Write the atomic weight of chlorine isotopes.

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Solution

There are two principal stable isotopes of Chlorine. They are ${C l}^{35}$ and ${C l}^{37}$ . Their respective atomic weights are $35$ and $37$ .

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Naturally occurring chlorine consists of two isotopes whose atomic weights are 35 and 37. The atomic weight of natural chlorine is 35.5, then what is the ratio of $C l^{35} t o C l^{37}$ ?

Q. It can be shown using mass spectrometry that the ratio of naturally occurring chlorine -35 to its isotope chlorine -37 is 3 : 1. Assuming that no other isotopes existed, what would be the atomic weight of chlorine?

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Q. Consider the following isotopes of chlorine:

_{17} C l^{35},_{17} C l^{37}

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Atomic masses of these isotopes are different, while their chemical properties are same. In the Mendeleev's periodic table isotopes of chlorine was placed:

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Write the atomic weight of chlorine isotopes.

There are two principal stable isotopes of Chlorine. They are Cl35 and Cl37. Their respective atomic weights are 35 and 37.

There are two principal stable isotopes of Chlorine. They are ${C l}^{35}$ and ${C l}^{37}$ . Their respective atomic weights are $35$ and $37$ .