Isotopes

Introduction

• Isotopes are atoms of the same chemical element that have different mass numbers.
• They share the same number of protons in their nuclei, ensuring they remain the same element.

Atomic Structure

• Each element is defined by its atomic number (Z), representing the number of protons in its nucleus.
• For example, carbon (C) has an atomic number of 6, indicating it has 6 protons.

Mass Number (A)

• The mass number is the sum of protons and neutrons in the nucleus of an atom.
• It is displayed at the top-left corner of an element's symbol.
• Example: Carbon-12 (12C) has a mass number of 12, while carbon-14 (14C) has a mass number of 14.

Isotopes Defined

• Isotopes are atoms of the same element (same atomic number) but with different mass numbers.
• They differ in the number of neutrons they contain.
• For example, both carbon-12 (12C) and carbon-14 (14C) have the same atomic number (6 protons) but varying numbers of neutrons.

Variation in Neutron Count

• The variation in mass numbers between isotopes arises from differences in neutron counts.
• Carbon-12 (12C) has 6 neutrons, while carbon-14 (14C) has 8 neutrons.

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Isotopes

Significance of Isotopes

• Isotopes can have different physical properties, such as stability or radioactivity, due to their varying neutron counts.
• They are widely used in fields like radiometric dating, nuclear medicine, and scientific research.

In Summary

• Isotopes are atoms of the same element with different mass numbers, sharing the same number of protons.
• The mass number represents the sum of protons and neutrons in an atom's nucleus.
• Differences in neutron counts give rise to varying mass numbers and isotopes.
• Isotopes have practical applications in various scientific and medical fields.