I'm doing an intro to organic chem, and i'm looking at the functional groups of organic compounds. More specifically, I am looking at melting/boiling points. I keep reading that one has a greater m/b pt. than another, but another one has a greater m/b pt. that one but not another... etc..

Anyways, I'm getting quite confused. Could someone rank the following functinonal groups for m/b pts (highest to lowest or something)?
Alkane
Alkene
Alkyne
Halides
Alcohol
Ether
Amine
Aldehydes/Ketones
Carboxylic Acid
Ester
Amide

Frankly, I'm not sure you can generalize with so many functional groups. In some cases it is a matter of polarity and in some cases it's a matter of molar mass. How can one compare CH4 to CH3(CH2)30CH=CH2? Is that difference in mp/bp a matter of one being an alkane and the other an alkene or is it just a matter of molar mass?

Hydrochloric acid can be prepared using the reaction described by the chemical equation: 2 NaCl(s) + H2SO4(l) ----> 2 HCl(g) + Na2 SO4(s). How many grams of HCl can be prepared from 393 g of H2SO4 and 4.00 moles of NaCl?

To rank the functional groups in terms of their melting/boiling points (from highest to lowest), we need to consider various factors such as the strength of intermolecular forces, molecular size, and functional group structure. Here is a ranked list of the functional groups you mentioned:

1. Carboxylic Acid: Carboxylic acids have high melting/boiling points due to the presence of strong hydrogen bonding between the oxygen and hydrogen groups. The carboxylic acid group also increases molecular size, further enhancing intermolecular forces.

2. Amide: Amides also have relatively high melting/boiling points because they can form strong hydrogen bonds between the nitrogen and oxygen atoms. In addition, amides have larger molecular sizes compared to other functional groups.

3. Alcohol: Alcohols have moderately high melting/boiling points due to hydrogen bonding between the oxygen and hydrogen atoms. However, the strength of these intermolecular forces is lower compared to carboxylic acids and amides because the alcohol molecule has only one hydrogen bond donor and acceptor.

4. Amine: Amines have lower melting/boiling points compared to alcohols because they can form weaker hydrogen bonds due to the presence of nitrogen instead of oxygen. However, larger amines with more hydrogen bonding sites may have higher melting/boiling points.

5. Aldehyde/Ketone: Aldehydes and ketones have lower melting/boiling points compared to the previous functional groups. They have polar carbonyl groups but cannot form hydrogen bonds with themselves. Nevertheless, they still experience some dipole-dipole interactions, resulting in higher melting/boiling points compared to nonpolar functional groups.

6. Carboxylic Esters: Esters have lower melting/boiling points than carboxylic acids due to the absence of a hydrogen atom attached to the oxygen atom. Without this hydrogen bonding, intermolecular forces are weaker, resulting in lower melting/boiling points.

7. Ether: Ethers have relatively low melting/boiling points due to their inability to form hydrogen bonds. While ethers exhibit dipole-dipole interactions, they are generally weaker than other functional groups mentioned above.

8. Halides: Halides (compounds containing halogen atoms) have lower melting/boiling points compared to functional groups that can form hydrogen bonds or have polar groups. The strength of intermolecular forces in halides depends on the size and polarity of the halogen atom.

9. Alkyne: Alkynes have lower melting/boiling points compared to other functional groups because they have weaker intermolecular forces. The carbon-carbon triple bond in alkynes results in a relatively nonpolar nature, reducing their melting/boiling points.

10. Alkene: Alkenes generally have lower melting/boiling points compared to functional groups mentioned earlier. While alkenes have more electron density due to the presence of a double bond, they lack the ability to form strong hydrogen bonds or exhibit significant polarity.

11. Alkane: Alkanes have the lowest melting/boiling points compared to the other functional groups listed. They are nonpolar and have weak intermolecular forces, primarily consisting of London dispersion forces. The boiling/melting points generally increase with increasing molecular size and branching.