Ion isotope and atomic mass review worksheet - Free Printable
Educational worksheet: Ion isotope and atomic mass review worksheet. Download and print for classroom or home learning activities.
JPG
1000×1291
138.2 KB
Free · Personal Use
Quality Assured by Worksheets Library Team
Reviewed for educational accuracy and age-appropriateness
ID: #826907
⭐
Show Answer Key & Explanations
Step-by-step solution for: Ion isotope and atomic mass review worksheet
▼
Show Answer Key & Explanations
Step-by-step solution for: Ion isotope and atomic mass review worksheet
Let's solve this step-by-step. We'll go through each part of the worksheet and fill in the blanks with explanations.
---
We need to use the following key concepts:
- Atomic number (Z) = number of protons
- Mass number (A) = protons + neutrons
- Electrons = protons – charge (for ions), or equal to protons for neutral atoms
- Isotopic notation: $ ^{A}_{Z}X $
- Oxidation state tells us how many electrons are gained or lost
---
#### Row 1: $^{106}_{47}\text{Ag}^{+1}$
- Isotopic Notation: $^{106}_{47}\text{Ag}^{+1}$
- Isotope Name: Silver-106
- Oxidation #: +1 (given)
- Atomic Number: 47 (from subscript)
- Number Protons: 47 (same as atomic number)
- Number Neutrons: Mass # – protons = 106 – 47 = 59
- Number Electrons: Protons – charge = 47 – 1 = 46
- Mass Number: 106 (superscript)
✔ Filled:
| Isotopic Notation | Isotope Name | Oxidation # | Atomic Number | Protons | Neutrons | Electrons | Mass Number |
|-------------------|--------------|-------------|---------------|---------|----------|-----------|-------------|
| $^{106}_{47}\text{Ag}^{+1}$ | Silver-106 | +1 | 47 | 47 | 59 | 46 | 106 |
---
#### Row 2: Sulfur-34, Oxidation # = -2
- Isotope Name: Sulfur-34
- Oxidation #: -2 (given)
- Atomic Number: Sulfur has atomic number 16
- Protons: 16
- Mass Number: 34 (from name "Sulfur-34")
- Neutrons: 34 – 16 = 18
- Electrons: For ion with -2 charge → 16 + 2 = 18
- Isotopic Notation: $^{34}_{16}\text{S}^{-2}$
✔ Filled:
| Isotopic Notation | Isotope Name | Oxidation # | Atomic Number | Protons | Neutrons | Electrons | Mass Number |
|-------------------|--------------|-------------|---------------|---------|----------|-----------|-------------|
| $^{34}_{16}\text{S}^{-2}$ | Sulfur-34 | -2 | 16 | 16 | 18 | 18 | 34 |
---
#### Row 3: Oxidation # = 0, Protons = 10, Neutrons = 11
- Oxidation #: 0 → neutral atom
- Protons: 10 → Atomic number = 10 → Element is Neon (Ne)
- Neutrons: 11
- Mass Number: Protons + neutrons = 10 + 11 = 21
- Electrons: Same as protons = 10 (neutral)
- Isotope Name: Neon-21
- Isotopic Notation: $^{21}_{10}\text{Ne}$
✔ Filled:
| Isotopic Notation | Isotope Name | Oxidation # | Atomic Number | Protons | Neutrons | Electrons | Mass Number |
|-------------------|--------------|-------------|---------------|---------|----------|-----------|-------------|
| $^{21}_{10}\text{Ne}$ | Neon-21 | 0 | 10 | 10 | 11 | 10 | 21 |
---
#### Row 4: Electrons = 99, Mass Number = 155, Oxidation # = 0
- Oxidation # = 0 → neutral atom → electrons = protons
- So, protons = 99
- Atomic number = 99 → element is Einsteinium (Es)
- Mass number = 155 (given)
- Neutrons = 155 – 99 = 56
- Isotope Name: Einsteinium-155
- Isotopic Notation: $^{155}_{99}\text{Es}$
✔ Filled:
| Isotopic Notation | Isotope Name | Oxidation # | Atomic Number | Protons | Neutrons | Electrons | Mass Number |
|-------------------|--------------|-------------|---------------|---------|----------|-----------|-------------|
| $^{155}_{99}\text{Es}$ | Einsteinium-155 | 0 | 99 | 99 | 56 | 99 | 155 |
---
| Isotopic Notation | Isotope Name | Oxidation # | Atomic Number | Protons | Neutrons | Electrons | Mass Number |
