atomic structure
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.
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Question

Accepted Answer

# Explanation:
## Step1: Recall atomic structure facts
Atomic number = number of protons. Mass number = number of protons + number of neutrons. For neutral atoms, number of electrons = number of protons. For ions, adjust electrons based on charge. Isotopes have same atomic number but different mass numbers.
## Step2: Analyze $_1^2H$
Atomic number = 1 (from sub - script), so number of protons = 1. Mass number = 2 (from super - script), number of neutrons = mass number - number of protons = 2 - 1=1. For neutral $_1^2H$, number of electrons = 1. It is an isotope as it has a different mass number from the most common hydrogen ($_1^1H$). Ionic charge = 0.
## Step3: Analyze $_4^9Be$
Atomic number = 4, so number of protons = 4. Mass number = 9, number of neutrons = 9 - 4 = 5. For neutral atom, number of electrons = 4. It is an isotope as there are other beryllium isotopes. Ionic charge = 0.
## Step4: Analyze $_ {26}^{57}Fe$
Atomic number = 26, so number of protons = 26. Mass number = 57, number of neutrons = 57 - 26 = 31. For neutral atom, number of electrons = 26. It is an isotope. Ionic charge = 0.
## Step5: Analyze $_3^7Li^+$
Atomic number = 3, so 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, so number of protons = 8. Mass number = 16, number of neutrons = 16 - 8 = 8. For neutral atom, number of electrons = 8. It is an isotope. Ionic charge = 0.
## Step7: Analyze $_ {26}^{54}Fe$
Atomic number = 26, so number of protons = 26. Mass number = 54, number of neutrons = 54 - 26 = 28. For neutral atom, number of electrons = 26. It is an isotope. Ionic charge = 0.
## Step8: Analyze $_7^{14}N^{3 - }$
Atomic number = 7, so 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, so number of protons = 79. Mass number = 197, number of neutrons = 197 - 79 = 118. For neutral atom, number of electrons = 79. It is an isotope. Ionic charge = 0.
## Step10: Analyze $_ {17}^{37}Cl$
Atomic number = 17, so number of protons = 17. Mass number = 37, number of neutrons = 37 - 17 = 20. For neutral atom, number of electrons = 17. It is an isotope. Ionic charge = 0.
## Step11: Analyze $_ {12}^{26}Mg^{2 + }$
Atomic number = 12, so 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, so number of protons = 22. Mass number = 50, number of neutrons = 50 - 22 = 28. For neutral atom, number of electrons = 22. It is an isotope. Ionic charge = 0.
## Step13: Analyze $_ {15}^{33}P$
Atomic number = 15, so number of protons = 15. Mass number = 33, number of neutrons = 33 - 15 = 18. For neutral atom, number of electrons = 15. It is an isotope. Ionic charge = 0.
## Step14: Analyze $_ {15}^{33}P^+$
Atomic number = 15, so number of protons = 15. Mass number = 33, number of neutrons = 33 - 15 = 18. Since it has a + 1 charge, number of electrons = 15 - 1 = 14. It is an ion. Ionic charge = + 1.
## Step15: Analyze $_ {29}^{63}Cu$
Atomic number = 29, so number of protons = 29. Mass number = 63, number of neutrons = 63 - 29 = 34. For neutral atom, number of electrons = 29. It is an isotope. Ionic charge = 0.
## Step16: Analyze $_ {35}^{80}Br^-$
Atomic number = 35, so 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.
## Step17: Analyze $_ {13}^{27}Al^{3 + }$
Atomic number = 13, so 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.
## Step18: Analyze $_6^{13}C$
Atomic number = 6, so number of protons = 6. Mass number = 13, number of neutrons = 13 - 6 = 7. For neutral atom, number of electrons = 6. It is an isotope. Ionic charge = 0.
## Step19: Analyze $_ {14}^{29}Si$
Atomic number = 14, so number of protons = 14. Mass number = 29, number of neutrons = 29 - 14 = 15. For neutral atom, number of electrons = 14. It is an isotope. Ionic charge = 0.
## Step20: Analyze $_ {20}^{40}Ar$
Atomic number = 20, so number of protons = 20. Mass number = 40, number of neutrons = 40 - 20 = 20. For neutral atom, number of electrons = 20. It is an isotope. Ionic charge = 0.
## Step21: Analyze $_ {16}^{32}S^{2 - }$
Atomic number = 16, so 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.
## Step22: Analyze $_ {11}^{23}Na^+$
Atomic number = 11, so 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.

# Answer:
| Atomic Symbol | Atomic Number | Mass Number | # of Protons | # of Neutrons | # of Electrons | Isotope or Ion? | Ionic Charge |
|---|---|---|---|---|---|---|---|
| $_1^2H$ | 1 | 2 | 1 | 1 | 1 | Isotope | 0 |
| $_4^9Be$ | 4 | 9 | 4 | 5 | 4 | Isotope | 0 |
| $_ {26}^{57}Fe$ | 26 | 57 | 26 | 31 | 26 | Isotope | 0 |
| $_3^7Li^+$ | 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 |
| $_ {15}^{33}P^+$ | 15 | 33 | 15 | 18 | 14 | Ion | + 1 |
| $_ {29}^{63}Cu$ | 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 |
| $_ {20}^{40}Ar$ | 20 | 40 | 20 | 20 | 20 | Isotope | 0 |
| $_ {16}^{32}S^{2 - }$ | 16 | 32 | 16 | 16 | 18 | Ion | - 2 |
| $_ {11}^{23}Na^+$ | 11 | 23 | 11 | 12 | 10 | Ion | + 1 |

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Question

Explanation:

Step1: Recall atomic structure facts

Step2: Analyze $_1^2H$

Step3: Analyze $_4^9Be$

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

Step5: Analyze $_3^7Li^+$

Step6: Analyze $_8^{16}O$

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

Step8: Analyze $_7^{14}N^{3 - }$

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

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

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

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

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

Step14: Analyze $_ {15}^{33}P^+$

Step15: Analyze $_ {29}^{63}Cu$

Step16: Analyze $_ {35}^{80}Br^-$

Answer:

Atomic Symbol	Atomic Number	Mass Number	# of Protons	# of Neutrons	# of Electrons	Isotope or Ion?	Ionic Charge
$_4^9Be$	4	9	4	5	4	Isotope	0
$_ {26}^{57}Fe$	26	57	26	31	26	Isotope	0
$_3^7Li^+$	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
$_ {15}^{33}P^+$	15	33	15	18	14	Ion	+ 1
$_ {29}^{63}Cu$	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
$_ {20}^{40}Ar$	20	40	20	20	20	Isotope	0
$_ {16}^{32}S^{2 - }$	16	32	16	16	18	Ion	- 2
$_ {11}^{23}Na^+$	11	23	11	12	10	Ion	+ 1