Functional Groups- ALCOHOLS AND HALIDES

To spice things up, organic compounds can contain elements other than C & H! These are called functional groups. There are 9 different functional groups- the two we'll be looking at right here are alcohols and halides!

Alcohols
An alcohol is a hydrocarbon with an -OH bonded to it! The same naming rules apply as usual, but the parent chain ending is -ol.

Example

The carbon chain has TWO carbons so we know that there will be eth- as the beginning of the parent chain! And the ending will be -ol, so putting it together, thats ETHANOL!

 Let's try a harder example:

The longest parent chain has 3 carbons, making the prefix prop-
There is a methyl side chain coming from the 2nd carbon, and the OH, making it an alcohol, is also on the 2nd carbon!
That makes this 2 methyl 2 propanol

Also, a note to remember:  When benzene makes alcohol, put an OH anywhere (attached to any carbon) and it will be called "Phenol".

If you want to get to know alcohol a little bit better, you can read this page!
http://www.talktalk.co.uk/reference/encyclopaedia/hutchinson/m0009891.html

Now, on to Halides!
Group 7 elements (F, Cl, Br, I) can bond to a hydrocarbon chain as well! Naming follows the exact same rules, except that you add the prefix floro- , chloro-, bromo-, and iodo- accordingly


Some examples:

Ignore the one on the left!
So for the middle one, there is a chloro from the second carbon in the propane chain, so it will be called 2 chloro propane!|
For the one on the right, there is an iodine on the second one, and there is also a methyl. This makes it 2 iodo 2 methyl propane!

A last, more complicated example:

Outdated- MULTIPLE DOUBLE BONDS

Alrighty, this and the next few posts are a bit outdated, but its better late than never! Now we'll have all of our posts!


So, lets learn about multiple double bonds!
This happens when there is more than one double bond in a molecule. Just use the same multiplier that you've been using as a prefix for side chains, except put it in the name of the molecule!
For example:

Let's start as we always do, looking at the base chain. There are 8 carbons, and there is a double bond after 1, 3, 5, 7. So now lets name it:
1, 3, 5, 7 octatetraene
note that there is a TETRA in there, because there are FOUR double bonds!
and REMEMBER to change the ending to 'ene' for a double bond!
A lot simpler than you thought, right?

BUBBLE BUBBLE TOIL AND TROUBLE!

The Final Lab!

The final lab of the year was an esterfication lab, with absolutely no questions to do!
The task which Grace and I were presented with was trying to make a wintergreen scent, and I say try because we tried and failed. However the experiment didn't work out because of our own error, it was because of the extremely limited class time.
So in order to make the wintergreen smell you just need to use some of that methyl alcohol and salicylic acid that you had lying around in the back of your pantry.
First you put a scoop of Salicyliic acid to to the test tube then combine 15 drops/1 squirt of methanol and 204 drops of sulphuric acid, mix well.
Soak the the test tube in hot water for 15 min, then transfer the test tube to a prepared container of iced water.
After your test tube has sat there for the allotted time waft the wintry smell of your esterfication.

Hopefully your home experiment will work better than ours.
Okay, our lab wasn't that bad.

Esters!!!!!!!

YAY this is our second last blog and the last blog that has new material! On the other hand.............Chem 11 is almost over :(

So Esters are really cool because they create smells like orange, spearmint, ect. We will be making esters next class, through a process called esterfication!

The functional group for Esters looks like this.....



so basically a double bonded oxygen conected to a carbon which is also conected to another oxygen and then a carbon chain on either side.

here are some more examples:



so the chain that is conected to the oxygens forms the stem, with the ending - oate and the second chain goes in front.simple right?

now lets learn how Esters are formed.....

Esters are formed by the reaction of a carboxylic acid and an alcohol. Water is also a byproduct of this reaction.



this picture illustrates how Esters are formed. Ta Da!!!

Here are some fun smelling Esters!

Carboxylic Acids, Ethers, Amines and Amides

Okay so I will give you a brief introduction to each of the topics and then show some example, first off...
Carboxylic Acids [kahr-bok-sil-ic] (now you can pronounce it)
(the R represents a carbon chain)
So for carboxylic acids you use the normal naming system and just add '-oic acid' on to the end
An example of how you would write the name is methanoic acid (the simplest carboxylic acid)

Ethers

Yes, ethers are two carbon chains connected to a Oxygen, a little note- name the smaller side chain first
Once you have named it just add ether onto the end.
Also here is a video if you are still confused, however just watch these parts: 1:02-1:50 then, 5:58-7:13, or you could just watch all of it and risk being even more confused than you were before, your choice.