|-------------------|--------------------|-------------|---------------|---------|----------|-----------|-------------|
| $^{106}_{47}\text{Ag}^{+1}$ | Silver-106 | +1 | 47 | 47 | 59 | 46 | 106 |
| $^{34}_{16}\text{S}^{-2}$ | Sulfur-34 | -2 | 16 | 16 | 18 | 18 | 34 |
| $^{21}_{10}\text{Ne}$ | Neon-21 | 0 | 10 | 10 | 11 | 10 | 21 |
| $^{155}_{99}\text{Es}$ | Einsteinium-155 | 0 | 99 | 99 | 56 | 99 | 155 |
---
Use:
- Atomic number = # protons
- Mass number = protons + neutrons
- Charge = protons – electrons → electrons = protons – charge
---
#### Row 5: Gain 1 e⁻, p⁺ = 85, mass # = 219
- Protons = 85 → element is Astatine (At)
- Gains 1 electron → becomes anion with charge -1 → formula: At⁻
- Electrons = 85 + 1 = 86
- Neutrons = 219 – 85 = 134
- Atomic # = 85
- Mass # = 219
✔ Filled:
| Ion Chemical Formula | Type of Ion | Type/# of particles lost/gained | # p⁺ | # e⁻ | # n⁰ | Atomic # | Mass # |
|----------------------|-------------|----------------------------------|------|------|------|----------|--------|
| At⁻ | Anion | Gain 1 e⁻ | 85 | 86 | 134 | 85 | 219 |
---
#### Row 6: Loses 2 e⁻, neutrons = 132, atomic # = 88
- Atomic # = 88 → element is Radium (Ra)
- Protons = 88
- Loses 2 electrons → charge = +2 → Ra²⁺
- Electrons = 88 – 2 = 86
- Neutrons = 132 (given)
- Mass # = protons + neutrons = 88 + 132 = 220
✔ Filled:
| Ion Chemical Formula | Type of Ion | Type/# of particles lost/gained | # p⁺ | # e⁻ | # n⁰ | Atomic # | Mass # |
|----------------------|-------------|----------------------------------|------|------|------|----------|--------|
| Ra²⁺ | Cation | Loses 2 e⁻ | 88 | 86 | 132 | 88 | 220 |
---
#### Row 7: In³⁺, mass # = 109
- In = Indium → atomic number = 49
- So, protons = 49
- Charge = +3 → lost 3 electrons → electrons = 49 – 3 = 46
- Mass # = 109 → neutrons = 109 – 49 = 60
- Type of ion: Cation (loses electrons)
✔ Filled:
| Ion Chemical Formula | Type of Ion | Type/# of particles lost/gained | # p⁺ | # e⁻ | # n⁰ | Atomic # | Mass # |
|----------------------|-------------|----------------------------------|------|------|------|----------|--------|
| In³⁺ | Cation | Loses 3 e⁻ | 49 | 46 | 60 | 49 | 109 |
---
#### Row 8: p⁺ = 34, e⁻ = 36, n⁰ = 40
- Protons = 34 → element is Selenium (Se)
- Electrons = 36 → more than protons → gained 2 electrons → charge = -2 → Se²⁻
- Atomic # = 34
- Mass # = protons + neutrons = 34 + 40 = 74
✔ Filled:
| Ion Chemical Formula | Type of Ion | Type/# of particles lost/gained | # p⁺ | # e⁻ | # n⁰ | Atomic # | Mass # |
|----------------------|-------------|----------------------------------|------|------|------|----------|--------|
| Se²⁻ | Anion | Gain 2 e⁻ | 34 | 36 | 40 | 34 | 74 |
---
| Ion Chemical Formula | Type of Ion | Type/# of particles lost/gained | # p⁺ | # e⁻ | # n⁰ | Atomic # | Mass # |
|----------------------|-------------|----------------------------------|------|------|------|----------|--------|
| At⁻ | Anion | Gain 1 e⁻ | 85 | 86 | 134 | 85 | 219 |
| Ra²⁺ | Cation | Loses 2 e⁻ | 88 | 86 | 132 | 88 | 220 |
| In³⁺ | Cation | Loses 3 e⁻ | 49 | 46 | 60 | 49 | 109 |
| Se²⁻ | Anion | Gain 2 e⁻ | 34 | 36 | 40 | 34 | 74 |
---
#### 9. a) A particle has 51 protons and has lost 5 electrons. Write the ion chemical formula.
- Protons = 51 → element is Antimony (Sb)
- Lost 5 electrons → charge = +5 → Sb⁵⁺
Answer: Sb⁵⁺
#### b) Type of ion?
- Lost electrons → Cation
Answer: Cation
---
#### 10. a) A particle has 16 protons and has gained 2 electrons. Write the ion chemical formula.
- Protons = 16 → element is Sulfur (S)
- Gained 2 electrons → charge = -2 → S²⁻
Answer: S²⁻
#### b) Type of ion?
- Gained electrons → Anion
Answer: Anion
---
#### 11. A neutral atom changes to an ion when it gains or loses which subatomic particle?
- Ions form by gaining or losing electrons.
