Educational worksheet on atomic structure focusing on ions and isotopes, including questions and a table for practice.

Problem Analysis and Solution

The provided worksheet focuses on atomic structure, ions, and isotopes. Let's solve each part step by step.

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## Part One: Ions

1) For Each of the Ions Listed, Identify the Total Number of Electrons for Each.

To determine the number of electrons in an ion, we need to:
- Start with the atomic number (number of protons), which is equal to the number of electrons in a neutral atom.
- Adjust the number of electrons based on the charge of the ion:
- Positive charge: Subtract the charge from the atomic number.
- Negative charge: Add the charge to the atomic number.

#### i) Al³⁺
- Atomic number of Al (Aluminum) = 13
- Charge = +3
- Electrons = 13 - 3 = 10

#### ii) Fe³⁺
- Atomic number of Fe (Iron) = 26
- Charge = +3
- Electrons = 26 - 3 = 23

#### iii) Mg²⁺
- Atomic number of Mg (Magnesium) = 12
- Charge = +2
- Electrons = 12 - 2 = 10

#### iv) Sn²⁺
- Atomic number of Sn (Tin) = 50
- Charge = +2
- Electrons = 50 - 2 = 48

#### v) Co²⁺
- Atomic number of Co (Cobalt) = 27
- Charge = +2
- Electrons = 27 - 2 = 25

#### vi) Co³⁺
- Atomic number of Co (Cobalt) = 27
- Charge = +3
- Electrons = 27 - 3 = 24

#### vii) Li¹⁺
- Atomic number of Li (Lithium) = 3
- Charge = +1
- Electrons = 3 - 1 = 2

#### viii) Cr³⁺
- Atomic number of Cr (Chromium) = 24
- Charge = +3
- Electrons = 24 - 3 = 21

#### ix) Rb¹⁺
- Atomic number of Rb (Rubidium) = 37
- Charge = +1
- Electrons = 37 - 1 = 36

#### x) Pt²⁺
- Atomic number of Pt (Platinum) = 78
- Charge = +2
- Electrons = 78 - 2 = 76

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2) Determine the Charges on the Following:

#### a) An Atom Having Lost Two Electrons
- Losing 2 electrons means the atom has a +2 charge.

#### b) An Atom Having Lost Six Electrons
- Losing 6 electrons means the atom has a +6 charge.

#### c) An Atom Having Gained One Electron
- Gaining 1 electron means the atom has a -1 charge.

#### d) An Atom Having Gained Three Electrons
- Gaining 3 electrons means the atom has a -3 charge.

#### e) An Atom Having Lost Five Electrons
- Losing 5 electrons means the atom has a +5 charge.

#### f) An Atom Having Gained Two Electrons
- Gaining 2 electrons means the atom has a -2 charge.

#### g) An Atom Having Lost One Electron
- Losing 1 electron means the atom has a +1 charge.

#### h) An Atom Having Gained Four Electrons
- Gaining 4 electrons means the atom has a -4 charge.

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## Part Two: Isotopes

1) Here Are Three Isotopes of an Element: ${}^{12}\text{C}_6$, ${}^{13}\text{C}_6$, ${}^{14}\text{C}_6$

#### a) The Element Is
- The element is identified by the subscript (6), which represents the atomic number. The element with atomic number 6 is Carbon (C).

#### b) The Number 6 Refers to the
- The number 6 refers to the atomic number, which is the number of protons in the nucleus.

#### c) The Numbers 12, 13, and 14 Refer to the
- The numbers 12, 13, and 14 refer to the mass number, which is the sum of protons and neutrons in the nucleus.

#### d) How Many Protons and Neutrons Are in the First Isotope?
- First isotope: ${}^{12}\text{C}_6$
- Atomic number (protons) = 6
- Mass number = 12
- Neutrons = Mass number - Protons = 12 - 6 = 6
- Protons = 6, Neutrons = 6

#### e) How Many Protons and Neutrons Are in the Second Isotope?
- Second isotope: ${}^{13}\text{C}_6$
- Atomic number (protons) = 6
- Mass number = 13
- Neutrons = Mass number - Protons = 13 - 6 = 7
- Protons = 6, Neutrons = 7

#### f) How Many Protons and Neutrons Are in the Third Isotope?
- Third isotope: ${}^{14}\text{C}_6$
- Atomic number (protons) = 6
- Mass number = 14
- Neutrons = Mass number - Protons = 14 - 6 = 8
- Protons = 6, Neutrons = 8

