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2. Formulae.

posted Mar 14, 2016, 2:33 PM by Upali Salpadoru   [ updated May 7, 2017, 7:37 PM ]

Meaning of a Chemical Formula.








Non-contact atomic force microscope (nc-AFM) images (center) of a molecule before and after a reaction improve immensely over images (top) from a scanning tunneling microscope and look just like the classic molecular structure diagrams (bottom).

 



       

The molecules are formed when atoms chemically combine.
For example water, H2O contains 2 atoms of Hydrogen and one of Oxygen.

How do we know this proportion?

If we know the masses of the ingredients that combine to form a compound and the Atomic masses, it is easy to calculate the number of atoms.

Let us take an example.

mass 10 g.                    mass 2 g

John has bought 500 g. of strawberries and 500 g. of grapes to be packeted and distribute among some children..

A strawberry has a Mass of  10 g .      

A grape has a Mass of  is 2 g.

Can you find the number of fruits in each category?
 Calculating the number of fruits.

Mass of straw berries  ........= 500g

Mass of one berry……………   =  10g
Number of berries=   500g ÷ 10 g 
                          =  50 fruits.

Mass of one grape …………    = 2g
  Number of grapes ……………= 500g ÷   2                                                 =  250 fruits


The number ratio of fruits strawberries : grapes =  50 : 250    =   1: 5
If you are to packet  according to availability  it should be in this ratio.
Each packet will have   =  strawberry 1 grapes  5

If we use S for strawberry and G for grapes, 

The formula of a packet will be S1G5     This can be given as  S G5

This is similar to a chemical formula.

If you can get the mass ratio of the ingredients of a pure compound  and their molecular masses, it is a simple process to get the formula.

Let us take and example:

 Number of Particles =  Total Mass ÷  Mass of a particle.

Example.1

   Fig.2 Magnesium burning inside a crucible.

When magnesium burns, a white coloured solid, magnesium oxide is formed. The formula is shown here.

The equation for the reaction:

Magnesium + Oxygen = Magnesium oxide
Here are the readings of an experiment performed.
Mass of crucible                             =  10.5 g
Mass of crucible + Magnesium        =   13.5 g
Mass after burning                        =    15.5 g

Mass ratio 

Mass of Magnesium          =   3.0 g

Mass of Oxygen combined =   2.0 g

    Mg: O    =  3 : 2




 
Particle Ratio

Atomic mass of Mg= 24.
Atomic mass of O  = 16

Mg: O  = 3/24  :   2/16.
           =  1/8  : 1/8
           =  1 : 1
Formula = Mg1 O1  =  MgO

 Example 2.

Finding the percentage composition of Ammonium sulphate.

Molecular mass of (NH4)2SO4…………………………………=  132

 Element Mass proportion Percentage by mass
 N-14 14x2=28 28x100/132 = 21.21%
 H-  1 1x8=8 8 ÷ 132 x 100 =  6.06 %
 S-32   S=32 32 ÷  132 x 100=  24,24%
 o=16 4x16=  64 64÷ 132 x 100= 48.48 %


Use this Periodic Table to get the Relative atomic mass.


 Some in alphabetical order for your convenience. (Without decimals)

Ag

Al

Ar

Au

B

Ba

Be

Br

C

Ca

Cd

Cl

Cu

Cr

Fe

H

He

Hg

108

27.0

40.0

197

10.8

137

9.0

80

12.0

40.

112

35.5

64

52.0

56

1.01

4.0

201

 

I

K

Li

Mg

Mn

N

Na

O

P

Pb

S

Sn

Si

Zn

127

39.

6.9

24.3

54.0

14.0

23.0

16.0

31.0

207

32.

119

26.

119

 Example 3.

A chemical consisting of three elements  had the  following percentages by mass.

Na = 43.40 %     C = 11.30 %   O  =  45.3 %

Find the formula of the compound.

 Element Percentage.by Mass Mass÷  Mass of an atom simple ratio
 Na-23  43.40 % 43.4/ 23 = 1.89 2
 C- 12   11.30 % 11.3/ 12 = 0.942 1
 O- 16   45.3 %   45.3/ 16=2.83 3

Formula of the chemical is       =  Na2 C1 O3    (We don’t have to write the 1 for C.  ) 

                                 Na2CO3         This is the formula of Sodium carbonate

   Verification

The total of percentages must add up to 100.

