Filled-out chemistry worksheet detailing the atomic structure of various ions and isotopes.

It looks like you've uploaded a completed "Ions and Isotopes Worksheet" with all the answers filled in. However, since you're asking to "solve the problem and explain the solution," I’ll assume your goal is to understand how each value was determined — especially for students learning about atomic structure, ions, isotopes, and charge.

Let’s go through the key concepts and how each column was filled, using examples from the table.

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🔬 Key Concepts

1. Atomic Number (Z):
- The number of protons in the nucleus.
- Defines the element.
- For neutral atoms: # protons = # electrons.

2. Mass Number (A):
- Protons + Neutrons.
- Shown as superscript in notation (e.g., O-17 → mass number = 17).

3. Neutrons:
- Mass Number – Atomic Number = Neutrons.

4. Electrons:
- In neutral atoms: equal to protons.
- In ions: adjusted by charge:
- Positive charge → fewer electrons (lost electrons).
- Negative charge → more electrons (gained electrons).

5. Charge:
- Charge = (Protons) – (Electrons)

6. Isotopes:
- Atoms of the same element (same atomic number) but different mass numbers (different neutrons).

7. Ions:
- Charged atoms due to gain/loss of electrons.

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✔ Let's Walk Through Examples:

#### 1. Oxygen-17 (O-17)

| Column | Value | Explanation |
|-------|------|-----------|
| Symbol | O-17 | Oxygen isotope with mass number 17 |
| Element | Oxygen | Atomic number 8 |
| Atomic Number | 8 | From periodic table |
| Protons | 8 | Equal to atomic number |
| Neutrons | 9 | 17 (mass) – 8 (protons) = 9 |
| Electrons | 8 | Neutral atom → electrons = protons |
| Atomic Mass | 17 | Given in symbol |
| Charge | 0 | Neutral |

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#### 2. Sodium Ion (Na⁺)

| Column | Value | Explanation |
|-------|------|-----------|
| Symbol | Na⁺ | Sodium ion with +1 charge |
| Element | Sodium ion | Name includes “ion” |
| Atomic Number | 11 | Sodium has atomic number 11 |
| Protons | 11 | Same as atomic number |
| Neutrons | 12 | Mass number 23 – 11 = 12 |
| Electrons | 10 | Lost one electron → 11 – 1 = 10 |
| Atomic Mass | 23 | Standard isotope of sodium |
| Charge | +1 | Given by superscript |

> ✔ Charge = 11 – 10 = +1 ✔️

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#### 3. Aluminum Ion (Al³⁺)

| Column | Value | Explanation |
|-------|------|-----------|
| Symbol | Al³⁺ | Aluminum with +3 charge |
| Element | Aluminum ion | Name indicates it's an ion |
| Atomic Number | 13 | Aluminum's atomic number |
| Protons | 13 | Always equals atomic number |
| Neutrons | 14 | 27 (mass) – 13 = 14 |
| Electrons | 10 | Lost 3 electrons → 13 – 3 = 10 |
| Atomic Mass | 27 | Most common isotope |
| Charge | +3 | Given in symbol |

> ✔ Charge = 13 – 10 = +3 ✔️

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#### 4. Arsenic Ion (⁷⁵As⁻³)

| Column | Value | Explanation |
|-------|------|-----------|
| Symbol | ⁷⁵As⁻³ | Arsenic with mass 75 and -3 charge |
| Element | Arsenic | Atomic number 33 |
| Atomic Number | 33 | From periodic table |
| Protons | 33 | Equal to atomic number |
| Neutrons | 39 | 75 – 33 = 39 |
| Electrons | 36 | Gained 3 electrons → 33 + 3 = 36 |
| Atomic Mass | 75 | Given |
| Charge | -3 | Given |

> ✔ Charge = 33 – 36 = -3 ✔️

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#### 5. Sulfide Ion (³²S²⁻)

| Column | Value | Explanation |
|-------|------|-----------|
| Symbol | ³²S²⁻ | Sulfur with -2 charge |
| Element | Sulfide ion | Name indicates ion |
| Atomic Number | 16 | Sulfur’s atomic number |
| Protons | 16 | Equal to atomic number |
| Neutrons | 16 | 32 – 16 = 16 |
| Electrons | 18 | Gained 2 electrons → 16 + 2 = 18 |
| Atomic Mass | 32 | Given |
| Charge | -2 | Given |

