The number of neutrons present in a nitrogen atom is ________.
7
Understanding the Number of Neutrons in a Nitrogen Atom
To find the number of neutrons in an atom, we need to know its atomic number and its mass number. The atomic number tells us the number of protons, and the mass number is the total number of protons and neutrons in the nucleus.
Key Concepts: Atomic Number and Mass Number
- Atomic Number (Z): This is unique to each element and equals the number of protons in the nucleus of an atom of that element. For a neutral atom, the number of electrons also equals the atomic number.
- Mass Number (A): This is the total number of protons and neutrons in the nucleus of a specific isotope of an element.
- Neutrons: These are neutral particles found in the nucleus. The number of neutrons can vary for atoms of the same element, leading to different isotopes.
Calculating the Number of Neutrons
The number of neutrons in an atom is calculated by subtracting the atomic number (number of protons) from the mass number (total number of protons and neutrons).
The formula is:
\(\text{Number of Neutrons} = \text{Mass Number} - \text{Atomic Number}\)
Or, using symbols:
\(N = A - Z\)
Applying the Formula to Nitrogen
Nitrogen is element number 7 on the periodic table. This means its atomic number (Z) is 7. The most common isotope of nitrogen is Nitrogen-14 (\(^{14}\text{N}\)), which has a mass number (A) of 14.
| Property | Value for Nitrogen-14 |
|---|---|
| Atomic Number (Z) | 7 (Number of protons) |
| Mass Number (A) | 14 (Protons + Neutrons) |
Now, we can use the formula to find the number of neutrons in a nitrogen atom (Nitrogen-14 isotope):
\(\text{Number of Neutrons} = \text{Mass Number} - \text{Atomic Number}\)
\(\text{Number of Neutrons} = 14 - 7\)
\(\text{Number of Neutrons} = 7\)
Therefore, a nitrogen atom (specifically the Nitrogen-14 isotope) contains 7 neutrons.
Conclusion: Neutrons in Nitrogen
Based on the atomic and mass numbers for the most common isotope of nitrogen (\(^{14}\text{N}\)), the number of neutrons is 7.
Revision Table: Atomic Structure
| Particle | Location in Atom | Charge | Determines |
|---|---|---|---|
| Proton | Nucleus | +1 | Element Identity (Atomic Number) |
| Neutron | Nucleus | 0 (Neutral) | Isotope (along with protons) |
| Electron | Orbiting Nucleus | -1 | Chemical Properties, Ion Charge |
Additional Information: Nitrogen Isotopes and Neutron Count
While Nitrogen-14 is the most common isotope, nitrogen also exists as other isotopes. For example, Nitrogen-15 (\(^{15}\text{N}\)) is another stable isotope used in scientific studies.
- For \(^{15}\text{N}\):
- Atomic Number (Z) = 7 (still nitrogen)
- Mass Number (A) = 15
- Number of Neutrons = \(A - Z = 15 - 7 = 8\) neutrons
The question refers to "a nitrogen atom" without specifying an isotope. In general chemistry contexts, unless otherwise stated, properties often refer to the most abundant isotope or the average atomic mass. However, the options provided correspond directly to a specific number of neutrons (7 or 8 would be typical possibilities based on common isotopes). Since 7 is an option and corresponds to the abundant Nitrogen-14, this is the intended answer.
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