Answer: Electrons
---
#### 12. Which subatomic particle identifies an element?
- The number of protons (atomic number) defines the element.
Answer: Protons
---
#### 13. Which subatomic particle causes one isotope of an atom to change to a different isotope of the same element?
- Isotopes differ in number of neutrons, but same number of protons.
Answer: Neutrons
---
#### Part I Table:
| Isotopic Notation | Isotope Name | Oxidation # | Atomic Number | Protons | Neutrons | Electrons | Mass Number |
|-------------------|--------------------|-------------|---------------|---------|----------|-----------|-------------|
| $^{106}_{47}\text{Ag}^{+1}$ | Silver-106 | +1 | 47 | 47 | 59 | 46 | 106 |
| $^{34}_{16}\text{S}^{-2}$ | Sulfur-34 | -2 | 16 | 16 | 18 | 18 | 34 |
| $^{21}_{10}\text{Ne}$ | Neon-21 | 0 | 10 | 10 | 11 | 10 | 21 |
| $^{155}_{99}\text{Es}$ | Einsteinium-155 | 0 | 99 | 99 | 56 | 99 | 155 |
#### Part II Table:
| Ion Chemical Formula | Type of Ion | Type/# of particles lost/gained | # p⁺ | # e⁻ | # n⁰ | Atomic # | Mass # |
|----------------------|-------------|----------------------------------|------|------|------|----------|--------|
| At⁻ | Anion | Gain 1 e⁻ | 85 | 86 | 134 | 85 | 219 |
| Ra²⁺ | Cation | Loses 2 e⁻ | 88 | 86 | 132 | 88 | 220 |
| In³⁺ | Cation | Loses 3 e⁻ | 49 | 46 | 60 | 49 | 109 |
| Se²⁻ | Anion | Gain 2 e⁻ | 34 | 36 | 40 | 34 | 74 |
#### Part III:
9a) Sb⁵⁺
9b) Cation
10a) S²⁻
10b) Anion
#### Part IV:
11. Electrons
12. Protons
13. Neutrons
---
✔ All answers are now complete and explained!
---
Part I: Fill in the table using given information
We need to use the following key concepts:
- Atomic number (Z) = number of protons
- Mass number (A) = protons + neutrons
- Electrons = protons – charge (for ions), or equal to protons for neutral atoms
- Isotopic notation: $ ^{A}_{Z}X $
- Oxidation state tells us how many electrons are gained or lost
---
#### Row 1: $^{106}_{47}\text{Ag}^{+1}$
- Isotopic Notation: $^{106}_{47}\text{Ag}^{+1}$
- Isotope Name: Silver-106
- Oxidation #: +1 (given)
- Atomic Number: 47 (from subscript)
- Number Protons: 47 (same as atomic number)
- Number Neutrons: Mass # – protons = 106 – 47 = 59
- Number Electrons: Protons – charge = 47 – 1 = 46
- Mass Number: 106 (superscript)
✔ Filled:
| Isotopic Notation | Isotope Name | Oxidation # | Atomic Number | Protons | Neutrons | Electrons | Mass Number |
|-------------------|--------------|-------------|---------------|---------|----------|-----------|-------------|
| $^{106}_{47}\text{Ag}^{+1}$ | Silver-106 | +1 | 47 | 47 | 59 | 46 | 106 |
---
#### Row 2: Sulfur-34, Oxidation # = -2
- Isotope Name: Sulfur-34
- Oxidation #: -2 (given)
- Atomic Number: Sulfur has atomic number 16
- Protons: 16
- Mass Number: 34 (from name "Sulfur-34")
- Neutrons: 34 – 16 = 18
- Electrons: For ion with -2 charge → 16 + 2 = 18
- Isotopic Notation: $^{34}_{16}\text{S}^{-2}$
✔ Filled:
| Isotopic Notation | Isotope Name | Oxidation # | Atomic Number | Protons | Neutrons | Electrons | Mass Number |
|-------------------|--------------|-------------|---------------|---------|----------|-----------|-------------|
| $^{34}_{16}\text{S}^{-2}$ | Sulfur-34 | -2 | 16 | 16 | 18 | 18 | 34 |
---
#### Row 3: Oxidation # = 0, Protons = 10, Neutrons = 11
- Oxidation #: 0 → neutral atom
- Protons: 10 → Atomic number = 10 → Element is Neon (Ne)
- Neutrons: 11