Nitrogen… =  21.21 Hydrogen…=    6.06Sulphur ..=  24.24 Oxygen……=  48.48

Total =         99.99    gets rounded up to 100.                                                                                           

   1.0  Determine the percentage composition of these compounds.

    

 Compound Molecule Molecular mass Percentages
  Example
Lead dioxide 
 PbO2 207+ 16.x 2 
          =239 
 Pb. =   207 ÷ 239 x 100   =  86.6 %
 2xO   =    32  ÷ 239 x 100 = 13.4 %
 1.Calcium carbonate CaCO3 a. Ca =        b.
  C  =       c.
3xO =      d.
 2. Potassium              permanganate.            KMnO4 e. K =          f.
 Mn =        g.
4x O  =     h.
 3. Potassium ferri    cyanide  K3Fe(CH)6 i. 3xK=       j.
 
Fe  =       k.
 6xC =      l.
6xH  =      m.
 4.Octane. C8H18 96+18=114 8xC  =    n.
18xH  =    O.

2x15=30 marks

  2.0   Find the formulae of these;  Mass ratio or the percentages by mass are given.

 Elements  Ratio Number  Ratio Simple ratio  Formula  
 Example
Hg - 201
O -16
 
Hg= 50 g
  O = 4 g.
 
Hg  50 ÷ 201= 0.25
 O    4 
÷  16 =  0.25
 0.25:0.25 = 1:1 HgO
 H -1
 O- 16
 H = 20 g
O=320g.
 H = 20 ÷ 1 =20
320 
÷ 16 =20
 a. b.
 Cu-
O- 
 Cu = 1.6
 O=  0.2 
  c. d.
 Ca-40.
 O - 16
 H- 1 
 Ca=54.05%
 O= 43.24%
 H = 2.71%
  e. f.
 Pb-207
 O- 16
 Pb= 2.07
 O = 0.32
  g. h.
 H -1
 O = 16
 H= 20 g
 O = 320
  i. j.
3x10 = 30

.

3.   On heating 50g of mercury oxide 46 g  of mercury was obtained. Derive the formula of the mercury oxide.

4.  On heating 1.6g of copper 1.8g of a copper oxide was formed. Find the formula of the oxide.

5.  By reducing 2.39 mg of lead 2.07 mg of lead was obtained. Find the empirical formula of the oxide.

6.A compound has the following percentage composiion. Derive the empirical formula.

 Carbon =  40%       Hydrogen = 6.7 %    Oxygen= 53.3 %

8x4 =32


7. 

Canvas.jpg

These are the 3 common isotopes of Hydrogen.

Although the water forming from them would be chemically the same mass ratios will not be the same.

Calculate the Oxygen percentage in the 3 types of water.





 1H2O

2H2O

3H2O

සමස්කඵානික ස්කන්ධය

 18

20

v.

ඔක්සිජන් ස්කන්ධය

.  16

.16

16

ඔක්සිජන්  ප්‍රතිශතය

w.

x.

y.

සැලකිිය යුතුයි:- සාමාන්‍ය හයිඩ්‍රජන් සැම්පලයක H-1 සමස්ඵානික 99.99% ක්ම තිබ‍ෙන බැව් සැලකිිය යුතුය.

                                                                                                                               2x4= 8 Marks

             


                                                  

    Answers:1. HgO,    2. H1O1, (There is no compound like this. This compound really is H2O2,)    3. Cu2O,   4.  Ca O2H2  (This really is Ca(OH)2 ,    5.  PbO.

Answers

Q.No.

1.1

1.2

2.1

2.2

2.3

3.1

4.1

4.2

5.1

5.2

Answer

86.61%

13.38%

40 %

12%

48 *

27.27 %

40.51 %

40.51 g

35.8

47.6

 3. Steps for the calculation.

Mass ratio of  Hg:O  is  ---:-----

Atom ratio is  ----/201 : -----/16  =  ----- : ------

Get the approximate ratio leaving for experimental errors.

Therefore the formula must be ---------

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