Nitrogen has three occurring isotopes: Nitrogen-13, Nitrogen-14, Nitrogen-15.
The most abundance isotope is nitrogen-14 because of its stability and resistance to radioactive decay.
Isotopes are variants of a chemical element that have the same number of protons (which defines the element) but a different number of neutrons in their nuclei. This means that isotopes of the same element have slightly different atomic masses. In the case of nitrogen, its three naturally occurring isotopes are nitrogen-13 (N-13), nitrogen-14 (N-14), and nitrogen-15 (N-15).
The abundance of an isotope refers to the percentage of that isotope present in a naturally occurring sample of the element. The different isotopes of an element are usually found in different proportions, and the most abundant isotope is the one that appears most frequently in nature.
Nitrogen Isotopes:
a) Nitrogen-14 (N-14):
Nitrogen-14 is the most abundant isotope of nitrogen. It has 7 protons and 7 neutrons in its nucleus. N-14 makes up about 99.63% of naturally occurring nitrogen. This high abundance is primarily due to the relatively stable nuclear configuration of N-14, making it less prone to radioactive decay.
b) Nitrogen-15 (N-15):
Nitrogen-15 is the second most abundant isotope of nitrogen. It has 7 protons and 8 neutrons in its nucleus. N-15 makes up a much smaller percentage of naturally occurring nitrogen, around 0.37%. While N-15 is less abundant than N-14, it is still significant and plays a role in various scientific and environmental studies.
c) Nitrogen-13 (N-13):
Nitrogen-13 is the least abundant of the three naturally occurring nitrogen isotopes. It has 7 protons and 6 neutrons in its nucleus. N-13 is radioactive and is not as stable as N-14 and N-15.
The higher abundance of nitrogen-14 can be attributed to its relative stability compared to the other isotopes. The number of neutrons in an isotope's nucleus affects its stability, and N-14 has a balanced number of neutrons to maintain its stability. This stability prevents it from undergoing radioactive decay at a significant rate, allowing it to persist in higher proportions in nature.
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Explanation:
Nitrogen-14 is the most abundant isotopes of Nitrogen.
O B. Only in the home
C. Mostly outside
O D. Everywhere
Answer:
I believe the correct answer is D.
Explanation:
You are breathing in dinitrogen and dioxygen. You exhale dinitrogen and carbon dioxide. And the atmosphere contains traces of other gases. You drink water. You have a wash with water, and soap. You eat carbohydrates and proteins. You ride to work on a vehicle powered by hydrocarbons, which spits out carbon dioxide exhaust fumes, and also some nitrogen oxides. And so your exposure to chemicals is pervasive, and unavoidable.
Answer:
d
Explanation:
(2) are gained by the atoms
(3) return to lower energy states within the atoms
(4) move to higher energy states within the atoms
Answer:
Explanation:
Equilibrium position
Entropy
Keq
Answer:
entropy
Explanation:
gradpoint
b. the energy required to remove an electron from the element in its gaseous state
c. the energy released by the element in forming an ionic bond
d. the energy released by the element upon receiving an additional electron
e. none of the above
The ionization energy is energy required to remove an electron from element in it's gaseous state.
Ionization energy is defined as the minimum energy required to remove an electron from its valence shell of an isolated gaseous atom,positive ion or molecule.Ionization energy is positive for neutral atoms from which it can be concluded that ionization is an endothermic process.
Closer are the valence electrons to nucleus ,higher is the ionization energy.It is usually expressed in electron volts or joules.Ionization energy increases from left to right in a period as more energy is required to remove electrons with small atomic size.
Ionization energy decreases down the group as atomic size increases due to which electrons are easily lost from the valence shell.
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Answer:
According to the kinetic molecular theory, which statement describes the particles in a sample of an ideal gas? The motion of the gas particles is random and in a straight-line.
Explanation: