practice: isotope calculations #1
part 1 use the notation below to answer the following questions.
¹²c ¹³c ¹⁴c
1 different versions of the same element, like pictured above, are known as
2 the numbers 12, 13, and 14 refer to the
3 what subatomic particle makes each of these isotopes different?
4 how many does each have of #3?
5 what subatomic particle makes each of these isotopes the same?
6 how many does each have of #5?
7 this form of notation is known as
8 the other form of isotope notation is known as
9 for each isotope, write it in the form listed in #8

part 2 complete the chart below.
10.
| isotope (hyphen form) | isotope (nuclear form) | atomic # | mass # | # of p⁺ | # of n⁰ | # of e⁻ |
| ---- | ---- | ---- | ---- | ---- | ---- | ---- |
| uranium-235 | | | | | | |
| | | 5 | | | 5 | |
| | ³⁷k | | | | | |
| | | | 11 | 5 | | |
| | | | | 47 | 60 | |
| | ²³⁸u | | | | | |
| oxygen-17 | | | | | | |
| | | | 108 | | 61 | |

Question

practice: isotope calculations #1
part 1 use the notation below to answer the following questions.
¹²c ¹³c ¹⁴c
1 different versions of the same element, like pictured above, are known as
2 the numbers 12, 13, and 14 refer to the
3 what subatomic particle makes each of these isotopes different?
4 how many does each have of #3?
5 what subatomic particle makes each of these isotopes the same?
6 how many does each have of #5?
7 this form of notation is known as
8 the other form of isotope notation is known as
9 for each isotope, write it in the form listed in #8

part 2 complete the chart below.
10.
| isotope (hyphen form) | isotope (nuclear form) | atomic # | mass # | # of p⁺ | # of n⁰ | # of e⁻ |
| ---- | ---- | ---- | ---- | ---- | ---- | ---- |
| uranium-235 |  |  |  |  |  |  |
|  |  | 5 |  |  | 5 |  |
|  | ³⁷k |  |  |  |  |  |
|  |  |  | 11 | 5 |  |  |
|  |  |  |  | 47 | 60 |  |
|  | ²³⁸u |  |  |  |  |  |
| oxygen-17 |  |  |  |  |  |  |
|  |  |  | 108 |  | 61 |  |

Accepted Answer

### Part 1
1.
# Brief Explanations:
Different versions of the same element with different mass numbers (due to different neutron counts) are called isotopes.
# Answer:
isotopes

2.
# Brief Explanations:
The numbers 12, 13, 14 in $^{12}\text{C}$, $^{13}\text{C}$, $^{14}\text{C}$ represent the mass number, which is the sum of protons and neutrons in the nucleus.
# Answer:
mass number

3.
# Brief Explanations:
Isotopes of an element have the same number of protons (atomic number) but different numbers of neutrons, so neutrons are the subatomic particle that differs.
# Answer:
neutron

4.
# Brief Explanations:
For carbon, atomic number (number of protons) is 6. Using the formula $ \text{Number of neutrons} = \text{Mass number} - \text{Atomic number} $. For $^{12}\text{C}$: $ 12 - 6 = 6 $; $^{13}\text{C}$: $ 13 - 6 = 7 $; $^{14}\text{C}$: $ 14 - 6 = 8 $.
# Explanation:
## Step 1: Recall atomic number of carbon
Carbon has an atomic number ($Z$) of 6, so number of protons ($p^+$) is 6.
## Step 2: Calculate neutrons for each isotope
- For $^{12}\text{C}$: $ \text{Neutrons} (n^0) = 12 - 6 = 6 $
- For $^{13}\text{C}$: $ \text{Neutrons} (n^0) = 13 - 6 = 7 $
- For $^{14}\text{C}$: $ \text{Neutrons} (n^0) = 14 - 6 = 8 $
# Answer:
$^{12}\text{C}$: 6; $^{13}\text{C}$: 7; $^{14}\text{C}$: 8

5.
# Brief Explanations:
Isotopes of an element have the same atomic number, which means they have the same number of protons. Protons determine the element's identity, so protons are the subatomic particle that is the same.
# Answer:
proton

6.
# Brief Explanations:
Carbon has an atomic number of 6, which is the number of protons (and also electrons in a neutral atom). So each carbon isotope has 6 protons (and 6 electrons in neutral state).
# Answer:
6 (protons and electrons, since the atom is neutral)

7.
# Brief Explanations:
The notation $^{A}\text{X}$ (where $A$ is mass number, $X$ is element symbol) is called nuclear notation or isotopic notation.
# Answer:
nuclear notation (or isotopic notation)

8.
# Brief Explanations:
The other common isotope notation is the hyphen notation, which is written as $\text{Element - Mass number}$ (e.g., Carbon - 12, Carbon - 13, Carbon - 14).
# Answer:
hyphen notation (e.g., Carbon - 12)

9.
# Brief Explanations:
For $^{12}\text{C}$, hyphen notation is Carbon - 12; for $^{13}\text{C}$, it's Carbon - 13; for $^{14}\text{C}$, it's Carbon - 14.
# Answer:
Carbon - 12, Carbon - 13, Carbon - 14

### Part 2 (Completing the Chart)
We use the following relationships:
- Atomic number ($Z$) = number of protons ($p^+$) = number of electrons ($e^-$) (in neutral atom).
- Mass number ($A$) = number of protons ($p^+$) + number of neutrons ($n^0$) → $n^0 = A - Z$.
- Hyphen notation: $\text{Element - Mass number}$; Nuclear notation: $^{A}\text{Element symbol}$.

