Explain with examples (i) Atomic number,(ii) | vedclass

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(A) $(i)$ Atomic number: The atomic number of an element is defined as the total number of protons present in the nucleus of an atom of that element.

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Atomic number definition with example.

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(A) $(i)$ Atomic number: The atomic number of an element is defined as the total number of protons present in the nucleus of an atom of that element. It is denoted by $Z$. For example,a nitrogen atom contains $7$ protons,so its atomic number is $7$.$(ii)$ Mass number: The mass number of an element is the sum of the total number of protons and neutrons present in the nucleus of an atom of that element. It is denoted by $A$. For example,a boron atom has $5$ protons and $6$ neutrons,so its mass number is $5 + 6 = 11$.Uses of isotopes:$1$. An isotope of uranium is used as a fuel in nuclear reactors.$2$. An isotope of iodine is used in the treatment of goitre.

Atomic Number	Mass Number	Number of Neutrons	Number of Protons	Number of Electrons	Name of the Atomic Species
$9$	-	$10$	-	-	-
$16$	$32$	-	-	-	sulphur
-	$24$	-	$12$	-	-
-	$2$	-	$1$	-	-
-	$1$	$0$	$1$	$0$	-

Explain with examples $(i)$ Atomic number,$(ii)$ Mass number. Give any two uses of isotopes.

Similar Questions

Complete the following table.

Atomic Number Mass Number Number of Neutrons Number of Protons Number of Electrons Name of the Atomic Species

$9$ - $10$ - - -

$16$ $32$ - - - sulphur

- $24$ - $12$ - -

- $2$ - $1$ - -

- $1$ $0$ $1$ $0$ -

Find out the mass number of oxygen and sulphur atoms.

Compare the properties of electrons,protons,and neutrons.

Rutherford's alpha-particle scattering experiment was responsible for the discovery of

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