http://www.onemanga.com/Naruto/441/
( Watch Naru-tard own Pein )


http://www.onemanga.com/Bleach/351/
( Come on Kensei APPEAR ALREADY !! )


I know this has nothing to do with chemistry but its the weekends got to de-stress myself.

Removed all pictures in my recent posts due to the fact that Ms Jee is experiencing Pop-up advertisements. This blog feels dead/boring just like reading something out of a chemisty textbook. Forgot to mention that Orbital is a 3-D region* from my previous post. Currently going throught the notes we printed out ourselves because there is going to be a test on MOLE on Monday. Got to start memorising/understanding formulas and defination since I'm expecting 80% - 100% of the test to be Short-answer question rather than MCQs. Hund's rule is really helpful when it comes to the questions in tutorial 3. Yawns, off to sleep now.

Got this defination from Ashvin's blogspot very helpful.

Isotopic: Atoms, ions or molecules containing same number of protons.
Isotonic: Atoms, ions or molecules containing same number of neutrons.
Isoelectronic: Atoms, ions or molecules containing same number of electrons.

Aufbau principle
Electrons occupy orbitals of the lowest energy available.

Pauli Exclusion Principle
Each orbital can accommodate only two electrons whose spins are always opposite.

Hund's Rule
When electrons are added successively to a subshell, they occupy the orbitals singly first before pairing occurs.

I feel dead tired, just came home around 9.30. Today we learnt about Atoms in a much more deeper concept which is totally O.O to me. Shells and sub-shells are still fine by me since its still related to the electronic configuration that we learned in Secondary level but ORBITAL is totally a new concept that I need to grasp fast. If I'm not wrong this is what Mr.Tan said, "Orbital is the region whereby it is possible to indicate where the electrons are most likely to be found." Maybe he wrote that or said it, doesn't matter and Orbital can be divided in to s, p, d, and f.

Just printed my own set of notes and reading ahead and found more familiar stuff coming back to haunt us during our 3 years in M.I. Stuffs like bonding, but looking at the my thick notes, we're going in depth regarding the topic bonding. Something about Ionisation and determining/caculating the shape of a molecules scares the living crap out of me. Ok off to sleep.

Ok just stolen some notes from Jasmine's blog. I just wondered, why do I have friends that have similar names like Jazz ( BJ ), Jesslyn ( LPP), Jasmine ( Don't know her chinese name ). It's really going to be hard calling their nicknames like "Jazz", "Jess" and "Jas". Ok this is really ridiculous. Nevermind about that particular topic.

Here's something I stole from " Jasmine's " blog. And by the way I don't just steal any particular information from some TomDickHarry, in fact I steal quality bullcrap which by the way is from Wikipedia.

What Kensei learned.

The equivalence point, or stoichiometric point, of a chemical reaction occurs during a chemical titration when the amount of titrant added is equivalent, or equal, to the amount of analyte present in the sample.

Different methods to determine the equivalence point include:

pH indicator
This is a substance that changes colour in response to a chemical change. An acid-base indicator (e.g., phenolphthalein) changes colour depending on the pH. Redox indicators are also frequently used. A drop of indicator solution is added to the titration at the start; when the colour changes the endpoint has been reached, this is an approximation of the equivalence point.

pH meter
This is a potentiometer which uses an electrode whose potential depends on the amount of H+ ion present in the solution. (This is an example of an ion selective electrode. This allows the pH of the solution to be measured throughout the titration. At the equivalence point there will be a sudden change in the measured pH. It can be more accurate than the indicator method, and is very easily automated.

Color change
In some reactions, the solution changes colour without any added indicator. This is often seen in redox titrations, for instance, when the different oxidation states of the product and reactant produce different colours.

Precipitation
If the reaction forms a solid, then a precipitate will form during the titration. A classic example is the reaction between Ag+ and Cl- to form the very insoluble salt AgCl. Surprisingly, this usually makes it difficult to determine the endpoint precisely. As a result, precipitation titrations often have to be done as back titrations.

Wikipedia is really a pal when it comes to educational stuff which I include in news as well, do not underestimated the power of Wikipedia it will someday save your life like it did for mine which is particularly today. As compared to other people's blogs in 09s2 my blog is not that educational ot helpful to you my fellow classmate so feel free to comment me on the way I present my daily chemistry studies.

