Question

parts of an isotope and ion
use the atomic symbol to fill in the blanks in the table. determine whether its an isotope or an ion and its ionic charge.
atomic number mass number # of protons # of neutrons # of electrons isotope or ion? ionic charge
score:_____/20

Explanation:

Step1: Recall atomic number and mass number concepts

The atomic number (sub - script) is the number of protons. The mass number (super - script) is the sum of protons and neutrons. For neutral atoms, the number of electrons equals the number of protons. For ions, adjust the number of electrons based on the charge. Isotopes are atoms of the same element with different numbers of neutrons.

Step2: Analyze $_{1}^{2}H$

Atomic number = 1, so number of protons = 1. Mass number = 2, number of neutrons = mass number - number of protons = 2 - 1=1. For neutral $_{1}^{2}H$, number of electrons = 1. It is an isotope (of hydrogen). Ionic charge = 0.

Step3: Analyze $_{4}^{9}Be$

Atomic number = 4, number of protons = 4. Mass number = 9, number of neutrons = 9 - 4 = 5. For neutral $_{4}^{9}Be$, number of electrons = 4. It is an isotope (of beryllium). Ionic charge = 0.

Step4: Analyze $_{26}^{57}Fe$

Atomic number = 26, number of protons = 26. Mass number = 57, number of neutrons = 57 - 26 = 31. For neutral $_{26}^{57}Fe$, number of electrons = 26. It is an isotope (of iron). Ionic charge = 0.

Step5: Analyze $_{3}^{7}Li^{+}$

Atomic number = 3, number of protons = 3. Mass number = 7, number of neutrons = 7 - 3 = 4. Since it has a + 1 charge, number of electrons = 3 - 1=2. It is an ion. Ionic charge = + 1.

Step6: Analyze $_{8}^{16}O$

Atomic number = 8, number of protons = 8. Mass number = 16, number of neutrons = 16 - 8 = 8. For neutral $_{8}^{16}O$, number of electrons = 8. It is an isotope (of oxygen). Ionic charge = 0.

Step7: Analyze $_{26}^{54}Fe$

Atomic number = 26, number of protons = 26. Mass number = 54, number of neutrons = 54 - 26 = 28. For neutral $_{26}^{54}Fe$, number of electrons = 26. It is an isotope (of iron). Ionic charge = 0.

Step8: Analyze $_{7}^{14}N^{3 - }$

Atomic number = 7, number of protons = 7. Mass number = 14, number of neutrons = 14 - 7 = 7. Since it has a - 3 charge, number of electrons = 7+3 = 10. It is an ion. Ionic charge = - 3.

Step9: Analyze $_{79}^{197}Au$

Atomic number = 79, number of protons = 79. Mass number = 197, number of neutrons = 197 - 79 = 118. For neutral $_{79}^{197}Au$, number of electrons = 79. It is an isotope (of gold). Ionic charge = 0.

Step10: Analyze $_{17}^{37}Cl$

Atomic number = 17, number of protons = 17. Mass number = 37, number of neutrons = 37 - 17 = 20. For neutral $_{17}^{37}Cl$, number of electrons = 17. It is an isotope (of chlorine). Ionic charge = 0.

Step11: Analyze $_{12}^{26}Mg^{2+}$

Atomic number = 12, number of protons = 12. Mass number = 26, number of neutrons = 26 - 12 = 14. Since it has a + 2 charge, number of electrons = 12 - 2 = 10. It is an ion. Ionic charge = + 2.

Step12: Analyze $_{22}^{50}Ti$

Atomic number = 22, number of protons = 22. Mass number = 50, number of neutrons = 50 - 22 = 28. For neutral $_{22}^{50}Ti$, number of electrons = 22. It is an isotope (of titanium). Ionic charge = 0.

Step13: Analyze $_{15}^{33}P$

Atomic number = 15, number of protons = 15. Mass number = 33, number of neutrons = 33 - 15 = 18. For neutral $_{15}^{33}P$, number of electrons = 15. It is an isotope (of phosphorus). Ionic charge = 0.

Step14: Analyze $_{29}^{63}Cu$

Atomic number = 29, number of protons = 29. Mass number = 63, number of neutrons = 63 - 29 = 34. For neutral $_{29}^{63}Cu$, number of electrons = 29. It is an isotope (of copper). Ionic charge = 0.

