CU-ATS CHEMISTRY FORMULAE

John Dalton found…

The idea of atoms

J.J. Thomson found…

Electrons

Eugen Goldstein found…

Protons

Robert Millikan found…

Mass and charge of electrons

Ernest Rutherford found…

Nucleus

James Chadwick found…

Neutrons

Niles Bohr found…

Electron shells, circular orbits

Heisenberg found…

that velocity & position of particles can’t be measured at the same time

De Broglie found…

Electrons can act as standing waves

Einstein found…

That light can be photons

Schrödinger found…

Orbitals, cloud of electrons

Quantum number, n

Principle quantum number 1,2,3

Quantum number, $l$

Angular quantum number - s=0, p=1, d=2, f=3

Quantum number $ml$

Magnetic quantum number, which orbital - range is plus minus angular quantum number

Quantum number $ms$

Spin quantum number, plus minus 1/2

Bond geometry names for 5 electron domains

5) trigonal Bioyramidal

4) seesaw

3) T-shaped

2) Linear

Bond geometry names for 6 electron domains

6) Octahedral

5) square pyramidal

4)square planar

Concentration - %w/v

mass of solute/volume of solution

Concentration - %w/w

mass of solute/mass of solution

Concentration - %v/v

volume of solute/volume of solution (solute plus solvent)

Molality

mol of solute/kg of solvent

Colligative properties

$\Delta T=i\times molal\times k$ - i is how many dissociated

PV whose law

Boyle’s law

V/T whose law

Charles Law

P/T whose law

Guy Lusaac law

Partial pressure of a gas

Partial pressure = mole fraction x total pressure

Total pressure = pressure 1 + pressure 2

Rate of diffusion

$$\frac{rate1}{rate2}=\sqrt{\frac{Mr2}{Mr1}}$$

Rate of reaction with k and concentrations

Rate = k$\left\lbrack a\right.\rbrack^{m}\left\lbrack b\right.\rbrack^{n}$

Finding reaction orders

(x of concentration)^m = (x of rate)

Finding equilibrium constant Kc

$$kc=\frac{\left(P\right)^{p}}{\left(R\right)^{r}}$$

Finding equilibrium with pressure Kp

$$Kp=\frac{\left(pressureA\right)^{a}}{\left(pressureB\right)^{b}}$$

Ksp solubility constant

Ksp =$\left(A\right)^{a}\left(B\right)^{b}$

Kw

Concentration of H+ x concentration of OH- , or $10^{-14}$

pH and pOH from concentration

pH = $-\log_{10}$ [H+]

Concentration from pH or pOH

Concentration of H+ = $10^{-pH}$

Concentrations of H+ or OH- for weak acids$\sqrt{Ka\times Macid}$

[H+] = $\sqrt{Ka\times Macid}$

% dissociation of weak acid

% =$\sqrt{\frac{Ka}{Macid}}\times100$

pH or pOH of a buffer solution

pH = $pKa-\log_{10}\left(\frac{\left\lbrack acid\right\rbrack\rbrack}{\left\lbrack salT\rbrack\right\rbrack}\right)$ or mol ofacid and salt

Titration concentration and volume

aCV = bCV

How to balance a redox reaction

1. ดูว่าอันไหน redox แล้วตั้งสอง equations

2. เอา H2O ดุล Oxygen

3. เอา H+ ดุล Hydrogen

4. แล้วเอา e- ดุล charge

5. รวมสมการ

6. ถ้าใน basic condition ให้ เติม OH- ในฝั่งที่มี H+ แล้วแปลงเป็นน้ำ

What is 1 Faraday

96,500 coulombs

Electrolysis ดูด electron Eo เยอะหรือน้อย

เยอะ

Electrolysis เสีย electron Eo น้อยหรือเยอะ

น้อย

Cell notation

anode ซ้าย Cathode ขวา

Eo cell =

Eo cathode - Eo anode

R-OH

Alcohol, -ol

R-O-R

Ether, -yl -yl ether, -alkoxy -ane

R-C(=O) -H

Aldehyde, -al

R-C(=O) -R

Ketone, -one

R-C(=O)-OH

Carboxylic acid, -oic acid, -ic acid

R-C(=O)-O-R

Ester, -yl -oate

R-NH2

Amine, -amine

R-C(=O) - NH2

Amide, -amide

Esterification is a reaction between who and who

Carboxylic acid plus alcohol with acid

Hydrolysis is the reverse.

Saponification is a reaction between who and who

Ester plus a base into an alcohol with a Carboxylic acid but with a cation instead of H

Test for starch

Iodine solution - turns black

Test for protein

Biuret’s reagent - turns purple

Test for reducing sugars

Benedict’s solution and heat - turns red

Test for non-reducing sugars (sucrose)

HCl - NaHCO3 - heat - turns red

Test for lipids

Ethanol and shake - turns cloudy

Test for unsaturated lipids

Bromine water and shake - colour bleached out.

What makes up lipids

Glycerol back bone and Fatty acids (Carboxylic acid)