Page 80 - ICSE Chemistry 8
P. 80

RELATIVE ATOMIC MASS
                                                                                         Thirst for Knowledge
                 Atoms are too small to be weighed. So scien  sts  focused
                 on fi nding out a standard atom and calcula  ng the rela  ve        The average mass of one atom of an
                 weight of atoms of other elements by comparing it with the         element is used because elements
                 mass of the standard atom.                                         may have atoms of diff erent masses.
                                                                                    This is because the number of
                 Earlier hydrogen atom was chosen as the standard atom
                                                                                    neutrons in the nucleus may diff er
                 for this purpose. As   me passed, the scale of atomic weight       from atom to atom.
                 based on hydrogen was abandoned and the term atomic
                 weight was also replaced by another term called the rela  ve atomic mass of an element.
                 The rela  ve atomic mass of an element is the number of   mes by which the average mass of one atom of
                 an element is heavier than 1/12th of the mass of a carbon atom (assigned atomic mass 12). It is unitless
                 as it is a pure ra  o.

                                                             Average mass of one atom of an element
                                 Rela  ve atomic mass =
                                                        One-twel  h of the mass of one atom of carbon-12

                 It is expressed in unifi ed atomic mass unit (and denoted as u).

                 Thus, the atomic mass of hydrogen atom is 1 u and that of oxygen atom is 16 u

                 ISOTOPES


                 Atoms of the same element having same atomic number but diff erent mass number are known as
                                         14
                                                 15
                 isotopes. For example,  N and  N are the two isotopes of nitrogen. There are 7 protons and 7 electrons
                                          7       7                   14
                 in both the isotopes. But the fi rst atom of nitrogen ( N) has 7 neutrons and the second atom of nitrogen
                  15                                                     7
                 ( N) has 8 neutrons.
                     7
                                                                               e                   e                   e
                 Let’s understand this with the help of other
                 examples.                                                 1 P                1 P                 2 N
                                                                                              1 N                 1 P
                     •  Hydrogen has three isotopes.
                                     1
                        Pro  um     ( H)
                                                                             1
                                                                                                                     3
                                                                                                   2
                                      1                                protium ( H)       deuterium ( H)       tritium ( H)
                                     2                                         1                    1                 1
                        Deuterium ( H)                              (ordinary hydrogen)
                                      1
                                     3
                        Tri  um     ( H)                                          Fig. 4.13: Isotopes of hydrogen
                                      1
                 All three isotopes of hydrogen have same number of electrons and protons, i.e., equal to 1. However, the
                 number of neutrons vary. Pro  um has no neutron, deuterium has 1 neutron and tri  um has 2 neutrons.
                     •  Similarly, carbon also has three isotopes.
                                    12
                        Carbon-12 [ C]
                                       6
                                    13
                        Carbon-13 [ C]
                                       6
                                    14
                        Carbon-14 [ C]
                                       6
                 Here also, we can see that the number of electrons and protons are same, i.e., equal to 6 in all three
                 isotopes. But there are 6 neutrons in the fi rst isotope, 7 neutrons in the second isotope and 8 neutrons
                 in the third isotope.


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