Step15: Analyze $_{35}^{80}Br^{-}$

Atomic number = 35, number of protons = 35. Mass number = 80, number of neutrons = 80 - 35 = 45. Since it has a - 1 charge, number of electrons = 35 + 1 = 36. It is an ion. Ionic charge = - 1.

Step16: Analyze $_{13}^{27}Al^{3+}$

Atomic number = 13, number of protons = 13. Mass number = 27, number of neutrons = 27 - 13 = 14. Since it has a + 3 charge, number of electrons = 13 - 3 = 10. It is an ion. Ionic charge = + 3.

Step17: Analyze $_{6}^{13}C$

Atomic number = 6, number of protons = 6. Mass number = 13, number of neutrons = 13 - 6 = 7. For neutral $_{6}^{13}C$, number of electrons = 6. It is an isotope (of carbon). Ionic charge = 0.

Step18: Analyze $_{14}^{29}Si$

Atomic number = 14, number of protons = 14. Mass number = 29, number of neutrons = 29 - 14 = 15. For neutral $_{14}^{29}Si$, number of electrons = 14. It is an isotope (of silicon). Ionic charge = 0.

Step19: Analyze $_{18}^{40}Ar$

Atomic number = 18, number of protons = 18. Mass number = 40, number of neutrons = 40 - 18 = 22. For neutral $_{18}^{40}Ar$, number of electrons = 18. It is an isotope (of argon). Ionic charge = 0.

Step20: Analyze $_{16}^{32}S^{2 - }$

Atomic number = 16, number of protons = 16. Mass number = 32, number of neutrons = 32 - 16 = 16. Since it has a - 2 charge, number of electrons = 16+2 = 18. It is an ion. Ionic charge = - 2.

Step21: Analyze $_{11}^{23}Na^{+}$

Atomic number = 11, number of protons = 11. Mass number = 23, number of neutrons = 23 - 11 = 12. Since it has a + 1 charge, number of electrons = 11 - 1 = 10. It is an ion. Ionic charge = + 1.

| Atomic Symbol | Atomic Number | Mass Number | # of Protons | # of Neutrons | # of Electrons | Isotope or Ion? | Ionic Charge |
|---|---|---|---|---|---|---|---|
| $_{1}^{2}H$ | 1 | 2 | 1 | 1 | 1 | Isotope | 0 |
| $_{4}^{9}Be$ | 4 | 9 | 4 | 5 | 4 | Isotope | 0 |
| $_{26}^{57}Fe$ | 26 | 57 | 26 | 31 | 26 | Isotope | 0 |
| $_{3}^{7}Li^{+}$ | 3 | 7 | 3 | 4 | 2 | Ion | + 1 |
| $_{8}^{16}O$ | 8 | 16 | 8 | 8 | 8 | Isotope | 0 |
| $_{26}^{54}Fe$ | 26 | 54 | 26 | 28 | 26 | Isotope | 0 |
| $_{7}^{14}N^{3 - }$ | 7 | 14 | 7 | 7 | 10 | Ion | - 3 |
| $_{79}^{197}Au$ | 79 | 197 | 79 | 118 | 79 | Isotope | 0 |
| $_{17}^{37}Cl$ | 17 | 37 | 17 | 20 | 17 | Isotope | 0 |
| $_{12}^{26}Mg^{2+}$ | 12 | 26 | 12 | 14 | 10 | Ion | + 2 |
| $_{22}^{50}Ti$ | 22 | 50 | 22 | 28 | 22 | Isotope | 0 |
| $_{15}^{33}P$ | 15 | 33 | 15 | 18 | 15 | Isotope | 0 |
| $_{29}^{63}Cu$ | 29 | 63 | 29 | 34 | 29 | Isotope | 0 |
| $_{35}^{80}Br^{-}$ | 35 | 80 | 35 | 45 | 36 | Ion | - 1 |
| $_{13}^{27}Al^{3+}$ | 13 | 27 | 13 | 14 | 10 | Ion | + 3 |
| $_{6}^{13}C$ | 6 | 13 | 6 | 7 | 6 | Isotope | 0 |
| $_{14}^{29}Si$ | 14 | 29 | 14 | 15 | 14 | Isotope | 0 |
| $_{18}^{40}Ar$ | 18 | 40 | 18 | 22 | 18 | Isotope | 0 |
| $_{16}^{32}S^{2 - }$ | 16 | 32 | 16 | 16 | 18 | Ion | - 2 |
| $_{11}^{23}Na^{+}$ | 11 | 23 | 11 | 12 | 10 | Ion | + 1 |

Answer:

See the above - filled table.