Ok for real.

This chemistry blog is for real people. Teachers are invading and reading Each and Everyone of our Post. It feels weird but that is the reason why this blog is created ( keep reminding myself ). Ok here I go.

Strength / Weakness in chemistry :

Apparently my only which makes it the most important strength in chemistry is how good I am with memorising big details and picturing them into smaller points. In other words, I'm very good at memorising stuff last minute which happends to be a very bad habit of mine I can't control well. I keep telling myself its time to change my POV of studying through thick skull of mine. At the same time this becomes my weakness. When I tend to do last minute studying I don't study as much as others who studied much earlier than me, this prove to be a very big dissadvantage to me. I won't say this is much of a strength but instead this is a very Big weakness of mine which has to change. In conclusion, I have no Strength in Chemistry but trying to build up one by putting aside my weakness and trying to change it to my advantage.



Comments on Feedbacks

Hi Mr Tan, I'm really sorry if this offends you but do I know you from chemistry class? Were you the teacher during our lesson in the chemistry lab the one with the specs or did I get the wrong person?

Ok equipped my blog with many things very unrelated to chemistry, hope Ms Jee allows it. The reason, to brighten up my blog just abit so it would not be so "Boring".

Only been my 3rd post. I've started comparing the old periodic table used in our Secondary schools days and now, so much different. There's alot more elements with decimals in their number of Atomic mass. So shocked. Ok I lied, I've not learned much in the holidays but revised on Secondary school basic Chemistry. Ok off to "Study".

Is it me or am I missing out something? Why is everyone writing out thier ambition/ I - wanna - be - when - I - grow - up . Is is part of our assignment? In that case I SHALL WRITE too.

I wanna be a Cook, want to know why? Because Food is everything, I want to explore the unexplored which others fail to do. So basically I plan be an "Art" Chef creating what is impossible in any average cuisine, by breaking normal boundaries of ordinary culinary skills and building new bonds between different culture's culinary skills and therefore creating a new style of cuisine of my own.

Dead. This is only my 2nd post in this blog and Ms Jee is starting notice that lazy people excluding me ( too busy ) are not updating their chemistry blog. Ok here I go, I gonna summarise what I learnd during my 2 weeks of chemistry lesson which is gonna be short; due to the fact that I'm absence for most of Ms Jee's lesson ( too sick ). Ok. So far i covered most of my doubt in the chapter ( Atoms, Molecules and Stoichiometry( <- how the fish do you pronounce this word)).

What Kensei covered.

-Defination of terms <br>

(1). Relative Isotopic Mass. Defined as mass of one atom of an isotope compared to 1/12 the mass of carbon -12.

(2). Relative Atomic Mass. Defined as mass of one atome of an element compared to 1/12 the mass of carbon -12.

(3). Abundance. Is the percentage of isotpe found in the naturally occuring element.

(4). Relative Molecular Mass. Is the sum of the relative atomic masses of all atoms in one molecule in a covalent compound.

(5). Relative Formula Mass. Is the relative molecular mass of an ionic and giant molecular compound.

(6). Avogadro's constant, ( 6.02 x 10 to the power of 23 ). Is equal to one mole of any substance's amount of particles.

(7) Crap, for now that's all I learned.

Sorry for not updating for a long time, I live in Hougang ( not to make it into an excuse). I take around 2 hours to go forth and back to school. Tiring but I'll try my best to update this blog as soon I learn something ( which is really hard ) or if I'm free and has no massive amount of homework.

We learned Titration during one of our lessons this week. We are expected to be very ( damn ) accurate because most of our results are wrong ( duh ) or we just screwed up last minute due to the time constrain or, the apparatus is not rinsed well and its contaminated.

What Kensei learned.

(1). No consuming of any edible substances in the lab, not even the chemicals. ( Even if they're tempting )

(2). Accuracy. Consistantly record your observation even if its the slightlest reading.

(3). The Litmus test. ( Which i flunged hard )

(4). How expensive the apparatus are and to handle them with care. ( $ is involved, CAREFUL )