How many stable isotopes are there in the nitrogen atom?

2

The correct answer is option (3) 2.

Isotopes of an element have the same number of protons (and thus the same atomic number), but they differ in their number of neutrons (and consequently their mass number). Nitrogen (symbol: N) has several isotopes, but only two of them are stable, meaning they do not undergo radioactive decay. Here's an explanation of the stable isotopes of nitrogen:

1. Nitrogen-14 \((^{14}N)\):

Nitrogen-14 is the most abundant and stable isotope of nitrogen. It consists of 7 protons and 7 neutrons. This isotope makes up approximately 99.6% of naturally occurring nitrogen. Nitrogen-14 is the predominant form of nitrogen found in the Earth's atmosphere and in most nitrogen-containing compounds.

2. Nitrogen-15 \((^{15}N)\):

Nitrogen-15 is the other stable isotope of nitrogen. It consists of 7 protons and 8 neutrons. Although less abundant than nitrogen-14, nitrogen-15 still occurs naturally and makes up about 0.4% of naturally occurring nitrogen. Nitrogen-15 is often used in scientific research, particularly in isotopic labeling experiments and studies of nitrogen cycling in ecosystems.

These stable isotopes of nitrogen have similar chemical properties since they have the same number of protons and electrons, which determine the element's chemical behavior. However, they differ in their atomic masses due to their varying numbers of neutrons.

Other isotopes of nitrogen, such as nitrogen-12 \((^{12}N)\), nitrogen-13 \((^{13}N)\), and nitrogen-16 \((^{16}N)\), are unstable and undergo radioactive decay, making them less prevalent in nature and less relevant for everyday applications.