<p>I need a study aid for chemistry, specifically one that explains hybridization thoroughly. </p>
<p>I know that AP books often gloss over this subject as it is not tested often; however, is there another study aid that offers a comprehensive testbook supplement?</p>
<p>I didn't use a study aid for Chem, but I can explain hybridization if that'd help.</p>
<p>That'd be really appreciated. I understand VSEPR and Lewis Dot really well and supposedly that guarantees understanding of hybridization, but I guess not.</p>
<p>Our teacher skipped the entire chapter that deals with all the orbitals (spdf what ever) so I guess that's my problem. I understand basically what those are, but get confused with the labels sp, sp^2, etc. when we're done drawing the hybrid but need to label it. </p>
<p>Here's a problem:
Hybrid of CH(4): </p>
<p>Copied from the book (Zumdahl/Zumdahl sixth):
"... the mixing of native atomic orbitals are called sp^3 orbitals because they are formed from one 2s and three 2p orbitals (s^1p^3)..."</p>
<p>I thought Carbon was 2s^2,2p^2? ANd hydrogen 1s^2? Where did we get those numbers to get sp^3?</p>
<p>Since you know Lewis Dot, that's great. Basically, draw the molecule out with all the electrons included. The hybridization can be thought of as "the number of occupied sides" an atom in the molecule has. "Occupied" as in, is there a bond or unbonded electron pair. If 1 side is occupied, the hybridization is "s". 2 sides is "sp" and 3 sides is sp2 and 4 sides is sp3.</p>
<p>*for the sake of my convenience sp3 = sp^3 :D</p>
<p>When you draw the typical lewis dot, you have a S orbital and 3 p orbitals.</p>
<p>A carbon atom has a hybridization of sp3.</p>
<p>A hydrogen atom (in CH4) has a hybridization of s.</p>
<p>Examples:</p>
<p>NaCl ~ Hybridization:(Na = sp) (Cl = sp3)
BaI2 ~ (Ba = sp) (each I = sp3)
AlF3 ~ (Al = sp2) (F = sp3)
SiF4 ~ (Si = sp3) (F = sp3)</p>
<p>Now comes the tricky part.</p>
<p>The atoms with 1 or more unbonded electron pairs, can split one or more electron pairs to form more bonds. This creates atoms with a hybridization in the dsp3 and d^2sp^3. dsp3 is when one pair is split. d2sp3 is when 2 are split.</p>
<p>For example:</p>
<p>PF5 ~ (P = dsp3) (F=sp3)
SF4 ~ (S = dsp3) (F=sp3)
ClF3 ~ (Cl = dsp3) (F=sp3)</p>
<p>SF6 ~ (S = d2sp3) (F=sp3)
ClF5 ~ (Cl = d2sp3) (F=sp3)
XeF4 ~ (Xe = d2sp3) (F=sp3)</p>
<p>Since you said you get VSEPR, I trust that you know how to draw the structural shapes of the atoms and know the shapes/bond angles.</p>
<p>Hybridization is really just "counting" how many "sides" of each element is taken up with an unbonded electron pair or by a bond.</p>
<p>Typically, only the center atom will have a hybridization of dsp3 or d2sp3.</p>
<p>I don't remember which edition of Zumdahl's Chemistry my class used last year, but it was the same book. Look at the diagrams and it helps to make a huge chart in your notebook of every possible combination of element (include shape, bond angles, attraction forces, molecule type, hybridization and eventually resonance form (if available) and formal charge.)</p>
<p>Thanks a lot; that really helped me. </p>
<p>So I reviewed the first section that dealt with hybridization and the second section that dealt with The Molecular Orbit MOdel an they seem okay.</p>
<p>Now, the homonuclear diatomic molecules what ever stuff is killing me. I get completely lost with paramagnetism/diablahblah and that stupid chart with arrows going up and down. I'll do my best to study on my own, but it will help if someone gives me a few tips.</p>
<p>In oxygen gas (O2) does each one do sp3 or sp2 hybridization? Basically I am asking where the double bond is counted as two pairs when you count the pairs of shared or unshared electrons occupying the sides of the atom.</p>
<p>sp2 hybridization.</p>
<p>Ok, so a double and single bond are counted the same.
Just to make sure, in CO2, oxygen does sp3 hybridization right?</p>
<p>Nevermind, its still sp2....
I am trying to think of a compound that makes oxygen use sp3 hybridization.. I remember I had that question on a test before.</p>
<p>CH3OH.</p>
<p>O has sp3 hybridization.</p>
<p>Sorry but what you said was not correct
For example C in graphite is sp2 hybridization, C in diamond is sp3 hybridization
They just ask about hybridization in central atom. So, for example, PF5, SF4,CO2 etc. don't worry about O, F hybridization. There's no point for them to be hybridized and tesk makers never ask about their hybridization. Just care about Central atoms like P, S, C.
Compounds like NaCl, BaI2 etc, is ion compound. So there's no hybridization.</p>
<p>All atoms in a molecule are hybridized. Although I agree that the primary concern should be the hybridization of the center atom, it is incorrect to think that only the center atom has hybridization. An AP student should realize this, even if it is not tested on the exam.</p>
<p>Hybridization describes the bonding atoms from an atom's point of view, not exclusively the center atom.</p>
<p>As to your attempt to catch a mistake about the hybridization of carbon, I was responding to the original poster's question about the hybridization of C in CH4, which is sp3.</p>
<p>Furthermore, my post was an exact replica of my notes. So unless Zumdahl has published incorrect information, I stand by by examples.</p>
<p>But thank you for dedicating your first post to proving me wrong. I'm flattered.</p>
<p>Zumdahl's a jerk!!</p>
<p>Thats all i have to say.</p>
<p>omg i have that book too ZUmdahl! Its terrible.. Even my teacher says its terrible!!~!~!~ I also need a new book.</p>
<p>and yes... i understand everything so far.. but stupid hybridization and Lewis Structures aren't explained well in the book... heck.. nothing is explained well in the book.. im stuck on hybridization too.</p>
<p>zumdahl sucks balls. one of the worst chemistry books ever, i don't think i ever learned anything from it. nothing is explained in simple terms in it.</p>
<p>I find that zumdalh is one of the more bearable chemistry texts available... Our textbook for Chem 1... now that was something.</p>
<p>i liked zumdahl a lot >:O</p>