#### 1. Uranium - 235
- **Isotope (Nuclear form)**: Uranium has atomic number $Z = 92$, mass number $A = 235$ → $^{235}\text{U}$
- **Atomic #**: $Z = 92$ (uranium's atomic number)
- **Mass #**: $A = 235$
- **# of $p^+$**: $Z = 92$
- **# of $n^0$**: $235 - 92 = 143$
- **# of $e^-$**: $Z = 92$ (neutral atom)

#### 2. Atomic # = 5 (Boron, since $Z = 5$ is boron)
- **Mass #**: $A = p^+ + n^0 = 5 + 5 = 10$
- **Isotope (Hyphen form)**: Boron - 10
- **Isotope (Nuclear form)**: $^{10}\text{B}$
- **# of $p^+$**: $Z = 5$
- **# of $e^-$**: $Z = 5$

#### 3. $^{37}\text{K}$ (Potassium - 37)
- Potassium has atomic number $Z = 19$ (so $p^+ = 19$, $e^- = 19$).
- **Mass #**: $A = 37$
- **# of $n^0$**: $37 - 19 = 18$
- **Isotope (Hyphen form)**: Potassium - 37

#### 4. Mass # = 11, $p^+ = 5$ (Boron, $Z = 5$)
- **Atomic #**: $Z = 5$
- **# of $n^0$**: $11 - 5 = 6$
- **# of $e^-$**: $Z = 5$
- **Isotope (Hyphen form)**: Boron - 11
- **Isotope (Nuclear form)**: $^{11}\text{B}$

#### 5. $p^+ = 47$, $n^0 = 60$
- Atomic number $Z = 47$ (Silver, Ag).
- Mass number $A = 47 + 60 = 107$.
- **Isotope (Hyphen form)**: Silver - 107
- **Isotope (Nuclear form)**: $^{107}\text{Ag}$
- **Atomic #**: $47$
- **Mass #**: $107$
- **# of $e^-$**: $47$

#### 6. $^{238}\text{U}$ (Uranium - 238)
- **Isotope (Hyphen form)**: Uranium - 238
- Atomic number $Z = 92$ (uranium), Mass number $A = 238$.
- **# of $n^0$**: $238 - 92 = 146$
- **# of $p^+$**: $92$
- **# of $e^-$**: $92$

#### 7. Oxygen - 17
- Oxygen has atomic number $Z = 8$ (so $p^+ = 8$, $e^- = 8$).
- Mass number $A = 17$.
- **Isotope (Nuclear form)**: $^{17}\text{O}$
- **Atomic #**: $8$
- **# of $n^0$**: $17 - 8 = 9$

#### 8. Mass # = 108, $n^0 = 61$
- Atomic number $Z = p^+ = A - n^0 = 108 - 61 = 47$ (Silver, Ag).
- **Isotope (Hyphen form)**: Silver - 108
- **Isotope (Nuclear form)**: $^{108}\text{Ag}$
- **Atomic #**: $47$
- **# of $p^+$**: $47$
- **# of $e^-$**: $47$

### Filled Chart (Row - by - Row)

| Isotope (Hyphen form) | Isotope (Nuclear form) | Atomic # | Mass # | # of $p^+$ | # of $n^0$ | # of $e^-$ |
|-----------------------|------------------------|----------|--------|--------------|--------------|--------------|
| Uranium - 235         | $^{235}\text{U}$     | 92       | 235    | 92           | 143          | 92           |
| Boron - 10            | $^{10}\text{B}$      | 5        | 10     | 5            | 5            | 5            |
| Potassium - 37        | $^{37}\text{K}$      | 19       | 37     | 19           | 18           | 19           |
| Boron - 11            | $^{11}\text{B}$      | 5        | 11     | 5            | 6            | 5            |
| Silver - 107          | $^{107}\text{Ag}$    | 47       | 107    | 47           | 60           | 47           |
| Uranium - 238         | $^{238}\text{U}$     | 92       | 238    | 92           | 146          | 92           |
| Oxygen - 17           | $^{17}\text{O}$      | 8        | 17     | 8            | 9            | 8            |
| Silver - 108          | $^{108}\text{Ag}$    | 47       | 108    | 47           | 61           | 47           |

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