Yesterday, we have discussed on the atomic number (Z) and atomic mass (A) that are related to a chemical element.
Today, we shall continue with the discussion on Isotopes where many students tends to lose marks in exams.
Definition of Isotopes:
–> Atoms of the same element with the same number of protons but different number of neutrons
Charareristics:
- Same proton or atomic number
- Different nucleon or mass number
- Same chemical properties (since chemical reactions involve electrons only)
- Slightly different physical properties (since relative masses of isotopes differ)
Just with the above information, it will allow you to score all the marks you need in examinations with questions related to Isotopes.
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Most elements are commonly made up of isotopes. Only a few elements exist without isotopes.
Hydrogen has 3 Isotopes, with mass numbers 1, 2 and 3. They contain the same number of protons and electrons, but differ in number of neutrons.
Hydrogen-1 has no neutrons, Hydrogen-2 has one neutron and Hydrogen-3 has two neutrons.
Let’s check out an exam-based question related to Isotopes.
Question 1:
Uranium-235 and uranium-238 are two isotopes of uranium.
The table below shows the numbers of the particles in one atom of uranium-235.Particle Number
Electron?? ?92
Neutron??? 143
Proton?????? 92(a) Define Isotopes.
(b) Suggest a reason why this is known as uranium-235.
(c) Give the numbers of particles found in an atom of uranium-238.
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