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
14 7n
35 17cl
43 20ca
7 3li+
56 26fe
39 19k
12 6c
11 5b3+
4 2he
80 35br-
32 16s2-
8 3li+
55 24mn
40 20ar
3 1h
79 34se
195 78pt
27 13al3+
23na
28 14si
score: ____/20

Explanation:

Step1: Recall atomic number and mass number concepts

The atomic number (sub - script in atomic symbol) is the number of protons. The mass number (super - script in atomic symbol) is the sum of protons and neutrons. For a neutral atom, the number of electrons equals the number of protons. For an ion, the number of electrons is adjusted according to the ionic charge.

Step2: Analyze $^{14}_{7}N$

Atomic number = 7, so number of protons = 7. Mass number = 14, number of neutrons = 14 - 7=7. For neutral $N$, number of electrons = 7. It is a neutral atom (not an ion), so it's an isotope. Ionic charge = 0.

Step3: Analyze $^{35}_{17}Cl$

Atomic number = 17, protons = 17. Mass number = 35, neutrons = 35 - 17 = 18. For neutral $Cl$, electrons = 17. It's an isotope, ionic charge = 0.

Step4: Analyze $^{43}_{20}Ca$

Atomic number = 20, protons = 20. Mass number = 43, neutrons = 43 - 20 = 23. For neutral $Ca$, electrons = 20. It's an isotope, ionic charge = 0.

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

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

Step6: Analyze $^{56}_{26}Fe$

Atomic number = 26, protons = 26. Mass number = 56, neutrons = 56 - 26 = 30. For neutral $Fe$, electrons = 26. It's an isotope, ionic charge = 0.

Step7: Analyze $^{39}_{19}K$

Atomic number = 19, protons = 19. Mass number = 39, neutrons = 39 - 19 = 20. For neutral $K$, electrons = 19. It's an isotope, ionic charge = 0.

Step8: Analyze $^{12}_{6}C$

Atomic number = 6, protons = 6. Mass number = 12, neutrons = 12 - 6 = 6. For neutral $C$, electrons = 6. It's an isotope, ionic charge = 0.

Step9: Analyze $^{11}_{5}B^{3 + }$

Atomic number = 5, protons = 5. Mass number = 11, neutrons = 11 - 5 = 6. Since it has a + 3 charge, electrons = 5 - 3 = 2. It's an ion, ionic charge = + 3.

Step10: Analyze $^{4}_{2}He$

Atomic number = 2, protons = 2. Mass number = 4, neutrons = 4 - 2 = 2. For neutral $He$, electrons = 2. It's an isotope, ionic charge = 0.

Step11: Analyze $^{80}_{35}Br^{-}$

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

Step12: Analyze $^{32}_{16}S^{2 - }$

Atomic number = 16, protons = 16. Mass number = 32, neutrons = 32 - 16 = 16. Since it has a - 2 charge, electrons = 16 + 2 = 18. It's an ion, ionic charge = - 2.

Step13: Analyze $^{8}_{3}Li^{+}$

Atomic number = 3, protons = 3. Mass number = 8, neutrons = 8 - 3 = 5. Since it has a + 1 charge, electrons = 3 - 1 = 2. It's an ion, ionic charge = + 1.

Step14: Analyze $^{55}_{24}Mn$

Atomic number = 24, protons = 24. Mass number = 55, neutrons = 55 - 24 = 31. For neutral $Mn$, electrons = 24. It's an isotope, ionic charge = 0.

Step15: Analyze $^{40}_{20}Ar$

Atomic number = 20, protons = 20. Mass number = 40, neutrons = 40 - 20 = 20. For neutral $Ar$, electrons = 20. It's an isotope, ionic charge = 0.

Step16: Analyze $^{3}_{1}H$

Atomic number = 1, protons = 1. Mass number = 3, neutrons = 3 - 1 = 2. For neutral $H$, electrons = 1. It's an isotope, ionic charge = 0.

Step17: Analyze $^{79}_{34}Se$

Atomic number = 34, protons = 34. Mass number = 79, neutrons = 79 - 34 = 45. For neutral $Se$, electrons = 34. It's an isotope, ionic charge = 0.

Step18: Analyze $^{195}_{78}Pt$

Atomic number = 78, protons = 78. Mass number = 195, neutrons = 195 - 78 = 117. For neutral $Pt$, electrons = 78. It's an isotope, ionic charge = 0.

Step19: Analyze $^{27}_{13}Al^{3 + }$

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

Step20: Analyze $^{23}_{11}Na$

Atomic number = 11, protons = 11. Mass number = 23, neutrons = 23 - 11 = 12. For neutral $Na$, electrons = 11. It's an isotope, ionic charge = 0.

Step21: Analyze $^{28}_{14}Si$

Atomic number = 14, protons = 14. Mass number = 28, neutrons = 28 - 14 = 14. For neutral $Si$, electrons = 14. It's an isotope, ionic charge = 0.

| Atomic Symbol | Atomic Number | Mass Number | # of Protons | # of Neutrons | # of Electrons | Isotope or ion? | Ionic Charge |
|---|---|---|---|---|---|---|---|
| $^{14}_{7}N$ | 7 | 14 | 7 | 7 | 7 | Isotope | 0 |
| $^{35}_{17}Cl$ | 17 | 35 | 17 | 18 | 17 | Isotope | 0 |
| $^{43}_{20}Ca$ | 20 | 43 | 20 | 23 | 20 | Isotope | 0 |
| $^{7}_{3}Li^{+}$ | 3 | 7 | 3 | 4 | 2 | Ion | + 1 |
| $^{56}_{26}Fe$ | 26 | 56 | 26 | 30 | 26 | Isotope | 0 |
| $^{39}_{19}K$ | 19 | 39 | 19 | 20 | 19 | Isotope | 0 |
| $^{12}_{6}C$ | 6 | 12 | 6 | 6 | 6 | Isotope | 0 |
| $^{11}_{5}B^{3 + }$ | 5 | 11 | 5 | 6 | 2 | Ion | + 3 |
| $^{4}_{2}He$ | 2 | 4 | 2 | 2 | 2 | Isotope | 0 |
| $^{80}_{35}Br^{-}$ | 35 | 80 | 35 | 45 | 36 | Ion | - 1 |
| $^{32}_{16}S^{2 - }$ | 16 | 32 | 16 | 16 | 18 | Ion | - 2 |
| $^{8}_{3}Li^{+}$ | 3 | 8 | 3 | 5 | 2 | Ion | + 1 |
| $^{55}_{24}Mn$ | 24 | 55 | 24 | 31 | 24 | Isotope | 0 |
| $^{40}_{20}Ar$ | 20 | 40 | 20 | 20 | 20 | Isotope | 0 |
| $^{3}_{1}H$ | 1 | 3 | 1 | 2 | 1 | Isotope | 0 |
| $^{79}_{34}Se$ | 34 | 79 | 34 | 45 | 34 | Isotope | 0 |
| $^{195}_{78}Pt$ | 78 | 195 | 78 | 117 | 78 | Isotope | 0 |
| $^{27}_{13}Al^{3 + }$ | 13 | 27 | 13 | 14 | 10 | Ion | + 3 |
| $^{23}_{11}Na$ | 11 | 23 | 11 | 12 | 11 | Isotope | 0 |
| $^{28}_{14}Si$ | 14 | 28 | 14 | 14 | 14 | Isotope | 0 |

Answer:

See the above - filled table.