Isotopy

SS1: CHEMISTRY – 1ST TERM Particulate Nature of Matter II | Week 6 Isotopy

Lesson 6, Topic 3

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Isotopy

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Topic Content:

Meaning of Isotopy
Isotopes of Hydrogen
Isotopes of Some Common Elements

What is Isotopy?

Isotopy is a phenomenon whereby atoms of an element exhibit the same atomic number but different mass numbers. This is due to the difference in the number of neutrons present in these atoms.

Isotopes are atoms of the same element with the same atomic number but different mass numbers. Hydrogen, the lightest element, has three Isotopes.

Isotopes of Hydrogen:

Isotope	Number of Protons	Number of neutrons	Mass Number
Protium	1	–	1
Deuterium	1	1	2
Tritium	1	2	3

Isotopes of Some Common Elements:

Element	Number of Protons	Number of Neutrons	Mass Number	Isotope
Oxygen	8	8	16	\( \scriptsize _{8} ^{16} \textrm {0} \)
	8	9	17	\( \scriptsize _{8} ^{17} \textrm {0} \)
	8	10	18	\( \scriptsize _{8} ^{18} \textrm {0} \)
Carbon	6	6	12	\( \scriptsize _{6} ^{12} \textrm {C} \)
	6	7	13	\( \scriptsize _{6} ^{13} \textrm {C} \)
	6	8	14	\( \scriptsize _{6} ^{14} \textrm {C} \)
Neon	10	10	20	\( \scriptsize _{10} ^{20} \textrm {Ne} \)
	10	11	21	\( \scriptsize _{10} ^{21} \textrm {Ne} \)
	10	12	22	\( \scriptsize _{10} ^{22} \textrm {Ne} \)
Chlorine	17	18	35	\( \scriptsize _{17} ^{35} \textrm {Cl} \)
	17	20	37	\( \scriptsize _{17} ^{37} \textrm {Cl} \)

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