explain with example
(I) atomic number (ii) Mass number (iii)isotopes and(iv) isobars
Answers
i) Atomic number is the total number of protons present in the nucleus of an atom. It is also equal to the number of electrons for a neutral atom.
Example, atomic number of sodium is 11.
ii) Mass number is the number of protons and neutrons in the nucleus taken together.
For example, mass number of sodium is 23 g/mol.
iii) Isotopes are elements with the same atomic number but different mass numbers.
Example, hydrogen has 3 isotopes - protium (1H1), deuterium (2H1) and tritium (3H1).
iv) Isobars are elemnts which have different atomic numbers but the same mass number. They are different chemical elements.
Example, iron and nickel, both have mass number 58, whereas atomic numbers are different.
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Answer:
(i) Atomic number: The atomic number is the total number of protons present in the atom. For example, the atomic number of Mg is 12. ... For example, the atomic number of Lithium is 4 which is equal to the number of protons, the number of neutrons of magnesium is 4. The mass number is equal to 8(4+4).
(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 4 which is equal to the number of protons, the number of neutrons of magnesium is 4. The mass number is equal to 8(4+4).
(iii)The number of nucleons (both protons and neutrons) in the nucleus is the atom's mass number, and each isotope of a given element has a different mass number. For example, carbon-12, carbon-13, and carbon-14 are three isotopes of the element carbon with mass numbers 12, 13, and 14, respectively.
(iv)Isobars are atoms (nuclides) of different chemical elements that have the same number of nucleons. ... An example of a series of isobars would be 40S, 40Cl, 40Ar, 40K, and 40Ca. While the nuclei of these nuclides all contain 40 nucleons, they contain varying numbers of protons and neutrons.
Explanation: