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“We must trust to nothing but facts: These are presented to us by Nature, and cannot deceive. We ought, in every instance, to submit our reasoning to the test of experiment, and never to search for truth but by the natural road of experiment and observation.” ― Antoine Lavoisier, Elements of Chemistry

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Friday, 28 March 2014

CP1 HOMEWORK-part2

Here is your homework part 2, click here to download
Submission: submit both of your homeworks (part1 and part2) on Mr. Markus desk on March, 10

CP1 : HOMEWORK-part 1

To download your homework, kindly click here

ANIONS AND CATIONS LIST

simple ions:
Hydride
H-
Oxide
O2-
Fluoride
F-
Sulfide
S2-
Chloride
Cl-
Nitride
N3-
Bromide
Br-
Iodide
I-
Oxoanions:
Arsenate
AsO43-
Phosphate
PO43-
Arsenite
AsO33-
Hydrogen phosphate
HPO42-
Dihydrogen phosphate
H2PO4-
Sulfate
SO42-
Nitrate
NO3-
Hydrogen sulfate
HSO4-
Nitrite
NO2-
Thiosulfate
S2O32-
Sulfite
SO32-
Perchlorate
ClO4-
Iodate
IO3-
Chlorate
ClO3-
Bromate
BrO3-
Chlorite
ClO2-
Hypochlorite
OCl-
Hypobromite
OBr-
Carbonate
CO32-
Chromate
CrO42-
Hydrogen carbonate
or Bicarbonate
HCO3-
Dichromate
Cr2O72-
Anions from Organic Acids:
Acetate
CH3COO-
formate
HCOO-

Others:
Cyanide
CN-
Amide
NH2-
Cyanate
OCN-
Peroxide
O22-
Thiocyanate
SCN-
Oxalate
C2O42-
Hydroxide
OH-
Permanganate
MnO4-
Common Cations: (ions grouped by charge)
Name
Formula
Other name(s)
Ammonium
NH4+
Barium
Ba+2
Calcium
Ca+2
Chromium(II)
Cr+2
Chromous
Chromium(III)
Cr+3
Chromic
Copper(I)
Cu+
Cuprous
Copper(II)
Cu+2
Cupric
Iron(II)
Fe+2
Ferrous
Iron(III)
Fe+3
Ferric
Hydrogen
H+
Hydronium
H3O+
Lead(II)
Pb+2
Magnesium
Mg+2
Manganese(II)
Mn+2
Manganous
Manganese(III)
Mn+3
Manganic
Mercury(I)
Hg2+2
Mercurous
Mercury(II)
Hg+2
Mercuric
Nitronium
NO2+
Strontium
Sr+2
Tin(II)
Sn+2
Stannous
Tin(IV)
Sn+4
Stannic





Wednesday, 5 March 2014

FOR CP1 ONLY

Here are the pointer to review for upcoming midterm test:
1. Kinetic theory of matter:
    -  The properties of solid, liquid and gas based on the kinetic theory of matter;
    -  gas pressure;
    -  dissolving process;
    -  diffusion;
2. Acids and Bases
    -  Acids and Bases properties;
    -  Indicators;
    -  pH;
    -  Examples of acids/bases

Workout these following question in your "EXERCISE BOOK" only. Submit it after Chemistry Test (Monday, March 10) on Mr. Markus desk.

  1. State the characteristics/properties of acids and bases (4 characteristic)                                 [8]

ACIDS PROPERTIES
BASES PROPERTIES

















    2. Fill in the blank in the table below, if P = alkali, Q = acid. The litmus paper turns in color.
Solution
P
Q
red litmus paper


blue litmus paper


                                                                                                                                                   [4]
       What are the other acid base indicators instead the litmus paper? [2]

3.  Sweat from the skin is slightly acidic and reacts with jewellery containing nickel.
(i)                  Suggest how you could find out the pH of the sweat on the surface of your skin. [2]
  
(ii)               Which one of the values represents a pH which is slightly acidic.
Put a ring around the correct answer. [1]
  
pH 2                               pH 6                       pH 7                      pH 8                      pH 13


4. A solution of perfume has a strong smell.
A beaker of perfume solution is put in the corner of a room which is free of draughts. At first, the girl by the closed window cannot smell the perfume. After 30 seconds she smells the perfume.
Use the kinetic particle theory to explain these facts. [2]


FOR CP2 ONLY!

Here are pointers to review for midterm test:
1. Exothermic and Endothermic reaction: 
    -  The principle of exothermic and endothermic reaction/process;
    -  describing exo endo reaction in the term of breaking bonds and forming bonds;
    -  exo-endo process in the changing state of matter
    -  The examples of exo endo
2. Chemical Equations: Balancing Chemical Equations
    -  describing chemical equations: the signs in equations
    -  balance a chemical equations

Balance the following equations.

1         1.  ___C2H3Cl   + ___O2 à ___CO2  + ___H2O   + ___HCl
2         2.      ___(NH4)2Cr2O7 à ___NH3  + ___H2O  + ___Cr2O3  + ___O2
3         3.      ___Al  + ___NaOH  + ___H2O à ___NaAl(OH)4  + ___H2
4         4.      ___NH4Cl   + ___Ca(OH)2 à ___CaCl2  + ___NH3   + ___H2O
5         5.      ___Al  + ___NH4ClO4 à ___Al2O3  + ___AlCl3  + ___NO  + ___H2O
6         6.      ___H2SO4  +  ___NaHCO3 à ___Na2SO4    + ___CO2    + ___H2O
7         7.      _____ NaOH (aq) + _____ H2SO4 (aq) → _____ H2O (l) + _____ Na2SO4 (aq)
8         8.      _____ K (s) + _____ H2O (l) → _____ KOH (aq) + _____ H2 (g)
9.      ____ H2 + ____ O2 à ____ H2O
10.  ____ Pb(OH)2 + ____ HCl à ____ H2O + ____ PbCl2
11.  ____ AlBr3 + ____ K2SO4 à ____ KBr + ____ Al2(SO4)3
12.  ____ CH4 + ____ O2 à ____ CO2 + ____ H2O
13.  ____ C8H18 + ____ O2 à ____ CO2 + ____ H2O
14.  ____ FeCl3 + ____ NaOH à ____ Fe(OH)3 + ____NaCl
15.  ____ Ag2O à ____ Ag + ____O2