Explain with examples (1) Atomic number, (ii) Mass number, 8. (ii) Isotopes and iv) Isobars. Give any two uses of isotopes.
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Step-by-step explanation:
Ar40,19K40 are isobars having the same atomic mass but different atomic numbers. The two uses of isotopes are: (i) As nuclear fuel: An isotope of uranium (U–235) is used as a nuclear fuel. (ii) An isotope of cobalt is used in the treatment of cancer.
Answer:
(i) Atomic number: The atomic number is the total number of protons present in the atom. For example, the atomic number of MgMg is 1212. It contains 1212 protons and 1212 electrons.
(ii) Mass number: It is the sum of the number of neutrons and the number of protons. For example, the atomic number of Lithium is 44 which is equal to the number of protons, the number of neutrons of magnesium is 44. The mass number is equal to 8(4+4)8(4+4).
(iii) Isotopes are the elements having the same atomic number but different mass numbers. They have the same chemical properties as the number of valence electrons is the same. For example, 6C12, 6C13, 6C14 are the three isotopes of carbon. They have the same atomic number but different mass numbers due to the difference in the number of neutrons.
(iv) Isobars are elements having the same mass number but different atomic numbers. For example. 18Ar40,19K40 are isobars having the same atomic mass but different atomic numbers.
The two uses of isotopes are:
(i) As nuclear fuel: An isotope of uranium (U–235)(U–235) is used as a nuclear fuel.
(ii) An isotope of cobalt is used in the treatment of cancer.