What kind of structure does each have? ((Chemical Bonding))?

Question

I need to know the structure of methanol, butane && glucose. Such as a straight chain, a ring or a branch chain.
Also I need to compare && contrast methanol, butane && glucose. Which means to find their similiaraties between all && how they are different.
PLEASE HURRY, my project is due fairly soon.
&& don't get any info. wrong :D

Answer 1

Look up methanol, butane and glucose on this site from th university of Akron. http://ull.chemistry.uakron.edu/erd/. You will find the structure and physical properties to compare them.

Answer 2

This is a very good, but very complex question. When you learn chemistry, they start with a very simple model of atomic and moleculat structure. This model works for many situations, but does not for most. They will continue to teach you more and different models, each model works to a limited degree, and then stops working. In short, chemistry involves alot of broken models. Part of the skill of a chemist is knowing when to use which model. The answer to this question lies in the last model you will probably learn. Consider the orbitals of the valence e- for carbon you have a 2s and a 2p orbital the 2s is full with two e- the 2p is partly full with another two e- in chemical bonding, all the bonding e- have the same energy level. the 2p orbital is higher energy than 2s. you can see the problem here... The theory is that the s and p orbitals join together to form a hybrid orbital where all the e- have the same energy level. now step back to the octet rule, an atom is happiest when it has 8 e- in orbit. Each orbital can hold two e-. So you have a maximum of 4 orbitals. These orbital are shapped like bowling pins, the atom is in the center, and the 4 orbitals project outward. Picture a pyrimid with a three sided based (tetrahedron) with the atom at the center, and the orbitals pointing into the corners. so, two C atoms come together and one hybrid orbital from each will mesh together forming what is called a sigma bond. This is a single bond, and leaves three unpaired e- remaining in each C atom. Now imagine one of the remaining orbitals from each atom bending over to the other atom to form another meshed orbital. This is called a pi bond, and it sort of morphs into a tube like shape above and below the sigma bond. This is a double bond Now do the same thing with another remaining orbital. This will morph into a tube like shape on either side of the sigma bond. You now have a triple bond. You have a two carbon atoms with triple bonds between them, and each has a lone e- remaining, these compounds are called alkynes. Add an H to each one and you have Ethyne. Now to answer your original question, the reason that a quadrupal bond will not form is because the two pi bonds that surround the sigma bond in triple bonding use up all the space. There is no space remaining to add another bond between the two. This long answer is an incredibly simplified version of what is going on, it should get your head in the right place though.

Answer 3

Methanol is CH3OH; butane is CH3CH2CH2CH3; glucose is CH2OH.CHOH.CH.OH.CHOH.CHOH,CH=O.

Methanol cannot be a chain, branched chain, or ring. Butane may be a straight chain or a branched chain, (CH3)2CHCH3. Glucose may form a hexagonal ring with one O at one of the corners.

Methanol and glucose are water soluble; butane is not. Butane is a vapor at room temperature and pressure. Methanol is a liquid. Glucose is a solid.