Amines
Okay, also note that the two hydrogen's can also be carbon chains.
Amines are carbon chains connected to a nitrogen, the ending is -amine (easy to remember)

Amides
These are two possibilities that are both considered Amides. As for the naming just add -amide onto the end.

Time for examples
Name these compounds

Answers: butamine   2,4 diethyl pentamine  diethyl ester    butyl phenly ester   4 propyl pentanoic acid    butanoic acid 4 phenyl

Ketones and Aldehydes

A Ketone is a hydrocarbon chain, double bonded to an oxygen. The catch is that the double bonded oxygen CANNOT  be at the end of a chain, only in the middle.

When dealing with Ketones, we add the ending -one to the stem. Other than that, standard naming rules apply.

The Simplest ketone looks like this:


This is called Propanone (the Rs stand for hydrocarbons).

Ketones can be combined with other things like Alicyclics, Alkenes, Alkynes, and Aromatics.

For now, here are some more Ketones



The next one is Aldehydes!!!!

Aldehydes are just like ketones but the double bonded oxygens are on the end of the chain. To differentiate, we add the ending -al to the stem.

Like this:

this is 3 Methyl 1 Butanal



and this is 3,3, 5 Trimethyl Hexanal

There you  have it short and sweet :)

Alicyclics and Aromatics

Now that you have been thoroughly befuzzeled by double and triple bonds in organic chemistry, lets confuse you even more!!! Todays topics are Alicyclics ( circular bonds) and Aromatics( mostly benzene).


Before we start, lets just go over the three ways that you can draw organic compounds:

1) Complete structural diagrams



These can be rather time and space consuming.....

2) Condensed Structural Diagrams


These are somewhat easier

3) Line Diagrams


These are the most simplistic way of drawing organic compounds


Alicyclics are carbon chains that form loops. When they form the parent chain or the side chain, normal naming rules apply with the addition of the prefix cyclo- .

Lets try some examples:

This is the simplest alicyclic, cyclopropane.



When you have side chains as well, standard naming rules apply but you can start counting anywhere in the ring, provided you end up with the smallest numbers possible. The occasion can also arise that the Alicyclic will be the side chain itself in which case you simply add the cyclo- to the beginning and -yl to the end of the stem.

Now name these three!!!


Aromatics ( Benzene)

Benzene(C6H6) is a unique cyclic hydrocarbon. Benzene looks like this.....



The lines indicate a double bond. Basically because there are 6 carbons and 3 double bonds, each carbon has a 1.5 bond which sounds kind of confusing but it allows Benzene to do some cool things because its electrons are free to roam.

Benzene can be a parent chain ( called Benzene) or a side chain ( called phenyl). 

Pour example:


This woulod be called 1 Methyl Benzene...... or Toulene( theres no reason for this name, its " just what chemists do" quoth Doktor)

But this...



would be 3 Methyl 1 Phenyl Butane

Comprende?

Thats all for today folks.

Alkenes and Alkynes

Okay, so you now know the basics of Organic Chemistry and I'm sure your feeling pretty proud of yourself. Well that ends about now.
Since it wouldn't be any fun to have you think this is easy I'm going to throw a curve ball and make it harder for you. Aren't I nice
So you've figured out how to identify butane and methane and all those other compounds, but how about 2 butyne.
That is what I will be teaching you today.
 So I know you can identify this, it's 2 2 dimethyl propane, what I want to draw your attention to is those dashes ( - ) connecting the C to the CH₃'s. Those dashes represent a single bond.
And I'm sure your wondering what this has to do with anything, but there organic compounds aren't connected by only single  bonds their also connected by double and triple bonds. Like I said, wouldn't want this to be too easy for you.
Fortunately for you there isn't too much more tor remember when dealing with double and triple bonds,
here's what you have to know:
-ene  =  double bond
-yne  =  triple bond
when numbering the parent chain the double/triple bond takes the lowest number.

Also if there is more than one double/triple bond you put a multiplier in. For example hexatriyne.

And one more extra tidbit if two adjacent Carbons are bonded by double bonds and side chains there are only two possible compounds they could be.
Trans 2 butene or Cis 2 butene

Simple right? (or at least not too difficult)
Now lets try a few examples.
Name the compounds.
(I'll go through the first one with you)

First circle the parent chain

Then number the carbons 1-5 either from left to right or right to left (remember the double bond must have the lowest number)

 You can now name the compound.
The compound is (*drum roll*)
2 ethyl 1 pentene!