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2) Complete the Following Chart

#### Isotope Name: 92 Uranium-235
- Atomic number (Z) = 92
- Mass number (A) = 235
- Protons = Atomic number = 92
- Neutrons = Mass number - Protons = 235 - 92 = 143
- Electrons = Protons (neutral atom) = 92

| Isotope name | Atomic # | Mass # | # of protons | # of neutrons | # of electrons |
|--------------|----------|--------|--------------|---------------|----------------|
| 92 uranium-235 | 92 | 235 | 92 | 143 | 92 |

#### Isotope Name: 92 Uranium-238
- Atomic number (Z) = 92
- Mass number (A) = 238
- Protons = Atomic number = 92
- Neutrons = Mass number - Protons = 238 - 92 = 146
- Electrons = Protons (neutral atom) = 92

| Isotope name | Atomic # | Mass # | # of protons | # of neutrons | # of electrons |
|--------------|----------|--------|--------------|---------------|----------------|
| 92 uranium-238 | 92 | 238 | 92 | 146 | 92 |

#### Isotope Name: 5 Boron-10
- Atomic number (Z) = 5
- Mass number (A) = 10
- Protons = Atomic number = 5
- Neutrons = Mass number - Protons = 10 - 5 = 5
- Electrons = Protons (neutral atom) = 5

| Isotope name | Atomic # | Mass # | # of protons | # of neutrons | # of electrons |
|--------------|----------|--------|--------------|---------------|----------------|
| 5 boron-10 | 5 | 10 | 5 | 5 | 5 |

#### Isotope Name: 5 Boron-11
- Atomic number (Z) = 5
- Mass number (A) = 11
- Protons = Atomic number = 5
- Neutrons = Mass number - Protons = 11 - 5 = 6
- Electrons = Protons (neutral atom) = 5

| Isotope name | Atomic # | Mass # | # of protons | # of neutrons | # of electrons |
|--------------|----------|--------|--------------|---------------|----------------|
| 5 boron-11 | 5 | 11 | 5 | 6 | 5 |

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## Final Answer

Part One: Ions

1.
- i) 10
- ii) 23
- iii) 10
- iv) 48
- v) 25
- vi) 24
- vii) 2
- viii) 21
- ix) 36
- x) 76

2.
- a) +2
- b) +6
- c) -1
- d) -3
- e) +5
- f) -2
- g) +1
- h) -4

Part Two: Isotopes

1.
- a) Carbon (C)
- b) Atomic number
- c) Mass number
- d) Protons = 6, Neutrons = 6
- e) Protons = 6, Neutrons = 7
- f) Protons = 6, Neutrons = 8

2.
| Isotope name | Atomic # | Mass # | # of protons | # of neutrons | # of electrons |
|--------------|----------|--------|--------------|---------------|----------------|
| 92 uranium-235 | 92 | 235 | 92 | 143 | 92 |
| 92 uranium-238 | 92 | 238 | 92 | 146 | 92 |
| 5 boron-10 | 5 | 10 | 5 | 5 | 5 |
| 5 boron-11 | 5 | 11 | 5 | 6 | 5 |

Boxed Final Answer:
\[
\boxed{
\begin{array}{l}
\text{Part One: Ions} \\
1. \text{i) 10, ii) 23, iii) 10, iv) 48, v) 25, vi) 24, vii) 2, viii) 21, ix) 36, x) 76} \\
2. \text{a) +2, b) +6, c) -1, d) -3, e) +5, f) -2, g) +1, h) -4} \\
\text{Part Two: Isotopes} \\
1. \text{a) Carbon (C), b) Atomic number, c) Mass number, d) Protons = 6, Neutrons = 6, e) Protons = 6, Neutrons = 7, f) Protons = 6, Neutrons = 8} \\
2. \begin{array}{|c|c|c|c|c|c|}
\hline
\text{Isotope name} & \text{Atomic \#} & \text{Mass \#} & \text{\# of protons} & \text{\# of neutrons} & \text{\# of electrons} \\
\hline
92 \text{ uranium-235} & 92 & 235 & 92 & 143 & 92 \\
\hline
92 \text{ uranium-238} & 92 & 238 & 92 & 146 & 92 \\
\hline
5 \text{ boron-10} & 5 & 10 & 5 & 5 & 5 \\
\hline
5 \text{ boron-11} & 5 & 11 & 5 & 6 & 5 \\
\hline
\end{array}
\end{array}
}
\]