I suck at Chemistry. Is there anyone here that understands it or knows it well? Please let me know. I’ve got a million questions to ask.
Re: Chemistry Tutor Needed
telling us what level of chemistry... and a short-list of topics you're having trouble with would help.
Re: Chemistry Tutor Needed
if it’s balancing equations, you’ll love me 
Re: Chemistry Tutor Needed
Right now, we’re on the Lewis Dot Structure. I’m having trouble figuring out how to know where the electrons, bonds, and double bonds should be placed.
I also have trouble with stoichiometric equations, converting grams to moles, and finding the limiting reactanct.
I finally understood electronic configuration as of yesterday 
Passionate - That’s easy peasy! Thanks anyways, though. 
Re: Chemistry Tutor Needed
aaaah lewis dot structures.i remember that was our last lesson in chem 101 (fall 2002), and I loved em :D
i am a bit rusty on them, but first of all what u need to figure out are the # of valence electrons. Keep a periodic table handy all the time, no guessing.
Now, th basic rule is (i think), that you need to fulfill the octet rule. (witht he exception of H, whre its the duet rule). Ofcourse ther are some cases wher the octet rule is violated but i am sure you're not gonna get tested on those.
start with really easy stuff first. When I think easy I think water, H2O.
O has 6 electrons in its valence shell, and 1 electron for each hydrogen.
Now, when you draw the O atom, draw it with two full pair of electrons and draw the other two electrons separately. Draw the hydrogen atoms with their one electron each, connect the electrons from O and H that dont have a partner. there's your lewis structure. O gets its octet and H gets its duet ( is the word, duet?).
You use double bonds to satisfy the octet rule as well. e.g, CO2
and dont draw it like this: H-O-H , there's an angle in the water molecule. But you havent asked abou that so m guessing you know about the shapes n stuff.
I'll do a couple of complicated examples on my own because i dont remember all the rules and then post some more examples.
p.s. practice makes perfect.
Re: Chemistry Tutor Needed
Can an element have just one electron dot? For example, Hydrogen on has one valence electron, so how do you signify just one electron for it?
The "bond" (the line connecting two elements in a molecule) represents two electrons. If Hydrogen has a bond going to Oxygen, will Hydrogen then have 2 electrons because of the bond, or 1 because it is only connected to one end of the bond?
Yea, we've gone over identifying the geometric shapes and whether it is polar or not. I understand that for the most part...
but what is the difference between a "bent" structure and a "linear" structure?
Re: Chemistry Tutor Needed
noone else replied 
hehe okay, i m sure you know all about ionic and covalent bonds right?
Well the bond between O and H is polar covalent. The electrons are shared between H and O, just that they’re attracted more towards the O than the H.
H has only one electron in its valence shell, needs one to fulfill it. And O has one electron available, so they form a bond. H doesnt take the electrons from O and vice versa. They just share the electrons.
But that should not affect you calculating the # of valence electrons in the beginning. H will always have 1 and O will always have 6. In H2O’s case, there are 6+1+1 electrons available to bond.
The difference I can think of right now between the structures is the angle. In linear structures the angle is 180 degrees. In other structues the angle varies, like from 104.5 to 90 etc.
Actually, you cant just say a shape is “bent” or linear" I mean there is a shape called linear like in CO2. But then there is tetrahedral and trigonal planar etc. I think the “bent” shape you get when you have a pair ( or two) of unbonded electrons present alongside bonds. e.g, in H2O. But dont qoute me on this. I was never really good with shapes.
Re: Chemistry Tutor Needed
Another thing about the Lewis structures is the formal charges. I dont know the formula off the top of my head, but it is something like valence electrons - unbonded electrons - something else.
Anyhow when you're drawing lewis structures for compounds with charges, e.g, NO3- , make sure that when u draw the structures and assign formal charges, the sum comes out to -1. If it doesnt, the structure is wrong. There is two different ways you can draw NO3- , one's ofcourse wrong, one's right. Try it and see what I am talking about.
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Okay I think I got it. Are these right???
Re: Chemistry Tutor Needed
Looks great!! :k:
now try some with charges on em.
Re: Chemistry Tutor Needed
No :( I'm gonna get it wrong.
No wait a minute. With the charges, you just put brackets around the whole model and put the number on the outside, yea?
Re: Chemistry Tutor Needed
yes thats right, but thats the last thing u shud be thinking about.
And try it before you say you’re gonna get it wrong 
Anyhow, if you have a negative charge on an entity like -1 just add one electron tot he # of valence electrons. If you have a +1 (2,3…) subtract one electron from the # of valence electrons that u need to draw.
Dont forget formal charges.
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Oh yea yea I already knew that. 
Re: Chemistry Tutor Needed
ye OF2 aur SiCl4......... kia bana diya?
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O is -2, F is -1, how can you make OF2? 
apni apni ijaad (innovation)?
Re: Chemistry Tutor Needed
No no...The subscript is "2" for OF. That's given (it's not like a set number)
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think they share electrons
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a part of my high school years i'd never like to see again :D
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^^ Sisters in hatred :)