Now it's your turn (answers below)
1)

2) (this one doesn't have the Hydrogen's but you should get the idea)

3)

(Answers 1) 3 methyl 1 propyne, 2) 2 methyl 2 pentene, 3) 2 methyl 1 propene )

Happy naming
and of course to finish off a comic
(by the way the one asking if they look fat is glucose)

Organic Chemistry

A new unit, woohoo! This is veery interesting so far

Organic chemistry is the study of carbon compounds

-Carbon forms A LOT of covalent bonds (miiiiiiilllions, in fact)

While there are only less than 100 000 non-organic compounds, there are over 17 000 000 organic compounds!

Carbon compounds can form chains, rings or branches. The simplest organic compounds are made of carbon and hydrogen. The simplest is CH4, which is methane. It just has one C, and thus has 4 H's to fill all the bonds of the C.

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

Now, let's learn how to name these! There are three categories of organic compounds:

1) Straight chains

2) Cyclic chains

3) Aromatics

Today we'll do only straight chains!

Some ground rules for naming straight chains:

1) Circle the longest continuous chain and name this as 'the base chain'

2) Number the base chain so side chains have the lowest possible numbers

3) Name each side chain using the -yl ending

4) Give each side chain the appropriate number

5) List side chains alphabetically

This'll all make much more sense through the examples!

Unfortunately, drawing out examples is a bit impossible on here, so I won't be able to show step by step... but I will explain it!

The first thing you would do is circle the longest possible chain (without repeating the same one). In this case, there are a few options, but lets take the simplest one, which is the bottom three (the straight row). This row has THREE and the prefix for three is 'prop' and since it ends in -ane, give it the name propane for now. In this case, numbering it will work either way, because either way the side chain will be number 2. There is only 1 off the side chain, so the prefix before the -yl is 'eth', making it ethyl. You want to remember to number it though, so it's 2 ethyl. That means that the full name is 2 ethyl propane!

Congrats, you've just named your first piece of organic chemistry!

Polar and Non-Polar Molecules

Okay for polar vs. non-polar molecules there is only one really important thing you have to remember. If when drawing a molecular diagram the molecule is symmetrical the molecule is non-polar, therefore if the molecule is unsymmetrical the molecule is polar.

Symmetrical = Non-Polar

Unsymmetrical = Polar

If you still don't understand here is a good video that explains it.

Now you should understand the general idea, now tell me which of the following molecules are polar and which are non- polar. Also using electronegativity figure out which side is partially positive and which side is partially negative (hint: the one with the most electronegativity is partially negative)

1)

2)

3)

  

Answers: 1--polar, the left side is partially negative

               2-- polar, the bottom half is partially negative
               3--non-polar

The reason why non-polar molecules have no partially negative/partially positive side is because the pull of electrons is balanced.

Acid-Base Reactions

This is a relatively simple unit, so there aren't too many notes. Basically
Strong acids dissociate to produce H⁺ ions
Strong bases dissociate to produce OH^-  ions
However, when strong acids and strong bases mix you get HOH and ionic salt

And since you also know that pH is the measure of H ions present in a solution, you also probably know that pOH would be the measure of OH ions in a solution.
Thus
pH = -log[ H⁺ ]
pOH = -log [ OH^- ]

So here's an example to test you knowledge of the new concept while still incorporating past knowledge.

If  .100 L of .40M of HNO₃ is added to .300L of .20M of NaOH
First find the limiting reactant
0.1 x (.40mol)/(1L) x 1/1 x (1L)/(.20mol) = .2 L of NaOH is needed
(since you have .300 L of NaOH)  HNO₃ is the Limiting Reactant

Then find how much NaOH will be left over.
So you find how much NaOH you use, and how much HNO₃ you use.
(.3L) x (.2mol)/(1L) = .06 mol of NaOH used
(.1L) x (.4mol)/(1L) = .04 mol of HNO₃ used
You then subtract the amount of NaOH used from the amount of HNO₃ used
.06-.04 = .02 mol of excess HNO₃

Next find the pH
pH = -log [ H⁺ ]
      =  -log(.02)
pH = 1.7           (there are no units)

Not too difficult, right? Now if you can do a question like that then you fully understand Acid-Base reactions.
And just make sure you remember your significant digits and decimal points