> ✔ Charge = 16 – 18 = -2 ✔️

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#### 6. Nitride Ion (N³⁻)

| Column | Value | Explanation |
|-------|------|-----------|
| Symbol | N³⁻ | Nitrogen with -3 charge |
| Element | Nitride ion | Name indicates ion |
| Atomic Number | 7 | Nitrogen’s atomic number |
| Protons | 7 | Equal to atomic number |
| Neutrons | 7 | 14 – 7 = 7 |
| Electrons | 10 | Gained 3 electrons → 7 + 3 = 10 |
| Atomic Mass | 14 | Most common isotope |
| Charge | -3 | Given |

> ✔ Charge = 7 – 10 = -3 ✔️

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#### 7. Copper (⁶⁵Cu)

| Column | Value | Explanation |
|-------|------|-----------|
| Symbol | ⁶⁵Cu | Copper isotope |
| Element | Copper | Atomic number 29 |
| Atomic Number | 29 | From periodic table |
| Protons | 29 | Equal to atomic number |
| Neutrons | 36 | 65 – 29 = 36 |
| Electrons | 29 | Neutral atom → equal to protons |
| Atomic Mass | 65 | Given |
| Charge | 0 | Neutral |

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#### 8. Mercury Isotope (¹²⁰Hg)

| Column | Value | Explanation |
|-------|------|-----------|
| Symbol | ¹²⁰Hg | Mercury isotope with mass 120 |
| Element | Mercury isotope | Not standard; likely artificial |
| Atomic Number | 80 | Mercury’s atomic number |
| Protons | 80 | Equal to atomic number |
| Neutrons | 40 | 120 – 80 = 40 |
| Electrons | 80 | Neutral atom |
| Atomic Mass | 120 | Given |
| Charge | 0 | Neutral |

> Note: This is not the most common isotope (common is Hg-200), but it's valid.

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#### 9. Zirconium (Zr)

| Column | Value | Explanation |
|-------|------|-----------|
| Symbol | Zr | Element symbol |
| Element | zirconium | Name |
| Atomic Number | 40 | Known from periodic table |
| Protons | 40 | Equal to atomic number |
| Neutrons | 51 | 91 – 40 = 51 |
| Electrons | 91 | Wait! This is incorrect! ✘

> ⚠️ Mistake in the worksheet?

Let’s check:
- Atomic Mass = 40? That can’t be right.
- But atomic mass is listed as 40, which is less than atomic number (40).
- Mass number must be ≥ atomic number.

Wait — this row has:
- Symbol: Zr
- Atomic Mass: 40
- Protons: 40
- Neutrons: 51
- Electrons: 91

This is impossible because:
- Neutrons = 51 → mass number = 40 + 51 = 91
- But atomic mass is listed as 40, which contradicts.

So either:
- The atomic mass should be 91, or
- The neutrons are wrong.

But wait — electrons = 91? That’s impossible for Zr (only 40 protons).

✔ This row appears to have errors.

Let’s re-evaluate:

If Zr has:
- Atomic number = 40 → 40 protons
- If neutral → 40 electrons
- If atomic mass = 91 → then neutrons = 91 – 40 = 51

Then:
- Electrons = 40 (not 91)
- Atomic mass = 91 (not 40)

So likely typo:
✔ Corrected values:
- Atomic Mass: 91
- Electrons: 40
- Charge: 0

But the worksheet says:
- Atomic Mass: 40
- Electrons: 91

✘ This is incorrect.

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🛠 Summary of Corrections Needed

| Symbol | Error | Corrected |
|--------|-------|----------|
| Zr | Atomic Mass = 40, Electrons = 91 | Should be: Atomic Mass = 91, Electrons = 40 |

> This appears to be a typo in the worksheet.

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✔ Final Notes

- All other rows are correctly filled.
- The only error is likely in the Zirconium row.
- For ions: adjust electrons based on charge.
- For isotopes: mass number = protons + neutrons.
- Atomic number = number of protons always.

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✔ How to Solve These Problems Step-by-Step

1. Find the atomic number from the element name or symbol.
2. Number of protons = atomic number.
3. Mass number is given in the symbol (e.g., O-17 → 17).
4. Neutrons = mass number – atomic number.
5. Electrons:
- If neutral: electrons = protons
- If ion: electrons = protons – charge (e.g., Na⁺ → 11 – 1 = 10)
6. Charge = protons – electrons

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✔ Final Answer

The worksheet is mostly correct, except for the Zirconium (Zr) row, which contains errors:

- Atomic Mass should be 91, not 40
- Electrons should be 40, not 91

✔ Corrected Row:

| Symbol | Name | Atomic Number | Protons | Neutrons | Electrons | Atomic Mass | Charge |
|--------|------|---------------|---------|----------|-----------|-------------|--------|
| Zr | zirconium | 40 | 40 | 51 | 40 | 91 | 0 |

All other entries are accurate.

Let me know if you'd like a version of this worksheet corrected and printable!