parts of an isotope and ion\nuse the atomic symbol to fill in the blanks in the table. determine whether its…

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.