is called isobutane.

4. The isomers have less boiling point than the original because less energy is needed to separate them

C. Reactions 1. Combustion is when the carbon compound reacts with oxygen to form carbon dioxide, water and heat. CH 3 -CH 2 -CH 3 + 5 O 2 —— > 3 CO 2 + 4 H 2 O + heat ===Incomplete combustion is when there is not enough oxygen so the reaction produces some carbon monoxide instead of carbon dioxide === CH 3 -CH 2 -CH 3 + 4 O 2 —— > CO 2 + 2 CO + 4 H 2 O + heat

2. When Alkanes react with halogens, they form alkyl halides. Reacting with Alkanes react with chlorine, they form alkyl chlorides.


 * || light ||  ||
 * CH4(//g//) + Cl2(//g//) || [[image:http://chemed.chem.purdue.edu/genchem/topicreview/bp/1organic/graphics/arrowr.gif width="68" height="12" caption=">"]] || CH3Cl(//g//) + HCl(//g//) ||

D. Resources http://www.citycollegiate.com/homologous_seriesXII.htm http://www.docbrown.info/page07/equilibria8c.htm http://dwb4.unl.edu/calculators/activities/bp.html http://research.cm.utexas.edu/nbauld/teach/note4.html#numbers http://www2.chemistry.msu.edu/faculty/reusch/VirtTxtJml/funcrx1.htm http://chemed.chem.purdue.edu/genchem/topicreview/bp/1organic/reaction.html

**ALKENES**

Alkenes like alkanes are pure hydrocarbons made up exclusively of carbon and hydrogen molecules. The single distinguishing feature is that alkenes contain at least one double carbon-carbon bond, whereas alkanes, by definition have only single carbon-carbon bonds.

Alkanes burn readily. When they do burn, carbon dioxide and water are the products. With increasing chain size, alkanes, given the same amount of oxygen, burn less easily, so that more carbon soot (elementary carbon) is formed with increasing chain size. In alkane molecules, all bonds are said to be saturated. For this reason, alkanes are not very reactive. They do tend to form compounds with halogens.
 * Saturated alkanes**

Alkenes are unsaturated compounds of carbon with hydrogen which contain one or two double bonds between atoms of carbon. They burn to form carbon soot and carbon dioxide and water. They are more reactive than alkanes because of the fact that they contain double bonds.
 * Unsaturated alkenes**

You can tell the difference between an alkane and alkene by adding bromine water to the substance and giving the tube a shake. When bromine water is added to an alkane the solution will turn red-brown (the color of bromine water) and stay that way on shaking. Alkenes however will turn red-brown, but then the color disappears on shaking, this is because the bromine has reacted with the alkene.
 * Telling the Difference**

both burn in presence of O2 and gives these products Co2+H2O+ENERGY.
 * Similarities between alkane and alkene**

Sources: [|**http://www.canadaconnects.ca/chemistry/10091/**] ** [] ** ** [] **


 * ORGANIC DERIVATIVES **


 * A. Naming**
 * Alcohol: add (-ol) e.g. Methane --> Methanol (hydroxyl functional group)
 * Aldehydes: add (-al) e.g. Methane --> Methanal (carbonyl functional group)
 * Ketanes: add (-one) e.g. Propane --> Propanone (carbonyl functional group)
 * Carboxylic Acids: add (-oic acid) e.g. Methane --> Methanoic Acid (carboxyl functional group)
 * Alkyl Halides: add the halogen [chloro-, bromo-, fluoro-, iodo-] e.g. Methane --> Iodomethane (halogen functional group)
 * Amines: add (-ylamine) e.g. Methane --> Methylamine (amino functional group)

Alcohol
Alcohols fall into different classes depending on how the -OH group is positioned on the chain of carbon atoms. There are some chemical differences between the various types.
 * The different kinds of alcohols**

In a primary (1°) alcohol, the carbon which carries the -OH group is only attached to one alkyl group.
 * Primary alcohols**



In a secondary (2°) alcohol, the carbon with the -OH group attached is joined directly to **two** alkyl groups, which may be the same or different.
 * Secondary alcohols**



In a tertiary (3°) alcohol, the carbon atom holding the -OH group is attached directly to **three** alkyl groups, which may be any combination of same or different.
 * Tertiary alcohols**



**Boiling Points** The chart shows the boiling points of some simple primary alcohols with up to 4 carbon atoms. They are: 

They are compared with the equivalent alkane (methane tobutane) with the same number of carbon atoms. <span style="font-family: Arial,Helvetica,sans-serif;"> <span style="font-family: Arial,Helvetica,sans-serif;">Notice that:


 * <span style="font-family: Arial,Helvetica,sans-serif;">The boiling point of an alcohol is always much higher than that of the alkane with the same number of carbon atoms.
 * <span style="font-family: Arial,Helvetica,sans-serif;">The boiling points of the alcohols increase as the number of carbon atoms increases.

<span style="font-family: Arial,Helvetica,sans-serif;">The patterns in boiling point reflect the patterns in intermolecular attractions.

<span style="font-family: Arial,Helvetica,sans-serif;">**Solubility of alcohols in water**
<span style="font-family: Arial,Helvetica,sans-serif;">The small alcohols are completely soluble in water. Whatever proportions you mix them in, you will get a single solution. <span style="font-family: Arial,Helvetica,sans-serif;">However, solubility falls as the length of the hydrocarbon chain in the alcohol increases. Once you get to four carbons and beyond, the fall in solubility is noticeable, and you may well end up with two layers in your test tube.