- Mass Number: Protons + neutrons = 10 + 11 = 21
- Electrons: Same as protons = 10 (neutral)
- Isotope Name: Neon-21
- Isotopic Notation: $^{21}_{10}\text{Ne}$
✔ Filled:
| Isotopic Notation | Isotope Name | Oxidation # | Atomic Number | Protons | Neutrons | Electrons | Mass Number |
|-------------------|--------------|-------------|---------------|---------|----------|-----------|-------------|
| $^{21}_{10}\text{Ne}$ | Neon-21 | 0 | 10 | 10 | 11 | 10 | 21 |
---
#### Row 4: Electrons = 99, Mass Number = 155, Oxidation # = 0
- Oxidation # = 0 → neutral atom → electrons = protons
- So, protons = 99
- Atomic number = 99 → element is Einsteinium (Es)
- Mass number = 155 (given)
- Neutrons = 155 – 99 = 56
- Isotope Name: Einsteinium-155
- Isotopic Notation: $^{155}_{99}\text{Es}$
✔ Filled:
| Isotopic Notation | Isotope Name | Oxidation # | Atomic Number | Protons | Neutrons | Electrons | Mass Number |
|-------------------|--------------|-------------|---------------|---------|----------|-----------|-------------|
| $^{155}_{99}\text{Es}$ | Einsteinium-155 | 0 | 99 | 99 | 56 | 99 | 155 |
---
✔ Part I Table Completed:
| Isotopic Notation | Isotope Name | Oxidation # | Atomic Number | Protons | Neutrons | Electrons | Mass Number |
|-------------------|--------------------|-------------|---------------|---------|----------|-----------|-------------|
| $^{106}_{47}\text{Ag}^{+1}$ | Silver-106 | +1 | 47 | 47 | 59 | 46 | 106 |
| $^{34}_{16}\text{S}^{-2}$ | Sulfur-34 | -2 | 16 | 16 | 18 | 18 | 34 |
| $^{21}_{10}\text{Ne}$ | Neon-21 | 0 | 10 | 10 | 11 | 10 | 21 |
| $^{155}_{99}\text{Es}$ | Einsteinium-155 | 0 | 99 | 99 | 56 | 99 | 155 |
---
Part II: Fill in the blanks
Use:
- Atomic number = # protons
- Mass number = protons + neutrons
- Charge = protons – electrons → electrons = protons – charge
---
#### Row 5: Gain 1 e⁻, p⁺ = 85, mass # = 219
- Protons = 85 → element is Astatine (At)
- Gains 1 electron → becomes anion with charge -1 → formula: At⁻
- Electrons = 85 + 1 = 86
- Neutrons = 219 – 85 = 134
- Atomic # = 85
- Mass # = 219
✔ Filled:
| Ion Chemical Formula | Type of Ion | Type/# of particles lost/gained | # p⁺ | # e⁻ | # n⁰ | Atomic # | Mass # |
|----------------------|-------------|----------------------------------|------|------|------|----------|--------|
| At⁻ | Anion | Gain 1 e⁻ | 85 | 86 | 134 | 85 | 219 |
---
#### Row 6: Loses 2 e⁻, neutrons = 132, atomic # = 88
- Atomic # = 88 → element is Radium (Ra)
- Protons = 88
- Loses 2 electrons → charge = +2 → Ra²⁺
- Electrons = 88 – 2 = 86
- Neutrons = 132 (given)
- Mass # = protons + neutrons = 88 + 132 = 220
✔ Filled:
| Ion Chemical Formula | Type of Ion | Type/# of particles lost/gained | # p⁺ | # e⁻ | # n⁰ | Atomic # | Mass # |
|----------------------|-------------|----------------------------------|------|------|------|----------|--------|
| Ra²⁺ | Cation | Loses 2 e⁻ | 88 | 86 | 132 | 88 | 220 |
---
#### Row 7: In³⁺, mass # = 109
- In = Indium → atomic number = 49
- So, protons = 49
- Charge = +3 → lost 3 electrons → electrons = 49 – 3 = 46
- Mass # = 109 → neutrons = 109 – 49 = 60
- Type of ion: Cation (loses electrons)
✔ Filled:
| Ion Chemical Formula | Type of Ion | Type/# of particles lost/gained | # p⁺ | # e⁻ | # n⁰ | Atomic # | Mass # |
|----------------------|-------------|----------------------------------|------|------|------|----------|--------|
| In³⁺ | Cation | Loses 3 e⁻ | 49 | 46 | 60 | 49 | 109 |
