To determine the number of electrons in the nitrogen-14 isotope, we need to follow these steps:
1. Identify the atomic number and mass number:
- The atomic number (the subscript, 7) represents the number of protons in the atom. For nitrogen-14 (with the symbol [tex]\(^7 N^{14}\)[/tex]), this number is 7.
2. Determine the number of electrons in a neutral atom:
- In a neutral atom, the number of electrons is equal to the number of protons. This is because the positive charge of the protons is exactly balanced by the negative charge of the electrons, resulting in no net charge.
3. Relate the given information:
- We have [tex]\( 7 \)[/tex] protons in nitrogen-14. Therefore, the number of electrons must also be [tex]\( 7 \)[/tex] to maintain electrical neutrality.
So, nitrogen-14 has:
- 7 protons [tex]\((7 p^+)\)[/tex]
- 7 electrons [tex]\((7 e^-)\)[/tex]
- The number of neutrons can be calculated as [tex]\( 14 - 7 = 7 \)[/tex] neutrons [tex]\((7 n^0)\)[/tex], though the number of neutrons is not needed to answer the electron question directly.
Hence, the nitrogen-14 isotope has 7 electrons.