---
#### Row 8: p⁺ = 34, e⁻ = 36, n⁰ = 40
- Protons = 34 → element is Selenium (Se)
- Electrons = 36 → more than protons → gained 2 electrons → charge = -2 → Se²⁻
- Atomic # = 34
- Mass # = protons + neutrons = 34 + 40 = 74
✔ Filled:
| Ion Chemical Formula | Type of Ion | Type/# of particles lost/gained | # p⁺ | # e⁻ | # n⁰ | Atomic # | Mass # |
|----------------------|-------------|----------------------------------|------|------|------|----------|--------|
| Se²⁻ | Anion | Gain 2 e⁻ | 34 | 36 | 40 | 34 | 74 |
---
✔ Part II Table Completed:
| Ion Chemical Formula | Type of Ion | Type/# of particles lost/gained | # p⁺ | # e⁻ | # n⁰ | Atomic # | Mass # |
|----------------------|-------------|----------------------------------|------|------|------|----------|--------|
| At⁻ | Anion | Gain 1 e⁻ | 85 | 86 | 134 | 85 | 219 |
| Ra²⁺ | Cation | Loses 2 e⁻ | 88 | 86 | 132 | 88 | 220 |
| In³⁺ | Cation | Loses 3 e⁻ | 49 | 46 | 60 | 49 | 109 |
| Se²⁻ | Anion | Gain 2 e⁻ | 34 | 36 | 40 | 34 | 74 |
---
Part III: Answer Questions
#### 9. a) A particle has 51 protons and has lost 5 electrons. Write the ion chemical formula.
- Protons = 51 → element is Antimony (Sb)
- Lost 5 electrons → charge = +5 → Sb⁵⁺
Answer: Sb⁵⁺
#### b) Type of ion?
- Lost electrons → Cation
Answer: Cation
---
#### 10. a) A particle has 16 protons and has gained 2 electrons. Write the ion chemical formula.
- Protons = 16 → element is Sulfur (S)
- Gained 2 electrons → charge = -2 → S²⁻
Answer: S²⁻
#### b) Type of ion?
- Gained electrons → Anion
Answer: Anion
---
Part IV: Short Answer Questions
#### 11. A neutral atom changes to an ion when it gains or loses which subatomic particle?
- Ions form by gaining or losing electrons.
Answer: Electrons
---
#### 12. Which subatomic particle identifies an element?
- The number of protons (atomic number) defines the element.
Answer: Protons
---
#### 13. Which subatomic particle causes one isotope of an atom to change to a different isotope of the same element?
- Isotopes differ in number of neutrons, but same number of protons.
Answer: Neutrons
---
✔ Final Answers Summary:
#### Part I Table:
| Isotopic Notation | Isotope Name | Oxidation # | Atomic Number | Protons | Neutrons | Electrons | Mass Number |
|-------------------|--------------------|-------------|---------------|---------|----------|-----------|-------------|
| $^{106}_{47}\text{Ag}^{+1}$ | Silver-106 | +1 | 47 | 47 | 59 | 46 | 106 |
| $^{34}_{16}\text{S}^{-2}$ | Sulfur-34 | -2 | 16 | 16 | 18 | 18 | 34 |
| $^{21}_{10}\text{Ne}$ | Neon-21 | 0 | 10 | 10 | 11 | 10 | 21 |
| $^{155}_{99}\text{Es}$ | Einsteinium-155 | 0 | 99 | 99 | 56 | 99 | 155 |
#### Part II Table:
| Ion Chemical Formula | Type of Ion | Type/# of particles lost/gained | # p⁺ | # e⁻ | # n⁰ | Atomic # | Mass # |
|----------------------|-------------|----------------------------------|------|------|------|----------|--------|
| At⁻ | Anion | Gain 1 e⁻ | 85 | 86 | 134 | 85 | 219 |
| Ra²⁺ | Cation | Loses 2 e⁻ | 88 | 86 | 132 | 88 | 220 |
| In³⁺ | Cation | Loses 3 e⁻ | 49 | 46 | 60 | 49 | 109 |
| Se²⁻ | Anion | Gain 2 e⁻ | 34 | 36 | 40 | 34 | 74 |
#### Part III:
9a) Sb⁵⁺
9b) Cation
10a) S²⁻
10b) Anion
#### Part IV:
11. Electrons
12. Protons
13. Neutrons
---
✔ All answers are now complete and explained!
Parent Tip: Review the logic above to help your child master the concept of isotope worksheet.
